AP Bonding

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.

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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.

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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.

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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.

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Which of the following Lewis diagrams best represents the bonding in the N₂O molecule, considering formal charges?

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