periodicity flashcards

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What is the definition of first ionisation energy?
The first ionisation energy is the amount of energy required to remove moles of electrons from one mole of gaseous atoms to form one mole of gaseous ions.
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What three things affect ionisation energy?
Nuclear charge, atomic radius (distance), electron shielding.
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How does nuclear charge affect ionisation energy?
The more protons in the nucleus of an atom, the greater the attraction between the nucleus and the outer electrons
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How does atomic radius affect ionisation energy?
the greater the distance between the nucleus and the outer electron, the less the attraction.
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How does electron shielding affect ionisation energy?
electron repulsion reduces the attraction between the nucleus and the highest energy electron
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What is the trend in ionisation energy down a group?
1. atomic radius increases 2. more shells so shielding increases 3. nuclear attraction decreases 4. ionisation energy decreases
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what is the trend in ionisation energy across a period?
1. nuclear charge increases 2. similar shielding 3. nuclear attraction increases 4. atomic radius decreases 5. ionisation energy decreases
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what is metallic bonding?
electrons are delocalised around the whole structure, they surround the positives catitons
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define metallic bonding?
the electrostatic attraction between cations and delocalised electrons
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why do metals have electrical conductivity?
the delocalised electrons can move to carry charge
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why do most metals have high boiling and melting points?
high amounts of energy are needed to overcome the strong electrostatic attraction between cations and electrons
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what 3 elements have a giant covalent lattice?
boron, carbon and silicon
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what are 3 properties of giant covalent lattice structures?
high melting points, insolubility and non-conductive
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What are the exceptions of conductivity in giant covalent lattices?
graphene and graphite
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why do giant covalent structures have high melting points?
there are strong covalent bonds that require high amounts of energy to break
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why are giant covalent structures insoluble?
the covalent bonds holding together atoms in the lattice are too strong to be broken by solvents
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Other cards in this set

Card 2

Front

What three things affect ionisation energy?

Back

Nuclear charge, atomic radius (distance), electron shielding.

Card 3

Front

How does nuclear charge affect ionisation energy?

Back

Preview of the front of card 3

Card 4

Front

How does atomic radius affect ionisation energy?

Back

Preview of the front of card 4

Card 5

Front

How does electron shielding affect ionisation energy?

Back

Preview of the front of card 5
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