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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 7.6, Problem 3Q
Textbook Problem
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Why are copper atoms (radius = 128 pm) slightly larger than iron atoms (radius = 124 pm)?

Interpretation Introduction

Interpretation:

The copper atoms are slightly larger than iron atoms; the reason has to be explained.

Concept Introduction:

Atomic radius: The concept explain chemical element is a measured of the size of its atoms, in other words to measure the distance from the center of the nucleus to the boundary of the surrounding cloud of number of electrons.

Electronic configuration: The electronic configuration is the distribution of electrons of an given molecule or respective atoms in atomic or molecular orbitals.

The aufbau principle: This rule statues that ground state of an atom or ions electrons fill atomic orbitals of the lowest available energy levels before occupying higher levels. Once the 1s shell is filled only then 2s subshell is occupied.

Hund's Rule: The every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.

Explanation of Solution

The copper (Cu) system is having d9 system in respective orbital shells but Iron (Fe) having d6 system. The Copper possess electrons repulsion much larger when compare to Fe orbital shells, so Iron atom radii little smaller.

Let us consider the (Cu)andFeelectronic configuration for using its orbital notations boxes.

  • Electronic configuration of Cupper (Cu):

  Atomicnumber (Z)ofCopper Cu= 29spdfwith noble gas notation=[Ar]3d104s1Orbitalboxnotation       = [Ar]3d10 </

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Chapter 7 Solutions

Chemistry & Chemical Reactivity
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Ch. 7.4 - 2. Which of the following ions has the largest...Ch. 7.4 - Which of the following species is most...Ch. 7.5 - Without looking at the figures for the periodic...Ch. 7.5 - What is the trend in sizes of the ions K+, S2, and...Ch. 7.5 - Locate the elements C, N, Si, and P in the...Ch. 7.6 - Give the electron configurations for iron and the...Ch. 7.6 - In hemoglobin, iron can be in the iron(II) or...Ch. 7.6 - Why are copper atoms (radius = 128 pm) slightly...Ch. 7.6 - In hemoglobin, the iron is enclosed by the...Ch. 7.6 - 1. Which of the following is an incorrect...Ch. 7.6 - 2. 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(a) Which...Ch. 7 - Compare the elements B. Al, C, and Si. (a) Which...Ch. 7 - Explain each answer briefly. (a) Place the...Ch. 7 - Explain each answer briefly. (a) Rank the...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Identify the element that corresponds to each of...Ch. 7 - Explain why the photoelectron spectra of hydrogen...Ch. 7 - Sketch the major features (number of peaks and...Ch. 7 - These questions are not designated as to type or...Ch. 7 - The deep blue color of sapphires comes from the...Ch. 7 - Using an orbital box diagram and noble gas...Ch. 7 - The rare earth elements, or lanthanides, commonly...Ch. 7 - A neutral atom has two electrons with n = 1, eight...Ch. 7 - Element 109, now named meitnerium (in honor of the...Ch. 7 - Which of the following is not an allowable set of...Ch. 7 - A possible excited state for the H atom has an...Ch. 7 - The magnet in the following photo is made from...Ch. 7 - Name the element corresponding to each...Ch. 7 - Arrange the following atoms in order of increasing...Ch. 7 - Rank the following in order of increasing...Ch. 7 - Answer the questions below about the elements A...Ch. 7 - Answer (he following questions about the elements...Ch. 7 - Which of the following ions are unlikely to be...Ch. 7 - Place the following ions in order of decreasing...Ch. 7 - Answer each of the following questions: (a) Of the...Ch. 7 - The following are isoelectronic species: Cl, K+,...Ch. 7 - Compare the elements Na. B. Al, and C with regard...Ch. 7 - Two elements in the second transition series (Y...Ch. 7 - The configuration for an element is given here....Ch. 7 - The configuration of an element is given here. (a)...Ch. 7 - Answer the questions below about the elements A...Ch. 7 - Answer the questions below concerning ground state...Ch. 7 - Nickel(II) formate [Ni(HCO2)2] is widely used as a...Ch. 7 - Spinets are solids with the general formula M2+...Ch. 7 - The following questions use concepts from this and...Ch. 7 - Which ions in the following list are not likely to...Ch. 7 - Answer the following questions about first...Ch. 7 - The ionization of the hydrogen atom can be...Ch. 7 - Compare the configurations below with two...Ch. 7 - The bond lengths in Cl2, Br2, and I2 are 200, 228,...Ch. 7 - Write electron configurations to show the first...Ch. 7 - What is the trend in ionization energy when...Ch. 7 - (a) Explain why the sizes of atoms change when...Ch. 7 - Which of the following elements has the greatest...Ch. 7 - What arguments would you use to convince another...Ch. 7 - Explain why the first ionization energy of Ca is...Ch. 7 - The energies of the orbitals in many elements have...Ch. 7 - The ionization energies for the removal of the...Ch. 7 - Using your knowledge of the trends in element...Ch. 7 - The densities (in g/cm3) of elements in Croups 6B,...Ch. 7 - The discovery of two new elements (atomic numbers...Ch. 7 - Explain why the reaction of calcium and fluorine...Ch. 7 - Thionyl chloride. SOCl2, is an important...Ch. 7 - Sodium metal reacts readily with chlorine gas to...Ch. 7 - Slaters rules are a way to estimate the effective...

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