Name: ____________________________________
Chapter 4 Review – Arrangement of Electrons
KEY
SOLVE THE FOLLOWING LIGHT & ENERGY PROBLEMS:
1. Find the energy of an infrared photon whose frequency is 2.0  1012 Hz.
1.3 x 10-21 J
2. What is the wavelength of a red light wave whose frequency is 4.3  1014 Hz?
7.0 x 10-7 m
3. Calculate the frequency of an X-ray wave that has a wavelength of 9.2 nm.
3.3 x 1016 Hz
4. What is the energy of a cosmic ray photon whose wavelength is 2.0 pm?
9.9 x 10-14 J
5. Find the frequency of a microwave that carries 3.4  10-25 J of energy.
5.1 x 108 Hz
NAME THE TERM DESCRIBED BY THE FOLLOWING DEFINITIONS:
Word Bank:
Anion
Aufbau
Cation
Excited
Ground
Photon
Valence
Heisenburg Uncertainty
Hund’s (rule) Principle
Pauli Exclusion Principle
6. _________________________
A packet of light energy that carries a quantum of energy.
7. _________________________
The state when all electrons of an atom are in the lowest possible energy levels.
8. _________________________
When an electron jumps up to a higher energy level, the atom is in its ___.
9. _________________________
The theory that it is impossible to know both the position and speed of an electron simultaneously.
10. __________________________
The theory that no two electrons in an atom can share the same 4 quantum numbers.
11. __________________________
The theory that electrons fill the lowest energy orbitals first.
12. __________________________
The theory that, within a sublevel, electrons prefer to occupy their own orbital.
13. __________________________
A term describing the outermost electrons in an atom.
14. ____________________________ , ______________________ Chapter 3 & 22
A positively charged ion is called a(n) ___. A negatively charged ion is called a(n) ___.
DRAW ORBITAL DIAGRAMS FOR THE FOLLOWING ELEMENTS: (LINES & ARROWS)
15. Mg
16. Si
17. Ti
WRITE LONGHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
18. N
19. K
20. Cr
WRITE SHORTHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
21. Sb
22. Bi
23. Tc
24. Ge
WRITE THE ION SYMBOL AND ITS SHORTHAND ELECTRON CONFIGURATION:
Element
Ion
(Charge)
Te
Te -2
B
B +3
Ba
Ba +2
Br
Br -1
K
K +1
Shorthand Electron Configuration
[Kr] 5s2 4d10 5p6
-2
25. What three principles guide the electron configuration of an atom? (Briefly explain)
1) Pauli Exclusion Principle 2) Aufbau’s Principle 3) Hund’s (Rule) Principle -
26. What is an octet of electron? __________________________________________
27. Which elements contain an octet of electrons? ___________________________
28. Identify the elements having the following electron configurations?
Answers (in alphabetical order): Argon, Arsenic, Potassium & Silicon
a) 1s22s22p63s23p6 = _______________________
b) [Ar] 4s1 = ___________________
c) contains four electrons in its third and outer main energy level = _____________
d) contains one set of paired and three unpaired electrons in its fourth and outer
main energy level = ______________________
29. Which has a longer wavelength, green or yellow light? ________________________
30. Which has a higher frequencies, an X ray or a microwave? ____________________
31. Which travels at a greater speed, ultraviolet or infrared light? ___________________
32. Quantum Number: Symbols, meanings, how they narrow down the address of an electron
Symbol
Name of Quantum #
Description
‘n
‘l
ml
ms
33. Circle the radiation with the lowest frequency?
a. gamma rays
b. x rays
c. blue light d. red light
e. radio waves
34. Circle the radiation with the shortest wavelength?
a. gamma rays
b. x rays
c. blue light d. red light
e. radio waves
35. Rank the following regions of the electromagnetic spectrum in order of increasing
energy.
Xrays,
microwaves,
infrared, ultraviolet, visible
(least energetic)
(most energetic)
36. Which of the following sets of quantum numbers is NOT permissible?
ANSWER: Possible = 3, Not possible = 2
a. n = 1, l = 0, ml = 0, ms = + 1/2
Possible
or
Not Possible
b. n = 4, l = 0, ml = 0, ms = + 1/2
Possible
or
Not Possible
c. n = 3, l = 3, ml = -3, ms = - 1/2
Possible
or
Not Possible
d. n = 2, l = 1, ml = 1, ms = - 1/2
Possible
or
Not Possible
e. n = 2, l = 1, ml = 2, ms = + 1/2
Possible
or
Not Possible
Word bank for #37 thru #42 (in alphabetical order):
Diffraction Interference
Quanta Wave Wavelength
3x108 m/s
37. The frequency of a light wave is inversely proportional to its ____________________
38. Light moves at a constant speed of _______________________________.
39. The bending of a wave as it passes by the edge of an object is called ______________
40. When waves overlap each other, ________________________ occurs.
41. Planck proposed that energy is emitted or absorbed by any object in fixed amounts
called _______________
42. Light is said to have properties of both particles and _______________.
43. How are colors created in a line-emission spectrum?
STUDYING FOR CHAPTER 4 TEST
Read over your notes and rework your homework assignments.
You will be given the E=hv and c= v formula and the periodic table.
You will do AWESOME on the test if you do the following things.
Electron Configuration
Using the periodic table:
Draw the orbital notation (arrows).
Write the longhand and shorthand (noble gas) electron configurations
Write the ion symbol and electron configurations of an ion.
Explain the following concepts:
How stability leads to exceptions in the electron configurations of Cu and Cr.
Know the difference between energy levels, sublevels, and orbitals?
Absorption Spectra & Emission Spectra – what are they?
Know the meaning of the following terms:
Aufbau Principle
Hund’s Rule
Unpaired Electrons
Photon
Ground State
Excited State
Orbital
Valence (Outer) Electrons
Core (Inner) Electrons
Heisenburg Uncertainty Principle
Pauli Exclusion Principle