Intermolecular Forces and Dipole Forces Questionnaire

ООООOrder the intermolecular forces (dipole-dipole, London dispersion, ionic, and hydrogen-bonding) from weakest to strongest.
London dispersion, dipole-dipole, hydrogen-bonding, and ionic
dipole-dipole, London dispersion, ionic, and hydrogen-bonding
London dispersion, ionic, dipole-dipole, and hydrogen-bonding
dipole-dipole, ionic, London dispersion, and hydrogen-bonding
hydrogen-bonding, dipole-dipole, London dispersion, and ionic
What type(s) of intermolecular forces are expected between H2O molecules?
ball & stick
+
labels
Indicate with a Y (yes) or an N (no) which apply.
dipole forces
induced dipole forces
hydrogen bonding
What type(s) of intermolecular forces are expected between CH3CH3 molecules?
H
H
H-
C
H
H
H
Indicate with a Y (yes) or an N (no) which apply.
dipole forces
induced dipole forces
hydrogen bonding
Which of the following would be expected to form hydrogen bonds with water?
Choose all that apply.
N-ethylpropanamide H-
H
H
hexane
H-
C
-H
H
11411
HHH
H
HT
c
H
H
H
propyl formate
H
C
0
H
H
H
ethylamine H-
None of the Above
Arrange the following molecules, H2S, F2, and CH3OH, in order of increasing strength of
intermolecular forces.
CH3OH, F2, H2S
H2S, F2, CH3OH
H2S, CH3OH, F2
OF2, H2S, CH3OH
CH3OH, H2S, F2
Which of the following compounds would have the highest boiling
point?
CH3CH2CH2CH2CH2OH
СН,ОН
CH3CH2CH2CH2CH2CH3
ОСН2СН3
Arrange the following molecules, H2S, F2, and CH3OH, in order of increasing strength of
intermolecular forces.
CH3OH, F2, H2S
H2S, F2, CH3OH
H2S, CH3OH, F2
OF2, H2S, CH3OH
CH3OH, H2S, F2
Use the following vapor pressure data to answer the questions:
Liquid
Vapor
Temperature,
Pressure,
°C
torr
A
400
100.8
C4H,OH
C2H5OC2H5
B
400
17.9
(1) In which liquid are the intermolecular attractive forces the
weakest ?
(2) Which liquid would be expected to have the highest vapor
pressure at 59.3 °C?
The normal boiling point of liquid ethane thiol is 309 K.
Assuming that its molar heat of vaporization is constant at 28.0
kJ/mol, the boiling point of C2H5SH when the external pressure
is 1.29 atm is
K.
The molar enthalpy of vaporization of NH3 is 23.3 kJ/mol at its
normal boiling point of -33.3 °C. How much energy is required
to evaporate 2.50 kg of ammonia at -33.3 °C?
58.3 kJ
3.42×103 kJ
1.59×104 kJ
992 kJ
4.89×103 kJ
Refer to the following phase diagram (not to scale!) for neon:
26.2
1.00
P
atm
0.425
24.4 24.5
27.1
44.4
I Kelvin
A sample of neon at a pressure of 0.425 atm and a temperature
of 19.3 K is compressed at constant temperature to a pressure
of 30.2 atm. Which of the following are true?
Choose all that apply
The sample is initially a solid.
The final state of the substance is a solid.
The liquid initially present will vaporize.
The sample is initially a gas.
No phase change will occur.
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