Q: A sodium lamp emits yellow light with a wavelength of $$589\ \mathrm{nm}. $$What is the frequency ($$\nu) of $$this light? (Speed of 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

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

Question 2

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

Accepted Answer

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

Question 3

Which phenomenon provided evidence that energy is quantized and not continuous?

Accepted Answer

The emission of light from hot objects (blackbody radiation)

Question 4

According to the Bohr model, what happens when an electron in a hydrogen atom transitions from $$n=3 to$$ $$n=2$$?

Accepted Answer

Energy is released and a photon is emitted.

Question 5

Which equation expresses the energy of a photon in terms of its frequency ($$
u) $$and Planck's constant ($$h$$)?

Accepted Answer

$$E = h 
u$$

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 statement about the Pauli Exclusion Principle is correct?

Accepted Answer

No two electrons in the same atom can have the same set of four quantum numbers.

Question 9

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

Accepted Answer

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

Question 10

Which orbital type is spherical in shape?

Accepted Answer

s orbital

Question 11

According to de Broglie's hypothesis, what is the wavelength ($$\lambda) of an $$electron with mass $$m$$ and velocity $$v$$?

Accepted Answer

$$\lambda = \frac{h}{mv}$$

Question 12

Which of the following best explains why the Bohr model fails for multi-electron atoms?

Accepted Answer

Electron-electron repulsion causes energy levels to split, so not all orbitals of the same principal quantum number are degenerate.

Question 13

Which rule states that the lowest energy is attained when the number of electrons with the same spin is maximized in degenerate orbitals?

Accepted Answer

Hund's Rule

Question 14

What is the total number of nodes in a $$4s$$ orbital?

Accepted Answer

3

Question 15

Which element has the electron configuration $$[Ar]\ 4s^1$\ 3d^5$ due to an anomaly in orbital filling?

Accepted Answer

Chromium (Cr)

Question 16

Which quantum number describes the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 17

If an electron in a hydrogen atom absorbs a photon and moves from $$n=2 to$$ $$n=4$$, what is the sign of $$\Delta E$$ for this process?

Accepted Answer

Positive

Question 18

Which of the following is true about the electron density in an $$ns$$ orbital as $$n$$ increases?

Accepted Answer

The electron density is more spread out and the probability of finding an electron farther from the nucleus increases.

Question 19

Which block of the periodic table corresponds to the filling of $$f$$ orbitals?

Accepted Answer

Inner transition elements

Question 20

Which principle states that it is impossible to know both the exact position and momentum of a particle simultaneously?

Accepted Answer

Heisenberg Uncertainty Principle

Electronic Structure of Atoms – General Chemistry Study Notes

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