Unit 4 Chemistry Review: IMFs, Polarity, Lewis Structures

Quiz
•
Science
•
9th - 12th Grade
•
Hard
+2
Standards-aligned
Stephen Francz
Used 65+ times
FREE Resource
20 questions
Show all answers
1.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Which of the following can result in a London dispersion force?
When a non-polar molecule becomes slightly polar for an instant
When the oppositely charged ends of a polar molecule attract each other.
When there is very strong dipole-dipole attraction between a hydrogen atom and a polar molecule
When an ion comes close enough to a non-polar molecule to change its electron density.
2.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
In liquid sulfur dioxide, which of the following types of intermolecular force(s) would be present?
London dispersion forces
London dispersion forces, dipole-dipole forces
London dispersion forces, dipole-dipole forces, hydrogen bonding
London dispersion forces, dipole-dipole forces, hydrogen bonding, covalent bonds
Tags
NGSS.HS-PS1-3
3.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Which one of the following substances will have hydrogen bonding as one of its intermolecular forces?
IV only
II and V
I and III
IV and II
Tags
NGSS.HS-PS1-4
4.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
Which phrase best completes the following statement: “The electrons in a bond between two iodine atoms (I2) are shared…”?
Equally, and the resulting bond is polar.
Equally, and the resulting bond is nonpolar.
Unequally, and the resulting bond is polar.
Unequally, and the resulting bond is nonpolar
5.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Which number represents the hydrogen that is capable of hydrogen bonding in acetic acid?
(i)
(ii)
(iii)
(iv)
Tags
NGSS.HS-PS1-3
6.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Consider the following structures. If the A-B bonds are polar, which of the following molecules are polar?
I and III
II and V
I, II, and IV
II and IV
Tags
NGSS.HS-PS1-2
7.
MULTIPLE CHOICE QUESTION
1 min • 1 pt
Water (H2O) and dihydrogen monosulfide (H2S) have similar chemical formulas and structures. At room temperature, H2O is a liquid and H2S is a gas. Which of the following best explains this difference?
H2S molecules are larger and exhibit stronger London dispersion forces and require a greater amount of energy to break.
H2S molecules are larger and thus the electrons are not attracted as strongly, which makes the covalent bonds in H2S molecules easier to break.
H2O molecules exhibit hydrogen bonding, and thus the attractive forces between water molecules are stronger than the attractive forces between H2S molecules.
H2O molecules are smaller and thus exhibit weaker London dispersion forces and require a lesser amount of energy to break
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