7. [intermolecular Forces] Practice
-
A.) What would the 3-D geometric configuration of the following Lewis structure be?
-
Bent (tetrahedral)
-
Trigonal planar
-
Linear
-
Octahedral
-
![7. [intermolecular Forces] Practice - Quiz](/quiz-school/images/description/Miscellaneous/2.jpg "7. [intermolecular Forces] Practice - Quiz")
NOTE THAT THIS IS THE PRACTICE QUIZ. TAKING THIS QUIZ WILL NOT AFFECT YOUR GRADE.
Quiz Preview
- 2.
D.) A drop of each of the following compounds was placed on a table and the amount of time required for the compound to evaporate was recorded. Which of the compounds likely had the weakest intermolecular forces?CompoundTime to EvaporateA10 sB48 sC30 sD120 s
-
A
-
B
-
C
-
D
Correct Answer
A. AExplanation
Intermolecular forces hold molecules together. When a substance evaporates, its molecules spread out to become a gas. The substance that evaporates the fastest is likely to have weak intermolecular forces.Rate this question:
-
- 3.
A.) What geometric configuration would a molecule of have?
-
Trigonal planar
-
Tetrahedral
-
Linear
-
Octahedral
Correct Answer
A. Trigonal planarExplanation
Boron only has three valence electrons, which means that it can only form three covalent bonds. When it does, there are no nonbonding pairs to cause repulsion, so the 3-D shape is simply triangular and flat.Rate this question:
-
- 4.
C.) If the H-F bond in the following molecule is polar, which of the following statements is true?
-
The molecule is a dipole.
-
The molecule is not a dipole.
-
The molecule is nonpolar.
-
The molecule has no dipole moment.
Correct Answer
A. The molecule is a dipole.Explanation
If the bond between Hydrogen and Fluorine is polar, then the electrons will spend more time orbiting the fluorine nucleus. This means that the Fluorine atom will have a partial negative charge while the Hydrogen will be partially positive. If you were to split this molecule in half, there would be a positive end and a negative end, so this molecule is a dipole.Rate this question:
-
- 5.
E.) Which of the following solvents could be used to dissolve sodium chloride?
-
Water
-
Vegetable Oil
-
Methanol
-
Acetone
Correct Answer
A. WaterExplanation
The charges of ionic compounds are attracted to the partial charges of polar molecules. Sodium chloride (an ionic compound) would therefore most likely dissolve in a polar solvent.Rate this question:
-
- 6.
E.) Solvent X is a highly polar solvent. Which of the following would NOT dissolve in (or mix with) solvent X?
-
Vegetable oil
-
Table Salt
-
Water
-
HCl
Correct Answer
A. Vegetable oilExplanation
"Like dissolves like", which means that nonpolar substances only dissolve in nonpolar solvents. Vegetable oil is a nonpolar substance, so it would no likely dissolve in solvent X. It is also worth mentioning that ionic compounds dissolve in polar solvents because the partial positive and negative charges of the polar molecules are attracted to the charged ions of ionic compounds.Rate this question:
-
- 7.
B.) Which of the following pairs of elements will likely form a polar covalent bond?
-
H + Cl
-
Na + Na
-
Na + Cl
-
H + H
Correct Answer
A. H + ClExplanation
Polar covalent bonds are formed between two nonmetal elements that do not share electrons evenly. In the case of Hydrogen and Chlorine, neither element is electronegative enough to remove electrons from the other. However, Chlorine is more electronegative than Hydrogen, so the electrons in the covalent bond that the two atoms share will spend more time orbiting Chlorine's nucleus.Rate this question:
-
- 8.
D.) Which of the following compounds will likely have the highest melting point?
-
NaCl (ionic)
-
CH4 (nonpolar)
-
CH3OH (slightly polar)
-
HCl (polar)
Correct Answer
A. NaCl (ionic)Explanation
Intermolecular forces between dipoles (like HCl) are stronger than they are between nonpolar compounds. However, intermolecular forces are, at best, between two partially charged atoms (that is, they have charges with values < 1). Ionic compounds (like NaCl) are between atoms with a charge of at least 1, so their forces of attraction will be stronger than any intermolecular force.Rate this question:
-
- 9.
B.) Which of the following pairs of elements will likely form a nonpolar covalent bond?
-
H + Cl
-
Na + Na
-
Na + Cl
-
H + H
Correct Answer
A. H + HExplanation
Nonpolar covalent bonds are formed when two atoms share electrons evenly. In the case of two Hydrogen atoms (a diatomic element), the electrons are shared due to Hydrogen being a nonmetal with a relatively high electronegativity. Because the two atoms are likely identical, the electrons spend an equal amount of time orbiting both nuclei.Rate this question:
-
- 10.
F.) Hemoglobin is a large molecule with no repeating structures. Which of the following terms can be used to describe hemoglobin?
-
Macromolecule
-
Network Solid
-
Allotrope
-
Polymer
Correct Answer
A. MacromoleculeExplanation
A macromolecule is just a big molecule that does not have any repeating units.Rate this question:
-
- 11.
F.) Polystyrene (styrofoam) is made up of a chain of identical molecules (shown below). Which of the following words could be used to describe polystyrene?
-
Both polymer and network solid
-
Both allotrope and macromolecule
-
Both polymer and allotrope
-
Both allotrope and element
Correct Answer
A. Both polymer and network solidExplanation
Polystyrene is made up of a chain of repeating structures, making it a network solid (not a macromolecule). Because the repeating units are compounds (not elements), polystyrene is a polymer.Rate this question:
-
- 12.
C.) If all of the bonds in the following molecules are polar, which compound will NOT be a dipole?
-
A
-
B
-
C
-
D
Correct Answer
A. BExplanation
Carbon dioxide molecules are symmetrical. If you were to cut the molecule in half, both sides would be partially negatively charged because the Oxygen atoms on both sides pull electrons to themselves. In order to be a dipole, a molecule has to have a positive and a negative side.Rate this question:
-
Quiz Review Timeline (Updated): Mar 21, 2023 +
Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.
-
Current Version
-
Mar 21, 2023Quiz Edited by
ProProfs Editorial Team -
Oct 07, 2014Quiz Created by
David Schouweiler