Q: A sodium street 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}$$\ \mathrm{Hz}$$

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

$$c = \lambda 
u$$

Question 2

A sodium street 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 could NOT be explained by the classical wave theory of light, but was explained by the quantum theory?

Accepted Answer

The photoelectric effect

Question 4

According to Planck’s theory, the energy of a photon is given by which equation?

Accepted Answer

$$E = h 
u$$

Question 5

Which of the following best describes the Bohr model’s explanation for the emission of light by hydrogen atoms?

Accepted Answer

Electrons emit photons when they transition from higher to lower energy levels.

Question 6

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 7

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

Accepted Answer

5

Question 8

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

Accepted Answer

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

Question 9

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 10

Which of the following electron configurations represents a violation of Hund’s Rule?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^4$$ with two paired electrons in one $$2p$$ orbital and the other $$2p$$ orbitals empty

Question 11

Which of the following elements has the ground-state electron configuration $$[\mathrm{Ar}]\ 4s^2$\ 3d^5$?

Accepted Answer

Chromium (Cr)

Question 12

Which orbital will fill first according to the Aufbau principle: $$4s or$$ $$3d$$?

Accepted Answer

$$4s$$

Question 13

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

Accepted Answer

18

Question 14

Which of the following best describes the Heisenberg Uncertainty Principle?

Accepted Answer

It is impossible to know both the exact position and momentum of a particle simultaneously.

Question 15

Which of the following is a correct condensed electron configuration for calcium (Ca, atomic number 20)?

Accepted Answer

$$[\mathrm{Ar}]\ 4s^2$

Question 16

Which quantum number is associated with the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 17

How many electrons can occupy all the $$p$$ orbitals in a single energy level?

Accepted Answer

6

Question 18

Which of the following statements about the $$2s$$ and $$2p$$ orbitals in a hydrogen atom is correct?

Accepted Answer

They have the same energy.

Question 19

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

Accepted Answer

Core electrons are in filled inner shells; valence electrons are in the outermost shell.

Electronic Structure of Atoms: Quantum Mechanics and Atomic Orbitals

Guida di studio - Domande di pratica

Study guide - Flashcard