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WorksheetsChemistry Unit 9 Test
Total questions: 25
Worksheet time: 13mins
Which of the following substances would you expect to have the highest melting point
carbon dioxide (CO2)
sulfur dioxide (SO2)
hydrogen peroxide (H2O2)
aluminum oxide (Al2O3)
When two atoms share three pairs of electrons with one another, what type of bond do they form?
triple ionic bond
triple covalent bond
double ionic bond
double covalent bond
What happens to electrons during covalent bonding?
They are given up by atoms.
They are taken in by atoms.
They are shared between atoms.
They are transferred between atoms.
Which of the following pairs of elements are most likely to form polar covalent bonds. (select all correct answers)
magnesium and nitrogen
silicon and oxygen
silicon and phosphorus
sulfur and chlorine
What is the largest difference in electronegativity between two atoms that form a nonpolar covalent bond?
0.4
2.78
0.0
1.7
Hydrogen and oxygen are gasses at room temperature because they have ____________________, while water is a liquid at room temperature because it has _____________________.
hydrogen bonding, London dispersion forces
London dispersion forces, hydrogen bonding
strong intermolecular forces, no intermolecular forces
hydrogen bonding, dipole-dipole forces
Hydrogen bonding most likely occurs in which compound?
NH3
LiH
CH4
SF2
Which element would be likely to form a strong intermolecular bond with hydrogen?
phosphorus
carbon
oxygen
aluminum
Which best explains the surface tension of water?
Density is greater at the surface, so there are more water molecules are there and the hydrogen bonding works better.
Intermolecular forces are greater at the surface.
Pressure increases with depth, so the hydrogen bonding is only strong enough to have surface tension at the top.
Surface molecules of water are attracted only downward and sideways by hydrogen bonding.
Which statement best describes the dipoles that cause London dispersion forces?
The dipoles are caused by a difference in electronegativity.
The dipoles are permanent separations of charges.
The dipoles are instantaneous and temporary.
The dipoles contain a hydrogen atom.
What causes the intermolecular force produced by hydrogen bonding?
Hydrogen atoms bonded to very electronegative elements have a strong partial negative charge because all their electrons are in the covalent bonds.
Hydrogen atoms bonded to very electronegative elements have a strong partial positive charge because none of their electrons are in the covalent bonds.
Hydrogen atoms bonded to very electronegative elements have a strong partial negative charge because none of their electrons are in the covalent bonds.
Hydrogen atoms bonded to very electronegative elements have a strong partial positive charge because all their electrons are in the covalent bonds.
What makes up the "poles" of a polar bond?
a charge of plus one and a charge of minus one
a north pole and a south pole
a partial negative charge and a partial positive charge
a proton and an electron
What do each of the two lines in this Lewis structure of sulfur difluoride represent?
1 bonding electron
2 bonding electrons
non valence electrons
a space where an electron is needed
Which statement describes the strength of dipole-dipole forces as an intermolecular force?
Dipole-dipole force is equal to the force between atoms within the molecule.
Dipole-dipole force is a fairly strong intermolecular force.
Dipole-dipole force is the weakest intermolecular force.
What causes London dispersion forces?
attraction between hydrogen and more electronegative atoms
constant motion of electrons randomly creating instantaneous dipoles
sharing of electrons in polar covalent bonds
differences in electronegativity of atoms below 1.7
Which pair of elements will form bonds with the highest degree of polarity?
germanium and sulfur
oxygen and carbon
phosphorus and chlorine
silicon and iodine
Select all statements that must be true for a molecule to be a dipole (polar molecule). (Select all correct answers)
molecular geometry that allows the electrons to be perfectly balanced on both sides of the molecule
molecular geometry that allows more electrons to be on one side the molecule than the other
polar covalent bonds
nonpolar covalent bonds
ionic bonds
Based on the types of bonds and the molecular geometry, this molecule is _______________.
a polar compound
a nonpolar compound
an ionic compound
cannot tell
Based on the types of bonds and the molecular geometry, this molecule is _______________.
a nonpolar compound
an ionic compound
a polar compound
cannot tell
Molecules of this compound most likely have which intermolecular forces?
dipole-dipole forces
London dispersion forces
hydrogen bonding
cannot tell
Molecules of this compound most likely have which intermolecular forces?
dipole-dipole forces
London dispersion forces
hydrogen bonding
cannot tell
1. Molecules of this compound most likely have which intermolecular forces?
dipole-dipole forces
London dispersion forces
hydrogen bonding
cannot tell
Which of the following compounds likely has a lower boiling point?
cannot tell
Arsenic trifluoride (AsF3) and carbon tetrachloride (CCl4) are both liquids at room temperature. Which will likely have stronger surface tension, and why?
carbon tetrachloride because it is more polar
carbon tetrachloride because it is nonpolar
arsenic trifluoride because it has stronger dipole-dipole forces
arsenic fluoride because its bonds are less polar
The electrostatic attraction between a silicon atom and a chlorine atom will be most likely _______________________.
an inoic bond
a metallic bond
a polar covalent bond
a nonpolar covalent bond
