Q: A photon of wavelength $500\ \mathrm{nm}$ is absorbed by an atom. What is the energy of this photon in joules? (Use $h=6.626\times10^{-34}\ \mathrm{J\cdot s}$ and $c=3.00\times10^8\ \mathrm{m/s}$)

$3.98\times10^{-19}\ \mathrm{J}$

Question 1

Which of the following statements best describes the difference between emission and absorption spectra in atomic transitions?

Accepted Answer

Emission and absorption involve the same energy jumps, but in opposite directions: emission is from higher to lower energy, absorption is from lower to higher energy.

Question 2

A hydrogen atom undergoes a transition from $n=3$ to $n=2$. Which type of spectrum is produced and what is the general region of the electromagnetic spectrum for this transition?

Accepted Answer

Emission spectrum; visible region

Question 3

Which quantum numbers are needed to uniquely identify an electron in an atom?

Accepted Answer

Principal quantum number $n$, azimuthal quantum number $l$, magnetic quantum number $m_l$, and spin quantum number $m_s$

Question 4

How many possible $d$ orbitals are there in the $n=3$ shell?

Accepted Answer

5

Question 5

Which set of quantum numbers is valid for an electron in a $3p$ orbital?

Accepted Answer

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

Question 6

Which of the following best explains why the $2p$ orbitals have three possible orientations?

Accepted Answer

Because $l=1$ for $p$ orbitals, and $m_l$ can be $-1, 0, +1$

Question 7

Which electron configuration correctly represents the element oxygen ($Z=8$)?

Accepted Answer

$1s^2 2s^2 2p^4$

Question 8

A photon of wavelength $500\ \mathrm{nm}$ is absorbed by an atom. What is the energy of this photon in joules? (Use $h=6.626	imes10^{-34}\ \mathrm{J\cdot s}$ and $c=3.00	imes10^8\ \mathrm{m/s}$)

Accepted Answer

$3.98	imes10^{-19}\ \mathrm{J}$

Question 9

Which of the following transitions in the hydrogen atom emits the highest energy photon?

Accepted Answer

$n=2$ to $n=1$

Question 10

Which principle explains why electrons fill the lowest available energy orbitals first?

Accepted Answer

Aufbau Principle

Question 11

If an atom has electrons in the $n=2$, $l=1$ subshell, how many electrons can occupy this subshell?

Accepted Answer

6

Question 12

Which quantum number determines the shape of an orbital?

Accepted Answer

Azimuthal quantum number $l$

Question 13

What is the maximum number of electrons that can occupy the $3d$ subshell?

Accepted Answer

10

Question 14

Which of the following elements has the electron configuration $1s^2 2s^2 2p^6 3s^2$?

Accepted Answer

Magnesium ($Z=12$)

Question 15

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

Accepted Answer

Pauli Exclusion Principle

Question 16

A sodium atom ($Z=11$) emits a photon as an electron transitions from the $3p$ to the $3s$ orbital. Which statement is true about the energy of the emitted photon?

Accepted Answer

The photon energy equals the difference in energy between the $3p$ and $3s$ orbitals.

Question 17

Which of the following best describes the electromagnetic spectrum?

Accepted Answer

It includes all wavelengths of electromagnetic radiation, from radio waves to gamma rays.

Question 18

Which orbital type has a spherical shape?

Accepted Answer

$s$ orbital

Question 19

If an electron has quantum numbers $n=4$, $l=3$, $m_l=2$, $m_s=+\frac{1}{2}$, which type of orbital is it in?

Accepted Answer

$4f$

Light, Energy, and Atomic Orbitals: Quantum Concepts in General Chemistry

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