7.4 Formal charges and resonance  (Page 4/9)

Write resonance forms that describe the distribution of electrons in each of these molecules or ions.

(a) selenium dioxide, OSeO

(b) nitrate ion, ${\text{NO}}_3{}^{\text{−}}$

(c) nitric acid, HNO ₃ (N is bonded to an OH group and two O atoms)

(d) benzene, C ₆ H ₆ :

(e) the formate ion:

Write resonance forms that describe the distribution of electrons in each of these molecules or ions.

(a) sulfur dioxide, SO ₂

(b) carbonate ion, ${\text{CO}}_3{}^{\text{2−}}$

(c) hydrogen carbonate ion, ${\text{HCO}}_3{}^{\text{−}}$ (C is bonded to an OH group and two O atoms)

(d) pyridine:

(e) the allyl ion:

Write the resonance forms of ozone, O ₃ , the component of the upper atmosphere that protects the Earth from ultraviolet radiation.

Sodium nitrite, which has been used to preserve bacon and other meats, is an ionic compound. Write the resonance forms of the nitrite ion, ${\text{NO}}_{\text{2}}{}^{\text{–}}\text{.}$

In terms of the bonds present, explain why acetic acid, CH ₃ CO ₂ H, contains two distinct types of carbon-oxygen bonds, whereas the acetate ion, formed by loss of a hydrogen ion from acetic acid, only contains one type of carbon-oxygen bond. The skeleton structures of these species are shown:

Write the Lewis structures for the following, and include resonance structures where appropriate. Indicate which has the strongest carbon-oxygen bond.

(a) CO ₂

(b) CO

Toothpastes containing sodium hydrogen carbonate (sodium bicarbonate) and hydrogen peroxide are widely used. Write Lewis structures for the hydrogen carbonate ion and hydrogen peroxide molecule, with resonance forms where appropriate.

Determine the formal charge of each element in the following:

(a) HCl

(b) CF ₄

(c) PCl ₃

(d) PF ₅

Determine the formal charge of each element in the following:

(a) H ₃ O ⁺

(b) ${\text{SO}}_4{}^{\text{2−}}$

(c) NH ₃

(d) ${\text{O}}_2{}^{\text{2−}}$

(e) H ₂ O ₂

Calculate the formal charge of chlorine in the molecules Cl ₂ , BeCl ₂ , and ClF ₅ .

Calculate the formal charge of each element in the following compounds and ions:

(a) F ₂ CO

(b) NO ^–

(c) ${\text{BF}}_4{}^{\text{−}}$

(d) ${\text{SnCl}}_3{}^{\text{−}}$

(e) H ₂ CCH ₂

(f) ClF ₃

(g) SeF ₆

(h) ${\text{PO}}_4{}^{\text{3−}}$

Draw all possible resonance structures for each of these compounds. Determine the formal charge on each atom in each of the resonance structures:

(a) O ₃

(b) SO ₂

(c) ${\text{NO}}_2{}^{\text{−}}$

(d) ${\text{NO}}_3{}^{\text{−}}$

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in nitrosyl chloride: ClNO or ClON?

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in hypochlorous acid: HOCl or OClH?

Based on formal charge considerations, which of the following would likely be the correct arrangement of atoms in sulfur dioxide: OSO or SOO?

Draw the structure of hydroxylamine, H ₃ NO, and assign formal charges; look up the structure. Is the actual structure consistent with the formal charges?

Iodine forms a series of fluorides (listed here). Write Lewis structures for each of the four compounds and determine the formal charge of the iodine atom in each molecule:

(a) IF

(b) IF ₃

(c) IF ₅

(d) IF ₇

Write the Lewis structure and chemical formula of the compound with a molar mass of about 70 g/mol that contains 19.7% nitrogen and 80.3% fluorine by mass, and determine the formal charge of the atoms in this compound.

Which of the following structures would we expect for nitrous acid? Determine the formal charges:

Sulfuric acid is the industrial chemical produced in greatest quantity worldwide. About 90 billion pounds are produced each year in the United States alone. Write the Lewis structure for sulfuric acid, H ₂ SO ₄ , which has two oxygen atoms and two OH groups bonded to the sulfur.