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12 Cards in this Set
- Front
- Back
- 3rd side (hint)
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What is ionisation energy? |
The energy needed to remove 1 mole of electrons from 1 mole of atoms in the gaseous state |
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Why does ionisation energy increase across a periods |
Due to the increase in nuclear charge keeping electrons more tightly held, closer to the nucleus and therefore harder to remove |
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Why does ionisation energy decrease down a group? |
Due to the increase in electron shells making electrons further from nucleus and not attracted as much. Also, additional screening effect from inner electron shells makes it easier to remove outer electrons |
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What is electronegativity? |
Measure of attraction an atom has for bonded electrons. |
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Why does electronegativity increase across a period? |
Due to the increase in nuclear charge, meaning electrons are more tightly held and closer to nucleus |
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Why does electronegativity decrease down a group? |
Due to the increase in electron shells, keeping electrons less tightly held and further from nucleus. Also, additional screening effect from inner electron shells |
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Why does covalent radius decrease across a period? |
Due to the increase in nuclear charge, keeping electrons more tightly held and closer to nucleus. |
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Why does covalent radius increase down a group. |
Due to the increase in electron shells causing electrons to be further form nucleus and less tightly held. |
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Name the elements with a metallic lattice structure |
Lithium, Beryllium, Sodium, Magnesium, Potassium, Aluminium, Calcium |
IUM !!!!! |
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Name the elements with a covalent network structure |
Boron, Silicon, Carbon (diamond, graphite) |
-ON!! |
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Name the covalent molecular elements |
Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Sulfur(8), Phosphorus (4), fullerene! C60 |
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Name the monatomic elements |
Noble gases |
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