Term
| THE EFFECT OF NUCLEAR CHARGE (Z) ON ORBITAL ENERGY |
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Definition
| "HIGHER nuclear charge LOWERS orbital energy (stabilizes the system) by INCREASING nucleus-electron attraction" |
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Term
| SHIELDING: THE EFFECT OF ELECTRON REPULSIONS ON ORBITAL ENERGY |
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Definition
| "Shielding by inner electrons greatly lowers the Zeff felt by outer electrons" |
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Term
| ORDER OF SUBLEVEL ENERGIES |
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Definition
s < p < d < f
"for a given n value, the lower the l value, the lower the sublevel energy" |
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Term
| ELECTROSTATIC INTERACTIONS DETERMINE ORBITAL ENERGIES BY: part 1 |
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Definition
| 1. Greater nuclear charge lowers orbital energy and makes electrons harder to remove. |
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Term
| ELECTROSTATIC INTERACTIONS DETERMINE ORBITAL ENERGIES BY: part 2 |
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Definition
| 2. Electron-electron repulsions raise orbital energy and make electrons easier to remove. Repulsions have the effect of SHIELDING electrons from the full nuclear charge, reducing it to an effective nuclear charge, Zeff. |
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Term
| ELECTROSTATIC INTERACTIONS DETERMINE ORBITAL ENERGIES BY: part 3 |
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Definition
| 3. Greater radial probability distribution near the nucleus (greater PENETRATION) makes an electron harder to remove because it is attracted more strongly and shielded less effectively. |
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Term
| In the Periodic Table, PERIODS are: |
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Definition
| Horizontal Rows (abrv.-phr) |
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Term
| In the Periodic Table, GROUPS are: |
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Definition
| Vertical Columns (abrv.-gvc) |
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Term
| TRENDS AMONG THE MAIN-GROUPS ELEMENTS: how is it increased? |
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Definition
| Atomic radius generally increases in a group from top to bottom (DOWN a group) |
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Term
| TRENDS AMONG THE MAIN-GROUPS ELEMENTS: how is it decreased? |
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Definition
| Atomic radius generally DECREASES in a period from left to right. (goes smaller as --->) |
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Term
| TRENDS IN IONIZATION ENERGY (IE): how does it decrease? |
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Definition
| IE generally DECREASES DOWN a group (easier to remove an outer electron from an element in Period 6 than Period 2) |
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Term
| TRENDS IN IONIZATION ENERGY (IE): how does it increase? |
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Definition
| IE generally INCREASES ACROSS a period. (easier to remove outer electron from an alkali metal than from a noble gas) |
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Term
| KEY POINTS in relative values of IE and Electron Affinity part 1 |
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Definition
| 1. REACTIVE NONMETALS: in their ionic compounds, they form negative ions |
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Term
| KEY POINTS in relative values of IE and Electron Affinity part 2 |
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Definition
| REACTIVE METALS: in their ionic compounds, they form positive ions. |
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Term
| KEY POINTS in relative values of IE and Electron Affinity part 3 |
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Definition
| 3. NOBLE GASES: these elements tend NOT to lose or gain electrons. |
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Term
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Definition
| a species with UNPAIRED electrons..it is attracted by an external magnetic field. |
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Term
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Definition
| a species with ALL electrons paired...it is not attracted (is slightly repelled) by a magnetic field). |
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Term
| Key Points in Ionic SIZE: |
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Definition
1. Ionic size INCREASES DOWN a GROUP.
2. Ionic size DECREASES ACROSS A PERIOD ...but increases from cations to anions.
3. Ionic size DECREASES with increasing positive (or decreasing negative) charge in an isoelectronic series.
4. Ionic size DEREASES as charge increase for different cations of a given element. |
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