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12 Cards in this Set
- Front
- Back
- 3rd side (hint)
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S orbital shape? |
Spherical |
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P orbital shape |
Dumbbell?! |
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Shell structure up to n=4 |
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How are orbitals often displayed? |
As boxes with arrows indicating spin. |
You could show it with a pen. |
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How do electrons fill orbitals? |
They join empty orbitals, then pair up. |
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How can electron configuration be shown in shorthand? |
[The previous noble gas] + any further subshells |
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What happens with 4s and 3d? |
4s fills first, but once filled the 3d energy level falls below 4s, so: 4s fills and empties first. |
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Period trend of 1st ionisation energy: |
Across a period elements have the same number of quantum shells. First ionisation energy increases (in general), as the is similar electron shielding, nuclear attraction increases, atomic radius decreases. |
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Group trends of first ionisation energy: |
Atomic radius increases, more inner shell, so shielding increases, more nuclear attraction, so first ionisation energy decreases. |
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What is first ionisation energy? |
The energy required to remove one electron from each atom in 1 mole of gaseous atoms of an element to form one more of gaseous 1+ ions. |
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Why does 1st ionisation energy fall from Be to B and from N to O? |
Be->B 2p has a higher energy level than 2s, so it is easier to remove an electron, so 1st ionisation energy of Be is higher than B. N->O 2p³ to 2p⁴ 2p³ has one electron in each orbital. I'm 2p⁴ there is a paired electron. These electrons repel, so 1st ionisation energy of O is lower than N. |
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Order of filling orbitals |
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