Chemistry 111: Chapter 3 Objectives - Atomic Mass, Ions, and Molar Mass - Prof. P. Coan | Study notes Chemistry

CHEM 111 Chapter 3 Objectives (Chang 9)

Dr. Eric R. Johnson

1. Know the names and chemical formulas for the following ions:

NO3

–

NO2

–

SO4

2–

SO3

2–

PO4

3–

PO3

3–

ClO–

ClO2

–

ClO3

–

ClO4

–

CO3

2–

nitrate

ion

nitrite

ion

sulfate

ion

sulfite

ion

phosphate

ion

phosphite

ion

hypo-

chlorite

ion

chlorite

ion

chlorate

ion

perchlorate

ion

carbonate

ion

Be able to do the following:

2. Define and explain the terms atomic mass, molecular mass, molar mass, mole, and Avogadro’s Number.

3. Calculate the average atomic mass for an element from the naturally occurring isotope masses and their abundances.

4. Know that a mole refers 6.022 x 1023 (Avogadro’s Number) particles.

5.Use appropriate conversion factors convert the mass of an element or compound to the number of moles and the

number of atoms or molecules.

6. Calculate the molecular mass and molar mass of a compound from its molecular formula and a periodic table.

7. Given a molecular formula and a periodic table, calculate the percent by mass for each element in a compound.

8. Given a periodic table and the percent composition by mass for each element in a compound, determine the empirical

formula for that compound.

9. Determine the molecular formula of a compound from the empirical formula and the molecular mass.

10. Given the reactants and products of a chemical reaction, write a balanced chemical equation.

11. Interpret a balanced chemical equation in terms of molecules and moles of reactants and products.

12. Using a periodic table, do mole-to-mole, gram-to-mole, mole-to-gram, and gram-to-mole-to-mole-to-gram

calculations from a balanced chemical equation.

13. Recognize that one of the reactants in a chemical reaction may be a limiting reagent.

14. Do limiting reagent calculations like Example 3.15 on p. 102 in Chang.

15. Distinguish between actual and theoretical yields.

16. Calculate the theoretical yield for a chemical reaction.

17. Calculate the % yield for a chemical reaction.

Assigned problems to work (These problems will not be collected): 3.6, 3.8, 3.10, 3.14, 3.16, 3.18, 3.20, 3.22, 3.24,

3.26, 3.28, 3.30, 3.40, 3.42, 3.44, 3.46, 3.48, 3.50, 3.52, 3.54, 3.58, 3.60, 3.62, 3.64, 3.66, 3.68, 3.70, 3.72, 3.74, 3.76,

3.78, 3.80, 3.82, 3.84, 3.86, 3.88, 3.90, 3.92, 3.94, 3.96, 3.104, 3.110, 3.118, 3.120, 3.126, 3.128, 3.132, 3.134, 3.144

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CHEM 111 Chapter 3 Objectives (Chang 9) Dr. Eric R. Johnson

Know the names and chemical formulas for the following ions: NO 3 –^ NO 2 –^ SO 42 –^ SO 32 –^ PO 43 –^ PO 33 –^ ClO–^ ClO 2 –^ ClO 3 –^ ClO 4 –^ CO 32 – nitrate ion nitrite ion sulfate ion sulfite ion phosphate ion phosphite ion hypo- chlorite ion chlorite ion chlorate ion perchlorate ion carbonate ion Be able to do the following:
1. Define and explain the terms atomic mass, molecular mass, molar mass, mole, and Avogadro’s Number.
2. Calculate the average atomic mass for an element from the naturally occurring isotope masses and their abundances.
3. Know that a mole refers 6.022 x 10^23 (Avogadro’s Number) particles. 5.Use appropriate conversion factors convert the mass of an element or compound to the number of moles and the number of atoms or molecules.
4. Calculate the molecular mass and molar mass of a compound from its molecular formula and a periodic table.
5. Given a molecular formula and a periodic table, calculate the percent by mass for each element in a compound.
6. Given a periodic table and the percent composition by mass for each element in a compound, determine the empirical formula for that compound.
7. Determine the molecular formula of a compound from the empirical formula and the molecular mass.
8. Given the reactants and products of a chemical reaction, write a balanced chemical equation.
Interpret a balanced chemical equation in terms of molecules and moles of reactants and products.
Using a periodic table, do mole-to-mole, gram-to-mole, mole-to-gram, and gram-to-mole-to-mole-to-gram calculations from a balanced chemical equation.
Recognize that one of the reactants in a chemical reaction may be a limiting reagent.
Do limiting reagent calculations like Example 3.15 on p. 102 in Chang.
Distinguish between actual and theoretical yields.
Calculate the theoretical yield for a chemical reaction.
Calculate the % yield for a chemical reaction. Assigned problems to work (These problems will not be collected): 3.6, 3.8, 3.10, 3.14, 3.16, 3.18, 3.20, 3.22, 3.24, 3.26, 3.28, 3.30, 3.40, 3.42, 3.44, 3.46, 3.48, 3.50, 3.52, 3.54, 3.58, 3.60, 3.62, 3.64, 3.66, 3.68, 3.70, 3.72, 3.74, 3.76, 3.78, 3.80, 3.82, 3.84, 3.86, 3.88, 3.90, 3.92, 3.94, 3.96, 3.104, 3.110, 3.118, 3.120, 3.126, 3.128, 3.132, 3.134, 3.

Chemistry 111: Chapter 3 Objectives - Atomic Mass, Ions, and Molar Mass - Prof. P. Coan, Study notes of Chemistry

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