3.1.3.7 Forces between molecules Flashcards
the strongest type of interaction that occurs between molecules of hydrogen peroxide and water
Hydrogen bond(ing) / H bonding / H bonds
in terms of electronegativity, why the boiling point of H2S2 is lower than H2O2
Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules
the strongest attractive force between two ammonia molecules
Hydrogen bonds / H bonds
the strongest type of intermolecular force in how the strongest type of intermolecular force in liquid HF arises (CH4)
Van der Waals/ vdw/London/ temporary (induced) dipole/ dispersion forces
the strongest type of intermolecular force in Ammonia (NH3)
Hydrogen bonds/H bonds
strongest type of intermolecular force present in Liquid F2
van der Waals’ / induced/temporary dipole-dipole / dispersion / London forces
strongest type of intermolecular force present in Liquid CH3F
dipole-dipole
strongest type of intermolecular force present in Liquid CH3F
hydrogen bonding
how the strongest type of intermolecular force in liquid HF arises
large difference in electronegativity between H and F / F most/very/much more electronegative
δ+H-Fδ- dipole created or dipole clearly implied
attraction/bond formed between δ+H and lone pair on F
the trend in the boiling points of the hydrogen halides from HCl to HI
van der Waals’ / induced/temporary dipole-dipole / dispersion / London forces / attractions
increase with the increasing Mr / size / mass / N 0 of e- / size of e- cloud (in the hydrogen halides)
reason why the boiling point of HF is higher than that of all the other hydrogen halides
hydrogen bonding stronger than van der Waals’ attraction/forces
why the boiling point of methanol is much higher than that of oxygen
van der Waals’ forces between oxygen molecules
Hydrogen bonding between methanol molecules
H-B stronger than van der Waals’ OR stronger IMF in methanol
in terms of the intermolecular forces present in each compound, why HF has a higher boiling point than HCl
HF = hydrogen bonding
HCl = (permanent) dipole-dipole bonding or even van de Waals’
Hydrogen bonding stronger / is the strongest IMF
the strongest type of intermolecular force between hydrogen fluoride molecules
Hydrogen bonds/hydrogen bonding/H bonds/H bonding
why the boiling point of fluorine is very low
vdw / van der Waals forces between molecules
IMF are weak / need little energy to break IMF / easy to overcome IMF
the structure of and bonding in graphite and explain why the melting point of graphite is very high
Layers of (C atoms)
Connected by covalent bonds within each layer
Van der Waals forces/IMF between layers/weak forces between layers
Many/strong covalent bonds need to be broken
why iodine vaporises when heated gently
Van der Waals forces are weak or easily broken
Van der Waals between molecules (or implied)
the strongest type of intermolecular force in water
Hydrogen/H bonds
the strongest type of intermolecular force in hydrogen sulfide (H2S)
van der Waals/vdw/dipole-dipole/London/temporarily induced dipole/dispersion forces
why the boiling point of water is much higher than the boiling point of hydrogen sulfide
Hydrogen bonds/IMF (in water) stronger
OR IMF/VDW/dipole-dipole forces (in H2S) are weaker
OR H bonding is the strongest IMF
why the boiling points increase from H2S to H2Te
Atoms/molecules get larger/more shells/more electrons/more surface area
therefore increased Van der Waals/IMF forces
three types of intermolecular force
Van der Waals’
dipole – dipole
hydrogen bonding
Why hydrogen fluoride requires more heat energy for melting than does hydrogen chloride
H-Bonding in HF
(dipole-) dipole/V dW in HCl
H-bonding is stronger than dipole-dipole or V.dW
Why hydrogen iodide requires more heat energy for melting than does hydrogen chloride
HI bigger molecule than HCl
Therefore the forces between HI molecules are stronger
why diamond and iodine (solid) have different melting points
Iodine Weak van der Waals’ forces / induced dipole-induced dipole
Diamond Covalent bonds would need to be broken
Many / strong covalent bonds OR much energy needed
the strongest type of intermolecular force between hydrogen fluoride molecules
Hydrogen bonding
Why HI molecules don’t have hydrogen bonding like HF molecules
Fluorine more/very electronegative or iodine less electronegative or electronegativity difference too small in HI
HI dipole weaker or bonding e– more equally shared
the strongest attractive force between two ammonia molecules
Hydrogen bonds / H bonds
why iodine has a higher melting point than fluorine
Iodine has more electrons / iodine is bigger (atom or molecule) / iodine has bigger Mr / bigger surface area
Stronger / more van der Waals forces / vdw / London / temporarily induced dipole / dispersion forces between molecules
the strongest type of intermolecular force in a sample of NHF2
Hydrogen bonds
Although phosphine molecules contain hydrogen atoms, there is no hydrogen bonding between phosphine molecules. Suggest an explanation for this.
Difference in electronegativity between P and H is too small
the strongest type of intermolecular force holding the water molecules together in the ice crystal
Hydrogen bonding
the strongest type of intermolecular force in methane
Van der Waals’/VdW
reason why the melting point of ice is higher than the melting point of methane
Hydrogen bonding is stronger (than van der Waals forces)/IMF in ice stronger (than IMF in methane)/H bonds take more energy to break
the strongest type of intermolecular force between CCl2F2 molecules
Dipole – dipole
why the boiling point of water is much higher than the boiling point of hydrogen sulfide
Hydrogen bonds/IMF (in water) stronger
IMF/VDW/dipole-dipole forces (in H2S) are weaker
H bonding is the strongest IMF
why the boiling points increase from H2S to H2Te
Atoms/molecules get larger/more shells/more electrons/more surface area
therefore increased Van der Waals/IMF forces
the strongest type of intermolecular force in Methane (CH4)
Van der Waals/ vdw/London/ temporary (induced) dipole/ dispersion forces
the strongest type of intermolecular force in Ammonia (NH3)
Hydrogen bonds/H bonds
how the strongest type of intermolecular force arises between two molecules of ammonia
(Large) electronegativity difference between N + H/ N very electronegative;
Forms N δ– / H δ+ or dipole explained in words
Lone pair on N attracts/forms weak bonds with H (δ+)
why HF has a higher boiling point than HCl
HF = hydrogen bonding
HCl = (permanent) dipole-dipole bonding or even van de Waals’
Hydrogen bonding stronger / is the strongest IMF
the strongest type of interaction that occurs between molecules of hydrogen peroxide and water
Hydrogen bond(ing) / H bonding / H bonds
why the boiling point of H2S2 is lower than H2O
Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules
the strongest attractive force between two ammonia molecules
Hydrogen bonds / H bonds
the strongest type of intermolecular force between hydrogen fluoride molecules
Hydrogen bonds/hydrogen bonding/H bonds/H bonding
the strongest type of interaction between polymer chains of Kevlar
Hydrogen bond(ing)
the strongest type of intermolecular force between one molecule of ammonia and one molecule of water
Hydrogen bonding / hydrogen bonds / H-bonding / H-Bonds
Phosphine (PH3) has a structure similar to ammonia. In terms of intermolecular forces, suggest the main reason why phosphine is almost insoluble in water.
(Phosphine) does not form hydrogen bonds (with water)
why iodine has a higher melting point than fluorine
Iodine has more electrons / iodine is bigger (atom or molecule) / iodine has bigger Mr / bigger surface area
Stronger / more van der Waals forces / vdw / London / temporarily induced dipole / dispersion forces between molecules
the strongest type of intermolecular force in a sample of NHF2
Hydrogen bonds
why the boiling point of methanol is much higher than that of oxygen
van der Waals’ forces between oxygen molecules;
Hydrogen bonding between methanol molecules;
H-B stronger than van der Waals’ OR stronger IMF in methanol;
why the boiling point of H2S2 is lower than H2O2
Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules
