KEY- Unit 1 Notes Handouts

Chemistry 1 Honors Unit 1 Notes- Introduction to Chemistry and Properties of Matter Section 1- Introduction to Chemistry: What is Chemistry?   Matter- Anything that has ______________ and ________________________________. mass occupies space Chemistry- The study of ________________ and the __________________ it undergoes. matter changes Main Branches of Chemistry:       There are many different subcategories of Chemistry. We will discuss some more in depth than others. Organic Chemistry- The study of all chemicals that contain _____________. carbon Inorganic Chemistry- The study of all chemicals that do not contain ______________. carbon Biochemistry- The study of the processes that take place in _______________________. living organisms Analytical Chemistry- The study of the ____________________________ composition whatit's made of of matter. Physical Chemistry- The study of reaction __________________________, rates of mechanisms processes _________________, and _______________________ that occur in a change in matter. reactions transfers energy The Scientific Method:   A ___________________________ approach to a scientific problem. All good science is systematic logical based in the scientific method. Steps: o Make _________________________ Observations o Make a _________________ (a proposed ________________ of an observation) explanation hypothesis o Test using an __________________________ indicating ____________________ variables experiment  Independent variable- ___________________ variables that you change manipulated during an experiment.  Dependent variable- _____________________ during the experiment. observed Also called the _____________________ variable. responding o Analyze _________ results and either __________________ revise experiment or ____________________ publish results Finalizing Results:   Theory- a well-tested _______________________ of a set of observations. Theories explanation _______________ a process, result, or procedure and can change with new information. summarize Scientific Law- A ________________________________ of nature. A law is a concise fundamental rule statement that _________________ the results of many observations and experiments. summarizes Laws do not __________________ relationships but only ______________. They cannot summarize explain change. Section 2- Measurement and Data: What is a Measurement?   Measurement- a quantity that contains a _________________ and a _______________. unit number Many measurements are often very large or very small numbers so we represent them with ______________________________________. scientific notation  In scientific notation, a quantity is written as a coefficient times a power of _____. to  If the power of 10 is ____________, the number is ________________ or equal to 1. than positive greater  If the power of 10 is ____________, the number is _________________ 1. less than negative Converting Measurements to Scientific Notation:   When the decimal moves _______________, add 1 to the power of 10 for every space. left When the decimal moves _______________, subtract 1 from the power of 10 for every right space. Example 1: Convert the following measurements to Scientific Notation: 102 km 12,9 889 107km spaiesleftlposi.tn 3 8 88 spaces 2 left 0.88888885kg 31 1082 poi 6.5 10 7kg 7spaces right negative 0.8888888432g 8spaces right 1.32 10 8g negative Multiplying and Dividing in Scientific Notation:    ________________________ or _________________ the _______________________. Coefficients Divide Multiply ____________ or ________________ the powers of 10. if subtract Add if Convert to __________________________________________ if necessary. notation appropriate scientific Example 2: Perform the Operations: 3.2 106 3 4.5 10 13.18 108 9.48 10 3.2 5.4 5.4 109 9 5.7 10 4.5 5.7 7.81 1012 32.18 7 5 10 5 1 8 10 147.28 10 2,5 1018 1 65 0,407 1010 1.728 10 101 2.565 102 10 4 4.07 10 s 1.264 10 10 Adding and Subtracting in Scientific Notation:   When adding or subtracting numbers in scientific notation, the powers of 10 must be _________________. equal Steps: o Convert the _____________ power into the ____________ power by moving the smaller larger decimal to the ___________. left o Add or Subtract the ____________________. coefficients o Convert back into __________________________________ if necessary. scientific notation Example 3: Perform the Operations: 6.8 402 9.4 44.8 10 8 10 10 3 2 15,0 10 72.0 10 201 10 108 15.4 10 2 10 8 0.5 0 8 9 6.8 4 3 4.2 10 3 10.7 10 703 10 3 4.9 10 2 7.3 10 0.048 10 5.9 101 5.352 10 8 Units of Measurement:     In science, we use the ____________________________ to measure quantities. metrit system The metric system is the superior system of measurement because it is __________________________ 10 internationally standardized and every measurement is in multiples of ________. The metric system uses _________________ to indicate powers of 10 of base units. prefixes The _______________ are the 7 standard base units for all measurements. All other SI Units units can be derived from these units. SI Base Units: Quantity Length Mass Temperature Time Amount of a Substance Luminous Intensity Electric Current SI Base Unit meter kilogram Symbol m kg Kelvin K Mole mol Ampere of Second Candela s Common Metric Prefixes: Prefix MegaKiloCentiMilliMicroNanoPico- Symbol M k C m µ n p Other Common Metric Conversions: I 1 cm 1mL m 1000L Meaning 1 106 baseunits Munit 1,000,000units 1 103 base units I Kunit 1000units 2 1 10 baseunits 1unit 100 units 3 1 10 baseunits unit 1000munits 1 10 6base units lunit 1,000,000munits 1 10 9 baseunits 1unit 1,000,000,000nunit 1 10 baseunits lunit 1,000,000,000,000 puni Measuring Temperature: • Temperature is measured in __________________________________________. Celsius and Kelvin • Celsius Scale: • • ______ °C = Freezing Point of water • ______ °C = Boiling Point of water Kelvin Scale: • • Measures the ____________________________ in the particles of matter. kinetil energy ____ OK is the point where all motion of particles stops, also called ______________________________ absolute zero • Equation: _____________________________ K 2 273 Example 4:  Convert from Celsius to Kelvin: K 25 273 298K 25 C K 75 273 348K 75 C  Convert from Kelvin to Celsius: 205 205K 9 273 576 9 273 576K 680C 303K Measuring Density:   Density is the ratio of ___________________________________ of a substance. to volume mass Equation: Density mass volume Example 5:  3 A block has a volume of ___ 10 g. Calculate the density of the block. 15 cm and a mass of ___ D 152 0.6791cm  A block has dimensions of ___ 20 cm x ___ 10 cm and a mass of _______ is cm x ___ 2500 g. Calculate the density of the block. Assume the block is a rectangular, right prism. V 15cm 20cm 10cm 3000cm D Y 38 4 D 0.8391cm Section 3- Unit Conversions: Unit Conversions using Dimensional Analysis:    Dimensional Analysis is a way to_________________ from one unit to another unit convert using a ___________________________________ conversion factor A conversion factor is a known ratio between_______________________________. two equivalent units DIMENSIONAL ANALYSIS IS ONE OF THE MOST IMPORTANT THINGS YOU WILL LEARN THIS YEAR. IT WILL NOT GO AWAY SO MAKE SURE YOU LEARN IT NOW. Example 1:  How many ______________ are in a week? minutes week xp  f 4,0 s 10,080minutes How many ____________ work week? 40 seconds are in an exactly ____-hour 40hr x 941in 94 144,000seconds Example 2: Perform the following conversions: • 125 cm into m. • 4.5 kL into L. 4 SKL 1,0 • 2 kg into mg. 2kg 19 • 450000 cm into km. 450,000 cmxtoomamx.jo 125cm him 1 1025m 4,5001 4 109 9 2,000,000mg n 4 5km Example 3: 22 An atom of gold has a mass of ______________________ g. How many atoms of gold are in 3 271 10 ____________ grams of gold? 5 00 5000g 3.2 1 1053 10 atoms 22 Example 4: Convert the following:  15 cm3 into liters.  7.38 g into kilograms.  6.7 s into milliseconds. 6 7s  94.5 g into centigrams 15cm If m 0.0152 0.00738kg 7038g 10,03ms 94.5g 1,0 9 6,700ms 9,450cg Example 5: • Convert 14.8 g of Boron into cm3. The density of boron is 2.34 g/cm3. 14.8gBx245 • Convert 4.62 g of mercury to cm3. The density of mercury is 13.5 g/cm3. 4 62g • 6.32cm gxiz.gg 0.34cm What is the mass of a sample of cough syrup that has a volume of 50.0 cm3? The density of the cough syrup is 0.950 g/cm3. 50.0cm 0 9g 47.5g Section 4- Physical Properties and Changes: Reminder- Matter is anything that has _________ and ________________________________. Mass Occupies Space Volume States of Matter:  Solids: o _____________________ Volume Fixed  o _____________________ Shape Fixed Liquids: o _____________________ Volume Fixed  o _____________________ Shape Variable Gases: o _____________________ Volume Variable o _____________________ Shape Variable Fixed doesnot change based on the container Variable changes based on container the Qualitative and Quantitative Properties:   Qualitative properties o Properties that are described using ________________________. words o Qualitative properties are evaluated using our __________________________. five senses Quantitative Properties o Properties that are described using a __________________________. measurement number o There are two main types of quantitative properties:  Extensive Properties:  Properties that are ________________ on the ________________ amount dependent ________________________________. substance of the  Examples: Mass Volume Entropy Energy Enthalpy  Intensive Properties:  Properties that are ________________ on the ________________ amount independent ________________________________. of the substance  Examples: Density Temperature P fifty Physical Properties and Physical Changes:      Physical Properties- characteristics of a substance that can change without the substance becoming a ______________________________________. different substance Physical Changes- A change in one of more ____________________________ but no physicalproperties change in the ___________________________________ that make up the substance. fundamental components In a physical change, the _______________________ chemical composition of the substance does not change. Changes in _________________________ are always physical changes. state of matter When a substance changes phase, the potential energy of the substance (the energy stored in the bonds) either increases or decreases depending on the change. Phase Changes: EYES Vaporization condensation Phase Diagrams:  A phase diagram is a graph of _________________ versus ____________________ that temperature pressure shows which phase a substance exists under different ___________________. conditions  There are lines in a phase diagram that indicate where a substance undergoes a ______________________________. phase change  The point where all three lines intersect is called the ______________________ point where a substance exists as _______________________________________________. all three states in eqtiffr.am  At the end of the _____________________ phase line the point is called the liquid gas ____________________ point. At this point, it is difficult to distinguish between the two critild phases and the substance is called a ____________________________ fluid. super critical solid phase If signifier i g liquid Friple point solid g Ph Gas Phase Temperature script the is Diagonal Lines show that the temperature changing so kinetic of the absorbed released changes the energy energy molecule and the molecules vibrate faster or slower Heating and Cooling Curves:  For individual substances, we can also create another type of phase diagram called a ________________ or ___________________ curve. cooling heating These curves show the ____________________ of a substance with respect to _______. time  temperature Horizontal Lines show that the substance is undergoing a phase change the absorbed released energy changes the potential energy stored so Example: Heating Curve in the bonds between the moderates that hold the molecules  For each segment of the heating curve below, answer the following questions: together o What state of matter or phase change is described in this segment? o What kind of energy is changing? o Is the energy change an increase or decrease? E D C B A Segment A Thesubstance is in solidform Thetemperature is increasing kineticenergy of the are moving faster substance is increasing so the andthe molecules B The substance is melting Thetemperatureremainsconstant but the moliates are absorbing energy The potential energy stored Segment between themolecules is increasing used to meltthe substanie iii segments the molecules move faster as theenergy absorbed is t.it I iig D The substance is evaporating The temperatureremains constant but themolecules absorb energy Thisabsorbed energy is used to change Segment the potential energy stored in the substance segmente i ii ii g j and the particles move faster the.si energy i Cooling Curve Example:  For each segment of the heating curve below, answer the following questions: o What state of matter or phase change is described in this segment? o What kind of energy is changing? o Is the energy change an increase or decrease? A B D t segmenta B Segment gg a liquid The energy IE the and is converting from a gas The temperature is constant so kineti energy is constant the bonds is converted into potential energy stored in Thesubstance is undergoing to ii s energy condensation as a liquid the molekles to bind them together The temperature is decreasing so the molecules The substance is a between Segment liquid slow down and the kinett energy decreases D The substanie is undergoing freezing Segment Thetemperature is constant so the the bonds that hold is ionverted into potential energy stored in energy the mole lull together as a solid The substanie is a solid and tooling down The temperature is decreasing Segment the kinetil energy so the moletules are slowing down and detreases Section 5- Classifications of Matter: Elements Substances Compounds Matter Homogeneous Mixtures Mixtures Heterogeneous Mixtures Substances:  In live, we tend to use the word “substance” to describe any kind of object. However, in Chemistry, it has a very specific meaning.  Substances are also called _______________________________. pure substances  Substances have a _________________ and ____________________ composition. If uniform unchanging either of those things change, then the substance has become a different substance.  There are two main types of substances: ________________ and _________________. elements compounds Elements:     The ___________ of the substance smallest form of a substance that has the ________________ properties (Oxygen, Hydrogen, Carbon, etc.) Can be __________________ with other elements combined Cannot be _____________________ further into smaller substances broken down Represented with _________________________ from the Periodic Table (O, H, C, etc.) chemilal symbols Compounds: • A substance that contains two or more elements ___________________ combined in a chemically _________________________ (Carbon Dioxide, Water, Glucose, etc.) fixed proportion • Always has same _______________________ • Always contain _______________________ elements different • Cannot be broken down through ______________________________________. • Represented with ___________________________________________ chemilal formulas composition physical changes The Periodic Table:    Elements are arranged based on ________________ and _______________ properties chemical physical Period- ________________________________ on the Periodic Table (____ Total) Groups- ________________________________ on the Periodic Table (____ Total) c.fi Mixtures: • Material of _____________ composition that contains two or more ________________ substances variable • Can be separated into pure substances of either elements and/or compounds with _________________________________ physiial thanges Two classifications of mixtures • • Homogeneous Mixtures- _______ throughout, also called _______________ Solutions Powder Examples: Milk Salt dater Baking • Heterogeneous Mixtures- contains regions of different __________________ Examples: FriedRite Assorted Candies Salad OPIE ater Separation Techniques for Mixtures: • Distillation- separating the components of a liquid mixture by ____________________. vaporization • Filtration- separating the components of a mixture containing a solid and a liquid by using a _________________. filter evaporation paper • Crystallization- separation technique that results in a ___________ forming out of a solid ________________________________. supersaturated solution • Chromatography- separating the components of a mixture passing it through a _____________ where the components move at different _________________. rates medium speeds Section 6- Chemical Properties and Changes: Chemical Properties:    Chemical Properties are properties of a substance that depends on the ______________ chemical _______________ of the substance. composition If the chemical property of the substance changes, that means that the substance has changed. Examples: Reactivity Electronegativity Oxidation State Aridity Enthalpy Flammability Chemical Changes:    Chemical Changes are changes to chemical properties of a substance. Chemical changes change the ___________________________________ of a substance chemilal composition and the substance becomes an ____________________________________________. entirely different substance Chemical changes are also called __________________________________. chemical reactions Components of a Chemical Reaction:   Reactants- The _____________________________ before a reaction (what reacts?) initial substances Products- The _____________________________ during the reaction (what forms?) substances produced Indicators of a Chemical Reaction:     ___________ Change (except for something dissolving) color Formation of a __________ (bubbles) Spheripitate Formation of a ____________________ (solid) Transfer of __________________ (heat is absorbed or released) energy The Law of Conservation of Mass:   Mass is neither __________________________, nor ___________________________ destroyed The total amount of ___________________ must be equal to the total amount of mass __________________. final mass Steps to Solve Conservation of Mass Problems: 1. 2. 3. 4. Identify __________________________ and ______________________________ Products Reactants Write a ________________________________ Reaition Equation Substitute ___________________________________ Given Values Solve for ____________________________________ Unknowns Example 1: Hydrogen and Oxygen react chemically to form water. How much water would form if ________ 408 grams of hydrogen reacted with _______ 3804 grams of oxygen? g 4.8g 38.4g Example 2: Water Oxygen Hydrogen 43.4g Water Water When solid sodium nitrate is heated, it decomposes to give solid sodium nitrite and oxygen gas. If __________ 4503 g of oxygen gas is produced, how much 9005 g of sodium nitrite and ________ sodium nitrate was heated? Sodium Nitrate Sodium Nitrite Oxygen SodiumNitrate 90.5g 45.3g g 135.8g Sodium Nitrate Example 3: Glucose is reacted with oxygen to form carbon dioxide and water. If _________ 5003 g of Glucose is reacted with 2503 ______ g of Oxygen and _____ 35 g of water is produced, how much Carbon Dioxide was produced? CarbonDioxide Water Glucose Oxygen soo 3g Xy 2503g 40.6g carbonDioxide 35g CarbonDioxide Example 4: You combine Sodium Hydroxide and Hydrochloric Acid to create a solution of Sodium Chloride and Water. If you started with ______ 40 g of Sodium Hydroxide 36.46g of Hydrochloric Acid and _____ and get ________ 18.02 g of Water, How much Sodium Chloride was produced? Sodium Hydroxide Hydrochloric 40g 36.46g 18.02g 58.44g Water Sodium Chloride Sodium Chloride Acid g Sodium Chloride