Unit 4 – Atomic Structure Study Guide
1. List the components of Dalton’s Atomic Theory.
2. Based upon Dalton’s Atomic Theory, explain the difference between a sodium atom and a chlorine
atom.
3. Based upon Dalton’s Atomic Theory, explain why Mg1.5Cl3 is not a valid formula.
4. Complete the following table on the subatomic particles.
PARTICLE
LOCATION
CHARGE
MASS (AMU)
5. Describe what Rutherford’s Gold Foil experiment showed about the structure of an atom.
6. In the symbol,
, explain what 11, 23, and Na represent.
7. Explain why 14C and 12C are isotopes.
8. Complete the following table.
SYMBOL
ATOMIC NO.
ATOMIC
MASS
13
27
NO.
PROTONS
NO.
ELECTRONS
2
2
6
40
NO.
NEUTRONS
20
7
9. Select the true statement.
a. There are more metals than nonmetals in the Periodic Table.
b. There are more nonmetals than metals in the Periodic Table.
10. True or False. The nonmetals are located on the left side of the Periodic Table.
11. Select the true statement.
a. All elements in the same Group/Family have similar chemical properties.
b. All elements in the same Period/Row have similar chemical properties.
12. Describe the trend in Atomic Radius in relationship to the Periodic Law.
13. Define the following:
a. ground state –
b. excited state –
14. Explain what happens during an electron’s transition from the ground state to an excited state and
the return to the ground state.
15. Describe the shape of and maximum number of electrons in the s and p orbitals.
16. In the electron configuration, He 1s2, explain what 1, s, and 2 represent.
17. Define the following terms and how their values can be obtained from the Periodic Table:
a. valence shell –
b. valence electron –
c. Lewis Dot Structure –
18. Give the electron configuration and Lewis Dot Structure for the following:
a. K
b. Ne
c. F