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14 Cards in this Set
- Front
- Back
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What is the shielding effect?
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It is the ability of inner electrons to "shield" outer electrons from the attractive force of the nucleus.
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What happens when you move across a period?
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-Electrons are added to the same energy level.
-RESULT: the amt. of inner electrons does not change, so the shielding effect remains constant. |
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What happens when you move down a group?
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-Electrons are added to the new energy levels.
-RESULT: The amt. of inner electrons increases, so the shielding effect increases. |
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Effective Nuclear Charge
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(# of protons in nucleus) - (# shielding electrons)
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Effective Nuclear Charge
-WHat happens as you move across a period? |
-Electrons are added to the same energy level
-the amt. of shielding electrons remains constant -RESULT: Nuc. charge increases, but shielding is constant, so the effective nuc. Charge increases as you move across the p. table. |
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As you move across a period what happens to the effective nuclear charge
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It increases
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Effective Nuclear Charge
-WHat happens as you move down a group? |
-Electrons are added to the new energy level
-the amt. of shielding electrons increases -RESULT: THe nuc. charge increases, but this is cancelled by the increase in shielding electrons, so the effective nuc. charge remains constant. |
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As you move down a group what happens to the effective nuclear charge
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It remains constant
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Atomic Size (Radius)
-What happens as you move across a period? |
-Electrons are added to the same energy level.
-Amt. of shielding electrons remains constant -the effective nuc. charge increases -RESULT: atomic size decreases from left to right across the p. table |
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From left to right on the p. table, atomic size:
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decreses
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Atomic Size (Radius)
-Down a group? |
-Electrons are added to new electron levels
-amt. of shielding electrons increases -the effective nuc. charge remains constant -RESULT: Atomic size increases from top to bottom |
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As you go down a group the atomic size (radius):
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increases.
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The element with the highest electronegativity
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Fluroine
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How does the IONIC radius of a typical metal atom compare to its atomic radius?
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Always smaller
NS |
