Question 1

Which statement best describes the difference between the Rutherford and Bohr models of the atom?

Accepted Answer

The Rutherford model described electrons moving randomly in mostly empty space, while the Bohr model introduced quantized energy levels for electron orbits.

Question 2

According to Bohr’s model, what happens when an electron in a hydrogen atom jumps from a higher energy level to a lower energy level?

Accepted Answer

The electron loses energy and emits light as electromagnetic radiation.

Question 3

Which quantum number determines the primary energy level of an electron in an atom?

Accepted Answer

Principal quantum number ($$n)$$

Question 4

How many electrons can occupy the $$n=3$$ energy level in an atom?

Accepted Answer

18

Question 5

Which of the following electron configurations correctly represents the element nitrogen (atomic number 7)?

Accepted Answer

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

Question 6

Which orbital type has a 'double peanut' shape and first appears in the $$n=3$$ energy level?

Accepted Answer

$$d$$ orbital

Question 7

What is the maximum number of electrons that can occupy a single $$p$$ sublevel?

Accepted Answer

6

Question 8

Which statement about atomic orbitals is correct?

Accepted Answer

Orbitals within a specific sublevel (e.g., the three $$2p$$ orbitals) are equal in energy.

Question 9

Which electron configuration uses the noble gas shortcut for silver (Ag, atomic number 47)?

Accepted Answer

$$[Kr] 5s^1$ 4d$$^{10}$$

Question 10

If an electron absorbs energy and moves from $$n=2 to$$ $$n=4$$, what is the process called?

Accepted Answer

Excitation

Question 11

Which of the following best explains why energy levels get closer together as $$n$$ increases?

Accepted Answer

The energy difference between levels decreases as the electron moves farther from the nucleus.

Question 12

Which quantum number is associated with the shape of an orbital?

Accepted Answer

Azimuthal quantum number ($$l)$$

Question 13

How many $$d$$ orbitals are present in the $$n=3$$ energy level?

Accepted Answer

5

Question 14

Which element has the electron configuration $$1s^2$$ $$2s^2$$ $$2p^6$$ $$3s^2$$ $$3p^6$$ $$4s^2$$ $$3d^{10}$$ $$4p^6$$?

Accepted Answer

Krypton (Kr)

Question 15

What is the total number of orbitals in the $$n=2$$ energy level?

Accepted Answer

4

Question 16

Which of the following statements about electron transitions is correct?

Accepted Answer

Electrons absorb energy when moving to a higher energy level.

Question 17

Which orbital type first appears in the $$n=4$$ energy level?

Accepted Answer

$$f$$ orbital

Question 18

What is the electron configuration for tungsten (W, atomic number 74) using the noble gas shortcut?

Accepted Answer

$$[Xe] 6s^2$ 4f$$^{14}$$ 5d^5$

Question 19

Which of the following best describes the difference between an orbital and an energy level?

Accepted Answer

An energy level is defined by the principal quantum number $$n$$, while an orbital is a specific region within an energy level defined by quantum numbers $$n$$, $$l$$, and $$m_l.$$

Atomic Structure, Electron Configuration, and Atomic Orbitals: Study Notes

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