AQA A-Level Chemistry (new spec) 1.3 Bonding
Study online at https://quizlet.com/_22jcbl
1. Ionic Bonding The electrostatic force of attraction between two oppositely charged ions formed
by electron transfer
2. Covalent Bond- A shared pair of electrons
ing
3. Dative Cova- Formed when the shared pair of electrons in the covalent bond come from only
lent Bonding one of the bonding atoms.
(AKA Co-ordinate
bonding)
4. Metallic Bonding The electrostatic force of attraction between the positive metal cations and the sea
of delocalised electrons
5. Factors affecting The more protons in the cations, the stronger the electrostatic force of attraction
the strength of between the cations and the sea of delocalised electrons
metallic bonding:
The number of
protons
6. Factors affecting The more delocalised electrons, the stronger the electrostatic force of attraction
the strength of
metallic bonding:
Number of delo-
calised electrons
per atom
7. Factors affecting The smaller the ion, the stronger the electrostatic force of attraction
the strength of
metallic bonding:
Size of ion
8. Electronegativity
1/8
, AQA A-Level Chemistry (new spec) 1.3 Bonding
Study online at https://quizlet.com/_22jcbl
The relative tendency of an atom in a covalent bond in a molecule to attract
electrons in a covalent bond towards itself
9. Why does elec- -The number of protons increased
tronegativity in- -The atomic radius decreases because the electrons in the same shell are pulled
crease as you go in more
across a period?
10. Why does elec- -Distance between the nucleus and the outer electrons increases
tronegativity de- -Shielding increases
crease as you go
down a group?
11. Why aren't the Because they don't form bonds
noble gases elec-
tronegative?
12. Using elec- If both atoms have a similar electronegativity, the pull on the electrons from them
tronegativity to will be of a similar strength, making a non-polar covalent bond.
predict bonding: If one atom has a stronger electronegativity than the other, the electrons will be
Covalent pulled more towards one atom, making the bond polar-covalent
13. Using elec- If the electronegativity difference is really large, the sharing of electrons is so
tronegativity to uneven that the more electronegative atom has full possession of the 2 electrons,
predict bonding: creating an ionic bond
Ionic
14. Using elec- If both atoms have a low electronegativity, neither can attract electrons, so the
tronegativity to electrons don't remain localised to the bond at all, causing a sea of delocalised
predict bonding: electrons and a metallic bond
Metallic
15.
2/8
Study online at https://quizlet.com/_22jcbl
1. Ionic Bonding The electrostatic force of attraction between two oppositely charged ions formed
by electron transfer
2. Covalent Bond- A shared pair of electrons
ing
3. Dative Cova- Formed when the shared pair of electrons in the covalent bond come from only
lent Bonding one of the bonding atoms.
(AKA Co-ordinate
bonding)
4. Metallic Bonding The electrostatic force of attraction between the positive metal cations and the sea
of delocalised electrons
5. Factors affecting The more protons in the cations, the stronger the electrostatic force of attraction
the strength of between the cations and the sea of delocalised electrons
metallic bonding:
The number of
protons
6. Factors affecting The more delocalised electrons, the stronger the electrostatic force of attraction
the strength of
metallic bonding:
Number of delo-
calised electrons
per atom
7. Factors affecting The smaller the ion, the stronger the electrostatic force of attraction
the strength of
metallic bonding:
Size of ion
8. Electronegativity
1/8
, AQA A-Level Chemistry (new spec) 1.3 Bonding
Study online at https://quizlet.com/_22jcbl
The relative tendency of an atom in a covalent bond in a molecule to attract
electrons in a covalent bond towards itself
9. Why does elec- -The number of protons increased
tronegativity in- -The atomic radius decreases because the electrons in the same shell are pulled
crease as you go in more
across a period?
10. Why does elec- -Distance between the nucleus and the outer electrons increases
tronegativity de- -Shielding increases
crease as you go
down a group?
11. Why aren't the Because they don't form bonds
noble gases elec-
tronegative?
12. Using elec- If both atoms have a similar electronegativity, the pull on the electrons from them
tronegativity to will be of a similar strength, making a non-polar covalent bond.
predict bonding: If one atom has a stronger electronegativity than the other, the electrons will be
Covalent pulled more towards one atom, making the bond polar-covalent
13. Using elec- If the electronegativity difference is really large, the sharing of electrons is so
tronegativity to uneven that the more electronegative atom has full possession of the 2 electrons,
predict bonding: creating an ionic bond
Ionic
14. Using elec- If both atoms have a low electronegativity, neither can attract electrons, so the
tronegativity to electrons don't remain localised to the bond at all, causing a sea of delocalised
predict bonding: electrons and a metallic bond
Metallic
15.
2/8
