Unit 2 Test Review

Question 1

Describe the process in which an atom emits visible light.

Answer 1

1. Electron absorbs energy
2. Moves from ground state–> excited state
3. Electron then moves back down
4. On the way, releases energy in form of light

Question 2

What is the wave-particle duality principle?

Answer 2

The wave-particle duality states that matter can act like a particle and a wave.

Question 3

Hertz

Answer 3

showed that energy can replace electrons (photoelectric effect)

Question 4

Planck

Answer 4

energy comes in small packets (quantum)

Question 5

Einstein

Answer 5

energy is beams of massless quanta (photon)

Question 6

How is energy produced using the photoelectric effect?

Answer 6

1. Light strikes certain metals, atoms may loose electron
2. Electron is made to move through a circuit, creating electricity
3. Higher energy, higher intensity light, create more power

Question 7

Wavelength

Answer 7

Shortest - Blue/Violet
Longest - Red light

Question 8

Frequency

Answer 8

Highest - Blue/Violet
Lowest- Red

Question 9

Photon Energy

Answer 9

Highest - Violet
Lowest - Red

Question 10

h

Answer 10

Plank’s constant

Question 11

What is the value of Plank’s constant (h)?

Answer 11

6.626 * 10^-34

Question 12

v =

Answer 12

frequency (Hz)

Question 13

c =

Answer 13

Speed of light

Question 14

Speed of Light value?

Answer 14

3 * 10^8

Question 15

λ =

Answer 15

Wavelength (nm)

Question 16

Nanometers

Answer 16

1e-9

Question 17

λ = c/v

Answer 17

Find wavelength

Question 18

E = hv

Answer 18

Find energy of a wave (with frequency)

Question 19

E = hc/λ

Answer 19

Find energy of wave (no frequency, with wavelength)

Question 20

How should electron orbital notations show Pauli’s exclusion principle and Hund’s rule?
Give an example of a configuration that violates these rules.

Answer 20

For Hund’s rule, keep electrons unpaired until needed to be paired. For Pauli Exclusion, paired electrons must have different spins.

Question 21

What do quantum numbers do?

Answer 21

Describe the regions electrons are most likely to be found in.

Question 22

What do the “1” and the “s” in 1s2 mean?

Answer 22

The 1 describes the the size of the region, and s describes shape of region.

Question 23

What is a positively charged Ion?

Answer 23

Cation

Question 24

What is a negatively charged Ion?

Answer 24

Anion

Question 25

What are horizontal sections of the periodic table called?

Answer 25

Rows/Periods

Question 26

What are vertical sections of the periodic table called?

Answer 26

Columns/Families/Groups

Question 27

What is ionization energy?

Answer 27

the energy required to remove an electron from it's atom

Question 28

What is the periodic trend for IE?

Answer 28

Increases from left to right, and decreases from top to bottom.

Question 29

What element has the highest IE?

Answer 29

Helium (He)

Question 30

What is electronegativity?

Answer 30

The ability to attract electrons in a compound.

Question 31

Period trend for electronegativity?

Answer 31

Increases from left to right, and decreases from top to bottom

Question 32

What element has the highest electronegativity

Answer 32

Fluorine (F) (Not noble gases; bond rarely)

Question 33

What is the atomic radius?

Answer 33

The size of one atom of an element

Question 34

What is the periodic trend for atomic radius?

Answer 34

Decreases from left to right, and increases from top to bottom

Question 35

Which element has the highest atomic radius?

Answer 35

Francium (Fr)

Question 36

What are the values on top of the periodic table called?

Answer 36

Ion Charge