Q: A sodium lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency ($$v) of $$this radiation? ($$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$5.09 \times 10$$^{14}$$\ \mathrm{Hz}$$

Q: A laser emits light with a frequency of $$4.69 \times 10$$^{14}$$\ \mathrm{s}^{-1}. $$What is the energy of one photon of this radiation? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s})$$

$$3.11 \times 10$$^{-19}$$\ \mathrm{J}$$

Q: What is the wavelength ($$\lambda) of an $$electron moving at $$2.65 \times 10^6$\ \mathrm{m/s}$$? (Mass of electron $$= 9.11 \times 10$$^{-31}$$\ \mathrm{kg}$$, $$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s})$$

$$2.73 \times 10$$^{-10}$$\ \mathrm{m}$$

Q: A photon with a wavelength of $$400\ \mathrm{nm} is $$absorbed by a hydrogen atom. What is the energy of this photon? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$4.97 \times 10$$^{-19}$$\ \mathrm{J}$$

Question 1

Which of the following statements best describes the relationship between the wavelength ($$\lambda) $$and frequency ($$v) of $$electromagnetic radiation?

Accepted Answer

They are inversely proportional; as wavelength increases, frequency decreases.

Question 2

A sodium lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency ($$v) of $$this radiation? ($$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

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

Question 3

Which equation correctly relates the energy of a photon ($$E) to $$its frequency ($$v$$)?

Accepted Answer

$$E = hv$$

Question 4

A laser emits light with a frequency of $$4.69 	imes 10$$^{14}$$\ \mathrm{s}^{-1}. $$What is the energy of one photon of this radiation? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s})$$

Accepted Answer

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

Question 5

According to the Bohr model, what happens when an electron in a hydrogen atom transitions from $$n=4 to$$ $$n=2$$?

Accepted Answer

A photon is emitted and the atom loses energy.

Question 6

Which of the following quantum number sets is NOT allowed for an electron in an atom?

Accepted Answer

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

Question 7

What is the wavelength ($$\lambda) of an $$electron moving at $$2.65 	imes 10^6$\ \mathrm{m/s}$$? (Mass of electron $$= 9.11 	imes 10$$^{-31}$$\ \mathrm{kg}$$, $$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s})$$

Accepted Answer

$$2.73 	imes 10$$^{-10}$$\ \mathrm{m}$$

Question 8

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 9

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

Accepted Answer

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

Question 10

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 11

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

Accepted Answer

18

Question 12

Which of the following best describes the difference between core and valence electrons in a chlorine atom ($$Z=17$$)?

Accepted Answer

Core electrons are in lower energy levels and do not participate in bonding, while valence electrons are in the highest energy level and participate in bonding.

Question 13

Which of the following ions is isoelectronic with $$\mathrm{Ar}$$?

Accepted Answer

$$\mathrm{K}^+$$

Question 14

Which quantum number defines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 15

A photon with a wavelength of $$400\ \mathrm{nm} is $$absorbed by a hydrogen atom. What is the energy of this photon? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$4.97 	imes 10$$^{-19}$$\ \mathrm{J}$$

Question 16

Which of the following best explains why the $$d-$$block elements often have anomalous electron configurations (such as $$\mathrm{Cu}$$: $$[Ar]\ 4s^1$\ 3d$$^{10}$$)?

Accepted Answer

Half-filled and fully filled $$d-$$subshells are particularly stable due to electron exchange energy.

Question 17

Which of the following transitions in a hydrogen atom corresponds to the absorption of energy?

Accepted Answer

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

Question 18

What is the maximum number of electrons that can have the quantum numbers $$n=4$$, $$l=2 in an $$atom?

Accepted Answer

10

Question 19

Which rule states that electrons fill degenerate orbitals singly before pairing up?

Accepted Answer

Hund's rule

Chapter 6: Electronic Structure of Atoms – Study Notes

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