Final Assessment

CHEMISTRY I

FINAL ASSESSMENT

Indicate the letter of the best answer on your answer sheet.

Objective 1.01: Design, conduct and analyze investigations to answer questions related to chemistry.

Objective 1.02: Evaluate reports of scientific investigations from an informed scientifically-literate viewpoint.

Objective 1.03: Evaluate experimental designs with regard to safety.

1. Which of the following is a qualitative measurement?

a. 27.0g b. 312 m c. blue d. 523 ml

2. In the chemistry lab, chemicals that you are finished working with should be —

poured into the sink
returned to their original containers
mixed together and dumped in a designated container

d. disposed of as directed by your teacher

3. For an experiment in which you are determining the freezing point of an unknown chemical, you record

the temperature every minute for 20 minutes. In this example, time is the —

control
dependent variable

c. independent variable

d. hypothesis

Objective 2.01: Analyze the historical development of the current atomic theory.

4. Which sequence represents a correct order of historical developments leading to the modern model of the atom?

a. The atom is a hard sphereàelectrons exist in orbitals outside the nucleusàmost of the atom is

empty space with a small dense nucleus.

b. The atom is a hard sphereàmost of the atom is empty space with a small dense

nucleusàelectrons exist in orbitals outside the nucleus

c. Most of the atom is empty space with a small, dense nucleusàelectrons exist in orbitals outside

the nucleusàthe atom is a hard sphere.

d. Most of the atom is empty space with a small dense nucleusàthe atom is a hard

sphereàelectrons exist in orbitals outside the nucleus.

5. The diagram below shows the results of Rutherford’s experiment in which he used a radioactive source to

“shoot” alpha particles at a thin sheet of gold foil. Based on these results, what were Rutherford’s conclusions?

a. Atoms are solid matter with positive and negative charges scattered throughout.

b. Atoms are solid, positively charged matter with negatively charged electrons scattered throughout.

c. Atoms are mostly empty space with small, dense, negatively charged centers.

d. Atoms are mostly empty space with small, dense, positively charged centers.

6. The arrangement of electrons in an atom of an element determines the chemical properties of that

element. Our present-day understanding of how electrons are arranged in an atom is the result of which of these scientific models —

Rutherford’s model based on the gold foil experiment that proved the existence of the nucleus.
Dalton’s model that was based on the law of definite composition.

c. The quantum (wave) mechanical model which explains the most probable location of the electron in the electron cloud.

Thompson’s model based on his discovery of the electron using the cathode ray tube.

Objective 2.02:

Examine the nature of atomic structure including subatomic particle, mass number, atomic number and isotopes.

7. Which statement correctly describes the charge of the nucleus and the charge of the electron

cloud of an atom?

a. The nucleus is positive and the electron cloud is positive.

b. The nucleus is positive and the electron cloud is negative.

c. The nucleus is negative and the electron cloud is positive.

d. The nucleus is negative and the electron cloud is negative.

Use the chart on the right to answer question 8.

8. The chart shows isotopes of some common elements. In what

two properties do the isotopes of oxygen differ?

a. Number of protons and number of neutrons

b. Atomic mass and number of protons

c. Atomic number and number of neutrons

d. Atomic mass and number of neutrons

9. An ion with 20 protons, 20 neutrons, and 18 electrons

is represented by

a. Ne b. Ca+2 c. Ca-2 d. Ca

Objective 2.03: Apply the language and symbols of chemistry.

You may need to use your reference tables to answer these questions.

10. What is the formula for a compound formed from sodium ions (Na1+) and oxygen ions (O2–)?

a. NaO b. Na2O c. NaO2 d. Na4O2

11. What is the Stock system name for CuO?

a. Copper (I) oxide b. Copper (II) oxide c. Copper (III) oxide d. copper oxide

12. What is the correct name for the compound HNO2?

a. Hydronitric acid

b. Nitric acid

c. Nitrous acid

d. Hyponitrous acid

13. What is the formula for sulfuric acid?

a. H2S b. H2SO4 c. H2SO3 d. H3N

14. The table shows some of the prefixes used to name binary covalent compounds. What name would be

given to the compound P2Br10?

a. Phosphorus tetrabromide

b. Monophosphorus pentabromide

c. Diphosphorus decabromide

d. Phosphorus hexabromide

15. Sodium Citrate has a formula of Na3C6H5O7. What would be the formula for magnesium citrate?

a. Mg (C6H5O7)2 b. MgC6H5O7 c. Mg3(C6H5O7)2 d. Mg3 C6H5O7

Objective 2.04: Identify substances using their physical properties.

You may need to use your reference tables to answer these questions.

Use the graph on the right to answer questions 16-17

16. According to these data, what is the approximate

number of grams of sodium nitrate that can be

dissolved in 100ml of water at a temperature of 50ºC?

a. 95 g b. 105 g c. 115 g d. 125 g

17. Based on the information in the graph, a solution of 130 g of

sodium nitrate in 100 ml of water at 60C is

a. dilute b. unsaturated c. saturated d. supersaturated

18. A nonpolar solvent will most likely dissolve in what type of solute?

a. polar b. nonpolar c. ionic d. metallic.

19. Which of the following is a possible freezing to boiling point temperature range for a solution of sugar in

water?

a. 0°C to 115.3 °C b. 0°C to 100 °C c. -5°C to 100 ° C d. -6.3 ° C to 102.6 ° C

20. When making a solution of calcium chloride in water, the water would be the

a. solution b. precipitate c. solvent d. solute

21. Bubbles arise on the surface of a newly opened bottle of a carbonated beverage. This action is explained

by the fact that the carbon dioxide is less soluble when

Temperature is increased
Temperature is decreased

c. Pressure is decreased

Pressure in increased

22. Which compound is insoluble in water?

a. BaSO4 b. KClO3 c. CaBr2 d. Na2S

23. Which process is a chemical change?

a. melting of ice b. boiling of water c. subliming of ice d. decomposing water into hydrogen and oxygen

24. 11.2 liters of a gas at STP has a mass of 35.5 grams. What is the identity of the gas?

a. Chlorine b. Hydrogen chloride c. Nitrogen d. Hydrogen

Objective 2.05: Analyze the basic assumptions of kinetic molecular theory and apply the gas laws.

25.

26. A sample of a gas is contained in a closed rigid cylinder. According to kinetic molecular theory, what occurs

when the gas inside the cylinder is heated?

a. The number of gas molecules increases.

b. The number of collisions between gas molecules per unit time decreases.

c. The average velocity of the gas molecules increases.

d. The volume of the gas decreases.

27. The stronger the intermolecular forces in a substance, the higher the boiling point of the substance.

Which of the following substances would be predicted to have the highest boiling point?

a. O2 b. Ar c. He d. NH3

28. The density of a substance undergoes the greatest change when

A liquid changes to gas
A liquid changes to a solid
A solid changes to a liquid

d. When a gas changes to a solid

29. What is the volume of 40.0 g of helium at STP?

a. 11.2 L b. 22.4 L c. 112 L d. 224 L

30. A diver finds the best corals at a depth of 10.0 m. The diver’s lung capacity at the surface is 2.40 L. The

surface air temperature is 32.0 °C and the pressure is 101.3 kPa. What is the volume of the diver’s lungs at 10.0 m at a temperature of 21.0 ° C and a pressure of 141.2 kPa?

a. 1.12 L b. 1.66 L c. 1.78 L d. 4.86 L

31. How many moles of Nitrogen gas, N2, are present in a 45.0 liter container at a pressure of 0.50 atm and a

temperature of 82 C?

a. 7.72 mol b. 3.34 mol c. 0.772 mol d. 1.23 mol

Objective 2.06: Assess bonding in metals and ionic compounds as related to chemical and physical properties.

32. Which substance contains bonds that involved the transfer of electrons from one atom to another?

a. CO2 b. KBr c. NH3 d. Cl2

33. An atom of which element is larger than its ion-

a. calcium b. chlorine c. oxygen d. iodine

34. This apparatus was most likely designed to show that —

a. the formation of an ionic compound is an exothermic reaction

b. ionic compounds conduct a current in solution

c. the formation of an ionic compound is an endothermic reaction

d. water is a good conductor of electricity

Use the chart below on questions 35-36

35. What type of bonding is mostly likely in compound A?

a. non-polar covalent b. polar covalent c. ionic d. metallic

36. What type of bonding is most likely in compound D?

a. non-polar covalent b. polar covalent c. ionic d. metallic

Use the diagram below in question 37.

37. The diagram represents the arrangement of atoms in a metallic solid. Scientists believe that electrons in

the outer energy levels of the bonding metallic atoms are free to move from one atom to the next. Because

they are free to move, these electrons are often referred to delocalized electrons and give metals ALL of the following properties EXCEPT.

a. Malleable and ductile. c. Conduct heat and electricity in the solid state.

b. Luster d. Brittle, break easily

Objective 2.07: Assess covalent bonding in molecular compounds as related to chemical and physical properties and molecular geometry.

38. The boiling point of HBr is lower than that of HF because:

HBr is heavier than HF and therefore it requires less energy to vaporize.

b. HBr has dipole-dipole attractions which are weaker than the hydrogen bonding found in HF.

The dispersion forces are weaker in HBr than in HF.

d. All of the above are correct.

39. Which substance(s) will exhibit hydrogen bonding between its molecules?

a. H2O b. N2 c. CH4 d. H2

40. Which of these molecules would be expected to be polar?

a. O2 b. HCl c. CO2 d. CCl4

41. What is the total number of pairs of electrons shared in a molecule of N2?

a. one pair b. three pairs c. two pairs d. four pairs

42. The ammonia, NH3, gas molecule exhibits what type of geometric shape?

a. trigonal planar b. tetrahedral c. bent or V-shaped d. trigonal pyramidal

C 43. Which diagram best represents the structure of a water molecule?

Objective 2.08: Assess the dynamics of physical equilibrium

44. What are the best conditions for condensing a gas into a liquid?

a. high temperature, high pressure

b. low temperature, high pressure

c. high temperature, low pressure

d. low temperature, low pressure.

Use the graph on the right for questions 45-46

45. What phase change takes place as a substance moves

from A to B?

a. condensation

b. melting

c. boiling

d. sublimation

46. What is the boiling point of this liquid at 0.8 atm of

pressure?

a. 81.0 K b. 83.5 K c. 85.5 K d. 87.5K

Objective 3.01: Analyze periodic trends in chemical properties and use the periodic table to predict properties of elements.

47. Which Period 4 element has the most metallic properties?

a. As b. Ge c. Br d. Sc

48. If two elements have similar chemical properties, which of the following would be similar in

both elements?

a. atomic radii c. number of energy levels

b. number of valence electrons d. atomic mass

49. Which of the following is the correct noble gas representation for calcium?

a. [Ar] 4s2 b. [Ne] 3s23p64s2 c. [Xe] 4s6 d. [Br] 4s2

Use the Chart Below to Answer Questions 50-52

1 18

2 13 14 15 16 17
A / B / 3 4 5 6 7 8 9 10 11 12 / C / D / E

50. Which element has the lowest ionization energy?

a. A b. B c. C d. D

51. What is the electron configuration of element D?

a. 1s2, 2s2, 2p6

b. 1s2, 2s2, 2p5

c. 1s2, 2s2, 3s1

d. 2s2, 2p3

52. What is the most common oxidation number for element C?

a. +3 b. +2 c. -2 d. -3

Objective 3.02: Apply the mole concept, Avogadro’s number and conversion factors to chemical calculations.

53. The gram molecular mass of oxygen (O2) is 32.0 grams/mol.

How many ATOMS of oxygen does this quantity represent?

a. 6.02 x 1023 atoms b. 2.0 atoms c. 2 x 6.02 x 1023 atoms d. 32.0 atoms

54. What is the number of moles of hydrogen contained in 1.0 mol of NH4HCO3?

a. 4.0 moles b. 1.0 mole c. 5.0 moles d. 10.0 moles

55. What is the molarity of a solution of 3.2L which contains 0.32moles of solute?

a. 1.0 M b. 0.1 M c. 0.01 M d. 10.0 M

56. How many grams of solute are contained in 125 mL of 0.0500 M solution of NaOH?

a. 0.00625 g b. 6.25 g c. 2.50 g d. 0.250 g

57. 7.00 moles of sodium have a mass of

a. 280 g b. 161 g c. 224 g d. 3.29 g