CHEMISTRY >CUSTOM<
14th Edition
ISBN: 9781259137815
Author: Julia Burdge
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 7, Problem 63QP
Interpretation Introduction
Interpretation:
The concept of ionic radius is to be defined and how the size of an atom is changed when it is converted into an anion and a cationis to be explained.
Concept introduction:
Ionic radius is defined as the distance between the center of the nucleus to its electron cloud.
When an atom loses an electron in order to become a cation, its radius decreasesdue to the decrease in electron–electron repulsion, which also results in decreased shielding effect for the valence shell electrons.
When an atom gains an electron, it becomes an anion. The radius of the anion increases because of the increased electron–electron repulsion.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
(b) A new element, "X", is discovered and found to have 2 electrons in its outer level.
Is X a metal or non-metal? Predict the formula its ion would have in any ionic
compounds it forms.
How many valence electrons does an element in each group contain: (a) 2A; (b) 4A; (c) 7A?
Hypothetical elements X and Y form a molecule XY2, in which both Y atoms are bonded to atom X (and not to one another). The X—X distance in the elemental form of X is 204 pm, and the Y—Y distance in elemental Y is 168 pm. What would you predict for the X—Y distance in the XY2 molecule? Explain your answer.
Chapter 7 Solutions
CHEMISTRY >CUSTOM<
Ch. 7.1 - Practice Problem ATTEMPT What element(s) would you...Ch. 7.1 - Practice Problem BUILD
Arrange the following...Ch. 7.1 - Practice ProblemCONCEPTUALIZE Three different...Ch. 7.1 - 7.1.1 Which of the following elements would you...Ch. 7.1 - Prob. 2CPCh. 7.1 - Prob. 3CPCh. 7.2 - Practice Problem ATTEMPT Without using a periodic...Ch. 7.2 - Practice ProblemBUILD Identify the elements...Ch. 7.2 - Prob. 1PPCCh. 7.2 - 7.2.1 Which electron configuration is correct for...
Ch. 7.2 - Which of the following equations correctly...Ch. 7.3 - Practice Problem ATTEMPT Referring only to a...Ch. 7.3 - Practice Problem BUILD
For which of the following...Ch. 7.3 - Practice Problem CONCEPTUALIZE
Based on size and...Ch. 7.4 - Practice Problem ATTEMPT Which element. Mg or Al,...Ch. 7.4 - Prob. 1PPBCh. 7.4 - Practice ProblemCONCEPTUALIZE Imagine an...Ch. 7.4 - 7.4.1 Arrange the elements in order of increasing...Ch. 7.4 - Arrange the elements Li. Be. and B in order of...Ch. 7.4 - For each of the following pairs of elements,...Ch. 7.4 - Prob. 4CPCh. 7.5 - Practice ProblemATTEMPT Would you expect Mg or Al...Ch. 7.5 - Prob. 1PPBCh. 7.5 - Practice ProblemCONCEPTUALIZE In the same...Ch. 7.5 - Prob. 1CPCh. 7.5 - 7.5.2 Which of the following pairs are...Ch. 7.5 - 7.5.3 Select the correct ground-state electron...Ch. 7.5 - Prob. 4CPCh. 7.6 - Practice Problem ATTEMPT Between which two charges...Ch. 7.6 - Practice ProblemBUILD What must the distance be...Ch. 7.6 - Prob. 1PPCCh. 7.6 - Which of the following species are isoelectronic...Ch. 7.6 - Which of the following are arranged correctly in...Ch. 7.6 - 7.6.3 Which of the following is the most realistic...Ch. 7.6 - Which of the following is the most realistic...Ch. 7.7 - Practice Problem ATTEMPT Write electron...Ch. 7.7 - Practice ProblemBUILD List all the species (atoms...Ch. 7.7 - Practice Problem CONCEPTUALIZE
Select the correct...Ch. 7.8 - Practice Problem ATTEMPT
Write electron...Ch. 7.8 - Practice Problem BUILD
What common d-block ion...Ch. 7.8 - Prob. 1PPCCh. 7.9 - Practice ProblemATTEMPT Arrange the following...Ch. 7.9 - Practice Problem BUILD
List all the common ions...Ch. 7.9 - Practice ProblemCONCEPTUALIZE Which periodic...Ch. 7 - Often we can compare properties of two elements...Ch. 7 - 7.2
The colored spheres represent the ions Based...Ch. 7 - Group 8A exhibits the highest first ionization...Ch. 7 - Which of the following best describes why Z eff...Ch. 7 - 7.1 Briefly describe the significance of...Ch. 7 - What is Moseley's contribution to the modern...Ch. 7 - 7.3 Describe the general layout of a modern...Ch. 7 - 7.4 What is the most important relationship among...Ch. 7 - Prob. 5QPCh. 7 - Prob. 6QPCh. 7 - Prob. 7QPCh. 7 - 7.8 What is a main group element? Give names and...Ch. 7 - 7.9 Without referring to a periodic table, write...Ch. 7 - Prob. 10QPCh. 7 - You are given a sample of a dark, shiny solid and...Ch. 7 - What are valence electrons? For main group...Ch. 7 - Write the outer electron configurations for the...Ch. 7 - Use the first-row transition metals ( Sc to Cu )...Ch. 7 - Arsenic is not an essential element for the human...Ch. 7 - 7.16 In the periodic table, the element hydrogen...Ch. 7 - 7.17 A neutral atom of a certain element has 34...Ch. 7 - 7.18 Group the following electron configurations...Ch. 7 - Group the following electron configurations in...Ch. 7 - Prob. 20QPCh. 7 - Specify the group of the periodic table in which...Ch. 7 - Prob. 22QPCh. 7 - Explain why the atomic radius of Be is smaller...Ch. 7 - The electron configuration of B is 1 S 2 2 S 2 2 P...Ch. 7 - 7 25 The electron configuration of C is . (a) If...Ch. 7 - Define atomic radius. Does the size of an atom...Ch. 7 - How does atomic radius change (a) from left to...Ch. 7 - Prob. 28QPCh. 7 - Sketch the outline of the periodic table, and show...Ch. 7 - Prob. 30QPCh. 7 - Explain the trends in electron affinity from...Ch. 7 - A hydrogen-like ion is an ion containing only one...Ch. 7 - Prob. 33QPCh. 7 - On the basis of their positions in the periodic...Ch. 7 - 7.35 Arrange the following atoms in order of...Ch. 7 - 7.36 Which is the largest atom in the third period...Ch. 7 - Which is the smallest atom in Group 7A ?Ch. 7 - Based on size, identify the spheres shown as Na,...Ch. 7 - Based on size, identify the spheres shown as K,...Ch. 7 - Why is the radius of the lithium atom considerably...Ch. 7 - Use the second period of the periodic table as an...Ch. 7 - Arrange the following in order of increasing first...Ch. 7 - Arrange the following in order of increasing first...Ch. 7 - 7.44 Use the third period of the periodic table as...Ch. 7 - In general, the first ionization energy increases...Ch. 7 - Prob. 46QPCh. 7 - 7.47 Two atoms have the electron configurations ....Ch. 7 - Prob. 48QPCh. 7 - Specify which of the following elements you would...Ch. 7 - Considering their electron affinities, do you...Ch. 7 - Explain why alkali metals have a greater affinity...Ch. 7 - 7.52 How does the electron configuration of ions...Ch. 7 - 7.53 What do we mean when we say that two ions or...Ch. 7 - Prob. 54QPCh. 7 - Give three examples of first-row transition metal...Ch. 7 - A M 2+ ion derived from a metal in the first...Ch. 7 - A metal ion with a net +3 charge has five...Ch. 7 - Prob. 58QPCh. 7 - 7.59 Group the species that are isoelectronic: .
Ch. 7 - 7.60 Write the ground-state electron...Ch. 7 - Prob. 61QPCh. 7 - 7.62 Which of the following species are...Ch. 7 - Prob. 63QPCh. 7 - Prob. 64QPCh. 7 - Indicate which one of the two species in each of...Ch. 7 - Prob. 66QPCh. 7 - Prob. 67QPCh. 7 - Prob. 68QPCh. 7 - Prob. 69QPCh. 7 - Prob. 70QPCh. 7 - Prob. 71QPCh. 7 - Prob. 72QPCh. 7 - Prob. 73QPCh. 7 - Prob. 74QPCh. 7 - Prob. 75QPCh. 7 - Prob. 76QPCh. 7 - Prob. 77QPCh. 7 - Prob. 78QPCh. 7 - 7 79 Write balanced equations for the reactions...Ch. 7 - Write formulas for and name the binary hydrogen...Ch. 7 - Prob. 81QPCh. 7 - Prob. 82APCh. 7 - Prob. 83APCh. 7 - Write equations representing the following...Ch. 7 - Prob. 85APCh. 7 - Write the empirical (or molecular) formulas of...Ch. 7 - 7.87 Arrange the following species in...Ch. 7 - In which of the following are the species written...Ch. 7 - Which of the following properties show a clear...Ch. 7 - Prob. 90APCh. 7 - Prob. 91APCh. 7 - 7.92 For each pair of elements listed, give three...Ch. 7 - Prob. 93APCh. 7 - Explain why the first electron affinity of sulfur...Ch. 7 - Prob. 95APCh. 7 - 7.96 Predict the products of the following oxides...Ch. 7 - 7.97 write the formulas and names of the oxides of...Ch. 7 - Prob. 98APCh. 7 - The formula for calculating the energies of an...Ch. 7 - 7.100 Why do noble gases have negative electron...Ch. 7 - 7.101 The atomic radius of K is 227 pm and that of...Ch. 7 - 7.102 The atomic radius of F is 72 pm and that of ...Ch. 7 - Match each of the elements on the right with its...Ch. 7 - Prob. 104APCh. 7 - Prob. 105APCh. 7 - Prob. 106APCh. 7 - Prob. 107APCh. 7 - Explain, in terms of their electron...Ch. 7 - 7.109 Write the formulas and names of the hydrides...Ch. 7 - Prob. 110APCh. 7 - Prob. 111APCh. 7 - Prob. 112APCh. 7 - Most transition metal ions are colored. For...Ch. 7 - Prob. 114APCh. 7 - Prob. 115APCh. 7 - Prob. 116APCh. 7 - 7.117 Although it is possible to determine the...Ch. 7 - Prob. 118APCh. 7 - Prob. 119APCh. 7 - Predict the atomic number and ground-state...Ch. 7 - Prob. 121APCh. 7 - 7.122 Match each of the elements on the right with...Ch. 7 - One way to estimate the effective charge ( Z eff )...Ch. 7 - Use your knowledge of thermochemistry to calculate...Ch. 7 - Prob. 125APCh. 7 - 7.126 On one graph, plot the effective nuclear...Ch. 7 - 7.127 One allotropic form of an element X is a...Ch. 7 - 7.128 Calculate the maximum wavelength of light...Ch. 7 - Prob. 129APCh. 7 - Element M is a shiny and highly reactive metal (...Ch. 7 - Write the ground-state electron configurations of...Ch. 7 - Thallium (Tl) is a neurotoxin and exists mostly in...Ch. 7 - Both Mg 2+ and Ca 2+ are important biological...Ch. 7 - Prob. 134APCh. 7 - Prob. 135APCh. 7 - Prob. 136APCh. 7 - Prob. 137APCh. 7 - 7.138 The ionization energy of a certain element...Ch. 7 - 7.139 Experimentally, the electron affinity of an...Ch. 7 - A halogen has valence electrons in which orbitals?...Ch. 7 - Prob. 2SEPPCh. 7 - Prob. 3SEPPCh. 7 - Prob. 4SEPP
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
- Arrange the following in the order of increasing mass. (a) a potassium ion, K+ (b) a phosphorus molecule, P4 (c) a potassium atom (d) a platinum atomarrow_forwardWhen a nonmetal oxide reacts with water, it forms an oxoacid with the same oxidation number as the nonmetal. Give the name and formula of the oxide used to prepare each of these oxoacids: (a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitric acid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.arrow_forward(c) Silicon (Si) is the most common chemical element in today's semiconductor industry. It has an atomic number of 14 and belongs to the Group IV (4) of the periodic table with its most common isotope being Si-29. (i) (ii) (iii) Explain what an isotope is. How many protons and how many neutrons are in the nucleus of this Silicon isotope? What is the electron configuration of Si?arrow_forward
- Fig 12.1 represents a neutral lithium atom. All the particles in the atom are shown on the diagram. (a) Use Fig. 12.1 to help you answer the following questions. (1) How many electrons does this atom have? (ii) What is the value of the proton number of this atom? (ii) How many neutrons does the atom have? (iv) What is the value of the nucleon number of this atom? (b) Write the appropriate numbers in the boxes below, to represent this atom of Lithium in nuclide notation. Li orbit nucleus Fig. 12.1 (c) Lithium-6 is another isotope of lithium. It has 6nucleons. (i) What is an isotope? (ii) How many protons does Lithium-6 have? (ii) How many neutrons does Lithium-6 havearrow_forwardAs you move down a family (group) of the periodic table the size of atoms increases from period 2 to period 3 by about 30-40 pm. For example, the radius of B is 84 pm and the radius of Al is 121 pm. However, as you move from aluminum (radius of 121 pm) to gallium (radius of 122 pm) the radius only increases by 1 pm. Which of the following explains this small increase in radius from Al to Ga? Select one: a. the scandide contraction b. the lanthanide contraction c. the mercurate elongation d. the zincate elongation e. Aluminum is just larger than you might expect.arrow_forwardName each of the following oxides. Assuming that thecompounds are ionic, what charge is associated with themetallic element in each case? (a) NiO, (b) MnO2, (c) Cr2O3,(d) MoO3.arrow_forward
- Write an electron-dot symbol for each element: (a) beryllium; (b) silicon; (c) iodine; (d) magnesium; (e) argon.arrow_forwardLook up the following information for the element iridium: (i) number of protons, neutrons, and electrons; (ii) atomic number and average atomic mass; (iii) the charge of the anion(s) or cation(s) that it commonly forms; (iv) the mass of its two most common isotopes and the number of protons and neutrons in each one. Also, comment briefly on the presence of this element in meteorite craters and the significance of this observation.arrow_forwardWrite an electron-dot symbol for each element: (a) sodium; (b) phosphorus.arrow_forward
- The isotope carbon11 does not occur in nature but has been made in the laboratory. This isotope is used in a medical imaging technique called positron emission tomography (PET, see Section 9.7A). Give the number of protons, neutrons, and electrons in an atom of carbon11.arrow_forwardWhich has the larger radius, N3- or P3-? Explain. (You may use a periodic table.)arrow_forwardElement "X" reacts with element "Y" to form an ionic compound containing X* and Y2- ions. Write a possible formula for the compound and suggest to which "Group" in the Periodic Table, the elements X and Y may belong to?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
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
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning