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Chapter 2: Problem 1

Cite the difference between atomic mass and atomic weight.

Short Answer

Expert verified
Answer: The key differences between atomic mass and atomic weight are: 1. Atomic mass is the mass of a single atom or isotope, while atomic weight is the weighted average mass of an element considering all its isotopes. 2. Atomic mass is expressed in atomic mass units (amu), whereas atomic weight is expressed in unified atomic mass units (u or Da). 3. Atomic mass deals with individual atoms, whereas atomic weight pertains to all the isotopes of an element collectively.

Step by step solution

01

Define Atomic Mass

Atomic mass refers to the mass of an individual atom or isotope, and is measured in atomic mass units (amu). It indicates the total number of protons and neutrons present in the nucleus of an atom. Step 2:
02

Define Atomic Weight

Atomic weight, also known as relative atomic mass, is the average mass of the atoms of an element, taking into account the abundance and mass of each isotope. It is a weighted average, and is generally expressed with a unit called unified atomic mass unit (u or Da). Step 3:
03

Identify Key Differences

1. Atomic mass is the mass of a single atom or isotope, while atomic weight is the weighted average mass of an element considering all its isotopes. 2. Atomic mass is expressed in atomic mass units (amu), whereas atomic weight is expressed in unified atomic mass units (u or Da). 3. Atomic mass deals with individual atoms, whereas atomic weight pertains to all the isotopes of an element collectively.

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Most popular questions from this chapter

Give the electron configurations for the following ions: \(\mathrm{Fe}^{2+}, \mathrm{Al}^{3+}, \mathrm{Cu}^{+}, \mathrm{Ba}^{2+}, \mathrm{Br}^{-}\), and \(\mathrm{O}^{2-}\)

(a) What electron subshell is being filled for the rare earth series of elements on the periodic table? (b) What electron subshell is being filled for the actinide series?

6 Allowed values for the quantum numbers of electrons are as follows: $$ \begin{aligned} n &=1,2,3, \ldots \\ l &=0,1,2,3, \ldots, n-1 \\ m_{l} &=0, \pm 1, \pm 2, \pm 3, \ldots, \pm l \\ m_{s} &=\pm \frac{1}{2} \end{aligned} $$ The relationships between \(n\) and the shell designations are noted in Table 2.1. Relative to the subshells, \(l=0\) corresponds to an \(s\) subshell \(l=1\) corresponds to a \(p\) subshell \(l=2\) corresponds to a \(d\) subshell \(l=3\) corresponds to an \(f\) subshell For the \(K\) shell, the four quantum numbers for each of the two electrons in the \(1 s\) state, in the order of \(n l m_{i} m_{s}\), are \(100 \frac{1}{2}\) and \(100\left(-\frac{1}{2}\right)\) Write the four quantum numbers for all of the electrons in the \(L\) and \(M\) shells, and note which correspond to the \(s, p\), and \(d\) subshells.

The net potential energy between two adjacent ions, \(E_{N}\), may be represented by the sum of Equations \(2.8\) and \(2.9\); that is, $$ E_{N}=-\frac{A}{r}+\frac{B}{r^{n}} $$ Calculate the bonding energy \(E_{0}\) in terms of the parameters \(A, B\), and \(n\) using the following procedure: 1\. Differentiate \(E_{N}\) with respect to \(r\), and then set the resulting expression equal to zero, because the curve of \(E_{N}\) versus \(r\) is a minimum at \(E_{0 \text { - }}\) 2\. Solve for \(r\) in terms of \(A, B\), and \(n\), which yields \(r_{0}\), the equilibrium interionic spacing. 3\. Determine the expression for \(E_{0}\) by substituting \(r_{0}\) into Equation \(2.11\).

Chromium has four naturally occurring isotopes: \(4.34 \%\) of \({ }^{50} \mathrm{Cr}\), with an atomic weight of \(49.9460\) amu; \(83.79 \%\) of \({ }^{52} \mathrm{Cr}\), with an atomic weight of \(51.9405 \mathrm{amu} ; 9.50 \%\) of \({ }^{53} \mathrm{Cr}\), with an atomic weight of \(52.9407 \mathrm{amu} ;\) and \(2.37 \%\) of \({ }^{54} \mathrm{Cr}\), with an atomic weight of \(53.9389\) amu. On the basis of these data, confirm that the average atomic weight of \(\mathrm{Cr}\) is \(51.9963 \mathrm{amu}\)
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