WorksheetsBonding Unit Review
Total questions: 42
Worksheet time: 1hrs 17mins
Based on your Reference Tables, the atoms of which of these elements have the strongest attraction for electrons in a chemical bond?
N
Na
P
Pt
A barium atom attains a stable electron configuration when it bonds with
one chlorine atom
two chlorine atoms
one sodium atom
two sodium atoms
Which pair of elements below will form a compound with the greatest ionic character?
Pb and F
Ca and O
Na and Cl
Cs and N
Which statement describes the energy and bonding changes as two atoms of fluorine become a molecule of fluorine?
Energy is absorbed as a bond is broken.
Energy is absorbed as a bond is formed.
Energy is released as a bond is broken.
Energy is released as a bond is formed.
Which element has metallic bonds at room temperature?
bromine
cesium
krypton
sulfur
Which statement describes the charge distribution and the polarity of a CH4 molecule?
The charge distribution is symmetrical and the molecule is nonpolar.
The charge distribution is asymmetrical and the molecule is nonpolar.
The charge distribution is symmetrical and the molecule is polar.
The charge distribution is asymmetrical and the molecule is polar.
State the shape of this molecule.
Bent
Pyramidal
Linear
Tetrahedral
The bonds in CO2 are best described as
covalent, because valence electrons are shared
covalent, because valence electrons are transferred
ionic, because valence electrons are shared
ionic, because valence electrons are transferred
A substance that has a melting point of 1074 K conducts electricity when dissolved in water, but does not conduct electricity in the solid phase. The substance is most likely
an ionic solid
a network solid
a metallic solid
a molecular solid
Which substance has nonpolar covalent bonds?
SiO2
SO3
Cl2
CCl4
A molecule must be nonpolar if the molecule
is linear
is neutral
has ionic and covalent bonding
has a symmetrical charge distribution
What is the number of pairs of electrons shared in a molecule of N2?
1
2
3
6
Which substance is an electrolyte?
CH3OH
C6H12O6
H2O
CaCl2
Which Group 16 element combines with hydrogen to form a compound that has the strongest hydrogen bonding between its molecules?
tellurium
selenium
sulfur
oxygen
Which statement describes a multiple covalent bond?
Two electrons are shared.
Four electrons are shared.
Two electrons are transferred.
Four electrons are transferred.
A substance was found to be a soft, non-conducting solid at room temperature. The substance is most likely
an ionic solid
a network solid
a molecular solid
a metallic solid
Which formulas represent one ionic compound and one molecular compound?
N2 and SO2
Cl2 and H2S
BaCl2 and N2O4
NaOH and BaSO4
What occurs in order to break the bond in a Cl2 molecule?
Energy is released.
Energy is absorbed.
The molecule creates energy.
The molecule destroys energy.
The chemical bond in a hydrogen molecule is
nonpolar covalent
polar covalent
ionic
electrovalent
A molecular compound is formed when a chemical reaction occurs between atoms of
chlorine and sodium
chlorine and yttrium
oxygen and hydrogen
oxygen and magnesium
Which of the following compounds has the highest boiling point?
H2Te
H2S
H2Se
H2O
Which type of bond exists between an atom of carbon and an atom of fluorine?
ionic
metallic
polar covalent
nonpolar covalent
Which type of bond is found between atoms of solid cobalt?
nonpolar covalent
polar covalent
metallic
ionic
Which formula represents a polar molecule?
H2
H2O
CO2
CCl4
Which type of substance can conduct electricity in the liquid phase but not in the solid phase?
ionic compound
molecular compound
metallic element
nonmetallic element
Molecules in a sample of NH3(l) are held closely together by intermolecular forces
existing between ions
existing between electrons
caused by different numbers of neutrons
caused by unequal charge distribution
In aqueous solution, a chloride ion is attracted to which end of the water molecule?
the hydrogen end, which is the positive pole
the hydrogen end, which is the negative pole
the oxygen end, which is the positive pole
the oxygen end, which is the negative pole
Two fluorine atoms are held together by a covalent bond. Which statement correctly describes this bond?
It is polar and forms a polar molecule.
It is polar and forms a nonpolar molecule.
It is nonpolar and forms a polar molecule.
It is nonpolar and forms a nonpolar molecule.
What is the maximum number of covalent bonds that a carbon atom can form?
1
2
3
4
Which molecule will have a triple covalent bond?
F2
O2
Cl2
N2
Which substance is correctly paired with its type of bonding?
NaBr – nonpolar covalent
HCl – nonpolar covalent
NH3 – polar covalent
Br2 – polar covalent
Covalent bonds are formed when electrons are
transferred from one atom to another
captured by the nucleus
mobile within a metal
shared between two atoms
Which of the following solids has the highest melting point?
H2O(s)
Na2O(s)
SO2(s)
CO2(s)
The unusually high boiling point of H2O is primarily due to the presence of
hydrogen bonds
ionic bonds
van der Waals forces
molecule-ion attractions
Based on Reference Table S, the atoms of which of these elements have the strongest attraction for electrons in a chemical bond?
N
Na
P
Pt
Which particles may be gained, lost, or shared by an atom when it forms a chemical bond?
Nucleons
Protons
Neutrons
Electrons
Which type of bond is formed by the transfer of electrons from one atom to another?
hydrogen bond
ionic bond
covalent bond
coordinate covalent bond
Which atoms are most likely to form covalent bonds?
nonmetal atoms that share electrons
metal atoms that share protons
nonmetal atoms that share protons
metal atoms that share electrons
H-I has what type of intermolecular forces of attraction between many molecules in a sample?
Dipole-Dipole
van der Waals
Hydrogen Bonding
Polar Covalent
Hydrogen bonds would NOT exist in a 100g sample of which of the following compounds?
H2O
HF
NH3
H2S
Which type of intermolecular force is the strongest?
Hydrogen Bonding
Covalent Bonding
Van Der Waals
Dipole-Dipole
A substance with which type of intermolecular forces would have the LOWEST melting and boiling points?
Hydrogen Bonding
Van Der Waals
Polar Covalent Bonding
Dipole-Dipole
