Q: Which equation correctly expresses the energy change when an electron transitions from an initial state $$n_i to a $$final state $$n_f in a $$hydrogen atom?

$$\Delta E = -2.18 \times 10$$^{-18}$$ \left( \frac{1}{n_f^2$} - \frac{1}{n_i^2$} \right) J$$

Question 1

A sodium vapor lamp emits yellow light with a wavelength of 589 nm. What is the frequency of this light? (Speed of light, $$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$5.09 	imes 10$$^{14}$$ Hz

Question 2

Which of the following statements best describes the relationship between wavelength and frequency for electromagnetic waves?

Accepted Answer

Wavelength and frequency are inversely proportional.

Question 3

Calculate the energy of a single photon of light with a frequency of $$4.69 	imes 10$$^{14}$$ s$$^{-1}$$. (h = 6.626$$ 	imes $$10^{-34} J$$·s)

Accepted Answer

$$3.11 	imes 10$$^{-19}$$ J

Question 4

A laser pointer emits light at 528 nm. What is the energy gap ($$\Delta E) $$between the ground state and excited state in the laser material? ($$h = 6.626 	imes 10$$^{-34}$$ J·s, c = 3.00$$ 	imes $$10^8 m/s)$$

Accepted Answer

$$3.76 	imes 10$$^{-19}$$ J

Question 5

Which of the following transitions in a hydrogen atom would result in the emission of the highest energy photon?

Accepted Answer

From $$n=4 to$$ $$n=1$$

Question 6

Which equation correctly expresses the energy change when an electron transitions from an initial state $$n_i to a $$final state $$n_f in a $$hydrogen atom?

Accepted Answer

$$\Delta E = -2.18 	imes 10$$^{-18}$$ \left( \frac{1}{n_f^2$} - \frac{1}{n_i^2$} ight) J$$

Question 7

A radio station broadcasts at 89.3 MHz. What is the wavelength of this radiation? ($$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$3.36 m$$

Question 8

Which of the following best explains why the line spectrum of hydrogen contains only certain wavelengths?

Accepted Answer

Electrons in hydrogen can only occupy specific, quantized energy levels.

Question 9

According to the de Broglie hypothesis, what is the wavelength of an electron (mass $$9.11 	imes 10$$^{-31}$$ kg) moving at 5.97$$ 	imes $$10^6 m/s$$? ($$h = 6.626 	imes 10$$^{-34}$$ J·s)

Accepted Answer

$$1.22 	imes 10$$^{-10}$$ m

Question 10

Which set of quantum numbers is NOT allowed for an electron in an atom?

Accepted Answer

$$n=3,\ l=0,\ m_l=1,\ m_s=+\frac{1}{2}$$

Question 11

How many electrons can occupy the $$n=3$$ shell in an atom?

Accepted Answer

18

Question 12

Which principle states that no two electrons in an atom can have the same set of four quantum numbers?

Accepted Answer

Pauli exclusion principle

Question 13

Which of the following electron configurations represents a transition metal ion with a completely filled $$d-$$subshell?

Accepted Answer

[Ar] $$3d^{10}$$

Question 14

Which of the following ions is isoelectronic with neon ($$[Ne]$$)?

Accepted Answer

Mg$$^{2+}$$

Question 15

Which of the following best describes Hund’s Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 16

Which quantum number defines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 17

Which of the following transitions in a hydrogen atom would result in the absorption of energy?

Accepted Answer

From $$n=2 to$$ $$n=6$$

Question 18

What is the condensed (noble-gas) electron configuration for calcium (Ca)?

Accepted Answer

[Ar] $$4s^2$$

Question 19

Which of the following best describes the difference between core and valence electrons?

Accepted Answer

Valence electrons are in the highest energy level and participate in bonding; core electrons are in lower energy levels and do not.

Question 20

Which of the following is the correct set of quantum numbers for a 3p electron?

Accepted Answer

$$n=3,\ l=1,\ m_l=0,\ m_s=+\frac{1}{2}$$

Chapter 6: Electronic Structure of Atoms – Study Notes

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