Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
15th Edition
ISBN: 9781269935678
Author: Nivaldo J. Tro
Publisher: Pearson Education
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 4, Problem 98E
Use electron configurations to explain why copper is paramagnetic while its 1+ ion is not.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 4 Solutions
Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
Ch. 4 - 1. According to Coulomb's law, if the separation...Ch. 4 - Prob. 2SAQCh. 4 - Choose the correct electron configuration for Se....Ch. 4 - Prob. 4SAQCh. 4 - Which set of four quantum numbers corresponds to...Ch. 4 - Prob. 6SAQCh. 4 - Which statement is true about electron shielding...Ch. 4 - Prob. 8SAQCh. 4 - What is the electron configuration for Fe2+?...Ch. 4 - Which species is diamagnetic? Zn Cr 2+ C Mn
Ch. 4 - Prob. 11SAQCh. 4 - Prob. 12SAQCh. 4 - Prob. 13SAQCh. 4 - Prob. 14SAQCh. 4 - Prob. 15SAQCh. 4 - Prob. 16SAQCh. 4 - What are periodic properties?Ch. 4 - Use aluminum as an example to explain how density...Ch. 4 - Explain the contributions of Dobereiner and...Ch. 4 - Who is credited with arranging the periodic table?...Ch. 4 - Prob. 5ECh. 4 - Prob. 6ECh. 4 - What is an electron configuration? Provide an...Ch. 4 - Prob. 8ECh. 4 - Prob. 9ECh. 4 - What is penetration? How does the penetration of...Ch. 4 - Why are the sublevels within a principal level...Ch. 4 - Prob. 12ECh. 4 - Prob. 13ECh. 4 - What are degenerate orbitals? According to Hund’s...Ch. 4 - List all orbitals from 1s through 5s according to...Ch. 4 - Prob. 16ECh. 4 - Copy this blank periodic table onto a sheet of...Ch. 4 - Explain why the s block in the periodic table has...Ch. 4 - Explain why the rows in the periodic table become...Ch. 4 - Explain the relationship between a main-group...Ch. 4 - Explain the relationship between an element's row...Ch. 4 - Which of the transition elements in the first...Ch. 4 - Explain how to write the electron configuration...Ch. 4 - Explain the relationship between the properties of...Ch. 4 - Prob. 25ECh. 4 - Prob. 26ECh. 4 - What is effective nuclear charge? What is...Ch. 4 - When an alkali metal forms an ion, what is the...Ch. 4 - When a halogen forms an ion, what is the charge of...Ch. 4 - Use the concepts of effective nuclear charge,...Ch. 4 - For transition elements, describe the trends in...Ch. 4 - Prob. 32ECh. 4 - Explain how to write an electron configuration for...Ch. 4 - Prob. 34ECh. 4 - Prob. 35ECh. 4 - Prob. 36ECh. 4 - What are the exceptions to the periodic trends in...Ch. 4 - Prob. 38ECh. 4 - Prob. 39ECh. 4 - What is metallic character? What are the observed...Ch. 4 - Prob. 41ECh. 4 - Prob. 42ECh. 4 - Determine whether each element is a main-group...Ch. 4 - Determine whether each element is a transition...Ch. 4 - Write the full electron configuration for each...Ch. 4 - Prob. 46ECh. 4 - Write the full orbital diagram for each element. N...Ch. 4 - Prob. 48ECh. 4 - Use the periodic table to write the electron...Ch. 4 - Use the periodic table to determine the element...Ch. 4 - Use the periodic table to determine each quantity....Ch. 4 - Use the periodic table to determine each quantity....Ch. 4 - Prob. 53ECh. 4 - Prob. 54ECh. 4 - Determine the number of valence electrons in each...Ch. 4 - Prob. 56ECh. 4 - Which outer electron configuration would you...Ch. 4 - Prob. 58ECh. 4 - Prob. 59ECh. 4 - List the number of valence electrons in each...Ch. 4 - Which pair of elements do you expect to be most...Ch. 4 - Prob. 62ECh. 4 - Predict the charge of the ion formed by each...Ch. 4 - Predict the charge of the ion formed by each...Ch. 4 - According to Coulomb’s law, which pair of charged...Ch. 4 - Prob. 66ECh. 4 - Prob. 67ECh. 4 - Arrange the atoms according to decreasing...Ch. 4 - If core electrons completely shielded valence...Ch. 4 - In Section 3.6/, we estimated the effective...Ch. 4 - Prob. 71ECh. 4 - Choose the larger atom in each pair. Sn or Si Br...Ch. 4 - Arrange these elements in order of increasing...Ch. 4 - Arrange these elements in order of decreasing...Ch. 4 - Write the electron configuration for each ion. O2...Ch. 4 - Write the electron configuration for each ion. Cl...Ch. 4 - Write orbital diagrams for each ion and determine...Ch. 4 - Write orbital diagrams for each ion and determine...Ch. 4 - Which is the larger species in each pair? LiorLi+...Ch. 4 - Which is the larger species in each pair? SrorSr2+...Ch. 4 - Arrange this isoelectronic series in order of...Ch. 4 - Arrange this isoelectronic series in order of...Ch. 4 - Choose the element with the higher first...Ch. 4 - Prob. 84ECh. 4 - Arrange these elements in order of increasing...Ch. 4 - Prob. 86ECh. 4 - For each element, predict where the “jump” occurs...Ch. 4 - Prob. 88ECh. 4 - Choose the element with the more negative (more...Ch. 4 - Prob. 90ECh. 4 - Choose the more metallic element in each pair....Ch. 4 - Prob. 92ECh. 4 - Prob. 93ECh. 4 - Prob. 94ECh. 4 - Prob. 95ECh. 4 - Prob. 96ECh. 4 - Both vanadium and its 3+ ion are paramagnetic. Use...Ch. 4 - Use electron configurations to explain why copper...Ch. 4 - Prob. 99ECh. 4 - Suppose you were trying to find a substitute for...Ch. 4 - Prob. 101ECh. 4 - Which pair of elements would you expect to have...Ch. 4 - Consider these elements: N, Mg, O, F, Al. Write...Ch. 4 - Consider these elements: P, Ca, Si, S, Ga. Write...Ch. 4 - Prob. 105ECh. 4 - Explain why vanadium (radius = 134 pm) and copper...Ch. 4 - The lightest noble gases, such as helium and neon,...Ch. 4 - The lightest halogen is also the most chemically...Ch. 4 - Prob. 109ECh. 4 - Prob. 110ECh. 4 - Prob. 111ECh. 4 - Write the electronic configurations of the six...Ch. 4 - You have cracked a secret code that uses elemental...Ch. 4 - The electron affinity of sodium is lower than that...Ch. 4 - Use Coulomb’s law to calculate the ionization...Ch. 4 - Prob. 116ECh. 4 - Consider the densities and atomic radii of the...Ch. 4 - Prob. 118ECh. 4 - Consider the metals in the first transition...Ch. 4 - Imagine a universe in which the value of ms can be...Ch. 4 - A carbon atom can absorb radiation of various...Ch. 4 - Only trace amounts of the synthetic element...Ch. 4 - What is the atomic number of the as yet...Ch. 4 - The trend in second ionization energy for the...Ch. 4 - Unlike the elements in groups 1A and 2A, those in...Ch. 4 - Using the data in Figures 3.19 and 3.20/,...Ch. 4 - Prob. 127ECh. 4 - Prob. 128ECh. 4 - The heaviest known alkaline earth metal is radium,...Ch. 4 - Predict the electronic configurations of the first...Ch. 4 - Prob. 131ECh. 4 - The outermost valence electron in atom A...Ch. 4 - Prob. 133ECh. 4 - Give a combination of four quantum numbers that...Ch. 4 - Prob. 135E
Knowledge Booster
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
- Fluoride ion, F, has no unpaired electrons. Vanadium forms four binary fluoridesVF2, VF3, VF4, and VF5. Assume that all four are ionic compounds. (a) Which fluoride is diamagnetic? (b) Which fluoride has the greatest attraction to a magnetic field? (c) Which fluoride has two unpaired electrons per vanadium?arrow_forwardUse the atomic radii of scandium, yttrium, lanthanum, and lutetium to answer the questions below. Explain why lutetium has a smaller atomic radius than lanthanum, even though it has a greater number of electrons. Do the atomic radii argue for the placement of La or Lu below Y in the periodic table? Explain.arrow_forwardWhich of these isoelectronic ions, Ba2+, Cs+, or La3+, is (a) the largest? (b) the smallest? Explain your reasoning.arrow_forward
- Does the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.arrow_forwardUse electron configurations to explain why (a) sulfur has a lower electron affinity than chlorine. (b) boron has a lower first ionization energy than beryllium. (c) chlorine has a lower first ionization energy than fluorine. (d) oxygen has a lower first ionization energy than nitrogen. (e) iodine has a lower electron affinity than bromine.arrow_forwardWhat is the electron configuration of the Ba3+ ion? Suggest a reason why this ion is not normally found in nature.arrow_forward
- Write the ground state electron configuration for (a) Mg, Mg2+(b) N, N3- (c) Ti, Ti4+ (d) Sn2+ Sn4+arrow_forwardWrite electron configurations for the following elements. a. The Group III A element in the same period as 4Be b. The Period 3 element in the same group as 5B c. The lowest-atomic-numbered metal in Group IIA d. The two Period 3 elements that have no unpaired electronsarrow_forwardIf potassium chlorate has the formula KClO3, what formula would you expect for lithium bromate?arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Introductory Chemistry: An Active Learning Approa...
Chemistry
ISBN:9781305079250
Author:Mark S. Cracolice, Ed Peters
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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