Name
Chemistry: Atomic Structure Review
Multiple Choice
_____1. Isotopes are atoms of the same element that differ in the
a. chemical properties
c. atomic number
b. number of neutrons
d. number of protons and electrons
_____ 2. Rutherford’s gold foil experiment led to the conclusion that the atom had
a. a densely packed positively charged core (nucleus)
b. a negatively charged core held loosely together
c. a densely packed neutral core
d. no definite structure
_____ 3. The sum of the protons and neutrons in an atom equals the
a. atomic number
b. number of electrons
c. atomic mass
_____ 4. All atoms of the same element have the same
a. number of protons
b. number of neutrons
d. mass number
c. mass number
d. mass
_____ 5. Which of these statements is false?
a. Electrons have a negative charge.
b. Electrons have a mass of 1 amu.
c. The nucleus of at atom is positively charged.
d. The neutron is found in the nucleus of an atom.
_____ 6. An atom of an element with atomic number 48 and mass number 120 contains
a. 48, protons, 48 electrons, and 72 neutrons
b. 72 protons, 48 electrons, and 48 neutrons
c. 120 protons, 48 electrons, and 72 neutrons
d. 72 protons, 72 electrons, and 48 neutrons
_____7. Most of the volume of an atom is
a. the nucleus
b. protons
c. empty space
d. neutrons
8. Complete the following table to compare the types of subatomic particles.
Particle
Proton
Electron
Neutron
Mass number in amu
9. Calculations:
Symbol
Percent
Abundance
Chlorine
Cl
75.77%
Chlorine
Cl
24.23%
Name
Relative charge
Average Atomic Mass ___________________
10. Fill in the following table
Atomic
number
Atomic
mass
Number of
protons
Number of
electrons
Number of
neutrons
Helium – 4
6
Carbon –
Potassium –
39
31
Nickel –
Boron – 11
50
Strontium –
Argon – 40
11.
Energy Number of
level
sublevels
1
2
3
4
Names of
sublevels
12. For the following diagrams use: Pauli exclusion principle, Aufbau principle, or Hund’s rule. You will use each
once.
a. Which rule for the filling of orbitals is being violated in the orbital diagram for Silicon?
b. Which rule for the filling of orbitals is being violated in the orbital diagram for Phosphorus?
c. Which rule for the filling of orbitals is being violated in the orbital diagram for Magnesium?
Write the electron configuration for the following elements in the space provided.
1. Manganese _____________________________________________________
2. Mercury _______________________________________________________
3. Potassium ______________________________________________________
4. Fluorine _______________________________________________________
5. Boron _________________________________________________________
Draw the orbital notation for the following elements in the space provided.
6. Sodium ________________________________________________________
7. Helium ________________________________________________________
8. Carbon ________________________________________________________
Answer the following questions for the element Aluminum.
9. How many electrons are in each atom?
10. What’s the atomic number of this element?
11. Write the orbital notation for aluminum’s electron configuration.
12. How many unpaired electrons does aluminum have?
13. What’s the highest occupied energy level?
14. How many inner-shell electrons does the atom have?
15. In which orbital(s) are these inner-shell electrons located?
Identify each of the following atoms on the basis of the electron configuration.
16. 1s22s22p5
17. 1s22s22p63s23p4
18. 1s1
19. 1s22s22p63s23p64s23d7
20. 1s22s22p63s23p64s23d104p65s1