Chemistry Midterm Exam Review



Chemistry Semester Exam Review

Complete all problems on notebook paper. Transfer your final answers to the answer sheet.

Measurements and Calculations

Significant Figures – adding, subtracting, multiplying, dividing

Scientific Notation - adding, subtracting, multiplying, dividing

Metric Conversions

Dimensional Analysis

Temperature Conversions

Density – D=m/V, V=LWH, V=(r2h, V=Vf - Vi

Determine the number of significant figures in the following numbers.

a. 1 SF b. 2 SF c. 4 SF d. 6 SF e. 10 SF

1. 0.0000787690 g d

2. 900000 km a

3. 0.009001 mm c

4. 9.100 cg c

Record your answer with the correct number of significant figures and units.

5. 45.6 g + 3.59 g

a. 49.19 g b. 49.0 g c. 49.2 g d. 49.20 g

6. 0.00134 mL - 0.00023 mL

a. 0.00111 mL b. 11 mL c. 0.0011 mL d. 0.00157 mL

7. (56.2 cm)(1.234 cm)

a. 69.3 cm2 b. 69.4 cm2 c. 69.3508 cm2 d. 69.35 cm2

8. (3.20 km2)/(4.0 km)

a. 13 km b. 8 km c. 0.80 km d. 2.56 km

Convert the following numbers from scientific notation to ordinary notation.

9. 3.02 x 10-3 g

a. .302 x 10-3 g b. 3.02 g c. 0.00302 g d. 3020 g

10. 5.791 x 105 m

a. 579100 m b. 5.791 m c. 0.00005791 m d. 57910 m

Convert the following numbers from ordinary notation to scientific notation.

11. 4560 cm

a. 456 x 103 cm b. 4.56 x 103 cm c. 4.56 x 10-3 cm d. 4.56 cm

12. 0.0076 g

a. 7.6 x 10-3 g b. 7.6 x 103 g c. 76 x 10-3 g d. 0.0076 x 10-3 g

Perform the following calculations.

13. How many kilograms are in 234 mg?

a. 234000 kg b. 234 kg c. 0.000234 kg d. 0.234 kg

14. How many micrometers are in 0.000325 km?

a. 325 μm b. 325000 μm c. 0.325 μm d. 0.000325 μm

15. The Density of Mercury is 13.0 g/mL. If you have 24.3 mL of Mercury, how much does it weigh?

a. 316 g b. 315.9 g c. 0.535 g d. 1.87 g

16. A cube of wood that weighs 16.5 g measures 24.21 cm by 1.45 cm by 7.34 cm. What is the density of the wood?

a. 7.25 g/cm3 b. 0.0640 g/cm3 c. 258 g/cm3 d. 4250 g/cm3

Matter

Chemical vs. Physical Properties

Chemical vs. Physical Changes

Elements and Compounds

Mixtures and Solutions

Classify the following as a) chemical property or b) physical property.

17. Color b) physical property

18. Flammability a) chemical property

19. Solubility b) physical property

Classify the following as a) chemical change or b) physical change.

20. tearing paper b) physical change

21. burning wood a) chemical change

22. boiling water b) physical change

Classify the following as an a) element or a b) compound.

23. Phosphorus a) element

24. carbon dioxide b) compound

25. water b) compound

Classify the following as a) mixture or b) pure substance.

26. a multivitamin tablet a) mixture

27. distilled water b) pure substance

28. tap water a) mixture

Classify the following as a) homogeneous mixture or b) heterogeneous mixture.

29. chunky peanut butter b) heterogeneous mixture

30. a solution of copper (II) sulfate a) homogeneous mixture

31. a bag of trail mix b) heterogeneous mixture

Chemical Foundations: Elements, Atoms, and Ions

Dalton’s Atomic Theory

Subatomic Particles – Protons, Neutrons, Electrons

History of the Atom

Isotopes

Atomic Numbers and Mass Numbers

Cation vs. Anion

Ratio of Atoms

Nuclear chemistry

Give the symbols for the following elements

a. B b. Be c. H d. He

32. Beryllium b. Be

33. Boron a. B

34. Helium d. He

35. Hydrogen c. H

Write the formula for the compound containing

36. a two to three ratio of iron to oxygen

a. Fe2O3 b. I2O3 c. Fe3O2 d. I3O2

37. six carbon, twelve hydrogen and six oxygen

a. CH2O b. C6H12O6 c. C6H6O6

Name the scientist responsible for the following. Put in order (c, b, a)

a. Gold Foil Experiment b. Plum Pudding Model c. Atomic Theory

38. John Dalton c. Atomic Theory (Solid Sphere Model)

39. Ernest Rutherford a. Gold Foil Experiment

40. JJ Thomson b. plum pudding model

Determine the number of protons, neutrons, and electrons in the following.

41. 41Ca

a. 41p, 41n, 41e b. 20p, 20n, 20e c. 20p, 41n, 20e d. 20p, 21n, 20e

42. 60Co+3

a. 27p, 60n, 27e b. 27p, 33n, 24e c. 24p, 41n, 27e d. 27p, 33n, 30e

43. 6Li+1

a. 6p, 6n, 7e b. 3p, 3n, 3e c. 3p, 3n, 2e d. 6p, 2n, 3e

44. 31P-3

a. 15p, 31n, 15e b. 15p, 16n, 15e c. 15p, 16n, 18e d. 31p, 15n, 17e

Complete the following nuclear equations by supplying the missing particle. Classify the type of decay

a.[pic], alpha decay b. [pic], beta decay c. [pic], alpha decay d. [pic], beta decay

45. [pic] a.[pic], alpha decay

46. [pic] a.[pic], alpha decay

47. [pic] d. [pic], beta decay

48. [pic] d. [pic], beta decay

Average Atomic Mass

Average Atomic Mass - the weighted average of the masses of the isotopes of

the element.

Average Atomic Mass = ([(isotope mass)(percent abundance)]

To solve for percent abundance assign the first isotope x and the second isotope equal to 100% - x.

49. There are two naturally occurring isotopes of rubidium: 85Rb, which has a mass of 84.91 amu and 87Rb, which has a mass of 86.92 amu. The atomic mass of rubidium is 85.47 amu. What is the percent abundance of each of the isotopes?

a. 85Rb = 72.1 %, 87Rb = 27.9% c. 85Rb = 27.9%, 87Rb = 72.1%

b. 85Rb = 85%, 87Rb = 15% d. 85Rb = 97.7%, 87Rb = 2.3%

85.47 amu * 100% = (84.91 amu * x) + [86.92 amu * (100% - x)]

8547 amu% = 84.91amu*x + 8692 amu% - 86.92amu*x

-145 amu% = -2.01amu*x

x = 72.1% 85Rb

100 – 72.1% = 27.9% 87Rb

50. If element X consists of 78.8% of atoms with a mass of 24.0 amu, 10.1% of atoms with a mass of 25.0 amu, and 11.2% of the atoms with a mass of 26.0 amu, what is the atomic mass of element X?

a. 25.0 amu b. 24.3 amu c. 33.3 amu d. 2434 amu

x * 100% = (24.0amu*78.8%) + (25.0amu*10.1%) + (26.0amu*11.2%)

x*100% = 1890 amu% + 253 amu% + 291 amu%

x*100% = 2430 amu%

x = 24.3 amu

Semester Exam Review Part 2

Complete all problems on notebook paper. Transfer your final answers to the answer sheet.

Nomenclature

Periodic Table

Naming Compounds

Ionic, Molecular, Acids

Writing Formulas for Compounds

Ionic, Molecular, Acids

51. Write the name for the following compounds.

a. AuBr3 gold (III) bromide

b. Co(CN)3 cobalt (III) cyanide

c. HNO2 nitrous acid

d. Mg3(PO4)2 magnesium phosphate

e. HCN hydrocyanic acid

f. B2H6 diboron hexahydride

g. Ag2SO4 silver sulfate

h. H2S hydrosulfuric acid

i. Be(OH)2 beryllium hydoxide

j. SF6 sulfur hexafluoride

k. CuO copper (II) oxide

52. Write the formula for the following compounds.

l. barium peroxide BaO2

a. tetraphosphorus decoxide P4O10

b. cesium sulfite Cs2SO3

c. manganese (II) acetate Mn(C2H3O2)2

d. sodium hypochlorite NaClO

e. nitric acid HNO3

f. tricarbon hexahydride C3H6

g. hydronitric acid H3N

h. zinc nitrate Zn(NO3)2

i. cobalt (III) hydroxide Co(OH)3

j. pentanitrogen octoxide N5O8

Modern Atomic Theory

atomic theory

electron configuration

orbital diagram

periodic table trends

Ionization energy

Electron affinity

Atomic radius

electronegativity

53. Name the element that corresponds to each of the following electron configurations.

a. 1s22s22p2 carbon

b. 1s22s22p63s23p4 sulfur

c. 1s22s22p63s23p64s23d5 Mn

d. 1s22s22p6 Ne

54. Write the electron configurations for the following elements.

a. Potassium 1s22s22p63s23p64s1

b. Barium 1s22s22p63s23p64s23d104p65s24d105p66s2

55. Write the orbital diagram for the following elements.

a. Bromine

1s (( 2s(( 2p (( (( (( 3s (( 3p (( (( (( 4s (( 3d(( (( (( (( (( 4p (( (( (

b. iron

1s (( 2s(( 2p (( (( (( 3s (( 3p (( (( (( 4s (( 3d(( ( ( ( (

56. Arrange the following elements in order of increasing atomic radius.

a. Cl, Mg, P, Na, Al Cl, P, Al, Mg, Na

b. Rb, Na, Cs, Li, K Li, Na, K, Rb, Cs

57. Arrange the following elements in order of increasing ionization energy.

a. Cl, Mg, P, Na, Al Na, Mg, Al, P, Cl

b. Rb, Na, Cs, Li, K Cs, Rb, K, Na, Li

58. Arrange the following elements in order of increasing electron affinity.

a. Cl, Mg, P, Na, Al Na, Mg, Al, P, Cl

b. Rb, Na, Cs, Li, K Cs, Rb, K, Na, Li

59. Arrange the following elements in order of increasing electronegativity

a. Cl, Mg, P, Na, Al Na, Mg, Al, P, Cl

b. Rb, Na, Cs, Li, K Cs, Rb, K, Na, Li

Chemical Bonding

Lewis structures

VSEPR

Linear

Bent

Trigonal planar

Trigonal pyramid

tetrahedral

polarity

60. Draw Lewis structures for the following:

a. Silicon[pic]

b. Potassium phosphide

[pic]

c. Nitrogen triiodide [pic]

61. Predict the shape and polarity of the following molecules

a. SiS2 linear, non-polar

b. OBr2 bent, polar

c. COCl2 trigonal planar, polar (because of O)

d. PH3 trigonal pyramid, polar

e. CF4 tetrahedral, non-polar

Chemical Composition

Moles

Avogadro’s Number

Molar Mass

Percent Composition

Empirical Formula

Molecular Formula

62. Calculate the molar mass of magnesium phosphate. Mg3(PO4)2

24.3 (3) + 31.0 (2) + 16.0 (8) = 262.9 g/mol

63. How many moles are in 7.23 grams of strontium oxide? SrO

7.23gSrO x 1 mol SrO = 0.0698 mol SrO

103.6g SrO

64. How many moles are in 3.02 x 1023 atoms of zinc?

3.02E23 atoms Zn x 1 mol Zn = 0.502 mol Zn

6.02E23 atoms Zn

65. How many grams are in 7.2 x 1046 molecules of copper (II) sulfate?

7.2E46 molec CuSO4 x 1 mol CuSO4 x 159.6g CuSO4 = 1.9x1025g CuSO4

6.02E23 molec 1 mol CuSO4

66. How many grams are in 1.00 moles of sodium oxalate?

1.00 mol Na2C2O4 x 134.0g Na2C2O4 = 134 g Na2C2O4

1 mol Na2C2O4

67. How many particles are in 3.45 grams of silver acetate?

3.45g AgC2H3O2 x 1 mol AgC2H3O2 x 6.02E23 part AgC2H3O2 = 1.24x1022 part AgC2H3O2

166.9 g AgC2H3O2 1 mol AgC2H3O2

68. How many molecules are in 1.26 x 1018 amu of LiCl?

1.26E18 amu LiCl x 1.66E-24g LiCl x 1 mol LiCl x 6.02E23 molec LiCl =2.97x1016molec LiCl

1 amu LiCl 42.4g LiCl 1 mol LiCl

69. Calculate the percent composition for each element in ammonium phosphate. NH4+ PO4 -3 ( (NH4)3PO4

14.0(3) + 1.0 (12) + 31.0 + 16.0(4) = 149.0 g/mol

%N = 14.0(3) / 149.0 * 100 = 28.2 %N

%H = 1.0(12) / 149.0 * 100 = 8.1 %H

%P = 31.0 / 149.0 * 100 = 20.8 %P

%O = 16.0(4) / 149.0 * 100 = 43.0 %O

70. Calculate the empirical formula for the compound that is 49.48 % carbon, 28.87 % nitrogen, 16.49 % oxygen, and 5.15 % hydrogen.

49.38gC x 1 mol C = 4.12 mol C / 1.03 mol = 4

12.0 g C

28.87gN x 1 mol N = 2.06 mol N / 1.03 mol = 2

14.0 g N

16.49gOx 1 mol O = 1.03 mol O / 1.03 mol = 1

16.0 g O

5.15gH x 1mol H = 5.15 mol H / 1.03 mol = 5

1.0 g H

C4N2OH5

71. Calculate the molecular formula for the compound that is 71.65 % chlorine, 24.27 % carbon, and 4.07 % hydrogen. The molar mass is 247.5 g/mol.

71.65gCl x 1 mol Cl = 2.02 mol Cl / 2.02 mol = 1

35.5 g Cl

24.27gC x 1 mol C = 2.02 mol C / 2.02 mol = 1

12.0 g C

4.07gHx 1 mol H = 4.07 mol H / 2.02 mol = 2

1.0 g H

ClCH2

247.5 g/mol = 5 Cl5C5H10

49.5 g/mol

Chemical Reactions

Reactants and Products

Symbols in Equations

Balancing Equations – Use of Coefficients

Balance the following equations.

a. ___ C2H5OH + _3_ O2 ( _2_ CO2 + _3_ H2O

b. ___ CaC2 + _2_ H2O ( ___ Ca(OH)2 + ___ C2H2

c. ___ Cl2 + _2_ KI ( _2_ KCl + ___ I2

d. _4_ NH3 + _3_ Cl2 ( _3_ NH4Cl + ___ NCl3

e. ___ PbCl2 + ___ K2SO4 ( ___ PbSO4 + _2_ KCl

72. Write and balance the following equations include state symbols.

a. Solid iron (III) oxide is heated strongly in carbon monoxide gas, it produces elemental iron and carbon dioxide gas.

Fe2O3 (s) + 3 CO (g) ( 2 Fe (s) + 3 CO2 (g)

b. Acetylene gas (C2H2) is burned in air to produce carbon dioxide gas and water vapor.

2 C2H2 (g) + 5 O2 (g) ( 4 CO2 (g) + 2 H2O (g)

73. Write word equations for the following reactions.

a. 2Ag (s) + H2S (g) ( Ag2S (s) + H2 (g)

Solid silver reacts with hydrosulfuric acid to produce solid silver sulfide and hydrogen gas.

b. 2FeO (s) + C (s) ( 2Fe (l) + CO2 (g)

Solid iron (II) oxide reacts with solid carbon to produce molten (liquid) iron and carbon dioxide gas.

Reactions in Aqueous Solutions

Solubility Rules

Activity Series

Writing Molecular, Complete Ionic, and Net Ionic Equations

Single Displacement Reactions

Double Displacement Reactions

Combustion Reactions – Complete and Incomplete

Decomposition Reactions

Synthesis Reactions

74. Determine whether the following compounds are soluble or insoluble.

a. sodium acetate soluble

b. silver hydroxide insoluble

c. lithium sulfide soluble

d. colbalt (II) sulfate soluble

75. Predict the products and balance the following equations. Include physical state symbols.

a. 2 C4H10 (g) + 13 O2 (g) ( 8 CO2 (g) + 10 H2O (g)

combustion

b. SO2 (g) + H2O (l) ( H2SO3 (aq)

synthesis

c. Ca (s) + H2O (l) ( CaO (s) + H2 (g)

single displacement, redox

d. MgSO3 (aq) ( MgO (s) + SO2 (g)

decomposition

e. AgC2H3O2 (aq) + KBr (aq) ( AgBr (s) + KC2H3O2 (aq)

Double displacement, precipitation

76. Classify 76a-e classify the reactions in as many ways as possible.

-----------------------

Si

-3

K + K + K + P ( 3 K+ P

N

I

I

I

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