CHEMISTRY REVIEW: FINAL EXAM Chapter 7 & 9: Ionic & Metallic Bonding In this chapter you will need to know how to: 1) Determine how many valence electrons an element has 2) Determine if an element will lose or gain electrons 3) Determine the type of ion an element will form 4) Name ionic compounds 5) Write formulas form ionic compounds 6) Explain how ionic bonds work 7) Explain how metallic bonds work Vocabulary: •
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Valence electron Octet rule •
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Cation Anion Ionic bond Formula unit Metallic bonds Alloy How are cations formed? How are anions formed? How are ionic bonds formed? What keeps them together? Give four (5) properties of ionic compounds/bonds: 1. 2. 3. 4. 5. How are metallic bonds formed? What keeps them together? For each of the following, give the # of valence e‐, the e‐ dot structure, the amount of e‐ lost/gained to form an ion 1. Ga 2. Xe 3. Mg 4. H 5. Rb 6. Br Write a formula for the following ionic compounds: 1. nickel (III) sulfide 3. silver acetate 2. manganese (II) phosphate 4. potassium carbonate Name the following ionic compounds: 3. Cu(OH)2 1. FePO4 2. K3N 4. Zn(NO2)2 Chapter 8 & 9: Covalent Bonding In this chapter you will need to know how to: 1) Determine if elements will form an ionic, covalent or metallic bond 2) Draw covalently bonded compounds 3) Name covalent compounds 4) Write formulas for covalent compounds 5) Determine if a bond will be polar or non‐polar 6) Determine if a molecule will be polar or non‐polar Vocabulary: •
Covalent bond •
Molecular compound •
Diatomic molecule •
Monatomic element •
Empirical formula •
Molecular formula What are the diatomic molecules? Name six monatomic elements: What is shared in a single covalent bond? Double covalent bond? Triple covalent bond? Give five (5) properties of covalent molecules/bonds: 1. 2. 3. 4. 5. What type of bond would each of the following sets of atoms form? (ionic/metallic/covalent) 1. Na & Mg 3. Na & S 5. Ca & I 2. Al & O 4. B & Cl 6. F & H Classify each of the following as an atom or a molecule: 1. Be 3. N2 5. Ne 2. CO 4. H2O Draw the structure of each of the following covalent molecules. They may contain single, double, or triple bonds: 1. SHF 4. C2H2 2. BH3 5. C2H6 3. P2H4 6. N2 What is a polar covalent bond? Would a bond between the following elements be polar or non‐polar? 1. C & I 2. Si & N 3. H & H Write formulas for the following covalent compounds: 1. Hexaboron nonasilicide 4. Iodine pentafluoride 2. Chlorine dioxide 3. Hydrogen diiodide 5. Carbon monosulfide 6. Dinitrogen heptoxide Write the names for the following covalent compounds: 3. B2Si7 1. P4S5 2. SeF6 Chapter 10: Chemical Quantities In this chapter you will need to know how to: 4. NF7 1) Convert between moles, grams, liters & atoms using dimensional analysis 2) Calculate % composition of a compound either starting with a formula or masses 3) Calculate an empirical formula if you are only given % composition 4) Calculate a molecular formula if you are only given an empirical formula and a molar mass Vocabulary: •
Mole •
Avogadro’s number •
Molar mass How many liters are in a mole of hydrogen? How many grams are in a mole of hydrogen? How many atoms are in a mole of hydrogen? Conversions using dimensional analysis: 1. How many molecules are in.78 moles of iron? 2. Calculate the volume of 5.0 moles of Al2O3. 3. How many atoms of helium do you need to fill a 5.50 liter balloon? What does percent composition tell you? Percent Comp. Calculations: 1. What is the percent composition of a sample containing 1.03g of N and 5.29 g of O? 2. Find the % comp of Pb(NO3)3. 3. Find the empirical formula of a molecule with 40.0% C, 6.67% H, and 53.33% O. (hint: convert % to grams, grams to moles, divide by the smallest amount, and find the smallest ratio) 4. Now, calculate the molecular formula for the compound above, if the molar mass is 90g/mol. Chapter 11: Chemical Reactions In this chapter you will need to know how to: 1) Balance chemical equations 2) Write an equations from a sentence/statement 3) Identify the type of reaction 4) Predict the products of a reaction if given reactants 5) Predict the precipitates in a double displacement reaction Vocabulary: •
Product •
Reactant •
Balanced chemical equations •
Combination reaction •
Decomposition reaction •
Single displacement reaction •
Double displacement reaction •
Combustion reaction • Precipitate Writing Chemical Equations: 1. Write the balanced equation for hydrogen and oxygen reacting to form water. What type of reaction is this? 2. Write the balanced equation for the following : silver nitrate + copper metal → silver metal + copper nitrate Balance the following reactions & identify the reaction typed. Then, predict the products. 1. ___ Br2 + ___ NaCl → 2. ___ HF → 3. ___ Zn(NO3)2 + ___ SnCl2 → 4. ___ CH2O + ___ O2 → 5. ___ Al + ___ H2 → For any of the double displacement reactions above, copy the full reaction and label any ppt’s: ________________________________________________________________________ Chapter 12: Stoichiometry & % Yield In this chapter you will need to know how to: 1) Determine the number of atoms/moles/molecules are being used in a reaction 2) Calculate molar ratios 3) Convert between grams/moles/liters of a reactant to grams/moles/liters of a product 4) Solve for theoretical yield using dimensional analysis 5) Solve for percent yield or actual yield Vocabulary: •
Stoichiometry •
Molar ratio •
Theoretical yield •
Actual yield •
Percent yield •
Error •
Percent yield formula Stoichiometry: ____ C2H6 + ____ O2 → ____ CO2 + ____ H2O 1. If you were given 3 grams of C5H9O how many grams of water would you produce? 2. If you were given 4.56 liters of O2 how many milli‐grams of carbon dioxide would you produce? Percent Yield: ____ NH3 + ____ N2SO4 → ____ (NH4)2SO4 + __ N2 1. I began this reaction with 200 grams of NH3 and excess N2SO4 what is my theoretical yield of (NH4)2SO4 ? 2. If I produced 20 grams of the product in the lab, what is my percent yield? 3. Instead, if I produced a 15% yield, what was my actual yield?