1
Bonding
94−105.5°
Hydrogen peroxide dissolves in water.
(i) State the strongest type of interaction that occurs between
molecules of hydrogen peroxide and water.
Hydrogen bonding
Draw a diagram to show how one molecule of hydrogen peroxide
interacts with one molecule of water.
Include all lone pairs and partial charges in your diagram.
, 2
Explain, in terms of electronegativity, why the boiling point of H2S2
is lower than H2O2.
1. Electronegativity of S lower than O
2. No hydrogen bonding between H2S2 molecules
The power of an atom to attract electrons towards itself In a covalent
bond
Suggest why the electronegativity of the elements increases from
, 3
lithium to fluorine.
1. More protons
2. Same shielding
State the type of bonding in lithium fluoride.
Explain why a lot of energy is needed to melt a sample of solid
lithium fluoride.
1. Ionic
2. Strong electrostatic attractions between + and − ions
Deduce why the bonding in nitrogen oxide is covalent rather than
ionic.
Small electronegativity difference
Oxygen forms several different compounds with fluorine.
(i) Suggest the type of crystal shown by OF2
(simple) molecular
, 4
Hydrogen bonds
Draw a diagram to show how two ammonia molecules interact with
each other in the liquid phase.
Include all partial charges and all lone pairs of electrons in your
diagram.
Ammonia reacts with boron trichloride to form a molecule with the
following structure.
Lone pair on N(H3) is donated to B(Cl3)
Bonding
94−105.5°
Hydrogen peroxide dissolves in water.
(i) State the strongest type of interaction that occurs between
molecules of hydrogen peroxide and water.
Hydrogen bonding
Draw a diagram to show how one molecule of hydrogen peroxide
interacts with one molecule of water.
Include all lone pairs and partial charges in your diagram.
, 2
Explain, in terms of electronegativity, why the boiling point of H2S2
is lower than H2O2.
1. Electronegativity of S lower than O
2. No hydrogen bonding between H2S2 molecules
The power of an atom to attract electrons towards itself In a covalent
bond
Suggest why the electronegativity of the elements increases from
, 3
lithium to fluorine.
1. More protons
2. Same shielding
State the type of bonding in lithium fluoride.
Explain why a lot of energy is needed to melt a sample of solid
lithium fluoride.
1. Ionic
2. Strong electrostatic attractions between + and − ions
Deduce why the bonding in nitrogen oxide is covalent rather than
ionic.
Small electronegativity difference
Oxygen forms several different compounds with fluorine.
(i) Suggest the type of crystal shown by OF2
(simple) molecular
, 4
Hydrogen bonds
Draw a diagram to show how two ammonia molecules interact with
each other in the liquid phase.
Include all partial charges and all lone pairs of electrons in your
diagram.
Ammonia reacts with boron trichloride to form a molecule with the
following structure.
Lone pair on N(H3) is donated to B(Cl3)
