3-100 Use the valence-shell electron-pair repulsion model to predict the shape of a molecule in which a central atom is surrounded by five regions of electron density−as, for example, in phosphorus pentafluoride, PF5. (Hint: Use molecular models or if you do not have a set handy, use marshmallows or gum drops and toothpicks.)

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Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759
BuyFind

Introduction to General, Organic a...

11th Edition
Frederick A. Bettelheim + 4 others
Publisher: Cengage Learning
ISBN: 9781285869759

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Chapter 3, Problem 3.100P
Textbook Problem

3-100 Use the valence-shell electron-pair repulsion model to predict the shape of a molecule in which a central atom is surrounded by five regions of electron density−as, for example, in phosphorus pentafluoride, PF5. (Hint: Use molecular models or if you do not have a set handy, use marshmallows or gum drops and toothpicks.)

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Chapter 3 Solutions

Introduction to General, Organic and Biochemistry
Ch. 3.7 - Problem 3-11 Draw a Lewis structure of a covalent...Ch. 3.8 - Problem 3-12 Name these binary covalent compounds:...Ch. 3.9 - Problem 3-13 Draw the contributing structure...Ch. 3.9 - Problem 3-14 Which sets are valid pairs of...Ch. 3.10 - Problem 3-15 Predict all bond angles for these...Ch. 3.11 - Problem 3-16 Which of these molecules are polar?...Ch. 3 - 3-17 Answer true or false. (a) The octet rule...Ch. 3 - 3-18 How many electrons must each atom gain or...Ch. 3 - 3-19 Show how each chemical change obeys the octet...Ch. 3 - 3-20 Show how each chemical change obeys the octet...Ch. 3 - 3-21 Write the formula for the most stable ion...Ch. 3 - 3-22 Why is Li- not a stable ion?Ch. 3 - 3-23 Predict which ions are stable: (a) (b) (c)...Ch. 3 - 3-24 Predict which ions are stable: (a) Br2- (b)...Ch. 3 - 3-25 Why are carbon and silicon reluctant to form...Ch. 3 - 3-26 Table 3-2 shows the following ions of copper:...Ch. 3 - 3-27 Answer true or false. (a) For Group lA and...Ch. 3 - 3-28 Name each polyatomic ion. (a) HCO3- (b) NO2-...Ch. 3 - 3-29 Answer true or false. (a) According to the...Ch. 3 - 3-30 Why does electronegativity generally increase...Ch. 3 - 3-31 Why does electronegativity generally increase...Ch. 3 - 3-32 Judging from their relative positions in the...Ch. 3 - 3-33 Toward which atom are the bonding electrons...Ch. 3 - 3-34 Which of these bonds is the most polar? The...Ch. 3 - 3-35 Classify each bond as nonpolar covalent,...Ch. 3 - 3-36 Classify each bond as nonpolar covalent,...Ch. 3 - 3-37 Answer true or false. (a) An ionic bond is...Ch. 3 - 3-38 Complete the chart by writing formulas for...Ch. 3 - 3-39 Write a formula for the ionic compound formed...Ch. 3 - 3-40 Although not a transition metal, lead can...Ch. 3 - 3-41 Describe the structure of sodium chloride in...Ch. 3 - 3-42 What is the charge on each ion in these...Ch. 3 - 3-43 Write the formula for the compound formed...Ch. 3 - 3-44 Write the formula for the ionic compound...Ch. 3 - 3-45 Which formulas are not correct? For each that...Ch. 3 - 3-46 Which formulas are not correct? For each that...Ch. 3 - 3-47 Answer true or false. (a) The name of a...Ch. 3 - 3-48 Potassium chloride and potassium bicarbonate...Ch. 3 - 3-49 Potassium nitrite has been used as a...Ch. 3 - 3-50 Name the polyatomic ion(s) in each compound....Ch. 3 - 3-51 Write the formulas for the ions present in...Ch. 3 - 3-52 Name these ionic compounds: (a) NaF (b) MgS...Ch. 3 - 3-53 Write formulas for the following ionic...Ch. 3 - 3-54 Write formulas for the following ionic...Ch. 3 - 3-55 Answer true or false. (a) A covalent bond is...Ch. 3 - 3-56 How many covalent bonds are normally formed...Ch. 3 - 3-57 What is: (a) A single bond? (b) A double...Ch. 3 - 3-58 In Section 2-3B, we saw that there are seven...Ch. 3 - 3-59 Draw a Lewis structure for each covalent...Ch. 3 - 3-60 What is the difference between a molecular...Ch. 3 - 3-61 State the total number of valence electrons...Ch. 3 - 3-62 Draw a Lewis structure for each of the...Ch. 3 - 3-63 What is the difference between (a) a bromine...Ch. 3 - 3-64 Acetylene (C2H2), hydrogen cyanide (HCN), and...Ch. 3 - 3-65 Why can’t hydrogen have more than two...Ch. 3 - 3-66 Why can’t second-row elements have more than...Ch. 3 - 3-67 Why does nitrogen have three bonds and one...Ch. 3 - 3-68 Draw a Lewis structure of a covalent compound...Ch. 3 - 3-69 Why does oxygen have two bonds and two...Ch. 3 - 3-70 Draw a Lewis structure of a covalent compound...Ch. 3 - 3-71 The ion O6+ has a complete outer shell. Why...Ch. 3 - 3-72 Draw a Lewis structure for a molecule in...Ch. 3 - 3-73 Which of the following molecules have an atom...Ch. 3 - 3-74 Answer true or false. (a) A binary covalent...Ch. 3 - 3-75 Name these binary covalent compounds. (a) SO2...Ch. 3 - 3-76 Write two acceptable contributing structures...Ch. 3 - 3-77 Ozone, O3, is an unstable blue gas with a...Ch. 3 - 3-78 Nitrous oxide, N20, laughing gas, is a...Ch. 3 - 3-79 Answer true or false. (a) The letters VSEPR...Ch. 3 - 3-80 State the shape of a molecule whose central...Ch. 3 - 3-81 Hydrogen and oxygen combine in different...Ch. 3 - 3-82 Hydrogen and nitrogen combine in different...Ch. 3 - 3-83 Predict the shape of each molecule. (a) CH4...Ch. 3 - 3-84 Predict the shape of each ion. (a) (b (c)Ch. 3 - 3-85 Answer true or false. (a) To predict whether...Ch. 3 - 3-86 Both CO2 and SO2 have polar bonds. Account...Ch. 3 - 3-87 Consider the molecule boron trffluoride, BF3....Ch. 3 - 3-88 Is it possible for a molecule to have polar...Ch. 3 - 3-89 Is it possible for a molecule to have no...Ch. 3 - 3-90 In each case, tell whether the bond is ionic,...Ch. 3 - 3-91 Account for the fact that chioromethane,...Ch. 3 - 3-92 (Chemical Connections 3A) What are the three...Ch. 3 - 3-93 (Chemical Connections 3B) Why is sodium...Ch. 3 - 3-94 (Chemical Connections 3B) What is a medical...Ch. 3 - 3-95 (Chemical Connections 3B) What is a medical...Ch. 3 - 3-96 (Chemical Connections 3A) What is the most...Ch. 3 - 3-97 (Chemical Connections 3C) In what way does...Ch. 3 - 3-98 Explain why argon does not form either (a)...Ch. 3 - 3-99 Knowing what you do about covalent bonding in...Ch. 3 - 3-100 Use the valence-shell electron-pair...Ch. 3 - 3-101 Use the valence-shell electron-pair...Ch. 3 - 3-102 Chlorine dioxide, ClO2, is a yellow to...Ch. 3 - 3-103 Using the information in Figure 2-16,...Ch. 3 - 3-104 Arrange the single covalent bonds within...Ch. 3 - 3-105 Consider the structure of Vitamin E shown...Ch. 3 - 3-106 Consider the structure of Penicillin G shown...Ch. 3 - 3-107 Ephedrine, a molecule at one time found in...Ch. 3 - 3-108 Allene, C3H4, has the structural formula...Ch. 3 - 3-109 Until several years ago, the two...Ch. 3 - 3-110 Name and write the formula for the fluorine...Ch. 3 - 3-111 If you read the labels of sun-blocking...Ch. 3 - 3-112 On packaged table salt, it is common to see...Ch. 3 - 3-113 We are constantly warned about the dangers...Ch. 3 - 3-114 If you read the labels of several liquid and...Ch. 3 - 3-115 Iron forms Fe2+ and Fe3+ ions. Which ion is...Ch. 3 - 3-116 Read the labels of several...Ch. 3 - 3-117 Write formulas for these compounds. (a)...Ch. 3 - 3-118 Many paint pigments contain transition metal...Ch. 3 - 3-119 Perchloroethylene, which is a liquid at room...Ch. 3 - 3-120 Vinyl chloride is the starting material for...Ch. 3 - 3-121 Tetrafluoroethylene is the starting material...Ch. 3 - 3-122 Some of the following structural formulas...Ch. 3 - 3-123 Sodium borohydride, NaBH4, has found wide...Ch. 3 - 3-124 Given your answer to Problem 3-123 and...Ch. 3 - 3-125 In Chapter 27, you will learn that adenosine...Ch. 3 - 3-126 Androstenedione, a muscle-building dietary...Ch. 3 - 3-127 Amoxicillin is an antibiotic used to treat...Ch. 3 - 3-128 Cyclopropane, an anesthetic with extreme...

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