Chemistry 1210 Study Guide Exam 1
Chemistry 1210 Study Guide Exam 1 Chem 1210
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This 12 page Study Guide was uploaded by Emily Notetaker on Sunday September 18, 2016. The Study Guide belongs to Chem 1210 at Ohio State University taught by Dr. Bartoszek-Loza in Summer 2016. Since its upload, it has received 410 views.
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Date Created: 09/18/16
Chemistry 1210 Study Guide – Ch. 1-4 Professor Loza Chapter 1: Define: Physical property – Chemical property – Chemical change – Physical property – Homogeneous mixture – Heterogeneous mixture – Law of constant composition – Law of definite proportions – Intensive properties – Extensive properties – Precision – Accuracy – List the prefix and abbreviation that correlates to the number: 15 3 -3 10 10 10 10 12 101 10 -6 10 9 10-1 10 -9 6 -2 -12 10 10 10 Classify the following mixtures as heterogeneous or homogeneous: Air - Stainless steel - syrup - Italian dressing - blood - wood - lemonade - There are three targets at a rifle range Target (A) has a group of bullet holes in the upper right quadrant of the target; Target (B) has a group of bullet holes in the middle of the target; and Target (C) has a bullet hole in each quadrant. The three targets were produced by (A) an instructor firing a newly acquired rifle; (B) an instructor firing his personal target rifle; (C) a student who has fired his target rifle only a few times. Discuss the precision and accuracy for each target. (A) (B) (C) In the process of attempting to characterize a substance, a chemist makes the following observations. The substance is a silvery white, lustrous metal. It melts at 649°C and boils at 1105°C. Its density at 20°C is 1.738 g/cm . The substance burns in air, producing an intense white light. It reacts with chlorine to give a brittle white solid. The substance can be pounded into thing sheets or drawn into wires. It is a good conductor of electricity. Which of these characteristics are physical properties, and which are chemical properties? Label each of the following as either a physical process or a chemical process: (a) rusting of a metal can (b) boiling a cup of water (c) pulverizing an aspirin (d) digesting a candy bar (e) exploding of nitroglycerin Solve each of the problems with the correct number of sig figs: (a) 14.3505 + 2.65 (b) 952.7 – 140.7389 (c) (3.29 x 10 )(0.2501) (d) 0.0588/0.677 (e) 320.5 – (6104.5/2.3) 5 3 (f) [(285.3 x 10 ) – (1.200 x 10 )] x 2.8954 (g) (0.0045 x 20,000.0) + (2813 x 12) (h) 863 x [1255 – (3.45 x 108)] Chapter 2: Define: isotopes – molecular formula – empirical formula – isomers – Dalton’s Atomic Theory: (1) (2) (3) (4) For the following people, explain their experiments and what discoveries they lead to. JJ Thomson: Robert Millikan: Ernest Rutherford: Chadwick: How many protons, neutrons, and electrons are in the following atoms? (a) 40Ar 65 (b) Zn (c) 7Ga 80 (d) Br (e) 18W 243 (f) Am Only two isotopes of copper occur naturally, 63Cu (atomic mass = 62.9296 65 amu; abundance 69.17%) and Cu (atomic mass = 64.9278 amu; abundance 30.83%). Calculate the atomic weight of copper. Predict the chemical formula of the compounds formed by the following pairs of ions: 3+ - (a) Cr and Br (b) Fe 3+and O 2- 2+ 2- (c) Hg 2 and CO 3 (d) Ca 2+ and ClO 3 + 3- (e) NH 4 and PO 4 Which of the following are molecular and ionic? (a) PF 5 (b) NaI (c) SCl2 (d) Ca(NO )3 2 (e) FeCl 3 (f) LaP (g) CoCO 3 (h) N 2 4 Name the following compounds: (a) Li2O (b) FeCl 3 (c) NaClO (d) CaSO 3 (e) Cu(OH) 2 (f) Fe(NO 3 2 (g) Ca(CH C3O) (h) Cr2(CO )3 3 (i) K2CrO 4 (j) (NH 4 2O 4 (k) SeO 2- -4 (l) HSe (m) HSeO 3- (n) N 2 (o) KCN (p) NaBrO 2 (q) Sr(OH) 2 (r) Fe (CO ) 2 3 3 (s) NaH P2 4 Give the chemical formula for each of the following substances: (a) sodium phosphate (b) zinc nitrate (c) barium bromate (d) iron (II) perchlorate (e) cobalt (II) hydrogen carbonate (f) chromium (III) acetate (g) potassium dichromate (h) aluminum hydroxide (i) potassium sulfate (j) copper (I) oxide (k) zinc nitrate (l) mercury (II) bromide (m) sodium hypobromite (n) hypochlorous acid (o) iodic acid (p) nitrous acid Chapter 3: Write a balanced equation for: (a) The combination reaction between lithium metal and fluorine gas (b) The decomposition reaction that occurs when solid barium carbonate is heated (two products form, a solid and a gas) What is the percentage of nitrogen, by mass, in calcium nitrate? Calculate the number of H atoms in 0.350 mol of C H O ? 6 12 6 Calculate the number of moles of glucose (C H O ) i6 12386 g of C H O . 6 12 6 Ascorbic acid contains 40.92% C, 4.58% H, and 54.50% O by mass. What is the empirical formula of ascorbic acid? A 5.325-g sample of methyl benzoate, a compound used in the manufacture of perfumes, contains 3.758 g of carbon, 0.316 g of hydrogen, and 1.251 g of oxygen. What is the empirical formula of this substance? Determine how many grams of water are produced in the oxidation of 1.00 g of glucose, C H6O 12 6 Solid lithium hydroxide is used in space vehicles to remove the carbon dioxide gas exhaled by astronauts. The hydroxide reacts with the carbon dioxide to form solid lithium carbonate and liquid water. How many grams of carbon dioxide can be absorbed by 1.00 g of lithium hydroxide? The most important commercial process for converting N from the air into 2 nitrogen-containing compounds is based on the reaction of N and H to for2 2 ammonia. How many moles of ammonia can be formed from 3.0 mol of N 2 and 6.0 mol of H ? 2 2C 6 12(l) + 5O (2) 2H C H2O6(l8 +42H O (g) 2 Assume that you carry out this reaction with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yield of adipic acid? If you obtain 33.5 g of adipic acid, what is the percent yield for the reaction? Hydrofluoric acid, HF (aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by HF(aq). Sodium silicate (Na S2O ),3for example, reacts as follows: Na 2iO (3) + 8HF(aq) H SiF (a2) +62NaF(aq) + 3H O(l) 2 (a)How many moles of HF are needed to react with 0.300 mol of Na SiO ? 2 3 (b)How many grams of NaF form when 0.500 mol of HF reacts with excess Na S2O ? 3 (c)How many grams of Na SiO can 2eact3with 0.800 g of HF? Chapter 4: Define: Solute – Solvent – Electrolyte – Non-electrolyte – Oxidation – Reduction – Reducing agent – Oxidizing agent – Classify these ionic compounds as soluble or insoluble in water: (a) sodium carbonate (b) lead sulfate Predict the identity of the precipitate that forms when aqueous solutions of BaCl 2nd K SO2ar4 mixed. Write the balanced chemical equation for the reaction. Write the net ionic equation for the precipitation reaction that occurs when aqueous solution of calcium chloride and sodium carbonate are mixed. Name the 7 strong acids: Name the 8 strong bases: Classify these dissolved substances as a strong electrolyte, weak electrolyte, or nonelectrolyte: CaCl 2 HNO , 3 H 2H5(ethanol), HCOOH (formic acid), KOH. For the reaction between aqueous solutions of acetic acid (CH COOH) and 3 barium hydroxide, write the balanced molecular equation, the complete ionic equation, the net ionic equation. Write the correct net ionic equation for the reaction of aqueous ammonia with nitric acid. Determine the oxidation number of sulfur in: (a) H 2 (b) S8 (c) SCl 2 (d) Na 2O 3 2- (e) SO 4 Write the balanced molecular and net ionic equations for the oxidation reaction of aluminum with hydrobromic acid. Will an aqueous solution of iron (II) chloride oxidize magnesium metal? If so, write the balanced molecular and net ionic equation.
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