Chapter 5 Study Guide
In your textbook, read about the wave nature of light.
Study your notes, charts, tables, and problems that we have completed in class.
Review information in your Science Workbook
Use the following terms below once to complete the passage.
Amplitude Energy Frequency Hertz
Light Wave Wavelength Speed
Electromagnetic radiation is a kind of (1) ___ Energy __________ that behaves like a(n) (2)
_________ Wave _____________ as it travels through space. (3) ____ Light ________ is one type of electromagnetic radiation. Other examples include x-rays, radio waves and microwaves.
All waves can be characteriszed by their wavelength, frequency and (4)
_______ Speed ______________. The shortest distance between equivalent points on a continuous wave is called a(n) (5) ______ Wavelength _____. The height of a wave from the origin to a crest or from the origin to the trough is the (6) ____ Amplitude ____. (7) _____ Frequency _____ is the number of waves that pass a given point in one second. The SI unit for frequency is the (8)
______ Hertz ____, which is equivalent to one waver per second.
Use the following figure to answer questions 9-10
4 8
1
3 5 7 9
2 6
9. Which number(s) represents one wavelength? _ any of the following: 2-6, 4-8, 1-5, 5-9 __
10. Which number(s) represent the amplitude? __ any of the following: 1-2, 3-4, 4-5, 6-5, ect.
_
11. Circle each of the following things that helped scientist discover the location of the
electrons. There may be more than one correct answer. a.
Different elements have different emission spectrums. b.
deBroglie equation predicted that all moving particles have wavelike characteristics. c.
The Heisenberg Uncertainty Principle d.
Schrödinger’s Wave equation
12. The minimum amount of energy that can be gained or lost by an atom is called
_____ Quantum ____________.
13. What was the major contribution to the understanding of the atom:
Einstein: proposed that light has a dual nature (particle and wave). Beam of light
Planck: determined that matter gains or loses energy in small amounts called quantum.
made of bundles of energy called photons. Photons with energy above the threshold will cause the photoelectric effect.

DeBroglie: proposed an idea that accounted for fixed energy levels. Everything could have a duality nature (matter could act like waves and waves could act like mater)
Bohr: hydrogen atom had certain allowable energy states the lowest energy state is called ground state. Quantum numbers assigned to energy levels.
Schrodinger: created the quantum mechanical model of the atom stating that electrons traveled like waves.
Heisenberg: determined that it is impossible to know where precisely both the velocity and position of a particle are at the same time. Assigned fixed pathway for electrons around the nucleus.
14. Define: a.
Quantum: The minimum amount of energy that can be gained or lost by an atom b.
Photon: A massless particle that carries a quantum of energy--Light is made up of these.
c.
Quantum Mechanical Model: Similar to the Bohr model in that it limits an electron’s energy to a certain value, however unlike Bohr’s model the quantum mechanical model makes no attempts to describe the electrons path around the nucleus. In other words electrons can be found in specific energy levels, but where they are within those energy levels is all based off of probability and there is no way to say exactly where they are.
Use the following figure to answer questions 15- 18
A
B
B
C
D
15. Which wave has the highest frequency? D
16. Which wave has the lowest frequency? A
17. Which wave has the longest wavelength? A
18. Which wave has the shortest wavelength? D
19. What is the maximum number of electrons that the each energy level can hold?
1=2e, 2=8e, 3=18e, 4=32e, 5=32e, 6=18e, 7=8e

20. How many orbitals are in each of the following sublevels: s / p / d / f
S=1 orbitals, p=3 orbitals, d=5 orbitals, f=7 orbitals
21. What is the role of a proton, neutron, and electron in the atom?
Protons are the “DNA” of the atom, they make the identity of the atom
Neutrons add to the protons to get the mass of the atom, they also help keep the atom together .
Electrons cause the atom to react and behave the way it does
22. What is Planck’s constant? h=6.626x10
-34
j*s
23. What is the speed of light?
C=3.00x10
8
m/s
Use the formula c = λν or E = hν to solve the following problems . (CP DON’T DO)
24. A radio wave has a wavelength of 3000 m, what is its frequency?
3.00x10
8
m/s = 3000(ν) v = 1x10
5 hz
25. A wave has a frequency of 2.3 x 10
3.00x10
8 m/s = (λ)2.3 x 10 6 Hz
6
Hz, what is the wavelength?
λ = 130 m/s
26. What is the energy of a wave that has a frequency of 4.5 x 10
7
Hz?
E = 6.626x10
-34
j*s (4.5 x 10
7
Hz) E = 3.0x10
-26
J
27. What is the frequency of a wave that has energy of 3.6 x 10 -16 J?
3.6 x 10
-16
J = 6.626x10
-34
j*s (v) v = 5.4x10
17
Hz
28. Describe each of the following:
Aufbau Principle: States that electrons will fill the lowest energy levels first before filling the higher energy levels
Pauli’s Exclusion Principle: States that two electrons fill 1 orbital but they must have opposite spins
Hund’s Rule: States that orbitals of the same energy (such as the 3 in a p subshell) will fill with one electron of one spin first before a second electron with an opposite spin will fill it.
29. Write the FULL electron configuration for Cu, Cr, S, Zn
Cu: 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
9
Cr: 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
4
S: 1s 2 2s 2 2p 6 3s 2 3p 4
Zn: 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
30. Write the Noble Gas Configuration for P, Fe, Br, Al
P: [Ne] 3s 2 3p 3
Fe: [Ar] 4s
2
3d
6
Br: [Ar] 4s
2
3d
10
4p
5

Al: [Ne] 3s
2
3p
1
31. Write the orbital notation for Ar, Mg, F
Ar: 1s
2
2s
2
2p
6
3s
2
3p
6
1s 2s 2p 3s
Mg: 1s
2
2s
2
2p
6
3s
2
3p
1s 2s 2p 3s
F: 1s
2
2s
2
2p
5
1s 2s 2p
32. Identify the elements from the following configurations:
a. 1s
2
2s
2
2p
6
3s
2
Magnesium
b. 1s
2
2s
2
2p
6
3s
2
3p
6
4s
1
Potassium
c 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 Cobalt
33. Identify the following elements from their valence configurations :(ALL: DON’T DO)
a. 3s
2
3p
6
b. 2s
2
2p
4
c. 4s
1
d. 5s
2
4d
8
e. 1s
2