Honors Chemistry Summer Assignment Use the Honors/AP text book, (Chemistry the Central Science) or Prentice Hall Chemistry Text and your prior knowledge to complete the summer packet. Packet will be collected the first day back to school in September. It will count as a grade for the first marking period. Each day late will lose 1 % from the total points. If you are having problems, please email me at cheryl.rehrig@irsd.k12.de.us Unit 1. Introduction: Chemistry, Matter and Measurement 1. The Study of Chemistry Define Chemistry: 2. Three States of Matter (,, ) Properties (identify states of matter) 1. : no fixed volume or shape, conforms to shape of container, compressible. 2. : fixed volume, takes shape of the container (no fixed shape), incompressible. 3. : fixed volume and shape (independent of container), rigid, incompressible. Properties described on the molecular level: (identify state of matter) : Molecules far apart, move at high speeds, collide often. : Molecules closer than gas, move rapidly but can slide over each other. : Molecules packed closely in definite arrangements. 3. Pure Substances vs Mixtures I. : Matter with fixed composition and distinct proportions. (two examples are elements and compounds) a. (only one kind of atom that cannot be decomposed into simpler substances). b. (consist of two or more elements chemically combined). II. : Combination of two or more pure substances physically combined. Each substance retains its own identity and the composition can vary. Two types of Mixtures 1. (do not have uniform composition, properties and appearance, e.g., sand). 2. (uniform throughout, e.g., air). Also known as. 4. Properties of Matter Each substance has a unique set of physical and chemical properties: : property measured without changing the substance (e.g., color, density, odor, melting point, etc.). : property describing how substances react or change to form different substances (e.g., hydrogen burns in oxygen).
2 Chapter 1 5. Physical and Chemical Changes : substance changes physical appearance without altering its identity (e.g., changes of state). : substances transform into chemically different substances (i.e. identity changes, e.g., decomposition of water, explosion of nitrogen triiodide). Classify the following properties as chemical or physical. a. color c. odor e. ductility (drawn into wires) b. flammability c. rusting f. melting of ice 6. Separation of Mixtures (chromatography, distillation, filtration, decantation) Separation techniques exploit differences in properties of the components. : Separate solid from liquid using filter paper. : Boil off one or more components of the mixture and condense the gas to a liquid. : Separate based on ability of the component to attract to a solid : pour off the liquid from a solid that has settled to the bottom of a container. 7. The Scientific Method: Guidelines for the practice of science 1. Make an and collect 2. Look for patterns, try to explain them and develop a (tentative explanation). 3. Perform an (test hypothesis) 4. Form a 5. Develop a (explanation of general principles with considerable evidence of supporting facts) or a (concise statement or equation that summarizes tested hypotheses). Unit 2: Units of Measurement The units most often used for scientific measurement are those of the system. 1. SI Units There are 5 base units (,,,, ) Length and Mass Mass is. SI base unit of length = (1 m = yards). SI base unit of mass = (1 kg = pounds). Give the name and abbreviation of the SI Unit for: Length Mass Time Temperature Amount 2
Introduction: Matter and Measurement 3 Give the name and the abbreviation of the SI or metric prefix for: 10-12 10 6 10-9 10-2 10-3 10 3 10-6 Temperature Scientific studies use and scales. Celsius scale: Water freezes at o C and boils at o C (sea level). Kelvin scale (SI Unit): Water freezes at K and boils at K (sea level). Zero is lowest possible temperature. It is kown as 0 K = o C. 2. Derived SI Units: are combinations of the 7 base units. Example: Density is mass/volume, so units of density are g/ml or g/cm 3. Volume: Units of volume = (units of length) 3 = m 3. 1cm 3 = 1 ml 1. What is the density of a piece of cement which has a mass of 8.76 g and a volume of 3.07 cm 3? 2. Limestone has a density of 2.72 g/cm 3. What is the mass of 981 cm 3 of limestone? 3. Uncertainty in Measurement All measurements have some degree of uncertainty or error associated with them. Precision and Accuracy : how well measured quantities agree with each other. : how well measured quantities agree with the true value. 4. Significant Figures In a measurement it is useful to indicate the exactness of the measurement. This exactness is reflected in the number of significant figures. Examples; 1.03 x 10 4 g has 3 significant figures. 0.013 has 2 significant figures 1.030 x 10 4 g has 4 significant figures. 0.0130 has 3 significant figures 1.0300 x 10 4 g has 5 significant figures. 1. How many significant digits are there in each of the following? a. 903.2 b. 0.0090 c. 0.0088 d. 0.0490 e. 70 f. 0.02 2. List the number of significant digits for each of the following: a. 1 x 10 8, b. 6.8 x 10 8 c. 4.90 00 x 10 9 d. 8.420 000 0 x 10 8 3
4 Chapter 1 5. Significant Figures in Calculations Multiplication and Division: Report to the least number of significant figures (e.g., 6.221 cm x 5.2 cm = 32 cm 2 ). Addition and Subtraction: Report to the least number of decimal places (e.g., 20.4 g 1.322 g = 19.1 g). In multiple step calculations always retain an extra significant figure until the end to prevent rounding errors. Perform the following calculations and give the answer with the correct number of significant figures. a. 30.84 + 9.74486 e. (7.601x10 7 ) x (8.9x10-4 ) b. 40.79-1.18432 f. 1.45 x 10-6 + 1.54x10-6 c. 1.43 x 0.84 f. 2.21 x 10-12 1.54x10-6 6. Scientific Notation Scientific notation is a more convienent way to express very large or very small numbers. Numbers in scientific notation are written as the product of 2 numbers: a number less than 10 multiplied by 10 raised to some power (exponent). A number greater than 1 will have a positive exponent. A number less than 1 will have a negative exponent. 76000000 is written as 7.6 x 10 7. 0.0000012 is written as 1.2 x 10-6 Express in correct scientific notation: a. 36.8 b. 0.0387 c. 0.0002165 d. 51300 e. 635.1 X 10 23 f. 635.1 X 10-26 g. 0.0023 X 10 23 h. 0.0056 X 10-6 7. Dimensional Analysis Given units can be multiplied and divided to give the desired units. Conversion factors are used to manipulate units: Desired unit = given unit x (conversion factor). The conversion factors are simple ratios: Conversion factor = (desired unit) / (given unit). Conversions: Convert 15miles to kilometers. (1.6 kilometers = 1 mile) Convert 12 gallons to liters. (0.26 gallons = 1 liter) Convert 35 Celsius to Kelvin. K = o C + 273 Convert 950 K to Celsius: o C = K 273 Convert 127 liters to moles (22.4 liter = 1 mole) 4
Introduction: Matter and Measurement 5 Unit 3: Atoms, Molecules, and Ions 1. are the building blocks of matter. Subatomic particles: those particles that make up the atom are: 2. Isotopes, Atomic Numbers, and Mass Numbers All atoms of a specific element have the same number of protons. of a specific element differ in the number of neutrons (and mass). (Z) = number of protons in the nucleus. (A) = total number of nucleons (i.e. protons and neutrons) in the nucleus Complete the following table Element Atomic Number Protons Neutrons Electrons Mass 1. Li 2. 25 30 3. 20 20 The Periodic Table is used to organize the elements in a meaningful way. As a consequence of this organization, there are periodic properties associated with the periodic table. Columns in the periodic table are called. There are groups in the periodic table Rows in the periodic table are called. Some of the groups in the periodic table are given special names.these names indicate the similarities between group members. Examples: (names for these groups) Group 1A: Group 2A Group 7A Group 8A: 1. Metals, Non-metals, Metalloids elements are located on the left-hand side of the periodic elements are located in the top right-hand side of the periodic table. Elements with properties similar to both metals and nonmetals are called and are located at the interface between the metals and nonmetals. 5
6 Chapter 1 Compounds (ionic and covalent) Given the following formulas, name the covalent compounds. SiF 4 CS 2 P 3 Br 7 Write the formulas of these covalent compounds, given the names. diboron hexahydride octanitrogen tribromide sulfur hexachloride Write the formula for the following ionic compounds, given the names: Aluminum chloride ammonium sulfite Potassium sulfide Calcium phosphate Name the following ionic compounds, given the formulas: CaF 2 Al 2 O 3 Na 3 PO 4 MgO Polyatomic Ion Names -1 NO 3 nitrate -2 SO 3-1 NO 2 nitrite -2 SO 2-3 sulfate PO 4 sulfite phosphate Chemical Equations Balance the following equations and identify the type of reaction combination (synthesis), decomposition, combustion, single replacement, double replacement 1. Pb(NO 3 ) 2 (aq) + NaI (aq) PbI 2 (s) + NaNO 3 2. CaCO 3 (s) CaO (s) + CO 2 (g) 3. P 4 + O 2 P 4 O 10 4. CH 4 + O 2 (g) CO 2 (g) H 2 O 5. AlPO 3 + Ca Ca 3 (PO 3 ) 2 + Al 6. H 2 + O 2 H 2 O 6