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WorksheetsIMF RETAKE
Total questions: 23
Worksheet time: 31mins
Solid carbon tetrachloride, CCl4, is represented by the diagram above. The attractions between the CCl4 molecules that hold the molecules together in the solid state are best identified as
polar covalent bond
nonpolar covalent compounds
intermolecular attractions resulting from temporary dipoles
intermolecular attractions resulting from permanent dipoles
At 298 K and 1 atm, Br2 is a liquid and Cl2 is a gas. Those observations provide evidence that under the given conditions, the
Inter molecular forces among Br2 molecules are stronger than those among Cl2 molecules
forces among Cl2 molecules are stronger than the Cl-Cl bond
Br-Br bond is stronger than the Cl-Cl bond
Cl-Cl bond is stronger than the Br-Br bond
Based on the structural formulas, which of the following identifies the compound that is more soluble in water and best helps to explain why?
Ethane, because the electron clouds of its molecules are more polarizable than those of propanol.
Ethane, because its molecules can fit into the spaces between water molecules more easily than those of propanol can.
Propanol, because its molecules have a greater mass than the molecules of ethane have.
Propanol, because its molecules can form hydrogen bonds with water molecules.
Based on the information in the table above, which of the compounds has the highest boiling point, and why?
Butanal, because it can form intermolecular hydrogen bonds
Pentane, because it has the longest carbon chain
Pentane, becaue it has the most C-H bonds
Propanoic acid, because it can form intermolecular hydrogen bonds
If the pressure of each gas is increased until condensation occurs, which gas will condense first?
methane
Ethane
Butane
All the gases will condense at the same pressure.
The structural formulas for two isomers of 1,2-dichloroethene are shown above. Which of the two liquids will evaporate first and why?
The cis-isomer, because it has dipole-dipole interactions, whereas the trans-isomer has only London dispersion forces
The cis-isomer, because it has only London dispersion forces, whereas the trans-isomer also has dipole- dipole interactions
The trans-isomer, because it has dipole-dipole interactions, whereas the cis-isomer has only London dispersion forces
The trans-isomer, because it has only London dispersion forces, whereas the cis-isomer also has dipole- dipole interactions
The London (dispersion) forces are weakest for which of the following gases under the same conditions of temperature and pressure?
H2
O2
Xe
F2
N2
The diagram above is a molecular model of Oxygen gas
(O2 )that is just above its boiling point. Intermolecular forces between the gas molecules will cause them to condense into the liquid phase if the temperature is lowered. Which of the following best describes how the model is limited in its depiction of the phenomenon?
It does not show how hydrogen bonds are constantly forming, breaking, and reforming, which results in a net force of attraction between the molecules.
It does not show how the interactions between ions and the induced molecular dipoles result in a net force of attraction between the molecules.
It does not show how the interacting permanent dipoles of the molecules result in a net force of attraction between the molecules.
It does not show how the temporary fluctuating dipoles of the molecule result in a force of attraction between the molecules.
Consider the molecules represented abov. Nonane and 2,3,4-trifluoropentane have almost identical masses, but nonane has a significantly higher boiling point. Which of the following statements best helps explain this observation?
The C–F bond is easier to break than the C–H bond.
The C–F bond is more polar than the C–H bond.
The carbon chains are longer in nonane than they are in 2,3,4-trifluoropentane.
The carbon chains are farther apart in a sample of nonane than they are in 2,3,4- trifluoropentane.
Which of the following best helps to explain why CCl4 carbon tetrachloride is a liquid whereas CI4 (carbon tetraiodide) is a solid when both are at 25°C?
The dipole of the CCl4 molecule is larger than that of the CI4 (carbon tetraiodide) molecule because chlorine is more electronegative than iodine.
The dipole moment of the CI4 (carbon tetraiodide) molecule is larger than that of the CCl4 (carbon tetrachloride) molecule because there is stronger repulsion between electrons in the C-I bonds compared to the repulsion between electrons in the C- Cl bonds.
The London dispersion forces are stronger in CCl4 (carbon tetrachloride) than in CI4 (crabon tetraiodide) because chlorine is more electronegative than Iodine,
The London dispersion forces are stronger in CI4 (carbon tetraiodide) than in CCl4 (carbon tetrachloride) because CI4 (carbon tetraiodide) has a more polarizable (larger) electron cloud than CCl4 (carbon tetrachloride)
HF is smaller than F2, however, HF has a much higher boiling point than F2 has. Which of the following explains how the dispersion-force model of intermolecular attraction does not account for the unusually high boiling point of HF?
F2 is soluble in water, whereas HF is insoluble in water.
The F2 molecule has a greater mass than the HF molecule has.
Liquid F2 has weak dispersion force attractions between its molecules, whereas liquid HF has strong ionic interactions between H+ and F- ions.
Liquid F2 has weak dispersion force attractions between its whereas liquid HF has both weak dispersion force attractions and hydrogen bonding interactions between its molecules
Four different liquid compounds in flasks are represented above. The table above identifies the compounds. Flask C shows the most particles that have evaporated. Which of the following is not shown in the model but best helps to explain why flask C must contain pentane?
The random motion of the particles within the liquids
The relative speeds of the vapor particles in each flask
The strength of the intermolecular forces between the particles in the liquids
The structural formula of the molecules of the liquid and vapor in each flask
The diagram above represents a particle dissolved in water. Which of the following statements about the particle is correct?
The particle must be a cation because the negative end of each water molecule is pointed toward it.
The particle must be negatively charged because the positive end of each water molecule is pointed toward it.
The charge of the particle cannot be determined because water molecules have no net charge.
The charge of the particle cannot be determined because the water molecules are arranged symmetrically and their partial charges cancel.
In the diagram above, which of the labeled arrows identifies hydrogen bonding in water?
A
B
C
D
Which of the following is the strongest type of interaction that occurs between the atoms within the circled areas of the two molecules represented above?
Polar covalent bond
Nonpolar covalent bond
Hydrogen bond
London dispersion forces
In which of the following liquids do the intermolecular forces include dipole-dipole forces?
F2(l)
CH4(l)
CF4(l)
CH2F2(l)
Which of the substances shown above would probably dissolve in oil?
a
b
c
d
e
All intermolecular forces involve
bonding by sharing electrons
hydrogen atoms that are involved a bond
bonding by transferring electrons
slightly positive and slightly negatively poles
In order for a bond to be polar it must have
a difference in electronegativity greater than 0.4
a hydrogen atom bonded to an oxygen atom
at least two different atoms
electrons
In order to have London Dispersion forces, a molecule must have...
differences in electronegativity and lack of symmetry
a hydrogen atom bonded to a fluorine, oxygen or nitrogen
at least two different atoms, regardless of the arrangement
electrons
Which of the following statements is true?
If a molecule has hydrogen bonding, then it is also polar
If a molecule has London Dispersion Forces it must be non polar
If a molecule has hydrogen bonding, then it is non polar
If a molecule has London Dispersion Forces it must be polar
Intermolecular forces are important because...
they impact chemical reactions
they involve electrons
they impact the properties of a substance
all of these are true
In order to have hydrogen bonding, a molecule must have...
differences in electronegativity and lack of symmetry
a hydrogen atom bonded to a fluorine, oxygen or nitrogen
at least two different atoms, regardless of the arrangement
electrons
