CHM2045 SI Midterm Review

CHAPTER 1

100

List all the noble gases elements (name and symbol).

What is:

He - Helium

Ne - Neon

Ar - Argon

Kr – Krypton

Xe – Xenon

Rn – Radon

200

What are the 2 types of mixtures? How do they differ? How are they similar? Give 2 examples of each mixture type.

What is:

Homogenous: Uniform composition (single phase) Examples: saltwater, air

Heterogenous: Non-uniform composition   Examples: sand, oil and water

300

List examples of chemical and physical changes. What are the differences between them?

What is:

Physical changes do not entail any changes in the chemical composition of the material, while chemical changes do. Examples physical: phase changes, like evaporation or melting. Examples chemical: burning firewood, rusting. (Think, does this change affect the composition of the material?)

400

570.0 m/s → mi/hr 

(Conversion factor: 1 mi = 1.609 km)

What is:

1275 mi/hr

500

725 μg/mm3 → g/mL

What is:

0.725 g/mL

CHAPTER 2

100

Write the name from the formula:

SF₆

KI

FeCrO₄

What is:

Sulfur Hexafluoride

Potassium Iodide

Iron (II) Chromate

200

Write the chemical formula:

Lead (II) Oxide

Diphosphorus Pentoxide

Aluminum Oxide

What is:

PbO

P₂O₅

Al₂O₃

300

Determine the amount of molecules in 650.0 grams of potassium oxide.

What is:

4.156*10^24 molecules K₂O

400

Nitrogen is made up of 2 isotopes, N-14 and N-15. Given that nitrogen's atomic weight is 14.007, what is the percent abundance of each isotope?

What is:

99.3% for N-14

0.7% for N-15

500

A compound is found to be 64.82 % carbon, 21.59% oxygen and 13.59 % hydrogen. In a separate experiment, it was found the molar mass of the compound was 222.1 g/mol. 

a. What is the empirical formula for this compound?

b. What is the molecular formula for this compound?

What is:

a. C₄H₁₀O

b. C₁₂H₃₀O₃

CHAPTER 3

100

Is water an acid or a base? What is the special case called for water?

What is:

Amphiprotic

200

Which ion is oxidized and which ion is reduced?

CO₃^2-+2H⁺ → CO₂+H₂O

What is:

This is not a redox reaction because the oxidation states of all the ions remain the same.

300

Write the balanced equation of iron (III) sulfate reacting with potassium oxide.

What is:

Fe₂(SO₄)₃ + 3K₂O -> 3K₂SO₄ + Fe₂O₃

400

Write the complete ionic equation for the reaction of lead (II) nitrate and potassium iodide.

What is:

Pb²⁺ (aq) + 2I^- (aq) + 2K⁺ + 2NO₃^- ->  PbI₂ (s) + 2K⁺ + 2NO₃^-

500

Write the net ionic equation for the reaction of sodium chloride and silver nitrate.

What is:

Cl^- (aq) + Ag⁺ (aq)  ->  AgCl (s)

CHAPTER 4

100

The hyrdonium ion concentration of a solution is 6.52*10^-7.What is the pH of the solution? Is the solution acidic or basic?

What is:

6.19

Acid

200

0.4 moles of sodium phosphate was added to 300 mL of solution. What is the concentration of sodium ions in the solution?

What is:

[Na⁺]=4.0 M

300

Copper (II) Chloride reacts with Sodium Fluoride. If 50.0 g of sodium fluoride produces 50.0 g of sodium chloride, what is the percent yield?

What is:

71.8%

400

650.0 grams of beryllium phosphate reacts with 700.0 grams chromium (IV) fluoride.

i) How many grams of beryllium fluoride will be produced?

ii) What's the limiting reactant?

What is:

i) 422.5 g BeF₂ will be produced

ii) Beryllium phosphate is the limiting reactant

500

What volume (in mL) of 0.603 M iron (II) nitrate will completely react with a 35.0 mL of 0.212 M magnesium bromide?

What is:

12.3 mL