# 8.A: Atomic Structure (Answers)

- Page ID
- 10333

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**8.1.** No. The quantum number \(\displaystyle m=−l,−l+1,…,0,…,l−1,l\). Thus, the magnitude of \(\displaystyle L_z\) is always less than **L** because \(\displaystyle <\sqrt{l(l+1)}\)

**8.2.** \(\displaystyle s=3/2<\)

**8.3.** frequency quadruples

## Conceptual Questions

**1. ****n** (principal quantum number) → total energy

\(\displaystyle l\) (orbital angular quantum number) → total absolute magnitude of the orbital angular momentum

\(\displaystyle m\) (orbital angular projection quantum number) → z-component of the orbital angular momentum

**3. **The Bohr model describes the electron as a particle that moves around the proton in well-defined orbits. Schrödinger’s model describes the electron as a wave, and knowledge about the position of the electron is restricted to probability statements. The total energy of the electron in the ground state (and all excited states) is the same for both models. However, the orbital angular momentum of the ground state is different for these models. In Bohr’s model, \(\displaystyle L(ground state)=1\), and in Schrödinger’s model, \(\displaystyle L(ground state)=0\).

**5.** a, c, d; The total energy is changed (Zeeman splitting). The work done on the hydrogen atom rotates the atom, so the **z**-component of angular momentum and polar angle are affected. However, the angular momentum is not affected.

**7. **Even in the ground state \(\displaystyle (l=0)\), a hydrogen atom has magnetic properties due the intrinsic (internal) electron spin. The magnetic moment of an electron is proportional to its spin.

**9.** For all electrons, \(\displaystyle s=½\) and \(\displaystyle m_s=±½\). As we will see, not all particles have the same spin quantum number. For example, a photon as a spin 1 (\(\displaystyle s=1\)), and a Higgs boson has spin 0 (\(\displaystyle s=0\)).

**11.** An electron has a magnetic moment associated with its intrinsic (internal) spin. Spin-orbit coupling occurs when this interacts with the magnetic field produced by the orbital angular momentum of the electron.

**13. **Elements that belong in the same column in the periodic table of elements have the same fillings of their outer shells, and therefore the same number of valence electrons. For example:

Li: \(\displaystyle 1s^22s^1\) (one valence electron in the \(\displaystyle n=2\) shell)

Na: \(\displaystyle 1s^22s2p^63s^1\) (one valence electron in the \(\displaystyle n=2\) shell)

Both, Li and Na belong to first column.

**15.** Atomic and molecular spectra are said to be “discrete,” because only certain spectral lines are observed. In contrast, spectra from a white light source (consisting of many photon frequencies) are continuous because a continuous “rainbow” of colors is observed.

**17.** UV light consists of relatively high frequency (short wavelength) photons. So the energy of the absorbed photon and the energy transition (\(\displaystyle ΔE\)) in the atom is relatively large. In comparison, visible light consists of relatively lower-frequency photons. Therefore, the energy transition in the atom and the energy of the emitted photon is relatively small.

**19. **For macroscopic systems, the quantum numbers are very large, so the energy difference (\(\displaystyle ΔE\)) between adjacent energy levels (orbits) is very small. The energy released in transitions between these closely space energy levels is much too small to be detected.

**21. **Laser light relies on the process of stimulated emission. In this process, electrons must be prepared in an excited (upper) metastable state such that the passage of light through the system produces de-excitations and, therefore, additional light.

**23. **A Blu-Ray player uses blue laser light to probe the bumps and pits of the disc and a CD player uses red laser light. The relatively short-wavelength blue light is necessary to probe the smaller pits and bumps on a Blu-ray disc; smaller pits and bumps correspond to higher storage densities.

## Problems

**25.** \(\displaystyle (r,θ,ϕ)=(\sqrt{6,}66°,27°)\).

**27. **\(\displaystyle ±3,±2,±1,0\) are possible

**29.** 18

**31.** \(\displaystyle F=−k\frac{Qq}{r^2}\)

**33.** (1, 1, 1)

**35. **For the orbital angular momentum quantum number, **l**, the allowed values of:

\(\displaystyle m=−l,−l+1,...0,...l−1,l\).

With the exception of \(\displaystyle m=0\), the total number is just **2l** because the number of states on either side of \(\displaystyle m=0\) is just **l**. Including \(\displaystyle m=0\), the total number of orbital angular momentum states for the orbital angular momentum quantum number, **l**, is: \(\displaystyle 2l+1\). Later, when we consider electron spin, the total number of angular momentum states will be found to twice this value because each orbital angular momentum states is associated with two states of electron spin: spin up and spin down).

**37.** The probability that the **1s** electron of a hydrogen atom is found outside of the Bohr radius is \(\displaystyle ∫^∞_{a_0}P(r)dr≈0.68\)

**39.** For \(\displaystyle n=2, l=0\) (1 state), and \(\displaystyle l=1\) (3 states). The total is 4.

**41. **The **3p** state corresponds to \(\displaystyle n=3, l=2\). Therefore, \(\displaystyle μ=μ_B\sqrt{6}\)

**43.** The ratio of their masses is 1/207, so the ratio of their magnetic moments is 207. The electron’s magnetic moment is more than 200 times larger than the muon.

**45.** a. The 3d state corresponds to \(\displaystyle n=3, l=2\). So,

\(\displaystyle I=4.43×10^{−7}A\).

b. The maximum torque occurs when the magnetic moment and external magnetic field vectors are at right angles \(\displaystyle (sinθ=1)\). In this case:

\(\displaystyle |\vec{τ}|=μB.\)

\(\displaystyle τ=5.70×10^{−26}N⋅m\)..

**47. **A **3p **electron is in the state \(\displaystyle n=3\) and \(\displaystyle l=1\). The minimum torque magnitude occurs when the magnetic moment and external magnetic field vectors are most parallel (antiparallel). This occurs when \(\displaystyle m=±1\). The torque magnitude is given by

\(\displaystyle |\vec{τ}|=μBsinθ\),

Where

\(\displaystyle μ=(1.31×10^{−24}J/T)\).

For \(\displaystyle m=±1\), we have:

\(\displaystyle |\vec{τ⃗}|=2.32×10^{21}N⋅m\).

**49.** An infinitesimal work **dW** done by a magnetic torque \(\displaystyle τ\) to rotate the magnetic moment through an angle \(\displaystyle −dθ\):

\(\displaystyle dW=τ(−dθ)\),

where \(\displaystyle τ=|\vec{μ}×\vec{B}∣\). Work done is interpreted as a drop in potential energy U, so

\(\displaystyle dW=−dU.\)

The total energy change is determined by summing over infinitesimal changes in the potential energy:

\(\displaystyle U=−μBcosθ\)

\(\displaystyle U=−\vec{μ}⋅\vec{B}\).

**51. **Spin up (relative to positive **z**-axis):

\(\displaystyle θ=55°\).

Spin down (relative to positive **z**-axis):

\(\displaystyle θ=cos^{−1}(\frac{S_z}{S})=cos^{−1}(\frac{−\frac{1}{2}}{\frac{\sqrt{3}}{2}})=cos^{−1}(\frac{−1}{\sqrt{3}})=125°.\)

**53. **The spin projection quantum number is \(\displaystyle m_s=±½\), so the z-component of the magnetic moment is

\(\displaystyle μ_z=±μ_B\).

The potential energy associated with the interaction between the electron and the external magnetic field is

\(\displaystyle U=∓μ_BB\).

The energy difference between these states is \(\displaystyle ΔE=2μ_BB\), so the wavelength of light produced is

\(\displaystyle λ=5.36×10^{−5}m≈53.6μm\)

**55.** It is increased by a factor of 2.

**57. **a. 32;

b.

__ℓ__ (2ℓ+1)

0 s 2(0+1) =2

1 p 2(2+1) =6

2 d 2(4+1) =10

__3 f 2(6+1) =14__

32

**59.** a. and e. are allowed; the others are not allowed.

b. \(\displaystyle l=3\) not allowed for \(\displaystyle n=1,l≤(n−1)\).

c. Cannot have three electrons in **s **subshell because \(\displaystyle 3>2(2l+1)=2\).

d. Cannot have seven electrons in **p** subshell (max of 6) \(\displaystyle 2(2l+1)=2(2+1)=6\).

**61.** \(\displaystyle [Ar]4s^23d^6\)

**63. **a. The minimum value of \(\displaystyle ℓ\) is \(\displaystyle l=2\) to have nine electrons in it.

b. \(\displaystyle 3d^9\).

**65.** \(\displaystyle [He]2s^22p^2\)

**67. **For \(\displaystyle He^+\), one electron “orbits” a nucleus with two protons and two neutrons (\(\displaystyle Z=2\)). Ionization energy refers to the energy required to remove the electron from the atom. The energy needed to remove the electron in the ground state of He+He+ ion to infinity is negative the value of the ground state energy, written:

\(\displaystyle E=−54.4eV\).

Thus, the energy to ionize the electron is \(\displaystyle +54.4eV\).

Similarly, the energy needed to remove an electron in the first excited state of \(\displaystyle Li^{2+}\) ion to infinity is negative the value of the first excited state energy, written:

\(\displaystyle E=−30.6eV\).

The energy to ionize the electron is 30.6 eV.

**69. **The wavelength of the laser is given by:

\(\displaystyle λ=\frac{hc}{−ΔE}\),

where \(\displaystyle E_γ\) is the energy of the photon and \(\displaystyle ΔE\) is the magnitude of the energy difference. Solving for the latter, we get:

\(\displaystyle ΔE=−2.795eV\).

The negative sign indicates that the electron lost energy in the transition.

**71.** \(\displaystyle ΔE_{L→K}≈(Z−1)^2(10.2eV)=3.68×10^3eV\).

**73.** According to the conservation of the energy, the potential energy of the electron is converted completely into kinetic energy. The initial kinetic energy of the electron is zero (the electron begins at rest). So, the kinetic energy of the electron just before it strikes the target is:

\(\displaystyle K=eΔV\).

If all of this energy is converted into braking radiation, the frequency of the emitted radiation is a maximum, therefore:

\(\displaystyle f_{max}=\frac{eΔV}{h}\).

When the emitted frequency is a maximum, then the emitted wavelength is a minimum, so:

\(\displaystyle λ_{min}=0.1293nm\).

**75.** A muon is 200 times heavier than an electron, but the minimum wavelength does not depend on mass, so the result is unchanged.

**77.** \(\displaystyle 4.13×10^{−11}m\)

**79. **72.5 keV

**81. **The atomic numbers for Cu and Au are \(\displaystyle Z=29\) and 79,** **respectively. The X-ray photon frequency for gold is greater than copper by a factor:

\(\displaystyle (\frac{f_{Au}}{f_{Cu}})^2=(\frac{79−1}{29−1})^2≈8\).

Therefore, the X-ray wavelength of Au is about eight times shorter than for copper.

**83. **a. If flesh has the same density as water, then we used \(\displaystyle 1.34×10^{23}\) photons.

b. 2.52 MW

## Additional Problems

**85. **The smallest angle corresponds to \(\displaystyle l=n−1\) and \(\displaystyle m=l=n−1\). Therefore \(\displaystyle θ=cos^{−1}(\sqrt{n−1}{n}\)).

**87. **a. According to Equation 8.1, when \(\displaystyle r=0, U(r)=−∞\), and when \(\displaystyle r=+∞,U(r)=0\). The former result suggests that the electron can have an infinite negative potential energy. The quantum model of the hydrogen atom avoids this possibility because the probability density at \(\displaystyle r=0\) is zero.

**89.** A formal solution using sums is somewhat complicated. However, the answer easily found by studying the mathematical pattern between the principal quantum number and the total number of orbital angular momentum states.

For \(\displaystyle n=1\), the total number of orbital angular momentum states is 1; for \(\displaystyle n=2\), the total number is 4; and, when \(\displaystyle n=3\), the total number is 9, and so on. The pattern suggests the total number of orbital angular momentum states for the nth shell is \(\displaystyle n^2\).

(Later, when we consider electron spin, the total number of angular momentum states will be found to be \(\displaystyle 2n^2\), because each orbital angular momentum states is associated with two states of electron spin; spin up and spin down).

**91. **50

**93. **The maximum number of orbital angular momentum electron states in the nth shell of an atom is \(\displaystyle n^2\). Each of these states can be filled by a spin up and spin down electron. So, the maximum number of electron states in the nth shell is \(\displaystyle 2n^2\).

**95.** a., c., and e. are allowed; the others are not allowed.

b. \(\displaystyle l>n\) is not allowed.

d. \(\displaystyle 7>2(2l+1)\)

**97. **\(\displaystyle f=1.8×10^9Hz\)

**99.** The atomic numbers for Cu and Ag are \(\displaystyle Z=29\) and 47, respectively. The X-ray photon frequency for silver is greater than copper by the following factor:

\(\displaystyle (\frac{f_{Ag}}{f_{Cu}})^2=2.7\).

Therefore, the X-ray wavelength of Ag is about three times shorter than for copper.

**101. **a. 3.24;

b. \(\displaystyle n_i\) is not an integer. c. The wavelength must not be correct. Because \(\displaystyle n_i>2\), the assumption that the line was from the Balmer series is possible, but the wavelength of the light did not produce an integer value for \(\displaystyle n_i\). If the wavelength is correct, then the assumption that the gas is hydrogen is not correct; it might be sodium instead.