Element FolioElement FolioAdvanced Materials Intelligence
⌕
LearnVideosCalculatorsTools
PSEMIC ERP ↗

Element Folio

Category: Elements & Periodic Table

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

  • Sulfur (S): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Sulfur (S) has atomic number 16 and is classified as a nonmetal. It sits in Group 16, period 3 of the periodic table. Its practical relevance includes sulfuric acid, fertilizers, rubber vulcanization, petroleum processing and chemical manufacture.

    Quick facts

    Atomic number 16 Symbol S
    Relative atomic mass 32.06 State at room temperature Solid
    Group 16 Period 3
    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.

    Sulfur belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Sulfur matters

    In engineering and technology, sulfur is associated with sulfuric acid, fertilizers, rubber vulcanization, petroleum processing and chemical manufacture. 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 sulfur depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Sulfur 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) · Selenium (Se) · Tellurium (Te) · Phosphorus (P)

    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

  • Chlorine (Cl): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Chlorine (Cl) has atomic number 17 and is classified as a halogen. It sits in Group 17, period 3 of the periodic table. Its practical relevance includes water disinfection, PVC production, bleaching, pharmaceuticals and industrial chemical synthesis.

    Quick facts

    Atomic number 17 Symbol Cl
    Relative atomic mass 35.45 State at room temperature Gas
    Group 17 Period 3
    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.

    Chlorine belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Chlorine matters

    In engineering and technology, chlorine is associated with water disinfection, PVC production, bleaching, pharmaceuticals and industrial chemical 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 chlorine depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Chlorine 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) · Bromine (Br) · Iodine (I) · Sulfur (S)

    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

  • Argon (Ar): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Argon (Ar) has atomic number 18 and is classified as a noble gas. It sits in Group 18, period 3 of the periodic table. Its practical relevance includes shielding gas for welding, inert processing atmospheres, lighting and semiconductor manufacture.

    Quick facts

    Atomic number 18 Symbol Ar
    Relative atomic mass 39.948 State at room temperature Gas
    Group 18 Period 3
    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.

    Argon belongs to period 3. Its position helps explain recurring trends such as atomic size, bonding behavior, oxidation states and the way it interacts with neighboring elements.

    Why Argon matters

    In engineering and technology, argon is associated with shielding gas for welding, inert processing atmospheres, lighting and semiconductor manufacture. 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 argon depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Argon 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) · Krypton (Kr) · Chlorine (Cl)

    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

  • Potassium (K): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Potassium (K) has atomic number 19 and is classified as a alkali metal. It sits in Group 1, period 4 of the periodic table. Its practical relevance includes fertilizers, glass production, soaps, specialty chemicals and biological systems.

    Quick facts

    Atomic number 19 Symbol K
    Relative atomic mass 39.0983 State at room temperature Solid
    Group 1 Period 4
    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.

    Potassium 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 Potassium matters

    In engineering and technology, potassium is associated with fertilizers, glass production, soaps, specialty chemicals and biological 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 potassium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Potassium 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) · Argon (Ar)

    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

  • Calcium (Ca): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Calcium (Ca) has atomic number 20 and is classified as a alkaline earth metal. It sits in Group 2, period 4 of the periodic table. Its practical relevance includes cement and lime, metallurgy, water treatment, construction materials and biological systems.

    Quick facts

    Atomic number 20 Symbol Ca
    Relative atomic mass 40.078 State at room temperature Solid
    Group 2 Period 4
    Classification alkaline earth metal Block s-block

    Position in the periodic table

    Alkaline earth metals are reactive s-block metals that commonly form +2 ions. Their compounds are important in construction, refractories, metallurgy, chemicals and biological systems.

    Calcium 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 Calcium matters

    In engineering and technology, calcium is associated with cement and lime, metallurgy, water treatment, construction materials and biological 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 calcium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Calcium 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

    Beryllium (Be) · Magnesium (Mg) · Strontium (Sr) · Potassium (K)

    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

  • Scandium (Sc): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Scandium (Sc) has atomic number 21 and is classified as a transition metal. It sits in Group 3, period 4 of the periodic table. Its practical relevance includes aluminum-scandium alloys, high-intensity lamps, aerospace research and specialty ceramics.

    Quick facts

    Atomic number 21 Symbol Sc
    Relative atomic mass 44.9559 State at room temperature Solid
    Group 3 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.

    Scandium 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 Scandium matters

    In engineering and technology, scandium is associated with aluminum-scandium alloys, high-intensity lamps, aerospace research and specialty ceramics. 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 scandium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Scandium 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

    Yttrium (Y) · Lutetium (Lu) · Lawrencium (Lr) · Calcium (Ca)

    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

  • Titanium (Ti): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Titanium (Ti) has atomic number 22 and is classified as a transition metal. It sits in Group 4, period 4 of the periodic table. Its practical relevance includes aerospace structures, chemical equipment, medical implants, marine service and titanium dioxide pigments.

    Quick facts

    Atomic number 22 Symbol Ti
    Relative atomic mass 47.867 State at room temperature Solid
    Group 4 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.

    Titanium 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 Titanium matters

    In engineering and technology, titanium is associated with aerospace structures, chemical equipment, medical implants, marine service and titanium dioxide pigments. 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 titanium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Titanium 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

    Zirconium (Zr) · Hafnium (Hf) · Rutherfordium (Rf) · Scandium (Sc)

    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

  • Vanadium (V): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Vanadium (V) has atomic number 23 and is classified as a transition metal. It sits in Group 5, period 4 of the periodic table. Its practical relevance includes high-strength steels, superalloys, catalysts and vanadium redox-flow batteries.

    Quick facts

    Atomic number 23 Symbol V
    Relative atomic mass 50.9415 State at room temperature Solid
    Group 5 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.

    Vanadium 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 Vanadium matters

    In engineering and technology, vanadium is associated with high-strength steels, superalloys, catalysts and vanadium redox-flow batteries. 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 vanadium depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Vanadium 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

    Niobium (Nb) · Tantalum (Ta) · Dubnium (Db) · Titanium (Ti)

    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

  • Manganese (Mn): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Manganese (Mn) has atomic number 25 and is classified as a transition metal. It sits in Group 7, period 4 of the periodic table. Its practical relevance includes steelmaking, aluminum alloys, dry-cell batteries and chemical oxidants.

    Quick facts

    Atomic number 25 Symbol Mn
    Relative atomic mass 54.9380 State at room temperature Solid
    Group 7 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.

    Manganese 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 Manganese matters

    In engineering and technology, manganese is associated with steelmaking, aluminum alloys, dry-cell batteries and chemical oxidants. 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 manganese depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Manganese 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

    Technetium (Tc) · Rhenium (Re) · Bohrium (Bh) · Chromium (Cr)

    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

  • Iron (Fe): Properties, Uses and Periodic Table Guide

    Periodic Table Guide

    Iron (Fe) has atomic number 26 and is classified as a transition metal. It sits in Group 8, period 4 of the periodic table. Its practical relevance includes structural steel, machinery, transportation, pipelines, tools and infrastructure.

    Quick facts

    Atomic number 26 Symbol Fe
    Relative atomic mass 55.845 State at room temperature Solid
    Group 8 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.

    Iron 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 Iron matters

    In engineering and technology, iron is associated with structural steel, machinery, transportation, pipelines, tools and infrastructure. 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 iron depends on concentration and interaction with the other constituents.

    Safety and handling

    The hazards associated with Iron 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

    Ruthenium (Ru) · Osmium (Os) · Hassium (Hs) · Manganese (Mn)

    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