Chemistry: The Central Science (13th Edition)
13th Edition
ISBN: 9780321910417
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 7, Problem 13E
(a) What is meant by the term effective nuclear charge? (b) How does the effective nuclear charge experienced by the valence electrons of an atom vary going from left to rightacross a period of the periodic table?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Q1.
This question is about atomic structure.
(a) Write the full electron configuration for each of the following species.
CH
Fe2+
(b) Write an equation, including state symbols, to represent the process that occurs
when the third ionisation energy of manganese is measured.
(c)
State which of the elements magnesium and aluminium has the lower first ionisation
energy
Explain your answer.
(d) A sample of nickel was analysed in a time of flight (TOF) mass spectrometer. The
sample was ionised by electron impact ionisation. The spectrum produced showed
three peaks with abundances as set out in the table.
m/z
Abundance /%
58
61.0
60
29.1
61
9.9
Give the symbol, including mass number, of the ion that would reach the detector
first in the sample.
Calculate the relative atomic mass of the nickel in the sample.
Give your answer to one decimal place.
Page 2 of 12
Symbol of ion
Relative atomic mass
(1) What is the valence electron configuration for the arsenic atom?
(2) What is the valence electron configuration for the fluorine atom?
5. The atoms and ions Ne, N³-, F, Mg2+, and Si4+ are part of an
isoelectronic series.
(a) Which of these will have the smallest effective nuclear
charge acting on the outermost electron?
(b) Which one possess the greatest effective nuclear charge?
(c) Which ion will be the largest in size? Explain why.
Chapter 7 Solutions
Chemistry: The Central Science (13th Edition)
Ch. 7.3 - Prob. 7.1.1PECh. 7.3 - Prob. 7.1.2PECh. 7.3 - Prob. 7.2.1PECh. 7.3 - Prob. 7.2.2PECh. 7.3 - Prob. 7.3.1PECh. 7.3 - Prob. 7.3.2PECh. 7.3 - Prob. 7.4.1PECh. 7.3 - Prob. 7.4.2PECh. 7.4 - Prob. 7.5.1PECh. 7.4 - Prob. 7.5.2PE
Ch. 7.4 - Prob. 7.6.1PECh. 7.4 - The atomic masses of hydrogen-2 (deuterium),...Ch. 7.4 - Prob. 7.7.1PECh. 7.4 - Prob. 7.7.2PECh. 7.6 - Prob. 7.8.1PECh. 7.6 - Prob. 7.8.2PECh. 7.6 - Prob. 7.9.1PECh. 7.6 - Prob. 7.9.2PECh. 7.7 - Prob. 7.10.1PECh. 7.7 - Prob. 7.10.2PECh. 7 - Prob. 1DECh. 7 - Prob. 1ECh. 7 - Prob. 2ECh. 7 - Prob. 3ECh. 7 - Prob. 4ECh. 7 - Prob. 5ECh. 7 - Prob. 6ECh. 7 - Prob. 7ECh. 7 - Prob. 8ECh. 7 - Prob. 9ECh. 7 - Prob. 10ECh. 7 - You might have expected that the elements would...Ch. 7 - Prob. 12ECh. 7 - (a) What is meant by the term effective nuclear...Ch. 7 - Prob. 14ECh. 7 - Prob. 15ECh. 7 - Prob. 16ECh. 7 - Prob. 17ECh. 7 - Prob. 18ECh. 7 - Prob. 19ECh. 7 - Why does the quantum mechanical description or...Ch. 7 - Prob. 21ECh. 7 - Prob. 22ECh. 7 - Prob. 23ECh. 7 - Prob. 24ECh. 7 - Prob. 25ECh. 7 - Prob. 26ECh. 7 - Prob. 27ECh. 7 - Prob. 28ECh. 7 - Prob. 29ECh. 7 - Prob. 30ECh. 7 - Prob. 31ECh. 7 - Prob. 32ECh. 7 - Prob. 33ECh. 7 - Prob. 34ECh. 7 - Prob. 35ECh. 7 - In the ionic compounds LiF, NaCl, KBr, and RbI,...Ch. 7 - Prob. 37ECh. 7 - Prob. 38ECh. 7 - Prob. 39ECh. 7 - Prob. 40ECh. 7 - Prob. 41ECh. 7 - Prob. 42ECh. 7 - Prob. 43ECh. 7 - Prob. 44ECh. 7 - Prob. 45ECh. 7 - Prob. 46ECh. 7 - Prob. 47ECh. 7 - Prob. 48ECh. 7 - Prob. 49ECh. 7 - Prob. 50ECh. 7 - 7.51 Although the electron affinity ofbromineis a...Ch. 7 - Prob. 52ECh. 7 - Prob. 53ECh. 7 - Prob. 54ECh. 7 - Prob. 55ECh. 7 - Prob. 56ECh. 7 - Prob. 57ECh. 7 - Prob. 58ECh. 7 - Prob. 59ECh. 7 - Prob. 60ECh. 7 - Prob. 61ECh. 7 - Prob. 62ECh. 7 - Prob. 63ECh. 7 - Prob. 64ECh. 7 - Prob. 65ECh. 7 - Why does xenon form stable compounds with...Ch. 7 - Prob. 67ECh. 7 - Prob. 68ECh. 7 - Prob. 69ECh. 7 - Prob. 70ECh. 7 - Prob. 71ECh. 7 - Prob. 72ECh. 7 - Prob. 73ECh. 7 - Prob. 74ECh. 7 - Prob. 75ECh. 7 - Prob. 76ECh. 7 - Prob. 77ECh. 7 - Prob. 78ECh. 7 - Prob. 79AECh. 7 - Prob. 80AECh. 7 - Prob. 81AECh. 7 - Prob. 82AECh. 7 - Prob. 83AECh. 7 - Prob. 84AECh. 7 - Prob. 85AECh. 7 - Prob. 86AECh. 7 - Prob. 87AECh. 7 - Prob. 88AECh. 7 - Prob. 89AECh. 7 - Prob. 90AECh. 7 - Prob. 91AECh. 7 - Write a chemical formula for each compound or ion,...Ch. 7 - Prob. 93AECh. 7 - Prob. 94AECh. 7 - Prob. 95AECh. 7 - Prob. 96AECh. 7 - Prob. 97AECh. 7 - Prob. 98AECh. 7 - Prob. 99AECh. 7 - Prob. 100AECh. 7 - Prob. 101AECh. 7 - Prob. 102AECh. 7 - Prob. 103AECh. 7 - Prob. 104AECh. 7 - Prob. 105AECh. 7 - Prob. 106AECh. 7 - Prob. 107AECh. 7 - Prob. 108AECh. 7 - Prob. 109AECh. 7 - Prob. 110IECh. 7 - Prob. 111IECh. 7 - Prob. 112IECh. 7 - Prob. 113IECh. 7 - Prob. 114IECh. 7 - Prob. 115IE
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
- Write the ground-state electron configurations of the following ions. (a) Li+ (b) N3− (c) In3+ (Use the noble gas core electron configuration in your answer.) (d) Tl+ (Use the noble gas core electron configuration in your answer.)arrow_forward(a) True or false: An element’s number of valence electronsis the same as its atomic number. (b) How many valenceelectrons does a nitrogen atom possess? (c) An atom has theelectron configuration 1s22s22p63s23p2. How many valenceelectrons does the atom have?arrow_forwardDetermine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) nitrogen; (b) potassium.arrow_forward
- (a) Write the electron configuration for Li and estimate theeffective nuclear charge experienced by the valence electron.(b) The energy of an electron in a one-electron atom or ion equals (-2.18 x 10-18 J) aZ2/n2 b, where Z is the nuclear chargeand n is the principal quantum number of the electron. Estimatethe first ionization energy of Li. (c) Compare the resultof your calculation with the value reported in Table 7.4 andexplain the difference. (d) What value of the effective nuclearcharge gives the proper value for the ionization energy? Doesthis agree with your explanation in part (c)?arrow_forwardGive the shell electron configuration for the following. (For example, the shell electron configuration of lithium is written 2,1.) (a) argon (b) magnesiumarrow_forward(B) 0.832 mL (C) 1.20 mL (D) 8.59 mL 2. Consider the Bohr Model of Phosphorus below. Which statement is FALSE? (A) The electrostatic potential energy of ALL electrons is negative. (B) The electrons with the least potential energy are closest to the nucleus. (C) Energy is released when the electron is ejected from the atom. (D) When an electron is infinitely far from the nucleus, the electrostatic potential energy is 0.arrow_forward
- The electron in the hydrogen atom (in its ground state) orbits the nucleus at a distance of 0.5292 Å. (a) Calculate the gravitational force and (b) the electrostatic force of attraction between the two. (c) Comment on the magnitude and the importance of these two forces. [G, gravitational constant = 6.672 x 10-11 N m2 kg-2; 4+Єo = 1.113 x 10-10 C2 m-1 J-1]arrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward(a) Why do successive IEs of a given element always increase? (b) When the difference between successive IEs of a given element is exceptionally large (for example, between IE1 and IE2 of K), what do we learn about its electron configuration? (c) The bars represent the relative magnitudes of the first five ionization energies of an atom: Identify the element and write its complete electron config uration, assuming it comes from (a) Period 2; (b) Period 3; (c) Period 4.arrow_forward
- Consider S, Cl, and K and their most common ions. (a) Listthe atoms in order of increasing size. (b) List the ions inorder of increasing size. (c) Explain any differences in theorders of the atomic and ionic sizes.arrow_forwardBoron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively.(a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?arrow_forward(1) What is the valence electron configuration for the sodium atom? (2) What is the valence electron configuration for the boron atom?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
Living By Chemistry: First Edition TextbookChemistryISBN:9781559539418Author:Angelica StacyPublisher:MAC HIGHER
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
Living By Chemistry: First Edition Textbook
Chemistry
ISBN:9781559539418
Author:Angelica Stacy
Publisher:MAC HIGHER
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