Unit 2 Review
Chapter 3, 4 and 5
1. Discuss the evolution of the atomic theory, including the following scientists:
a. Democritus
b. Aristotle
c. John Dalton
d. Antoine Lavioser
e. J.J Thomson
f. Ernest Rutherford
g. Neihls Bohr
h. Ernst Shroedinger
i. Max Planck
2. Explain the law of conservation of mass, the law of definite proportions and the law of multiple
proportions.
3. Differentiate between protons, neutrons and electrons based on mass, charge and location.
4. Differentiate between the four fundamental forces in nature.
a. Strong
b. Weak
c. Electromagnetic
d. gravity
5. Explain what isotopes are.
6. Identify the atomic number, mass number and atomic mass of all the elements on the periodic
table.
7. Define mole, avogadro’s number and molar mass.
8. Solve calculations involving converting grams to moles and moles to grams.
9. Determine the molar mass of different elements and compounds.
10. Calculate the atomic mass of various elements on the periodic table.
11. Calculate the frequency or wavelength of electromagnetic waves.
12. Discuss the concept of the quantum mechanical model.
13. Discuss Heisenberg’s uncertainty principle and explain the importance of this principle to
understanding the basics of electron cloud structure.
14. Draw Bohr models of different elements on the periodic table.
15. Discuss the relationship between amount of energy and the color of light produced by excited
electrons.
16. Define quantum and use it to disucss the organization of the electron cloud.
17. Differentiate between the ground state and excited state of an electron.
18. Explain why the atomic emission spectrum is like the fingerprint of an atom.
19. Discuss the relationship between energy level, sublevel and orbitals of an atom.
20. Differentiate between the four different types of sublevels.
21. Differentiate between the angular momentum quantum number and the magnetic quantum
number.
22. Discuss the three rules governing electron configurations.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
a. Aufbau principle
b. Pauli exclusion principle
c. Hund’s rule
Write electron configurations for any of the elements on the periodic table.
Explain the roles of Dmitri Mendeleev and Henry Moseley in the development of the modern
periodic table.
Discuss the periodic law and explain what it means for the overall organization of the periodic
table.
Identify the location and describe the general characteristics of alkali metals, alkaline earth
metals, transition metals, inner transition metals, halogens and noble gases.
Identify the location of the s, p, d and f block on the periodic table.
Define the following terms:
a. Electronegativity
b. Electron affinity
c. Nuclear shielding
d. Ionization energy
Determine the following trends for different elements on the periodic table
a. Atomic radius
b. Ionic radius
c. Electronegativity
d. Electron affinity
e. Nuclear shielding
f. Overall chemical reactivity
g. Ionization energy
Define valence electrons and determine the number of valence electrons of different elements
on the periodic table.
Differentiate between the 5 types of nuclear reactions discussed in class:
a. Alpha decay
b. Beta decay
c. Positron emission
d. Gamma decay
e. Electron capture
Predict the products of various alpha, beta, positron emission, electron capture reactions.
Complete a decay series.
Calculate the half-life of a radioactive isotope.