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Element Folio

Category: Advanced Materials Intelligence

Research, breakthroughs and emerging technologies across advanced materials science.

  • Platinum (Pt): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Platinum (Pt) has atomic number 78 and is classified as a transition metal. It sits in Group 10, period 6 of the periodic table. Its practical relevance includes catalysts, fuel cells, laboratory equipment, jewelry and high-temperature sensors.

    Quick facts

    Atomic number 78 Symbol Pt
    Relative atomic mass 195.084 State at room temperature Solid
    Group 10 Period 6
    Classification transition metal Block d-block

    Position in the periodic table

    Transition metals occupy the d-block and are central to structural alloys, catalysis, electrical systems and high-temperature engineering. Many display multiple oxidation states and form useful intermetallics or complex alloys.

    Platinum belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Platinum matters

    In engineering and technology, platinum is associated with catalysts, fuel cells, laboratory equipment, jewelry and high-temperature sensors. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of platinum depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Platinum depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Nickel (Ni) · Palladium (Pd) · Darmstadtium (Ds) · Iridium (Ir)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Gold (Au): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Gold (Au) has atomic number 79 and is classified as a transition metal. It sits in Group 11, period 6 of the periodic table. Its practical relevance includes electronics, connectors, aerospace coatings, dentistry, jewelry and financial reserves.

    Quick facts

    Atomic number 79 Symbol Au
    Relative atomic mass 196.96657 State at room temperature Solid
    Group 11 Period 6
    Classification transition metal Block d-block

    Position in the periodic table

    Transition metals occupy the d-block and are central to structural alloys, catalysis, electrical systems and high-temperature engineering. Many display multiple oxidation states and form useful intermetallics or complex alloys.

    Gold belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Gold matters

    In engineering and technology, gold is associated with electronics, connectors, aerospace coatings, dentistry, jewelry and financial reserves. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of gold depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Gold depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Copper (Cu) · Silver (Ag) · Roentgenium (Rg) · Platinum (Pt)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Mercury (Hg): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Mercury (Hg) has atomic number 80 and is classified as a transition metal. It sits in Group 12, period 6 of the periodic table. Its practical relevance includes scientific instruments, lamps and switches in legacy or restricted applications because of toxicity.

    Quick facts

    Atomic number 80 Symbol Hg
    Relative atomic mass 200.592 State at room temperature Liquid
    Group 12 Period 6
    Classification transition metal Block d-block

    Position in the periodic table

    Transition metals occupy the d-block and are central to structural alloys, catalysis, electrical systems and high-temperature engineering. Many display multiple oxidation states and form useful intermetallics or complex alloys.

    Mercury belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Mercury matters

    In engineering and technology, mercury is associated with scientific instruments, lamps and switches in legacy or restricted applications because of toxicity. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of mercury depends on concentration and interaction with the other constituents.

    Safety and handling

    Mercury and several of its compounds can present significant toxicological hazards. Exposure limits, waste controls and the exact chemical form must be considered before industrial use.

    Related elements

    Zinc (Zn) · Cadmium (Cd) · Copernicium (Cn) · Gold (Au)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Thallium (Tl): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Thallium (Tl) has atomic number 81 and is classified as a post-transition metal. It sits in Group 13, period 6 of the periodic table. Its practical relevance includes specialty electronics, infrared optics and research applications under strict toxicity controls.

    Quick facts

    Atomic number 81 Symbol Tl
    Relative atomic mass 204.38 State at room temperature Solid
    Group 13 Period 6
    Classification post-transition metal Block p-block

    Position in the periodic table

    Post-transition metals lie mainly in the p-block and often combine metallic conductivity with comparatively low melting points or distinctive alloying behavior. Their applications span electronics, solders, coatings and specialized process materials.

    Thallium belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Thallium matters

    In engineering and technology, thallium is associated with specialty electronics, infrared optics and research applications under strict toxicity controls. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of thallium depends on concentration and interaction with the other constituents.

    Safety and handling

    Thallium and several of its compounds can present significant toxicological hazards. Exposure limits, waste controls and the exact chemical form must be considered before industrial use.

    Related elements

    Boron (B) · Aluminum (Al) · Gallium (Ga) · Mercury (Hg)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Lead (Pb): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Lead (Pb) has atomic number 82 and is classified as a post-transition metal. It sits in Group 14, period 6 of the periodic table. Its practical relevance includes lead-acid batteries, radiation shielding, weights and legacy construction applications under strict controls.

    Quick facts

    Atomic number 82 Symbol Pb
    Relative atomic mass 207.2 State at room temperature Solid
    Group 14 Period 6
    Classification post-transition metal Block p-block

    Position in the periodic table

    Post-transition metals lie mainly in the p-block and often combine metallic conductivity with comparatively low melting points or distinctive alloying behavior. Their applications span electronics, solders, coatings and specialized process materials.

    Lead belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Lead matters

    In engineering and technology, lead is associated with lead-acid batteries, radiation shielding, weights and legacy construction applications under strict controls. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of lead depends on concentration and interaction with the other constituents.

    Safety and handling

    Lead and several of its compounds can present significant toxicological hazards. Exposure limits, waste controls and the exact chemical form must be considered before industrial use.

    Related elements

    Carbon (C) · Silicon (Si) · Germanium (Ge) · Thallium (Tl)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Bismuth (Bi): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Bismuth (Bi) has atomic number 83 and is classified as a post-transition metal. It sits in Group 15, period 6 of the periodic table. Its practical relevance includes pharmaceuticals, low-melting alloys, lead-free solders, pigments and thermoelectric research.

    Quick facts

    Atomic number 83 Symbol Bi
    Relative atomic mass 208.98040 State at room temperature Solid
    Group 15 Period 6
    Classification post-transition metal Block p-block

    Position in the periodic table

    Post-transition metals lie mainly in the p-block and often combine metallic conductivity with comparatively low melting points or distinctive alloying behavior. Their applications span electronics, solders, coatings and specialized process materials.

    Bismuth belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Bismuth matters

    In engineering and technology, bismuth is associated with pharmaceuticals, low-melting alloys, lead-free solders, pigments and thermoelectric research. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of bismuth depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Bismuth depend on its physical form, purity, compounds, process temperature and exposure route. Engineering decisions should use the applicable safety data sheet and project-specific risk assessment.

    Related elements

    Nitrogen (N) · Phosphorus (P) · Arsenic (As) · Lead (Pb)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Polonium (Po): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Polonium (Po) has atomic number 84 and is classified as a post-transition metal. It sits in Group 16, period 6 of the periodic table. Its practical relevance includes research, specialized heat-source and antistatic applications historically, with severe radiological controls.

    Quick facts

    Atomic number 84 Symbol Po
    Relative atomic mass [209] State at room temperature Solid
    Group 16 Period 6
    Classification post-transition metal Block p-block

    Position in the periodic table

    Post-transition metals lie mainly in the p-block and often combine metallic conductivity with comparatively low melting points or distinctive alloying behavior. Their applications span electronics, solders, coatings and specialized process materials.

    Polonium belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Polonium matters

    In engineering and technology, polonium is associated with research, specialized heat-source and antistatic applications historically, with severe radiological controls. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of polonium depends on concentration and interaction with the other constituents.

    Safety and handling

    Polonium is radioactive, so any practical work involving it requires specialist radiological controls, approved facilities and isotope-specific procedures.

    Related elements

    Oxygen (O) · Sulfur (S) · Selenium (Se) · Bismuth (Bi)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Astatine (At): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Astatine (At) has atomic number 85 and is classified as a halogen. It sits in Group 17, period 6 of the periodic table. Its practical relevance includes research and experimental targeted alpha therapy because of its short-lived radioactive isotopes.

    Quick facts

    Atomic number 85 Symbol At
    Relative atomic mass [210] State at room temperature Solid
    Group 17 Period 6
    Classification halogen Block p-block

    Position in the periodic table

    Halogens are reactive p-block elements that commonly form -1 ions and many important salts or organic compounds. Their industrial value is substantial, but elemental forms and some compounds can require strict corrosion, toxicity or containment controls.

    Astatine belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Astatine matters

    In engineering and technology, astatine is associated with research and experimental targeted alpha therapy because of its short-lived radioactive isotopes. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of astatine depends on concentration and interaction with the other constituents.

    Safety and handling

    Astatine is radioactive, so any practical work involving it requires specialist radiological controls, approved facilities and isotope-specific procedures.

    Related elements

    Fluorine (F) · Chlorine (Cl) · Bromine (Br) · Polonium (Po)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Radon (Rn): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Radon (Rn) has atomic number 86 and is classified as a noble gas. It sits in Group 18, period 6 of the periodic table. Its practical relevance includes research only; it is primarily important as a naturally occurring radioactive health hazard.

    Quick facts

    Atomic number 86 Symbol Rn
    Relative atomic mass [222] State at room temperature Gas
    Group 18 Period 6
    Classification noble gas Block p-block

    Position in the periodic table

    Noble gases have filled valence shells and are relatively unreactive under ordinary conditions. Their inertness is valuable in lighting, welding, semiconductor processing, cryogenics and scientific instrumentation.

    Radon belongs to period 6. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Radon matters

    In engineering and technology, radon is associated with research only; it is primarily important as a naturally occurring radioactive health hazard. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of radon depends on concentration and interaction with the other constituents.

    Safety and handling

    Radon is radioactive, so any practical work involving it requires specialist radiological controls, approved facilities and isotope-specific procedures.

    Related elements

    Helium (He) · Neon (Ne) · Argon (Ar) · Astatine (At)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons

  • Francium (Fr): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Francium (Fr) has atomic number 87 and is classified as a alkali metal. It sits in Group 1, period 7 of the periodic table. Its practical relevance includes fundamental atomic and nuclear research because only minute short-lived quantities exist.

    Quick facts

    Atomic number 87 Symbol Fr
    Relative atomic mass [223] State at room temperature Solid
    Group 1 Period 7
    Classification alkali metal Block s-block

    Position in the periodic table

    Alkali metals are highly reactive s-block metals with one valence electron. Their chemistry is dominated by +1 oxidation states, and they require careful handling because several react vigorously with air or water.

    Francium belongs to period 7. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Francium matters

    In engineering and technology, francium is associated with fundamental atomic and nuclear research because only minute short-lived quantities exist. The importance of the element may come from the pure element itself, from compounds containing it, or from its role as an alloying, electronic, catalytic or nuclear material.

    Engineering and scientific context

    Material behavior should never be inferred from the element name alone. Purity, isotope composition, crystal structure, processing history, temperature and the surrounding chemical environment can all change performance. In alloys and compounds, the contribution of francium depends on concentration and interaction with the other constituents.

    Safety and handling

    Francium is radioactive, so any practical work involving it requires specialist radiological controls, approved facilities and isotope-specific procedures.

    Related elements

    Hydrogen (H) · Lithium (Li) · Sodium (Na) · Radon (Rn)

    Reference sources

    For authoritative element data and current standard atomic-weight guidance, consult the Royal Society of Chemistry Periodic Table and the IUPAC Periodic Table of the Elements.

    Continue exploring: Periodic Table · Materials Library · Material Properties · Comparisons