Chapter 4 Quiz

Question 1

How is light as a wave?

Answer 1

A type of electromagnetic radiation, along with X-rays, ultraviolet and infrared light, microwaves, and radio waves.

Question 2

Waves have a _______ ______ and can be measured by ________ & _________.

Answer 2

repetitive nature; wavelength; frequency

Question 3

What are the units of wavelength?

Answer 3

cm or nm

Question 4

What are the units for frequency?

Answer 4

Waves/sec or hertz (Hz)

Question 5

How are frequency and wavelength related to each other?

Answer 5

c=wavelength x frequency

Question 6

What is c

Answer 6

c=speed of light or 3.00 x 10^8 m/s

Question 7

How is light as a particle?

Answer 7

By the photoelectric effect, when the emissions of electrons from metal when light shines on it
Light has to have a minimum frequency for this to occur

Question 8

What is Planck’s theory and constant?

Answer 8

• Objects do not emit electromagnetic energy constantly
• Instead energy is emitted in small specific packets called quanta

Question 9

What is a quantum of energy?

Answer 9

The minimum amount of energy that can be lost or gained by an atom

Question 10

E=hv

Answer 10

Equation showing relationship between quantum of energy and frequency

Question 11

Who expanded on Planck’s theory and how?

Answer 11

Einstein expanded on Planck’s theory by introducing that light has a dual wave-particle nature.

Question 12

Light can be thought of as …

Answer 12

a stream of particles

Question 13

What is a photon?

Answer 13

A particle of electromagnetic radiation w/no mass and carrying a quantum of energy

Question 14

What is ground state?

Answer 14

Lowest energy state of an atom

Question 15

What is excited state

Answer 15

An atom has a higher potential energy than in its ground state

Question 16

What happens when an electron returns to ground state?

Answer 16

It gives off energy in form of electromagnetic radiation

Question 17

What did specific frequencies of light and not a continuous spectrum show scientists?

Answer 17

Electrons exist in specific energy states

Question 18

What did the Bohr Model propose?

Answer 18

A hydrogen-atom model that linked the atom’s electron to photon emission

Question 19

According to the Bohr model…

Answer 19

the electron can circle the nucleus only in allowed paths or orbits​

Question 20

Electron and atoms are in the lowest energy state when the electron is…

Answer 20

in the orbit closest to the nucleus​

Question 21

Energy of the electron is higher when the electron is in orbit…

Answer 21

successively farther from the nucleus

Question 22

What were the issues with Bohr’s Model?

Answer 22

• The model does not explain atoms with more than one electron
• Does not explain the chemical behavior of atoms

Question 23

Behavior of electrons is similar to…

Answer 23

the behavior of waves

Question 24

When can electron waves exist?

Answer 24

Only at certain frequencies, which correspond to specific energies

Question 25

How are electrons detected?

Answer 25

By their interaction with photons, but the photons knock the electron off its course

Question 26

What is the Heisenberg Principle?

Answer 26

It is impossible to determine simultaneously both the position and velocity (speed) of an electron

Question 27

What did the Schrodinger Wave Equation develop?

Answer 27

an equation that treated electrons in atoms as waves and quantization of electron energies was an outcome of the equation.

Question 28

What is the quantum theory?

Answer 28

mathematically describes the wave properties of electrons and other very small particles. ​

Question 29

What are orbitals?

Answer 29

3D region around the nucleus that indicates the probable location of an electron.​

Question 30

What are the conclusions and beginnings of the Quantum Atomic Theory?

Answer 30

• Wave functions allow us to determine the probability of finding an electron at a given place around the nucleus
• Electrons don’t travel in neat orbits like Bohr proposed. They exist in certain regions called orbitals

Question 31

What are quantum numbers?

Answer 31

The properties of atomic orbitals and the properties of electrons in orbitals?

Question 32

What are the principals of Quantum Number?

Answer 32

• Symbolized by n
• Indicates the main energy level occupied by the electron
• As n increases the electron’s energy and its distance from the nucleus increases

Question 33

Can more than one electron have the same n value? Are they in the same shell?

Answer 33

Yes; yes

Question 34

The total number of orbitals in each shell or energy level is…

Answer 34

n^2

Question 35

What are electron configurations?

Answer 35

The arrangement of electrons in an atom

Question 36

Does each element have a unique electron configuration?

Answer 36

Yes

Question 37

What is ground -state electron configuration?

Answer 37

The lowest energy arrangement of the electrons for an element

Question 38

What is Aufbau Principle?

Answer 38

Electrons fill the lowest energy orbitals first

Question 39

What is Orbital Order?

Answer 39

1s,2s,2p,3s,3p,4s,3d,,4p,5s,4d,5p,6s,4f,5d,6p,7s,7p

Question 40

S orbital has a max subscript of…

Answer 40

2

Question 41

P orbital has a max subscript of…

Answer 41

6

Question 42

D orbital has a max subscript of…

Answer 42

10

Question 43

F orbital has a max subscript of…

Answer 43

14

Question 44

What is the Pauli Exclusion Principle?

Answer 44

Each orbital can hold TWO electrons with opposite spins.

Question 45

What is Hund’s Rule?

Answer 45

Within a sublevel, place one electron per orbital before pairing them.

Question 46

What is Noble Gas Configuration?

Answer 46

A shorthand method of writing the electron configuration?

Question 47

What is Planck’s constant?

Answer 47

6.626 x 10^-31