Periodicity

  • Created by: charley
  • Created on: 06-09-18 13:32
First Ionisation Energy
The energy required to remove one electron from each atom in one mole of gaseous atoms of an element
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Why does atomic radius effect the first ionisation energy?
The greater the distance between the nucleus and outer electrons, the less the nuclear attraction
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The shielding effect/Atomic shielding
The inner shell electrons repel the outer shell electrons, reducing the attraction between the nucleus and outer electrons
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What happens with successive ionisation?
The electrons get pulled closer to the nucleus as nuclear attraction increases. More energy is needed to remove each electron
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Second Ionisation Energy
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element
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What do large increases ionisation energy show?
They show when an electron has been removed from a different shell, closer to the nucleus and with less shielding
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What predictions can be made from successive ionisation energies?
The number of electrons in the outer shell, the group element and the identity of the element
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Why does the first ionisation energy decrease down a group?
The atomic radius and shielding increases and nuclear attraction decreases.
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Why does the first ionisation energy increase across a period?
The nuclear change and nuclear attraction increases and atomic radius decreases. They have similar shielding.
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Metallic bonding
The strong electrostatic attraction between positive metal ions and delocalised electrons
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Giant metallic lattice
Metal atoms held together by metallic bonding
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Properties of metals
Most metals have strong metallic bonds, high electrical conductivity and high melting and boiling points. They're insoluble as any interaction would lead to a reaction
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Simple covalent lattice
Held together by weak intermolecular forces. They have low melting and boiling points.
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Giant covalent lattice
Non-metal atoms held together by strong covalent bonds. They have high melting and boiling points. They're insoluble. They do not conduct electricity
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Graphite
Composed of parallel layers of graphene bonded by weak London forces. Conducts electricity because one electron from each carbon is delocalised
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What marks the the change from giant to simple molecular structures?
The increase of melting point from group 1 to 14 followed by the decrease in melting point from group 14 to 18
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Other cards in this set

Card 2

Front

The greater the distance between the nucleus and outer electrons, the less the nuclear attraction

Back

Why does atomic radius effect the first ionisation energy?

Card 3

Front

The inner shell electrons repel the outer shell electrons, reducing the attraction between the nucleus and outer electrons

Back

Preview of the back of card 3

Card 4

Front

The electrons get pulled closer to the nucleus as nuclear attraction increases. More energy is needed to remove each electron

Back

Preview of the back of card 4

Card 5

Front

The energy required to remove one electron from each ion in one mole of gaseous 1+ ions of an element

Back

Preview of the back of card 5
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