In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) SiF₄ and LaF₃ (for ionic or molecular substances) to assign a name to each compound: (b) FeCl₂ and ReCl₆ (c) PbCl₄ and RbCl.

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (a) TiCl₄ and CaF₂ (b) ClF₃ and VF₃

In the following pairs of binary compounds, determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances) to assign a name to each compound: (c) SbCl₅ and AlF₃.

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: c. SO₃²⁻

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: d. HCN (H and N are both bonded to C),

Draw Lewis structures that satisfy the octet rule for the following molecules and ions: f. HOCl

Write Lewis structures that satisfy the octet rule for the following molecules and ions: a. NH4+, b. C2F4 (the two C atoms are bonded to one another), c. COCl2 (the Cl atoms are bonded to C), d. HSO3− (H is bonded to one of the O atoms), e. HNC (H and C are both bonded to N), f. ClO3−.

Which one of these statements about formal charge is true? (a) Formal charge is the same as oxidation number. (b) To draw the best Lewis structure, you should minimize formal charge. (c) Formal charge takes into account the different electronegativities of the atoms in a molecule. (d) Formal charge is most useful for ionic compounds. (e) Formal charge is used in calculating the dipole moment of a diatomic molecule.

For each of the following ions of nitrogen and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: c. NO2+.

(b) With what allotrope of oxygen is it isoelectronic?

Consider the formate ion, HCO₂^-, which is the anion formed when formic acid loses an H⁺ ion. The H and the two O atoms are bonded to the central C atom. (b) Are resonance structures needed to describe the structure?

Predict the ordering, from shortest to longest, of the bond lengths in CO, CO₂, and CO₃^2- .

Consider a Lewis structure for SO3 that satisfies the octet rule. Which of the following statements is or are true?

i. SO3 has three equivalent resonance structures.

ii. There are one shorter and two longer S—O bond lengths in SO3.

iii. The S atom in SO3 has a nonzero formal charge.

Which of the following statements about benzene, C6H6, is or are true?

i. Benzene has two equivalent resonance structures.

ii. There are no nonbonding pairs in the Lewis structure for benzene.

iii. Benzene has three short and three long C—C bonds.

b. Which of these compounds or ions is an exception to the octet rule: nitrogen dioxide, borohydride (BH4−), borazine (B3N3H6 which is analogous to benzene with alternating B and N in the ring), or boron trichloride?

Draw the Lewis structures for each of the following molecules or ions. Identify instances where the octet rule is not obeyed; state which atom in each compound does not follow the octet rule; and state how many electrons surround these atoms: a. NO, b. BF₃, c. ICl₂⁻, d. OPBr₃ (the P is the central atom), e. XeF₄.

In the vapor phase, BeCl₂ exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule?

In the vapor phase, BeCl₂ exists as a discrete molecule. (c) On the basis of the formal charges, which Lewis structure is expected to be dominant for BeCl₂?

(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe¬O double bonds. (b) Do any of these resonance structures satisfy the octet rule for every atom in the molecule? (c) Do any of the four Lewis structures have multiple resonance structures? If so, how many resonance structures do you find? (d) Which of the Lewis structures in part (a) yields the most favorable formal charges for the molecule?

There are many Lewis structures you could draw for sulfuric acid, H₂SO₄ (each H is bonded to an O). (a) What Lewis structure(s) would you draw to satisfy the octet rule?

There are many Lewis structures you could draw for sulfuric acid, H2SO4 (each H is bonded to an O). (b) What Lewis structure(s) would you draw to minimize formal charge?

Some chemists believe that satisfaction of the octet rule should be the top criterion for choosing the dominant Lewis structure of a molecule or ion. Other chemists believe that achieving the best formal charges should be the top criterion. Consider the dihydrogen phosphate ion, H₂PO₄^-, in which the H atoms are bonded to O atoms. (b) What is the predicted dominant Lewis structure if achieving the best formal charges is the top criterion?

State whether each of these statements is true or false. e. Energy is stored in chemical bonds.