GenChem Q3 Quiz1 Flashcards
Which of the following explains why water is a universal solvent?
a. Due to the high specific heat of water
b. Due to the strong surface tension of water
c. Due to the cohesiveness and adhesiveness of water molecule
d. Due to its polarity, that allows to dissolve a great number of substances that contain ionized atoms or polar molecules.
Due to its polarity, that allows to dissolve a great number of substances that contain ionized atoms or polar molecules.
Which of the following choices would mean interaction between molecules?
a. Coulomb`s Law
b. Electrostatic force
c. Intermolecular force
d. Intramolecular forces
Intermolecular force
The strongest interparticle attractions exist between particles of a __________ and the weakest interparticle attractions exist between particles of a __________.
a. solid, liquid
b. solid, gas
c. liquid, gas
d. liquid, solid
e. gas, solid
f. gas, liquid
solid, gas
Which of the following compounds has a strong intermolecular force and high viscosity?
a. acetone
b. ethanol
c. glycerol
d. water
glycerol
Which from the choices refers to the amount of heat needed to raise the temperature of 1 gram of a substance 1 degree Celsius (°C)?
a. cohesion
b. polarity
c. specific heat
d. surface tension
specific heat
Which one of the following exhibits dipole-dipole attraction between molecules?
a. XeF4
b. AsH3
c. CO2
d. BCl3
e. Cl2
AsH3
True or False. Hydrogen bonding refers to a hydrogen from one molecule bonded to N, F, and Br to the other molecule.
False
Which of the following physical property of a liquid allows a spider to float on water?
a. Capillary action
b. Surface tension
c. Vapor pressure
d. Molar heat of vaporization
Surface tension
What is the predominant intermolecular force in CBr4?
a. London-dispersion forces
b. ion-dipole attraction
c. ionic bonding
d. dipole-dipole attraction
e. hydrogen-bonding
London-dispersion forces
What type of intermolecular force holds the molecules of water together?
a. covalent bond
b. hydrogen bond
c. ion-ion interaction
d. London dispersion force
hydrogen bond
True or False. Ion-dipole interaction leads to the building of forces between nonpolar molecules.
False
What type of intramolecular force holds the atoms of water together?
a. covalent bond
b. hydrogen bond
c. ion-ion interaction
d. polar covalent bond
covalent bond
For which of the following molecules apply dipole-dipole interactions?
a. CH4
b. C6H6
c. CCl4
d. CH2Cl2
CH2Cl2
When NaCl dissolves in water, aqueous Na+ and Cl– ions result. The force of attraction that exists between Na+ and water is called a(n) __________ interaction.
a. dipole-dipole
b. ion-ion
c. hydrogen bonding
d. ion-dipole
e. London dispersion force
ion-dipole
True or False. According to ion-ion interaction, the electrostatic force increases as the size of the magnitude of charges decreases.
False
What do you think is the effect of weak intermolecular forces to the vapor pressure of acetone?
a. low vapor pressure
b. high vapor pressure
c. does not affect at all
d. unstable vapor pressure
high vapor pressure
Hydrogen bonding is a special case of __________.
a. London-dispersion forces
b. ion-dipole attraction
c. dipole-dipole attractions
d. ion-ion interactions
dipole-dipole attractions
Rank the following in terms of increasing boiling point:
CaBr2, C2H5OH, C4H10
C4H10 < C2H5OH < CaBr2
Rank the following in terms of increasing melting point
MgCl2, NaCl, AlCl3
NaCl < MgCl2 < AlCl3
Why do ice floats on water?
a. Ice is denser than water
b. Ice has a crystalline structure
c. Water is less dense than ice cube
d. Water molecules of ice cube expand that decreases its density
Water molecules of ice cube expand that decreases its density
Which of the following types of intermolecular forces is the weakest?
a. Dipole-dipole
b. Hydrogen bonding
c. Ion-ion interaction
d. London dispersion
London dispersion
Which of the following best describes a hydrophobic compound?
a. nonpolar which doesn’t dissolve in water
b. polar molecules and ready to be dissolved in water
c. nonpolar molecules and ready to be dissolved in water
d. polar and ionic molecules and ready to be dissolved in water
nonpolar which doesn’t dissolve in water
True or False. Dipole-dipole interaction is significant between an dipole and a dipole molecule.
True
Which of these molecules will NOT form hydrogen bonds with water?
a. hydrogen fluoride
b. methane gas
c. ammonia
d. methanoic acid
methane gas
Which of the following choices is used to explain the behavior of states of matter from a microscopic point of view?
a. Atomic Theory
b. Coulomb`s Law
c. Kinetic Molecular Theory
d. Intramolecular forces
Kinetic Molecular Theory
Rank these substances from lowest to highest intermolecular forces
HF, F2, PCl3
F2 < PCl3 < HF
When water is poured into a test tube, a concave surface is usually observed. Why do you think this happens?
a. Because water molecules touching the glass adhere less to the test tube.
b. Because water molecules touching the glass adhere more to the test tube.
c. Because water molecules touching the glass adhere more to other water molecules.
d. Because water molecules touching the glass did not get attracted to the wall of the test tube.
Because water molecules touching the glass adhere more to the test tube.
Which of the intermolecular forces exists between molecules of iodine gas?
a. Dipole-dipole
b. Hydrogen bonding
c. Ion-ion interaction
d. London dispersion
London dispersion
Of the following substances, only __________ has London dispersion forces as its only intermolecular force.
a. CH3OH
b. NH3
c. H2S
d. CH4
e. HCl
CH4
True or False. London dispersion is evident in nonpolar molecules.
True
