CHEMISTRY QUESTIONAIREE
1. What are the three main subatomic particles that make up an atom?
2. What is the chemical symbol for silver?
3. Define isotopes and give an example.
4. What are the seven diatomic elements?
5. Explain periodic trends in atomic radius across a period.
6. Contrast ionic and covalent bonding.
7. Draw the Lewis structure for
a. carbon dioxide, CO2.
b. Water, H2O
c. Ammonia, NH3
8. What are the names of the groups in the periodic table?
9. What are the chemical and physical properties of
a. Halogens?
b. Alcohols
c. Alkanes
10. Write the chemical formula for
a. calcium chloride.
b. Hydrogen peroxide
c. Nitric acid
d. Sulfuric acid
11. What type of bond forms between a
a. metal and a nonmetal?
12. What is the outermost energy level of the
a. noble gases
b. Halogens
c. Alkali metals
13. Name the regions of the electromagnetic spectrum used in spectroscopy.
14. Describe crystalline solids and amorphous solids.
15. Define the
a. law of definite proportions
b. Pauli exclusion principle
c. Octlet rule.
d. Aufbau principle
16. What are the major attractions between molecules?
, 17. How many valence electrons are in the following atoms?
a. Oxygen
b. Phosphorous
c. Carbon
d. Nitrogen
e. Iron
18. Draw the structural formula of:
a. Butanol
b. Propyl
c. Benzene
d. Hexan-2-one
e. 2,3-dibromo pentane
18. Give one example each of a metal, nonmetal, and metalloid.
19. Contrast electrolytes and nonelectrolytes in solution.
20. Compare intermolecular forces in elements like Br2 vs Cl2.
21. Write the electron configuration for
a. neon.
b. Argon
c. Phosphorous
d. Calcium
e. magnesium
22. Differentiate among quantitative, qualitative, and common-ion effects.
23. What type of reaction involves the transfer of electrons between species?
24. Derive the formula for the
a. molarity of a solution.
b. Concentration
c. Relative molar mass
25. Predict products and state oxidation numbers in redox reactions.
26. Define and give examples of endothermic and exothermic processes.
27. Contrast strong and weak electrolytes.
28. Explain the dual nature of light as particles and waves.
29. What is the Kolbe reaction?
30. Write balanced net ionic equations when possible.
31. Name the chemical process when atoms combine to form a positively charged cation and
a negatively charged anion.
32. Write the solubility rules for ionic compounds.
1. What are the three main subatomic particles that make up an atom?
2. What is the chemical symbol for silver?
3. Define isotopes and give an example.
4. What are the seven diatomic elements?
5. Explain periodic trends in atomic radius across a period.
6. Contrast ionic and covalent bonding.
7. Draw the Lewis structure for
a. carbon dioxide, CO2.
b. Water, H2O
c. Ammonia, NH3
8. What are the names of the groups in the periodic table?
9. What are the chemical and physical properties of
a. Halogens?
b. Alcohols
c. Alkanes
10. Write the chemical formula for
a. calcium chloride.
b. Hydrogen peroxide
c. Nitric acid
d. Sulfuric acid
11. What type of bond forms between a
a. metal and a nonmetal?
12. What is the outermost energy level of the
a. noble gases
b. Halogens
c. Alkali metals
13. Name the regions of the electromagnetic spectrum used in spectroscopy.
14. Describe crystalline solids and amorphous solids.
15. Define the
a. law of definite proportions
b. Pauli exclusion principle
c. Octlet rule.
d. Aufbau principle
16. What are the major attractions between molecules?
, 17. How many valence electrons are in the following atoms?
a. Oxygen
b. Phosphorous
c. Carbon
d. Nitrogen
e. Iron
18. Draw the structural formula of:
a. Butanol
b. Propyl
c. Benzene
d. Hexan-2-one
e. 2,3-dibromo pentane
18. Give one example each of a metal, nonmetal, and metalloid.
19. Contrast electrolytes and nonelectrolytes in solution.
20. Compare intermolecular forces in elements like Br2 vs Cl2.
21. Write the electron configuration for
a. neon.
b. Argon
c. Phosphorous
d. Calcium
e. magnesium
22. Differentiate among quantitative, qualitative, and common-ion effects.
23. What type of reaction involves the transfer of electrons between species?
24. Derive the formula for the
a. molarity of a solution.
b. Concentration
c. Relative molar mass
25. Predict products and state oxidation numbers in redox reactions.
26. Define and give examples of endothermic and exothermic processes.
27. Contrast strong and weak electrolytes.
28. Explain the dual nature of light as particles and waves.
29. What is the Kolbe reaction?
30. Write balanced net ionic equations when possible.
31. Name the chemical process when atoms combine to form a positively charged cation and
a negatively charged anion.
32. Write the solubility rules for ionic compounds.
