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9 Cards in this Set
- Front
- Back
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Where are the s-, p- and d-blocks of elements in the periodic table?
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a) What are the trends in melting and boiling temperatures of the elements in Period 3?
b) How can these trends be explained in terms of bonding an structure? |
a) The left hand side is higher than the right hand side, with Silicon being a fair bit higher.
b) The left hand elements are giant metallic, where as the right hand elements (P^4,S^8, Cl^2) are molecular (van der Waals). Silicon is macro-molecular. |
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a) What are the trends in atomic radius of the elements in period 3?
b) Why? |
a) It decreases
b) Nuclear charge increases, pulling electrons closer, no additional shells to provide shielding |
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a) What are the trends in first ionisation energy of the elements in period 3?
b) Why? |
a) Generally increases
b) Increasing nuclear charge and atomic radius decreases make it increasingly difficult to remove electrons. |
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How do successive ionisation energies explain electron arrangements?
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It goes steadily up, but jumps up sharply when moving to another main level.
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What is the the nemonic for first ionisation energy?
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BeBNOMagnesiumAlPS.
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Why is there a decrease in first ionisation energy between Be-B and Mg-Al?
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The electron lost by B/Al is from the p sub-shell which is a higher energy level than Be/Mg's s sub-shell electron.
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Why is there a decrease in first ionisation energy between N-O and P-S?
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An electron in a pair will be easier to remove than one in an orbital on its own because it is already being repelled by the other electron. N/P has no pairs whereas O/S has one.
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What is the trend in ionisation energies down a group?
Why? |
Generally decreases (group 2) because the outer electron is in a main level that gets increasingly further away from nucleus. Though the nuclear charge increases, the positive charge felt by electrons in outer shell is less than nuclear charge because of inner electrons shielding it.
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