STUDY GUIDE CP Chemistry FINAL EXAM

Transcription

1 NAME PERIOD STUDY GUIDE CP Chemistry FINAL EXAM Format: 75 multiple choice (1 pts each) 1 open response stoichiometry problem (5 pts) 1 open response ACID-BASE problem OR molarity problem (5 pts) 1 open response gas law problem (5 pts) 2 open response SHORT ANSWER (5 pts each) OPEN RESPONSE SHORT ANSWER: * You will CHOOSE 2 to answer * 1) The table below shows the ph values of some substances used in the chemical industry. a. Classify each of the five substances as acidic, basic, or neutral. b. List the five substances in order of increasing hydrogen ion concentration. c. Describe what would happen to the ph of the CH 3OOH if the concentration was increased from 0.1 M to 1.0 M. EXPLAIN your reasoning. 2) The elements helium, neon, and xenon are located in Group 18 (8A) in the periodic table. a. Explain why the atomic number increases from helium to neon to xenon. b. Explain why helium, xenon, and neon are located in different periods in the periodic table. c. Describe the chemical reactivity of helium, neon, and xenon and EXPLAIN how the location of these elements in the periodic table relates to their chemical reactivity. 3) Large helium-filled balloons are used to carry instruments to altitudes high above Earth s surface. These balloons are used to collect data related to Earth s atmosphere. a. As the balloons rise to higher altitudes, the atmospheric pressure decreases. Describe changes in the balloons volumes resulting from the decrease in atmospheric pressure. b. Temperature also varies with altitude. Describe how a decrease in temperature will tend to affect the volumes of the balloons. c. A balloon may eventually reach an elevation where the density of the atmosphere is equal to the density of the balloon and the balloon will not rise any higher. Based on your responses to parts (a) and (b), how could the maximum altitude of a helium balloon be increased? You may explain in words, or draw and label a diagram.

2 Lab Safety and Equipment / Metrics & Measurement Identify the EIGHT (8) pieces of common laboratory equipment we learned in class. Convert between units of measure within the metric system (i.e. cm to m, km to mm, etc.) Explain the difference between precision and accuracy Calculate percent error. Explain what data represents the expected and experimental values. Identify # of significant figures in a given number Write a number in scientific notation Properties of Matter Classify matter according to properties (HINT: Use concepts from flowchart for physical/chemical, mixtures, homogenous/heterogeneous mixtures, substances, atoms, compounds, etc.). Provide examples for each type of classification. Describe colloid, solution, and alloy. Identify physical properties (i.e. melting point, boiling point, ductility, density, luster, solubility, hardness, color, odor, malleability, viscosity) Identify chemical properties (i.e. flammability, corrosiveness, reactivity, rust, ph,) Identify physical and chemical changes and explain differences between them Density Define and identify the correct units for mass, volume, and density Explain how to measure the mass and volume for blocks, cylinders, and irregularly-shaped objects Calculate volume of blocks, cylinders, and irregularly-shaped objects Identify the formula and variables for density, including correct units Use the formula for density (density = mass/volume) to solve for density, mass, or volume from word problems Atoms and the Periodic Table Define and identify elements and compounds Define and identify atoms, ions, and isotopes Define and determine the atomic mass, atomic number, mass number, # protons, # neutrons, and # electrons for a given element Define and explain the characteristics of protons, electrons, and neutrons Explain the basics of atomic theory (Bohr model, etc.) Define properties: malleable, ductile, conductor Classify elements based on location on periodic table, explain the characteristics of each (metals, metalloids, non-metals, alkali metals, alkaline earth metals, halogens, noble gases, transition metals, inner transition metals (rare earth metals) Define atomic radius, ionization energy, electron affinity, electronegativity Compare groups of elements and classify (high/low or small/big) according to trends for atomic radius, ionization energy, electron affinity, electronegativity Chemical Bonding Explain the octet rule Define valence electrons and identify # of valence electrons for representative elements using the periodic table Define anions and cations and explain how they get their charges Explain which types of elements tend to form ionic bonds and the characteristics of ionic compounds Explain which types of elements tend to form covalent bonds and the characteristics of molecular compounds Explain the characteristics of substances with metallic bonds Draw Lewis Dot structures for elements, ionic compounds, and molecular compounds

3 Nomenclature and Chemical Formulas Predict ionic charge for monoatomic ions using periodic table Identify monatomic and polyatomic ions (using list of 10 common polyatomic ions) Name ionic compounds from a given chemical formula Use criss-cross method to write chemical formula for ionic compounds from a given chemical name Explain how charges on ions cancel out to form a neutral ionic compounds, and why Name binary molecular compounds from a given formula (HINT: use prefixes correctly, following all rules) Write chemical formula for binary molecular compounds from a given compound name Chemical Quantities Define mole and Avogadro s number Determine/calculate molar mass for elements and compounds Identify conversion units for Avogadro s number and the mole Identify conversion units for molar mass and the mole Convert single-step dimensional analysis between particles and moles, and between moles and mass Convert double-step dimensional analysis using the MOLE MAP Chemical Reactions Identify 6 types of chemical reactions and describe what happens in each o Single replacement o Double replacement o Combustion o Synthesis o Decomposition o Acid-Base Identify oxidation and reduction for partial reaction equations (oxidation-reduction reactions) Compare and contrast oxidation and reduction Identify the parts of a chemical reaction (reactants, products, ALL of the symbols, etc.) Balance chemical equations Explain the process of corrosion and what can be done for preventative measures Identify mole ratios from a chemical equation (for TWO substances) Use stoichiometry to solve for unknown quantity of substance B (given substance A) Solutions and Acids & Bases Define aqueous solutions, solutions, solute, and solvent Identify/describe real-life examples of solutions Define molarity Determine concentration using molarity formula Use molarity formula to solve for molarity (M), volume of solution (L), or moles of solute Define solubility Compare/contrast saturated, unsaturated, and supersaturated solutions Determine solubility, unsaturated/saturated/supersaturated for substances using solubility curve (graph) data Compare and contrast properties of acids and bases What range of ph values do acids have? What range of ph values do bases have? What ph is neutral?

4 What does ph stand for (what does it mean)? Calculate ph and poh (from given molarity/concentration of H 3O + and/or OH - ) Calculate molarity (M, concentration) of H 3O + and/or OH - from given ph or poh Solve for Molarity or Volume of acids/bases in a titration experiment using the formula MaVa = MbVb Identify the components and procedure for a basic neutralization reaction (titration experiment setup) The Gas Laws Define temperature and pressure Identify the units for temperature and pressure Be able to convert between units of temperature Be able to convert between units of pressure Explain how a barometer works Compare/contrast properties of solids, liquids, and gases Describe ALL the properties of gasses Explain the effect of temperature on particle movement in solids, liquids, gases Describe how volume affects temperature and pressure of gasses Describe how temperature affects volume and pressure of gasses Describe how pressure affects temperature and volume of gasses Define STP For each of the following gas laws ~ BOYLE S, CHARLES, and COMBINED: Be able to explain it and answer multiple choice questions! Be able to identify real-life examples/examples from class & lab Be able to identify the formula Be able to use the formula to calculate for the unknown MISC. Practice Problems: 1) Classify the following as chemical or physical change: a) Iron rusting b) Ice melting c) Evaporation d) Acid-base reaction 2) Try these conversions: a) 5000mg = g b) 2 L = ml 3) Find the density of an unknown solid given that a 5.6 sample has a volume of 2.35 cm 3 4) What is the difference between a cation and an anion?

5 5) What is the charge for these ions? a) Li b) Cl c) Ba d) Na e) O 6) Name the following: a) KCl b) MgO 7) Calculate the molar masses of each substance below. a) SrCl 2 b) OF 2 c) Co(NO 3 ) 2 8) How many moles are in 72.9 g of HCl? 9) How many grams are in 3.5 mol of NaOH? 10) Element or compound? a) NaF b) Cl 2 c) Al d) He e) NH 3

6 11) WORD BANK: Proton atom mass number atomic mass electron mole atomic number neutron electron isotopes a) the total number of protons and neutrons in the nucleus of an atom b) the average mass of the atoms in a naturally occurring sample of an element c) the number of protons in the nucleus of an element d) atoms with the same number of protons but different number of neutrons e) negatively charged subatomic particle f) the smallest particle of an element that retains the properties of that element g) a counting unit; 6.02 x h) subatomic particle with no charge 12) Try these conversions: c) 5000mg = g d) 2 L = ml 13) When the equation P + O > P 2 O 5 is correctly balanced, the coefficient before O2 is (circle one:) 5/2/1/3 14) How does the particle movement and orientation change when a substance changes from solid, to liquid, to gas? What happens when you increase the temperature of a gas? 15) Define the following terms: SATURATED SOLUTION, SUPERSATURATED SOLUTION, UNSATURATED SOLUTION 16) A sample of hydrogen at 1.5 atm had its pressure decreased to 0.5 atm, producing a new volume of 750 ml. What was its original volume? Which gas law is this?

7 17) A sample of nitrogen occupies a volume of 250 ml at 25 C. What volume will it occupy at 95 C? Which gas law is this? STOICHIOMETRY Practice Problems: 1) Using the following equation: Fe 2 O H > 2 Fe + 3 H 2 O Calculate how many grams of iron can be made from 16.5 grams of Fe 2 O 3 2) Using the following equation: 2 I 2 + KIO 3 + 6HCl > 5ICl + KCl + 3H 2 O Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction 3) Using the following equation: 4 NH O > 4 NO + 6 H 2 O How many grams of oxygen (O 2 ) are needed to react with 56.8 grams of ammonia by this reaction?

8 4) Using the following equation: NaIO HI > 3 I 2 + NaI + 3 H 2 O Calculate the number of grams of iodine (I 2 ) that can be made this way from 16.4 grams of NaIO 3. ACID-BASE Practice Problems: 1) Find the ph of a solution whose [H 3 O + ] is: a M b x 10-7 M c x 10-3 M d. Classify each of the above solutions as acidic or basic. 2) Find the poh of a solution whose [OH - ] is: a x 10-2 M b x M c x ) Find the [H 3 O + ] in solutions of the following ph: a. ph = 2.00 b. ph = 13.0 c. ph = 4.60 d. ph = 7.00 MOLARITY Practice Problems: 1. What is the molarity of a solution that contains 1.7 moles of H 2 SO 4 in 3 L of solution? 2. What is the molarity of a solution prepared by dissolving 25g of HCl (g) to make a final volume of solution of 150mL? 3. What is the volume of solution needed to make a 0.1M HCl solution with 0.02 moles of solute?