Term
Explain: Potassium has a lower first-ionization energy than lithium |
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Definition
| As you go down the periodic table, n increases, potassium is larger than lithium and has less zeff than lithium and holds on to its valence e- less tightly. Therefore it is easier to remove valance e- from potassium, then it is from lithium. |
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Term
Explain: The ionic radius of N3-is larger than that of O2- |
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Definition
The more e- you gain, the larger the ion, and the lower the zeff. in addition e-/e- repulsions increase for both of these reasons nitrogen has less of a pull on its e- than O2- N3- O2- 7:10 8:10 |
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Term
Explain: A calcium atom is larger than a zinc atom |
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Definition
Zinc is greater than calcium becuase more protons are pulling on the same # of core e- which results in a smaller atom. |
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Term
Explain: The second ionization energy of sodium is about three times greater than the second ionization energy of magnesium |
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Definition
| It's harder to remove an e- from sodium because you would be taking from a core electron, whereas you wouldn't until the 3rd ionization energy level in Magnesium, zeff would be greater for sodium, and it's harder to remove core e- than valence e-. |
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Term
| Why is helium a member of group 18 & not 2? |
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Definition
| Because it is an inert gas and has a full valence shell. |
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Term
| State 5 differences between metals and nonmetals |
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Definition
Metals: luster, good conducters of heat and electricity, solid@ room temp., maleable, ductle
Non Metals: not luster, not good conducters of heat and electricity, gas a room temp, not maleable, not ductle |
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Term
| relationship between group numbers & valence e- for main group elements |
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Definition
the valence e-= the 1's place Ex: 13....valence e-=3 |
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Term
How do modern day periodic tables differ from Mendeleev's? (2 ways, must be in a chart) |
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Definition
Mendeleev: increasing atomic mass, similar properties,by row
Modern: increasing atomic #, elements w/similar properties, by groups(columns) |
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Term
| Why is fluorine the most electrongative element? |
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Definition
| As you go across the P.T. seff increases, but when you go down zeff decreases. Part of the halogens only holds one more e- to be stable. (has the greatest zeff, and is the smallest of the halogens) most likely to attract e- in a chemical bond. |
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Term
| Why do halogens have the most negative electron? |
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Definition
| Because they have the greatest zeff in each period, and are 1 electron away from being stable, which makes them the easiest elements to add an electron to. |
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Term
| Which group has the lowest 1st ionization energies? WHY? |
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Definition
| Group 1, because they have the lowest zeff and are the most to readily give up 1 e- to form stable ions. |
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