Name: ____________________________________________________ Period: _______ Teacher: ____________
Unit 4 – The Electron (Level)
26
27
28-29
30
Oct. 3
4
5-6
7
10
11
12-13
14
Vocabulary
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Wavelength
Frequency
Amplitude
Quanta
Electromagnetic spectrum
Concepts
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
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Electromagnetic Spectrum
Wavelength, amplitude and frequency
calculations
Quanta (light as a particle)
Photoelectric effect and photons
Emission spectra
Bohr Models
Lewis Dot Structures
Orbital diagrams
Electron configuration
Objectives:
1. List types of EMR in order of increasing energy.
2. Label the parts of a wave.
3. Mathematically relate wavelength and frequency to speed of EMR.
4. Compare the wave and particle models of light.
5. Define a quantum of energy and explain how it is related to the energy levels of electrons.
6. Identify a metal ion using a flame test and list uses of atomic emission spectral analysis.
7. Draw Bohr models for the first 30 elements.
8. Compare the Bohr and quantum mechanical models of the atom.
9. Identify the relationships among an atom’s energy levels, sublevels, and atomic orbitals
10. Apply the Pauli exclusion principle, the Aufbau principle, and Hund’s rule to fill in orbital diagrams.
11. Write the electron configuration for any element and be able to do the noble gas notation as well.
12. Identify the four blocks of the periodic table as they apply to electron configuration.
13. Define valence electrons and draw electron-dot structures representing an atom’s valence electrons.
Warm-ups
Mon, Sept. 26
Tues, Sept. 27
Thurs, Sept. 29
Fri, Sept. 30
Mon, Oct. 3
Tues, Oct. 4
Thurs, Oct. 6
Fri, Oct. 7
Scientific Notation Notes
What is the correct form for numbers written in scientific notation?
How do you put numbers in scientific notation from standard notation?
What is the difference between a positive and negative exponent in scientific notation?
Put the following numbers into scientific notation.
1. 6,400 __________________________________
4. 3,430,000,000,000 _______________________
2. 0.0000000452 ___________________________
5. 232,000 _______________________________
3. 0.0000056 ______________________________
6. 0.00132 _______________________________
How do you convert numbers from scientific notation to standard notation?
Put the following numbers into standard notation.
7. 6.41 x 10-11 _____________________________
10. 4.25 x 10-9 ______________________________
8. 8.66 x 10-4 ______________________________
11. 9.87 x 104 _______________________________
9. 1.05 x 1013 ______________________________
12. 5.08 x 1010 ______________________________
Scientific Notation Practice
Directions: Write the numbers in either standard notation or scientific notation (depending on the starting value)
1. 50,000 m/s2 ________________________
7. 7.6352 x 10-3 kg ________________________
2. 3.03 x 10-4 dg ________________________
8. 21,300,000 mL _________________________
3. 0.00000000062 kg _____________________
9. 990,900,000 m/s ________________________
4. 8.348 x 106 km ________________________
10. 3.02 x 10-5 s ____________________________
5. 3.402 x 103 g _________________________
11. 0.000000004 L __________________________
6. 0.000023 s ___________________________
12. 8.4 x 106 L ______________________________
Metric Conversion Review
Unit
Meters
Centimeters
Nanometers
Symbol
m
cm
nm
10x
100
10-2
10-9
a.
How many cm in 2.89 m? _____
b.
How many nm in 1,845.3 m? ___________________
c.
How many m in 514.8 cm? ____________________
d.
How many m in 714 nm? _______________________
Electromagnetic Spectrum Notes
Ground State and Excited State
Label the parts of the Electromagnetic Spectrum
Draw arrows and label to show increasing wavelength, increasing frequency and increasing energy.
What are 2 acronyms that you can use to help remember the order of the Electromagnetic Spectrum?
Electromagnetic Spectrum Practice
High
energy
High
frequency
Low energy
Long
wavelength
Visible Light Spectrum – part of the EMS that we can see
The diagram pictured above is called the electromagnetic spectrum. It shows the colors that humans see as visible light,
but it also represents all the other kinds of light that exist that we can’t see. Use the diagram to answer the questions
that follow.
1. Rank the types of visible light in order from longest to shortest wavelength: ________________,
________________, ________________, ________________, ________________, ________________, and
________________.
2. Which color on the visible light spectrum has the highest amount of energy? _______________________
3. Rank the types of radiation on the Electromagnetic Spectrum in order from lowest energy to highest energy:
_______________________, __________________________, ____________________,
_______________________, ______________________, ___________________________,
___________________
4. On the Electromagnetic Spectrum (EMS), which type of radiation has the highest frequency? ______________
5. On the EMS, does infrared light or ultraviolet light have a lower amount of energy? Please explain.
6. Between microwaves and radio waves, which one has a higher wavelength? Please explain.
7.
8.
9.
10.
What has a lower frequency than infrared light? ______________________________________________
Which color has a higher energy: blue or yellow? _____________________________________________
Which color has a higher frequency: orange or green? _________________________________________
What is the relationship between energy and frequency?
11. What is the relationship between frequency and wavelength?
Waves and Light Notes
Label the parts of a wave:
Wave Vocabulary:
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Wavelength:

Frequency:

Amplitude:

Speed of Light:

Energy:

Planck’s constant:

Quantum:
Equation showing relationship between wavelength and frequency:
Example 1: Calculate the υ of a wave that has a wavelength of 5.00 x 10-6 m.
Example 2: What is the λ of radiation with a frequency of 1.50 x 1013 Hz?
Who stated there was a relationship between the energy of a quantum and the frequency? __________________
Equation showing relationship between energy and frequency:
Example 1: Calculate the E of a wave that has a frequency of 7.66 x 1014 Hz .
Example 2: What is the υ of radiation with 8.35 x 10-18 J of energy?
Using both equations!
Example 1: What is the energy of a 9.3 x 10-3 m wave?
Example 2: What is the wavelength of a 1.528 x 10-13 J wave?
Parts of a Wave Practice
1.
The highest point on a wave is the __________, while the lowest point is the __________.
2. The __________ of a wave is a measure of the amount of energy it carries.
3. The distance from one crest to the next crest is the __________.
4. The __________ is a measure of the number of waves that pass a point in a given amount of time.
5. The illustration to the right shows a wave. Label each part in the space below:
a. ____________________
b. ____________________
c. ____________________
d. ____________________
e. ____________________
f. ____________________
g. ____________________
6. Use the five illustrations of waves drawn below to answer the following questions:
(a) Waves P and Q have the same __________, but wave P has twice the __________ of wave Q.
(b) Waves Q and R have the same __________, but wave R has twice the __________ of wave Q.
(c) Wave __________ shows a steady frequency but changing amplitude.
(d) Wave __________ shows steady amplitude but a changing frequency.
7. In words and in an equation, represent the following relationships:
(a) Energy and Frequency
(b) Energy and Wavelength
(c) Frequency and Wavelength
Speed of Light Calculations
Speed of EM waves = wavelength x frequency
c = λV
c = 3.00 x 108 m/s, speed of light
λ= wavelength, measured in m
f= frequency, measured in Hz (Hz = 1/s)
1. Green light has a frequency of 6.01 x 1014 Hz. What is the wavelength?
Given
Rearranged Equation
Work
Final Answer
2. Violet light has a wavelength of 4.10 x 10-12 m. What is the frequency?
Given
Rearranged Equation
Work
Final Answer
3. The speed of light is 300,000,000 m/s. What is the frequency of microwaves with a wavelength of 0.01 meter?
4. A radio is broadcast at approximately 18.9 MHz. What wavelengths does this correspond?
5. What is the wavelength of X-rays having a frequency of 4.80 x 1017 Hz?
6. A helium laser emits light with a wavelength of 633 nm. What is the frequency of the light?
Energy Calculations
Energy = Planck’s constant x frequency
c = λV
E = Energy, Joules (J)
h= 6.626 x 10-34 J∙s, Planck’s constant
f= frequency, measured in Hz (Hz = 1/s)
7. Calculate the energy of a photon of radiation with a frequency of 8.5 x 1014 Hz.
Given
Rearranged Equation
Work
Final Answer
8. What is the frequency of a wave carrying 8.35 x 10-18 J of energy?
Given
Rearranged Equation
Work
9. What is the energy of 109.6 MHz wave?
10. What is the energy of a 3.12 x 1018 s-1 wave?
11. What is the wavelength of X-rays having a frequency of 4.80 x 1017 Hz?
12. Calculate the energy of a photon of radiation with a wavelength of 6.4 x 10-7 m.
13. What is the energy of light whose wavelength is 4.06 x 10-11 m?
Final Answer
Electromagnetic Radiation Combined (EMR) Problems
1. What is the wavelength of the yellow sodium emission which has a frequency of 5.09 x 1014 s-1 ?
2. The frequency of the strong red line in the spectrum of potassium is 3.91 x 1014 s-1. What is the wavelength of this
light in nanometers?
3. What is the frequency of violet light with a wavelength of 408 nm?
4. An EMR has a wavelength of 344nm. What is its frequency?
5. What is the energy of the photon with a frequency of 2,300 kHz?
6. The red spectral line of lithium occurs at 671nm. Calculate the energy of one photon of this light.
7. What is the energy of the photon with a wavelength of 2,500 m?
8. The red line in the spectrum for excited hydrogen has a wavelength of 656nm. This light is released when an electron
drops from energy level 3 to energy level 2. What energy change is involved?
9. The energy needed to break a single Cl2 molecule into separate atoms is 3.97 x 10-19 J. What frequency of
electromagnetic radiation would be required to break this bond? Is this light in the visible range?
Blocks of the Periodic Table
Directions:
1. Label the rows of the periodic table (using numbers written to the left), starting at 1. This represents the energy
levels that surround the nucleus. This is the principal quantum number (n).
2. Each energy level contains energy sublevels that are referred to as s, p, d and f. These sublevels can be grouped
into “blocks” on the periodic table.
a. Color the first two columns (and helium) blue. Put a “s” in the first block of each row.
b. Color the last six columns (minus helium) red. Put a “p” in the first block of each row.
c. Color the middle ten columns (not the bottom) yellow. Put a “d” in the first block of each row.
d. Color the bottom two rows green. Put a “f” in the first block of each row.
3. Each of these energy sublevels will be designated with a quantum number (i.e., 2p, 5d, 4p).
a. s = n
b. p = n
N = principal energy level
c. d = n-1
d. f = n-2
4. Put the corresponding quantum number in front of each letter that you wrote on your periodic table.
# of Electrons per sublevel:
s: 2
p: 6
d: 10
f: 14
5. How many columns are in each of the blocks? How does this relate to the number of electrons per sublevel?
6. Read the periodic table like a book and write the order of the “blocks” as you go from left to right, up to down.
Pay careful attention to where the two “f blocks” fit into the periodic table. I’ll get you started:
1s, 2s, 2p,
Electron Configuration Notes
What is electron configuration?
Energy Levels
Energy
Level
Max # of
Electrons
Energy Level
# of Sublevels
Orbitals
Sublevel
# of Possible Orbitals
Max # of Electrons
in Sublevel
What does Aufbau’s principle state?
Incorrect Aufbau Diagram
Correct Aufbau Diagram
Explain in the space above why these diagrams are correct and incorrect.
Corresponding Sublevels
What does Hund’s Rule state?
Incorrect
Correct
Explain in the space above why these diagrams are correct and incorrect.
What does the Pauli Exclusion Principle state?
Incorrect
Correct
Explain in the space above why these diagrams are correct and incorrect.
Identify each error (and which rule it breaks) in the picture and explain how to correct it.
Electron Configuration
1. What are the different parts of the electron configuration? For example, 1s2
2. Let’s Practice!
•
H: _______________________________________________
•
He: _____________________________________________
•
Be: ______________________________________________
•
N: _______________________________________________
•
Na: _______________________________________________
•
Al: ________________________________________________
•
Ca: ________________________________________________
•
Br: _________________________________________________
3. How many electrons can each of the following orbitals hold?
a. 2s = ________
c. 5f = _________
e. 4p = ________
b. 3p = ________
d. 6d = ________
f. 3d = ________
4. How many “p” orbitals can there be in any energy level? ____________________________
5. What is the maximum number of electrons in the 3rd principle energy level? __________________
6. How many orbitals are in each of the following sublevels?
a. 4p sublevel ____________
c. 4f sublevel
b. 3d sublevel ____________
d. 2s sublevel ____________
7. Identify the element that:
a. Contains a full 3rd energy level
b. Contains 3 electrons in the 2p level____
____________
c. Outer energy level is 4s2
d. Contains 5 electrons in the 4d level____
8 For the following electron configurations, identify which element the configuration is identifying.
a. 1s2 2s22p6 3s23p6 4s2 3d10 4p4 _________________________________________
b. 1s2 2s22p6 3s23p6 4s2 3d10 4p5 ____________________________________________________
c. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s1 _________________________________________
d. 1s2 2s22p6 3s23p6 4s2 3d10 4p6 5s2 4d10 5p2 ___________________________________________
e. [Kr] 5s2 4d10 5p3 ________________________________________________
f. [Ar] 4s1 ____________________________________________________
g. [Xe] 6s2 4f10 _________________________________________________
h. [Ne] 3s2 3p1 _________________________________________________
Long Hand Configuration
1. Write the complete electron configuration for each atom on the blank line.
a. Lithium
b. Fluorine
c.
Carbon
d. Argon
e. Phosphorous
f.
Copper
g. Strontium
h. Xeon
Noble Gas Configuration
1. In the space below, write the Noble Gas (abbreviated) electron configurations of the following elements:
a. iron ________________________________________________
b. bromine ________________________________________________
c.
barium ________________________________________________
d. silver ________________________________________________
e. tellurium ________________________________________________
f.
radium ________________________________________________
2. What does the symbol of the noble gas represent in noble gas configuration?
Orbital Filling Diagrams
Write the long hand electron configuration and fill in the orbital diagrams, for the following elements.
1. Nitrogen ______________________________________________________________
1s
2.
1s
2s
2p
3s
Chlorine________________________________________________________________
2s
2p
3s
3p
3. Sodium _________________________________________________________________
1s
2s
2p
3s
3p
4. Neon ___________________________________________________________________
1s
2s
2p
3s
3p
5. Nickel ______________________________________________________________
1s
2s
2p
3s
3p
4s
3d
Mixed Practice
1. Determine which of the following electron configurations are not valid: State which rule has been violated.
a. 1s22s22p63s23p64s24d104p5 ____________________
b. 1s22s22p63s33d5 ____________________
c. [Ra] 7s25f8 ____________________
d. [Kr] 5s24d105p5 ____________________
2. Determine what elements are denoted by the following electron configurations:
a. 1s22s22p63s23p4 ____________________
b. 1s22s22p63s23p64s23d104p65s1 ____________________
c. [Kr] 5s24d105p3 ____________________
3. Write the long hand electron configuration, noble gas configuration, and orbital diagrams for the following elements.
a. Rubidium
Long hand: ___________________________________________________________________________________
Noble Gas: ___________________________________________________________________________________
Orbital filling: __________________________________________________________________________________
b. Mercury
Long hand: ___________________________________________________________________________________
Noble Gas: ___________________________________________________________________________________
Orbital filling:__________________________________________________________________________________
c. Tin
Long hand: ___________________________________________________________________________________
Noble Gas: ___________________________________________________________________________________
Orbital filling:__________________________________________________________________________________
d. Sulfur
Long hand: ___________________________________________________________________________________
Noble Gas: ___________________________________________________________________________________
Orbital filling:__________________________________________________________________________________
Electron Dot Structures and Bohr Models
How to Draw a Bohr Model
Which subatomic particles would be drawn in the center of the atom?
How do you determine the number of subatomic particles to put in your Bohr Model?
Energy Level
Max # of Electrons
1
2
3
4
Examples:
Nitrogen – 14
Chlorine - 35
Electron Dot Structures
Only uses valence electrons in dot structures:
How to determine valence electrons?
Consists of the element’s symbol surrounded by the atom’s valence electrons.
Directions: For each elements listed below, draw the
electron dot structure and the Bohr model.
S-32
5
6
7
O-15
Ca-40
Look at the locations of Iron and Zinc on the periodic
table. If these two elements have higher atomic
numbers than our examples above (thus having more
electrons), why do they have the same number of
valence electrons as Calcium? Would their valence
electrons be the last electrons to fill energy levels?
Explain.
Si-28
Electron Review 2016
Visible Light and the Electromagnetic Spectrum
1. What is the state of an electron at its lowest amount of energy? ______________________________________
2. What happens to an electron when it moves to an excited state? _____________________________________
3. What happens to the position of an electron when they release energy?
4. What happens to the position of an electron when they absorb energy?
5. What are the 7 types of electromagnetic radiation?
6. Which type of electromagnetic radiation has the lowest amount of energy? ________________________________
7. Which type of electromagnetic radiation has the highest amount of energy? _______________________________
8. What is the relationship between wavelength and frequency? Energy & frequency?
9. What is the relationship between frequency and energy? Wavelength & energy?
10. What are the colors in the visible spectrum? List in order from shortest wavelength to longest wavelength. Circle
the color with the highest frequency. Box the one that has the lowest energy.
11. Bohr’s model was accepted because it explained the spectral line puzzle. Explain how his model explained this.
12. Explain how the light emission spectrum of an element would appear different from the light absorption spectrum
of that element.
13. As an electron moves from ground state, energy is ______________. As an electron moves from the excited state
back down to the ground state, energy is ________________.
14. One electron is located in the second energy level. Another electron is located in the fourth energy level. Which
electron has the most energy? Explain.
Waves
15. What is the time it takes for one full wavelength to pass a certain point is called? ___________________________
16. Draw and Label a wave, include wavelength, point of origin, amplitude, crest and trough
17. What is the symbol used to represent wavelength? _____ frequency? _____ speed of light? _____ Plank’s
constant? _____ Energy of a photon? _____
18. What is the minimum amount of energy that can be gained or lost by an electron?
19. If the energy of a wave is high, what is the frequency: high or low?
20. If the frequency of a wave is high, what is the wavelength: long or short?
21. How do you calculate the speed of an electromagnetic wave?
22. What was Einstein’s contribution to the study of electrons and light?
23. Which of the following can you conclude based on the de Broglie equation?
a. Waves behave like particles.
c. All matter has an associated wavelength.
b. Most particles are electrons.
d. All matter behaves like particles.
24. Which of the following best describes the Heisenberg uncertainty principle?
a. Light behaves like a particle and like a wave.
b. The shorter the wavelength, the higher the frequency.
c. It is impossible to know both the velocity and the position of a particle at the same time.
d. You can measure an object without disturbing it.
25. What was Schrödinger’s contribution to the study of electrons and waves?
26. What is the wavelength of the yellow sodium emission which has a frequency of 5.09 x 1014
27. What is the energy of a photon having a frequency of 4.48 x 1014?
28. A helium-neon laser emits light with a wavelength of 833 nm. What is the frequency of this light?
29. What is the wavelength of X rays having a frequency of 7.80x1017 Hz?
30. An FM radio station broadcasts at a frequency of 104.1 MHz. What is the wavelength of the station’s broadcast
signal?
31. Calculate the energy of a photon of ultraviolet light that has a wavelength of 249.0 nm.
Electron Configuration
32. How many energy levels are occupied in an atom of the following elements?
a. Chlorine: _____
b. Tin: ____
33. Which sublevels are located in each of the following periods?
a. Period 1: _________
b. Period 2: __________
c. Magnesium: ____
c. Period 4: __________
34. Which of the following orbitals has the most amount of energy? Explain your answer in the space to the right.
a. 1s
c. 3p
b. 2p
d. 3d
35. How many electrons are found in each of the following sublevels?
a. s: ____
b. p: ____
c. d: ____
d. f: ____
36. How many orbitals are found in each of the following sublevels?
a. s: ____
b. p: ____
c. d: ____
d. f: ____
37. How do we represent electrons with opposite spins in an orbital diagram?
38. In the configuration “4p2”, what does each of the following pieces represent?
4: ____________________
p: ____________________
2
39. In the noble gas configuration [Xe] 6s , what does the [Xe] represent?
2: ____________________
40. If you were to write a noble gas configuration for the following elements, please write which noble gas would be
used for each.
a. Magnesium: ________________
c. Tin: ______________________________
b. Oxygen: _______________
d. Gold: ___________________________
41. Which elements are identified by the following electron configurations?
a. 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1: ______________________________________
b. [Ne] 3s2 3p2: ________________________________________
c. [Kr] 5s2 4d8: ________________________________________
42. Write the long hand electron configuration for the following elements.
a.
Gallium: _______________________________________________________________
b. Vanadium: _____________________________________________________________
c. Palladium: _____________________________________________________________
43. Write the short hand configuration for the following elements.
a.
Nitrogen: ___________________________________________
b. Calcium: ____________________________________________
c. Antimony: ___________________________________________
44. How many electrons can fit in –
a. the 1st energy level? _____
b. a 6p orbital? _______
c. the 3d sublevel? _____
d. the 2nd energy level? __
e. a 2p orbital? __
f. the 3rd energy level? __
45. What does Hund’s rule say?
46. Draw an aufbau diagram for nitrogen that violates Hund’s rule:
47. What does the Pauli Exclusion Principle say?
48. Draw an aufbau diagram for beryllium that violates the Pauli Exclusion Principle.
49. What can you conclude from the figure on the right?
a. Hund’s rule has been violated.
b. The Pauli exclusion principle has been violated.
c. The Aufbau principle has been violated.
d. This is a valid orbital diagram.
50. What can you conclude from the figure on the right?
a. Hund’s rule has been violated.
b. The Pauli exclusion principle has been violated.
c. The Aufbau principle has been violated.
d. This is a valid orbital diagram.
51. Draw a Bohr model of an atom and the electron dot structure of sulfur.
52. Name the sublevel that contains highest energy electrons in an atom of –
a. magnesium _______
c. Calcium ________
b. zinc _______
d. Chlorine _______
53. Name the last electron added when writing the configuration for each of these elements:
Kr (36) _______
Bromine (35) _______ Ca (20) ___________
Fe (26) _______
K (19) _______
Br (35) ____________
54. An orbital of an atom is defined as the most probable location of ___________________________.
55. Which atom in the ground state has an outermost electron with the most energy?
(A) Cs
(B) Li
(C) K
(D) Na
56. How many valence electrons are in each of the following atoms:
a. F? ____
b. Mg?___
c. B? ____
d. Xe? ___