Positive ions are formed when atoms lose electrons.
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Do metals or non-metals form cations?
Metals form cations.
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How are negative ions (anions) formed?
Negative ions are formed when atoms gain electrons.
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Do metals or non-metals form anions?
Non-metals form anions.
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When does ionic bonding occur?
Ionic bonding occurs between metals and non-metals.
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Are electrons given or shared in ionic bonding?
Electrons are given in ionic bonding.
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Define an ionic bond.
An ionic bond is the electrostatic force of attraction between oppositely charged ions.
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What do all ionic compounds exist as in the solid state?
In the solid state all ionic compounds exist as giant ionic lattices.
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What are giant ionic lattices?
They are regular 3D arrangements of positive and negative ions.
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When does covalent bonding occur?
Covalent bonding occurs between non-metals only.
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Are electrons given or shared in covalent bonding?
Electrons are shared in covalent bonding.
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Define a covalent bond.
A covalent bond is formed when atoms share a pair of electrons, one electron being contributed by each atom.
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What is the Octet rule?
The tendency for atoms to achieve a full outer shell is sometimes referred to as the Octet rule.
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In covalent bonding what are electron pairs that form bonds called?
Bonding pairs.
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What are pairs of electrons not involved in bonding called?
Lone pairs (non-bonding pairs).
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Define a dative covalent bond.
A dative covalent bond is a shared pair of electrons which has been provided by one of the bonding atoms only.
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How is a dative covalent bond shown?
A dative covalent bond is shown by an arrow pointing from the atom supplying the electrons to the atom which then shares them.
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What is metallic bonding?
Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons.
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When does metallic bonding occur?
Metallic bonding occurs between metals and metals.
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What are the outer shell electrons in a metal?
In a metal the outer shell electrons are delocalised, i.e. shared between all the atoms in the structure
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Why are metals good conductors of electricity?
Metals are good conductors of electricity because the delocalised electrons can move through the lattice.
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Why do metals have a high melting and boiling point?
The electrostatic attraction between the delocalised electrons and the metal ions is strong. This causes metals to have high melting and boiling points.
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What metal is an exception to having a high melting/boiling point?
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