(b) How many bonding electrons are in the structure?

(c) Would you expect the O—O bond in O₂ to be shorter or longer than the O—O bond in compounds that contain an O—O single bond? Explain.

(a) Construct a Lewis structure for hydrogen peroxide, H₂O₂, in which each atom achieves an octet of electrons.

(c) Do you expect the O—O bond in H₂O₂ to be longer or shorter than the O—O bond in O₂? Explain.

Which of the following statements about electronegativity is false? (a) Electronegativity is the ability of an atom in a molecule to attract electron density toward itself. (b) Electronegativity is the same thing as electron affinity. (c) The numerical values for electronegativity have no units. (d) Fluorine is the most electronegative element. (e) Cesium is the least electronegative element.

Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Se, Te, Br, I; (b) Be, Mg, C, Si (c) Al, Si, P, S (d) Zn, Ge, Ga, As.

By referring only to the periodic table, select (a) the most electronegative element in group 13; (b) the least electronegative element in the group As, Se and Br;

By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.

Which of the following bonds are polar? (a) C—O, (b) Sl—F, (c) N—Cl, (d) C—Cl. Which is the more electronegative atom in each polar bond?

Arrange the bonds in each of the following sets in order of increasing polarity: (a) C—F, O—F, Be—F (b) O—Cl,S—Br, C—P

Arrange the bonds in each of the following sets in order of increasing polarity: (c) C—S, B— F, N — O.

(a) From the data in Table 8.2, calculate the effective charges on the H atom of the HBr molecule in units of the electronic charge, e.

(b) If you were to put HBr under very high pressure, so its bond length decreased significantly, would its dipole moment increase, decrease, or stay the same, if you assume that the effective charges on the atoms do not change?

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 for the following: (a) CH₂Cl₂ (b) ClCN (c) SF₂

Draw Lewis structures for the following: (d) H₂SO₄ (H is bonded to O) (e) OF₂

Draw Lewis structures for the following: (f) NH₂OH

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 molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the atoms: (a) SO₂ Write a single Lewis structure that obeys the octet rule for SO₂ and assign the formal charges on all the atoms. (b) SO₃ Write a single Lewis structure that obeys the octet rule for SO₃ and assign the formal charges on all the atoms. (c) SO₃^2- Write a single Lewis structure that obeys the octet rule for SO₃^2- and assign the formal charges on all the atoms.

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

(c) What would you predict for the lengths of the bonds in NO₂^- relative to N¬O single bonds and double bonds?

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?

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. (c) Would you predict that the C—O bond lengths in the formate ion would be longer or shorter relative to those in CO₂?

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