Quiz Chapter 5

Question 1

What was incorrect about Bohr’s model of the atom?

Answer 1

Electrons orbit the nucleus in distinct paths.

Question 2

WHen we sketch an electron orbital as a cloud, the probability that an electron associated with that orbital will be found outside of the cloud’s boundary is..

Answer 2

10%

Question 3

Give the correct numbers for your answers.

For atomic orbitals, principal energy level 3 has X sublevels, X atomic orbitals, and can be occupied by a maximum of X electrons.

Answer 3

3 sublevels,
9 atomic orbitals,
18 electrons.

Question 4

Name the sublevels contained in principal energy level 3.

Answer 4

3s, 3p, and 3d.

Question 5

How many electrons can be contained in the 4d sublevel?

Answer 5

10

Question 6

Arrange these orbitals in order of increasing energy (lowest energy on the bottom to highest energy on top). You may use an Aufbau diagram.
3s 4s 3d 4p 4s 4f

Answer 6

4f, 4p, 3d, 4s, 3s

Question 7

According to the Hund’s rule, which of the following would be the correct configuation for 3 electrons in the 2p orbitals?|
⬆⬇ ⬆
or ⬆ ⬆ ⬆

Answer 7

⬆ ⬆ ⬆

Question 8

The 4s orbital has lower energy than the 3d orbital. Why is the ground state electron configuration of chromium 1s22s22p63s23p63d54s1

Answer 8

Because half-filled orbitals are exceptionally stable.

Question 9

The atomic emission spectrum of an element is caused by _________________.

Answer 9

excited electrons in the atom falling back to lower energy orbitals

Question 10

Complete the following formula:
speed of light =

Answer 10

wavelength x frequency

Question 11

What is the wavelength of light that has a frequency of 6.24x1014 hertz?

Answer 11

4.81x10^-7

Question 12

When an element is heated, electrons are excited from the 2s to the 3s atomic orbitals. When those electrons fall back to their ground state, the element emits green light with a wavelength of 555 nm. What is the energy difference between the 2s and 3s orbitals? (Use h = 6.626 x 10-34 J*s)

Answer 12

3.58 x 10^-19