first quarter chemistry progress...

Chemistry Final Study Guide Fall 2011

Chemical Names and Formulas

Multiple Choice: Select the correct formula for each given compound name.

1. sodium hydrogen carbonate

a. NaHCO b. NaHCO2 c. NaHCO3 d. NaHCO4

2. calcium carbonate

a. CaCO b. CaCO2 c. CaCO3 d. CaCO4

3. dinitrogen oxide

a. NO b. N2Oc. N3O d. N4Oe. N5O

4. sodium hydroxide

a. NaOH b. Na2OH c. Na2OH2 d. NaOH2 e. NaO2H

5. hydrochloric acid

a. HCl b. H2Cl c. HCl2 d. H2Cl2 e. 2HCl

6. carbon dioxide

a. CO b. C2O c. CO2 d. C2O2 f. 2CO

Multiple Choice: Select the term that best fits the given definition.

7. Ions formed from a single atom.

a. Monatomic b. Diatomic c. Triatomic d. Polyatomic

8. Compounds composed of two different elements.

a. Mono compounds b. Binary compounds c. Polyatomic compounds

9. The term that refers to methods of naming chemical compounds.

a. Chemistry b. Nomenclature c. Namenclature d. Termology

10. Polyatomic ions that contain oxygen.

a. Oxyanions b. Oxyions c. Oxycations d. Oxymorons

11. Acids containing hydrogen, oxygen, and a third element.

a. Hydroacids b. Oxyacids c. Triacids d. Hydroxyacids

12. An ionic compound composed of a cation and the anion from an acid.

a. Solution b. Salt c. Solvent d. Oxide e. Base

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Oxidation Numbers

Fill-in-the-blank: Select the word or phrase that best completes each sentence.

13. Oxidation numbers are also called oxidation ________________ .

a. States b. Levels c. Charges d. Elements e. Atoms

14. The algebraic ________ of the oxidation numbers of all atoms in a neutral compound is ______ .

a. Sum , Zero b. Difference , Neutral c. Difference , Zero

15. The algebraic ________ of the oxidation numbers of all atoms in a ____________ ion is equal to

the charge of the ion.

a. Total , Monatomic b. sum , diatomic c. sum , polyatomic

16. An uncombined element has an oxidation number of ________.

a. three b. two c. one d. zero

17. A _____________ ion has an oxidation number equal to its charge.

a. polyatomic b. monatomic c. catatomic d. diatomic

T / F : Select whether each statement is True or False.

18. Flourine has an oxidation number of -1 in all compounds.

19. Oxygen has an oxidation number of -2 in almost all compounds.

20. Hydrogen has an oxidation number of -1 in all compounds except those with metals, in which it

has an oxidation number of +1.

Using Chemical Formulas


21. The sum of the atomic masses of all the atoms represented in formula of any compound or

polyatomic ion.

a. formula weight b. formula mass c. atomic mass d. atomic weight

22. The percent by mass of each element in a compound.

a. mass composition b. mass percent c. percent composition

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Using Chemical Formulas ( cont. )

Calculations: For each of the following tasks, select the correct answer.

23. Calculate the formula mass for H2SO4.

a. 9.807 u b. .9807 u c. 98.07 u d. 980.7 u e. .09807 u

24. Calculate the formula mass for Ca(NO3)2.

a. 16.409 u b. 1.6409 u c. 1640.9 u d. .16409 u e. 164.09 u

25. Calculate the molar mass for NaNO3.

a. 8.49947 g b. 84.9947 g c. 849.947 g d. .849947 g

26. Calculate the molar mass for Ba(OH)2.

a. .17134 g b. 1.7134 g c. 17.134 g d. 171.34 g

27. Calculate the number of moles contained in 11.0 grams of CO2.

a. .0250 mol b. 0.250 mol c. 02.50 mol d. 025.0 mol

28. Calculate the number of moles contained in 6.60 grams of (NH4)2SO4.

a. .00500 mol b. 0.0500 mol c. 00.500 mol d. 005.00 mol

29. Calculate the number of moles contained in 4.5 kg Ca(OH)2.

a. 0.61 mol b. 6.10 mol c. 61.0 mol d. 610 mol

30. Calculate the percent composition of lead in PbCl2.

a. .7451 % b. 7.451 % c. 74.51 % d. 745.1 %

31. Calculate the percent composition of barium in Ba(NO3)2.

a. .52548 % b. 5.2548 % c. 52.548 % d. 525.48 %

32. How many grams of oxygen would be contained in 175 grams of the compound Magnesium

hydroxide which is 54.87 % oxygen by mass ?

a. .960 g b. 9.60 g c. 96.0 g d. 960 g

Determining Chemical Formulas

T / F : Select whether each statement is True or False.

33. The terminology “simplest formula” is the same as “empirical formula”.

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Chemical Equations


34. A representation using symbols and formulas to express the reactants and products in a chemical

reaction.

a. chemical formula b. chemical equation c. chemical expression

35. A small whole number that appears in front of a formula in a chemical equation.

a. cohesion b. correlation c. coefficient d. cooperate

36. An equation in which the reactants and products in a chemical reaction are represented by words.

a. chemical equation b. word equation c. simple equation

37. An equation that represents the reactants and products of a chemical reaction by using symbols

and/or formulas.

a. formula equation b. word equation c. chemical equation

General Knowledge

Multiple Choice – General Knowledge: Select the option that best answers the question or task.

38) Which of the following is NOT a major component of the scientific method?

a) observing b) generalizing c) measuring d) testing e) theorizing

39) Which of the following is an example of quantitative information?

a) volume b) color c) texture d) shape e) smell

40) Which of the following is an example of qualitative information?

a) density b) taste c) length d) weight e) area

41) The main difference between mass and weight is a factor known as:

a) quantity b) inertia c) gravity d) conservation e) composition

42) Among the following, which are examples of matter?

a) elements b) chemicals c) pure substances d) atoms e) all of the above

43) Which of the following are the two major types of energy?

a) kinetic and chemical b) potential and solar c) kinetic and potential

d) potential and mechanical e) solar and mechanical

44) Which of the following is NOT an example of potential energy?

a) water behind a dam b) water flowing over a dam c) a boulder at the top of a hill

d) a stretched rubber band e) a stick of dynamite

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45) Which of the following is NOT an example of kinetic energy?

a) a baseball in flight b) a water balloon c) a hurricane d) a burning candle

46) Which of the following is a state of matter?

a) solid b) liquid c) gas d) all of the above

47) Which of the following is NOT a physical property?

a) melting point b) height c) flammability d) volume e) color

48) Which of the following is NOT a chemical property?

a) density b) flammability c) toxicity d) reactivity e) oxidation state

49) Which of the following is an intensive physical property?

a) mass b) volume c) density d) length e) area

50) Which of the following is an extensive physical property?

a) color b) melting point c) ductility d) crystal structure e) weight

51) Which one of the following is an intensive property that is qualitative in nature?

a) density b) color c) mass d) length e) volume

52) Which one of the following is an intensive property that is quantitative in nature?

a) area b) melting point c) ductility d) crystal structure e) malleability

53) Which of the following is an example of a chemical change?

a) decomposition b) cooking c) rusting d) oxidation e) all of the above

54) Which of the following is an example of a physical change?

a) grinding a sugar cube into powder b) melting c) boiling d) freezing e) all of the

above

55) When ice melts, the water undergoes which of the following?

a) a chemical change b) a physical change c) both

56) The chopping of wood into smaller pieces can be classified as which of the following?


57) The burning of paper can be classified as which of the following?


58) When salt is dissolved in water, the salt undergoes which of the following?


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59) The boiling of water until it evaporates is an example of which of the following?


60) Which of the following is NOT an observable change that would indicate that a chemical reaction

has occurred?

a) The evolution of heat and light. b) The production of a gas.

c) The formation of a precipitate. d) The freezing of a solid.

61) Which of the following is NOT an example of an exothermic process?

a) combustion of fuels b) condensation of a vapor to a liquid c) explosion of a

firecracker d) the melting of ice e) the formation of snow flakes

62) Which of the following is NOT an example of an endothermic process?

a) the making of ice cream b) the melting of ice cream c) the eating of ice cream

63) In photosynthesis, the transfer of energy from sunlight to the plant’s cells is an example of which

of the following processes?

a) endothermic b) exothermic c) both a & b d) neither a nor b

64) The transferring of energy during both a 100 megaton nuclear bomb explosion and a drop of

water freezing is an example of which of the following processes?


65) Which of the following processes describes what happens to the energy (heat) in the air that

surrounds solid water (ice) as the water turns into a liquid?


66) Each sample of matter can be classified into which of the following types?

a) a pure substance b) a mixture c) both a & b d) either a or b

67) Referring to samples of matter, which of the following is NOT an example of a mixture?

a) gasoline b) air c) sugar d) Dr. Pepper e) grapefruit juice

68) Referring to samples of matter, which of the following is NOT an example of a pure substance?

a) milk b) distilled water c) salt d) oxygen e) silver

69) Which of the following is an example of a heterogeneous mixture?

a) vegetable soup b) milk c) chocolate chip cookies d) all of the above

70) Which of the following is an example of a homogeneous mixture?

a) air b) sea water c) Mountain Dew d) chocolate syrup e) all of the above

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71) The two categories for classifying samples of homogeneous matter are homogeneous mixture and

which of the following?

b) pure substances b) pure solutions c) pure phases d) pure precipates

72) Which of the following is an example of an element?

c) salt b) water c) copper d) NaCl e) H2O

73) Which of the following is an example of a compound?

d) gold b) silver c) copper d) calcium e) salt

For the following questions, #37 & #38, refer to the chemical equation as diagramed in the box (fig 1) below.

fig 1:

74) In reference to the above chemical reaction, which substance or substances are the reactants?

e) 2H b) O c) H2O d) both a & b e) both b & c

75) In reference to the above chemical reaction, which substance or substances are the products?

f) 2H b) O c) H2O d) both a & b e) both b & c

For the following questions 46 – 51, refer to the periodic table.

76) Which of the following sets is a representation of a periodic table group?

g) [ Li, Be, B, C, N, O, F, Ne ] b) [ F, Cl, Br, I, At ]

77) Which of the following sets is a representation of a periodic table period?

h) [ Na, Mg, Al, Si, P, S, Cl, Ar ] b) [ B, Al, Ga, In, Tl ]

78) Which of the following sets is a representation of periodic table metals?

i) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl,

Br, I ]

79) Which of the following sets is a representation of periodic table non-metals?

j) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl,

Br, I ]

80) Which of the following sets is a representation of periodic table metalloids?

k) [ Mg, Co, Ga, In, Os, Ba, Ra ] b) [ B, Si, Ge, As, Se, Sb, Te ] c) [ C, N, P, S, Cl,

Br, I ]

81) Which of the following is NOT a physical property of the element copper?

l) metallic luster b) ductile c) malleable d) translucent

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2H + O → H2O

True or False: Read the statement, decide if the statement is true or false, then bubble A for true or B for false.

82) T / F : The Periodic Table arranges the elements according to their properties.

83) T / F : In the Periodic Table, elements with similar properties are found in the same period

(row).

84) T / F : The ultimate goal of scientific investigations is to explain and predict natural

phenomena.

85) T / F : Pharmaceutical Chemistry is the study of substances found within the atomic nucleus.

86) T / F : In the scientific method, testing and experimenting are basically the same thing.

87) T / F : In the scientific method, a hypothesis and a theory are basically the same thing.

88) T / F : A pure substance can be either a homogeneous sample of matter or a heterogeneous sample of matter.

89) T / F : Every sample of a given pure substance can have different physical and chemical

properties.

90) T / F : Every sample of a given pure substance has exactly the same chemical composition.

91) T / F : A pure substance cannot be separated into other substances without changing its

identity.

92) T / F : A pure substance is an element and never a compound.

93) T / F : A solution in which water is the solvent is referred to as an aqueous solution.

94) T / F : The volume of an object is the amount it weighs.

95) T / F : In the Periodic Table, elements within a period have many similar properties.

96) T / F : The noble gases do not fit into other classes within the Periodic Table because of their non- reactive natures.

97) T / F : The micro-electronics revolution, which has resulted in PCs, smart-phones, digital cameras, and hundreds of other gadgets that are changing global communication, business, economies, and politics, is based upon semi-conducting elements.

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Diagram:Use the three diagrams below to answer the next three questions.

98) Which diagram shows the boulder when its kinetic energy is at its greatest?

a Diagram A b) Diagram B c) Diagram C

99) Which diagram shows the boulder when its potential energy is at its least?


100) Which diagram shows the boulder when its potential energy is at its greatest?


Multiple Choice – Terms: Select the term that best fits the given definition.

101) Numerical information.a Quantitative Information b) Qualitative Information

102) Non-numerical information.a Quantitative Information b) Qualitative Information

103) A broad generalization that explains a body of known facts or phenomena.a Theory b) Law c) Hypothesis

104) A generalization that describes a wide variety of behaviors in nature.a Theory b) Law c) Hypothesis

105) A testable statement.a Theory b) Law c) Hypothesis

106) The study of the composition and structure of materials and the changes they undergo.a Chemistry b) Biology c) Physics d) Botany e) Zoology

107) A logical approach to the solution of problems that lend themselves to investigations by observing, generalizing, theorizing, and testing.a Scientific Method b) Scientific Calculations c) Scientific Calculator d) Science Stuff

108) The study of the properties and transformations of matter in terms of fundamental physical properties.a Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

A CB

109) The study of substances containing carbon and hydrogen.a Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

110) The study of all substances and processes that occur in living things.a Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

111) The study of all substances not classified as organic chemicals.a Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

112) Resistance to change in motion.a Inertia b) Weight c) Mass d) Matter e) Energy

113) A measure of the earth’s gravitational attraction for matter.

a Inertia b) Weight c) Mass d) Matter e) Energy

114) A measure of the quantity of matter.


115) Anything that has mass and occupies space.


Using Scientific Measurements

Multiple Choice:

1) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times and records readings of 8.42 mL, 8.41 mL, and 8.40 mL. The student’s readings are: (choose

one)a. Accurate b. Precise c. both d. neither

2) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times and records readings of 8.92 mL, 8.93 mL, and 8.94 mL. The student’s readings are: (choose one)

a. Accurate b. Precise c. both d. neither

3) The true volume of a liquid sample is 8.4125 mL. A student measures the volume of this sample three times and records readings of 8.92 mL, 8.41 mL, and 9.34 mL. The student’s readings are: (choose one)

b. Accurate b. Precise c. both d. neither

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Diagram: Refer to the following three scales (A, B, C) for questions # 4 - 6

Scale A:

_______|___________|____________|____________|____________|___________|_________10 20 30 40 50 60

Scale B:

_|_____|______|______|______|______|______|_____|_____|______|______|______|______|___10 11 12 13 14 15

Scale C:

__|_____|______|______|______|______|______|______|______|______|______|______|______|___10.4 10.5 10.6 10.7 10.8 10.9

4) Which scale will have readings up to two (2) significant figures?

a) Scale A b) Scale B c) Scale C

5) Which scale will have readings up to three (3) significant figures?


6) Which scale will have readings up to four (4) significant figures?


True or False:

7) T / F : A set of measurements can be precise without being accurate.

8) T / F : A set of measurements can be accurate without being precise.

9) T / F : A single measurement amongst a set of measurements can be accurate without the set being accurate.

10) T / F : A single measurement amongst a set of measurements can be precise without the set being precise.

11) T / F : A single measurement amongst a set of measurements can be precise without the set being accurate.

Rounding Off: For each of the following numbers, choose which answer is correctly rounded to 4 sig figs.

12) 42.6854 g = a. 42.69 g b. 42.68 g c. 42.67 g

13) 17.3356 m = a. 17.32 m b. 17.33 m c. 17.34 m

14) 2.7851 cm = a. 2.784 cm b. 2.785 cm c. 2.786 cm

15) 4.6350 kg = a. 4.634 kg b. 4.635 kg c. 4.636 kg

16) 78.6544 mL = a. 78.64 mL b. 78.65 mL c. 78.66 mL

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Multiple Choice: Determine the number of significant figures in each of the following measurement

examples.

17) 438 g = a. 1 b. 2 c. 3 d. 4 e. 5

18) 26.42 m = a. 1 b. 2 c. 3 d. 4 e. 5

19) 1.7 cm = a. 1 b. 2 c. 3 d. 4 e. 5

20) 0.653 L = a. 1 b. 2 c. 3 d. 4 e. 5

21) 10,050 mL = a. 1 b. 2 c. 3 d. 4 e. 5

22) 900.43 kg = a. 1 b. 2 c. 3 d. 4 e. 5

23) 60.0 K = a. 1 b. 2 c. 3 d. 4 e. 5

24) 0.06 g = a. 1 b. 2 c. 3 d. 4 e. 5

25) 0.0047 L = a. 1 b. 2 c. 3 d. 4 e. 5

26) 0.8 g = a. 1 b. 2 c. 3 d. 4 e. 5

27) 8.0 g = a. 1 b. 2 c. 3 d. 4 e. 5

28) 300 m = a. 1 b. 2 c. 3 d. 4 e. 5

Calculations: Calculate the following and select the correct answer.

29) 213.67 m + 98 m = a. 311.67 m b. 310 m c. 312 m d. 311.6 m

30) 107.38 km – 65 km = a. 42.38 km b. 42 km c. 43 km d. 42.0 km e. 42.3 km

31) 12.0 cm x 4.3 cm = a. 51.6 cm2 b. 51.0 cm2 c. 52 cm2 d. 52.0 cm2 e. 51.5 cm2

Multiple Choice: For each number, select the correct Scientific Notation for it.

32) 4,325,045.2 = a. 4.32 x 106 b. 43.25 x 105 c. 4.32 x 105 d. 432 x 106

33) 0.00000361 = a. .361 x 105 b. 36.1 x 10-5 c. 3.61 x 10-6 d. 361 x 10-8

34) 85,000,000 = a. 8.5 x 106 b. 8.5 x 107 c. 85.0 x 106 d. 85.0 x 107

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Multiple Choice: For each Scientific Notation, select the correct number for it.

35) 2.31 x 10-6 = a. .0000000231 b. .000000231 c. 0.0000231 d.

0.00000231

36) 5.3 x 104 = a. 53000.00 b. 53,000 c. 53,000.00 d. 5,300.00

37) 7 x 105 = a. 700,000 b. 700,000.00 c. 70,000.00 d. 70,000

Solving Quantitative Problems

Calculations:

38) Calculate the number of seconds in exactly one week.

a. 604,800 b. 64,800 c. 60,800 d. 6,480 e. 60,400

39) What is the volume of a 12 g piece of gold? (d = 19.3 g/cm3 )

a. 6.2 cm3 b. 0.62 cm3 c. 62 cm3 d. 620 cm3 e. 6,200 cm3

40) An object travels at a speed of 7500 cm / s. How far will it travel in a day?

a. 648,000,000 cm b. 6,480,000 m c. 6.48 x 108 cm d. 6,480 km e. all of the

above

The AtomMatch-up:

41) Law of Multiple Proportions A- A law used in science that states: Matter can neither be created nor destroyed.

42) Law of Conservation of Mass B- A law used in science that states: If two or more different compounds are composed of the same two elements, the

masses of the second element combined with a certain mass of the first element can be expressed as ratios of small whole numbers.

43) Law of Definite Composition C- A law used in science that states: Energy can neither be created nor destroyed.

44) Law of Conservation of Energy D- A law used in science that states: Every chemical compound has a definite composition by mass.

True or False:

45) T / F : The word “atom” comes from an Epytian word meaning dividable.

46) T / F : Dalton developed his Atomic Theory mainly from his observations of gases in the atmosphere.

47) T / F : Mass is always conserved in chemical reactions.

48) T / F : In all chemical reactions, a portion of energy used by the reaction is destroyed.

49) T / F : Chemical reactions are simply the combination, separation, or rearrangement of atoms.

50) T / F : Scientists often use more than one method to gather data.

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The Structure of the AtomMatch-up:

51) Atomic Structure A- The identity and arrangement of smaller particles within atoms.

52) Electron B- A negatively charged sub-atomic particle.

53) Proton C- A subatomic particle that has a positive charge equal in magnitude to the negative charge of an electron and is present in atomic nuclei.

54) Neutron D- Atoms of the same element that have different masses.

55) Isotopes E- An electrically neutral, sub-atomic particle found in atomic nuclei.

True or False:

56) T / F : Every element has exactly the same number of protons as electrons.

57) T / F : Every element has isotopes.

58) T / F : The only difference between isotopes of the same element is the number of electrons.

59) T / F : Nuclear forces are responsible for the delicate balance held within an atom.

Weighing and Counting AtomsMatch-up:

60) Atomic Number A- The weighted average of the atomic masses of the naturally occurring isotopes of an element.

61) Mass Number B- The mass of an atom that is expressed in atomic mass units.

62) Atomic Mass C- The mass in grams of one mol of an element.

63) Average Atomic Mass D- The total number of protons and neutrons in the nucleus of an isotope.

64) Molar Mass E- The number of protons in the nucleus of each atom of that element.

Multiple Choice:

For each of the following isotopes, select the correct nuclear symbol.

65) sodium-23 = a. 2311 Na b. 11

23 Na c. 2211 Na d. 11

22 Na

66) calcium-40 = a. 2040 Ca b. 41

20 Ca c. 4021 Ca d. 40

20 Ca

67) carbon-13 = a. 136 C b. 12

6 C c. 612 Cd. 6

13 C

For each of the following isotopes, select the correct hyphen notation.

68) 6429 Cu =a. copper-64 b. copper-29 c. copper- 63 d. copper-35

69) 10847 Ag =a. silver-47 b. silver-61 c. silver-107 d. silver-108

70) 13356 Cs =a. cesium-56 b. cesium-133 c. cesium-132 d. cesium-77

71) 23592 U = a. uranium-235 b. uranium-92 c. uranium-238 d. uranium-143

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True or False:

72) T / F : The term atomic weight is sometimes used synonymously with the term atomic mass.

73) T / F : The term nuclide atomic mass is sometimes used synonymously with the term relative atomic mass.

74) T / F : The isotopes protium, deuterium, and tritium are isotopes of helium.

75) T / F : Most isotopes are identified only by their mass numbers and have no individual names.

76) T / F : Avogadro was smart Spaniard who got his bachelor’s degree at the age of 16.

77) T / F : Most elements occur naturally on Earth as isotopes.

78) T / F : The super script placed before an element’s nuclear symbol is that element’s mass number.

79) T / F : The subscript placed before an element’s nuclear symbol is that element’s atomic number.

Diagram: On the back of your scantron test sheet, make a Bohr model sketch of the Lithium atom showing and labeling all sub-atomic particles and their proper locations. (12 points)

Refinements of the Atomic Model Multiple Choice:For each of the following, select the term that best fits the given definition.

1. A form of energy that exhibits wavelike behavior as it travels through space.a. Electromagnetic Radiation b. Frequency c. Wavelength d. Line Spectrum

2. The measured distance between corresponding points on adjacent waves.a. Frequency b. Wavelength c. Line Spectrum d. Quantum e. Photon

3. The number of waves that pass a given point in a specific amount of time.a. Frequency b. Wavelength c. Line Spectrum d. Quantum e. Photon

4. A spectrum in which all wavelengths within a given range are included.a. Line Spectrum b. Continuous Spectrum c. Electromgnetic Spectrum

5. A spectrum that is produced when an electron drops from a higher-energy orbit to a lower energy orbit.a. Line Spectrum b. Continuous Spectrum c. Electromgnetic Spectrum

6. All of the electromagnetic radiation, arranged according to increasing wavelength.a. Line Spectrum b. Continuous Spectrum c. Electromagnetic Spectrum

7. The emission of electrons by certain metals when light shines on them.a. Photoelectric Effect b. Quantum c. Photon d. Orbital e. Excited State

8. A finite quantity of energy that can be gained or lost by an atom.a. Photoelectric Effect b. Quantum c. Photon d. Orbital e. Excited State

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9. A quantum of light.a. Photoelectric Effect b. Quantum c. Photon d. Orbital e. Excited State

10. The state of lowest energy of an atom.a. Quantum b. Excited State c. Ground State d. Photon e. Orbital

11. A state in which an atom has a higher potential energy than it has in its ground state.a. Quantum b. Excited State c. Ground State d. Photon e. Orbital

12. Describes mathematically the wave properties of electrons and other very small particles.a. Quantum b. Quantum Theory c. Photoelectric Effect d. Orbital

13. A three-dimensional region about the nucleus of an atom in which a particular electron can be located.a. Quantum b. Quantum Theory c. Photoelectric Effect d. Orbital

14. Some Danish physicist dude who developed a valid model of the atom.a. Rutherford b. Bohr c. Mr. J d. Avogadro e. Kyle

True or False:15. T / F : Wavelength and frequency are inversely related. 16. T / F : The symbol: λ is the lower case Greek lambda.17. T / F : The symbol: υ is the lower case Greek nu.

Diagram: For questions # 18 through # 21Refer to the four Bohr models below and determine which is Nitrogen, Sodium, Neon, & Oxygen.

A B C D

18. Bohr model A above is:a. Nitrogen b. Sodium c. Neon d. Oxygen

19. Bohr model B above is:a. Nitrogen b. Sodium c. Neon d. Oxygen

20. Bohr model C above is:a. Nitrogen b. Sodium c. Neon d. Oxygen

21. Bohr model D above is:a. Nitrogen b. Sodium c. Neon d. Oxygen

Electron Configuration and the Periodic Table Multiple Choice:For each of the following, select the term that best fits the given definition.

22. The elements of group 17.a. Alkali Metals b. Alkali Earth Metals c. Transition Elements

d. Main-group Elements e. Halogens23. The p-block elements together with the s-block elements.

a. Alkali Metals b. Alkali Earth Metals c. Transition Elementsd. Main-group Elements e. Halogens

24. The d-block elements.a. Alkali Metals b. Alkali Earth Metals c. Transition Elements

d. Main-group Elements e. Halogens25. The elements of group 2.

a. Alkali Metals b. Alkali Earth Metals c. Transition Elementsd. Main-group Elements e. Halogens

26. The elements of group 1.a. Alkali Metals b. Alkali Earth Metals c. Transition Elements

d. Main-group Elements e. Halogens

*** continued ***

Fill in the blanks:For each sentence below, select the word or phrase that best completes the sentence.27. The _______________ are the common characteristics shared by each element in a specific group.

a. number of valence electrons b. physical properties c. chemical propertiesd. chemical reactivity e. all of the above

28. The _______________ are the blocks that the Periodic Table be divided into to illustrate the relationships between electron configurations and Periodic Table placement.

a. The s block b. The d block c. The p block d. The f block e. all of the above

True or False:29. T / F : Thorium is an element in the f-block portion of the Periodic Table. 30. T / F : Fluorine, Chlorine, Bromine, and Iodine are all members of the p-block of the Periodic Table.31. T / F : Mercury, Tungsten, and Vanadium are all members of the d-block of the Periodic Table.

Electron Properties and Periodic PropertiesMultiple Choice:For each of the following, select the term that best fits the given definition.

32. One half the distance between the nuclei of atoms joined in a molecule. a. Ionic Radius b. Atomic Radius c. Ionization Energy d. - Electronegativity

33. Any process that results in the formation of an ion.a. Anion b. Cation c. Valence Electron d. Ionization e. Electronegativity

34. The energy required to remove one electron from an atom of an element.a. Ionic Radius b. Atomic Radius c. Ionization Energy d. - Electronegativity

35. One half the diameter of an ion in an ionic compound.a. Ionic Radius b. Atomic Radius c. Ionization Energy d. - Electronegativity

36. An ion with a positive charge.a. Anion b. Cation c. Valence Electron d. Ionization e. Electronegativity

37. An ion with a negative charge.a. Anion b. Cation c. Valence Electron d. Ionization e. Electronegativity

38. The electrons available to be lost, gained, or shared in the formation of chemical compounds.a. Anion b. Cation c. Valence Electron d. Ionization e. Electronegativity

39. A measure of the ability of an atom in a chemical compound to attract electrons.a. Anion b. Cation c. Valence Electron d. Ionization e. Electronegativity

*** continued ***

True or False:

40. T / F : Atomic radii decrease from right to left across a period in the Periodic Table.41. T / F : Atomic radii increase from down to up across a group in the Periodic Table.42. T / F : Period trends are patterns that exist in the Periodic Table groups.43. T / F : Group trends are patterns that exist in the Periodic Table periods.44. T / F : Metals are less electronegative than non-metals.

Diagram:

Refer to the diagram below for question # 45.

45. If the diameter of Cation X is 50pm, and the diameter of Anion Y is 100pm, what is the Atomic Radius

of the molecule XY ?

a. 50 pm b. 75 pm c. 100 pm d. 125 pm e. 150 pm

Chemical BondingMultiple Choice:For each of the following, select the term that best fits the given definition.

46. A link between atoms that results from the mutual attraction of their nuclei for electrons. a. Chemical Bond b. Ionic Bond c. Covalent Bond

47. The chemical bond resulting from electrostatic attraction between positive and negative ions.a. Chemical Bond b. Ionic Bond c. Covalent Bond

48. A chemical bond resulting from the sharing of electrons between two atoms.a. Chemical Bond b. Ionic Bond c. Covalent Bond

*** continued ***

= ? pm

Ionic Bonding and Ionic CompoundsMultiple Choice:For each of the following, select the term that best fits the given definition.

49. The simplest collection of atoms from which a compound’s formula can be established.a. Ionic Compound b. Formula Unit c. Lattice Energy

50. A compound that is composed of positive and negative ions combined so that the positive and negative charges are equal.

a. Ionic Compound b. Formula Unit c. Lattice Energy51. The energy released when one mole of an ionic crystalline compound is formed from gaseous ions.

a. Ionic Compound b. Formula Unit c. Lattice Energy

True or False:

52. T / F : When describing an ionic compound, you should not refer to “molecules” but rather to formula units.

53. T / F : Charges of ions are not usually included in formulas for ionic compounds.54. T / F : Potential energy decreases as ions assume their positions in the orderly array of ions in a crystal.55. T / F : Attraction between positive and negative ions causes planes of ions in a crystalline ionic

compound to resist motion..

Diagram:

Refer to the diagram below for questions # 56 and # 57

56. If the charge on element X is negative, what is the charge on element Y ?

a. Negative b. Positive c. It can be either negative or positive

57. If the charge on element X is positive, what is the charge on element Z ?

a. Negative b. Positive c. It can be either negative or positive

X

Y

Z

first quarter chemistry progress...

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