Name Teacher Period Academic Chemistry 2016 Fall Final Exam Review DUE THE DAY YOU TAKE THE FINAL FOR 5 BONUS POINTS on the final exam Unit 1 Matter and Change 1. Complete the chart. Definite shape? (y/n) Definite volume? (y/n) Effect of Pressure? Density (high/med/low) Solid Liquid Gas 2. What is a physical property? 3. What is a chemical property? 4. Write (I) for intensive and (E) for extensive property: mass density melting point length conductivity color texture ductility luster volume 5. What is a physical change? 6. What is a chemical change? 7. List the 4 indicators that a chemical change has occurred 8. Classify the following as physical (P) or chemical (C) changes: food spoils candle melts salt dissolves in water burning coal 9. What is the law of conservation of matter (or mass)? 10. According to the law of conservation of matter, if 22.99 grams of sodium are added to 35.45 grams of chlorine, how much sodium chloride should be produced? 11. Calculate the density of a substance with a mass of 6.25 g that occupies a volume of 5.2 ml. 12. Gold has a density of 19.3 g/ml. Calculate the mass of a piece of gold that occupies 7 ml.
13. Classify each substance as element, compound, or mixture. zinc river water soda salt oxygen sugar copper kool-aid water 14. Classify each mixture as homogeneous or heterogeneous. Sugar water iced tea soil M&M s oreo cookie Gatorade Unit 2 Safety and Scientific Measurement 1. What is the proper attire for lab activities (5 things)? 2. If an accident or spill occurs, you should always. 3. What is the proper procedure when heating materials in lab (3 things)? 4. To dispose of all chemicals you should 5. How many significant figures are in the following numbers? a. 0.00890 b. 3056.0 c. 875,000 d. 10.0320 e. 2050 f. 875.00 6. Complete these problems using correct sig figs in answer. a. 10.18 m x 0.00740 m = b. 302,000 mm x 3.5 mm = c. 27.54 s - 3.8 s = d. 765 g + 37.2 g = g. 3.2 m 3.563 s =
7. Accuracy is 8. Precision is 9. Three different students measured a 26.30cm length of twine three times each. Indicate if the student was accurate, precise, BOTH, or NEITHER! Trial 1 Trial 2 Trial 3 Accurate, Precise, Both, Neither Rachel 26.32 cm 26.29 cm 26.31 cm Chloe 38.12 cm 28.13 cm 26.32 cm Roel 36.39 cm 36.40 cm 36.40 cm Unit #3 Atomic Structure 1. What is an Atom?. John Dalton 2. All matter is made up of particles called. 3. Atoms of one element are the. Atoms of different elements are. Ernest Rutherford 4. Discovered the nucleus in the gold foil experiment. Most alpha particles passed through unaffected => concluded the atom is mostly space. Few particles deflected greatly =>concluded that at the center of the atom was a small, nucleus with a charge. J.J. Thomson 5. Discovered the in his investigations with a Crookes tube. Found ALL substances contained these charged particles. Stated the atom must be a clump of charged material with negatively charged particles dispersed throughout. Niels Bohr 6. Developed the model of the atom based on how he theorized moved around the nucleus. 7. Define atomic number mass number average atomic mass isotope
8. The nucleus of an atom is composed of and. 9. Isotopes have the same number of, but different numbers of. 10. Are the following groups of atoms isotopes? (YES or NO) a. b. 8 protons and 9 neutrons 8 protons and 8 neutrons 5 protons and 6 neutrons 6 protons and 6 neutrons 80 81 83 38 38 38Sr c. Sr Sr d. Si 15 and P 15 e. 25 p + and 30 n 0 25 p + and 33 n 0 11. Most of the mass of an atom is in the because protons and neutrons have a much ( LARGER / SMALLER ) mass than electrons. 12. Why are atoms neutral (no charge)? 13. Nitrogen has two naturally occurring isotopes, nitrogen-14 and nitrogen-15. The atomic mass of nitrogen is 14.007 amu. Which isotope is more abundant in nature? 14. What is the charge on a proton, a neutron, and an electron? 15. What is the mass, in amu, of a proton, a neutron, and an electron? 16. What does the number 60 in cobalt-60 mean? 17. Complete the following table. Symbol Atomic # # of protons # of neutrons # of electrons Mass # 23 11Na 8 8 47 60 7 14 18. Calculate the atomic mass of the following element with the given isotope information: amu 107 109 47Ag= 52.34% 47Ag= 47.66% 19. Write the shorthand notation for a particle which has 9 neutrons and 10 protons. 20. Write the shorthand notation for a particle with a mass # of 88 and 38 protons. 21. Lead 206 has neutrons. 226 22. How many particles are in the nucleus of this radium atom? 88Ra 23. An alpha particle is the same as the nucleus of a atom. It has a charge.
24. A beta particle is a high-speed and has a charge. It is the product of a becoming a. 25. Balance the following nuclear reactions: 22 15 a. P e + 1 0 4 2 206 82 b. He + Pb 119 50 c. e + Sn 239 94 4 2 1 0 d. Pu He + 26. For the following decay prompts, write the complete nuclear reaction. a. Bohrium-272 decays by alpha emission b. The decay of rhodium 109 by beta emission 27. Complete the chart: Type of Radiation Shorthand Notation Material needed to stop/shield radiation How far does radiation penetrate a person? Beta Alpha Gamma Unit #4 Waves and Electrons 1. What is the frequency of a wave if its wavelength is 5.25 x 10-15 m? 2. What is the energy of light having a frequency of 5.00 x 10 12 Hz? 3. What is the energy of a wave if its wavelength is 7.70 x 10 16 m? 4. What is the difference between an excited and a ground state electron? 5. Valence Electrons - Electrons in the energy level of Atom. This is where electrons can be gained or Lost 6. A(n) has a high probability (90%) of containing an electron. 5
7. What element has the identifying square 4p 3? 8. The atomic number for an element with an electron configuration of 1s 2 2s 2 2p 6 3s 2 is? 9. Write the complete electron configuration for the following elements. a. sodium b. silver c. krypton 10. Write the noble gas configuration for a. manganese b. bromine 11. Write the orbital notation for Mo (Molybdenum). 12. Complete the chart about sublevels and their orbitals. s p d f Shape # of orbitals Maximum # of e- Unit #5 Periodic Table Major Categories of Elements 1. Groups on the periodic table are ( VERTICAL COLUMNS / HORIZONTAL ROWS ). 2. Elements in a GROUP have SIMILAR chemical and physical. This is because they have the same number of. 3. List all Elements with Similar in physical and Chemical Characteristics as Calcium: 4. PERIODS on the periodic table are ( VERTICAL COLUMNS / HORIZONTAL ROWS ). Elements in a period have the same number of. Elements in a period have property similarity. 5. Metals are on the side of the periodic table (except ). Nonmetals are on the side of the periodic table. Metalloids are found along the line (except ). 6. Write the symbols for all of the metalloids: Classifying Elements 7. Octet Rule - Atoms want in their Outer Energy Level 6
8. Groups 3 12 are called. 9. Complete the following chart Name Of Group Valence Electrons Gain or Lose Electrons Oxidation # Periodic Trends 1 2 13 14 15 16 17 18 NA NA NA NA 10. Draw and label arrows in the periodic tables that represent the 4 trends discussed in class. You must write the name of the trend in the box below the periodic table. Element Identification a. The smallest noble gas atom. Trend Application b. 3 valence electrons in Period 4. c. The element in period 2 with 7 valence e-. d. Halogen in Period 5. e. The most reactive alkali metal. 1. Which of the following is most electronegative? Li, B, N, or Ne 2. Which of the following is most reactive? Rb, Y, Nb, or Ag f. Alkaline earth metal in Period 6. g. Metalloid in Period 2. h. Nonmetal in Group 14. i. Element in period 3 that forms a +2 ion. j. Element in period 5 that forms a 1 ion. 3. Which of the following is least reactive? O, S, Se, or Po 4. Which of the following has the largest atomic radius? Li, B, Ne, or F 5. Which of the following has the greatest ionization energy? C, Si, Ge or Pb 7
Unit #6 Naming 1. Nonmetals either have,, or valence electrons, ( GAIN / LOSE ) electrons to form ( + / ) charged ions called ( CATIONS / ANIONS ). 2. Metals either have,, or valence electrons, ( GAIN / LOSE ) electrons to form ( + / ) charged ions called ( CATIONS / ANIONS ). 3. What is the Octet Rule? 4. List the 10 prefixes used for naming covalent compounds: 1 2 3 4 5 6 7 8 9 10 5. Complete the chart. Chemical Formula Covalent (C), Ionic (I), Polyatomic ionic (IP), Ionic with Transition Metal (IT), Ionic w/ Polyatomic and Transition Metal (IPT), Binary Acid (Ab) Ternary Acid (At) Chemical Name NaNO3 SiI4 N2O3 Li3N AlPO4 NiF2 H3PO4 BaS NH4Br HCl 8
FeSO4 P2O5 CoCl3 10. Complete the chart. Chemical Name dichlorine heptoxide Covalent (C), Ionic (I), Polyatomic ionic (IP), Ionic with Transition Metal (IT), Ionic w/ Polyatomic and Transition Metal (IPT), Binary Acid (Ab) Ternary Acid (At) Chemical Formula iron (II) cyanide calcium nitride gold (I) sulfide trisilicon tetranitride phosphorous acid sulfur hexachloride magnesium phosphoride sodium oxide barium acetate tetraphosphorus decoxide calcium hydroxide nitric acid 9
Unit #7 Moles 1. What is a mole? 2. What is molar mass? 3. What are the 3 types of representative particles? Use the conversion guide: MASS (g) MOLES PARTICLES 1 mol molar mass(g) 6.02 x 10 23 particles 1 mole 4. Calculate the molar mass of Ca3(PO4)2. 5. How many moles are in 3.54 grams H2S? 6. How many grams are in 1.97 moles of carbon dioxide? 7. How many atoms are in 700 g of lithium? 8. How many molecules are in 0.42 moles of C3H8? 10