Chemistry Finals Study BookletMeasurement & Matter Topic 01 Summary • CHEM 1406 Finals Core Pillar 1 of 7 The Scientific Method Observation: Data collected using senses or instruments. Hypothesis: A testable, tentative explanation. Experiment: Controlled testing of the hypothesis. Conclusion: Statement on hypothesis support. Significant Figures Rule 1: Non-zeros are ALWAYS significant. Rule 2: Captured zeros are significant (102). Rule 3: Leading zeros NEVER sig (0.004). Rule 4: Trailing with decimal ARE sig (50.0). Matter & Temperature Physical Change: Identity remains same (melting). Chemical Change: Identity changes (burning). TF = 1.8(TC) + 32 Density Mastery Formula: Density = Mass / Volume Displacement: Vobj = Vfinal - Vinitial Topic 01 Notes Atoms & Periodic Table Topic 02 Summary • CHEM 1406 Finals Core Pillar 2 of 7 Dalton's Atomic Theory 1. Matter is made of indestructible atoms. 2. Atoms of different elements have different properties. 3. Law of Conservation of Mass applies to reactions. 4. Compounds form from specific atomic ratios. Structure ParticleChargeProton+1Neutron0Electron-1 Mass Number = P + N Isotopes Same protons, different neutrons. Atomic mass on Periodic Table is a weighted average. Periodic Trends Groups: Vertical. Same valence electron count. Ionization Energy: Decreases DOWN; Increases ACROSS. Topic 02 Notes Bonds & Compounds Topic 03 Summary • CHEM 1406 Finals Core Pillar 3 of 7 Ionic Bonds Metal + Non-metal. Electrons TRANSFERRED. Naming: Metal + Non-metal "-ide". Neutral charge required. Covalent Bonds Non-metal + Non-metal. Electrons SHARED. Uses prefixes (di, tri, tetra). Goal: Full Octet (8 valence). VSEPR Molecular Shapes Linear (HCN) Tetrahedral (CH4) Bent (H2O) Trigonal Planar (BF3) IMFs Dispersion: In all; only force for non-polar. Dipole-Dipole: Between polar molecules. H-Bonding: Strongest. H bonded to N, O, or F. Topic 03 Notes Reactions & Quantities Topic 04 Summary • CHEM 1406 Finals Core Pillar 4 of 7 Reaction Types Comb: A+B → AB Decomp: AB → A+B Single Rep: A+BC → AC+B Double Rep: AB+CD → AD+CB Moles Mass = moles × Molar Mass Ex: 4 mol Na × 23 g/mol = 92 g Energy 1 kcal = 4.184 kJ Exo: Heat released. Endo: Heat absorbed. Redox (LEO GER) Loss = Oxidation Gain = Reduction Topic 04 Notes Solutions & Acid-Bases Topic 05 Summary • CHEM 1406 Finals Core Pillar 5 of 7 Concentration Formulas M = mol / L M1V1 = M2V2 % m/v = (g/mL)×100 Acid-Base Acid: H+ Donor. Base: H+ Acceptor. Buffers Weak acid + Conjugate base salt. Ex: HF + NaF Solute: Smaller amount; being dissolved. Solvent: Larger amount; doing dissolving. Isotonic: Identical osmotic pressure as blood. Topic 05 Notes Organic Chemistry Topic 06 Summary • CHEM 1406 Finals Core Pillar 6 of 7 Functional Groups Aldehyde: R-CHO Ketone: R-CO-R Ester: R-COO-R Carb Acid: R-COOH Amide: R-CONH-R Ether: R-O-R Naming 1. Find longest chain. 2. Number from branch side. Ex: 2,4-dimethylpentane Reactions Aldehyde → Carboxylic Acid (Oxid) Amide + NaOH → Salt + Aniline "L-isomer: fursthest chiral -OH is on the LEFT." Topic 06 Notes Intro to Biochemistry Topic 07 Summary • CHEM 1406 Finals Core Pillar 7 of 7 Carbohydrates Aldose: Aldehyde functional group. Ketose: Ketone functional group. Ex: Ribulose is a Ketopentose (5 carbons, ketone sugar). Enzymes Lower Activation Energy (Ea) by providing an alternative reaction pathway. Proteins Dipeptide: Named AA1-yl-AA2 (Ex: Serylphenylalanine). Structural: Collagen (provides framework). Transport: Hemoglobin (carries oxygen). Topic 07 Notes
Comprehensive CHEM 1406 Finals Review TestComprehensive CHEM 1406 Finals Review Practice Exam • Total 50 Questions Name: Date: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. The name of a dipeptide with Serine at the N-terminal and Phenylalanine at the C-terminal is ________. A) serinephenylanine B) tyrosylserine C) serylphenylalanine D) seryltyrosine E) phenylalanylserine 4.00 moles of sodium (Na) have a mass of ________. A) 92.0 g B) 4.60 g C) 44.0 g D) 23.0 g E) 11.0 g A piece of iron with a mass of 119 g is placed in a graduated cylinder where the water level is 57 mL. The water level rises to 72 mL. What is the density of the iron? A) 2.1 g/mL B) 0.13 g/mL C) 24 g/mL D) 1.7 g/mL E) 7.9 g/mL Which of the following are characteristics of organic compounds: (i) contain C and H; (ii) have high melting points; (iii) are water soluble; (iv) are flammable? A) i, ii, and iv B) i, ii, and iii C) i and iii D) i and ii E) i and iv Which of the following is a chemical change? A) Hammering gold into foil B) Burning natural gas C) Melting ice D) Cutting paper E) Cutting a tomato You notice that there is more traffic between 8 and 9 in the morning. This would be a(n) ________. A) observation B) hypothesis C) experiment D) conclusion E) all the above The grades on the first exam are: 30 A's, 20 B's and 10 C's. What is the percentage of B's on the test? A) 100% B) 30% C) 20% D) 50% E) 33% Collagen, found in tendons and cartilage, is classified as a ________ protein. A) hormone B) storage C) catalytic D) structural E) transport The correct name for the compound SeO3 is ________. A) selenium trioxide B) selenium(VI) oxide C) selenium oxide D) triselenium oxide E) sulfur trioxide When an amide (e.g. acetanilide) is hydrolyzed with NaOH, the products are ________. A) acetic acid and aniline B) sodium acetate and anilinium chloride C) sodium benzoate and aniline D) sodium benzoate and anilinium chloride E) sodium acetate and aniline The shape of the HCN molecule is ________. A) linear B) tetrahedral C) trigonal pyramidal D) bent (109°) E) trigonal planar The elements sodium, magnesium, and silicon ________. A) are in the same group B) have the same number of neutrons C) have the same mass number D) are isotopes of each other E) are in the same period of elements A solution with the same osmotic pressure as the blood is ________. A) hypertonic B) molar C) isotonic D) hypotonic E) nontonic Which of the following is not a chemical? A) Water B) Carbon dioxide C) Salt D) Sugar E) Light According to atomic theory, which statement is true? A) all matter is made of electrons B) atoms are neither created nor destroyed C) atoms of different elements are same D) atoms are same element have different mass E) atoms can be split in chemical reactions What is the classification for this reaction: SO3 + H2O → H2SO4? A) Decomposition B) Replacement C) Combination D) Combustion E) Double replacement A mixture is prepared by dissolving 2 g of KCl in 100 g of H2O. KCl is the ________. A) covalent compound B) solvent C) solution D) solute E) liquid What element has the electron arrangement 2, 8, 8? A) Neon B) Sulfur C) Silicon D) Argon E) Oxygen In the number 12.345, the 4 is in the ________ place. A) tens B) ones C) tenths D) hundredths E) thousandths Which of the following examples illustrates a number correctly rounded to three significant figures? A) 0.03954 to 0.040 B) 4.05438 to 4.054 C) 109 526 to 109 500 D) 103.692 to 103.7 E) 20.0332 to 20.0 Chlorine has two isotopes, Cl-35 (75.8%) and Cl-37 (24.3%). The atomic mass of Cl is ________. A) exactly 35 B) more than 37 C) 24.3 D) less than 35 E) between 35 and 37 The correct formula for the compound formed from K and P is ________. A) K3P B) KP C) K2P D) KP2 E) KP3 The molecule N2O4 has ________ valence electrons. A) 16 B) 11 C) 6 D) 34 E) 22 Which of the following is not a characteristic of Group 1A elements (alkali metals)? A) Good conductors of heat B) Most are liquids at room temp C) React vigorously with water D) Shiny E) Good conductors of electricity 9.31 g is the same mass as ________. A) 9310 mg B) 931 μg C) 0.0931 dg D) 931 kg E) 93.1 cg Fe2(SO4)3 is called ________. A) iron(III) sulfate B) iron trisulfate C) diiron trisulfate D) iron(II) sulfate E) iron sulfate If the temperature is 20 °C, what is the temperature in Fahrenheit? A) 94 °F B) 43 °F C) -22 °F D) 239 °F E) 68 °F In 2Al + 3Br2 → 2AlBr3, what is oxidized and what is reduced? A) AlBr3 oxidized, Al reduced B) AlBr3 reduced, Al oxidized C) Al reduced, Br2 oxidized D) Al oxidized, Br2 reduced E) Al oxidized, AlBr3 reduced An L-enantiomer is defined by having the furthest chiral -OH group on the ________ side. A) Bottom B) Top C) Right D) Left E) Middle Ribulose is a 5-carbon ketone sugar. To what class does it belong? A) Aldopentose B) Aldotetrose C) Ketopentose D) Ketotetrose E) Ketohexose What volume (mL) of a 15% (m/v) NaOH solution contains 120 g NaOH? A) 13 mL B) 0.13 mL C) 18 mL D) 800 mL E) 120 mL Evaluate: (-4) x (-5) = ________. A) 0 B) 20 C) -1 D) -20 E) 1 Which of the following contains an aldehyde functional group? A) CH3-O-CH3 B) CH3-CH2-OH C) CH3-CHO D) CH3-CO-CH3 E) CH3-CH3 The main type of intermolecular force between particles of CH2I2 is ________. A) ionic bonds B) hydrogen bonds C) dispersion D) dipole-dipole E) dispersion forces 13.2 kJ is the same amount of energy as ________. A) 36.2 kcal B) 3.15 kcal C) 3.15 cal D) 55.2 kcal E) 55.2 cal An aldehyde forms a carboxylic acid by ________. A) hydrogenation B) oxidation C) neutralization D) hydrolysis E) reduction The function of the enzyme-substrate complex is to ________. A) raise the energy of products B) increase reactant concentration C) change the product formed D) lower the substrate energy E) lower activation energy Which is not a characteristic of the solid state? A) Definite shape B) Fixed positions C) Definite volume D) Particles move fast E) Close together What coefficient goes in front of O2 to balance: C5H8 + ? O2 → 5CO2 + 4H2O? A) 3 B) 1 C) 5 D) 9 E) 7 What is molarity of KCl made by diluting 75.0 mL of 0.200 M to 100 mL? A) 0.267 M B) 6.67 M C) 0.150 M D) 0.200 M E) 0.100 M Identify the Brønsted-Lowry base in: H2O + CO32- ⇌ HCO3- + OH-. A) HCO3- B) CO32- C) OH- D) H2CO3 E) H2O What is the IUPAC name of the ester formed from butanoic acid and ethanol? A) Butyl ethanoate B) Propyl ethanoate C) Ethyl butyrate D) Ethyl propanoate E) Ethyl butanoate How many moles of CaCl2 are in 250 mL of a 3.0 M solution? A) 750 moles B) 0.75 mole C) 83 moles D) 3.0 moles E) 1.3 moles A value of 36 mL is a measure of ________. A) density B) temperature C) volume D) mass E) length What is the IUPAC name of the 5-carbon alkane with methyl groups on C2 and C4? A) 1,1,3-trimethylbutane B) 2,4-dimethylpentane C) 2-methylhexane D) Heptane E) 2,2-dimethylpentane The ionization energy of atoms ________ going down within a group. A) increases B) decreases C) stays same D) doubles E) vanishes If apples are $0.67/lb, what is the cost of 2.5 kg of apples? (1 kg = 2.205 lb) A) $ 1.68 B) $ 0.27 C) $ 3.69 D) $ 2.63 E) $ 0.76 Which of the following could be a buffer? A) NaF(aq) B) NaF(aq) + H2O(l) C) HF(aq) + NaF(aq) D) HF(aq) + H2O(l) E) NaCl(aq) + HF(aq) How many centimeters are there in 57.0 in.? (1 in = 2.54 cm) A) 0.0445 cm B) 145 cm C) 22.4 cm D) 140 cm E) 22 cm What is the mass number of an isotope of silver (At# 47) with 62 neutrons? A) 107.9 B) 62 C) 109 D) 76 E) 47
Chem 1406 Finals Step by Step KeyStep-by-Step Answer Key (1-25) CHEM 1406 Finals Mastery 1 C. Serylphenylalanine. N-terminal amino acid (Ser) changes suffix to "-yl"; C-terminal (Phe) stays normal. 2 A. 92.0 g. Na = 23.0 g/mol. Mass = 4.00 mol * 23.0 g/mol = 92.0 g. 3 E. 7.9 g/mL. Vol = 72 - 57 = 15 mL. Density = 119 g / 15 mL = 7.93 g/mL. 4 E. i and iv. Organics contain C/H and are flammable. Most have low melting points and are water-insoluble. 5 B. Burning natural gas. Combustion creates new chemical identities (chemical change). 6 A. Observation. Stating a fact seen/noticed without explaining why or testing it yet. 7 E. 33%. Total = 30+20+10 = 60. (20 B's / 60 Total) * 100 = 33.3%. 8 D. Structural. Collagen provides mechanical support to tissues. 9 A. Selenium trioxide. Covalent naming uses prefixes. Se = Selenium, O3 = trioxide. 10 E. Sodium acetate and aniline. Amide hydrolysis with NaOH produces a carboxylate salt and the amine. 11 A. Linear. HCN has a triple bond between C and N and a single bond to H. 180 deg angle. 12 E. Same period. Na, Mg, and Si are all in Period 3 of the Periodic Table. 13 C. Isotonic. Iso = same; tonic = pressure. 0.9% NaCl is the standard isotonic solution. 14 E. Light. Light is energy (photons), not matter (chemicals). 15 B. Atoms neither created nor destroyed. This is the law of conservation of mass in Dalton's theory. 16 C. Combination. Two reactants join to form one single product. 17 D. Solute. The substance being dissolved (smaller amount) is the solute. 18 D. Argon. Total e- = 2+8+8 = 18. Argon has Atomic Number 18. 19 D. Hundredths. 1(tens) 2(ones) . 3(tenths) 4(hundredths) 5(thousandths). 20 E. 20.0. All digits in 20.0 are significant because of the decimal point. 21 E. Between 35 and 37. Average atomic mass is a weighted average of isotopes. 22 A. K3P. K is Group 1 (+1); P is Group 5 (-3). Need three +1 to balance one -3. 23 D. 34. N (5 val) * 2 = 10. O (6 val) * 4 = 24. 10 + 24 = 34. 24 B. Most are liquids. Alkali metals are solids at room temp (except Cs/Fr near melting). 25 A. 9310 mg. 9.31 g * 1000 mg/g = 9310 mg. Step-by-Step Answer Key (26-50) CHEM 1406 Finals Mastery 26 A. Iron(III) sulfate. Fe is +3 here to balance 3 sulfates (-2 each). 27 E. 68 F. Temp = 1.8(20) + 32 = 36 + 32 = 68. 28 D. Al oxidized, Br2 reduced. Al loses e- (0 to +3); Br gains e- (0 to -1). 29 D. Left. L for Left. The OH on the chiral center furthest from carbonyl is on left. 30 C. Ketopentose. Keto = ketone; pentose = 5 carbons. 31 D. 800 mL. 15 g / 100 mL = 120 g / X mL. X = (120 * 100) / 15 = 800. 32 B. 20. Negative times negative equals positive. 33 C. CH3-CHO. CHO is the condensed formula for an aldehyde group. 34 E. Dipole-dipole. (Correcting original key: CH2I2 is polar, so dipole-dipole is dominant). 35 B. 3.15 kcal. 13.2 kJ / 4.184 kJ/kcal = 3.154... kcal. 36 B. Oxidation. Adding an O atom or removing H atoms is oxidation. 37 E. Lower activation energy. Enzymes provide an easier path for reaction. 38 D. Particles move fast. In solids, particles vibrate in fixed positions; they move fast in gases. 39 E. 7. Right side has (5*2) + 4 = 14 Oxygen atoms. 14 / 2 = 7 in front of O2. 40 C. 0.150 M. M1V1 = M2V2. (0.200 M)(75 mL) = (X M)(100 mL). X = 15 / 100 = 0.150. 41 B. CO3^2-. It accepts the H+ from water to become bicarbonate. 42 E. Ethyl butanoate. Named alcohol-part (ethyl) + acid-part-oate (butanoate). 43 B. 0.75 mole. M = mol / L. Mol = 3.0 M * 0.250 L = 0.75. 44 C. Volume. mL is a unit of volume. 45 B. 2,4-dimethylpentane. 5C chain (pentane) with methyls at 2 and 4. 46 B. Decreases. Atoms get larger, valence e- are further from nucleus and easier to remove. 47 C. $3.69. 2.5 kg * 2.205 lb/kg = 5.5125 lb. 5.5125 lb * $0.67/lb = $3.69. 48 C. HF + NaF. Weak acid (HF) and its conjugate base salt (NaF). 49 B. 145 cm. 57.0 in * 2.54 cm/in = 144.78 cm. Round to 145. 50 C. 109. Mass Number = 47 (protons) + 62 (neutrons) = 109.
