For each pair of compounds, identify the one with the higher boiling point.
I)GeCl4 or SnCl4
II)PF3 or PF5
III)H2O or H2S
SnCl4
PF3
H2O
thanks
SiH4 or PbH4
To determine which compound in each pair has a higher boiling point, we need to consider the intermolecular forces between their molecules. Generally, compounds with stronger intermolecular forces tend to have higher boiling points.
I) GeCl4 or SnCl4:
To compare the boiling points of GeCl4 and SnCl4, we need to consider their molecular structures and intermolecular forces. Both compounds are tetrahedral in shape. However, SnCl4 has a larger atomic size relative to GeCl4. Larger atoms or molecules tend to have stronger London dispersion forces, which are a type of intermolecular force. Therefore, SnCl4 likely has higher boiling point than GeCl4.
II) PF3 or PF5:
To compare the boiling points of PF3 and PF5, we again need to consider their molecular structures and intermolecular forces. PF3 has a trigonal pyramidal shape, while PF5 has a trigonal bipyramidal shape. PF3 molecules have a lone pair of electrons, which can create dipole-dipole interactions between molecules. On the other hand, PF5 is symmetrical and doesn't have a lone pair, resulting in weaker intermolecular forces. Therefore, PF3 likely has a higher boiling point than PF5.
III) H2O or H2S:
To compare the boiling points of H2O and H2S, we need to consider their molecular structures and intermolecular forces. Both compounds are bent in shape. However, H2O has two lone pairs of electrons, which creates stronger dipole-dipole interactions due to hydrogen bonding. On the other hand, H2S only has one lone pair, resulting in weaker intermolecular forces. Therefore, H2O likely has a higher boiling point than H2S.
Overall, the compounds with the higher boiling point in each pair are:
I) SnCl4
II) PF3
III) H2O