Chemistry
Chemistry
9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Book Icon
Chapter 8, Problem 54E

For each of the following groups, place the atoms and/or ions in order of decreasing size.

a. V, V2+, V3+, V5+

b. Na+, K+, Rb+, Cs+

c. Te2−, I, Cs+, Ba2+

d. P, P, P2−, P3−.

e. O2−, S2−, Se2−, Te2−

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The given ions are to be placed in decreasing order of size.

Concept introduction: The ionic size depends on the number of electrons transferred. The atomic size of cations is smaller than anions. Also the size of ions increases by gaining electrons whereas size decreases by accepting electrons.

To determine: The decreasing order of size of ions V,V2+,V3+,V5+.

Answer to Problem 54E

The size of ions V,V2+,V3+,V5+ decreases in the order V>V2+>V3+>V5+.

Explanation of Solution

In a periodic table the size of ions depends on the nuclear attraction on the valence electrons. Positive ions are formed by removing electrons from outer shell. Hence, formation of positive ions or cation not only vacant the orbitals but also decrease the electron-electron repulsion. As a result size of cations is smaller than neutral atom.

The ions V2+,V3+andV5+ are positive ions where V5+ is smallest because it contains large positive charge and have high nuclear attraction.

Hence, the decreasing order is V>V2+>V3+>V5+.

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The given ions are to be placed in decreasing order of size.

Concept introduction: The ionic size depends on the number of electrons transferred. The atomic size of cations is smaller than anions. Also the size of ions increases by gaining electrons whereas size decreases by accepting electrons.

To determine: The decreasing order of size of ions Na+,K+,Rb+andCs+.

Answer to Problem 54E

The size of ions Na+,K+,Rb+andCs+ decreases in the order Cs+>Rb+>K+>Na+.

Explanation of Solution

In a periodic table, the size of elements increases down the group. The elements Na,K,RbandCs lie in 1st group. Hence, the decreasing order is Cs>Rb>K>Na.

The size of ions also depends on the nuclear attraction on the valence electrons. Positive ions are formed by removing electrons from outer shell. Hence, formation of positive ions or cation not only vacant the orbitals but also decrease the electron-electron repulsion. As a result size of cations is smaller than neutral atom.

Hence, the decreasing order of ions is Cs+>Rb+>K+>Na+.

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The given ions are to be placed in decreasing order of size.

Concept introduction: The ionic size depends on the number of electrons transferred. The atomic size of cations is smaller than anions. Also the size of ions increases by gaining electrons whereas size decreases by accepting electrons.

To determine: The decreasing order of size of ions Te2,I,Cs+,Ba2+.

Answer to Problem 54E

The size of ions Te2,I,Cs+,Ba2+ decreases in the order Te2>I>Cs+>Ba2+.

Explanation of Solution

In a periodic table, the size of elements decreases from left to right along the period. Also if the periodic number increases then atomic size also increases. The elements CsandBa lie in 6th period and elements TeandI lie in 5th period. Hence, the decreasing order of atomic size is Cs>Ba>Te>I.

The electronic configuration of ions Te2,I,Cs+,Ba2+ is,

Te2:1s22s22p63s23p63d104s24p64d105s25p6

I:1s22s22p63s23p63d104s24p64d105s25p6

Cs+:1s22s22p63s23p63d104s24p64d105s25p6

Ba2+:1s22s22p63s23p63d104s24p64d105s25p6

The number of electrons present in Te2,I,Cs+,Ba2+ ions is 54. Hence these ions are isoelectronic. Since the atomic size is increased with increase of anion charge and decrease with increase of cation charge for isoelectronic configuration, the order of decreasing size of ions is Te2>I>Cs+>Ba2+,

Conclusion

For isoelectronic ions, the size of atom decreases with increase in cation charge and increase with anion charge. Hence, the decreasing size of ions is Te2>I>Cs+>Ba2+.

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The given ions are to be placed in decreasing order of size.

Concept introduction: The ionic size depends on the number of electrons transferred. The atomic size of cations is smaller than anions. Also the size of ions increases by gaining electrons whereas size decreases by accepting electrons.

To determine: The decreasing order of size of ions P,P,P2,P3.

Answer to Problem 54E

The size of ions P,P,P2,P3 decreases in the order P3>P2>P>P.

Explanation of Solution

Addition of electrons leads to increase in electron-electron repulsion which causes the electrons to spread out more in space. As a result, size of anion is larger than neutral atom.

Hence, the decreasing order of ions is P3>P2>P>P.

Conclusion

The size of ions depends on the gaining or losing of electrons. The size of ions increases by gaining electrons whereas size decreases by losing electrons. The decreasing order of ions is P3>P2>P>P

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The given ions are to be placed in decreasing order of size.

Concept introduction: The ionic size depends on the number of electrons transferred. The atomic size of cations is smaller than anions. Also the size of ions increases by gaining electrons whereas size decreases by accepting electrons.

To determine: The decreasing order of size of ions O2,S,Se2,Te2.

Answer to Problem 54E

The size of ions O2,S,Se2,Te2 decreases in the order Te2>Se2>S>O2.

Explanation of Solution

In a periodic table, the size of elements increases down the group. The elements O,S,Se,Te lie in 16th group. Hence, the decreasing order is Te>Se>S>O.

Addition of electrons leads to increase in electron-electron repulsion which causes the electrons to spread out more in space. As a result, size of anion is larger than neutral atom.

Hence, the decreasing order of ions is Te2>Se2>S>O2.

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
Y For parts a to f, consider the loss of electrons by atoms of the element X, and a gain of electrons by atoms of the element Y, if X is in Group 2A (2), Period 3, and Y is in Group 7A (17), Period 3. a. Which reactant has higher electronegativity? b. What are the ionic charges of X and Y? c. Write the electron arrangements for the atoms of X and Y. d. Write the electron arrangements for the ions of X and Y. e. Give the names for the noble gases with the same electron arrangements as the X and Y ions. f. Write the formula and name for the ionic compound formed from X and Y. e. a) Y has the higher electronegativity b)
1. Read the section above about balancing charges and give formulas that represent overall neutral compounds between the following pairs of ions. + a. Cs and Cl- + b. Cs and Se²- c. Fe2+ and Br d. Fe3+ and Br e. Fe2+ and CO3²- 2-
Write the formula for the ionic compound that is formed from each of the following pairs of ions. f. Al3+ and HPO42- g. Mg2+ and CO32- h.Pb2+and I- i. Cu2+ and N3- j.Fe3+ and SO32-

Chapter 8 Solutions

Chemistry

Ch. 8 - The ionic compound AB is formed. The charges on...Ch. 8 - Prob. 3ALQCh. 8 - The bond energy for a CH bond is about 413 kJ/mol...Ch. 8 - Prob. 5ALQCh. 8 - Which has the greater bond lengths: NO2 or NO3?...Ch. 8 - The following ions are best described with...Ch. 8 - The second electron affinity values for both...Ch. 8 - What is meant by a chemical bond? Why do atoms...Ch. 8 - Why are some bonds ionic and some covalent?Ch. 8 - How does a bond between Na and Cl differ from a...Ch. 8 - Arrange the following molecules from most to least...Ch. 8 - Does a Lewis structure tell which electron come...Ch. 8 - Describe the type of bonding that exists in die...Ch. 8 - Some plant fertilizer compounds are (NH4)2SO4,...Ch. 8 - Some of the important properties of ionic...Ch. 8 - What is the electronegativity trend? Where does...Ch. 8 - Give one example of a compound having a linear...Ch. 8 - When comparing the size of different ions, the...Ch. 8 - In general the higher the charge on the ions in an...Ch. 8 - Combustion reactions of fossil fuels provide most...Ch. 8 - Which of the following statements is/are true?...Ch. 8 - Three resonance structures can be drawn for CO2....Ch. 8 - Which of the following statements is(are) true?...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict the order of...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Without using Fig. 3-4, predict which bond in each...Ch. 8 - Prob. 31ECh. 8 - Prob. 32ECh. 8 - Which of the following incorrectly shows the bond...Ch. 8 - Indicate the bond polarity (show the partial...Ch. 8 - Predict the type of bond (ionic, covalent, or...Ch. 8 - List all the possible bonds that can occur between...Ch. 8 - Hydrogen has an electronegativity value between...Ch. 8 - Rank the following bonds in order of increasing...Ch. 8 - State whether or not each of the following has a...Ch. 8 - The following electrostatic potential diagrams...Ch. 8 - Prob. 41ECh. 8 - Prob. 42ECh. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Predict the empirical formulas of the ionic...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Write electron configurations for a. the cations...Ch. 8 - Which of the following ions have noble gas...Ch. 8 - What noble gas has the same electron configuration...Ch. 8 - Give the formula of a negative ion that would have...Ch. 8 - Prob. 50ECh. 8 - Give three ions that are isoelectronic with neon....Ch. 8 - Consider the ions Sc3+, Cl, K+, Ca2+, and S2....Ch. 8 - Prob. 53ECh. 8 - For each of the following groups, place the atoms...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Which compound in each of the following pairs of...Ch. 8 - Use the following data for potassium chloride to...Ch. 8 - Use the following data for magnesium fluoride to...Ch. 8 - Consider the following energy changes: E(kJ/mol)...Ch. 8 - Compare the electron affinity of fluorine to the...Ch. 8 - Prob. 61ECh. 8 - Use the following data (in kJ/mol) to estimate E...Ch. 8 - Rationalize the following lattice energy values:...Ch. 8 - The lattice energies of FeCl3, FeCl2, and Fe2O3...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Use bond energy values (Table 3-3) to estimate E...Ch. 8 - Prob. 67ECh. 8 - Acetic acid is responsible for the sour taste of...Ch. 8 - Use bond energies to predict E for the following...Ch. 8 - The major industrial source of hydrogen gas is by...Ch. 8 - Use bond energies to estimate E for the combustion...Ch. 8 - Prob. 72ECh. 8 - Prob. 73ECh. 8 - Consider the following reaction: A2+B22AB E =...Ch. 8 - Compare your answers from parts a and b of...Ch. 8 - Compare your answers from Exercise 72 to the H...Ch. 8 - The standard enthalpies of formation for S(g),...Ch. 8 - Use the following standard enthalpies of formation...Ch. 8 - The standard enthalpy of formation for N2H2(g) is...Ch. 8 - The standard enthalpy of formation for NO(g) is...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - One type of exception to the octet rule are...Ch. 8 - Lewis structures can be used to understand why...Ch. 8 - The most common exceptions to the octet rule are...Ch. 8 - Prob. 88ECh. 8 - Write Lewis structures for the following. Show all...Ch. 8 - Prob. 90ECh. 8 - Benzene (C6H6) consists of a six-membered ring of...Ch. 8 - Borazine (B3N3H6) has often been called inorganic...Ch. 8 - An important observation supporting the concept of...Ch. 8 - Consider the following bond lengths: CO143pmC9O123...Ch. 8 - A toxic cloud covered Bhopal, India, in December...Ch. 8 - Peroxyacetyl nitrate, or PAN, is present in...Ch. 8 - Prob. 99ECh. 8 - Use formal charge arguments to explain why CO has...Ch. 8 - Write Lewis structures that obey the octet rule...Ch. 8 - Write Lewis structures for the species in Exercise...Ch. 8 - Oxidation of the cyanide ion produces the stable...Ch. 8 - When molten sulfur reacts with chlorine gas, a...Ch. 8 - Prob. 106ECh. 8 - Prob. 108ECh. 8 - Predict the molecular structure and bond angles...Ch. 8 - Predict die molecular structure and bond angles...Ch. 8 - There are several molecular structures based on...Ch. 8 - Two variations of the octahedral geometry (see...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Predict the molecular structure (including bond...Ch. 8 - Prob. 117ECh. 8 - Which of the molecules in Exercise 120 have net...Ch. 8 - Which of the molecules in Exercise 121 have net...Ch. 8 - Which of the molecules in Exercise 122 have net...Ch. 8 - Write Lewis structures and predict the molecular...Ch. 8 - Write Lewis structures and predict whether each of...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Consider the following Lewis structure where E is...Ch. 8 - Prob. 125ECh. 8 - Two different compounds have the formula XeF2Cl2....Ch. 8 - Arrange the following in order of increasing...Ch. 8 - For each of the following, write an equation that...Ch. 8 - Use bond energies (table 3-3), values of electron...Ch. 8 - Write Lewis structures for CO32, HCO3, and H2CO3....Ch. 8 - Which member of the following pairs would you...Ch. 8 - What do each of the following sets of...Ch. 8 - Prob. 133AECh. 8 - Although both Br3 and I3 ions are known, the F3...Ch. 8 - Which of the following molecules have not dipole...Ch. 8 - Prob. 137AECh. 8 - Look up the energies for the bonds in CO and N2....Ch. 8 - Classify the bonding in each of the following...Ch. 8 - List the bonds PCl, PF, OF, and SiF from least...Ch. 8 - Arrange the atoms and/or ions in the following...Ch. 8 - Use the following data to estimate E for the...Ch. 8 - Use bond energy values to estimate E for the...Ch. 8 - Which of the following compounds or ions exhibit...Ch. 8 - The formulas of several chemical substances are...Ch. 8 - Predict the molecular structure, bond angles, and...Ch. 8 - Use Coulombs Jaw, V=Q1Q240r=2.311019Jnm(Q1Q2r) to...Ch. 8 - Prob. 148CPCh. 8 - Calculate the standard heat of formation of the...Ch. 8 - Given the following information: Energy of...Ch. 8 - Prob. 151CPCh. 8 - Think of forming an ionic compound as three steps...Ch. 8 - The compound NF3 is quite stable, but NCl3, is...Ch. 8 - Three processes that have been used for the...Ch. 8 - The compound hexaazaisowurtzitane is one of the...Ch. 8 - Many times extra stability is characteristic of a...Ch. 8 - The study of carbon-containing compounds and their...Ch. 8 - Draw a Lewis structure for the N,...Ch. 8 - Prob. 159CPCh. 8 - Consider the following computer-generated model of...Ch. 8 - A compound, XF5, is 42.81% fluorine by mass....Ch. 8 - Identify the following elements based on their...
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.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
Text book image
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Text book image
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
Text book image
General, Organic, and Biological Chemistry
Chemistry
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:Cengage Learning
Text book image
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY
Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
General Chemistry 1A. Lecture 12. Two Theories of Bonding.; Author: UCI Open;https://www.youtube.com/watch?v=dLTlL9Z1bh0;License: CC-BY