Q: Which equation describes the energy difference between two levels in the hydrogen atom according to the Bohr model?

$\Delta E = h\nu = E_{n_2} - E_{n_1}$

Question 1

Which of the following statements best describes electromagnetic (EM) radiation?

Accepted Answer

It consists of energy propagated by oscillating electric and magnetic fields that are perpendicular to each other and to the direction of propagation.

Question 2

A sodium vapor lamp emits light with a wavelength of $589	imes10^{-9}$ m. What is the frequency of this radiation? (Speed of light $c = 2.998	imes10^8$ m/s)

Accepted Answer

$5.09	imes10^{14}$ s^{-1}$

Question 3

Which phenomenon provided evidence that light behaves as both a wave and a particle?

Accepted Answer

Photoelectric effect

Question 4

According to Planck’s theory, the energy of a photon is given by $E = hv$. If the frequency of light is doubled, what happens to the energy of each photon?

Accepted Answer

It is doubled.

Question 5

Which statement about the photoelectric effect is correct?

Accepted Answer

Electrons are emitted only if the frequency of light is above a threshold value, regardless of intensity.

Question 6

Which equation describes the energy difference between two levels in the hydrogen atom according to the Bohr model?

Accepted Answer

$\Delta E = h
u = E_{n_2} - E_{n_1}$

Question 7

The Balmer series in the hydrogen spectrum corresponds to electronic transitions ending at which principal quantum number?

Accepted Answer

$n=2$

Question 8

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Azimuthal (angular momentum) quantum number ($l$)

Question 9

How many individual atomic orbitals are present in the $p$ subshell?

Accepted Answer

3

Question 10

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

Accepted Answer

$(n=3, l=3, m_l=0, m_s=+\frac{1}{2})$

Question 11

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

Accepted Answer

10

Question 12

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 13

According to Hund’s rule, when filling degenerate orbitals, electrons will:

Accepted Answer

Occupy orbitals singly with parallel spins before pairing.

Question 14

Which of the following is the correct ground-state electron configuration for tin ($Z=50$)?

Accepted Answer

$[Kr]4d^{10}5s^2 5p^2$

Question 15

What is the wavelength associated with an electron (mass $9.109	imes10^{-31}$ kg) moving at $2.998	imes10^7$ m/s? ($h = 6.626	imes10^{-34}$ J·s)

Accepted Answer

$2.42	imes10^{-11}$ m

Question 16

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

Accepted Answer

Magnetic quantum number ($m_l$)

Question 17

Which block of the periodic table corresponds to elements whose last electron enters a $d$ orbital?

Accepted Answer

d-block

Question 18

If an atom absorbs a photon and an electron transitions from $n=2$ to $n=5$, what is the sign of the energy change ($\Delta E$)?

Accepted Answer

Positive

Question 19

Which statement about the Heisenberg uncertainty principle is correct?

Accepted Answer

The product of the uncertainties in position and momentum is always greater than or equal to $\frac{h}{4\pi}$.

Question 20

Which of the following best explains why elements in the same group of the periodic table have similar chemical properties?

Accepted Answer

They have the same number of valence electrons.

Atomic Structure & Atomic Properties of Elements: Quantum Theory and Electron Configuration

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