1.17: Additional Exercises

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Bond Formation: The Octet Rule

1-1 Identify the number of valence electrons for each of the following elements. Then, identify the maximum number of covalent bonds it can form with other atoms while keeping a neutral net charge.

a) Oxygen

b) Carbon

c) Chlorine

d) Sulfur

e) Hydrogen

f) Boron

1-2 Which of the following atoms can bond with Br - to satisfy the octet rule?

a) Mg⁺²

b) O^-2

c) Cl^-

d) K⁺

1-3 Draw the Lewis dot structure of the correct answer from the previous problem 1-2 (a) - (d).

1-4 Identify which of the following compounds could not form due to an unfilled octet.

a) NCl₃

b) NaOH

c) PCl

d) CF₄

Lewis Structures

1-5 Draw the Lewis structures for the following compounds.

a) H₂O

b) O₃

c) BH₃

d) SOCl₂

1-6 Name the element that corresponds to each electronic configuration and identify how many valence electrons it has.

a) 1s²2s²2p⁶

b) 1s²2s²2p⁶3s²

c) 1s²2s²2p⁴

d) 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p5

1-7 Draw the Lewis structures for PF₃ and PF₅.

1-8 Draw the Lewis structure for furan.

1-9 Identify the correct Lewis structure for hydroperoxyl, HO₂.

Electronegativity and Bond Polarity

1-10 For the indicated bond in each of the following compounds, identify which atom is more electronegative, if applicable.

1-11 For each of the compounds in the previous problem, add a dipole moment arrow.

Formal Charges

1-12 For the following compounds, draw the structural formula. Then calculate the formal charge on each atom other than hydrogen.

a) N(CH₃)₄⁺

b) HSO₄^-

c) CH₃CC^-

1-13 Identify the formal charge for the following compounds.

1-14 Identify the formal charges for the central carbon in each of the following compounds.

Ionic Structures

1-15 Identify the substituent ions that make up the following salts.

a) NaCl

b) MgBr₂

c) KNO₃

d) NaH₂PO₄

1-16 Identify the products of the following reactions.

1-17 Give the correct nomenclature or write the correct chemical formula for the following ionic compounds.

a) NaCN

b) calcium oxalate

c) Al(OH)₃

d) tin (II) phosphate

e) potassium hypochlorite

Resonance

1-18 For the following structure, draw its resonance structure(s).

1-19 Which resonance form from the previous problem has the most stable carbocation? Explain your answer.

1-20 Draw the important resonance forms to show the delocalization of charges in the following compounds.

1-21 Explain how resonance contributes to the lower pKa of acetic acid CH₃CO₂H (pKa= 4.75) compared to the pKa of ethanol CH₃CH₂OH (pKa=15.9).

1-22 Draw the resonance structure(s) for fulminic acid (HCNO).

Structural, Molecular and Empirical Formulas

1-23 Identify the molecular and empirical formula for the following structures.

1-24 Draw all possible structural formulas for the following compounds.

a) C₄H₁₀

b) CHN

c) C₄H₉Cl

1-25 True or False: You can always calculate the exact molecular weight of a molecule from its empirical formula.

1-26 For the following molecular formulas, provide the empirical formula.

a) C₄H₄O₂

b) C₈H₆N₂

c) C₉H₂₁N₃O₃

Acids and Bases - Arrhenius, Bronsted-Lowry, and Lewis

1-27 Briefly explain the three different definitions of acids and bases.

1-28 Calculate the Ka of nitric acid (HNO₃). pKa of nitric acid is -1.4.

1-29 Rank the following in order of decreasing acidity: NH₄⁺ HF H₃O⁺ H₂O

1-30 Rank the following in order of decreasing basicity: HSO₄^- H₂O CH₃COO^- NH₂^-

1-31 Identify which compound is the stronger base. Identify which compound is the stronger acid.

1.32 Identify which group is more likely to grab a H⁺.

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