Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
bartleby

Videos

Textbook Question
Book Icon
Chapter 3, Problem 3.24P

3-24 Predict which ions are stable:

(a) Br2-

(b) C4-

(c) Ca+

(d) Ar+

(e) Na+

(f) Cs+

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether Br2 ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

Br2 ion is not stable.

Explanation of Solution

The atomic number or number of electrons of Br is 35, the electronic configuration of Br is as follows:

Br35:1s2 2s22p6  3s23p63d10   4s24p5

When Br will gain 2 electrons; the electronic configuration of its ion will not become as the nearest noble element.

Br233:1s2 2s22p6  3s23p63d10   4s24p3

Hence, the ion Br2 is not stable.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether C4 ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

C4 ion is stable.

Explanation of Solution

The atomic number or number of electrons of C is 6, the electronic configuration of C is as follows:

C6:1s2 2s22p4 

When C will gain 4 electrons; the electronic configuration of its ion will become as the nearest noble element.

C410:1s2 2s22p6  [Ne]

Hence, the ion C4 is stable.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether Ca+ ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

Ca+ ion is not stable.

Explanation of Solution

The atomic number or number of electrons of Ca is 20, the electronic configuration of Ca is as follows:

Ca20:1s2 2s22p6  3s23p6   4s2

When Ca will lose 1 electron; the electronic configuration of its ion will not become as the nearest noble element.

Ca+19:1s2 2s22p6  3s13p6   4s1

Hence, the ion Ca+ is not stable.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether ar+ ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

ar+ ion is not stable.

Explanation of Solution

The atomic number or number of electrons of ar is 18, the electronic configuration of ar is as follows:

ar18:1s2 2s22p6  3s23p6

When ar will gain 1 electron; the electronic configuration of its ion will not become as the nearest noble element.

ar+19:1s2 2s22p6  3s13p63d10   4s1

Hence, the ion ar+ is not stable.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether Na+ ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

Na+ ion is stable.

Explanation of Solution

The atomic number or number of electrons of Na is 11, the electronic configuration of Na is as follows:

Na11:1s2 2s22p6  3s1

When Na will gain 1 electron; the electronic configuration of its ion will become as the nearest noble element.

Na+10:1s2 2s22p6  

Hence, the ion Na+ is not stable.

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

Whether Cs+ ion is stable or not should be determined.

Concept Introduction:

Octet rule: generally all atoms will lose, gain or share electrons to attain 8 valence electrons; the electronic configuration of the nearest noble element.

Duet rule: generally some atoms like hydrogen, lithium, beryllium will lose, gain or share electrons to attain 2 valence electrons; the electronic configuration of the nearest noble element like helium.

Answer to Problem 3.24P

Cs+ ion is stable.

Explanation of Solution

The atomic number or number of electrons of Cs is 55, the electronic configuration of Cs is as follows:

Cs55:1s2 2s22p6  3s23p63d10   4s24p64d10 5s22p6  6s1

When Cs will lose 1 electron; the electronic configuration of its ion become as the nearest noble element Xeon as follows:

Cs+54:1s2 2s22p6  3s23p63d10   4s24p64d10 5s22p5[Xe] 

Hence the ion Cs+ is not stable.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Students have asked these similar questions
(f) SO: Best Lewis Structure 3 e group geometry:_ shape/molecular geometry:, (g) CF2CF2 Best Lewis Structure polarity: e group arrangement:_ shape/molecular geometry: (h) (NH4)2SO4 Best Lewis Structure polarity: e group arrangement: shape/molecular geometry: polarity: Sketch (with angles): Sketch (with angles): Sketch (with angles):
1. Problem Set 3b Chem 141 For each of the following compounds draw the BEST Lewis Structure then sketch the molecule (showing bond angles). Identify (i) electron group geometry (ii) shape around EACH central atom (iii) whether the molecule is polar or non-polar (iv) (a) SeF4 Best Lewis Structure e group arrangement:_ shape/molecular geometry: polarity: (b) AsOBr3 Best Lewis Structure e group arrangement:_ shape/molecular geometry: polarity: Sketch (with angles): Sketch (with angles):
(c) SOCI Best Lewis Structure 2 e group arrangement: shape/molecular geometry:_ (d) PCls Best Lewis Structure polarity: e group geometry:_ shape/molecular geometry:_ (e) Ba(BrO2): Best Lewis Structure polarity: e group arrangement: shape/molecular geometry: polarity: Sketch (with angles): Sketch (with angles): Sketch (with angles):

Chapter 3 Solutions

Introduction to General, Organic and Biochemistry

Ch. 3.7 - Prob. 3.11PCh. 3.8 - Prob. 3.12PCh. 3.9 - Prob. 3.13PCh. 3.9 - Prob. 3.14PCh. 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 - Prob. 3.30PCh. 3 - 3-31 Why does electronegativity generally increase...Ch. 3 - 3-32 Judging from their relative positions in the...Ch. 3 - Prob. 3.33PCh. 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 - Prob. 3.40PCh. 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 - Prob. 3.49PCh. 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 - Prob. 3.52PCh. 3 - 3-53 Write formulas for the following ionic...Ch. 3 - 3-54 Write formulas for the following ionic...Ch. 3 - Prob. 3.55PCh. 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 - Prob. 3.59PCh. 3 - Prob. 3.60PCh. 3 - Prob. 3.61PCh. 3 - Prob. 3.62PCh. 3 - 3-63 What is the difference between (a) a bromine...Ch. 3 - 3-64 Acetylene (C2H2), hydrogen cyanide (HCN), and...Ch. 3 - Prob. 3.65PCh. 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 - Prob. 3.69PCh. 3 - 3-70 Draw a Lewis structure of a covalent compound...Ch. 3 - Prob. 3.71PCh. 3 - Prob. 3.72PCh. 3 - Prob. 3.73PCh. 3 - 3-74 Answer true or false. (a) A binary covalent...Ch. 3 - Prob. 3.75PCh. 3 - Prob. 3.76PCh. 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 - Prob. 3.80PCh. 3 - Prob. 3.81PCh. 3 - 3-82 Hydrogen and nitrogen combine in different...Ch. 3 - Prob. 3.83PCh. 3 - Prob. 3.84PCh. 3 - Prob. 3.85PCh. 3 - Prob. 3.86PCh. 3 - 3-87 Consider the molecule boron trffluoride, BF3....Ch. 3 - Prob. 3.88PCh. 3 - 3-89 Is it possible for a molecule to have no...Ch. 3 - Prob. 3.90PCh. 3 - Prob. 3.91PCh. 3 - Prob. 3.92PCh. 3 - Prob. 3.93PCh. 3 - Prob. 3.94PCh. 3 - Prob. 3.95PCh. 3 - Prob. 3.96PCh. 3 - Prob. 3.97PCh. 3 - Prob. 3.98PCh. 3 - 3-99 Knowing what you do about covalent bonding in...Ch. 3 - Prob. 3.100PCh. 3 - Prob. 3.101PCh. 3 - Prob. 3.102PCh. 3 - Prob. 3.103PCh. 3 - Prob. 3.104PCh. 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 - Prob. 3.108PCh. 3 - 3-109 Until several years ago, the two...Ch. 3 - 3-110 Name and write the formula for the fluorine...Ch. 3 - Prob. 3.111PCh. 3 - Prob. 3.112PCh. 3 - Prob. 3.113PCh. 3 - Prob. 3.114PCh. 3 - Prob. 3.115PCh. 3 - Prob. 3.116PCh. 3 - Prob. 3.117PCh. 3 - Prob. 3.118PCh. 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 - Prob. 3.124PCh. 3 - Prob. 3.125PCh. 3 - Prob. 3.126PCh. 3 - 3-127 Amoxicillin is an antibiotic used to treat...Ch. 3 - Prob. 3.128P
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Recommended textbooks for you
Text book image
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning
Periodic Properties of Elements | Chemistry | IIT-JEE | NEET | CBSE | Misostudy; Author: Misostudy;https://www.youtube.com/watch?v=L26rRWz4_AI;License: Standard YouTube License, CC-BY
Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE; Author: Melissa Maribel;https://www.youtube.com/watch?v=0h8q1GIQ-H4;License: Standard YouTube License, CC-BY