Q: A laser used in eye surgery emits light with a wavelength of $640.0\ \text{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 \times 10^8\ \text{m/s}$)

$4.688 \times 10^{14}\ \text{s}^{-1}$

Question 1

Which of the following statements best explains why the frequency of electromagnetic radiation increases as the wavelength decreases, as shown in the first image?

Accepted Answer

Because the number of wave cycles passing a point per second increases as the wavelength gets shorter.

Question 2

A laser used in eye surgery emits light with a wavelength of $640.0\ 	ext{nm}$. What is the frequency of this light? (Speed of light $c = 3.00 	imes 10^8\ 	ext{m/s}$)

Accepted Answer

$4.688 	imes 10^{14}\ 	ext{s}^{-1}$

Question 3

Which region of the electromagnetic spectrum has the shortest wavelength and the highest frequency?

Accepted Answer

Gamma rays

Question 4

According to the concept of quantization, as illustrated by the person walking up steps, which statement is correct?

Accepted Answer

Energy increases in discrete, fixed amounts as the person moves up each step.

Question 5

Which phenomenon could NOT be explained by the classical wave model of light, leading to the development of quantum theory?

Accepted Answer

Photoelectric effect

Question 6

The energy of a photon is given by $E = hv$. If the frequency of light is doubled, what happens to the energy of the photon?

Accepted Answer

The energy is doubled.

Question 7

Which equation allows you to calculate the wavelength of light emitted during an electronic transition in hydrogen?

Accepted Answer

$\frac{1}{\lambda} = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)$

Question 8

In the Bohr model, what does a negative value for $\Delta E$ indicate about the electron transition?

Accepted Answer

A photon is emitted and the electron moves to a lower energy level.

Question 9

Which quantum number determines the shape of an orbital?

Accepted Answer

Angular momentum quantum number ($l$)

Question 10

How many possible values of $m_l$ are there for a $d$ orbital?

Accepted Answer

5

Question 11

Which electron configuration represents the ground state of sodium (Na)?

Accepted Answer

$1s^2 2s^2 2p^6 3s^1$

Question 12

According to Hund’s Rule, how are electrons arranged in degenerate orbitals?

Accepted Answer

Electrons fill each orbital singly with parallel spins before pairing.

Question 13

What is the condensed electron configuration for potassium (K)?

Accepted Answer

$[Ar]4s^1$

Question 14

Which element has the electron configuration $[Ar]4s^2 3d^5$?

Accepted Answer

Manganese (Mn)

Question 15

How many unpaired electrons are present in a phosphorus (P) atom?

Accepted Answer

3

Question 16

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

Accepted Answer

Magnetic quantum number ($m_l$)

Question 17

Which of the following is a correct electron configuration for the chloride ion ($	ext{Cl}^-$)?

Accepted Answer

$1s^2 2s^2 2p^6 3s^2 3p^6$

Question 18

Which of the following elements has a half-filled $d$ subshell, making its electron configuration anomalous?

Accepted Answer

Chromium (Cr)

Question 19

Which quantum number(s) must be different for two electrons in the same atom according to the Pauli Exclusion Principle?

Accepted Answer

At least one of the four quantum numbers ($n$, $l$, $m_l$, $m_s$)

Chapter 6: Electronic Structure of Atoms – Mini-Textbook Study Notes

Study Guide - Practice Questions

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