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

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

Q: According to de Broglie's hypothesis, what is the wavelength ($$\lambda) of an $$electron with mass $$9.11 \times 10$$^{-31}$$\ \mathrm{kg}$$ moving at $$2.00 \times 10^6$\ \mathrm{m/s}$$? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s})$$

$$3.63 \times 10$$^{-10}$$\ \mathrm{m}$$

Question 1

Which of the following statements best describes the relationship between wavelength ($$\lambda) $$and frequency ($$
u) $$for electromagnetic radiation traveling at the speed of light ($$c$$)?

Accepted Answer

As wavelength increases, frequency decreases, since $$c = \lambda 
u.$$

Question 2

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

Accepted Answer

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

Question 3

Which phenomenon cannot be explained by the classical wave model of light and led to the development of quantum theory?

Accepted Answer

The photoelectric effect

Question 4

According to Planck's theory, energy is quantized and can be described by the equation $$E = h
u. $$What does the constant $$h$$ represent?

Accepted Answer

Planck's constant

Question 5

Which statement about the Bohr model of the atom is correct?

Accepted Answer

Electrons exist only in certain discrete energy levels and emit or absorb energy when transitioning between them.

Question 6

An electron in a hydrogen atom transitions from $$n=4 to$$ $$n=2. $$What is true about the energy change ($$\Delta E) $$and the photon involved?

Accepted Answer

$$\Delta E is $$negative; a photon is emitted.

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 8

How many possible values of the magnetic quantum number ($$m_l) $$are there for a $$d$$ orbital?

Accepted Answer

5

Question 9

Which of the following electron configurations represents a transition metal?

Accepted Answer

[Ar] $$4s^2$$ $$3d^5$$

Question 10

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

Accepted Answer

Pauli Exclusion Principle

Question 11

What is the condensed electron configuration for selenium (Se, atomic number 34)?

Accepted Answer

[Ar] $$4s^2$$ $$3d^{10}$$ $$4p^4$$

Question 12

Which orbital type has a spherical shape and only one orientation?

Accepted Answer

s orbital

Question 13

According to de Broglie's hypothesis, what is the wavelength ($$\lambda) of an $$electron with mass $$9.11 	imes 10$$^{-31}$$\ \mathrm{kg}$$ moving at $$2.00 	imes 10^6$\ \mathrm{m/s}$$? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s})$$

Accepted Answer

$$3.63 	imes 10$$^{-10}$$\ \mathrm{m}$$

Question 14

Which of the following best describes Hund's Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly with parallel spins before pairing.

Question 15

What is the maximum number of electrons that can occupy the $$n=3$$ shell?

Accepted Answer

18

Question 16

Which element has the electron configuration $$[Xe] 6s^2$ 4f$$^{14}$$ 5d$$^{10}$$ 6p^2$?

Accepted Answer

Lead (Pb)

Question 17

Which quantum number is responsible for the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 18

Why does chromium have the electron configuration $$[Ar] 4s^1$ 3d^5$ instead of $$[Ar] $$4s^2$$ $$3d^4$$?

Accepted Answer

Because half-filled d subshells are more stable due to exchange energy.

Question 19

Which statement about the energy of orbitals in many-electron atoms is correct?

Accepted Answer

Orbitals in the same subshell are degenerate, but subshells of the same shell are not.

Electronic Structure of Atoms: Wave Nature, Quantum Theory, and Electron Configuration

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