I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at 1085 C. Teflon is highly resistant to corrosion. A copper (II) nitrate solution is blue. 2) Chemical or physical changes? burning bubbling breaking boiling corroding grinding condensing tarnishing 3) Classify as SUBSTANCE or MIXTURE. If it is a substance, classify as element or compound. If it is a mixture, classify as homogeneous or heterogeneous Element, Compound (Subs) Substance or Mixture? Homo, Heterogeneous (Mix) Sand and water Gold Sodium chloride dissolved in water Sulfur hexafluoride 4) State the Law of Conservation of Mass 5) A 16 g sample of methane reacts with 64 g of oxygen to produce water and 44 g of carbon dioxide. How much water was produced? 1
6) An object with a mass of 7.5g raises the level of water in a graduated cylinder from 25.1mL to 30.1mL. What is the density of the object? 7) Convert the following showing all work: a. 783kg to centigrams b. 10 m to megameters 8) The accepted density for aluminum is 2.7g/ml. Calculate the percent error if your result was 2.1g/ml. 9) How many significant figures are in the following: c. 0.004210g d. 3.87563 s e. 2,500,875 m f. 0.08763 ml g. 100,000 L II. Atomic Theory/ Nuclear Chemistry 1) Here are three isotopes of an element: 12 6 C 6 13 C 6 14 C (What are isotopes?) a. The name of the element is: b. The number 6 refers to the c. The numbers 12, 13, and 14 refer to the d. How many protons and neutrons are in the first isotope? e. How many protons and neutrons are in the second isotope? f. How many protons and neutrons are in the third isotope? 2
2) Fill in the following table: Name Symbol Atomic # Mass # Protons Neutrons Electrons Vanadium- 51 39 19 K 10 21 26 31 28 27 2 1 3) Write a balanced nuclear reaction for each of the following. a. Beta emission of carbon-14. 238 b. Alpha emission of U. III. Electrons and Light 1) Provide full electron configurations and full orbital diagrams for each of the following elements. a) S b) C 2) Provide noble gas electron configuration and noble gas orbital diagrams for each of the following elements. b) Sr c) Nb 3
IV. Periodic Table 1) Write the number of valence electrons and the Lewis Dot diagram for each of the following. a) Li b) Aluminum c) Oxygen d) Kr 2) On the periodic table: a. Locate the representative elements, transition elements, and inner transition elements. (Where are the lanthanides and actinides?) b. Locate the metals, nonmetals, and metalloids. c. Locate the alkali metals, alkaline earth metals, halogens, noble gases. 4
3). Define ionization energy. What periodic trends exist for ionization energy? 4) Define atomic radius. What periodic trends exist for atomic radii? 5). Define electronegativity. What periodic trends exist for electronegativity? V. Ionic Compounds and Naming 1) Show the number of valence electrons for the following group. Then state the type of ion the elements in each group would form. (ex.: Alkali metals have 1 valence electron and form a +1 ion) 5
2) What is the difference between and ionic and a covalent bond? 3) What type of elements form ionic bonds? Covalent bonds? 4) Ionic Compound Name Compound Formula 5) Acid Name Acid Formula a. magnesium nitrate b. iron (III) oxide a. Hydrochloric acid c. sodium phosphide b. Chloric acid d. calcium phosphate e. titanium (II) hydroxide f. lead (IV) chloride c. Sulfurous acid d. HF g. (NH4)3PO4 e. HNO 3 h. V2O3 i. SnCl2 j. Ca(NO3)2 k. CrSO4 6
VI. Covalent Compounds 1) Molecular (Covalent) Compound Name Compound Formula a. Carbon dioxide b. Diphosphorus pentoxide c. Dinitrogen monoxide d. CCl 4 e. H 2 O f. SeF 6 2) For each compound, draw the Lewis structure, state the shape, and tell if the molecule is polar or nonpolar. a) H 2 O b) CCl 4 c) NH 3 d) BF 3 VII. The Mole 1) What is the molar mass of the following: (you must show work for compounds) a) MgCl2 b) (NH4)2SO4 7
2) Determine the percent composition of the elements in MgCl 2 above to the nearest hundredth. 3) Name the following hydrates or give the formula: a. Na2CO3 * 10H2O b. BaCl2 * 4H2O d. Copper Sulfate trihydrate e. Magnesium Chloride heptahydrate 4) Calculate the missing quantities. Show work in blank space below Remember 1 mole = 6.02 * 10 23 particles 1 mole = molar mass (gram formula mass) 1 mole = 22.4 Liters at STP a) Compound Number of Moles Molar Mass Mass Molecules Volume Li(OH) 5.57 moles a) b) c) N/A Mg2(PO4)3 d) e) f) 5.66 * 10 21 atoms N/A CO2 g) h) 100 grams i) j) b) c) d) 8
e) f) g) h) i) 5) How many magnesium atoms are there in 5.66 * 10 21 atoms of Mg2(PO4)3? 6) What is the empirical formula of a compound if the percent composition is aluminum 15.77%, sulfur 28.11% and oxygen 56.12%? 9
7) The molar mass of a compound is 92g/mole. Analysis of the compound shows 0.608g of N and 1.388g O. What is the molecular formula of this compound? VIII. Stoichiometry Use the following equation to calculate the following: 4 FeS(s) + 9 O2(g) 2 Fe2O3(s) + 4 SO3(g) 1) What is the mole ratio of sulfur trioxide to iron (III) oxide? 2) How many moles of iron (III) oxide are produced from 12 moles of iron (II) sulfide? 3) How many grams of oxygen are needed to react completely with 5 moles of iron (II) sulfide? 4) How many grams of iron (II) sulfide are needed to react with oxygen to produce 168 g of sulfur trioxide? 12. For the reaction 2 H2 + O2 2 H2O calculate the percent yield if 860. g of water are produced when 100. g of hydrogen react with an excess of oxygen. 10
IX. Chemical Reactions Balance each equation. Determine if type of reaction: Synthesis, Decomposition, Combustion, Single Replacement, Double Replacement 1) H 2 + N 2 NH 3 2) Fe + CuNO 3 Fe(NO 3 ) 2 + Cu 3) CaCl 2 + HNO 3 Ca(NO 3 ) 2 + HCl 4) Al 2 O 3 Al + O 2 5) CH 4 + O 2 CO 2 + H 2 O X. States of Matter and Gases 1) What is STP? 2) What is absolute zero? 3) What is the relationship between pressure and volume of a confined gas? What gas law is this? 4) What is the relationship between temperature and volume of a confined gas? What gas law is this? 5) What is the relationship between temperature and pressure of a confined gas? What gas law is this? 6) What is the combined gas law? Ideal gas law? Dalton s Law of partial pressures? 7). What is the difference between effusion and diffusion? 11
8) Which gas will effuse faster, dihydrogen sulfide or diatomic bromine gas? Why? 9) A sample of air in a syringe exerts a pressure of 102.7 kpa at a temperature of 22ºC. The syringe is placed in a boiling water bath at 100.ºC. The pressure of air is increased to 1.23atm by pushing the plunger in, which reduced the volume to 0.224 ml. What was the original volume of the air? 10) What is the temperature of the gas inside a 750 ml balloon filled with 0.030 g H 2 gas? The pressure of the balloon is 1.2 atm. 11) Using your knowledge of molecular structure, identify the main intermolecular force in the following compounds. You may find it useful to draw Lewis structures to find your answer. a) PF 3 b) H 2 O c) CO 2 12
12) Where is the triple point on this diagram? 13) What phase of matter does region C represent? 14) What phase of matter will this substance be in at room temperature and pressure? 15) At a temperature of 0 C what pressure does the substance have to be under to be a solid? 16) At a pressure of 30 atm, what is the boiling point? XI. Solutions, Acids and Bases 1) How many grams of HCl are there in 37ml of 2.5M hydrochloric acid? 2) 15.6 grams of potassium chloride is dissolved in 120.ml of solution. What is the concentration of the solution? 3) A solution has a ph of 3. What is the [H + ]? poh? [OH -- ]? Is this an acid or a base? 13