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Understanding the Periodic Table: Elements, Properties, and Reactivity

Explore the diverse elements on the periodic table, from hydrogen to rare earth metals. Discover their properties, reactivity levels, and unique characteristics. Learn about valence electrons, electron shells, and chemical bonding.

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Understanding the Periodic Table: Elements, Properties, and Reactivity

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  1. Periodic Table

  2. hydrogen • highly reactive(chemical property), colorless, odorless gas (normally) • Highly flammable • * most common element found in the universe (90% + atoms)

  3. Alkali metals Group 1 • Very reactive (chemical property), do not occur freely in nature • Physical property- malleable, ductile, good conductor of heat and electricity, solid @ room temp. low densities, low melting pts. • Chemical property- explode if exposed to H₂O, produce chemicals, metals, glass, petr. products

  4. Alkaline earth metals group 2 • Metals, very reactive (chem. Prop.) • Most are good conductors of elect. (phy prop) • Give up 2 electrons during reactions • Never found free in nature

  5. Transitional metals group 3-12 • Chem: less reactive than groups 1 or 2 • Phys: ductile, malleable, good cond. of heat and elect. • Produce magnetic field: iron, cobalt, nickel • Used for: jewelry, industry (copper wiring) foods • Lanthanide and Actinide- Rare Earth Metals

  6. Other metals • Al, Ga, In, Sn, Tl, Pb, Bi • Phys. Prop: ductile, malleable, solids, high densities • Opaque- no luster, do not reflect light

  7. Metalloids • B, Si, Ge, As, Sb, Te, Po, At • Stairs • Have properties of both metals and nonmetals • Appearance varies, some semi-conductors • Useful in computers and calculators

  8. Halogens Group 17 • Halogens means “salt formers” • Compounds containing halogens=“salts” • Very reactive non-metals form salts when combined w/ metal (most) often bond w/ grp 1 elements, used to kill harmful micro-organisms in hospitals, purify drinking H₂O • Solids- Iodine, Astatine • Liquids- Bromine • Gas- Fluorine, Chlorine • (exist as molecule)

  9. Noble Gases Group 18 • Exist as gases • Non-metals, full outer energy levels • DO NOT REACT WITH OTHER ELEMENTS

  10. OTHER NON METALS • C, N, P, O, S, Se • Do not cond. Elect. or heat • Exist in either gases & solids • Phys. Prop.- brittle (break easily), not ductile, not malleable, no luster

  11. Rare Earth Metals Lanthanide and Actinides • Silver, silvery white/grey metals • Good conductors of elect. • LANTH- many forms, some magn. Props. • ACT- all radioactive

  12. Notes • Groups 13-16 are called by the 1st Element in the group • Contain a mixture of different types of elements • Ex. Grp 13- called the Boron Group contains 1 metalloid, 4 metals • Grp 14- called the Carbon Group contains 1 non-metal, 2 metalloids, 2 metals

  13. Notes • Green means- GO!! REACTIVE • Red means- STOP!! UNREACTIVE • Blue means- varied reactivity • Shared characteristics- Groups/Families • Periods (rows) • Group #’s - # of valence electrons for that group of elements • Period #’s- # of energy levels for those elements

  14. Valence Electrons • All the electrons on an element’s outermost energy level (shells) • Important in determining (deciding) how an atom reacts chemically w/ other atoms. • Bohr- nucleus w/ shells ● • Electron Dot diagram- uses ● ex. ●Al●

  15. Notes • Stable- full energy level “resist change” • Chemical bond- force that holds atoms together (strong attachment) • Covalent bond- atoms share electrons co-together- full energy level • Ions- atoms that gain or lose electrons become charged (+ or -) more electrons- more negative more protons + more positive • Ionic bond- oppos. Charged ions attract and form a bond.

  16. Electrons Shells • 1st- 2 • 2nd- 8 • 3rd- 8 or 18 (8 available for bonding) • 4th – 32 • 5th- 50 • 6th- 72

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