AQA A-Level Chemistry (new spec) 1.3
Bonding questions and answers
Ionic Bonding - The electrostatic force of attraction between two oppositely
charged ions formed by electron transfer
Covalent Bonding - A shared pair of electrons
Dative Covalent Bonding (AKA Co-ordinate bonding) - Formed when the shared
pair of electrons in the covalent bond come from only one of the bonding atoms.
Metallic Bonding - The electrostatic force of attraction between the positive metal
cations and the sea of delocalised electrons
Factors affecting the strength of metallic bonding: The number of protons - The
more protons in the cations, the stronger the electrostatic force of attraction
between the cations and the sea of delocalised electrons
Factors affecting the strength of metallic bonding: Number of delocalised
electrons per atom - The more delocalised electrons, the stronger the electrostatic
force of attraction
, AQA A-Level Chemistry (new spec) 1.3
Bonding questions and answers
Factors affecting the strength of metallic bonding: Size of ion - The smaller the ion,
the stronger the electrostatic force of attraction
Electronegativity - The relative tendency of an atom in a covalent bond in a
molecule to attract electrons in a covalent bond towards itself
Why does electronegativity increase as you go across a period? - -The number of
protons increased
-The atomic radius decreases because the electrons in the same shell are pulled in
more
Why does electronegativity decrease as you go down a group? - -Distance
between the nucleus and the outer electrons increases
-Shielding increases
Why aren't the noble gases electronegative? - Because they don't form bonds
Using electronegativity to predict bonding: Covalent - If both atoms have a similar
electronegativity, the pull on the electrons from them will be of a similar strength,
making a non-polar covalent bond.
Bonding questions and answers
Ionic Bonding - The electrostatic force of attraction between two oppositely
charged ions formed by electron transfer
Covalent Bonding - A shared pair of electrons
Dative Covalent Bonding (AKA Co-ordinate bonding) - Formed when the shared
pair of electrons in the covalent bond come from only one of the bonding atoms.
Metallic Bonding - The electrostatic force of attraction between the positive metal
cations and the sea of delocalised electrons
Factors affecting the strength of metallic bonding: The number of protons - The
more protons in the cations, the stronger the electrostatic force of attraction
between the cations and the sea of delocalised electrons
Factors affecting the strength of metallic bonding: Number of delocalised
electrons per atom - The more delocalised electrons, the stronger the electrostatic
force of attraction
, AQA A-Level Chemistry (new spec) 1.3
Bonding questions and answers
Factors affecting the strength of metallic bonding: Size of ion - The smaller the ion,
the stronger the electrostatic force of attraction
Electronegativity - The relative tendency of an atom in a covalent bond in a
molecule to attract electrons in a covalent bond towards itself
Why does electronegativity increase as you go across a period? - -The number of
protons increased
-The atomic radius decreases because the electrons in the same shell are pulled in
more
Why does electronegativity decrease as you go down a group? - -Distance
between the nucleus and the outer electrons increases
-Shielding increases
Why aren't the noble gases electronegative? - Because they don't form bonds
Using electronegativity to predict bonding: Covalent - If both atoms have a similar
electronegativity, the pull on the electrons from them will be of a similar strength,
making a non-polar covalent bond.
