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Net molecular dipole

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1. Which of the following molecules has NO net molecular dipole?
a. CH3OH
b. CH2O
c. CH3Cl
d. H2C=CH2

2. Which of the following molecules can hydrogen bond to another of the same compound?
c. (CH3CH2)2CHOH

3. What term best describes the relationship between the following two compounds?
CHCl=CHCl vs CCl2=CH2
a. same compounds
b. unrelated compounds
c. constitutional isomers
d. geometric isomers

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1. The net molecular dipole exist due to the fact that some element is more electronegative then others. The most electronegative ...

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Multiple Choice questions on General Chemistry

1) According to the kinetic-molecular theory, molecules of different gases at the same temperature always have the same __________.

a. average density
b. volume
c. pressure
d. molecular mass
e. average kinetic energy

2) The van der Waals equation for real gases recognizes that ____________.

a. the non-zero volumes of gas particles effectively decrease the amount of "empty space" between them
b. the molecular attractions between particles of gas decreases the pressure exerted by the gas
c. molar volumes of gases of different types are different
d. gas particles have non-zero volumes and interact with each other
e. All of the above statements are true.

3) As a solid element melts, the atoms become ________ and they have __________ attraction for one another.

a. closer together, more
b. larger, greater
c. more separated, more
d. closer together, less
e. more separated, less

4) The weakest interparticle attractions exist between particles of a _____ and the strongest interparticle attractions exist between particles of a _____.

a. liquid, gas
b. gas, liquid
c. liquid, solid
d. solid, gas
e. gas, solid

5) Which one of the following exhibits dipole-dipole attraction between molecules?

a. BCl3
b. XeF4
c. AsH3
d. Cl2
e. CO2

6) The strength of London dispersion forces between like-molecules depends on __________ and __________.

a. polarizability, size
b. molecular mass, volatility
c. molecular mass, polarizability
d. size, shape
e. vapor pressure, size

7) Elemental iodine (I2) is a solid at room temperature. What is the major attractive force that exists among different I2 molecules in the solid?

a. ionic-dipole interactions
b. dipole-dipole rejections
c. covalent-ionic interactions
d. dipole-dipole attractions
e. London dispersion forces

8) What intermolecular force is responsible for the fact that ice is less dense than liquid water?

a. London dispersion forces
b. Dipole-dipole forces
c. Ionic bonding
d. Hydrogen bonding
e. Ion-dipole forces

9) The heat of fusion of water is 6.01 kJ / mol. The heat capacity of liquid water is 75.2 J / mol . K. The conversion of 50.0 g of ice at 0.00oC to liquid water at 22.0oC requires ___________ kJ of heat.

a. 0.469
b. 17.2
c. 3.8 x 102
d. Insufficient data are given.

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