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FUNDAMENTALS Name: ___KEY________________ Period: ____ SEMESTER TWO FINAL REVIEW SHEET Below are the types of questions you can expect to see on your final for Fundamentals. The topics are arranged in the order that we learned the concepts. If there are problems you do not understand, or need additional practice on, please revisit that unit’s review sheet from my website. In addition to a periodic table, scientific calculator and ion chart, you may also use this HANDWRITTEN review sheet. You may choose to answer directly on this sheet or on a separate sheet of paper and attach it. UNIT 5: CHEMICAL REACTIONS BALANCING AND TYPES OF REACTIONS 1. Definitions to know: chemical reaction, conservation of mass, endothermic, exothermic, subscript, coefficient, reactants, and products. 2. Calculate the number of atoms of each element shown in each of the following: a. Na2SO4 7 c. Cu(NO3)2 9 b. 2 MgCl2 6 d. Al2(CO3)3 14 3. Balance each of the following equations: a. ____ Na2CO3 + _ 2___ HCl __ 2__ NaCl + ____ H2O + ___ CO2 b. ____ Fe + __ 2__ HCl ____ FeCl2 + ____ H2 c. ____ F2 + _ 2___ KCl __ 2__ KF + ____ Cl2 4. What is an exothermic reaction? How could you tell if a reaction was exothermic? Reaction where energy is released and heat is released to the surroundings; gets warmer 5. What is an endothermic reaction? How could you tell if a reaction was endothermic? Reaction where energy is absorbed and heat is absorbed from the surroundings; gets cold 6. Name four factors that can affect the rate of a chemical reaction? Be able to explain each one. As an example: What would happen to the rate of reaction if: a catalyst was added, a sugar cube was crushed or 6M HCl was used instead of 2M HCl? Concentration, surface area, temperature, catalyst 7. What are the seven indicators of a chemical reaction occurred. Explosion, temperature change, color change, new odor produced, light produced, gas forms, new precipitate formed 8. Identify the types of reactions shown in each of the following equations: a. CaO + H2O Ca(OH)2 synthesis c. Mg(NO3)2 + KCl MgCl2 + KNO double rep b. 2 Al + NiBr2 AlBr3 + Ni single rep. d. PbO2 Pb + O2 decomp 9. Balance the following reactions with polyatomic ions and state which type of reaction it is. a. ___ AlCl3 + _3__ LiOH ___ Al(OH)3 + _3__LiCl b. ___ Ba(CN)2 + ___ H2SO4 ___ BaSO4 + _2__HCN CARBON BASED MOLECULES (Macromolecules) 1. Definitions to know: monomer, polymer, biochemistry, hydrocarbon, carbohydrate, protein, lipids, and nucleic acids. Monomer: a molecule of any class of compounds, mostly organic that can react with other molecules that can form larger molecules Polymer: any of a class of natural or synthetic substances composed of very large molecules, called macromolecules, that are multiples of simpler chemical units called monomers. Biochemistry: sometimes called biological chemistry, is the study of chemical processes within and relating to living organisms Hydrocarbon: are the simplest organic compounds. Containing only carbon and hydrogen, they can be straight-chain, branched chain or cyclic Carbohydrate: is a biological molecule consisting of carbon (C), hydrogen (H) and oxygen (O) atoms, usually with a hydrogen : oxygen atom ratio of 2:1 (as in water) Protein: are large biological molecules, or macromolecules, consisting of one or more long chains of amino acid residues. Lipids: one of the four macromolecules that is made up of fatty acids Nucleic acid: large biomolecules, essential for all known forms of life, which include DNA and RNA are made from monomers known as nucleotides 2. What is organic chemistry? The study of carbon based molecules 3. What properties of carbon make it the building block of life? Has four valence electrons and the ability to bond with many other atoms to form complex molecules 4. What are three examples of pure carbon? Diamond, graphite, charcoal 5. How many valence electrons does carbon have and what would the Lewis Dot Diagram look like? four 6. Be able to fill in a chart like the one shown below: MACROMOLECULE FOOD EXAMPLE MONOMER CARBOHYDRATES Bread, pasta, starches Monosaccharides (sugar) Proteins Eggs, fish, meat Amino acids NUCLEIC ACIDS N/A NUCLEOTIDES Lipids BUTTER, OIL Fatty acids FUNCTION IN BODY Energy storage BUILD MUSCLE DNA/RNA Insulation for organs, storage ACIDS AND BASES 1. Definitions: acid, base, neutral, amphoteric, and pH scale. Acids: ionic compounds (a compound with a positive or negative charge) that break apart in water to form a hydrogen ion (H+) Bases: ionic compounds that break apart to form a negatively charged hydroxide ion (OH-) in water Neutral: A solution that has a pH of 7. It is neither acidic nor basic Amphoteric: a substance that can act as an acid or base under various conditions pH scale: a measure of the strength of acidity or basicity based on the number of H+ ions in a solution 2. Know the chemical formulas for the five common acids (ex. Nitric, phosphoric, etc.) Acetic acid CH3COOH, Hydrochloric acid HCl, Nitric acid HNO3, Sulfuric acid H2SO4 Phosphoric acid H3PO4 3. What are three characteristics of acids? What are three characteristics of bases? Acids are sour, corrosive and typically plot in the red/orange range Bases are chalky, bitter and typically plot in the blue/purple range 4. What is the pH for a substance that is neutral? What is an example of a neutral substance? 7, water 5. Know the definition of Bronsted-Lowry acids and know how it is different from an Arrhenius acid. Bronsted-Lowry: Acid- proton donor, Base- proton acceptor Arrhenius: Acids release H+ ions and bases release OH6. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction: NH3 (g) + HOH (l) ⇄ NH4+(aq) + OH-(aq) Base Acid C.A. C.B. 7. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction: HCO3 -(aq) + HOH (l) ⇄ CO3 2-(aq) + H3O+ (aq) Acid Base C.B. C.A. 8. Rank these substances from most acidic to most basic: milk of magnesia, water, vinegar, soda, blood, hydrochloric acid and lye. HCl, vinegar, soda, water, blood, milk of magnesia, lye UNIT 6: MOLE CONVERSIONS, MOLE RATIOS, EMPIRICAL/MOLECULAR FORMULA 1. Definitions: mole, Avogadro’s number, molar mass, molar volume, molecules (atoms/particles), empirical formula, molecular formula, and percent composition. Mole: The amount of elementary particles that are in exactly 12 g of Carbon. A mole is Avogadro’s number of particles; 1Mole = 6.02 × 1023 particles = gram formula mass of an element/compound Avogadro’s Number: 6.02 × 1023 particles of any substance Molar Mass: The total mass (in g/M) of all substances in the compound or the element Molar Volume: at STP, one mole of any gas is equal to 22.4L Molecules: smallest physical unit of an element orcompound, consisting of one or more like atoms in an element and twoor more different atoms in a compound. Empirical formula a chemical formula showing the simplest ratio of elements in a compound rather than the total number of atoms in the molecule Molecular formula: a formula giving the number of atoms of each of the elements present in one molecule of a specific compound Percent composition: the percent of the total mass of the compound that is due to that component FORMULA MASS, MOLAR MASSES, MOLE CONVERSIONS 1. Calculate the formula mass in a.m.u. of the following: a. CaSO4 136.14 amu b. RbNO3 147.47 amu c. H2O 18.02 amu d. NaCl 58.5 amu 2. Calculate the gram formula mass (molar mass in grams) of the following: a. Li2CO3 73.89 amu c. CF4 88.00 amu b. AlPO4 121.95 amu d. Mg(OH)2 120.37 amu 3. Make the following conversions. a. What is the number of moles of CaS in 250 grams of the compound? 3.5 moles b. How many moles is 18.06×1023 molecules of SO2? 3 moles c. How many molecules of CO2 are in .75 moles? 4.515 × 1023 molecules d. How many moles are in 800 g of HCl? 21.94 moles e. How many moles are in 50 g Fe2O3? 0.3125 moles f. How many moles are in 44.8 L of CO2 gas at S.T.P.? 2 moles g. What is the volume of 5.6 moles of Cl2 gas at S.T.P.? 125.44 liters h. How many ions of Al=3 are present in one mole of AlCl3? 6.02 × 1023 PERCENT COMPOSITION, EMPIRICAL, AND MOLECULAR FORMULAS 1. What is the percentage composition of all elements in the compound calcium carbonate, Na2CO3? 43.38% Na 11.33% C 45.29% O 2. What is the percentage composition of oxygen in strontium nitrate, Sr(NO3)2? 41.402% Sr 13.237% N 45.361% O 3. Calculate the percent composition of each element in C6H12O6. 40.001% C 6.714% H 53.285% O 4. Calculate the percent composition of oxygen in N2O. 36.352% 5. How are empirical and molecular formula related? The molecular mass is a whole number multiple of the empirical formula mass. The empirical formula is always in lowest or simplest terms 6. Determine the empirical formulas for each of the following molecular formulas. a. C10H20….. CH2 d. C6H12…… CH2 b. H2O2…… HO e. Na2C2O4... NaCO2 c. Hg2Cl4….. HgCl2 7. The empirical formula for ethylene is CH. The empirical formula mass is 13 g/mole. Find the molecular formula if the molecular mass is 78 g/mol. C6H6 8. A compound has an empirical formula of OCNCl and an empirical mass that is equal to 77.5 grams. The molecular mass is 232.41 grams. What is the molecular formula? O3C3N3Cl3 MOLE RATIOS 1. Given this equation: N2 + 3 H2 ---> 2 NH3, write the following molar ratios: a. N2 / H2 1 / 3 b. N2 / NH3 1 / 2 c. H2 / NH3 3 / 2 2. Answer the following questions for this UNBALANCED equation: ___ H2 + ___O2 --> ___ H2O a. Balance the equation: _2__ H2 + ___O2 --> _2__ H2O b. What is the H2 / H2O molar ratio? 1 / 1 c. What is the O2 / H2O molar ratio? 1 / 2