Ch 5: Electrons in Atoms/Electrons

Question 1

What could Rutherford’s atomic model not explain?

Answer 1

The chemical properties of elements.

Question 2

What did Bohr propose about an electron?

Answer 2

It is found only in specific circular paths, or orbits, around the nucleus.

Question 3

What did Bohr note that atoms emit?

Answer 3

Light of specific colors and wavelengths.

Question 4

What did Bohr determine light came from?

Answer 4

Excited electrons when energy is lost.

Question 5

Electrons could only have certain _________ energies.

Answer 5

quantized

Question 6

What are these characteristics of:

1. Atoms only emit a few energies of light.
2. Energy can only have certain specific qualities.
3. Energy levels are clearly defined values and are not flexible.
4. If there were any random value, a continuous spectrum of light would be emitted.

Answer 6

Quantized energy

Question 7

What was Bohr correct about? What was Bohr incorrect about?

Answer 7

Correct: energy levels.
Incorrect: the orbits.

Question 8

The energy levels in an atom are not _______ ______. The higher energy levels are ______ ________.

Answer 8

equally spaced.

closer together.

Question 9

Who developed the Quantum Mechanical Model?

Answer 9

Erwin Schrödinger.

Question 10

What does the quantum mechanical model determine?

Answer 10

The allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus.

Question 11

Electrons in atoms behave like _____.

Answer 11

waves.

Question 12

Electrons: there is a fundamental ___________ about their behavior; cannot map path.

Answer 12

uncertainty

Question 13

Electrons: waves are ___________, but we can assign a location based on ___________.

Answer 13

delocalized

probability.

Question 14

Atomic orbitals: each energy sub level corresponds to an orbital of a different _____, which describes where the electron is likely to be _____.

Answer 14

shape

found.

Question 15

Atomic orbitals: the region where there is a ___ ______ of finding an electron is called an _______.

Answer 15

90% chance

orbital.

Question 16

Atomic orbitals: what are orbitals characterized by?

Answer 16

Energy levels and sub levels.

Question 17

What three rules tell how to find the electron configuration of atoms?

Answer 17

1. Aufbau principle
2. Pauli exclusion principle
3. Hund’s rule

Question 18

Some actual electron configurations differ from those assigned using the aufbau principle because ____-______ sub levels are not as stable as ______ sub levels. They are more stable than other ______________.

Answer 18

half-filled
filled
configurations.

Question 19

What are the 5 properties of waves?

Answer 19

1. speed
2. wavelength
3. frequency
4. energy
5. hertz

Question 20

The __________ and _________ of light are inversely proportional to each other.

Answer 20

wavelength

frequency

Question 21

What type of waves does the electromagnetic spectrum include?

Answer 21

Radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays.

Question 22

What is the electromagnetic spectrum?

Answer 22

The full range of electromagnetic energy (waves of electric and magnetic fields, oscillating at right angles to each other).

Question 23

What is the dual nature of light?

Answer 23

Light is made up of matter and waves.

Question 24

When atoms absorb energy, electrons move into ____ energy levels.
These electrons lose the energy by emitting _____ when they return to lower energy levels.

Answer 24

high

light

Question 25

According to the Aufbau principle, in the ______ _____, electrons have the lowest energy level possible.

Answer 25

ground state

Question 26

Each energy level () has a certain number of sub levels (, _, _, _).

Answer 26

n

s, p, d, f

Question 27

Each sub level has a certain number of orbitals (_, _, _, _).

Answer 27

1, 3, 5, 7

Question 28

Two electrons can share an orbital only if they have ________ _____.

Answer 28

opposite spins

Question 29

At the highest energy level, the electrons will ______ ___ to be ________ where possible. All ________ electrons will have the ____ spin.

Answer 29

spread out
unpaired
unpaired
same

Question 30

A _______ of energy in the form of _____ is emitted when the electron drops back to a lower energy level. This single step is known as __________ __________.

Answer 30

quantum
light
electronic transition

Question 31

The light emitted by an electron moving from a higher to a lower energy level has a _________ directly proportional to the ______ ______ of the electron.

Answer 31

frequency

energy change

Question 32

Classical mechanics adequately describes the motions of bodies much ______ than atoms, while quantum mechanics describes motions of _________ _________ and _____ as waves.

Answer 32

larger
subatomic particles
atoms

Question 33

Quantum mechanics is considered the _____ theory.

Classical mechanics is considered the _____ theory.

Answer 33

newer

older

Question 34

Planck discovered _____ _______ (E=hf).

Answer 34

light photons

Question 35

Einstein said: light has ____; it is ______ (E=mc^2).

Answer 35

mass

matter

Question 36

DeBroglie said: As the mass _________, the __________ decreases. Electrons behave like _____.

Answer 36

increases
wavelength
waves.