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Name: _________________________________ folder #: ________

Fall 2012 First Quarter Chemistry Progress Assessment Study Guide ( not complete )

General Knowledge

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

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

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

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

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

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

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

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

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

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

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

6) 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

7) 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

8) 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

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

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

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

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

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

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

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

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

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

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

*** continued ***

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

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

15) 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

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

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

17) 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

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

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

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

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

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

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

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

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

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

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

23) 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.

24) 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

25) 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

26) 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

*** continued ***

27) 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?

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

28) 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?

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

29) 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

30) 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

31) 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

32) 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

33) 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

34) The two categories for classifying samples of homogeneous matter are homogeneous mixture and which of the following?

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

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

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

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

a) 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:

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

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

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

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

*** continued ***

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

46) T / F : In the Periodic Table, elements with similar properties are found in the same period (row).

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

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

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

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

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

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

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

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

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

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

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

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

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

60) 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.

*** continued ***

Diagram:

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

[pic]

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

a) Diagram A b) Diagram B c) Diagram C

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

a) Diagram A b) Diagram B c) Diagram C

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

a) Diagram A b) Diagram B c) Diagram C

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

64) Numerical information.

a) Quantitative Information b) Qualitative Information

65) Non-numerical information.

a) Quantitative Information b) Qualitative Information

66) A broad generalization that explains a body of known facts or phenomena.

a) Theory b) Law c) Hypothesis

67) A generalization that describes a wide variety of behaviors in nature.

a) Theory b) Law c) Hypothesis

68) A testable statement.

a) Theory b) Law c) Hypothesis

69) The study of the composition and structure of materials and the changes they undergo.

a) Chemistry b) Biology c) Physics d) Botany e) Zoology

70) 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

71) 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

*** continued ***

72) The study of substances containing carbon and hydrogen.

a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

73) The study of all substances and processes that occur in living things.

a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

74) The study of all substances not classified as organic chemicals.

a) Biochemistry b) Physical Chemistry c) Organic Chemistry d) Inorganic Chemistry

75) Resistance to change in motion.

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

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

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

77) A measure of the quantity of matter.

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

78) Anything that has mass and occupies space.

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

Lab book Investigations section:

Inv # 1

Term match-up: Match the term with its definition.

79) ______ Interaction

80) ______ Observation

81) ______ Conductivity

82) ______ Chemical Name

83) ______ Chemical Formula

84) ______ Classification System

85) ______ Clarity

86) ______ Color

87) ______ Solution

88) ______ Slovent

89) ______ Solute

90) ______ Soluble

91) ______ Insoluble

92) ______ Dissolve

93) ______ Quantitative Information

94) ______ Qualitative Information

Term match-up ( continued ): Match the term with its definition.

95) ______ Interpret

96) ______ Criteria

97) ______ Characteristics

98) ______ Homogenous

99) ______ Heterogeneous

100) _______ Analyze

101) _______ Suspension

102) _______ Mixture

103) _______ Distributed

104) _______ Particles

105) _______ Derive

106) _______ Colloidal

107) _______ Disperse

Short Essay:

108) Describe where in the world of science the term “test” is used, its correct usage, and explain its proper and improper usage and why people use words improperly._______________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

_____________________________________________________________________________________

109) If sugar dissolves in water to form a solution, then why would a certain amount of sugar stop dissolving in a certain amount of water? ____________________________________________________

_____________________________________________________________________________________

Multiple Choice:

110) If the mass of a solute is 10 g and its volume is 2 ml, what is its density ?

a) 0.05 g/ml b) 0.5 g/ml c) 5.0 g/ml d) 50 g/ml e) 500 g/ml

Multiple Choice ( continued ):

111) If the density of a solution is 20 g/ml and its volume is 5.0 ml, what is its mass ?

a) .100 g b) 1.00 g c) 10.0 g d) 100 g e) 0.01 g

112) If the density of a solvent is 6 g/ml and its mass is 120 g, what is its volume ?

a) .002 ml b) .02 ml c) .20 ml d) 2.0 ml e) 20 ml

113) The ability for an aqueous solution to transfer electrons between positive and negative poles is called:

a) conductivity b) ion exchangeability c) electron flowability d) all of the above

Inv # 2

Term match-up: Match the term with its definition.

114) _______ Substance

115) _______ Evaporation

116) _______ System

117) _______ Percentage

118) _______ Calculate

119) _______ Value

120) _______ Conclusion

121) _______ Procedure

122) _______ Record

123) _______ Physical Change

124) _______ Chemical Change

125) _______ Reversible

126) _______ Irreversible

127) _______ Complex

128) _______ Informative

129) _______ Uniformly

130) _______ Fermentation

131) _______ Effervescent

132) _______

133) Give three ( 3 ) examples of numbers that have digits in two decimal places.

________________ __________________ ________________

134) The investigation manual uses the word “test” often during experiments. Is this a correct usage of the word test? (circle one) yes no

135) Where else in the world of science is the term “test” used? _______________________________ _______________________________________________________________________________

Inv # 3

Term match-up: Match the term with its definition.

136) _____ Property ( as used in science, not real estate )

137) _____ Sample

138) _____ Appropriate

139) _____ Alcohol

140) _____ Graduated ( as it applies to glassware )

141) _____ Collect

142) _____ Transfer

143) _____ Density

144) _____ Relationship

145) _____ Average

146) _____ Apparatus

147) _____ Compare

148) _____ Determine

149) _____ Evidence

150) _____ Experiment

151) _____ Appearance

152) _____ Cylindrical

153) _____ Assume

154) _____ Absorb

155) _____ Displacement

156) _____ Scientific Hypothesis

157) _____ Scientific Theory

158) _____ Scientific Law

Supplemental General Knowledge

What is Chemistry?

Match-up:For each numbered term, enter the letter corresponding to the definition that best matches the term.

____ 1- Chemistry A- Numerical information.

____ 2- Scientific Method B- A broad generalization that explains a body of known facts or phenomena.

____ 3- Quantitative Information C- The study of the composition and structure of materials and the changes they undergo.

____ 4- Qualitative Information D- Non-numerical information.

____ 5- Hypothesis E- A generalization that describes a wide variety of behaviors in nature.

____ 6- Law F- A testable statement.

____ 7- Theory G- A logical approach to the solution of problems that lend themselves to investigations by observing, generalizing, theorizing, and testing.

____ 8– Organic Chemistry H- The study of the properties and transformations of matter in terms of fundamental physical properties.

____ 9- Inorganic Chemistry I- The study of substances containing carbon and hydrogen.

____ 10- Physical Chemistry J- The study of all substances and processes that occur in living things.

____ 11- Biochemistry K- The Identification of materials and the qualitative and quantitative determination of the composition of materials.

____ 12- Analytical Chemistry L- The study of all substances not classified as organic chemicals.

____ 13- Chemical M- A substance produced by or used in a chemical process.

Scientific Method:

Put the following scientific method categories listed in the right column in their typical proper order as explained and diagramed in your textbook. (Reminder: “Categories” are groupings of the individual scientific method steps that scientists take within a particular category grouping. Do not confuse categories with steps. For example: Testing is a category meaning to test or “confirm” or “challenge” a theory or hypothesis; and experiment is a step within the observing category.)

14 ______ a- Theorizing

15 ______ b- Generalizing

16 ______ c- Testing (note: “Testing” is not “Experimentation” )

17 ______ d- Observing

Short Answer:

18, 19: What are the two categories of natural sciences? ___________________ _______________________

20: Into which of the above two categories of natural science does chemistry fall? ________________________

21, 22: Give two examples of a chemical: _______________________ ___________________________

23, 24: Name the two laws mentioned in the reading that are studied in chemistry: ____________ , _____________

25: What type of microscope mentioned in the reading can magnify a specimen 100 million times? ______________

True or False:

26: T / F -- The ultimate goal of scientific investigations is to explain and predict natural phenomena.

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

Matter and Energy

Match-up:

_____ 1 – Mass A- Resistance to change in motion.

_____ 2 – Matter B- A measure of the earth’s gravitational attraction for matter.

_____ 3 – Energy C- A measure of the quantity of matter.

_____ 4 – Weight D- Anything that has mass and occupies space.

_____ 5 – Solid State E- A proven theory stating that matter cannot be either created nor

destroyed in ordinary chemical or physical changes.

_____ 6 – Inertia F- The ability to cause change or the ability to do work.

_____ 7 – Kinetic Energy G- The energy of an object in motion.

_____ 8 – Potential Energy H- The energy that an object has because of its position or composition.

_____ 9 – Law of Conservation of Matter I – A proven theory stating that energy can be converted from one form to another, but it cannot be created nor destroyed in ordinary chemical or physical changes.

_____ 10 – Law of Conservation of Energy J- The state of any matter that has a definite shape and volume.

_____ 11 – Liquid State K-The state of any matter that has a definite volume but an indefinite shape.

_____ 12 – Physical Property L- The state of any matter that has neither a definite shape nor a definite volume.

_____ 13 – Properties M- Characteristics that enable us to distinguish one kind of matter from another.

_____ 14 – Intensive Physical Properties N –A type of property that can be observed or measured without altering the identity of a material.

_____ 15 – Extensive Physical Properties O –A type of physical property determined from the amount of matter present and includes mass, length, and volume.

_____ 16 – Gaseous State P – A type of physical property determined not from the amount of matter present and includes melting point, boiling point, density, ductility, malleability, color, crystalline shape, and refractive index.

_____ 17 – Changes of State Q – Any change in a property of matter that does not result in a change of identity.

_____ 18 – Physical Change R – The physical changes between gaseous, liquid, or solid forms.

_____ 19 – Chemical Property S – A type of property in reference to the ability of a substance to undergo a change that alters its identity.

_____ 20 – Exothermic T – Any change in which one or more substances are converted into

different substances with different characteristic properties.

_____ 21 – Chemical Change (chemical reaction) U – The substances that undergo a chemical reaction.

_____ 22 – Precipitate V – The new substances produced by a chemical reaction.

_____ 23 – Products W – A solid that separates from a solution.

_____ 24 – Endothermic X – A process that releases heat.

_____ 25 – Reactants Y – A process that absorbs heat.

Short Answer:

26: What is the difference between weight and mass? __________________________________________________________________________________________

27: What is the difference between kinetic energy and potential energy? __________________________________________________________________________________________

28: What is the difference between extensive physical properties and intensive physical properties of matter? __________________________________________________________________________________________

29: What is the difference between physical properties and chemical properties of matter? ___________________________________________________________________________________________

30: What is the difference between physical changes and chemical changes? ___________________________________________________________________________________________

31: What is the difference between exothermic processes and endothermic processes? ___________________________________________________________________________________________

Classification of Matter

Match-up:

____ 1- Law of Definite Composition A- A combination of two or more kinds of matter each of which retains its own composition and properties.

____ 2- Solutions B- A type of mixture in which the composition and properties are not uniform; they differ from point to point in the mixture.

____ 3- Phase C- Where portions of matter have both the same chemical and physical

properties.

____ 4- Pure Substance D- A type of mixture in which the composition and properties are uniform throughout the mixture.

____ 5- Homogeneous E- Another way to describe homogeneous mixtures.

____ 6- Chemical Compound F- A homogeneous sample of matter that has the same composition and properties, whatever its sourcs.

____ 7- Heterogenous G- A substance that cannot be separated into other substances by any ordinary chemical change.

____ 8– Element H- A pure substance that can be decomposed into two or more simple substances by an ordinary chemical change.

____ 9- Mixture I – A law that states: A chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound.

Short Answer:

Give two examples of a homogeneous mixture.

10)______________________________________________________________________________

11)______________________________________________________________________________

Give two examples of a heterogeneous mixture.

12)______________________________________________________________________________

13)______________________________________________________________________________

The Chemical Elements

Match-up:

____ 1- Groups or Families A- The vertical columns of elements in the Periodic Table are referred to as these.

____ 2- Non-metal B- The name for the horizontal rows of elements in the Periodic Table.

____ 3- Periods C- An element that is a good conductor of heat and electricity.

____ 4- Metalloid D- An element that is a poor conductor of heat and electricity.

____ 5- Metal E- An Element that has some properties characteristic of metals and

others characteristic of nonmetals.

Short Answer:

6: Cuprum is the older name for which element? ______________________

7: Aurum is the older name for which element? _______________________

8: Ferrum is the older name for which element? _______________________

9: Natrium is the older name for which element? ______________________

10: The elements in Group 18 are known as ____________ ____________

11: In reference to the Periodic Table, what are the groups? ____________________________________________

12: In reference to the Periodic Table, what are the periods? ____________________________________________

Fill-in-the-blanks:

13, 14, 15: The general _____________ among the ________________ of different elements provide one way of _________________ them.

16 : Because aluminum foil is ______________ , it resists breaking when reshaped, folded, or crumpled.

17: The ____________________ are also referred to as semimetals or semi-conducting elements.

The three general classes of elements are: 18: _______________ 19: ________________ 20: ________________.

21: A _________________ is somewhat like a metal, but not entirely.

22: All metals except for __________________ are solids under ordinary conditions.

True or False:

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

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

natures.

25) 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.

Units of Measurement

Match-up:

____ 1- Meter A- A physical quantity of a defined size.

____ 2- Fundamental Unit B- Objects or natural phenomena of constant value, easy to preserve

and reproduce, and practical in size that are used to define units for measuring.

____ 3- Kilogram C- The abbreviation for the International System of Units.

____ 4- Conversion Factor D- A unit that is defined by a physical standard of measurement.

____ 5- Second E- The SI standard unit for length.

____ 6- Factor-label F- The SI standard unit for mass.

____ 7- Derived Unit G- The SI standard unit for time.

____ 8- Density H- A problem solving method based upon treating units in calculations

as if they are algebraic factors.

____ 9- Volume I- A ratio derived from the equality between two different units and can

be used to convert from one unit to the other.

____ 10-Standards of Measurements J- A unit that can be obtained from combinations of fundamental units.

____ 11- SI K- The amount of space occupied by an object.

____ 12-Unit of Measurement L- A ratio of the mass of an object or substance to it’s volume.

Short Answer:

What are the fundamental SI units for the following:

13) length: _____________ 14) mass: ________________ 15) time: ________________

16) temperature: __________________ 17) amount of substance: _________________

18: The system that uses units of inches, ounces, and pounds is known as the __________________ system.

19: The measurement system used by most scientists and countries of the world is the ________

Fill-the-chart:

20 - 41

|Prefix |Symbol |Exponential Factor |Meaning |

|tera | | |1,000,000,000,000 |

|giga |G | | |

|mega | | |1,000,000 |

| |k |103 | |

|hecto | | |100 |

|deca |da | | |

|deci | | |1/10 (0.1) |

|centi | |10-2 | |

|milli | | |1 / 1,000 (0.001) |

|micro |µ | |1 / 1,000,000 (0.000001) |

|nano | |10-9 | |

|pico | | | |

Conversions:

42) 43) Express 24 meters in: centimeters; __________________ kilometers; _________________

44) 45) Express 5.6 kilograms in: grams; __________________ milligrams; _____________

*** continued on back ***

Calculations: Calculate the following:

46) 2 kg x 6 kg = ________

47) 2 m x 6 m = ________

48) 4 quarters ÷ 1 dollar = ________ (don’t forget to convert)

49) 75 dollars x 4 quarters = ________ ___________ (don’t forget to cancel units)

1 dollar

50) 40 cm x 2 cm = _________ (don’t forget to reduce)

8 square

51) The density for a substance that has a mass of 600 grams and a volume of 20 cm3

52) The mass for a 40 mL solution sample that has a density of 2 grams per mL

53) The volume of a substance that weighs 10 grams and has a density of 2 grams per cm3

54) What volume of water, in liters, would be required to fill a tank 30 cm long, 20 cm wide, and 10 cm deep?

True or False:

55) T / F : Fundamental Units are also known as “Base Units”.

56) T / F : One liter is equal to one cubic decimeter.

57) T / F : 1 cg = 10 mg

58) T / F : 1 g = 100 cg

59) T / F : The volume of most kinds of matter changes with temperature.

60) T / F : To “calibrate” a measuring device means to adjust its scale reading to agree with a measurement

standard.

Circle the answer:

61) What is more dense, cork or lead ?

62) What is more dense, a gas or a liquid ?

63) The area of a circle would be expressed in units that are: squared cubed other

64) The volume of a liquid would be expressed in units that are: squared cubed other

Heat and Temperature

Match-up:

____ 1- Celsius A- A measure of the average kinetic energy of the particles in a sample of matter.

____ 2- Calorie B- The sum total of the kinetic energies of the particles in a sample of matter.

____ 3- Heat Capacity C- A unit of temperature developed by some Swedish astronomer guy.

____ 4- Joule D- The unit of temperature developed by an English Lord and is the fundamental SI unit for temperature.

____ 5- Specific Heat E- The degree scale for temperature used by the United States.

____ 6- Kelvin F- An older unit originally defined as the quantity of heat required to raise the temperature of 1 g of water from 14.5 degrees C to 15.5 degrees C.

____ 7- Temperature G- The amount of heat energy needed to raise the temperature of a given sample of matter by one Celsius degree.

____ 8- Heat (heat energy) I- The amount of heat energy required to raise the temperature of 1g of a substance by one Celsius Degree.

____ 9- Fahrenheit J – The SI unit for heat energy and all forms of energy.

Short Answer:

10) Distinguish between temperature and heat, and then state the SI units for each. _____________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________________

11) Give the names of the two temperature scales that are commonly used in chemistry.

_______________________________________________________________________________________

12) How much heat would be absorbed by 75 g of iron, which has a specific heat index of 0.444, when heated

from 22 degrees C to 28 degrees C? _______________________________________________________________________________________

Conversions:

13) Convert 30 degrees C to K. ___________________________________________________________

14) Convert -20 degrees C to K ___________________________________________________________

15) Convert 200 K to degrees C __________________________________________________________

16) Convert 110 calories to J _____________________________________________________________

17) Convert 22 kJ to calories _____________________________________________________________

18) Convert 275 calories to joules ________________________________________________________

19) Convert 355 calories to kilojoules _____________________________________________________

20) Convert 55 calories to joules _________________________________________________________

21) Convert 650 joules to calories _________________________________________________________

*** continued on back ***

Calculations: Calculate the following:

A 4.0 g sample of glass was heated from 0oC to 41oC and was found to have absorbed 32 J of heat.

22) What is the specific heat of this type of glass? _____________________________________________________________________________

23) How much heat did the same glass sample gain when it was heated from 41oC to 70o ___________________________________________________________________________________________________________________

24) Determine the specific heat of a material if a 12 g sample absorbed 48 J as it was heated from 20oC to 40oC. ______________________________________________________________________________

True or False:

25) T / F : Normal boiling and freezing points are those at 1 atm.

26) T / F : The direction of heat flow is determined by the temperature differences between two masses.

27) T / F : If the final temperature is lower than the initial temperature, then delta t is negative.

Chart: Complete the following chart:

28 - 39

|Kelvin |Celsius |Fahrenheight | |

|373.15 | | |Boiling point of water |

| |0o | |Freezing point of water |

| | |-320.44 |Boiling point of nitrogen |

| |-273.15 | |Lowest possible temp. |

|6,000 | | |The sun’s surface temp. |

| | |100 |Current temp outside |

Using Scientific Measurements

Match-up:

____ 1- Significant Figures A- Refers to the closeness of a measurement to the true or accepted value of the quantity measured.

____ 2- Precision B- Refers to the agreement among the numerical values of a set of

measurements of the same quantity made in the same way.

____ 3- Scientific Notation C- The numerical values in a measurement that consist of all the digits

that are known with certainty plus one final digit, which is

uncertain or estimated.

____ 4- Accuracy D- Numbers that are written in the form M x 10n.

Multiple Choice:

5) 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: (circle one)

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

6) 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: (circle one)

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

7) 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: (circle one)

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

Conversions:

8) In scientific notation Avogardo’s number is 6.022 x 1023. Write this number in non-scientific notation. _________________________________________________________________________________

9) The mass of an electron is 0.0000000000000000000000000000009109 kg. Write this number in scientific notation: ___________________________________________________________

Diagram: Refer to the following three scales (A, B, C) for questions # 10 - 12

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

10) Which scale will have readings up to three ( 3 ) significant figures? A B C

11) Which scale will have readings up to two ( 2 ) significant figures? A B C

12) Which scale will have readings up to one ( 1 ) significant figures? A B C

*** continued on other side ***

True or False:

13) T / F : A set of measurements can be both accurate and precise.

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

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

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

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

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

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

20) T / F : Exact conversion factors have no uncertainty numbers.

21) T / F : Exact numbers can be considered to have an unlimited number of sig figs.

Rounding Off:

Round the following numbers to three (3) significant figures.

22) 42.68 g = _________________

23) 17.32 m = ________________

24) 2.7851 cm = _______________

25) 4.635 kg = ________________

26) 78.65 mL = _______________

Round off each of the following measurements to the indicated number of significant figures.

27) 35.27 g -- 3 sig figs: ___________________

28) 0.414 kL -- 2 sig figs: __________________

29) 87.257 dm -- 3 sig figs: ________________

30) 1.35K -- 2 sig figs: ____________________

31) 6250 cm -- 2 sig figs: __________________

32) 6.42 g -- 2 sig figs: ____________________

33) 7.535 mL -- 3 sig figs: _________________

34) 4.681 cm -- 2 sig figs: _________________

35) 56.45 kg -- 3 sig figs: _________________

*** continued on other side ***

Chart: Complete the following chart:

| |Measurement Examples |Number of Sig Figs |

|36 |438 g | |

|37 |26.42 m | |

|38 |1.7 cm | |

|39 |0.653 L | |

|40 |506 dm | |

|41 |10,050 mL | |

|42 |900.43 kg | |

|43 |4830 km | |

|44 |60 g | |

|45 |4830.0 L | |

|46 |60.0 K | |

|47 |0.06 g | |

|48 |0.0047 L | |

|49 |0.005o C | |

|50 |0.8 g | |

|51 |8.0 g | |

|52 |16.40 dm | |

|53 |35.000 L | |

|54 |1.60 sec | |

|55 |605.03 g | |

|56 |0.00603 mL | |

|57 |450 m | |

|58 |300.0 dm | |

|59 |0.8030 L | |

|60 |20.00 cm | |

|61 |0.000070 kg | |

|62 |350.0 K | |

*** continued on other side ***

Calculations: Calculate the following and express your answers with the correct number of sig figs:

63) 213.67 m + 98 m = _____________________________________

64) 6.43 L + 2.015 L = ____________________________________

65) 6.821 g + 2.0 g = _____________________________________

66) 107.38 km – 65 km = _____________________________________

67) 12.0 cm x 4.3 cm = ______________________________________

68) 2.50 g ÷ 0.04 cm3 = _____________________________________

69) 26.50 dm x 0.062 dm = ___________________________________

70) 1.30 mL ÷ 0.02 mL = _____________________________________

71) 2.30 cm x 10 cm x 6.01 cm = _______________________________

72) (6.3 x 104) + (2.1 x 105) = __________________________________

73) (23.5 x 105) – (2.35 x 106) = ________________________________

74) (6.85 x 107) ÷ (2.0 x 103) = _________________________________

75) (9.9 x 105) ÷ (3.0 x 1010) = _________________________________

76) (6.81 x 1010) ÷ (1.2 x 10-2) = ________________________________

77) (4.3 x 108) x (2.51 x 10-4) = _________________________________

78) (3 x 107) + (5 x 106) = _____________________________________

79) (4.6 x 105) + (3.2 x 105) = __________________________________

80) (5.7 x 106) x (2.8 x 109) = __________________________________

81) (7.7 x 10-12) ÷ (2.5 x 105) = __________________________________

82) 430.62 m + 6.1 m + 10.5300 m = _____________________________

83) 804.00 g ÷ 20 cm3 = ______________________________________

84) 68 – 3.1 x 103 = __________________________________________

85) 55.5 x 10-2 + .445 = _______________________________________

*** continued on other side ***

Chart: Complete the following chart:

| |Number |Scientific Notation |

|86 |4,325,045.2 | |

|87 |0.00000361 | |

|88 |85,000,000 | |

|89 |0.0009 | |

|90 |74,000 | |

|91 |0.000005 | |

|92 |30,000,000,000 | |

|93 |864,000 | |

|94 |0.000602 | |

|95 |4700 | |

|96 | |2.31 x 10-7 |

|97 | |5.3 x 104 |

|98 | |7 x 10-5 |

|99 | |4.2 x 10-6 |

|100 |45,000 | |

|101 |0.0000027 | |

|102 | |301 x 1011 |

Solving Quantitative Problems

Match-up:

____ 1- Variable A- A quantity that can change in value.

____ 2- inversely proportional B- A relationship between two variables in which dividing one by the other

gives a constant value.

____ 3- directly proportional C- A relationship between two variables in which their product has a constant

value.

Short Answer:

4) List and explain the four steps in problem solving.

1-__________________________________________________________________________________

2-__________________________________________________________________________________

3-__________________________________________________________________________________

4-__________________________________________________________________________________

Calculations:

5) Calculate the number of seconds in exactly one week. Answer here:_____________

6) What is the volume of a 12 g piece of gold? (d = 19.3 g/cm3 ) Answer here: _____________

7) An object travels at a speed of 7500 cm / s. How far will it travel in a day? Answer here: ____________

What type of relationship is illustrated between the variables A and B in each of the following?

8) As A increases, B decreases, and A x B = 35 ____________________________

9) As A increases, B increases, and A / B = ½ . _____________________________

The Atom

Match-up:

____ 1- Law of Multiple Proportions A- A law used in science that states: Matter can neither be created nor destroyed.

____ 2- 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.

____ 3- Law of Definite Composition C- A law used in science that states: Energy can neither be created nor destroyed.

____ 4- Law of Conservation of Energy D- A law used in science that states: Every chemical compound has a definite composition by mass.

____ 5- Law of Murphy E- A law proposed by some Irish dude that states: Anything that can go wrong, will go wrong.

____ 6- Law of Teenagers F- A myth that exists amongst teenagers that states: Everyone in the world doesn’t know what they’re talking about and thus can never prove I am wrong; therefore, I know everything and am always right no matter what people say or can prove otherwise so don’t even try cuz if you do I’ll just tune you out and do my own thing anyways and be rich some day despite the way you put me down in front of my friends who agree with me and support my every decision no matter how ridiculous and crazy you think it is so like, you know, stop hassling me dude and like chill and get off my case man.

Short Answer:

7 -11) List the five essential points of Dalton’s atomic theory:

1-__________________________________________________________________________________

2-__________________________________________________________________________________

3-__________________________________________________________________________________

4-__________________________________________________________________________________

5-__________________________________________________________________________________

True or False:

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

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

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

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

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

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

Fill-in-the-blanks:

18: ________________________ was the name of the Greek dude that lived around 400 BC who came up with the name “Atom” for tiny particles that can’t be divided any further.

19: ________________________ , another Greed dude who lived about 50 years later than the Greek dude in number xx above did not believe in atoms, but rather that all matter was ____________________________ .

20: Over 2,000 years later than the Greek dudes above, an English dude named _____________ ______________ , who was a school teacher, developed a theory that in five basic statements summarizes the Atomic Model.

Chart: Complete the following chart:

|Quiz # |Compound Name |Compound Symbol |

|21 |Carbon Monoxide | |

|22 | |CO2 |

|23 |Di-hydrogen Monoxide | |

|24 | |NaCl |

|25 | |C6H12O6 |

|26 |Sulphuric Acid | |

|27 |Hydrochloric Acid | |

|28 |Nitric Acid | |

|29 | |CaCO3 |

|30 |Hydrogen Peroxide | |

|31 |Ethanol | |

Short Essay: ( Small writing; bonus points for cursive, must fill-up rest of page.)

32) Topic: What laws can be explained through the use of Dalton’s theory? ( 20 points)

Instructions: State each law and describe how Dalton’s atomic theory can be used to explain the law.

Hint: There are 4 laws mentioned in this quiz that can be explained using Dalton’s theory.

The Structure of the Atom

Match-up:

____ 1- Atom A- The short-range proton-neutron, proton-proton, and neutron-neutron forces that hold the nuclear particles within an atom together.

____ 2- Atomic Structure B- The identity and arrangement of smaller particles within atoms.

____ 3- Electron C- A negatively charged sub-atomic particle.

____ 4- Nucleus D- The positively charged dense center portion of the atom that contains nearly all of it’s mass but takes up only an insignificant fraction of it’s volume.

____ 5- Proton E- A subatomic particle that has a positive charge equal in magnitude to the negative charge of an electron and is present in atomic nuclei.

____ 6- Neutron F- Atoms of the same element that have different masses.

____ 7- Nuclear Forces G- The smallest unit of an element that can exist alone or in combination with other elements.

____ 8- Isotopes H- An electrically neutral, sub-atomic particle found in atomic nuclei.

True or False:

9) T / F : Hydrogen and its isotopes have different nuclei.

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

11) T / F : Every element has isotopes.

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

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

Fill-in-the-blanks:

14: The discovery of _________________ was made in 1897 by an English physicist dude named Sir Joseph John Thompson who built and used cathode-ray tubes to identify these sub-atomic ______________. Although cathode-ray tubes were useful in figuring-out the structure of the ___________, their real usefulness came about 50 years later when they were used to make the first _________ sets in America which resulted in the end of the radio entertainment era. Further refinement of the cathode-ray tube, which energizes different types of ________ to make different colors, resulted in a type of sign that used to light-up the __________ strip but are now a rare sign to see.

15: An American physicist dude named Robert Millikan figured out the mass of an __________________ in 1909.

16: In 1909 a dude from New Zealand named Ernest Rutherford discovered that the atom has a _________________ and that it gives off a ___________________ charge.

17: In 1986, the ______________ Prize in science achievement was shared by Ernst Ruska, Gerd Binning, and Heinrich Rohrer for their work on ________________________.

Diagram:

18) In the space below, make a model sketch of the Lithium atom showing and labeling all sub-atomic particles and their proper locations. (12 points)

Short Essay: ( Small writing; bonus points for cursive, must fill-up rest of page.) ( 20 points )

19) Explain how the three isotopes of hydrogen compare in terms of the numbers of sub-atomic particles in each.

Hint: This is basically the definition of an isotope but in more detail.

Weighing and Counting Atoms

Match-up:

____ 1- Atomic Number A- The number of particles in exactly one mole of a pure substance.

____ 2- Mass Number B- The amount of a substance that contains the same number of particles as the number of atoms in exactly 12 grams of carbon-12.

____ 3- Nuclide C- The relative atomic mass of atoms of a nuclide.

____ 4- Atomic Mass Unit D- The weighted average of the atomic masses of the naturally occurring isotopes of an element.

____ 5- Atomic Mass E- A general term for any isotope of any element.

____ 6- Average Atomic Mass F- Symbolized by the letter u, and is exactly 1/12th the mass of a carbon-12 atom, or 1.66 x 10-24 grams.

____ 7- Nuclide Atomic Mass G- The mass of an atom that is expressed in atomic mass units.

____ 8- Mole H- The total number of protons and neutrons in the nucleus of an isotope.

____ 9- Avogadro’s Number I- The abbreviation for the Mole.

____ 10- Molar Mass J- The number of protons in the nucleus of each atom of that element.

____ 11- mol K- The mass in grams of one mol of an element.

Calculations:

12 – 15) Determine the number of protons, electrons, and neutrons in each of the following isotopes.

12) sodium-23 | 13) calcium-40

P = _________ | P = _________

|

E = _________ | E = _________

|

N = ________ | N = ________

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

14) 6429 Cu | 15) 10847 Ag

P = _________ | P = _________

|

E = _________ | E = _________

|

N = ________ | N = ________

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

16 – 18) Determine and write both the nuclear symbol and the hyphen notation for each of the following described neutral isotopes using the given information.

16) Mass number = 28, Atomic number = 14

17) 26 Protons and 30 Neutrons

18) 56 Electrons and 82 Neutrons

Calculations continued:

19) To three decimal places, what is the relative atomic mass of Potassium ? ____________________________

20) To three decimal places, what is the molar mass of Calcium ? ______________________________

21) What is the mass in grams of 2.00 mol N ? _______________________________

22) What is the mass in grams of 3.01 x 1023 atoms of Cl ? _________________________

23) How many moles are in 12.15 g Mg ? ______________________________

24) How many moles are in 1.50 x 1023 atoms of F ? ____________________________

25) How many atoms are contained in 2.50 mol Zn ? ____________________________

26) How many atoms are contained in 1.50 g C ? _____________________________

True or False:

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

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

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

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

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

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

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

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

Last question:

159) Which one of the following is NOT part of a lab report ?

a) hypothesis b) conclusion c) methods d) theory e) results

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

2H + O ’! H2O

A

C

B

b)

→ H2O

A

C

B

................
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