Question 1
Put the following EM waves in order of highest frequency to lowest frequency:

Microwaves, Ultraviolet, X-rays, Infrared radiation

Microwaves, Infrared radiation, Ultraviolet, X-rays
X-rays, Ultraviolet, Infrared radiation, Microwaves
Microwaves, Ultraviolet, Infrared radiation, X-rays
X-rays, Infrared radiation, Ultraviolet, Microwaves


Question 2
What is the electron configuration of sulfur?

1s22s22p4
1s22s22p63s23p64s1
1s22s22p63s23p4
1s22s22p23s63p2



Question 3
Which of type of EM waves have the longest wavelength?
Radio waves
X-rays
Microwaves
Gamma rays


Question 4
Which of the following EM waves has the highest energy?
Ultraviolet
Infrared radiation
Radio waves
Visible light


Question 5
What is the maximum number of electrons possible in the 3rd principal energy level?
18
2
8
32


Question 6
Which of the following statements expresses Hund's rule?
Single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy the same orbitals.
P orbitals may contain up to six electrons.
Electrons in orbitals must possess opposite spins.
Electrons with the same spin fill all orbitals.


Question 7
If a radio station were to increase its frequency from 94.5 MHz to 99.1 MHz, what would happen to the station's wavelength?
The wavelength would go up.
The wavelength would not change.
The wavelength would go down.
The wavelength would double.


Question 8
Which of the following statements is true?
Each set of d orbitals can hold a maximum of 14 electrons.
The first energy level contains only s and p orbitals.
All s orbitals are spherically shaped.
Each set of d orbitals contains seven orbitals.


Question 9
The lowest allowable energy of an atom is called ___________.

excited state
sublevel
ground state
atomic emission


Question 10
How many electrons can an orbital contain?
6
2
1
3


Question 11
What is the orbital notation for a carbon atom?
  
       
        
       


Question 12
Which orbitals are associated with most energy 3s, 3d, 3p, or 4s?
3s
3d
3p
4s


Question 13
The electron configuration 1s22s22p63s23p6 represents atoms of which element in the ground state?
Neon
Chlorine
Argon
Sulfur


Question 14
Select the electron configuration of the orbital notation below.



        

1s22s22p6
1s22p6
1s22s22p2
1s22s22p4


Question 15
During a flame test, ions of a specific metal are heated in the flame of a gas burner. A characteristic color of light is emitted by these ions in the flame when the electrons
gain energy as they return to lower energy levels.
gain energy as they move to higher energy levels.
emit energy as they move to higher energy levels.
emit energy as they return to lower energy levels.


Question 16
What is the orbital notation for an atom of neon in the ground state?