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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 d) potential and mechanical c) kinetic and potential 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 d) a stretched rubber band c) a boulder at the top of a hill 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 *** continued *** e) weight 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 d) the melting of ice c) explosion of a firecracker 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 *** continued *** d) neither a nor b 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: 2H + O → H2O 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 *** continued *** e) both b & c 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 nonreactive 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. B A C 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 c) Mass d) Matter e) Energy c) Mass d) Matter e) Energy c) Mass d) Matter e) Energy 76) A measure of the earth’s gravitational attraction for matter. a) Inertia b) Weight 77) A measure of the quantity of matter. a) Inertia b) Weight 78) Anything that has mass and occupies space. a) Inertia b) Weight 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 108) 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: 109) If the mass of a solute is 10 g and its volume is 2 ml, what is its density ? a) 0.05 g/ml 110) d) 50 g/ml e) 500 g/ml b) 1.00 g c) 10.0 g d) 100 g e) 0.01 g If the density of a solvent is 6 g/ml and its mass is 120 g, what is its volume ? a) .002 ml 112) c) 5.0 g/ml If the density of a solution is 20 g/ml and its volume is 5.0 ml, what is its mass ? a) .100 g 111) b) 0.5 g/ml b) .02 ml c) .20 ml d) 2.0 ml e) 20 ml 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. 113) _______ Substance 114) _______ Evaporation 115) _______ System 116) _______ Percentage 117) _______ Calculate 118) _______ Value 119) _______ Conclusion 120) _______ Procedure 121) _______ Record 122) _______ Physical Change 123) _______ Chemical Change 124) _______ Reversible 125) _______ Irreversible 126) _______ Complex 127) _______ Informative 128) _______ Uniformly 129) _______ Fermentation 130) _______ Effervescent 131) _______ 132) Give three ( 3 ) examples of numbers that have digits in two decimal places. ________________ 133) ________________ The investigation manual uses the word “test” often during experiments. Is this a correct usage of the word test? (circle one) 134) __________________ yes no Where else in the world of science is the term “test” used? _______________________________ _______________________________________________________________________________ Inv # 3 Term match-up: Match the term with its definition. 135) _____ Property ( as used in science, not real estate ) 136) _____ Sample 137) _____ Appropriate 138) _____ Alcohol 139) _____ Graduated ( as it applies to glassware ) 140) _____ Collect 141) _____ Transfer 142) _____ Density 143) _____ Relationship 144) _____ Average 145) _____ Apparatus 146) _____ Compare 147) _____ Determine 148) _____ Evidence 149) _____ Experiment 150) _____ Appearance 151) _____ Cylindrical 152) _____ Assume 153) _____ Absorb 154) _____ Displacement 155) _____ Scientific Hypothesis 156) _____ Scientific Theory 157) _____ 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 _____ 2 – Matter A- Resistance to change in motion. 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? ____________________________________________ 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 ____ 2- Fundamental Unit ____ 3- Kilogram ____ 4- Conversion Factor ____ 5- Second ____ 6- Factor-label ____ 7- Derived Unit ____ 8- Density ____ 9- Volume ____ 10-Standards of Measurements ____ 11- SI ____ 12-Unit of Measurement A- A physical quantity of a defined size. 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. C- The abbreviation for the International System of Units. D- A unit that is defined by a physical standard of measurement. E- The SI standard unit for length. F- The SI standard unit for mass. G- The SI standard unit for time. H- A problem solving method based upon treating units in calculations as if they are algebraic factors. I- A ratio derived from the equality between two different units and can be used to convert from one unit to the other. J- A unit that can be obtained from combinations of fundamental units. K- The amount of space occupied by an object. 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: ________________ 16) temperature: __________________ 15) time: ________________ 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 tera giga mega Meaning 1,000,000,000,000 G 1,000,000 k hecto deca deci centi milli micro nano pico Exponential Factor 3 10 100 da 1/10 (0.1) 10-2 1 / 1,000 (0.001) 1 / 1,000,000 (0.000001) µ 10-9 Conversions: 42) 43) Express 24 meters in: centimeters; __________________ kilometers; _________________ 44) 45) Express 5.6 kilograms in: grams; __________________ milligrams; _____________ Calculations: Calculate the following: 46) 2 kg x 6 kg = ________ 47) 2 m x 6 m = ________ 48) 4 quarters ÷ 1 dollar = ________ 49) 75 dollars x 4 quarters = ________ ___________ 1 dollar 50) 40 cm x 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? 2 cm = _________ 8 square (don’t forget to convert) (don’t forget to cancel units) (don’t forget to reduce) 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 64) The volume of a liquid would be expressed in units that are: cubed squared other cubed other Heat and Temperature Match-up: ____ 1- Celsius ____ 2- Calorie ____ 3- Heat Capacity ____ 4- Joule ____ 5- Specific Heat ____ 6- Kelvin ____ 7- Temperature ____ 8- Heat (heat energy) ____ 9- Fahrenheit A- A measure of the average kinetic energy of the particles in a sample of matter. B- The sum total of the kinetic energies of the particles in a sample of matter. C- A unit of temperature developed by some Swedish astronomer guy. D- The unit of temperature developed by an English Lord and is the fundamental SI unit for temperature. E- The degree scale for temperature used by the United States. 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. G- The amount of heat energy needed to raise the temperature of a given sample of matter by one Celsius degree. I- The amount of heat energy required to raise the temperature of 1g of a substance by one Celsius Degree. J – The SI unit for heat energy and all forms of energy. 10) Give the names of the two temperature scales that are commonly used in chemistry. _______________________________________________________________________________________ 11) 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: 12) Convert 30 degrees C to K. ___________________________________________________________ 13) Convert -20 degrees C to K ___________________________________________________________ 14) Convert 200 K to degrees C __________________________________________________________ 15) Convert 110 calories to J _____________________________________________________________ 16) Convert 22 kJ to calories _____________________________________________________________ 17) Convert 275 calories to joules ________________________________________________________ 18) Convert 355 calories to kilojoules _____________________________________________________ 19) Convert 55 calories to joules _________________________________________________________ 20) Convert 650 joules to calories _________________________________________________________ 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. 21) What is the specific heat of this type of glass? _____________________________________________________________________________ 22) How much heat did the same glass sample gain when it was heated from 41oC to 70o ___________________________________________________________________________________________________________________ 23) 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: Kelvin Celsius Fahrenheight 373.15 Boiling point of water 0o Freezing point of water -320.44 -273.15 Boiling point of nitrogen Lowest possible temp. The sun’s surface temp. 6,000 100 Current temp outside Using Scientific Measurements Match-up: ____ 1- Significant Figures ____ 2- Precision ____ 3- Scientific Notation ____ 4- Accuracy A- Refers to the closeness of a measurement to the true or accepted value of the quantity measured. B- Refers to the agreement among the numerical values of a set of measurements of the same quantity made in the same way. 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. 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 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: _________________ Chart: Complete the following chart: Measurement Examples 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 Number of Sig Figs 57 450 m 58 300.0 dm 59 0.8030 L 60 20.00 cm 61 0.000070 kg 62 350.0 K 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 = _______________________________________ Chart: Complete the following chart: Number 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 Scientific Notation 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 ____ 2- inversely proportional ____ 3- directly proportional A- A quantity that can change in value. B- A relationship between two variables in which dividing one by the other gives a constant value. 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 ____ 2- Law of Conservation of Mass ____ 3- Law of Definite Composition ____ 4- Law of Conservation of Energy A- A law used in science that states: Matter can neither be created nor destroyed. 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. C- A law used in science that states: Energy can neither be created nor destroyed. D- A law used in science that states: Every chemical compound has a definite composition by mass. 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 21 Carbon Monoxide 22 23 Compound Symbol CO2 Di-hydrogen Monoxide 24 NaCl 25 C6H12O6 26 Sulphuric Acid 27 Hydrochloric Acid 28 Nitric Acid 29 CaCO3 30 Hydrogen Peroxide 31 Ethanol The Structure of the Atom Match-up: ____ 1- Atom ____ 2- Atomic Structure ____ 3- Electron ____ 4- Nucleus ____ 5- Proton ____ 6- Neutron ____ 7- Nuclear Forces ____ 8- Isotopes A- The short-range proton-neutron, proton-proton, and neutron-neutron forces that hold the nuclear particles within an atom together. B- The identity and arrangement of smaller particles within atoms. C- A negatively charged sub-atomic particle. 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. 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. F- Atoms of the same element that have different masses. G- The smallest unit of an element that can exist alone or in combination with other elements. 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 Boron atom showing and labeling all sub-atomic particles and their proper locations. (12 points) 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. C- The relative atomic mass of atoms of a nuclide. ____ 3- Nuclide ____ 4- Atomic Mass Unit ____ 5- Atomic Mass D- The weighted average of the atomic masses of the naturally occurring isotopes of an element. E- A general term for any isotope of any element. ____ 7- Nuclide 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. 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. ____ 6- Average Atomic Mass 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. Chemistry Investigation # 5 Pre-read Quiz / 54 1. Define “Composition”: ______________________________________________________________ 2. Define “Compound”: _______________________________________________________________ 3. Define “Formula”: ________________________________________________________________ 4. Define “Exploration”: ______________________________________________________________ 5. Define “Residue”: _________________________________________________________________ 6. Define “Integer”: __________________________________________________________________ 7. Define “System”; _________________________________________________________________ 8. Explain what an “evaporating dish” is: _______________________________________________ 9. Explain what a “crucible” is: ________________________________________________________ 10. Explain the difference between an “evaporating dish” and a “crucible” is: _____________________ 11. A student weighs a crucible and a crucible lid three times ( 3 trials ) and obtains the following data: trial # 1: 5.02 grams trial # 2: 4.96 grams trial # 3: 5.00 grams What is the average weight of the crucible w/ lid? ______________________ A student puts a strip of magnesium metal ribbon in a crucible and covers the crucible with a lid then weighs the system three times and obtains the following weights: trial # 1: 7.02 grams trial # 2: 6.96 grams trial #3: 7.00 grams 12. What is the average weight of the system? ______________________ 13. What is the calculated weight of the magnesium? ______________________ 14. Explain what it means to heat a system gently. ________________________________________ _______________________________________________________________________________ 15. Explain what it means to heat a system strongly. _____________________________________ ______________________________________________________________________________ 16. Explain what a mathematical operation is: ____________________________________________ ______________________________________________________________________________ 17. List the four ( 4 ) basic operations of mathematics: _____________________________________ _____________________________________ _____________________________________ _____________________________________ 18. Give the symbol for magnesium: ______________ 19. Give the name for Mg: ______________________ 20. Give the symbol for copper: __________________ 21. Give the symbol for sulphur: _________________ 22. Give the symbol for oxygen: _________________ 23. Give the formula for the compound: sulfate ____________________ 24. Give the formula for the compound: copper (II) sulfate ____________________________________ 25. Explain what “hydrated” means: _______________________________________________________ 26. Explain what it means to make a “prediction”: ____________________________________________ __________________________________________________________________________________ 27. Explain what “Expansion of an Idea” means: _____________________________________________ __________________________________________________________________________________ Chemistry Investigation # 4 Pre-read Quiz 28. Define “Pure Substance”: ______________________________________________________________ 29. Define “Heating”: ________________________________________________________ 30. Define “Cooling”: _______________________________________________________ 31. Define “ Physical Change”: _________________________________________________________ 32. Define “Chemical Change”: _________________________________________________________ 33. Define “System”; _________________________________________________________________ 34. Define “ Evidence” : ______________________________________________________________ 35. How many phases ( or states ) of matter are there? _______________ and what are their names? : ______________________ 36. Are phase changes physical _______________________ or chemical _____________________ in nature? ( circle one ) 37. What is a coordinate axis? ( hint: think graph ) _____________________________________________ Chemistry Investigation # 2 Pre-read Quiz 38. Define “Evaporation”: ______________________________________________________________ _______________________________________________________________ Round the following weights to two ( 2 ) decimal places: ( don’t forget to include the units ) 39. 05.8556 g ______________ 40. 11. 45678 g ______________ 41. 3.9876 g ______________ 42. 1.94587 g ______________ 43. Define “Physical Property”: ________________________________________________________ 44. Define “Chemical Property”: _______________________________________________________ 45. Define “ Physical Change”: _________________________________________________________ 46. Define “Chemical Change”: _________________________________________________________ 47. Define “system”; _________________________________________________________________ 48. Give the chemical formula for ordinary table salt: _______________ 49. Give the chemical formula for the element Calcium: _____________ Chemical Names and Formulas Terms: Define the following terms: Chemical name: Chemical formula: Chemical compound: ion: monatomic ion: binary compound: Nomenclature: polyatomic ion: oxyanion: oxyacid: salt: Oxidation Numbers Match-up: ____ 1- Oxidation number A- Numbers that are assigned to the atoms in molecules, icluding molecular ions, to show the general distribution of electrons among the bonded atoms. ____ 2- Oxidation state B- Also called oxidation state. True or False: 3) T / F : An uncombined element has an oxidation number of zero. 4) T / F : A monatomic ion has an oxidation number equal to its charge. 5) T / F : Flourine has an oxidation number of -1 in all compounds. 6) T / F : Oxygen has an oxidation number of -2 in almost all compounds. 7) T / F : Hydrogen has an oxidation number of -1 in all compounds except those with metals, in which it has an oxidation number of +1. 8) T / F : The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 9) T / F : The algebraic difference of the oxidations number of all atoms in a polyatomic ion is equal to zero. 10) T / F : The algebraic sum of the oxidation numbers of all atoms in a neutral compound is equal to the charge of the ion. Fill-in-the-blank: Select the word or phrase that best completes each sentence. 11. Oxidation numbers are also called oxidation ________________ . a. States b. Levels c. Charges d. Elements e. Atoms 12. The algebraic ________ of the oxidation numbers of all atoms in a neutral compound is ______ . b. Sum , Zero b. Difference , Neutral c. Difference , Zero 13. The algebraic ________ of the oxidation numbers of all atoms in a ____________ ion is equal to the charge of the ion. c. Total , Monatomic b. sum , diatomic c. sum , polyatomic 14. An uncombined element has an oxidation number of ________. d. three b. two c. one d. zero 15. A _____________ ion has an oxidation number equal to its charge. e. polyatomic b. monatomic c. catatomic d. diatomic Using Chemical Formulas Multiple Choice: Select the term that best fits the given definition. 2. 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 3. The percent by mass of each element in a compound. a. mass composition b. mass percent c. percent composition Calculations: For each of the following tasks, select the correct answer. 4. Calculate the formula mass for H2SO4. a. 9.807 u b. .9807 u c. 98.07 u d. 980.7 u e. .09807 u d. .16409 u e. 164.09 u 5. Calculate the formula mass for Ca(NO3)2. a. 16.409 u b. 1.6409 u c. 1640.9 u 6. Calculate the molar mass for NaNO3. a. 8.49947 g b. 84.9947 g c. 849.947 g d. .849947 g c. 17.134 g d. 171.34 g 7. Calculate the molar mass for Ba(OH)2. a. .17134 g b. 1.7134 g 8. 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 9. 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 10. 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 11. Calculate the percent composition of lead in PbCl2. a. .7451 % b. 7.451 % c. 74.51 % d. 745.1 % 12. Calculate the percent composition of barium in Ba(NO3)2. a. .52548 % b. 5.2548 % c. 52.548 % d. 525.48 % 13. 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 Match-Up: For each of the following terms on the left, select from the right its definition. A – The form of a formula that consists of the symbols for the elements combined, with subscripts showing the smallest whole-number ratio of the atoms. 2) _____ empirical formula B – Another way to say “Empirical Formula”. 1) _____ simplest formula Calculations: Evaluate each of the following word problems. 3) A compound is found to contain 36.48% sodium, 25.41% sulfur, and 38.02% oxygen. Find it’s simplest formula. 4) Find the simplest formula of a compound found to contain 53.70% iron and 46.30% sulfur. 5) Analysis of a compound indicates that it contains 1.04 g K, 0.70 g Cr, and 0.82 g O. Find it’s simplest formula. 6) If 4.04 g N combine with 11.46 g O to produce a compound with a formula mass of 108.0 u, what is the molecular formula of this compound? 7) The formula mass of a compound is 92 u. Analysis of a sample of the compound indicates that it contains 0.606 g N and 1.390 g O. Find it’s molecular formula. History of the Periodic Table Match-up: ____ 1- Ionic Radius ____ 2- Atomic Radius ____ 3- Ionization Energy ____ 4- Electronegativity ____ 5- Anion ____ 6- Cation ____ 7- Valence Electron ____ 8- Ionization A- One half the distance between the nuclei of identical atoms joined in a molecule. B- Any process that results in the formation of an ion. C- The energy required to remove one electron from an atom of an element. D- One half the diameter of an ion in an ionic compound. E- An ion with a positive charge. F- An ion with a negative charge. G- The electrons available to be lost, gained, or shared in the formation of chemical compounds. H- A measure of the ability of an atom in a chemical compound to attract electrons. True or False: 9) T / F : Atomic radii decrease from right to left across a period in the Periodic Table. 10) T / F : Atomic radii increase from down to up across a group in the Periodic Table. 11) T / F : Period trends are patterns that exist in the Periodic Table groups. 12) T / F : Group trends are patterns that exist in the Periodic Table periods. 13) T / F : Metals are more electronegative than non-metals. Short Answer: 15. State the general period and group trends among main-group elements with respect to each of the following: a. Atomic radii ____________________________________________________________________ b. First ionization energy ____________________________________________________________ c. Electron affinity _________________________________________________________________ d. Ionic radii ______________________________________________________________________ e. Electronegativity ________________________________________________________________ 16. Among the main-group elements, what is the relationship between group number and the number of valence electrons among group members? __________________________________________________________ _________________________________________________________________________________________ 17. ( part A ) In general, how do the periodic properties of the d-block elements compare with those of the maingroup elements? _________________________________________________________________________ __________________________________________________________________________________________ ( part B ) Explain your reasoning for the comparisons you made in part A above: ______________________ __________________________________________________________________________________________ __________________________________________________________________________________________ Rules for determining significant figures involving zeros _____________Rule________________________________________________Examples_____# of sig fig___ __________________________________________________________________________________________ 1. All nonzero digits are significant. 438 g 3 26.42 m 4 1.7 cm 2 0.653 L 3 2. All zeros between two nonzero digits are significant. 506 dm 10,050 mL 900.43 kg 3. Zeros to the right of a nonzero digit, but to the left of an understood decimal point, are not significant. If such zeros are known to have been measured, however, they are significant and should be specified as such by inserting a decimal point to the right of the zero. 3 4 5 4,830 km 3 1 60 g 4,830. L 60. K 4 2 4. In decimals less than one, zeros to the right of a decimal point that are to the left of the first non-zero digit are never significant. They are simply placeholders. 0.06 g 0.0047 L 0.005o 1 5. In decimals less than 1, the zero to the left of the decimal is never significant. It is there to make sure the decimal point is not overlooked. 0.8 g 1 6. All zeros to the right of a decimal point and to the right of a nonzero digit are significant. 8.0 dm 16.40 g 35.000 L 1.60 sec 2 2 1 4 5 3 Rules for Rounding Off Numbers If the digit immediately to the right of the last significant digit you want to retain is: Then the last significant Example (rounding for 3 digit should: significant figures): 1) Greater than 5 be increased by 1 42.68 g → 42.7 g 2) Less than 5 stay the same 17.32 m → 17.3 m 3) 5, followed by nonzero digit(s) be increased by 1 2.7851 cm → 2.79 cm 4) 5, not followed by nonzero digit(s), and preceded by an odd digit be increased by 1 4.635 kg → 4.64 kg (since 3 is odd) 5) 5, not followed by nonzero digit(s), and the preceding significant digit is even 78.65 mL → 78.6 mL (since 6 is even) stay the same In addition or subtraction, the arithmetic result should be rounded off so that the final digit is in the same place as the leftmost uncertain digit. In multiplication and division, the arithmetic product or quotient should be rounded off to the same number of significant figures as in the measurement with the fewest significant figures. T(K) = t(Co) + 273.15 t(Co) = 5/9 x [t(Fo) – 32] one calorie = 4.184 J specific heat = heat lost or gained / mass (g) x change in temperature (Co) SI prefixes Scientific notation 8 24 1000 10 1000000000000000000000000 Septillion Quadrillion 1E24 7 21 1000 10 1000000000000000000000 Sextillion Trilliard 1E21 6 18 1000 10 1000000000000000000 Quintillion Trillion 1E18 5 15 1000 10 1000000000000000 Quadrillion Billiard 1E15 4 12 1000 10 1000000000000 Trillion Billion 1E12 3 9 1000 10 1000000000 Billion Milliard 1E9 2 6 1000 10 1000000 Million 1E6 1 3 1000 10 1000 Thousand 1E3 2/3 2 1000 10 100 Hundred 1E2 1/3 1 1000 10 10 Ten 1E1 0 0 1000 10 1 One – −1/3 −1 1000 10 0.1 Tenth 1E-1 −2/3 −2 1000 10 0.01 Hundredth 1E-2 −1 −3 1000 10 0.001 Thousandth 1E-3 −2 −6 1000 10 0.000001 Millionth 1E-6 −3 −9 1000 10 0.000000001 Billionth Milliardth 1E-9 −4 −12 1000 10 0.000000000001 Trillionth Billionth 1E-12 −5 −15 1000 10 0.000000000000001 Quadrillionth Billiardth 1E-15 −6 −18 1000 10 0.000000000000000001 Quintillionth Trillionth 1E-18 −7 −21 1000 10 0.000000000000000000001 Sextillionth Trilliardth 1E-21 −8 −24 1000 10 0.000000000000000000000001 Septillionth Quadrillionth 1E-24 Prefix Symbol 1000m 10n yotta zetta exa peta tera giga mega kilo hecto deca Y Z E P T G M k h da deci centi milli micro nano pico femto atto zepto yocto d c m μ n p f a z y 1. Decimal Short scale Long scale ^ The metric system was introduced in 1795 with six prefixes. The other dates relate to recognition by a resolution of the CGPM. Since[n 1] 1991 1991 1975 1975 1960 1960 1960 1795 1795 1795 – 1795 1795 1795 1960 1960 1960 1964 1964 1991 1991