Nick Connor, Autor Material Properties

Bromine and Iodine – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of bromine and iodine, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Bromine vs Iodine.

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Bromine and Iodine – About Elements

Bromine

Bromine is the third-lightest halogen, and is a fuming red-brown liquid at room temperature that evaporates readily to form a similarly coloured gas. Its properties are thus intermediate between those of chlorine and iodine.

Iodine

Iodine is the heaviest of the stable halogens, it exists as a lustrous, purple-black metallic solid at standard conditions that sublimes readily to form a violet gas. Iodine is the least abundant of the stable halogens, being the sixty-first most abundant element. It is even less abundant than the so-called rare earths. It is the heaviest essential mineral nutrient.

Bromine in Periodic Table

Iodine in Periodic Table

Source: www.luciteria.com

Bromine and Iodine – Applications

Bromine

A wide variety of organobromine compounds are used in industry. Some are prepared from bromine and others are prepared from hydrogen bromide, which is obtained by burning hydrogen in bromine. Brominated flame retardants represent a commodity of growing importance, and make up the largest commercial use of bromine. One of the major uses of bromine is a water purifier/disinfectant, as an alternative to chlorine. Bromine compounds are effective pesticides, used both as soil fumigants in agriculture, particularly fruit-growing, and as a fumigant to prevent pests from attacking stored grain and other produce.

Iodine

In addition to nutrition products, iodine and iodine derivatives are used in a wide range of medical, agricultural, and industrial applications. About half of all produced iodine goes into various organoiodine compounds, another 15% remains as the pure element, another 15% is used to form potassium iodide, and another 15% for other inorganic iodine compounds. The leading application is in the production of X-ray contrast media (22%). Iodine’s high atomic number and density make it ideally suited for this application, as its presence in the body can help to increase contrast between tissues, organs, and blood vessels with similar X-ray densities. It is used as an antiseptic for external wounds. Another application driving the demand for iodine is in polarizing film in liquidcrystal display (LCD) screens.

Bromine and Iodine – Comparison in Table

Element	Bromine	Iodine
Density	3.12 g/cm3	4.94 g/cm3
Ultimate Tensile Strength	N/A	N/A
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	N/A	N/A
Mohs Scale	N/A	N/A
Brinell Hardness	N/A	N/A
Vickers Hardness	N/A	N/A
Melting Point	-7.3 °C	113.5 °C
Boiling Point	59 °C	184 °C
Thermal Conductivity	0.122 W/mK	0.449 W/mK
Thermal Expansion Coefficient	N/A	N/A
Specific Heat	0.473 J/g K	0.214 J/g K
Heat of Fusion	5.286 kJ/mol	7.824 kJ/mol
Heat of Vaporization	15.438 kJ/mol	20.752 kJ/mol

Selenium and Iodine – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of selenium and iodine, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Selenium vs Iodine.

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Selenium and Iodine – About Elements

Selenium

Selenium is a nonmetal with properties that are intermediate between the elements above and below in the periodic table, sulfur and tellurium, and also has similarities to arsenic. It rarely occurs in its elemental state or as pure ore compounds in the Earth’s crust.

Iodine

Selenium in Periodic Table

Iodine in Periodic Table

Source: www.luciteria.com

Selenium and Iodine – Applications

Selenium

The chief commercial uses for selenium today are glassmaking and pigments. Selenium finds applications in the various industries, for example, solar cells and photoconductor applications, manganese electrolysis, DC power surge protection or X-ray crystallography.

Iodine

Selenium and Iodine – Comparison in Table

Element	Selenium	Iodine
Density	4.819 g/cm3	4.94 g/cm3
Ultimate Tensile Strength	300 MPa	N/A
Yield Strength	150 MPa	N/A
Young’s Modulus of Elasticity	10 GPa	N/A
Mohs Scale	2	N/A
Brinell Hardness	740 MPa	N/A
Vickers Hardness	N/A	N/A
Melting Point	221 °C	113.5 °C
Boiling Point	685 °C	184 °C
Thermal Conductivity	2.04 W/mK	0.449 W/mK
Thermal Expansion Coefficient	37 µm/mK	N/A
Specific Heat	0.32 J/g K	0.214 J/g K
Heat of Fusion	6.694 kJ/mol	7.824 kJ/mol
Heat of Vaporization	37.7 kJ/mol	20.752 kJ/mol

Arsenic and Cadmium – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of arsenic and cadmium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Arsenic vs Cadmium.

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Arsenic and Cadmium – About Elements

Arsenic

Arsenic occurs in many minerals, usually in combination with sulfur and metals, but also as a pure elemental crystal. Arsenic is a metalloid.

Cadmium

Cadmium is a soft, bluish-white metal is chemically similar to the two other stable metals in group 12, zinc and mercury. In nuclear industry cadmium is commonly used as a thermal neutron absorber due to very high neutron absorption cross-section of 113Cd. 113Cd has specific absorption cross-section.

Arsenic in Periodic Table

Cadmium in Periodic Table

Source: www.luciteria.com

Arsenic and Cadmium – Applications

Arsenic

Arsenic is used as a doping agent in semiconductors (gallium arsenide) for solid-state devices. It is also used in bronzing, pyrotechnics and for hardening shot. Arsenic compounds can be used to make special glass and preserve wood.

Cadmium

Cadmium is primarily consumed for the production of rechargeable nickel cadmium batteries. In 2009, 86% of cadmium was used in batteries, predominantly in rechargeable nickel-cadmium batteries. Other end uses include pigments, coatings and plating, and as stabilizers for plastics. Solar cell manufacturing may become another significant market for cadmium in the future. In nuclear industry cadmium is commonly used as a thermal neutron absorber due to very high neutron absorption cross-section of 113Cd. 113Cd has specific absorption cross-section.

Arsenic and Cadmium – Comparison in Table

Element	Arsenic	Cadmium
Density	5.727 g/cm3	8.65 g/cm3
Ultimate Tensile Strength	N/A	75 MPa
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	8 GPa	50 GPa
Mohs Scale	3.5	2
Brinell Hardness	1440 MPa	203 MPa
Vickers Hardness	N/A	N/A
Melting Point	817 °C	321.07 °C
Boiling Point	614 °C	767 °C
Thermal Conductivity	50 W/mK	97 W/mK
Thermal Expansion Coefficient	5.6 µm/mK	30.8 µm/mK
Specific Heat	0.33 J/g K	0.23 J/g K
Heat of Fusion	N/A	6.192 kJ/mol
Heat of Vaporization	34.76 kJ/mol	99.57 kJ/mol

Arsenic and Antimony – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of arsenic and antimony, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Arsenic vs Antimony.

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Arsenic and Antimony – About Elements

Arsenic

Arsenic occurs in many minerals, usually in combination with sulfur and metals, but also as a pure elemental crystal. Arsenic is a metalloid.

Antimony

Antimony is a lustrous gray metalloid, it is found in nature mainly as the sulfide mineral stibnite. Antimony compounds have been known since ancient times and were powdered for use as medicine and cosmetics, often known by the Arabic name, kohl.

Arsenic in Periodic Table

Antimony in Periodic Table

Source: www.luciteria.com

Arsenic and Antimony – Applications

Arsenic

Antimony

The largest applications for metallic antimony are an alloy with lead and tin and the lead antimony plates in lead–acid batteries. Alloys of lead and tin with antimony have improved properties for solders, bullets, and plain bearings. Antimony can be used in fire retardants for many commercial and domestic products. Antimony trichloride is used in the manufacturing flame-proofing compounds as well as paints, ceramic enamels, glass and pottery. Other uses include ball bearings and mixing with alloys with percentages ranging from 1 to 20 greatly increasing the hardness and mechanical strength of the lead. The capability to strengthen already strong alloys is its largest and most widespread use.

Arsenic and Antimony – Comparison in Table

Element	Arsenic	Antimony
Density	5.727 g/cm3	6.697 g/cm3
Ultimate Tensile Strength	N/A	11 MPa
Yield Strength	N/A	N/A
Young’s Modulus of Elasticity	8 GPa	55 GPa
Mohs Scale	3.5	3.15
Brinell Hardness	1440 MPa	300 MPa
Vickers Hardness	N/A	N/A
Melting Point	817 °C	631 °C
Boiling Point	614 °C	1950 °C
Thermal Conductivity	50 W/mK	24 W/mK
Thermal Expansion Coefficient	5.6 µm/mK	11 µm/mK
Specific Heat	0.33 J/g K	0.21 J/g K
Heat of Fusion	N/A	19.87 kJ/mol
Heat of Vaporization	34.76 kJ/mol	77.14 kJ/mol

Arsenic and Lead – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of arsenic and lead, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Arsenic vs Lead.

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Arsenic and Lead – About Elements

Arsenic

Arsenic occurs in many minerals, usually in combination with sulfur and metals, but also as a pure elemental crystal. Arsenic is a metalloid.

Lead

Lead is a heavy metal that is denser than most common materials. Lead is soft and malleable, and has a relatively low melting point. Lead is widely used as a gamma shield. Major advantage of lead shield is in its compactness due to its higher density. Lead has the highest atomic number of any stable element and concludes three major decay chains of heavier elements.

Arsenic in Periodic Table

Lead in Periodic Table

Source: www.luciteria.com

Arsenic and Lead – Applications

Arsenic

Lead

Lead metal has several useful mechanical properties, including high density, low melting point, ductility, and relative inertness. Lead is widely used for car batteries, pigments, ammunition, cable sheathing, weights for lifting, weight belts for diving, lead crystal glass, radiation protection and in some solders. The largest use of lead in the early 21st century is in lead–acid batteries. The lead in batteries undergoes no direct contact with humans, so there are fewer toxicity concerns. Lead is used in high voltage power cables as sheathing material to prevent water diffusion into insulation; this use is decreasing as lead is being phased out. A lead is widely used as a gamma shield. Major advantage of lead shield is in its compactness due to its higher density. On the other hand depleted uranium is much more effective due to its higher Z. Depleted uranium is used for shielding in portable gamma ray sources.

Arsenic and Lead – Comparison in Table

Element	Arsenic	Lead
Density	5.727 g/cm3	11.34 g/cm3
Ultimate Tensile Strength	N/A	17 MPa
Yield Strength	N/A	5.5 MPa
Young’s Modulus of Elasticity	8 GPa	16 GPa
Mohs Scale	3.5	1.5
Brinell Hardness	1440 MPa	38 MPa
Vickers Hardness	N/A	N/A
Melting Point	817 °C	327.5 °C
Boiling Point	614 °C	1740 °C
Thermal Conductivity	50 W/mK	35 W/mK
Thermal Expansion Coefficient	5.6 µm/mK	28.9 µm/mK
Specific Heat	0.33 J/g K	0.13 J/g K
Heat of Fusion	N/A	4.799 kJ/mol
Heat of Vaporization	34.76 kJ/mol	177.7 kJ/mol

Zinc and Selenium – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of zinc and selenium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Zinc vs Selenium.

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Zinc and Selenium – About Elements

Zinc

In some respects zinc is chemically similar to magnesium: both elements exhibit only one normal oxidation state (+2), and the Zn2+ and Mg2+ ions are of similar size.

Selenium

Zinc in Periodic Table

Selenium in Periodic Table

Source: www.luciteria.com

Zinc and Selenium – Applications

Zinc

Corrosion-resistant zinc plating of iron (hot-dip galvanizing) is the major application for zinc. Coating of steel constitutes the largest single use of zinc, but it is used in large tonnages in zinc alloy castings, as zinc dust and oxide, and in wrought zinc products. Galvanized steel is just plain carbon steel that has been coated with a thin zinc layer. The zinc protects iron by corroding first, but zinc corrodes at much lower rates than do steel. Other applications are in electrical batteries, small non-structural castings, and alloys such as brass. A variety of zinc compounds are commonly used, such as zinc carbonate and zinc gluconate (as dietary supplements), zinc chloride (in deodorants), zinc pyrithione (anti-dandruff shampoos), zinc sulfide (in luminescent paints), and dimethylzinc or diethylzinc in the organic laboratory. A key part of the modern materials world in which zinc finds itself is recycling. Zinc, in common with all metals (and unlike synthetic materials) can be recycled indefinitely without degradation.

Selenium

Zinc and Selenium – Comparison in Table

Element	Zinc	Selenium
Density	7.14 g/cm3	4.819 g/cm3
Ultimate Tensile Strength	90 MPa	300 MPa
Yield Strength	75 MPa	150 MPa
Young’s Modulus of Elasticity	108 GPa	10 GPa
Mohs Scale	2.5	2
Brinell Hardness	330 MPa	740 MPa
Vickers Hardness	N/A	N/A
Melting Point	419.53 °C	221 °C
Boiling Point	907 °C	685 °C
Thermal Conductivity	116 W/mK	2.04 W/mK
Thermal Expansion Coefficient	30.2 µm/mK	37 µm/mK
Specific Heat	0.39 J/g K	0.23 J/g K
Heat of Fusion	7.322 kJ/mol	6.694 kJ/mol
Heat of Vaporization	115.3 kJ/mol	37.7 kJ/mol

Zinc and Indium – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of zinc and indium, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Zinc vs Indium.

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Zinc and Indium – About Elements

Zinc

In some respects zinc is chemically similar to magnesium: both elements exhibit only one normal oxidation state (+2), and the Zn2+ and Mg2+ ions are of similar size.

Indium

Indium is a post-transition metal that makes up 0.21 parts per million of the Earth’s crust. Very soft and malleable, indium has a melting point higher than sodium and gallium, but lower than lithium and tin. Chemically, indium is similar to gallium and thallium.

Zinc in Periodic Table

Indium in Periodic Table

Source: www.luciteria.com

Zinc and Indium – Applications

Zinc

Indium

The primary consumption of indium worldwide is LCD production. Demand rose rapidly from the late 1990s to 2010 with the popularity of LCD computer monitors and television sets, which now account for 50% of indium consumption. It is most notably used in the semiconductor industry, in low-melting-point metal alloys such as solders, in soft-metal high-vacuum seals, and in the production of transparent conductive coatings of indium tin oxide (ITO) on glass. Indium is considered a technology-critical element.

Zinc and Indium – Comparison in Table

Element	Zinc	Indium
Density	7.14 g/cm3	7.31 g/cm3
Ultimate Tensile Strength	90 MPa	2.5 MPa
Yield Strength	75 MPa	1 MPa
Young’s Modulus of Elasticity	108 GPa	11 GPa
Mohs Scale	2.5	1.2
Brinell Hardness	330 MPa	10 MPa
Vickers Hardness	N/A	N/A
Melting Point	419.53 °C	156.6 °C
Boiling Point	907 °C	2072 °C
Thermal Conductivity	116 W/mK	82 W/mK
Thermal Expansion Coefficient	30.2 µm/mK	32.1 µm/mK
Specific Heat	0.39 J/g K	0.23 J/g K
Heat of Fusion	7.322 kJ/mol	3.263 kJ/mol
Heat of Vaporization	115.3 kJ/mol	231.5 kJ/mol

Gallium and Arsenic – Comparison – Properties

2021-01-21 by Nick Connor

This article contains comparison of key thermal and atomic properties of gallium and arsenic, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Gallium vs Arsenic.

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Gallium and Arsenic – About Elements

Gallium

Gallium has similarities to the other metals of the group, aluminium, indium, and thallium. Gallium does not occur as a free element in nature, but as gallium(III) compounds in trace amounts in zinc ores and in bauxite.

Arsenic

Arsenic occurs in many minerals, usually in combination with sulfur and metals, but also as a pure elemental crystal. Arsenic is a metalloid.

Gallium in Periodic Table

Arsenic in Periodic Table

Source: www.luciteria.com

Gallium and Arsenic – Applications

Gallium

Gallium consumption is centred on the superconductor industry. Semiconductor applications dominate the commercial demand for gallium, accounting for 98% of the total. When alloyed with arsenic to produce gallium arsenide (GaAs), it can convert electricity to light. Due to such properties, it is used in LEDs, and has been found to produce less heat than silicon, rendering it suitable for use in supercomputers.

Arsenic

Gallium and Arsenic – Comparison in Table

Element	Gallium	Arsenic
Density	5.904 g/cm3	5.727 g/cm3
Ultimate Tensile Strength	15 MPa	N/A
Yield Strength	8 MPa	N/A
Young’s Modulus of Elasticity	9.8 GPa	8 GPa
Mohs Scale	1.5	3.5
Brinell Hardness	60 MPa	1440 MPa
Vickers Hardness	N/A	N/A
Melting Point	29.76 °C	817 °C
Boiling Point	2204 °C	614 °C
Thermal Conductivity	40.6 W/mK	50 W/mK
Thermal Expansion Coefficient	18 µm/mK	5.6 µm/mK
Specific Heat	0.37 J/g K	0.33 J/g K
Heat of Fusion	5.59 kJ/mol	N/A
Heat of Vaporization	258.7 kJ/mol	34.76 kJ/mol

Copper and Gold – Comparison – Properties

2021-07-232021-01-20 by Nick Connor

This article contains comparison of key thermal and atomic properties of copper and gold, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Copper vs Gold.

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Copper and Gold – About Elements

Copper

Copper is a soft, malleable, and ductile metal with very high thermal and electrical conductivity. A freshly exposed surface of pure copper has a reddish-orange color. Copper is used as a conductor of heat and electricity, as a building material, and as a constituent of various metal alloys, such as sterling silver used in jewelry, cupronickel used to make marine hardware and coins, and constantan used in strain gauges and thermocouples for temperature measurement.

Gold

Gold is a bright, slightly reddish yellow, dense, soft, malleable, and ductile metal. Gold is a transition metal and a group 11 element. It is one of the least reactive chemical elements and is solid under standard conditions. Gold is thought to have been produced in supernova nucleosynthesis, from the collision of neutron stars.

Copper in Periodic Table

Gold in Periodic Table

Source: www.luciteria.com

Copper and Gold – Applications

Copper

Historically, alloying copper with another metal, for example tin to make bronze, was first practiced about 4000 years after the discovery of copper smelting, and about 2000 years after “natural bronze” had come into general use. An ancient civilization is defined to be in the Bronze Age either by producing bronze by smelting its own copper and alloying with tin, arsenic, or other metals. The major applications of copper are electrical wire (60%), roofing and plumbing (20%), and industrial machinery (15%). Copper is used mostly as a pure metal, but when greater hardness is required, it is put into such alloys as brass and bronze (5% of total use). Copper and copper-based alloys including brasses (Cu-Zn) and bronzes (Cu-Sn) are widely used in different industrial and societal applications. Some of the common uses for brass alloys include costume jewelry, locks, hinges, gears, bearings, ammunition casings, automotive radiators, musical instruments, electronic packaging, and coins. Bronze, or bronze-like alloys and mixtures, were used for coins over a longer period. is still widely used today for springs, bearings, bushings, automobile transmission pilot bearings, and similar fittings, and is particularly common in the bearings of small electric motors. Brass and bronze are common engineering materials in modern architecture and primarily used for roofing and facade cladding due to their visual appearance.

Gold

Gold is used extensively in jewellery, either in its pure form or as an alloy. About 75% of all gold produced is used in the jewelry industry. Pure gold is too soft to stand up to the stresses applied to many jewelry items. Craftsmen learned that alloying gold with other metals such as copper, silver, and platinum would increase its durability. The term ‘carat’ indicates the amount of gold present in an alloy. 24-carat is pure gold, but it is very soft. 18- and 9-carat gold alloys are commonly used because they are more durable. Gold’s high malleability, ductility, resistance to corrosion and most other chemical reactions, and conductivity of electricity have led to its continued use in corrosion resistant electrical connectors in all types of computerized devices (its chief industrial use). Gold is also used in infrared shielding, colored-glass production, gold leafing, and tooth restoration. Only 10% of the world consumption of new gold produced goes to industry, but by far the most important industrial use for new gold is in fabrication of corrosion-free electrical connectors in computers and other electrical devices.

Copper and Gold – Comparison in Table

Element	Copper	Gold
Density	8.92 g/cm3	19.3 g/cm3
Ultimate Tensile Strength	210 MPa	220 MPa
Yield Strength	33 MPa	205 MPa
Young’s Modulus of Elasticity	120 GPa	79 GPa
Mohs Scale	3	2.75
Brinell Hardness	250 MPa	190 MPa
Vickers Hardness	350 MPa	215 MPa
Melting Point	1084.62 °C	1064 °C
Boiling Point	2562 °C	2970 °C
Thermal Conductivity	401 W/mK	320 W/mK
Thermal Expansion Coefficient	16.5 µm/mK	14.2 µm/mK
Specific Heat	0.38 J/g K	0.128 J/g K
Heat of Fusion	13.05 kJ/mol	12.55 kJ/mol
Heat of Vaporization	300.3 kJ/mol	334.4 kJ/mol

Copper and Silver – Comparison – Properties

2021-01-20 by Nick Connor

This article contains comparison of key thermal and atomic properties of copper and silver, two comparable chemical elements from the periodic table. It also contains basic descriptions and applications of both elements. Copper vs Silver.

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Copper and Silver – About Elements

Copper

Silver

Silver is a soft, white, lustrous transition metal, it exhibits the highest electrical conductivity, thermal conductivity, and reflectivity of any metal. The metal is found in the Earth’s crust in the pure, free elemental form (“native silver”), as an alloy with gold and other metals, and in minerals such as argentite and chlorargyrite. Most silver is produced as a byproduct of copper, gold, lead, and zinc refining.

Copper in Periodic Table

Silver in Periodic Table

Source: www.luciteria.com

Copper and Silver – Applications

Copper

Silver

Silver has long been valued as a precious metal. Silver metal is used in many bullion coins, sometimes alongside gold. Silver has many important, far-reaching technological and electronic applications. It’s used in everything from cell phones, computers and semiconductors to automobiles, water-purification systems and—because it is the best conductor of heat of all elements—spacecraft solar radiation tiles. Silver is of the upmost importance in photography (where approximately 30% of the U.S. Industrial consumption goes into this application). The medical uses of silver include its use in wound dressings, creams, and as an antibiotic coating on medical devices. Wound dressings containing silver sulfadiazine or silver nanomaterials may be used on external infections.

Copper and Silver – Comparison in Table

Element	Copper	Silver
Density	8.92 g/cm3	10.49 g/cm3
Ultimate Tensile Strength	210 MPa	110 MPa
Yield Strength	33 MPa	45 MPa
Young’s Modulus of Elasticity	120 GPa	83 GPa
Mohs Scale	3	3.25
Brinell Hardness	250 MPa	210 MPa
Vickers Hardness	350 MPa	251 MPa
Melting Point	1084.62 °C	961.78 °C
Boiling Point	2562 °C	2162 °C
Thermal Conductivity	401 W/mK	430 W/mK
Thermal Expansion Coefficient	16.5 µm/mK	18.9 µm/mK
Specific Heat	0.38 J/g K	0.235 J/g K
Heat of Fusion	13.05 kJ/mol	11.3 kJ/mol
Heat of Vaporization	300.3 kJ/mol	250.58 kJ/mol