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ionization energy
- minimum energy required to remove an electron from gaseous atom/ion
- first: Na(g)-> Na+(g) + e-
- 2nd: Na+(g) -> Na2+(g) + e-energy increases to remove from 1st,2nd, 3rd, etc. ionization energy levels
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ionization energy trends
- as i.e. INCREASES, harder to remove electron
- Generally INC. left to right, bottom to top (pull of electrons increases going bottom to up)
- exceptions: high group 2 and 5 (having to add an extra electron to an already balanced electron orbital)
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electron affinity
- energy that comes with adding an electron to a gaseous atom
- measures attraction between e- and atom, so the more negative electron affinity = higher/easier attraction
- NEGATIVE numbers (usually)
- equation: Cl(g) + e- -> Cl-(g)
- energy is released
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electron affinity trends
- very high: halogens (G 7)
- slightly high: 1,3,4,6
- positive: some G 2, 5, ALL G 8 (to add an e-) to an already filled orbital decreases attraction
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electronegativity:
- ability of atom (in a molecule) to attract electrons to itself
- based off of electron affinity and ionization energy
- INCREASES: left to right, bottom to top
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using electronegative values to calculate type of bond (non-polar, polar-covalent, ionic)
- subtract one electronegative value from the other to get positive value
- < 0.3 non polar
- .3-2.0 polar covalent
- >2 ionic
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resonance
when molecule as alternate but equivalent resonance structures
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