Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals, Alkaline Earth metals, Halogens, Noble Gases, Lathanide Series, Actinide Series, Transition Metals, Metalloids Define group- 3. Add in the trends to the periodic table above for electronegativity, ionization energy, atomic and ionic radii. 4. Define and give the reason for each trend: Define period- Electronegativity- Ionization Energy- Atom Size- 5. Label the following groups and periods on the above periodic table. 6. List the location (nucleus or outside shells), mass, and charge of each of the subatomic particles Ionic Radii- Protons- Neutrons- Electrons- 7. The mass of an atom is located in the. 8. The charge in the nucleus is Final Review Page 1
9. The charge of the outside shells is 10. Which historical experiment confirmed what is known about the nucleus? (Choose 1) Rutherford s Gold Foil, Thompson s Cathode Ray Tube, or Millikan s Oil Drop 11. What is the charge on X, and Y in the following chemical formulas? X 3 N, YO 12. Which group on the periodic table would X and Y be found in? 13. Define the following terms: matter, heat, energy, weight, mass, density 14. What types of substances can be decomposed by chemical change? Elements or compounds? 15. Define: Cation and give an example 16. Define Anion and give an example 17. Define Isotopes and give an example 18. Define amu 19. Which element is most chemically similar to chlorine? (1) Ar (3) Fr (2) F (4) S 20. Which two particles each have a mass approximately equal to one atomic mass unit? (1) electron and neutron (2) electron and positron (3) proton and electron (4) proton and neutron 21. What is the total charge of the nucleus of a carbon atom? (1) 6 (3) +6 (2) 0 (4) +12 22. A sample composed only of atoms having the same atomic number is classified as (1) a compound (3) an element (2) a solution (4) an isomer 23. When a metal is heated in a flame, the flame has a distinctive color. This information was eventually extended to the study of the stars because a. The color spectra of the stars indicate which elements are present. b. A red shift in star color indicates stars are moving away c. Star color indicates absolute distance d. It allows the observer to determine the size of stars Final Review Page 2
24. Which of the following ordered pairs of elements shows an increase in atomic number but a decrease in average atomic mass? e. Ag to Pd f. Co to Ni g. Ge to Sn h. Cr to Mo 25. Which of the following atoms has six valence electrons? i. Magnesium (Mg) j. Silicon (Si) k. Sulfur (S) l. Argon (Ar) 26. Which statement best describes the density of an atom s nucleus? m. The nucleus occupies most of the atom s volume but contains little of its mass n. The nucleus occupies very little of the atom s volume and contains little of its mass o. The nucleus occupies most of the atom s volume and contains most of its mass p. The nucleus occupies very little of the atom s volume but contains most of its mass. 27. Why are enormous amounts of energy required to separate a nucleus into its component protons and neutrons even though the protons in the nucleus repel each other? q. The force of the protons repelling each other is small compared to the attraction of the neutrons to each other r. The electrostatic forces acting between other atoms lowers the force of repulsion of the protons s. The interactions between neutrons and electrons neutralize the repulsive forces between the protons t. The forces holding the nucleus together are much stronger than the repulsion between the protons. Chemical Bonds 1. Define 2. Describe the molecular motion of each of the following: Solid- Liquid- Gas- Solid- Liquid- Gas- 3. What prevents substances from changing states of matter? 4. The sharing or exchanging of results in chemical bonds? 5. What types of electrons to Lewis Dot Structures show? 6. Draw Lewis dot structures for the following elements: Na, Mg, Al, Si, P, S, Cl, Ar Final Review Page 3
7. Draw Lewis Dot Structures for the following molecules: NH 3, N 2, H 2 O, CO 2, O 2, C 2 H 2 8. What do the pairs of dots in the above diagrams of molecules represent? 9. When metals become ions do they gain or lose electrons? 10. When metals become ions what kind of charge do they have? 11. When non-metals become ions do they gain or lose electrons? 12. When non-metals become ions what kind of charge do they have? 13. How can you tell how many electrons an element will gain or lose to become an ion? 14. Define Valence Electrons Covalent Bond- Ionic Bond- Cation- Anion- 15. What types of elements form Covalent Bonds? 16. What types of elements form Ionic Bonds? 17. What type of bond is present in all biological molecules? Stoichiometry 1. Write formulas for the following names: Magnesium Phosphate, Copper (II) Nitrate, Lead (IV) Sulfate, Sodium Sulfide, Iron (III) Nitrate, Acetic Acid, hydrochloric acid 2. Define atomic mass unitmole (number of particles)- mole (definition)- STP- STP (molar volume of gas conversion factor) 3. At STP, what is the total volume occupied by 32g sample of O 2? Final Review Page 4
4. Define and give an example of each of the following Synthesis Reaction Decomposition Reaction Combustion Reaction Single Replacement Reaction Double Displacement Reaction 5. When the equation Al (s) + O 2(g) ---> Al 2 O 3(s) is correctly balanced using the smallest whole numbers, the coefficient of Al (s) is: 6. Given the reaction: (NH 4 ) 2 CO 3 ---> 2NH 3 + CO 2 + H 2 O What is the minimum amount of ammonium carbonate (in moles) that reacts to produce 8.0 mole of ammonia? 7. What is the total number of atoms contained in a sample of the following: Argon 1.00 moles Oxygen 0.50 moles 8. How many moles of the following are contained in each sample? 28.00g N 2 10.0g Ne 62g P 6.02x10 23 molecules of O 2 12.6x10 23 molecules of ZnCl 2 9. Given the reaction 6CO 2 (g) + 8H 2 O(g) 2C 3 H 7 OH (g) + 9O 2 (g) What is the total number of moles of water required to make 6.0 mol of C 3 H 7 OH 10. Calculate the molar mass of the following: (NH 4 ) 2 CO 3 Al 2 (C 2 O 4 ) 3 11. Given the reaction: 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O (g) What is the total number of grams of oxygen needed to react completely with 2.50 moles of C 2 H 2 (g)? 12. In the following reaction how many grams of Fe2O3 would be produced by the complete oxidation of 224g of Fe? 4 Fe + 3 O 2 2 Fe 2 O 3 Final Review Page 5
13. Given the following reactants, predict the products and write the balanced chemical reactions: Silver Nitrate and Sodium Chloride Potassium Sulfate and Lead (II) Nitrate 14. Given the reaction: 2Al(s) + 6HCl(aq) 2AlCl 3 (aq) + 3H 2 (g) What is the mole to mole ratio between aluminum and hydrogen gas? 15. A reaction that hs be calculated to produce 75.0 g of CuCl2 actually produces 62.g of CuCl2. What is the percent yield? 16. Define Theoretical yield 17. Define Actual Yield 18. Define Limiting Reactant 19. Determine the percent composition of carbon in CH 4. 20. Convert 3500. ml to liters. Gasses and Their Properties 1. What do the following variables represent? P- V- R- T- n- add units to the above variables 2. Write the equations, corresponding graphs and if each relationship is direct or indirect for each of the following laws: Boyles Law Charles Law Lussac s Law 3. Write the equations for the following laws Combined Law Ideal Gas Law 4. What is the volume of 2.36 moles of gas at a temperature of 25.8 o C and a pressure of 1.15 atm. 5.Define and give values for: Absolute Zero STP 6.What will happen to over-filled balloons on a hot day? Why? Final Review Page 6
7. Convert to Kelvin Convert to Celsius 100 o C 273 K 0 o C 300 K 23 o C 0 K 8. The cylinder is filled with gas at STP. Calculate the volume of the cylinder of 5.0 moles of gas fit inside the cylinder at STP. GAS 9. Define Diffusion 10. Using the concept of gasses and diffusion, describe how air fresheners work. Chemical Thermodynamics 1. Write the 3 thermodynamics equations we use to solve problems and define each variable. 2. How many calories of heat are needed to change 20 grams of ice to water at the melting point temperature? 3. How much heat is required to raise the temperature of 100 grams of aluminum by 1.0 o C? How about Carbon? 4. List the indicators of a chemical change: 5. Draw a graph for an exothermic reaction. Is H positive or negative for the process? Is energy absorbed or released? Specific Heats of Some Substances Substance Specific Heat, J/g ºC H 2 O (l) 4.184 H 2 O (s) 2.03 Al (s) 0.89 C (s) 0.71 Fe (s) 0.45 6. Draw a graph for an endothermic reaction. Is H positive or negative for the process? Is energy absorbed or released? Hg (l) 0.14 Final Review Page 7
7. Is the substance in the graph below being heated or cooled? Label the following on the graph: Solid, liquid, gas, melting, boiling 8. Define each of the following terms and state if energy is absorbed or released by the process: Sublimation Condensation Freezing Melting Deposition Evaporation 9. Answer the following questions about the graph: Which part of the graph represents gas heating? Which part of the graph represents liquid heating? How much energy does it take to heat the liquid? Which part of the graph represents vaporizing? How much energy does it take to vaporize the sample? Which part of the graph represents melting? Final Review Page 8
How much energy does it take to melt the sample? Which part of the graph represents solid heating? 10. Label the graphs endothermic and exothermic: A B Reaction Rates 1. Define Reaction Rate- 2. List the conditions that make a reaction go faster: 3. According to the collision theory, what conditions must be met in order for a reaction to be successful? 4. Answer the following question about the graph How much product is initially present? How much reactant is initially present? At what time are the amounts of product and reactant equal? At what time to the amounts of product and reactants become constant? As the reaction proceeds forward, what happens to the amount of product? As the reaction proceeds forward, what happens to the amount of reactant? As the reaction goes to completion what happens to the concentration of reactants? As the reaction goes to completion what happens to the concentration of products? 5. Define catalyst 6. How do catalysts work? Final Review Page 9
Equilibrium 1. What types of chemicals (solid, liquid, gas aqueous) are included in equilibrium expressions (K)? 2. What is the only 1 thing that affects K values? 3. Write an equilibrium expression for each of the following: 4A(s) +2B(g) 3C(aq) + 2D(l) E(g) + 3F(g) 2G(g) + 4H(g) 4. A large K value indicates that are favored. 5. A small K value indicates that are favored. 6. Define equilibrium- 7. How do you know when equilibrium of a system is attained? 8. For the system SO 2 (g) + Cl 2 (g) SO 2 Cl 2 (g) at equilibrium, write the effect on each reactant and product if Cl 2 (g) is added. 9. The statement represents a chemical reaction at equilibrium A + B C + D + heat List at least 3 ways to increase substance D 10. In the reaction N 2 + 3H 2 2 NH 3 + heat, why would an increase in pressure forces the reaction to the right? 11. Note the equation: AgCl (s) + 2(S 2 O 3 ) -2 (aq) Ag(S 2 O 3 ) -3 + Cl 1 (aq ). List the effects on each species if more (S 2 O 3 ) -2 (aq) is added to the system. Density 1. What is the density of a substance that has a mass of 5.9 grams and a volume of 61 L? Average Atomic Mass 1. Calculate the average atomic mass of iridium using the following data for two iridium isotopes. Isotope mass (g/mol) percent abundance Ir-191 191.0 37.58% Ir-193 193.0 62.42% Molecular Shapes Final Review Page 10
1. Write down the names of the 5 molecular shapes. For each give a brief description (atoms bonded to the central atom, loner pairs of electrons, bond angles) 2. What is the molecular shape of the following compounds? a. CO 2 b. H 2 O c. NH 3 d. CH 4 e. CH 2 O Empirical/Molecular Formulas 1. The molecular formula of the antifreeze ethylene glycol is C2H6O2. What is the empirical formula? 2. A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C2H4NO. If its molar mass is 116.1 g/mol, what is the molecular formula of the compound? Limiting Reactants 1. What is the limiting reactant when 2.0 moles of magnesium react with 2.0 moles of nitrogen to produce magnesium nitride? Gases 1. What volume will 2.5 mol of O 2 gas occupy at STP? 2. Balance the chemical equation and use it to solve for the following problem: Al(s) + H 2 SO 4 (aq) What volume of Hydrogen gas will be produced @ STP from 36.1g of Aluminum? 3. A gas occupies 11.2 liters at 0.860 atm. What is the pressure if the volume becomes 15.0 L? 4. If 4.0 moles of a gas at a pressure of 5.4 atm has a volume of120 L, what is the temperature Types of Reactions Final Review Page 11
1. Which of the following single replacement reactions will occur? a. magnesium and hydrochloric acid b. zinc and lithium chloride c. copper and iron (III) oxide d. sodium and silver nitrate 2. For a double displacement reaction in which silver sulfate and sodium phosphate are the reactants, what are the products? Write a balanced chemical equation for this reaction. Don t forget states of matter. 3. From the problem above, what is the net ionic equation? Nuclear Chemistry 1. What is the equation for the beta decay of lead-206? 2. What is the equation for the alpha decay of radon-222? 3. What type of material can stop alpha particles? Beta? Gamma rays? 4. How much of a 10. g sample of Cs-137 would be left after 90 years? (1/2 life = 30 years) 5. Define fusion and give an example of a fusion reaction. 6. Define fission and give an example of a fusion reaction. Electron Arrangement 1. Draw an electron configuration, orbital diagram, lewis dot structure and bohr model diagram for each of the following elements: Lithium, Calcium, Flourine, Aluminum Final Review Page 12