CP Chemistry Midterm Study guideName:______

Part I: Vocab (define the following terms)

Matter

Compound

Element

Density

Heterogeneous mixture

Homogeneous mixture

Filtration

Chromatography

Distillation

Chemical property / change

Physical property / change

Atomic number

Mass number

Isotope

Percent error

Noble gas

Halogen

Metal

Metalloid

Ductile

Malleable

Ion

Polyatomic ion

Oxyanion

Binary compound

Diatomic gas (O2,N2,F2,I2,Cl2,Br2)

Synthesis reaction

Decomposition reaction

Combustion reaction

Single replacement reaction

Double replacement reaction

meniscus

Part II: Describe the following:

  1. Atomic theory
  2. Atomic structure (use protons, neutrons, electrons)
  3. Law of conservation of mass
  4. The difference between an observation, hypothesis and conclusion

Part III: Know the following formulas / information

  1. Density = grams / volume
  2. Percent error = error X 100%

Accepted value

3. When adding or subtracting, exponents must be the same. (10x)

4. When multiplying, exponents are added (103 X 105 = 108)

5. When dividing, exponents are subtracted (105 ÷ 103 = 102)

6. When multiplying or dividing, the answer should have the same number of significant figures as the value with the least number of significant figures.

7. When adding or subtracting: 5.06 + 4.3 = 9.3 (cannot go past the tenths place because the value 4.3 does not go past the tenths place.

8. a. How to draw a best fit line.

b. regression equation: y = mx + b (y = dependent variable, x = independent variable, m= slope, b = y intercept)

9. When measuring, one estimated value is allowed.

Part IV: Solve the following problems

  1. A 5mL sample of water has a mass of 5g. What is the density of water?
  2. A cube of aluminum with volume = 5 cm3 has a mass of 20g. What is the density of aluminum?
  3. What is the volume of a sample that has a mass of 20g and density of 4 g/mL?
  4. Express the following in scientific notation:
  1. 900
  2. 6,500,000
  3. 0.00000086
  1. How many significant figures in the following numbers?
  1. 304.0
  2. 0.0067
  3. 604,000
  4. 4.00500 X 108
  5. 0.03005
  1. 3 X 102 + 4 X 103 =
  2. 5 X 10-4 - 7 X 10-2 =
  3. 3 X 107 X 9 X 103 =
  4. 4.5 X 10-4 ÷ 9.0 X 103 =
  5. Three measurements are taken: 34.5m, 38.4m, 35.3m. The actual measurement is 36.7m. What are the percent errors for the measurements taken?
  1. 5g of tin react with hydrochloric acid, producing 8.1g of tin chloride and hydrogen gas. How much hydrochloric acid reacted?
  1. Compound I contains 5.63g tin and 3.37 g chlorine. Compound II contains 2.5g tin and 2.98g chlorine. Are the compounds the same?
  1. Silver has two naturally occurring isotopes. Ag-107 has a relative abundance of 51.82% and a mass of 106.9 amu. Ag-109 has a relative abundance of 48.18% and a mass of 108.9 amu. Calculate the atomic mass of silver.
  1. What is the atomic number for the following elements?

a. at atom with 37 electrons

b. an atom with 72 protons

c. an atom with 1 electron

d. an atom with 6 neutrons and a mass number of 12

15. Predict the result of the following reactions using the activity series:

a. Al + FeCl3

b. Br2 + 2LiI

c. Cu + MgSO4

16. How many electrons do the following ions have:

a. Mg+2

b. Na+1

c. O-2

d. N-3

17. What are the products of the following double replacement reactions?

a. LiI + AgNO3

b. BaCl2 + K2CO3

18. Calculate the mass in grams of 2.22 mol of Ti.

19. How many moles of Co are in 7.65g?

20. What is the molar mass of zinc oxide (ZnO)?

21. A compound is analyzed and found to have 69.58% Ba, 24.32% O, and 6.09% C. What is the compound’s empirical formula?

22. . A compound is found to have 26.76% C, 2.21% H and 71.17% O.

a. What is it’s empirical formula?

b. It has a molar mass of 90.04 g/mol. What is its molecular formula?

23. What is the empirical formula for glucose, C6H12O6?

24. How many atoms are in the following:

a. 1mol of Zn

b. 3mol of O2

c. 2mol of silver

25. How many moles are in the following?

a. 40g of gold

b. 5 g of NaCl

c. 6.89g of CuSO4

26. Analysis of a hydrate of Iron (III) chloride revealed that in a 100.00g sample of the hydrate, 6.00g is anhydrous iron (III) chloride and 4.00g are water. Determine the formula and name of the hydrate.

27. Consider the hydrate: CuSO4 5H2O

a. What is the formula mass?

b. What is the percent water by mass?

c. How many grams of water would be found in 470.0g of this hydrate?

d. How many grams of sulfur will combine with 6.5 g of copper to make this hydrate?

28. Examine the following reaction:

4 A + 13 B 5 C + 17 D

If 0.87 moles of A react, fine the number of moles of B, C, and D.

29. Balance the following equation:

______NaOH + _____ CuCl2 ______NaCl + ______Cu(OH)2

a. How many grams of copper (I) chloride will react with 5.67g of NaOH?

b. How many grams of NaCl will be produced?