CP1 Chemistry 16-17 Midterm Exam Reviewcollisonchemistry.weebly.com/uploads/3/8/2/4/38246343/16-17chem… · CP1 Chemistry 16-17 Midterm Exam Review Practice Open Response Questions:

CP1 Chemistry 16-17 Midterm Exam Review

Chemistry Midterm Review Exam date: Wednesday, 2/15 during class

The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains questions from the units below. You cannot replace your score with a cumulative exam score

Topics include: Unit One- Matter and Measurement Chapter 2: Properties of matter, Classification, Chemical vs. physical changes Chapter 3: Reading scales, Metric units, Significant Digits, Density Chapter 4: Problem solving techniques, Dimensional analysis Unit Two- Atomic Structure and the Periodic Table Chapter 5: History of atomic models, Atomic structure, Periodic table arrangement, isotopes, ions Sections 7.1 & 7.2: Mole conversions for an element (mass and particles) Chapter 13: Atomic structure, Electron configuration (up to atomic number 20), Lewis dot symbols and valence electrons Chapter 14: Period & Group trends (atomic & ionic radius, ionization energy, electronegativity, reactivity) Section 15.1: Electron configuration of ions Unit Three- Chemical Bonding Ch 6: Types of compounds, properties of compounds, names & formulas of ionic compounds, binary

molecular compounds and acids Sections 7.2 & 7.3: Mole conversions of a compound (mass and particles), % composition based on mass,

empirical and molecular formulas Chapters 15 &16: Ionic & covalent bonding, Lewis structures, bond polarity, shape & polarity of

molecules, attraction between molecules Unit Four- Chemical Reactions Chapter 8: Writing word and formula equations, balancing equations, classifying types of reactions, using

solubility rules to identify states of matter, predicting products Section 19.1: Collision Theory, Rates of reactions and factors affecting rates Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting

reactant , % yield Unit Six- Gases Chapter 12: Properties of Gases (KMT) and factors affecting gas pressure, gas law (combined and ideal),

factors affecting movement of gases, Dalton’s law of partial pressure


Practice Open Response Questions: Unit One- Matter and Measurement 1. How many significant figures are there in each of these numbers?

a. 0.0120 m Three b. 180. Mg Three c. 3050 mL Three Classify the following as an element, compound, heterogeneous mixture, homogeneous mixture (solution):

b. a. Co(s) b. CO(g) c. NaCl(aq) d. oil + water Element Compound Homogeneous Mixture Heterogeneous

Mixture Unit Two- Atomic Structure and the Periodic Table 2. Define an isotope and an ion. Write the nuclear symbol for two isotopes of potassium and an ion of potassium. Isotopes of the same element have the same atomic number but different atomic masses due to a different number of neutrons (5.3)

● Two Isotopes of K: An ion is an atom or group of atoms that has a positive or negative charge (6.1)

● An Ion of K: 3. Give the charge and location in the atom of each of the following particles:

Particle Charge Location in Atom Proton + Nucleus Electron - Outside the nucleus- in orbitals/shells/rings Neutron 0 Nucleus

4. Fill in the following table: Atom or ion Atomic No. Mass No. # p # e # n Avg. atomic mass

Hg

80 201 80 80 121 200.59amu

K

19 40 19 19 21 39.098amu

K+

19 39 19 18 20 39.098amu

Cl

17 35 17 17 18 35.453amu

Cl-1

17 35 17 18 18 35.453amu

Fe+2

26 56 26 24 30 55.847amu

S–2

16 30 16 18 14 32.06amu


Uranium-235 92

235 92 92 143 238.03amu

5.Give the electron dot (Lewis) structures for:

Ba

S–2

K+

C

6.Write the electron configuration (1s22s2p6 etc.) of P: 1s22s22p63s23p3

7.Write the electron configuration of potassium: 1s22s22p63s23p64s1 8.Write the electron configuration of Cl-1: 1s22s22p63s23p6 9.On the Periodic Table, identify: a) noble gases (Grp 18) b) alkali metals (Grp 1) c) halogens (Grp 17) d) transition metals (Grp 3-12) e) metalloids (B, Si, Ge, As, Sb, Te, Po) f) transuranium elements (Lanthanides and Actinides)

10. Define electronegativity. Which elements have the largest electronegativity? the smallest? Why? Electronegativity: the tendency for an atom to attract electrons to itself when it is chemically combined with another element (14.2) F is the most electronegative (higher # of valence electrons and it’s a smaller atom) Fr is the least electronegative (smaller # of valence electrons and it’s a larger atom) 11.Which element in Group 1A has the largest atomic radius and why? Fr (larger number of energy levels) 12.What element in Period 3 has the largest atomic radius and why? Na (it has the lowest number of protons and, therefore, the smallest effective nuclear charge) 13.For the same element, rank in order of size, the neutral element, the cation and the anion. cation < atom < anion


Unit Three- Chemical Bonding 14.What is an ionic bond? What is a covalent bond? Ionic Bond: when electrons are transferred; typically between a metal and a nonmetal Covalent Bond: when electrons are shared between nonmetals 15.Write the correct formulas for the following. Include states of matter when possible (assume room

temp).

a) iron (II) hydroxide b) dihydrogen monoxide c) silver sulfate Fe(OH)2 (s) H2O (l) Ag2SO4 (s)

d) carbon tetrachloride e) ammonium chromate f) potassium sulfide

CCl4 (NH4)2CrO4 (s) K2S (s) 16.Name the following compounds: a) CrCl3 → chromium(III)chloride b) Mg(NO3)2 → magnesium nitrate c) Na2SO3 → sodium sulfite d) PH3 → phosphorus trihydride e) Ba(HCO3)2 → barium hydrogen carbonate f) AlI3 → aluminum iodide 17. Draw electron dot (Lewis) structures, name the shape, and determine if the molecule is polar.

Name Formula Ionic or molecular

Lewis dot structure

Shape (if molecular)

Polarity (if molecular)

Ammonia (Nitrogen

trihydride)

NH3

M

trigonal pyramidal

polar

Sodium Iodide

NaI

I

N/A N/A

Carbon dioxide

CO2

M

linear nonpolar


18. a. What molecular compound (covalent bonding) above would experience the greatest attraction between molecules? Lowest attraction?

Greatest: NH3

Lowest: CO2

b. Which would have a higher boiling point, H2O or CCl4? Explain your answer. H2O → Polar CCl4 → Nonpolar H2O would have a higher boiling point due to the fact that it has stronger intermolecular forces

between molecules. This requires more energy for H2O to move into the gaseous phase. 19. What properties distinguish an ionic solid from a molecular solid? An ionic solid does not melt easily and can conduct electricity in solution. Unit Four: Chemical Reactions 20. Complete and balance the following equations and write states of matter for reactants and products. Label the type of reaction. a. Single Replacement 2 Na (s) + 1 H2O (l) → 1 H2 (g) + 1 Na2O (aq)

b. Decomposition 2KClO3 (aq) → 2KCl (s) + 3O2 (g) c. Single Replacement 2KI + 1 Cl2 → 2KCl (aq) + 1 I2 (s)

d. Double Replacement 1 AgNO3 + 1 NaBr → 1 AgBr (s) + 1 NaNO3 (aq) e. Double Replacement 1 NaCl (aq) + 1 K2O →KCl (aq) + Na2O (aq)

21. Write a chemical equation to show the complete combustion of propane (C3H8) 2 C3H8 + 5O2 → 3CO2 + 4H2O 22. Write the chemical equation with states of matter for the reaction between silver nitrate and sodium

sulfide. 2 AgNO3 (aq) + 1 Na2S (aq) → 1 Ag2S (s) + 2 NaNO3 (aq) 23. Using your solubility rules, identify whether each of the following compounds are soluble or insoluble in water:

a. Na2CO3 b. Pb(NO3)2 c. Mg3(PO4)2 d. AgCl soluble soluble insoluble insoluble

24. How does each of the following affect the rate of reaction?

a. concentration? b. temperature? c. catalyst? a). increasing concentration increases rate b). increasing temperature increases rate c). adding a catalyst increases rate


Unit Five: Chemical Quantities 25. Convert to Moles.

a. 25 g of Al2(CO3)3 b. 189 mL CO2 at STP c. 6.02 x 1022 atoms of Li 0.11 mol 0.00844 mol 0.100 mol

26. Convert to Grams. a. 10. moles of NaOH b. 1.2 L of CO2 c. 3.00 x 1024 molecules of O2

4.0 x 102 g 2.4 g 79.7 g 27. How many moles of hydroxide ions are in 3.5 mol of Ca(OH)2? 7.0 mol OH- 28. Determine the % of Na in NaOH. Show work 57.5 % 29. Determine the empirical formula for a compound composed of 70.0% Fe and 30.0% O. Fe2O3

30. The empirical formula of a compound is CH, its molecular mass is 78. What is its molecular formula? C6H6

Unit Six: Gases 31. What is STP? Equal moles of H2(g) and CO2(g) are in a balloon at STP. Which gas molecules are

moving faster and why? 273 K, 1.0 atm H2 is moving faster because it is a lighter molecule 32. A popcorn kernel contains a hard outer shell, with a water and starch mixture on the inside. Explain, using kinetic molecular theory, why heating the popcorn kernels causes them to pop. In your answer be sure to explain changes to pressure, volume, temperature as the kernel is popped. Water is heated and turned to a gas, temperature increases and velocity of gas particles increase. Particles collide more with kernel, pressure increases, volume increases. 33. A gas occupies 11.2 L at a pressure of 655 kPa and a temperature of 227°C. What will its volume be at STP? 39.5 L 34. If 30 ml of a gas exerts a pressure of 2 atm, what will be the pressure if the volume of the gas is reduced to 20ml? 3 atm 35. An engineer pumps 5.00 mol of carbon monoxide gas into a cylinder that has a capacity of 20.0 L. What is the pressure in atmospheres of CO inside the cylinder at 25°C? 6.1 atm Measurement and Lab 36. How could you test for the presence of oxygen, hydrogen and carbon dioxide? What would the results of the test(s) be? Flame test. Oxygen flares up with no noise; hydrogen creates a popping noise; carbon dioxide causes the flame to go out.

37. Record the measurements, in cm, indicated by arrows A,B, C &D. A _____ B _____ C ______ D ______ 0.122 cm 0.146 cm 0.200 cm 0.255 cm Sample Multiple Choice Problems

1. Which measurement below shows the

temperature to the correct precision?


a. 26.3 oC b. 26 oC c. 26.25 oC d. 26.30 oC 2. The density of copper is known to be 8.96

g/mL. A student’s experimental result shows that the density of her copper cube is 8.79 g/mL. The percent error in this data is___________.

a. 1.93% b. 0.17 % c. 1.90% d. 0.98% 3. Which measurement is written to 4 sig.

figs.? a. 15.20 kg b. 3,500 km c. 0.0003 m d. 0.032 m 4. Which value is the same as 1.52 x 10-3? a. 0.000152 b. 152,000 c. 1520 d. 0.00152 5. Which property is always conserved

during a chemical reaction? a. mass b. volume c. pressure d. solubility

6. A cylinder is weighed empty and with a liquid.

Cylinder with liquid

51.85 g

Cylinder, empty 40.11 g

Volume of liquid in cylinder

7.0 mL

What is the density of the liquid? a. 13 g/mL b. 7.4 g/mL c. 5.7 g/mL d. 1.7 g/mL

7. Which process is a chemical change? a. the melting of ice b. the burning of a candle c. the magnetizing of steel d. the liquifaction of oxygen

8. Which set consists only of elements?

a. Na, Ca, H2 b. H3O+, Cl-, I3- c. NaCl, CH4, Br2 d. H2S, CuCl2, KI

9. How does the average kinetic energy (KE)

of hydrogen molecules compare with that of oxygen molecules when both gases are at 25 oC? a. They have equal KE’s. b. The KE of hydrogen is ¼ as great. c. The KE of hydrogen is 1/16 as great. d. The KE of hydrogen is 4 times as great.

10. The description of the atom as an entity

having most of its mass in a tiny nucleus with electrons moving about in the space of the atom surrounding the nucleus is credited to a. Dalton b. Democritus c. Thomson d. Rutherford

11. How many neutrons are present in an

atom of silver which has a mass number of 108? a. 14 b. 47 c. 61 d. 108

12. A natural sample of element X consists of

about 20% that has an atomic mass of 30 and about 80% with an atomic mass of


31. The mass of element X would be _________________. a. 30.8 amu b. 31.2 amu c. 30.2 amu d. 31.0 amu

13. The electron configuration for

magnesium is a. 1s22s23s3 b. 1s22s22p2 c. [Ar]2s2 d. [Ne]3s2

14. Element 114 should have properties

similar to those of: a. platinum, Pt b. lead, Pb c. astatine, At d. mercury, Hg

15. The name of FeCl3 is

a. iron (III) chloride b. iron chloride c. iron (III) chlorine d. iron trichloride

16. What characteristic of fluorine causes it to

be the most active member of the halogen family?

a. it forms diatomic molecules. b. it has the smallest atomic

radius. c. It has no naturally occurring

isotopes. d. It has seven electrons in its outer

shell.

17. Which set contains only transition elements? a. Elements 11, 12 and 13 b. Elements 15, 16, 17 c. Elements 26, 27, and 28 d. Elements 48, 49, 50

18. Which trend is observed as the atomic

numbers of Group II, the alkaline earth metals, increase?

a. atomic size decreases b. metallic properties decrease c. ionization energy increases d. the tendency to lose electrons

increases

19. Which family of elements always forms

ions with a charge of -1 in compounds? a. halogens b. transition metals c. alkali metals d. alkaline earth metals

20. Which element of Period 3 has the

greatest ionization energy? a. Na b. Al c. P d. Cl

21. Which formula represents and ionic

compound? a. NH3 b. CH4 c. KI d. Cl2O

22. The O-O bond is non-polar, while the H-Cl bond is polar. This is caused by

a. the difference in electronegativities

b. a metal bonding with a nonmetal c. ionic bonding d. the difference in electron affinities

23. What is the correct reading of the

thermometer?

a. 5 oC b. 0.3 oC c. 4.3 oC d. 4oC


24. Expressed to the correct number of significant figures, the sum of two masses is 445.2 grams. Which two masses produce this answer?

a. 210.10 g + 235.100 g b. 210.100 g + 235.10 g c. 210.1 g + 235.1 g d. 210.10 g + 235.10 g

25. A dry mixture of salt and sand could be

separated by a. adding water to the mixture and

filtering b. adding water to the mixture and

evaporating c. heating the mixture to a high

temperature d. cooling the mixture to a low

temperature

26. As the atoms in Period 3 of the Periodic Table are considered from left to right, the atoms generally show

a. an increase in radius and an increase in ionization energy

b. an increase in radius and a decrease in ionization energy

c. a decrease in radius and an increase in ionization energy

d. a decrease in radius and a decrease in ionization energy

27. Which bond is most polar? a. H—F b. H—Br c. H—Cl d. H—I

28. Which formula represents a compound

that is formed by sharing electrons? a. KCl b. CrCl3 c. CaCl2 d. CCl4

29. What is the total number of valence

electrons in a fluorine atom? a. 5 b. 7 c. 2 d. 9

30. What is the total number of neutrons in

an atom of Li-7?

a. 7 b. 3 c. 10 d. 4

31. Which type of matter is composed of two or more different elements that are chemically combined in a definite ratio? a. a solution b. a compound c. a homogeneous mixture d. a heterogeneous mixture

32. Two basic properties of the gas phase are

a. definite shape, definite volume b. definite shape, indefinite volume c. indefinite shape, definite volume d. indefinite shape, indefinite volume

33. Which of the following is the correct

electron dot diagram for water? A

34. Which of the following is the correct electron dot diagram for carbon dioxide? C

35. Which element has the electron configuration below?

a. V b. Ca c. P d. As e. Se 39. Which of the following is the electron configuration of O-2?

F. 1s22s22p6


40. Which Lewis dot notation for atoms and ion is is correct for the reaction of the formation of calcium phosphide from calcium and phosphorus? E

41. How many unshared pairs of electrons

are around the central nitrogen atom in a Lewis dot diagram of NH3? a. one b. two c. three d. four

42. Which Lewis dot diagram below is incorrect? B

43. The ability of carbon to attract electrons

is a. greater than that of nitrogen, but

less than that of oxygen b. less than that of nitrogen, but

greater than that of oxygen c. greater than that of nitrogen and

oxygen d. less than that of nitrogen and

oxygen

44. Which statement best describes the substance that results when electrons are transferred from a metal to a nonmetal?

a. it contains ionic bonds and has a low melting point

b. it contains ionic bonds and has a high melting point

c. it contains covalent bonds and has a low melting point

d. it contains covalent bonds and has a high melting point


45. Which statement explains why the radius of a lithium atom is larger than the radius of a lithium ion?

a. Metals lose electrons when forming an ion.

b. Metals gain electrons when forming an ion.

c. Nonmetals lose electrons when forming an ion.

d. Nonmetals gain electrons when forming an ion.

46. The atoms of the elements in Group II,

have the same a. mass number b. atomic number c. number of protons d. number of valence electrons

47. Which element has the highest electrical

conductivity? a. Mg b. He c. H d. Cl

48. The number of significant digits in

0.013060 is a. 7 b. 4 c. 5 d. 6

49. 2.17 + 4.32 + 401.278 + 21.821 is equal to

a. 430 b. 429.589 c. 429.59 d. 429.590

50. 13.0 x 12.50 = a. 162 b. 163 c. 162.5 d. none of these

51. Which of the following can be separated

only by chemical means? a. elements b. compounds c. homogenous mixtures d. b and c only e. a and b only

52. Which of the following is a chemical change? a. evaporation of water b. distillation of water c. freezing of water d. forming hydrogen and oxygen from water

53. The statement which describes a physical

property of the element oxygen is a. oxygen supports the burning of

paper b. oxygen is needed for the rusting of

iron c. oxygen must be present for food to

decay d. oxygen has a density of 1.43

grams per liter e. oxygen is a component of water

54. Only a physical change takes place in

a. producing water by burning hydrogen in air

b. breaking water into its elements by an electric current (electrolysis)

c. change water into ice by lowering its temperature

55. Three different observers measure the

melting temperature of a substance and agree on the same value, but the value they obtain does not agree with the accepted value. Their measurements can be described as a. both accurate and precise b. precise, but not accurate c. neither accurate nor precise d. accurate but not precise


56. In general, when elements combine chemically to form compounds

a. they retain all their original properties

b. a mixture results c. new substances with new and

different properties are formed d. solutions are formed

57. What is the mass number of an ion of

potassium, K+, with 18 electrons, 19 protons and 20 neutrons? a. 36 b. 37 c. 38 d. 39

58. What is the total number of atoms

contained in 2.00 moles of nickel? a. 58.9 b. 118 c. 6.02 x 1023 d. 1.20 x 1024

59. What is the formula for aluminum

acetate? a. AlC2H3O2 b. Al3C2H3O2

c. AlC6H9O6 d. Al(C2H3O2)3

60. Given the unbalanced equation: Al + O2→ Al2O3 When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients? a. 9 b. 7 c. 5 d. 4

61. What is the empirical formula of the

compound whose molecular formula is P4O10?

a. PO b. PO2 c. P2O5 d. P8O20

62. What is the molar mass of K2CO3? a. 138 g b. 106 g c. 99 g d. 67 g

63. What is the percent by mass of oxygen in magnesium oxide, MgO?

a. 20% b. 40% c. 50% d. 60%

64. A compound is 86% carbon and 14%

hydrogen by mass. What is the empirical formula for this compound?

a. CH b. CH2 c. CH3 d. CH4

65. What is the mass in grams of 3.0 x 1023

molecules of CO2? a. 22 g b. 44 g c. 66 g d. 88 g

66. What is the percent by mass of water in the hydrate Na2CO3 * 10H2O (formula mass = 286)?

a. 6.89% b. 14.5% c. 26.1% d. 62.9%

1) All of the following are physical changes except: a. water boiling b. natural gas burning c. table salt dissolving d. melting silver 2) Which statement is true about the law of conservation of mass as applicable to a chemical reaction? a. Energy is not created nor destroyed. b. Mass can be destroyed through the evolution of a gas. c. The number of molecules of reactants equals the number of molecules of products. d. The mass of reactants must equal the mass of the products.


3) Elements on the right side of the periodic table become more active as we move a. downward because the atoms get larger b. downward because the atoms get smaller c. upward because the atoms get larger d. upward because the atoms get smaller 4) Al3+ is caused by a. a gain of 3 protons by Al b. a gain of 3 electrons by Al c. the sharing of 3 electrons by Al d. the loss of 3 electrons by Al 5) The element with the electron configuration 1s22s22p63s23p3 is a. Al c. Si b. Mg d. P 6) The electron configuration for the Na+ ion is a. 1s22s22p63s13p3 c. 1s22s22p6 b. 1s22s22p63s1 d. 1s22s22p63s2 7) What is the mass of a solid whose density is 5.60 g/cm3 and volume is 10.0 cm3? a. 0.560 g b. 1.79 g c. 15.6 g d. 56.0 g 8) Isotopes of an element differ in their number of: a. neutrons b. protons c. electrons d. electron shells 9) A neutral atom with atomic number 16 and mass number 34 contains: a. 16 protons, 18 neutrons and 16 electrons b. 16 protons, 34 neutrons and 16 electrons c. 34 protons, 16 neutrons and 16 electrons d. 16 protons, 16 neutrons and 18 electrons 10) Which of the following lists the element, number of protons and number of electrons correctly? a. H, 1 proton, 1 electron b. He, 2 protons, 4 electrons c. C, 6 protons, 12 electrons d. Ne, 10 protons, 10.179 electrons

11) In which of the following is the number of neutrons correctly computed? a. C-13 has 13 neutrons b. N-15 has 7 neutrons c. O-18 has 10 neutrons d. Zn-70 has 100 neutrons 12) Which of the following elements would react most similar to chlorine? a. sulfur b. argon c. carbon d. bromine 13) When an atom forms a cation, it: a. gains protons and becomes positively charged. b. loses electrons and becomes positively charged. c. gains electrons and becomes negatively charged. d. loses protons and becomes negatively charged. 14) In which list are the charges of each ion shown correctly? a. Li+,Na2+,K3+ b. Na+,Mg2+,Al3+ c. N3+,O2+,F+ d. N-,O2-,F3- 15) Which of the following is a molecular compound? a. NaCl b. MgSO4 c. N2O d. Al2O3 16) What is the formula for ammonium sulfate? a. NH4S b. NH4SO4 c. (NH4)2SO4 d. NH4(SO4)2 17) Which of the following has the correct formula for the name given? a. PbCO3, lead (II) carbonate b. Fe2O3, iron (II) oxide c. PCl3, phosphorous chloride d. Li2S, dilithium monosulifde 18) What is the name for P4O10? a. phosphorous oxide b. tetraphosphorous decaoxygen c. tetraphosphorous decaoxide d. phosphorous decaoxide


19) What are the coefficients, listed in order, of the following reaction when it is properly balanced?

C3H6(g) + O2(g) → CO(g) + H2O(g) a. 1,3,3,3 b. 3,2,1,2 c. 9,2,2,3 d. 1,2,3,3 20) What are the coefficients, listed in order, of the following reaction when it is properly balanced?

F2(g) + Al2O3(aq) → AlF3(aq) + O2(g) a. 3,1,2,2 b. 1,1,2,3 c. 2,2,4,3 d. 6,2,4,3 21) The reaction below is an example of:

F2(g) + Al2O3(aq) → AlF3(aq) + O2(g) a. combination b. single-replacement c. decomposition d. double-replacement 22) What are the coefficients, listed in order, of the following reaction when it is properly balanced? hydrochloric acid + magnesium hydroxide → magnesium chloride + water a. 1,1,1,1 b. 2,1,1,2 c. 1,2,2,1 d. 1,2,1,2 23) Which of the following is a property of an ionic compound? a. relatively low melting point b. conducts electricity in the solid state c. relatively low boiling point d. conducts electricity when dissolved in water 24) Which of the following is true of molecular compounds? a. relatively low melting point b. conducts electricity in the solid state c. always contain ionic bonds d. conducts electricity when dissolved in water 25) How many significant figures are in the measurement 0.0405 g? a. 2 b. 3 c. 4 d. 5

27 ) How many significant figures are in the measurement 120,000 cm? a. 2 b. 3 c. 4 d. 5 28) A student used a balance and a graduated cylinder to collect the following data: Sample mass 10.23 g Volume of water 20.0

mL Volume of water + metal sample 21.5

mL What is the calculated density of the metal? a. 0.512 g/cm3 b. 0.476 g/cm3 c. 6.8 g/cm3 d. 2.1 g.cm3 30) What is the reading on the graduated cylinder below?

a. 35 mL b. 36 mL c. 35.0 mL d. 36.0 mL 31) What is the mass of a solid whose density is 5.60 g/cm3 and volume is 10.0 cm3? a. 0.560 g b. 1.79 g c. 15.6 g d. 56.0 g 32) What is the gram formula mass of sodium phosphate? a. 70 g/mol b. 116 g/mol c. 164 g/mol d. 257 g/mol 33) A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula? a. MgN b. Mg3N2 c. Mg2N3 d. Mg3N


34) Which of the following is NOT an empirical formula? a. CO2 b. C6H12O c. C6H12O6 d. Al3O2 35) What is the percentage of water in sodium tungstan dihydrate, Na2WO4 • 2 H2O?

a. 5.77% b. 0.109% c. 36.0% d. 10.9% 36) Which of the following products is insoluble? a. K2SO4 b. NaCl c. BaCl2 d. Na2CO3 37) What is the percentage, by mass, of sodium in Na2S2O3? a. 29.1% b. 40.5% c. 30.4% d. 28.5%

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