CHAPTER 5: ELECTRONS IN ATOMS
CHEMISTRY
True/False
Indicate whether the statement is true or false.
____
1. There are a total of 5 d-orbitals.
____
2. The photoelectric effect describes the emission of electrons from a metal’s surface when light at a specific
frequency shines on it.
____
3. Although the precise location of an electron cannot be determined, it is possible to determine the probability
that an electron will occupy a certain region around the nucleus.
____
4. In the visible light spectrum, red light has a greater frequency (energy) than violet light.
____
5. [Kr]5s24d105p5 is the correct electron configuration for the element Bromine.
____
6. The maximum number of allowed valence electrons in any atom is 8.
____
7. Each element has its own unique emission spectrum.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
8. Which label identifies the amplitude of the wave shown?
a. A
c. C
b. B
d. D
____ 9. Which label identifies the wavelength of the wave shown?
a. A
c. C
b. B
d. D
____ 10. Which label identifies the trough of the wave shown?
a. A
c. C
b. B
d. D
____ 11. Which diagram shows a wave with the highest frequency?
a. A
b. B
c. C
d. D
____ 12. Which type of wave has a wavelength of approximately 10-12 meters?
a. microwaves
c. Gamma rays
b. AM radio
____ 13. Which is the correct number of valence electrons in the element Gallium (Ga, Z=31)?
a. 3
c. 1
b. 31
____ 14. Which is the correct number of valence electrons in the element Sulfur (S, Z=16)?
a. 16
c. 4
b. 6
____ 15. Which is the correct electron configuration for the element Molybdenum (Mo, Z=42)?
a. 1s22s22p63s23p64s23d104p65s6
c. 1s22s22p63s23p64s23d4
2 2
6 2
6 2
10
6 2
4
b. 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d
____ 16. According to __________, one electron must occupy each orbital before a second electron of opposity spin is
added.
a. Heisenberg Uncertainty Principl
c. Aufbau Principle
b. Hund’s Rule
____ 17. Which is the correct electron dot diagram for the element Silicon (Si, Z=14)?
a.
c.
Si
Si
b.
____ 18.
____ 19.
____ 20.
____ 21.
Si
Which scientist is credited for the Planetary Atomic Model of the atom?
a. Rutherford
c. Schoedinger
b. Bohr
Which scientist is credited for the Quantum Mechanical Model (electron cloud model) of the atom?
a. Rutherford
c. Bohr
b. Schoedinger
The _____________ states that is is impossible to know both the velocity and location of a particle at the
same time.
a. Pauli Exclusion Principle
c. Aufbau Principle
b. Heisenberg Uncertainty Principle
An element has an electron configuration of [Ar] 4s2 3d10 4p4. How many valence electron are there?
a. 4
c. 6
b. 16
____ 22. The electron configuraion of S is [Ne] 3s2 3p4. Which is the correct electron dot structure?
a.
c.
S
S
b.
S
____ 23. Once atoms gain energy, their electrons may jump to a(n) ___________ state.
a. excited
c. valence
b. ground
____ 24. The __________ are the electrons found in the highest prinipal energy level.
a. valence
c. critical
b. excited
____ 25. The arrangement of electrons in an atom is called the ____________________ of an atom.
a. electron configuation
c. electron dot diagram
b. orbital diagram
____ 26. The ____________________ principle states that a maximum of two electrons may occupy a single atomic
orbital, but only if the electrons have opposite spins.
a. Heisenberg Uncertainty Principle
c. Hund’s Rule
b. Pauli Exclusion Principle
Short Answer
27. A student records the following electron configuration for the element Arsenic (As). Please correct any
mistakes.
1s22s22p63s23p64s24d104p3
28. A student draws the following orbital diagram for Phosphorus. If there are any mistakes, please correct them.
29. Is this orbital diagram correct? If not, please correct.
Problem
30. For the element At (85 electrons):
a.)
b.)
c.)
d.)
Write its electron configuration using noble gas notation
Draw its orbital diagram
Circle its valence electrons in the electron configuration
Draw its electron dot structure
BONUS
31. What is the maximum number of valence electrons an atom can have? Can there ever be any valence
electrons in the d or f orbitals? Explain.