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Element Folio

Category: Elements & Periodic Table

Element profiles, periodic trends, groups and periodic-table reference guides.

  • Cobalt (Co): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Cobalt (Co) has atomic number 27 and is classified as a transition metal. It sits in Group 9, period 4 of the periodic table. Its practical relevance includes superalloys, rechargeable batteries, hard metals, pigments and permanent magnets.

    Quick facts

    Atomic number 27 Symbol Co
    Relative atomic mass 58.9332 State at room temperature Solid
    Group 9 Period 4
    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.

    Cobalt belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Cobalt matters

    In engineering and technology, cobalt is associated with superalloys, rechargeable batteries, hard metals, pigments and permanent magnets. 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 cobalt depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Cobalt 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

    Rhodium (Rh) · Iridium (Ir) · Meitnerium (Mt) · Iron (Fe)

    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

  • Nickel (Ni): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Nickel (Ni) has atomic number 28 and is classified as a transition metal. It sits in Group 10, period 4 of the periodic table. Its practical relevance includes stainless steels, superalloys, batteries, plating, catalysts and corrosion-resistant equipment.

    Quick facts

    Atomic number 28 Symbol Ni
    Relative atomic mass 58.6934 State at room temperature Solid
    Group 10 Period 4
    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.

    Nickel belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Nickel matters

    In engineering and technology, nickel is associated with stainless steels, superalloys, batteries, plating, catalysts and corrosion-resistant equipment. 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 nickel depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Nickel 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

    Palladium (Pd) · Platinum (Pt) · Darmstadtium (Ds) · Cobalt (Co)

    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

  • Copper (Cu): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Copper (Cu) has atomic number 29 and is classified as a transition metal. It sits in Group 11, period 4 of the periodic table. Its practical relevance includes electrical wiring, motors, transformers, heat exchangers, plumbing and electronic systems.

    Quick facts

    Atomic number 29 Symbol Cu
    Relative atomic mass 63.546 State at room temperature Solid
    Group 11 Period 4
    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.

    Copper belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Copper matters

    In engineering and technology, copper is associated with electrical wiring, motors, transformers, heat exchangers, plumbing and electronic systems. 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 copper depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Copper 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

    Silver (Ag) · Gold (Au) · Roentgenium (Rg) · Nickel (Ni)

    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

  • Gallium (Ga): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Gallium (Ga) has atomic number 31 and is classified as a post-transition metal. It sits in Group 13, period 4 of the periodic table. Its practical relevance includes gallium-arsenide and gallium-nitride semiconductors, LEDs, RF electronics and solar technologies.

    Quick facts

    Atomic number 31 Symbol Ga
    Relative atomic mass 69.723 State at room temperature Solid
    Group 13 Period 4
    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.

    Gallium belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Gallium matters

    In engineering and technology, gallium is associated with gallium-arsenide and gallium-nitride semiconductors, LEDs, RF electronics and solar technologies. 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 gallium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Gallium 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

    Boron (B) · Aluminum (Al) · Indium (In) · Zinc (Zn)

    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

  • Germanium (Ge): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Germanium (Ge) has atomic number 32 and is classified as a metalloid. It sits in Group 14, period 4 of the periodic table. Its practical relevance includes fiber-optic systems, infrared optics, semiconductors and high-efficiency solar cells.

    Quick facts

    Atomic number 32 Symbol Ge
    Relative atomic mass 72.630 State at room temperature Solid
    Group 14 Period 4
    Classification metalloid Block p-block

    Position in the periodic table

    Metalloids sit near the boundary between metals and nonmetals. Their intermediate electrical and chemical behavior makes several of them especially important in semiconductors, glass, ceramics and electronic materials.

    Germanium belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Germanium matters

    In engineering and technology, germanium is associated with fiber-optic systems, infrared optics, semiconductors and high-efficiency solar cells. 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 germanium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Germanium 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

    Carbon (C) · Silicon (Si) · Tin (Sn) · Gallium (Ga)

    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

  • Arsenic (As): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Arsenic (As) has atomic number 33 and is classified as a metalloid. It sits in Group 15, period 4 of the periodic table. Its practical relevance includes compound semiconductors, specialty alloys and limited industrial chemical applications under strict controls.

    Quick facts

    Atomic number 33 Symbol As
    Relative atomic mass 74.9216 State at room temperature Solid
    Group 15 Period 4
    Classification metalloid Block p-block

    Position in the periodic table

    Metalloids sit near the boundary between metals and nonmetals. Their intermediate electrical and chemical behavior makes several of them especially important in semiconductors, glass, ceramics and electronic materials.

    Arsenic belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Arsenic matters

    In engineering and technology, arsenic is associated with compound semiconductors, specialty alloys and limited industrial chemical 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 arsenic depends on concentration and interaction with the other constituents.

    Safety and handling

    Arsenic 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

    Nitrogen (N) · Phosphorus (P) · Antimony (Sb) · Germanium (Ge)

    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

  • Selenium (Se): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Selenium (Se) has atomic number 34 and is classified as a nonmetal. It sits in Group 16, period 4 of the periodic table. Its practical relevance includes photovoltaics, glassmaking, electronics, pigments and metallurgical additives.

    Quick facts

    Atomic number 34 Symbol Se
    Relative atomic mass 78.971 State at room temperature Solid
    Group 16 Period 4
    Classification nonmetal Block p-block

    Position in the periodic table

    Nonmetals show very different bonding and physical behavior from metals. They are essential to chemistry, energy, biological systems and many modern materials, often appearing as gases, molecular solids or network structures.

    Selenium belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Selenium matters

    In engineering and technology, selenium is associated with photovoltaics, glassmaking, electronics, pigments and metallurgical additives. 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 selenium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Selenium 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

    Oxygen (O) · Sulfur (S) · Tellurium (Te) · Arsenic (As)

    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

  • Bromine (Br): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Bromine (Br) has atomic number 35 and is classified as a halogen. It sits in Group 17, period 4 of the periodic table. Its practical relevance includes flame-retardant chemistry, drilling fluids, water treatment and specialty organic synthesis.

    Quick facts

    Atomic number 35 Symbol Br
    Relative atomic mass 79.904 State at room temperature Liquid
    Group 17 Period 4
    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.

    Bromine belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Bromine matters

    In engineering and technology, bromine is associated with flame-retardant chemistry, drilling fluids, water treatment and specialty organic synthesis. 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 bromine depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Bromine 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

    Fluorine (F) · Chlorine (Cl) · Iodine (I) · Selenium (Se)

    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

  • Krypton (Kr): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Krypton (Kr) has atomic number 36 and is classified as a noble gas. It sits in Group 18, period 4 of the periodic table. Its practical relevance includes specialty lighting, lasers, insulating window fills and scientific instrumentation.

    Quick facts

    Atomic number 36 Symbol Kr
    Relative atomic mass 83.798 State at room temperature Gas
    Group 18 Period 4
    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.

    Krypton belongs to period 4. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Krypton matters

    In engineering and technology, krypton is associated with specialty lighting, lasers, insulating window fills and scientific instrumentation. 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 krypton depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Krypton 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

    Helium (He) · Neon (Ne) · Argon (Ar) · Bromine (Br)

    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

  • Rubidium (Rb): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Rubidium (Rb) has atomic number 37 and is classified as a alkali metal. It sits in Group 1, period 5 of the periodic table. Its practical relevance includes research, atomic-frequency standards, specialty glass and photoelectric applications.

    Quick facts

    Atomic number 37 Symbol Rb
    Relative atomic mass 85.4678 State at room temperature Solid
    Group 1 Period 5
    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.

    Rubidium belongs to period 5. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Rubidium matters

    In engineering and technology, rubidium is associated with research, atomic-frequency standards, specialty glass and photoelectric applications. 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 rubidium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Rubidium 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

    Hydrogen (H) · Lithium (Li) · Sodium (Na) · Krypton (Kr)

    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