$$\Delta E = -2.18 \times 10$$^{-18}$$ \left( \dfrac{1}{n_f^2$} - \dfrac{1}{n_i^2$} \right) \text{J}$$

Question 1

Which equation correctly relates the energy of a photon to its wavelength?

Accepted Answer

$$E = \dfrac{hc}{\lambda}$$

Question 2

A hydrogen atom electron transitions from $$n=4 to$$ $$n=2. $$Which type of electromagnetic radiation is emitted?

Accepted Answer

Visible

Question 3

Which of the following best describes the Heisenberg Uncertainty Principle?

Accepted Answer

It is impossible to know both the exact position and momentum of an electron at the same time.

Question 4

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 5

What is the maximum number of electrons that can occupy all the $$p$$ orbitals in a single energy level?

Accepted Answer

6

Question 6

Which statement best explains why the Bohr model fails for atoms other than hydrogen?

Accepted Answer

It cannot account for electron-electron interactions and wave properties of electrons.

Question 7

A photon of wavelength $$486 nm is $$emitted from a hydrogen atom. What energy transition does this correspond to?

Accepted Answer

$$n=4 to$$ $$n=2$$

Question 8

Which orbital is spherical in shape?

Accepted Answer

$$s$$ orbital

Question 9

How many $$d$$ orbitals are present in a single principal energy level (starting from $$n=3$$)?

Accepted Answer

5

Question 10

Which of the following best describes an atomic orbital?

Accepted Answer

A region in space where there is a high probability of finding an electron.

Question 11

Which equation is used to calculate the energy difference between two energy levels in a hydrogen atom?

Accepted Answer

$$\Delta E = -2.18 	imes 10$$^{-18}$$ \left( \dfrac{1}{n_f^2$} - \dfrac{1}{n_i^2$} ight) 	ext{J}$$

Question 12

Which process is responsible for the emission lines observed in the hydrogen spectrum?

Accepted Answer

Electrons falling from higher to lower energy levels, emitting photons.

Question 13

Which of the following is a real-world application of fluorescence, as seen in the image of depression glass?

Accepted Answer

Detecting counterfeit currency using UV light.

Question 14

Which quantum number(s) are needed to uniquely describe an electron in an atom?

Accepted Answer

Principal ($$n$$), angular momentum ($$l$$), magnetic ($$m_l$$), and spin ($$m_s)$$

Question 15

Which statement best describes the difference between the Bohr model and the quantum mechanical model of the atom?

Accepted Answer

The Bohr model uses fixed orbits, while the quantum mechanical model uses probability distributions for electron locations.

Question 16

If a photon has a frequency of $$6.17 	imes 10$$^{14}$$ Hz, what is its energy? (h = 6.626$$ 	imes $$10^{-34} J$$·s)

Accepted Answer

$$4.09 	imes 10$$^{-19}$$ J

Question 17

Which of the following transitions in a hydrogen atom would emit the highest energy photon?

Accepted Answer

$$n=2 to$$ $$n=1$$

Question 18

Which property of light is directly proportional to its energy?

Accepted Answer

Frequency

Question 19

Which scientist mathematically related the wave and particle properties of electrons, leading to the quantum mechanical model?

Accepted Answer

Schrödinger

Question 20

How many electrons can exist in the $$n=3$$ shell of a magnesium ion ($$	ext{Mg}^{2+}$$)?

Accepted Answer

0

Quantum Mechanics, Electron Configurations, and Atomic Models

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