CS₂ is totally symmetrical i.e. the two dipoles cancel out.

CS₂ is polar

permanent dipole-dipole forces are the strongest intermolecular force in CS₂

The C–S double bond is polar

CCl₄

CH₃CH₃

PBr_³

at room temperature and pressure, some covalent compounds are solids, some are liquids, and some are gases

covalent bonds exist between molecules

in covalent bonds, electrons are transferred between atoms

SiO₂ contains covalent bonds

ionic bonding

London forces

permanent dipole-dipole forces

hydrogen bonding

CO₂, CS₂, CSe₂

CH₃Cl, NO, HF

CH₂Cl₂, CO, PBr₃

H₂O, H₂Se, H₂S

"The hydrogen bonds in H₂O are stronger and take more energy to break."

"The hydrogen bonds in H₂O are stronger than the permanent dipole-dipole forces in H₂S. Hydrogen bonding takes more energy to break."

"Hydrogen bonding in water is stronger than the London forces in H₂S"

"The H₂O molecules are held in an open lattice"

CS₂ has more electrons and stronger London forces

CS₂ has more electrons and the bonds between molecules are stronger than in CO₂

the C=O bond is more polar than the C=S bond, because O is more electronegative than S

CO₂ only has London forces, whereas CS₂ has permanent dipole-dipole forces

hydrogen bonds are hold apart water molecules in an open lattice, so the solid substance is less dense

the molecule is totally symmetrical, so the bond dipoles cancel.

the bonds between molecules are broken when boiling

ionic bonds are much stronger than intermolecular forces so need more energy to overcome

1) does the molecule contain O, F, or N atoms? 2) is the molecule polar?

1) does the molecule contain an O–H, N–H, F–H bond? 2) does the molecule contain lone pairs?

1) does the molecule contain OH, NH, FH 2) is the molecule polar?

1) does the molecule contain an O–H, N–H, F–H bond? 2) is the molecule polar?

the melting and boiling points will be anomalously high

the molecule must contain an O–H bond

it must also have London forces

it must also have permanent dipole-dipole forces