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DO NOT WRITE ON THIS!!!! MSL REVIEW 1) List the 5 postulates of Dalton’s Atomic Theory. 2) How was Dalton’s Atomic Theory proven to be wrong? 3) What was Democritus’s contribution to the early Atomic Theory? 4) Describe the results of the Cathode Ray, Oil Drop, and Gold Foil experiments. 5) As the wavelength gets longer, the frequency will ____________________. This is an example of an _________________ relationship between wavelength and frequency. 6) The higher the energy, the greater the ____________________. This is an example of a _______________________ relationship. 7) When an electron moves from a low energy to a high energy level energy is _________________. 8) When an electron moves from a high energy to a low energy level, energy is _____________ and a _________________ is emitted. 9) Arrange the following from low to high energy: Infrared, Radio waves, Gamma rays, X-rays, Microwaves. 10) Which type of light has the shortest wavelength and the highest frequency? 11) Which type of energy is produced when an electron moves from n=4 to n=2? 12) What are the 3 subatomic particles? Identify their location in the atom? 13) Define isotope. Identify the number of protons, neutrons and electrons for the following. 109 63 a. a. 107 Cu, 65Cu c. 112 Sn,115Sn 47 Ag , 47 Ag b. 14) When writing nuclear symbols, A represents the _________________ and Z represents the __________________. 15) What is the difference between the atomic mass and mass number? 16) Write the hyphen notation and nuclear symbol for an atom that has 13 protons and 14 neutrons. 17) Identify the names for the following symbols: s, l, g, aq. Describe each phase. Identify the phase that has the greatest amount of disorder. 18) What is the difference between a ternary and a binary compound? 1 DO NOT WRITE ON THIS!!!! 19) Write the formula for the following compounds. Identify the bond type and if the compound is ionic or molecular. a. a. Magnesium chloride b. sodium hydroxide c. copper II sulfide b. d. carbon monoxide e. aluminum sulfate f. ammonium phosphate c. g. dinitrogen pentoxide 20) Write the name for the following compounds. Identify the bond type and if the compound is ionic or molecular. a. a. CuCl b. ZnSO4 c. CCl4 b. d. CaCO3 e. NaOH f. P2O5 c. g. PCl3 h. CuBr2 i. FeO 21) Write the name for the following acids. a. a. HCl b. HNO3 b. d. HC2H3O2 c. H2SO4 22) Write the formula for the following acids. a. a. hydrobromic acid b. phosphoric b. d. carbonic acid e. chloric acid c. hydroiodic 23) A student collected the data shown below to determine experimentally the density of distilled water. a. Mass of graduated cylinder + distilled H2O sample…163g b. Mass of empty graduated cylinder….141g c. Mass of distilled H2O sample….____g d. Volume of distilled H2O sample….25.3mL 24) A cube has a volume of 8.0 cm3 and a mass of 21.6 grams. The density of the cube is… 25) A chemistry student is given the task of analyzing three unknown samples. Her data is listed in Data Table 1. Use Data Table 1 to answer the questions below. Data Table 1 Trial Trial 1 Trial 2 Trial 3 Average Sample A Mass Volume (in (in mL) grams) 80.72 10.01 80.64 10.00 80.91 10.05 80.76 10.02 Sample B Mass (in grams) 95.41 92.33 93.78 93.84 2 Volume (in mL) 10.72 10.51 10.62 10.62 Sample C Mass (in grams) 72.28 72.32 72.34 72.30 Volume (in mL) 10.00 9.99 9.95 9.98 DO NOT WRITE ON THIS!!!! The student compares her data to the following chart in the back of her textbook. Can she identify Samples A, B, and C based on the data she recorded? Table A Properties of Common Metals Name Color at room temperature Aluminum Silver metal Copper Red metal Iron Silver metal Nickel Silver metal Tin White metal Density 2.701 8.92 7.86 8.90 7.28 26) Review Handout on Solubility Curves 27) The Diagram below represents four 500-milliliter flasks. Each flask contains the gas represented by its symbol. All gas samples are at STP. Each flask contains the same number of atoms/molecules/atoms and molecules. 28) Gas Laws a. A sample of a gas is at STP. As the pressure decreases and the temperature b. increases, the volume of the gas _______________. c. Under which condition will the volume of a given sample of a gas decrease 1. decreased pressure and decreased temperature. 2. decreased pressure and increased temperature. 3. increased pressure and decreased temperature. 4. increased pressure and increased temperature. d. e. f. g. h. i. j. If 10 liters of H2 (g) at STP is heated to a temperature of 546 K, pressure remaining constant, the new volume of the gas will be 20 liters. d. Draw the graph representing Boyle’s Law. Label the X & Y axis. e. Draw the graph representing Charles’s Law. Label the X & Y axis. f. Draw the graph representing Gay-Lussac’s Law. Label the X & Y axis. g. At a temperature of 273 K, a 400 milliliter gas sample has a pressure of 769 millimeters of mercury. If the pressure is changed to 380 millimeters of mercury at which temperature will this gas sample have a volume of 551 milliliters? How many moles of gas does it take to occupy 120 liters at a pressure of 2.3 atmospheres and temperature of 340K? 29) Describe the difference between cations and anions. How are they formed? 3 DO NOT WRITE ON THIS!!!! 30) An atom has 2 electrons in its valence shell. To what group does the atom belong? Will the atom for an anion or a cation? What will be the oxidation number of the ion? 31) An intermolecular force that holds ionic compounds together is called electrostatic attraction. 32) Describe the 3 intermolecular forces? Which of these forces is the strongest? weakest? 33) How are intermolecular forces different from chemical bonds? Which is stronger? 34) If the electronegativity difference between atoms is greater than 1.7, what type of bond will form? If the difference is less than 1.7, what type of bond will form? 35) What type of molecule has an electronegativity difference of 0? 36) Ionic compounds have high/low melting points, high/low boiling points, and can conduct electricity in the _________________ state and in ____________________solutions. 37) Metallic bonds can be described as a _____________ of ______________ electrons. 38) List 6 properties of metals. 39) Atoms bond to become ________________________. _________________ energy lowers when unstable atoms bond. 40) Which group on the table does not need to bond in order to be stable? 41) Which diatomic molecules have single covalent bond? double covalent bond? triple covalent bond? Draw the Lewis Structure for each. 42) Draw Lewis Structures for the following. Identify the geometry and polarity of each molecule. a. a. PH3 b.CCl4 c. CO2 d. SO3 e. H2O f. H2S b. g. SO2 h. NH3 43) Which bond type is the shortest…single, double or triple? Which has the greatest bond energy….single, double or triple? 44) Draw the Lewis structures for the following molecules, I2, O2, N2. Which has the shortest bond length? Which has the longest bond length? Which has the greatest bond energy? 45) The process that occurs when a solid turns into a gas is called ______________. 46) When looking at a heating/cooling curve, phase changes occur at __________________ temperature. 47) When held at constant pressure, what change will occur when the pressure is increased over boiling water? 48) Identify the 6 phase changes that water can undergo. 4 DO NOT WRITE ON THIS!!!! 49) Identify the number of main groups on the periodic table and the name of each one. 50) How many periods are on the periodic table? 51) Groups are __________________ columns and periods are _________________ rows on the periodic table. 52) Elements within the same _________________ have similar chemical properties, the same _______________ number and the same number of _____________ ____________. 53) ______________ ________________ are responsible for the chemical reactivity of elements. 54) As you move _____________ the group, the reactivity of ____________ increases. As you move _______ the group for _______________, the reactivity increases. 55) The ____________ metals are located in the ____________ of the periodic table. 56) _____________ numerals are used to identify the ____________________ number of transition metals. 57) Write electron configurations and noble gas configurations for the following elements/ions. a. Ne b. Ca c. Au d. Br e. Mg f. Potassium ion g. Phosphide h. Aluminum ion j. Sulfide k. O2l. Mg2+ 58) Identify the following elements based on the electron configuration. a. 1s22s22p63s23p1 b. 1s22s22p63s23p63d84s2 c. [Ne} 3s1 d. [Ar]3d34s2 59) S block elements include groups ________. P block elements include groups__________. D block elements are groups ___________. F block elements are located _______________. 60) Identify the number of valence electrons from the following electron configurations in problems 58 a-l and 59 a-d 61) How many electrons were lost/gained for letter 58 f-l? What is the oxidation number for each? 62) Define ionization energy. Write the group and period trend. Arrange the following elements in order of decreasing ionization energy. a. a. Cl, Br, F, I b. C, B, N, O c. Ca, Sr, Mg, Ba 63) Define atomic radius. Write the group and period trend. Arrange the following elements in order of increasing atomic radius. a. a. Cl, Br, F, I b. C, B, N, O c. Ca, Sr, Mg, Ba 5 DO NOT WRITE ON THIS!!!! 64) Define ionic radius. Write the group and period trend. Arrange the following elements in order of decreasing ionic radius. a. a. Cl-, Br-, F-, I-, b. P3-, S2-, N3-, O2c. Ca2+, Sr2+, Mg2+, Ba2+ 65) Define electronegativity. Write the group and period trend. Arrange the following elements in order of increase electronegativity. a. a. Cl, Br, F, I b. C, B, N, O c. Ca, Sr, Mg, Ba 66) Complete the following conversions. a. a. 4.2 moles C to atoms b. c. 1.6 x 1019 molecules H2 to moles c. e. 4.7g C to atoms d. g. 5.2 x 1012 molecules CH4 to g e. 0.23 moles H2 to L b. 2.94 moles CO2 to molecules d. 6.1 x 1026 atoms S to moles f. 2.73 g SO2 to molecules h. 4.7L CH4 to moles 67) 1 mole of any gas at STP equals ______________. 68) How many grams of ammonium chloride are contained in 0.5 L of a 2 M solution? 69) What is the molarity of a solution on KNO3 that contains 404 grams of KNO3 in 2L of solution? 70) What is the molarity of a solution containing 20 grams of sodium hydroxide in .5 L of solution? 71) What is the total number of moles in 2 liters of 3 M of sodium hydroxide? 72) The empirical formula of a compound is CH2 and its molecular mass is 70. What is the molecular formula of the compound? 73) If the empirical formula for an organic compound is CH2O, then the molecular mass of the compound could be….135,45,60,15. 74) A compound consists of 40% sulfur and 60% oxygen by mass. What is the empirical formula of this compound? 75) What is the empirical formula of a compound if a sample contains 8.52 grams of carbon and 1.42 grams of hydrogen? 76) What is the percent by mass on nitrogen in the compound NH4NO3? 77) Given the unbalanced equation N2(g) + H2(g) NH3(g), when the equation is balanced, the ratio of moles of hydrogen consumed to moles of ammonia produced is _______.3:2 78) Na + H2O NaOH + H2 What is the total number of moles hydrogen produced when 4 moles of sodium react completely? 2 6 DO NOT WRITE ON THIS!!!! 79) C2H2(g) + O2(g) CO2 + H2O(g) What is the total number of grams of O2(g) needed to react completely with 0.50 mole of C2H2? 40g 80) CO2(g) + H2O(l) CO2(s) + O2(g) What is the minimum number of liters of CO2(g) measured at STP, needed to produce 32 grams of oxygen? 22.4L 81) H2 + O2 H2O The total number of grams of O2 needed to produce 54 grams of water is….48g 82) Write the balanced equation for the reaction of lead (II) nitrate with sodium iodide to form sodium nitrate and lead (II) iodide. a. If I start with 25.0 grams of lead (II) nitrate and 15.0 grams of sodium iodide, how many grams of sodium nitrate can be formed? b. What is the limiting reagent in the reaction? c. How much of the excess reagent is used? How much remains? 83) Which 2 solutions when mixed together will undergo a double replacement reaction and form a white solid substance? a. NaCl(aq) and LiNO3(aq) b. KCl(aq) and AgNO3(aq) c. KCl(aq) and LiCl(aq) d. NaNO3 and AgNO3(aq) 84) Be able to distinguish between single replacement, double replacement, synthesis, and decomposition reactions. Refer to reference tables 85) Predict the products of the following reactions. Use the reference table for assistance. a. ____ Ca(OH)2 + ____ HF b. NaC2H3O2 + ____ H2SO4 c. Aluminum bromide and chlorine gas react to form … 86) What must be present for combustion to take place? What are the products of a combustion reaction? 87) Neutralization is a type of _________________ reaction. Neutralization occurs between _____________and _______________. The products of this reaction are _____________ and ____________. 88) An atom in an _______________ state is above its ground state because of the absorption of ___________ resulting _____________ moving to a ___________ energy level. When the atoms returns to its ___________ state, the electron releases energy in the form of a ___________ that resembles energy from the electromagnetic spectrum. 7 DO NOT WRITE ON THIS!!!! 89) a. b. c. d. e. f. What is the boiling point of the substance? Solid and liquid phases can exist in equilibrium between points…. Which segments represent potential energy? Which segments represent kinetic energy? Is this an example of a heating or cooling curve? Which segment(s) represent an endothermic process? 90) Endothermic means heat energy is going ________; Exothermic means heat energy is going _______. 91) a. b. c. d. e. At point A, what phase change will take place as the pressure decreases and temperature remains constant? At what point do all three phases exist in equilibrium? At point J, what phase change will take place as the temperature decreases and pressure remains constant? 92) . The universe tends towards __________. This is called ____________. Arrange the following in order of increasing entropy—g, l, s; ionic solutions, ionic compound 93) Write the symbols for: a. alpha particle_______________; b. beta particle______________; c. gamma particle _________________. 8 DO NOT WRITE ON THIS!!!! 94) In the equation X 95) In the equation 234 91 226 88 Ra 24He , X represents… Pa X + 10 e , X represents… 96) Define half-life. Review the half-life calculations. 97) What is the different between fusion and fission? 98) In order to satisfy the Law of Conservation of Mass, chemical equations must be ________________. 99) In a balanced chemical equation, the mass of the ____________ = the mass of the _____________. 100) Describe the difference between a total/complete ionic equation and a net ionic equation. a. NaCl(aq) + Pb(NO3)2(aq) PbCl2(s) + NaNO3(aq) 101) If ∆H+=endothermic; ∆H-=exothermic 102) List properties of acids/bases. 103) What is the formula for concentration? 104) What is the difference between strength and concentration as related to an acid? 105) Identify the 6 strong acids and bases. 106) Write the equation for dilution. 107) If the pH is below 7, the substance is a(n) ____________, above 7 is a(n) ___________, and equal to 7 is ______________. 108) Litmus is __________in an acid and ____________in a base. 109) 110) 111) 112) Write the equation used to calculate pH. Review the pH and pOH calculations. Review the dilution calculations. Name the following acids: a. HCl b. H2NO3 c. H3PO4 d. HBr 9 DO NOT WRITE ON THIS!!!! 113) a. b. c. d. e. f. g. h. Which letter represents the activation energy? Is this a diagram of an endothermic or exothermic reaction? Which letter represents the activation energy for the reverse reaction? Is the reverse of the reaction endothermic or exothermic? Which letter represents the potential energy? Which letter represents the heat of reaction? What will change as a result of the addition of a catalyst. Review the handouts on potential energy. You should be able to do the calculations. 114) Given the equation 12.6 kcal + H2(g) + I2(g) 2HI(g), identify the equilibrium shift based on the changes. a. Add H2 b. Remove I2 c. Increase temperature d. decrease pressure e. Increase pressure 115) Given the equation NaOH(s) Na+(aq) + OH- (aq) + 10.6 kcal HINT: pure solids and liquids do not affect equilibrium. a. Add NaOH b. Increase temperature c. decrease pressure 10