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Nickel – Periodic Table – Atomic Properties

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Nickel-density-atomic-number-mass-radius

Nickel is a silvery-white lustrous metal with a slight golden tinge. Nickel belongs to the transition metals and is hard and ductile.

Summary

Element Nickel
Atomic number 28
Atomic mass [amu] 58.6934
Atomic mass [pm] 124
Density at STP [g/cm3] 8.908
Number of protons 28
Number of neutrons (typical isotopes) 60; 61; 62; 64
Number of electrons 28
Electron configuration [Ar] 3d8 4s2
Oxidation states +2,3
Electron affinity [kJ/mol] 112
Electronegativity [Pauling scale] 1.91
First ionization energy [eV] 7.6398

Atomic Number – Protons, Electrons and Neutrons in Nickel

Proton Number - Atomic NumberNickel is a chemical element with atomic number 28 which means there are 28 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Nickel are 60; 61; 62; 64.

Atomic Mass of Nickel

Atomic mass of Nickel is 58.6934 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Nickel

The atomic radius of Nickel atom is 124pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Nickel is 28. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Nickel is [Ar] 3d8 4s2.

Possible oxidation states are +2,3.

Density of Nickel

Density of Nickel is 8.908g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Nickel-protons-neutrons-electrons-configuration

Nickel-affinity-electronegativity-ionization

Electron Affinity – Nickel

Electron affinity of Nickel is 112 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Nickel

Electronegativity of Nickel is 1.91.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Nickel is: χ = 1.91

First Ionization Energy of Nickel

First Ionization Energy of Nickel is 7.6398 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Nickel atom, for example, requires the following ionization energy to remove the outermost electron.

Ni + IE → Ni+ + e−        IE = 7.6398 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Nickel-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Nickel - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Nickel

 

Cobalt – Periodic Table – Atomic Properties

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Cobalt-density-atomic-number-mass-radius

Cobalt is found in the Earth’s crust only in chemically combined form, save for small deposits found in alloys of natural meteoric iron. The free element, produced by reductive smelting, is a hard, lustrous, silver-gray metal.

Summary

Element Cobalt
Atomic number 27
Atomic mass [amu] 58.9332
Atomic mass [pm] 126
Density at STP [g/cm3] 8.9
Number of protons 27
Number of neutrons (typical isotopes) 59
Number of electrons 27
Electron configuration [Ar] 3d7 4s2
Oxidation states +2,3
Electron affinity [kJ/mol] 63.7
Electronegativity [Pauling scale] 1.88
First ionization energy [eV] 7.881

Atomic Number – Protons, Electrons and Neutrons in Cobalt

Proton Number - Atomic NumberCobalt is a chemical element with atomic number 27 which means there are 27 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Cobalt are 59.

Atomic Mass of Cobalt

Atomic mass of Cobalt is 58.9332 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Cobalt

The atomic radius of Cobalt atom is 126pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Cobalt is 27. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Cobalt is [Ar] 3d7 4s2.

Possible oxidation states are +2,3.

Density of Cobalt

Density of Cobalt is 8.9g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Cobalt-protons-neutrons-electrons-configuration

Cobalt-affinity-electronegativity-ionization

Electron Affinity – Cobalt

Electron affinity of Cobalt is 63.7 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Cobalt

Electronegativity of Cobalt is 1.88.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Cobalt is: χ = 1.88

First Ionization Energy of Cobalt

First Ionization Energy of Cobalt is 7.881 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Cobalt atom, for example, requires the following ionization energy to remove the outermost electron.

Co + IE → Co+ + e−        IE = 7.881 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Cobalt-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Cobalt - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Cobalt

 

Iron – Periodic Table – Atomic Properties

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Iron-density-atomic-number-mass-radius

Iron is a metal in the first transition series. It is by mass the most common element on Earth, forming much of Earth’s outer and inner core. It is the fourth most common element in the Earth’s crust. Its abundance in rocky planets like Earth is due to its abundant production by fusion in high-mass stars.

Summary

Element Iron
Atomic number 26
Atomic mass [amu] 55.845
Atomic mass [pm] 132
Density at STP [g/cm3] 7.874
Number of protons 26
Number of neutrons (typical isotopes) 56; 57; 58
Number of electrons 26
Electron configuration [Ar] 3d6 4s2
Oxidation states +2,3
Electron affinity [kJ/mol] 15.7
Electronegativity [Pauling scale] 1.83
First ionization energy [eV] 7.9024

Atomic Number – Protons, Electrons and Neutrons in Iron

Proton Number - Atomic NumberIron is a chemical element with atomic number 26 which means there are 26 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Iron are 56; 57; 58.

Atomic Mass of Iron

Atomic mass of Iron is 55.845 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Iron

The atomic radius of Iron atom is 132pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Iron is 26. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Iron is [Ar] 3d6 4s2.

Possible oxidation states are +2,3.

Density of Iron

Density of Iron is 7.874g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Iron-protons-neutrons-electrons-configuration

Iron-affinity-electronegativity-ionization

Electron Affinity – Iron

Electron affinity of Iron is 15.7 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Iron

Electronegativity of Iron is 1.83.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Iron is: χ = 1.83

First Ionization Energy of Iron

First Ionization Energy of Iron is 7.9024 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Iron atom, for example, requires the following ionization energy to remove the outermost electron.

Fe + IE → Fe+ + e−        IE = 7.9024 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Iron-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Iron - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Iron

 

Manganese – Periodic Table – Atomic Properties

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Manganese-density-atomic-number-mass-radius

Manganese is a metal with important industrial metal alloy uses, particularly in stainless steels.

Summary

Element Manganese
Atomic number 25
Atomic mass [amu] 54.938049
Atomic mass [pm] 139
Density at STP [g/cm3] 7.47
Number of protons 25
Number of neutrons (typical isotopes) 55
Number of electrons 25
Electron configuration [Ar] 3d5 4s2
Oxidation states +2,3,4,7
Electron affinity [kJ/mol] —
Electronegativity [Pauling scale] 1.55
First ionization energy [eV] 7.434

Atomic Number – Protons, Electrons and Neutrons in Manganese

Proton Number - Atomic NumberManganese is a chemical element with atomic number 25 which means there are 25 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Manganese are 55.

Atomic Mass of Manganese

Atomic mass of Manganese is 54.938049 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Manganese

The atomic radius of Manganese atom is 139pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Manganese is 25. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Manganese is [Ar] 3d5 4s2.

Possible oxidation states are +2,3,4,7.

Density of Manganese

Density of Manganese is 7.47g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Manganese-protons-neutrons-electrons-configuration

Manganese-affinity-electronegativity-ionization

Electron Affinity – Manganese

Electron affinity of Manganese is — kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Manganese

Electronegativity of Manganese is 1.55.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Manganese is: χ = 1.55

First Ionization Energy of Manganese

First Ionization Energy of Manganese is 7.434 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Manganese atom, for example, requires the following ionization energy to remove the outermost electron.

Mn + IE → Mn+ + e−        IE = 7.434 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Manganese-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Manganese - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Manganese

 

Chromium – Periodic Table – Atomic Properties

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Chromium-density-atomic-number-mass-radius

Chromium is a steely-grey, lustrous, hard and brittle metal[4] which takes a high polish, resists tarnishing, and has a high melting point. A major development was the discovery that steel could be made highly resistant to corrosion and discoloration by adding metallic chromium to form stainless steel.

Summary

Element Chromium
Atomic number 24
Atomic mass [amu] 51.9961
Atomic mass [pm] 139
Density at STP [g/cm3] 7.14
Number of protons 24
Number of neutrons (typical isotopes) 50; 52-54
Number of electrons 24
Electron configuration [Ar] 3d5 4s1
Oxidation states +2,3,6
Electron affinity [kJ/mol] 64.3
Electronegativity [Pauling scale] 1.66
First ionization energy [eV] 6.7666

Atomic Number – Protons, Electrons and Neutrons in Chromium

Proton Number - Atomic NumberChromium is a chemical element with atomic number 24 which means there are 24 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Chromium are 50; 52-54.

Atomic Mass of Chromium

Atomic mass of Chromium is 51.9961 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Chromium

The atomic radius of Chromium atom is 139pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Chromium is 24. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Chromium is [Ar] 3d5 4s1.

Possible oxidation states are +2,3,6.

Density of Chromium

Density of Chromium is 7.14g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Chromium-protons-neutrons-electrons-configuration

Chromium-affinity-electronegativity-ionization

Electron Affinity – Chromium

Electron affinity of Chromium is 64.3 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Chromium

Electronegativity of Chromium is 1.66.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Chromium is: χ = 1.66

First Ionization Energy of Chromium

First Ionization Energy of Chromium is 6.7666 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Chromium atom, for example, requires the following ionization energy to remove the outermost electron.

Cr + IE → Cr+ + e−        IE = 6.7666 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Chromium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Chromium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Chromium

 

Vanadium – Periodic Table – Atomic Properties

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Vanadium-density-atomic-number-mass-radius

Vanadium is a hard, silvery grey, ductile, and malleable transition metal. The elemental metal is rarely found in nature, but once isolated artificially, the formation of an oxide layer (passivation) stabilizes the free metal somewhat against further oxidation.

Summary

Element Vanadium
Atomic number 23
Atomic mass [amu] 50.9415
Atomic mass [pm] 153
Density at STP [g/cm3] 6.11
Number of protons 23
Number of neutrons (typical isotopes) 51
Number of electrons 23
Electron configuration [Ar] 3d3 4s2
Oxidation states +2,3,4,5
Electron affinity [kJ/mol] 50.6
Electronegativity [Pauling scale] 1.63
First ionization energy [eV] 6.7463

Atomic Number – Protons, Electrons and Neutrons in Vanadium

Proton Number - Atomic NumberVanadium is a chemical element with atomic number 23 which means there are 23 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Vanadium are 51.

Atomic Mass of Vanadium

Atomic mass of Vanadium is 50.9415 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Vanadium

The atomic radius of Vanadium atom is 153pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Vanadium is 23. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Vanadium is [Ar] 3d3 4s2.

Possible oxidation states are +2,3,4,5.

Density of Vanadium

Density of Vanadium is 6.11g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Vanadium-protons-neutrons-electrons-configuration

Vanadium-affinity-electronegativity-ionization

Electron Affinity – Vanadium

Electron affinity of Vanadium is 50.6 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Vanadium

Electronegativity of Vanadium is 1.63.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Vanadium is: χ = 1.63

First Ionization Energy of Vanadium

First Ionization Energy of Vanadium is 6.7463 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Vanadium atom, for example, requires the following ionization energy to remove the outermost electron.

V + IE → V+ + e−        IE = 6.7463 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Vanadium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Vanadium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Vanadium

 

Titanium – Periodic Table – Atomic Properties

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Titanium-density-atomic-number-mass-radius

Titanium is a lustrous transition metal with a silver color, low density, and high strength. Titanium is resistant to corrosion in sea water, aqua regia, and chlorine. Titanium can be used in surface condensers. These condensers use tubes that are usually made of stainless steel, copper alloys, or titanium depending on several selection criteria (such as thermal conductivity or corrosion resistance). Titanium condenser tubes are usually the best technical choice, however titanium is very expensive material and the use of titanium condenser tubes is associated with very high initial costs.

Summary

Element Titanium
Atomic number 22
Atomic mass [amu] 47.867
Atomic mass [pm] 160
Density at STP [g/cm3] 4.507
Number of protons 22
Number of neutrons (typical isotopes) 46-50
Number of electrons 22
Electron configuration [Ar] 3d2 4s2
Oxidation states +2,3,4
Electron affinity [kJ/mol] 7.6
Electronegativity [Pauling scale] 1.54
First ionization energy [eV] 6.8282

Atomic Number – Protons, Electrons and Neutrons in Titanium

Proton Number - Atomic NumberTitanium is a chemical element with atomic number 22 which means there are 22 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Titanium are 46-50.

Atomic Mass of Titanium

Atomic mass of Titanium is 47.867 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Titanium

The atomic radius of Titanium atom is 160pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Titanium is 22. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Titanium is [Ar] 3d2 4s2.

Possible oxidation states are +2,3,4.

Density of Titanium

Density of Titanium is 4.507g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Titanium-protons-neutrons-electrons-configuration

Titanium-affinity-electronegativity-ionization

Electron Affinity – Titanium

Electron affinity of Titanium is 7.6 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Titanium

Electronegativity of Titanium is 1.54.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Titanium is: χ = 1.54

First Ionization Energy of Titanium

First Ionization Energy of Titanium is 6.8282 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Titanium atom, for example, requires the following ionization energy to remove the outermost electron.

Ti + IE → Ti+ + e−        IE = 6.8282 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Titanium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Titanium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Titanium

 

Scandium – Periodic Table – Atomic Properties

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Scandium-density-atomic-number-mass-radius

Scandium is a silvery-white metallic d-block element, it has historically been sometimes classified as a rare-earth element, together with yttrium and the lanthanides.

Summary

Element Scandium
Atomic number 21
Atomic mass [amu] 44.9559
Atomic mass [pm] 170
Density at STP [g/cm3] 2.985
Number of protons 21
Number of neutrons (typical isotopes) 45
Number of electrons 21
Electron configuration [Ar] 3d1 4s2
Oxidation states +3
Electron affinity [kJ/mol] 18.1
Electronegativity [Pauling scale] 1.36
First ionization energy [eV] 6.5614

Atomic Number – Protons, Electrons and Neutrons in Scandium

Proton Number - Atomic NumberScandium is a chemical element with atomic number 21 which means there are 21 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Scandium are 45.

Atomic Mass of Scandium

Atomic mass of Scandium is 44.9559 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Scandium

The atomic radius of Scandium atom is 170pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Scandium is 21. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Scandium is [Ar] 3d1 4s2.

Possible oxidation states are +3.

Density of Scandium

Density of Scandium is 2.985g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Scandium-protons-neutrons-electrons-configuration

Scandium-affinity-electronegativity-ionization

Electron Affinity – Scandium

Electron affinity of Scandium is 18.1 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Scandium

Electronegativity of Scandium is 1.36.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Scandium is: χ = 1.36

First Ionization Energy of Scandium

First Ionization Energy of Scandium is 6.5614 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Scandium atom, for example, requires the following ionization energy to remove the outermost electron.

Sc + IE → Sc+ + e−        IE = 6.5614 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Scandium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Scandium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Scandium

 

Calcium – Periodic Table – Atomic Properties

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Calcium-density-atomic-number-mass-radius

Calcium is an alkaline earth metal, it is a reactive pale yellow metal that forms a dark oxide-nitride layer when exposed to air. Its physical and chemical properties are most similar to its heavier homologues strontium and barium. It is the fifth most abundant element in Earth’s crust and the third most abundant metal, after iron and aluminium.

Summary

Element Calcium
Atomic number 20
Atomic mass [amu] 40.078
Atomic mass [pm] 176
Density at STP [g/cm3] 1.55
Number of protons 20
Number of neutrons (typical isotopes) 40; 42; 43; 44; 46
Number of electrons 20
Electron configuration [Ar] 4s2
Oxidation states +2
Electron affinity [kJ/mol] 2.37
Electronegativity [Pauling scale] 1
First ionization energy [eV] 6.1132

Atomic Number – Protons, Electrons and Neutrons in Calcium

Proton Number - Atomic NumberCalcium is a chemical element with atomic number 20 which means there are 20 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Calcium are 40; 42; 43; 44; 46.

Atomic Mass of Calcium

Atomic mass of Calcium is 40.078 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Calcium

The atomic radius of Calcium atom is 176pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Calcium is 20. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Calcium is [Ar] 4s2.

Possible oxidation states are +2.

Density of Calcium

Density of Calcium is 1.55g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Calcium-protons-neutrons-electrons-configuration

Calcium-affinity-electronegativity-ionization

Electron Affinity – Calcium

Electron affinity of Calcium is 2.37 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Calcium

Electronegativity of Calcium is 1.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Calcium is: χ = 1

First Ionization Energy of Calcium

First Ionization Energy of Calcium is 6.1132 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Calcium atom, for example, requires the following ionization energy to remove the outermost electron.

Ca + IE → Ca+ + e−        IE = 6.1132 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Calcium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Calcium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Calcium

 

Potassium – Periodic Table – Atomic Properties

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Potassium-density-atomic-number-mass-radius

Potassium was first isolated from potash, the ashes of plants, from which its name derives. In the periodic table, potassium is one of the alkali metals. All of the alkali metals have a single valence electron in the outer electron shell, which is easily removed to create an ion with a positive charge – a cation, which combines with anions to form salts. Naturally occurring potassium is composed of three isotopes, of which 40K is radioactive. Traces of 40K are found in all potassium, and it is the most common radioisotope in the human body.

Summary

Element Potassium
Atomic number 19
Atomic mass [amu] 39.0983
Atomic mass [pm] 203
Density at STP [g/cm3] 0.856
Number of protons 19
Number of neutrons (typical isotopes) 39; 41
Number of electrons 19
Electron configuration [Ar] 4s1
Oxidation states +1
Electron affinity [kJ/mol] 48.4
Electronegativity [Pauling scale] 0.82
First ionization energy [eV] 4.3407

Atomic Number – Protons, Electrons and Neutrons in Potassium

Proton Number - Atomic NumberPotassium is a chemical element with atomic number 19 which means there are 19 protons in its nucleus. Total number of protons in the nucleus is called the atomic number of the atom and is given the symbol Z. The total electrical charge of the nucleus is therefore +Ze, where e (elementary charge) equals to 1,602 x 10-19 coulombs.

The total number of neutrons in the nucleus of an atom is called the neutron number of the atom and is given the symbol N. Neutron number plus atomic number equals atomic mass number: N+Z=A. The difference between the neutron number and the atomic number is known as the neutron excess: D = N – Z = A – 2Z.

For stable elements, there is usually a variety of stable isotopes. Isotopes are nuclides that have the same atomic number and are therefore the same element, but differ in the number of neutrons. Mass numbers of typical isotopes of Potassium are 39; 41.

Atomic Mass of Potassium

Atomic mass of Potassium is 39.0983 u. 

The atomic mass is the mass of an atom. The atomic mass or relative isotopic mass refers to the mass of a single particle, and therefore is tied to a certain specific isotope of an element. The atomic mass is carried by the atomic nucleus, which occupies only about 10-12 of the total volume of the atom or less, but it contains all the positive charge and at least 99.95% of the total mass of the atom. Note that, each element may contain more isotopes, therefore this resulting atomic mass is calculated from naturally-occuring isotopes and their abundance.

Atomic Radius of Potassium

The atomic radius of Potassium atom is 203pm (covalent radius).

Atomic Radius of Chemical Elements

It must be noted, atoms lack a well-defined outer boundary. The atomic radius of a chemical element is a measure of the distance out to which the electron cloud extends from the nucleus. However, this assumes the atom to exhibit a spherical shape, which is only obeyed for atoms in vacuum or free space. Therefore, there are various non-equivalent definitions of atomic radius.

Electrons and Electron Configuration

The number of electrons in an electrically-neutral atom is the same as the number of protons in the nucleus. Therefore, the number of electrons in neutral atom of Potassium is 19. Each electron is influenced by the electric fields produced by the positive nuclear charge and the other (Z – 1) negative electrons in the atom.

Since the number of electrons and their arrangement are responsible for the chemical behavior of atoms, the atomic number identifies the various chemical elements. The configuration of these electrons follows from the principles of quantum mechanics. The number of electrons in each element’s electron shells, particularly the outermost valence shell, is the primary factor in determining its chemical bonding behavior. In the periodic table, the elements are listed in order of increasing atomic number Z.

Electron configuration of Potassium is [Ar] 4s1.

Possible oxidation states are +1.

Density of Potassium

Density of Potassium is 0.856g/cm3.

Typical densities of various substances are at atmospheric pressure.

Density is defined as the mass per unit volume. It is an intensive property, which is mathematically defined as mass divided by volume:

ρ = m/V

Atomic Masses of Elements

Periodic Table of Elements - atomic mass

Atomic Radii of Elements

Periodic Table of Elements - atomic radius

Densities of Elements

Periodic Table of Elements - density

Potassium-protons-neutrons-electrons-configuration

Potassium-affinity-electronegativity-ionization

Electron Affinity – Potassium

Electron affinity of Potassium is 48.4 kJ/mol.

In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as:

the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.

X + e– → X– + energy        Affinity = – ∆H

In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. Electron affinities are more difficult to measure than ionization energies.

Electronegativity of Potassium

Electronegativity of Potassium is 0.82.

Electronegativity, symbol χ, is a chemical property that describes the tendency of an atom to attract electrons towards this atom. For this purposes, a dimensionless quantity the Pauling scale, symbol χ, is the most commonly used.

The electronegativity of Potassium is: χ = 0.82

First Ionization Energy of Potassium

First Ionization Energy of Potassium is 4.3407 eV.

Ionization energy, also called ionization potential, is the energy necessary to remove an electron from the neutral atom.

X + energy → X+ + e−

where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed (positive ion), and e− is the removed electron.

A Potassium atom, for example, requires the following ionization energy to remove the outermost electron.

K + IE → K+ + e−        IE = 4.3407 eV

Electronegativity of Elements

Periodic Table of Elements - electronegativity

Ionization Energy of Elements

Periodic Table of Elements - ionization energy

Potassium-periodic-table

Source: www.luciteria.com

 

Properties of other elements

Potassium - Comparison of Atomic Properties

Periodic Table in 8K resolution

Other properties of Potassium