WorksheetsAP Bonding
Total questions: 24
Worksheet time: 29mins
Which of the following scientific claims about the bond in the molecular compound is HFmost likely to be true?
There is a partial negative charge on the H atom.
Electrons are shared equally between the H and F atoms.
The bond is extremely weak.
The bond is highly polar.
A particle-level diagram of a metallic element is shown above. Typically, metals are both malleable and ductile. The best explanation for these properties is that the electrons involved in bonding among metal atoms are
unequally shared and form nondirectional bonds
unequally shared and form highly directional bonds
equally shared and form nondirectional bonds
equally shared and form highly directional bonds
Two pure elements react to form a compound. One element is an alkali metal, X, and the other element is a halogen, Z. Which of the following is the most valid scientific claim that can be made about the compound?
It has the formula XZ2
It does not dissolve in water.
It contains ionic bonds.
It contains covalent bonds.
The elements C and Se have the same electronegativity value, 2.55. Which of the following claims about the compound that forms from C and Se is most likely to be true?
The carbon-to-selenium bond is unstable.
The carbon-to-selenium bond is nonpolar covalent.
The compound has the empirical formula CSe.
A molecule of the compound will have a partial negative charge on the carbon atom.
Which of the following correctly indicates whether the solid represented by the particulate model shown above conducts electricity and explains why or why not?
It conducts electricity because it is made of positive and negative ions.
It conducts electricity because it is made of particles of different sizes.
It does not conduct electricity because its ions cannot move freely within the solid.
It does not conduct electricity because there are small spaces between the particles.
Has a central atom with less than an octet of electrons
H2O
NH3
BH3
CH4
SiH4
Has two lone pairs of electrons
H2O
NH3
BH3
CH4
SiH4
The energy required to dissociate an ionic solid into gaseous ions (lattice energy) for the
compounds NaF and MgF2 is shown in the table above. On the basis of Coulomb’s law, which of the following best helps to explain the large difference between the lattice
energies of NaF and MgF2?
The solubility of MgF2 is less than that of NaF.
The electronegativity of Mg is greater than that of Na.
The mass of the Mg cation is greater than that of the Na cation.
The charge of the Mg cation is larger than that of the Na cation.
The diagram above shows two resonance structures for a molecule of C6H6 . The phenomenon shown in the diagram best supports which of the following claims about the bonding in C6H6?
In the C6H6 molecule, all the bonds between the carbon atoms have the same length.
Because of variable bonding between its carbon atoms, C6H6 is a good conductor of electricity.
The bonds between carbon atoms in C6H6 are unstable, and the compound decomposes quickly.
The C6H6 molecule contains three single bonds between carbon atoms and three double bonds between carbon atoms.
Which of the following Lewis diagrams best represents the bonding in the N2O molecule, considering formal charges?
Of the following compounds, which is the most ionic?
SiCl4
BrCl
PCl3
Cl2O
CaCl2
Of the following molecules, which has the largest dipole moment?
CO
CO2
O2
HF
F2
Of the following single bonds, which is the LEAST polar?
N-H
H-F
O-F
I-F
Resonance is most commonly used to describe the bonding in molecules of which of the following?
CO2
O3
H2O
CH4
SF6
Steel is an alloy containing Fe atoms and C atoms. Which of the following diagrams best represents the particle-level structure of steel?
The electron-dot structure (Lewis structure) for which of the following molecules would have two unshared pairs of electrons on the central atom?
H2S
NH3
CH4
HCN
CO2
The table above provides some information about two types of steel, both of which are alloys of iron and carbon. Which of the following best helps to explain why high-carbon steel is more rigid than low-carbon steel?
Elemental carbon is harder than elemental iron.
The additional carbon atoms within the alloy make the high-carbon steel less dense.
The additional carbon atoms within the alloy increase the thermal conductivity of the high-carbon steel.
The additional carbon atoms within the alloy make it more difficult for the iron atoms to slide past one another.
The lattice energy of a salt is related to the energy required to separate the ions. For which of the following pairs of ions is the energy that is required to separate the ions largest? (Assume that the distance between the ions in each pair is equal to the sum of the ionic radii.)
Na+(g) and Cl−(g)
Cs+(g) and Br−(g)
Mg2+(g) and O2−(g)
Ca2+(g) and O2−(g)
The melting point of MgO is higher than that of NaF. Explanations for this observation include which of the following?
I. Mg2+ is more positively charged than Na+.
II. O2- is more negatively charged than F-.
III. The O2- ion is smaller than the F- ion.
II only
I and II only
I and III only
II and III only
I, II, and III
The molecule with only one double bond
CO2
H2O
CH4
C2H4
PH3
The potential energy of a system of two atoms as a function of their internuclear distance is shown in the diagram above. Which of the following is true regarding the forces between the atoms when their internuclear distance is x?
The attractive and repulsive forces are balanced, so the atoms will maintain an average internuclear distance x.
There is a net repulsive force pushing the atoms apart, so the atoms will move further apart.
There is a net attractive force pulling the atoms together, so the atoms will move closer together.
It cannot be determined whether the forces between atoms are balanced, attractive, or repulsive, because the diagram shows only the potential energy
Which of the following arranges the molecules N2, O2, and F2 in order of their bond enthalpies, from least to greatest?
F2 < O2 < N2
O2 < N2 < F2
N2 < O2 < F2
N2 < F2 < O2
Which of the following molecules contains only single bonds?
CH3COOH
CH3CH2COOCH3
C2H6
C6H6
HCN
Which of the following molecules has the shortest bond length?
N2
O2
Cl2
Br2
I2
