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Periodic Table

Periodic Table. Trends. Let’s Make Sense of This. Trends to explore. Atomic Radii. Increases from top to bottom because atom is getting larger. Decreases from left to right because electron affinity increases. Electron affinity. Defines how strongly atoms of an element want more electrons.

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Periodic Table

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  1. Periodic Table Trends

  2. Let’s Make Sense of This

  3. Trends to explore

  4. Atomic Radii • Increases from top to bottom because atom is getting larger. • Decreases from left to right because electron affinity increases.

  5. Electron affinity • Defines how strongly atoms of an element want more electrons. • Elements in group VII want them most.

  6. Ionization energy • Energy needed to remove electrons. • It makes sense that more energy is needed to remove electrons from atoms that want to gain them (like group VII)

  7. Metallic character • A metal is a good conductor of both electricity and heat. • A metal forms cations and ionic bonds with nonmetals • A cation has a net positive charge (more protons than electrons). • An anion has a net negative charge (more electrons than protons). • Cations and anions attract and form ionic bonds.

  8. Periodic law • Elements are arranged by increasing number of protons (atomic number) • Mendeleev arranged by mass • Neutrons also contribute to mass

  9. Rows and columns • Each row is called a period because chemical properties repeat (are periodic) • Each column is called a group because all members of the same group have similar electron configurations and therefore similar chemical properties. • Configuration = arrangement (vocab)

  10. Orbitals • s=2, p=6, d=10, and f=14 • Arrange as follows: 1s 2s, 2p 3s, 3p, 3d 4s, 4p, 4d, 4f 5s, 5p, 5d, 5f 6s, 6p, 6d

  11. Order of electron filling

  12. S, p, d, and f blocks

  13. Practice with: • C • S • Mg • H • Ar • Ir

  14. Valence electrons • Electrons in the highest occupied energy level. • Number increases from left to right • Practice electron dot diagrams: • N • Cl • Na • Ca • Al

  15. Electron dot diagrams

  16. Atom stability • Stable when highest energy level is full. • Noble gasses are stable. • Groups I-III want to lose e- and form cations. • Groups V-VII want to gain e- and form anions.

  17. Ionic bonding • Cations and anions combine to form compounds. • They are held together by ionic bonds. • Ex: Mg2+ and Cl- = MgCl2 • Ex: Na+ and O2- = Na2O • Ex: Al3+ and S2- = Al2S3

  18. Covalent bonding • Electrons are shared • Usually happens between two nonmetals • Ex: O and F = OF2 • Ex: C and O = CO2 • Ex: C and Cl = CCl4 • Ex: C and N = CN- ???

  19. Multiple bonds • Double bond = 4 electrons shared • Triple bond = 6 electrons shared • Remember: in order to be stable all 8 valence electron positions need to be taken.

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