Download - Test Review - Periodicity
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Jin Ho Park (Class of 2012)
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PERIODICITY
1. Periodic Table – historical approach
1718 – Organized atoms with properties
1789 – French revolution
H20 – before diagram
1869 Mandalay
- Tried to leave space for atoms that he couldn’t found
Put ‘?’ for ones that were wrongly measured
2. Periodic Law
3. Regions of P.T. – groups, periods, blocks
Period - # of shells/ energy levels
Group - # of valence electron
Block – What kind of outer shell
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4. Change in character and properties of elements across the P.T.
Metals
- LEFT of Metalloids
- Solid (expt. Hg)
- Good conductor of electricity & heat
- Shiny, Silver (except. Au, Cu)
- Malleable
- Ductile
- High melting and boiling point
- Insoluble (some react)
Metalloids
- Between metal & non-metals
- Solids
- Semi-conductors
- Like metal
- Weak conductive
- High ductile
- Insoluble (may heat)
Non-metals
- RIGHT of metalloids
- All states possible
- Not conducts
- Insulator (expt. Graphite (pure carbon))
- Shiny, Silvery?? (no)
- Brittle
- Insoluble (may react)
Noble gases
- Nonmetals
- does not form an ion (except helium)
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- stable
- colorless
5. General description of P.T. groups (physical & chemical properties)
1) Alkaline metals
- Forms 1+ ion
- Metals
- Very reactive
- Soft, silvery, shiny, low density
2) Alkaline-earth metals
- Forms 2+ ion
- Metals
- Very reactive but less than alkali metals
- Silvery, higher density than alkali metals
3) – 12) Transition metals
- Forms 2+ ion
- Metals
- Less reactive than alkaline-earth metals
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- Silvery, good conductor of thermal energy and electric current, higher densities and melting points
than alkaline earth metals
13) – 16) Metals, metalloids, non-metals
-
17) Halogens
- Nonmetals
- Forms 1- ion
- Poor conductors of electric current
- Reactions with alkali metals18) Noble gases
- Nonmetals
- does not form an ion (except helium)
- stable
- colorless
?) Hydrogen
- Nonmetals
- Group 1
- Reactive
- Colorless
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6. Periodic trends along periods and groups
Atomic radius
- Decrease across a period and increase down a group
Ionisation energy
- Increase across a period and decrease down a group
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Electro negativity
- Increase across a period and decrease down a group
Electron affinity