Explanation The transition metals are the elements that have the electrons in the d subshell. The electronic configuration of any element is written keeping in mind three rules. Afbau principle, Hund’s rule of maximum multiplicity and Pauli exclusion principle. According to Afbau principle electrons should be filled in order of increasing energy of the orbitals. The order of increasing energy is, 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p Hund’s rule of maximum multiplicity states that pairing of orbitals cannot be done unless each orbital of same energy gets one electron. Pauli exclusion principle states that each orbital can have maximum of two electrons and they must have opposite spins. The maximum number of electrons in different s, p, d and f subshells are 2, 6, 10 and 14 respectively. The first example of the ion that has an electronic configuration of n d 8 is Ni 2 + . The atomic number of Ni is 28 and the electronic configuration of Ni is [ Ar ] 3d 8 4s 2 . When Ni oxidizes to Ni 2 + , the two electrons are removed from the 4s orbital as it is the valence shell orbital. Therefore, the electronic configuration of Ni 2 + is [ Ar ] 3d 8 . The second example of the ion that has an electronic configuration of n d 8 is Pd 2 +

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

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Question

Chapter 16.7, Problem 16.16.2PE

Interpretation Introduction

To determine: The three examples of the ions that has an electronic configuration of nd8 where (n=3, 4, 5,...) .

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Chapter 16.7, Problem 16.16.1PE

Chapter 16.8, Problem 16.17.1PE

Chapter 16 Solutions

Chemistry: The Central Science (13th Edition)

Ch. 16.2 - Consider the following equation: Ca + (g) + e-...Ch. 16.2 - 7.55(a) Does metallic character increase,...Ch. 16.2 - Prob. 16.2.1PE Ch. 16.2 - Predict whether each of the following oxides is...Ch. 16.2 - Prob. 16.3.1PE Ch. 16.2 - Would you expect manganese(II) oxide, MnO, react...Ch. 16.3 - Prob. 16.4.1PE Ch. 16.3 - Prob. 16.4.2PE Ch. 16.3 - An element X reacts with oxygen to form X02 and...Ch. 16.3 - Prob. 16.5.2PE

Ch. 16.4 - Prob. 16.6.1PE Ch. 16.4 - Prob. 16.6.2PE Ch. 16.4 - Prob. 16.7.1PE Ch. 16.4 - Prob. 16.7.2PE Ch. 16.5 - Write a balanced equation for the reaction that...Ch. 16.5 - (a) As described in Section 7.7 , the alkali...Ch. 16.5 - Prob. 16.9.1PE Ch. 16.5 - Prob. 16.9.2PE Ch. 16.6 - Arrange each of the following sets of atoms and...Ch. 16.6 - Prob. 16.10.2PE Ch. 16.6 - In the ionic compoundsLiF,NaCI,KBr, andRbl, the...Ch. 16.6 - Prob. 16.11.2PE Ch. 16.6 - 7.38 Write equations that show the process for...Ch. 16.6 - Prob. 16.12.2PE Ch. 16.6 - Prob. 16.13.1PE Ch. 16.6 - Prob. 16.13.2PE Ch. 16.6 - (a) What is the trend in first ionization energies...Ch. 16.6 - Prob. 16.14.2PE Ch. 16.7 - Prob. 16.15.1PE Ch. 16.7 - Prob. 16.15.2PE Ch. 16.7 - Prob. 16.16.1PE Ch. 16.7 - Prob. 16.16.2PE Ch. 16.8 - Prob. 16.17.1PE Ch. 16.8 - Write an equation for the second electron affinity...Ch. 16.9 - If the electron affinity for an element is a...Ch. 16.9 - Prob. 16.18.2PE Ch. 16.9 - 7.52 What is the relationship between the...Ch. 16.9 - Prob. 16.19.2PE Ch. 16.10 - Prob. 16.20.1PE Ch. 16.10 - Prob. 16.20.2PE Ch. 16 - Mercury in the environment can exist in oxidation...Ch. 16 - When magnesium metal is burned in air (Figure 3.6...Ch. 16 - The dipole moment of chlorine monofluoride,...Ch. 16 - Prob. 3E Ch. 16 - Consider the element silicon, Si. Write its...Ch. 16 - Prob. 5E Ch. 16 - Prob. 6E Ch. 16 - Prob. 7E Ch. 16 - Prob. 8E Ch. 16 - Prob. 9E Ch. 16 - Prob. 10E Ch. 16 - Prob. 11E Ch. 16 - Prob. 12E Ch. 16 - Prob. 13E Ch. 16 - Prob. 14E Ch. 16 - Prob. 15E Ch. 16 - Prob. 16E Ch. 16 - Prob. 17E Ch. 16 - Prob. 18E Ch. 16 - Prob. 19E Ch. 16 - Prob. 20E Ch. 16 - Which of the these elements is most likely to from...Ch. 16 - Prob. 22E Ch. 16 - Which of the following bond is the most polar? H-F...Ch. 16 - Prob. 24E Ch. 16 - Prob. 25E Ch. 16 - Prob. 26E Ch. 16 - Which of the following bonds is the most polar? a....Ch. 16 - Which of the following bonds is most polar: S-Cl,...Ch. 16 - Prob. 29E Ch. 16 - How many valence electrons should appear in the...Ch. 16 - Compare the lewis symbol for neon the structure...Ch. 16 - Prob. 32E Ch. 16 - Prob. 33E Ch. 16 - Prob. 34E Ch. 16 - Prob. 35E Ch. 16 - Prob. 36E Ch. 16 - Which of the statements about resonance is true?...Ch. 16 - Prob. 38E Ch. 16 - Prob. 39E Ch. 16 - Prob. 40E Ch. 16 - Prob. 41E Ch. 16 - A portion of a two-dimensional "slab" of NaCl(s)...Ch. 16 - Prob. 43E Ch. 16 - Prob. 44E Ch. 16 - Incomplete Lewis structures for the nitrous acid...Ch. 16 - Prob. 46E Ch. 16 - Prob. 47E Ch. 16 - Prob. 48E Ch. 16 - True or false: The hydrogen atom is most stable...Ch. 16 - Prob. 50E Ch. 16 - What is the Lewis symbol for each of the following...Ch. 16 - Using Lewis symbols, diagram the reaction between...Ch. 16 - Use Lewis symbols to represent the reaction that...Ch. 16 - Predict the chemical formula of the ionic compound...Ch. 16 - Prob. 55E Ch. 16 - Prob. 56E Ch. 16 - Prob. 57E Ch. 16 - Is lattice energy usually endothermic or...Ch. 16 - NaCI and KF have the same crystal structure. The...Ch. 16 - Consider the ionic compounds KF, NaCl, NaBr, and...Ch. 16 - Which of the following trends in lattice energy is...Ch. 16 - Energy is required to remove two electrons from Ca...Ch. 16 - Prob. 63E Ch. 16 - Use data from Appendix C, Figure 7.10, and Figure...Ch. 16 - Prob. 65E Ch. 16 - Prob. 66E Ch. 16 - Prob. 67E Ch. 16 - Using Lewis symbols and Lewis structures, diagram...Ch. 16 - Use Lewis symbols and Lewis structures to diagram...Ch. 16 - Prob. 70E Ch. 16 - What is the trend in electronegativity going from...Ch. 16 - Prob. 72E Ch. 16 - By referring only to the periodic table, select...Ch. 16 - which of the following bonds are polar? B-F,...Ch. 16 - Prob. 75E Ch. 16 - Prob. 76E Ch. 16 - Prob. 77E Ch. 16 - In the following pairs of binary compounds,...Ch. 16 - Prob. 79E Ch. 16 - Prob. 80E Ch. 16 - Draw the dominant Lewis structure for the...Ch. 16 - Prob. 82E Ch. 16 - Prob. 83E Ch. 16 - Prob. 84E Ch. 16 - Prob. 85E Ch. 16 - Prob. 86E Ch. 16 - Prob. 87E Ch. 16 - Prob. 88E Ch. 16 - Prob. 89E Ch. 16 - Prob. 90E Ch. 16 - 8.62 For Group 3A-7A elements in the third row of...Ch. 16 - Draw the Lewis structures for each of the...Ch. 16 - Prob. 93E Ch. 16 - Prob. 94E Ch. 16 - 8.66 Describe the molecule xenon trioxide, XeO3,...Ch. 16 - 8.67 There are many Lewis structures you could...Ch. 16 - Prob. 97E Ch. 16 - Using Table 8.3, estimate H for each of the...Ch. 16 - Using Table 8.3, estimate H for the following...Ch. 16 - Prob. 100AE Ch. 16 - Prob. 101AE Ch. 16 - Prob. 102AE Ch. 16 - Prob. 103AE Ch. 16 - Consider the stable elements through lead (Z =...Ch. 16 - 17.80]Figure 7.4 shows the radial probability...Ch. 16 - (a) If the core electrons were totally effective...Ch. 16 - Prob. 107AE Ch. 16 - Prob. 108AE Ch. 16 - Prob. 109AE Ch. 16 - The following observations are made about two...Ch. 16 - Prob. 111AE Ch. 16 - Prob. 112AE Ch. 16 - Prob. 113AE Ch. 16 - Prob. 114AE Ch. 16 - Prob. 115AE Ch. 16 - Prob. 116IE Ch. 16 - Prob. 117IE Ch. 16 - Prob. 118IE Ch. 16 - Prob. 119IE Ch. 16 - Prob. 120IE Ch. 16 - The electron affinities. in kJ/mol, for the group...Ch. 16 - 7.99 Hydrogen is an unusual element because it...Ch. 16 - Prob. 123IE Ch. 16 - Prob. 124IE Ch. 16 - Which of the following is the expected product of...Ch. 16 - Elemental cesium reacts more violently with water...

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