i need answers to this please! Daily Problem #3 Determine the kinds of intermole
ID: 575255 • Letter: I
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i need answers to this please!
Daily Problem #3 Determine the kinds of intermolecular forces present in each element or compound. Draw the Lewis Dot Structure for each element or compound and determine whether it is polar or nonpolar. A) PH3 B) HBr C) CH3OH D) I2 1. 2. The binary hydrogen compounds of the Group 4A elements and their boiling points are: CH4, -162°C; SiH4, -112°C; GeH4, -88°C; and SnH4, -52°C. Explain the increase in boiling points from CH4 to SnH4. Which member of each of the following pairs of substances would you expect to have a higher boiling point? A) 02 or Cl2 B) SO2 or CO2 C) HF or HI What kind of attractive forces must be overcome in order to A) melt ice B) boil molecular bromine C) melt solid iodine D) dissociate F2 into F atoms? 3. 4.Explanation / Answer
(1)
PH3, HBr and CH3OH are all polar molecules so they have dipole intermolecular forces. I2 is non-polar so the only intermolecular forces present in it are Van Der Waal's forces.
(2)
As we move down the group, the molecular mass keeps on increasing which causes an increase in the Van Der Waal's forces. As these intermolecular forces increase, the boiling point also increases. This is why the boiling point keeps on increasing down the group.
(3)
(a)
Cl2 has higher boiling point, because it has higher molecular mass and hence stronger intermolecular Van Der Waal's forces.
(b)
SO2 has higher boiling point because SO2 is a polar molecule and hence it has strong intermolecular dipole forces of attraction.
(c)
HF has higher boiling point because of strong H-bonding between the molecules.
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