2 nd Semester Final Review

1. 2nd Semester Final Review 5 days to review and create a study book Final Exam on May 12th & 13th *the info in this review does not cover everything on the final – but it’s a good starting place

2. Instructions: • Take 5 pieces of BIG paper and fold in half to make a booklet. Staple along the fold to hold them together. • Write some sort or a title on the front page (you may need room to add notes here as well). Don’t forget your name and period#. • Each day you will be given a topic and some review questions to work on. The slides will be up for 5-10 minutes before moving on to the next one. Use you time wisely so you do not miss out on any review. • You may write whatever you want in the review booklet.

3. Day 1 #1 FUNDAMENTALS OF CHEMISTRY: MATTER AND CHANGE • Define chemistry. • Which of the following observations is evidence used to imply that a chemical reaction has occurred? a. gas evolution b. a precipitate forms c. the color changes d. temperature changes e. the odor changes f. sound is produced g. change in taste • Describe a physical property vs. a chemical property. • What is the difference between a physical change and a chemical change? • Identify each type of change (physical or chemical). a. boiling water b. rusting iron c. burning candles d. breaking glass e. melting wax • Be able to classify matter: mixtures (homogeneous, heterogeneous) vs. pure substances (compounds or elements) • Identify each as an element, compound or mixture. a. lead b. water c. kool-aid d. table salt e. soda f. oxygen • What are the characteristic of a metal, metalloid and non-metal? Identify each type of element: a. Zn b. As c. S d. Ne e. Na

4. Day 1 #2 MEASUREMENTS AND CALCULATIONS • Discuss the steps in the scientific method. • What are the rules/guidelines of determining significant figures? • How many significant figures in: a. 1234 b. 123.0 c. 123400 d. 0.001234 e. 0.01230 • Report the above problems (a-e) in correct scientific notation. • What are the common SI Units? Know the prefixes from milli to kilo and be able to convert between units in the metric system. • What is the difference between mass and weight? • Multiply: 5.98 mm x 3.2 mm = ? • Add 3.258 cm + 12.0 cm = ? • Give an example of a qualitative observation • Give an example of a quantitative observation. • What is the difference between accuracy and precision? • How many grams of mercury would you have if you had 32 cm3 of mercury? The density of mercury is 13.6 g/cm3. • Ronnie has a piece of aluminum which has a mass of 10.8 grams and a volume of 4 cubic centimeters. Calculate the density of aluminum.

5. Day 1 #3 ATOMIC THEORY AND NUCLEAR CHEMISTRY • Describe Dalton’s Atomic Theory. • What did we learn from Rutherford’s Gold Foil Experiment and how did it work? • What did J. J. Thomson discover with his Cathode Ray experiment? • Define the atomic number, mass number, average atomic mass and isotopes. • Explain the difference between atoms, ions, cations, anions. • Know the charge, location and size of the three subatomic particles. • An element has 30 protons, 35 neutrons, and 30 electrons. What element is this? • An ion of an element has 29 protons, 35 neutrons, and 27 electrons. What ion is this? Write its symbol with the correct charge. • State the Law of Conservation of Mass (Matter). • Most of the volume of the atom is taken up by the electron cloud. True or False? • How many particles are there in 1 mole of anything? What is the name for this number of particles? • What is the molar mass of sodium? What is the molar mass of Na2SO4? • Indicate the number of molecules, and the total number of each type of atom for each of the following: 4H2O 2Al2(SO4)3 • Be able to convert: Grams to Moles or Moles to Grams and Grams to Atoms or Atoms to Grams • How many moles are in 222 g of copper? • How many atoms are in 4.00 g of sulfur? • What is Avogadro’s number? What is the significance of it? • Be able to balance simple nuclear equations. • What is radioactive decay? Half-life? (no equations) • Describe the process of nuclear fission and nuclear fusion? • What are the penetrating strength differences between alpha particles, beta particles and gamma rays?

6. Day 2 #1 ELECTRON CONFIGURATIONS • What is the frequency of an electromagnetic wave traveling at the speed of light with a wavelength of 6.80 x 10-7 m? • All types of electromagnetic radiation have the same _________. • Identify the parts of an electromagnetic wave on a diagram (i.e. wavelength, amplitude, etc.). • What is a quantum of electromagnetic energy called? • Write the full electron configuration for: C, As, and S2- • How many outer electrons does each of the following have? Na As Br O2- K+ • How many electrons must each of the following lose or gain to achieve an octet? (State whether it loses or gains and how many) ClCaXe P • Which element has similar chemical properties like Si? Why? At Al N C • When electrons absorb energy, what is the result? • What color of light has the most energy? • What is the probability map for an electron called? • What occurs when an electron moves from a higher energy level to a lower energy level in an atom? • The indicates the main energy level occupied by the electrons (n). • How many electrons can occupy an s orbital, p orbital, d and f orbitals? • Which atom would have an octet of electrons (full s and p orbitals): Fe, Ar, O or He

7. Day 2 #2 PERIODIC TABLE • Who is Dmitri Mendeleev? • What charge do all elements in the following columns form when they are ions? 1, 2, 13, 15, 17, 18 • What is the chemical family name for column: 1, 2, 17 and 18? • What are the following groups most characteristic properties? 1, 2, 17, 18 • Write the complete electron structure for a neutral sodium atom. According to its electron structure, what period of the periodic table should sodium be in? How many valence electrons does it have? What ion will sodium tend to form? • What is meant by a noble gas electron configuration? Why are they more stable? • Define:electronegativity, ionization energy, electron affinity • Describe the trends (across a period, down a group) in the periodic table for: Atomic radius, Ionization energy, Electronegativity • State the periodic law.

8. Day 2 #3 CHEMICAL BONDING • What is a chemical bond? • What are valence electrons and why are they important? • State the octet rule. • What is the difference between ionic, covalent and metallic bonding? • What type of bond (ionic or covalent) will form in the following compounds? How do you know? CO2NaCl F2 • Using an electronegativity chart identify each type of bonding (ionic, polar covalent, nonpolar covalent): Cs – Cl H – O Br – ICl– Cl • List the seven diatomic molecules. • What is a polar molecule? • What is VSEPR theory? • Use VSEPR theory to predict the molecular geometry of the following (common geometries: linear, trigonal planar, tetrahedral): CO2 CH4 BF3

9. Day 3 #3 NOMENCLATURE AND USING CHEMICAL FORMULAS • Use the following ions and write the correct formula for the compound made from them: a. Na+ and Br- b. Mg2+ and I- c. Ca2+ and NO3-d. Fe3+ and SO42- • Name the above compounds (a-d) and the following: e. KOH f. CuF g. CuSO4 • Which compounds below are ionic? Which are molecular (covalently bonded)?a. N2b. CaF2c. NO2d. CuSO4 e. CCl4 • Given SO42- and the compound Zr2(SO4)3 , what is the charge on Zirconium? • What is the chemical formula for potassium chloride? What is the formula for iron(III) sulfide? • What is the formula for lithium carbonate? • What is the molar mass of an element? What is the molar mass of CuSO4? • What is the percent composition of carbon in carbon dioxide? • Name each of the following acids:a. HClb H2SO4 c. HNO3 d. HI

10. Day 4 #1 Stoichiometry Defining Stoichiometry • Describe the types of relationships indicated by a balanced chemical equation • State the mole ratios from a balanced chemical equation • Explain role of limiting reagent Stoichiometric Calculations (no show work, however need to solve) • Moles to moles Chemical Reactions Writing Chemical Reactions • Writing Chemical Formulas • Balancing • States Classifying Reactions • Synthesis • Decomposition • Single Replacement • Double Replacement • Combustion

11. Day 4 #2 States of Matter Identify Characteristics of the States of Matter Forces of Attraction • Identify the types of intermolecular forces, how they work, which is strongest • Hydrogen bonding • Dispersion forces • Dipole-Dipole • Identify the role of intermolecular force in states of matter Phase Changes • Explain phase/state changes • Explain how the addition and removal of energy can cause a phase change • Interpret a phase diagram Interpret a Temperature-Time Graph (Heating or Cooling Curve of Water) • Recognize phase and temperature • Identify endo- and exothermic processes and constant temperature

12. Day 4 #3 Gases The Gas Laws • State the relationships among pressure, temperature and volume of a constant amount of gas • Apply the gas laws to problems involving the pressure, temperature, and volume of a constant amount of gas • Combined Gas Law (will be given equation on front of final exam) • Boyle’s Law • Charles’s Law • Gay-Lussac’s Law • Ideal Gas Law (will be given equation on front of final exam) • Remember all gas laws in Kelvin (be able to convert temperature from °C) • Relate number of particles and volume using Avogadro’s principle (molar volume)

13. Day 5 #1 Solutions Types of Mixtures • Compare the properties of solutions, suspensions and colloids • Brownian motion • Tyndall effect • Electrolytes versus Nonelectrolytes Factors Affecting Solvation • Understand/define solvation • Factors affecting rate of dissolution • Solubility of liquids and gases • Role of polarity in dissolution • Define/recognize solubility • Unsaturated solutions • Saturated solutions • Supersaturated solutions • Precipitate Concentrations of Solutions • Molarity (know this formula) Colligative Properties • Explain/define • Discuss how colligative properties affects the freezing-point and boiling point of a substance

14. Day 5 #2 Thermodynamics • Energy • Define energy • Understand the First Law of Thermodynamics • Heat • Define • Know the equation for calculating heat • Recognize thermochemical equations • Describe enthalpy Acids and Bases Properties of Acids and Bases • Characteristics of acids and bases • Strong vs. weak acids and bases • Definitions • Arrhenius • Bronsted-Lowry • Lewis • Explain amphoteric • Discuss self-ionization of water • Calculate • pH • pOH • Concentration • Meaning of Kw

15. Day 5 #3 Chemical Kinetics and Equilibrium Energy Diagram • Identify parts of an energy diagram • Recognize if energy diagram represents an exo- or endothermic reaction Reaction Rates • Understand reaction rates • Know the factors that affect rates (temperature, size, concentration, catalyst) Equilibrium • Meaning of equilibrium conditions • Equilibrium constant (Keq) • Define • Know that Keq varies with temperature • Understand magnitude---favors products or reactants • Write an expression • Calculate Keq and/or unknown concentration • Apply Le Chatelier’s Principle – how temperature, pressure, concentration change equilibrium position

16. The End! • Hopefully you worked hard and wrote everything down in your booklet • You WILL be able to use this book on the final! • You’re welcome. • Don’t forget it on Monday – I will not feel sorry for you. • If you slacked – you can still add to it this weekend – the PowerPoint will be posted to the school website today.