Welcome to the Quiz!
This quiz contains 27 questions from a mix of 1 subtopics.
What type of dipole-dipole forces exist between polar molecules?
induced only
permanent only
induced and permanent
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The strength of induced dipole-dipole forces increases with the number of in a molecule.
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Which of the following factors affects the strength of permanent dipole-dipole forces?
the number of hydrogen atoms in the molecule
the strength of the covalent bond(s) in the molecule
the polarity of the molecule
the number of electrons in the molecule
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Which noble gases has the lowest boiling point?
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What is the main reason to explain why hydrogen chloride, HCl, has a higher boiling point than fluorine, F2?
HCl has a higher molecular mass
HCl has more electrons
HCl has stronger induced dipole-dipole forces
HCl has permanent dipole-dipole forces
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Give three properties of water that are influenced by hydrogen bonding?
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What type of intermolecular forces are present in iodine molecules, I2?
both permanent and induced dipole-dipole forces
induced dipole-dipole forces only
permanent dipole-dipole forces only
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What intermolecular forces are present in molecules of hydrogen iodide, HI?
(Select all that apply).
hydrogen bonding
covalent bonding
induced dipole-dipole forces
permanent dipole-dipole forces
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Polar covalent substances dissolve in polar solvents because the polar solute molecules and polar solvent molecules...
attract each other
have weak intermolecular forces
repel each other
have strong covalent bonds
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What is a hydrogen bond?
a type of ionic bond
a type of permanent dipole-dipole force
a type of covalent bond
a type of metallic bond
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Which trio of atoms can form hydrogen bonds?
C, N and O
O, F and Cl
N, O and F
F, Cl and Br
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Why is ice less dense than liquid water?
ice molecules are closer together than water molecules
ice has more hydrogen bonds than water
ice molecules are further apart than water molecules
ice has fewer hydrogen bonds than water
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Which of the following molecules has the lowest boiling point?
H2O
CH4
NH3
HCl
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Hydrogen bonds form between molecules that have a atom bonded to a very atom with a lone pair of electrons.
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Select ALL of the intermolecular forces that are present in molecules of hydrogen fluoride, HF.
hydrogen bonding
covalent bonding
permanent dipole-dipole forces
induced dipole-dipole forces
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How many hydrogen bonds can each molecule of H2O form?
0
1
2
3
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What is the strongest type of intermolecular force in H2O?
covalent bonds
induced dipole-dipole forces
permanent dipole-dipole forces
hydrogen bonds
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What is the strongest type of intermolecular force in CHCl3?
covalent
induced dipole-dipole
permanent dipole-dipole
hydrogen
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What is the strongest type intermolecular force in CH4?
covalent
induced dipole-dipole
permanent dipole-dipole
hydrogen
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Which type of intermolecular force exists between all molecules?
permanent dipole-dipole forces
induced dipole-dipole forces
hydrogen bonding
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Compare the strength of hydrogen bonds with covalent bonds.
hydrogen bonds are weaker than covalent bonds
hydrogen bonds are stronger than covalent bonds
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Which molecules are capable of hydrogen bonding?
(Select all that apply).
CH4
H2O
NH3
HCl
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Which molecule has the higher solubility in water?
C3H8
C2H5OH
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Which molecule has the lower boiling point?
CH3OH
C2H6
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Simple molecular substances have melting and boiling points because the weak forces require little energy to overcome.
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Select TWO properties of simple molecular substances:
high boiling points
low boiling points
unable to conduct electricity
conduct electricity
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In simple molecular substances, the individual molecules are held together by forces that exist between the molecules. These intermolecular forces are weak and so don't require very much to break. As a result most simple molecular substances exist in the state at room temperature.
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