Chemistry First Semester Final Review Topics

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1 Chemistry First Semester Final Review Topics Name 1. Intro-be able to: Define and give examples of : an element, a compound State the difference between a physical change and a chemical change. Review your sig figs and how to use them in calculations. Calculate Density 2. Periodic Table- be able to: Identify groups, periods, metals, nonmetals, semimetals, states of matter for elements in the periodic table, group names in the periodic table (alkali metals, alkaline earth metals, transition metals, noble gases, halogens) and determine valence electrons. Write electron configurations for atoms and ions Define : isotopes, subatomic particles(protons, electrons, neutrons), atomic mass, atomic number Define- ionization energy, electro negativity, atomic and ionic radius; know how they increase/decrease across a period or up/down the group 3. Stoichiometry - be able to: Balance chemical equations Calculate molar mass Convert between mass to moles, particles and vice versa; know Avogadro s number Solve Stoichiometry problems (conversions mass to mass) List diatomic molecules 4. Gases be able to: State Kinetic Molecular Postulates and Properties Convert between different pressure, temperature and volume units, Describe the three gas laws including their graphs Use the ideal and combined gas law to solve problems State Avogadro s Hypothesis Define: STP, Absolute zero List the instruments used to measure the volume, pressure, mass and specify the needed unit 5. Ionic Compounds- be able to: Name ionic compounds Draw the structure for table salt List properties for ionic compounds Describe how an ionic bond forms Explain the dissolving in water of an ionic compound 6. Covalent Compounds- be able to: Name covalent compounds Differentiate between polar and non- polar covalent compounds Describe how a covalent bond forms 7. What is the difference between an ionic and a covalent bond 8. Organic Chemistry be able to: Differentiate between monomers and polymers; amino acids and proteins What kind of bonding do large biological molecules have

2 Chemistry First Semester Final Review WKS 1 Name Per Intro Review 1. Identify the number of significant figures: mm 7000 L.0002 m mm 2. Work out the following problems: 12.0g / 6.0cm 3 = 22.33mL mL mL= 6.5cm x cm x 4cm = 5.77g g g = 3. Write the numbers in exponential notation: 730mL= g= 4. Write the following exponential numbers in regular notation. (2.15x10-4 ml) (4.3 x10-5 ml) = 7.05x102m x 1.1x104 m x 5.0x10-2m = 5. Identify the following as an atom, molecule, element, and/or compound (may have multiple answers): O2, He, C6H12O6 Periodic Table Review: Isotope Protons Neutrons Electrons Mass # Atomic # Pt Se B Write the isotopic notation for a cation with 74 protons, 109 neutrons, and 71 electrons. 11. Which of the three subatomic particles carries a negative charge? No charge? Positive charge? 12. Which of the three subatomic particles has a larger mass the protons or the electrons?

3 The Mole Review: 13. Balance the following equations: C5H12 + O2 CO2 + H2O FeS2 + O2 Fe2O3 + SO2 Al (OH)3 + H2SO4 Al2 (SO4)3 + H2O KClO3 KCl + O2 O2 + H2O H2O2 Na2O2 NaOH + O2 Zn + H2SO4 ZnSO4 + H2 P4 + O2 P2O5 14. Find out the molar mass (MM) for the following compounds. Show work. Ba(NO3)2 Al2(SO4)3 Mg3(PO4)2 BaSO4 (NH4)3(PO4)2 NH4I 15. Calculate the percent composition for NaBr. 16. Calculate the number of moles for 44.0g of H2SO4 17. Calculate the mass of 0.25 moles of NaHCO3 18. Calculate how many moles are in 100. g of Cu(NO3)2 19. Calculate the mass of 19.0 moles of C22H How many moles are in 6.022x10 23 atoms of Na 21. Calculate how many grams are in 3.01x10 23 formula units of NaOH 22. Calculate the number of molecules in 68.0g of H2S

4 Chemistry First Semester Final Review WKS 2 Name Per Stoichiometry Review: Use all stoichiometry steps and show all your work: 23. a. Calculate how many moles of oxygen gas are produced when 45.0 g of KClO3 are decomposed according to the following reaction: KClO3 KCl + O2 a. Calculate how many grams of KCl are formed when 45.0 g of KClO3 decomposes. b. Calculate how many liters of oxygen are produced when 45.0 g of KClO3 decomposes. 24. Calcium carbonate (CaCO 3 ) decomposes if heated to form calcium oxide (CaO) and carbon dioxide (CO 2 ). If 24.5 grams of calcium carbonate decompose a. How many moles of calcium carbonate reacted? b. How many moles of calcium oxide are formed? c. How many grams of calcium oxide are formed?

5 25. Diesel fuel (C 18 H 38 ) burns by combining with oxygen (O 2 ) to form carbon dioxide and water. If 56.5 grams of diesel burn a. Calculate the moles of diesel fuel that burned. b. Calculate the grams of water produced. c. Calculate the grams of carbon dioxide that are produced. 26. Use the following unbalanced equation to answer the questions below: SiO2 + C SiC + CO a. If 50.0 grams of SiO2 react, how many grams of SiC are formed? b. If the actual yield of SiC is 27.9 grams, what is the percent yield? 27. Aluminum reacts with chlorine gas (Cl2) to produce aluminum chloride (AlCl3). If 15.5 grams of aluminum reacts with chlorine, a. Calculate the mass of aluminum chloride that could be produced. b. If 43.6 grams of aluminum chloride are formed, calculate the percent yield.

6 Chemistry First Semester Final Review WKS 3 Name Per Gas Review: 28. Convert: torr= Pa and 3.5 atm = mmhg 29. The volume of a gas-filled balloon is 31.0L at 40 C and 150 kpa pressure. What volume will the balloon have at standard temperature and pressure? 30. You fill a rigid steel cylinder with a volume of 80.0L with nitrogen gas to a final pressure of torr at 39 C. How many moles of N2 gas does the cylinder occupy? 31. A gas at a temperature of 63 C occupies 9055 ml at 308.0kPa. What will be the new volume if the temperature changes to 96 C and the new pressure is kpa? 32. What pressure exerted by 1.43g of Krypton in a 25.9mL container at 9.0 C? 33. State and draw the graphs for the following laws a. Boyles Law b. Chales s Law c. Gay-Lussacs Law

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