Chapter 4

Question 1

How many nanometers in a meter

Answer 1

1 nanometer - 10^-9 meters

1 meter - 10^9 nanometers

Question 2

What is the speed of light (c)

Answer 2

3.00x10^8 m/s

Question 3

What is electromagnetic radiation

Answer 3

• a form of energy that travels in waves that are produced when charged particles move or vibrate relative to each other
• exists in small increments- photons

Question 4

Electromagnetic spectrum

Answer 4

From low frequency, long wavelength to high frequency short wavelength:
Radio- Microwave- Infared- visible- UV- X-rays- Gamma rays

Question 5

Visible spectrum

Answer 5

The middle of the electromagnetic spectrum, a narrow range of radiation that our eyes can detect, we perceive it as visible light.

Question 6

Wavelength, Lambda (λ)

Answer 6

The distance from a point on one wave cycle to the same point on the next cycle. Typically measured in meters or nanometers.

Question 7

Frequency, nu (ν)

Answer 7

The number of waves that pass through a point in one second.

Question 8

What is 1 Hertz (Hz) equal to

Answer 8

1 wave/ second

Question 9

Three ways that 10,000 waves can be written

Answer 9

10,000 Hz, 10,000/ s, 10,000 s^-1

Question 10

How are wavelength and frequency related to eachother

Answer 10

inversely

• Wavelength decreases, frequency increases
• Frequency decreases, wavelength increases

Question 11

relationship of wavelength and frequency described mathematically

Answer 11

c=λν
Speed of light = Wavelength x Frequency
units: m/s = m x 1/s

Question 12

Energy of light depends on

Answer 12

Frequency and wavelength
longer wavelength, lower frequency-less oscillations thus lower energy
Shorter wavelength, higher frequency- more oscillations thus higher energy

Question 13

Energy of a photon (equation)

Answer 13

E=hν
Energy=Plank’s Constant x Frequency
J = J*s x 1/s

Question 14

Planks Constant

Answer 14

6.63x10^-34 J*s

Question 15

Energy of a photon in terms of wavelength

Answer 15

Energy of a photon: E= hv
v= c/λ
E= hc/λ

Question 16

Bohr Model

Answer 16

The electrons orbit the nucleus like planets orbit the sun when an electron absorbs light it jumps to a higher energy level. when it drops to a lower energy level it releases energy as light.
line spectra related to the light produced when electrons drop to lower levels

Question 17

Quantum Model

Answer 17

Describes electrons by:
-energy
-possible location
Main Ideas:
-the uncertainty principle 
-wave nature of electrons

Question 18

Heisenberg’s uncertainty principle

Answer 18

The principle deals with velocity, mass, and location of subatomic particles
A central idea: It is impossible to precisely know the exact velocity and location of a particle.

Question 19

Quantum mechanics

Answer 19

describes electrons in terms of their probable locations or their energies
(We describe them by the shape they occupy.)

Question 20

The wave nature of electrons

Answer 20

Tiny, fast moving particles also behave as waves

Question 21

Four rules of configuration of electrons within the atom.

Answer 21

1) Electrons occupy different energy levels
2) Each energy level contains one or more sublevels
3) Each sublevel contains one or more orbitals
4) Each orbital holds up to two electrons

Question 22

Principle quantum number, n

Answer 22

the id of dif levels that electrons occupy (n = 1, 2,3)

The lowest energy level (1) lies closest to the nucleus

Question 23

Electron capacity of levels of an electron

Answer 23

Level Electron Capacity
1 2
2 8
3 18
4 32

Question 24

the four common (sublevels) energy levels, in order

Answer 24

s, d, p, f

each sublevel can hold a set number of electrons

Question 25

Orbital

Answer 25

a region where electrons are most likely to be found

Question 26

Number of orbitals in each sublevel

Answer 26

s - 1
p - 3
d - 5
f - 7

Question 27

Level one sublevel(s), # of orbitals, and electron capacity

Answer 27

One sublevel (s), one orbital, capacity of two electrons

Question 28

Level two sublevel(s), # of orbitals, and electron capacity

Answer 28

Two sublevels (s, p), three orbitals, capacity of eight electrons

Question 29

Level three sublevel(s), # of orbitals, and electron capacity

Answer 29

Three sublevels (s, p, & d), five orbitals, capacity of eighteen electrons

Question 30

Level four sublevel(s), # of orbitals, and electron capacity

Answer 30

Four sublevels (s, p, d, & f), seven orbitals, capacity of 32 electrons

Question 31

Energy level growth pattern

Answer 31

With each new level is an additional sublevel, two orbitals, and four electrons

Question 32

Order of energy in sublevels

Answer 32

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d. 5p etc

Question 33

Which two sublevels form an atom’s valence

Answer 33

s & p

Question 34

Max # of electrons in the highest energy level of an atom, which sublevels do these occupy

Answer 34

8 electrons max and s & p sublevels

Question 35

Spin

Answer 35

The magnetic fields of electrons, oriented in oppisite directions

Question 36

Hund’s Rule

Answer 36

If orbitals of the same energy level are available, electrons singly occupy orbitals rather than paring together.

Question 37

Valence level

Answer 37

The highest occupied energy level

Question 38

Octet Rule

Answer 38

An atom is stabilized by having its highest occupied (valence) level filled.

Question 39

Isoelectronic

Answer 39

When ( ) have the same electron configuration

Question 40

Way of telling how many valence electrons an atom has

Answer 40

the number of valence electrons corresponds with the number of the 1A-8A columns (exa: column 3A, 3 valence electrons)