Final Review Chemistry 101 You should know density, specific heat, dilution, ideal gas, and light equations.

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1 You should know density, specific heat, dilution, ideal gas, and light equations. 1) Which of the following elements is a transition metal? a) V b) Mg c) Si d) Br 2) Convert kg into milligrams. a) mg b) mg c) mg d) mg 3) The volume of a flask is measured to be 1.10 L. When filled with a gas, the mass is g. The mass of the flask is g when empty. Calculate density to the correct number of significant figures. a) g/l b) 1.27 g/l c) 1.3 g/l d) 0.79 g/l 4) Calculate the volume of an irregularly shaped piece of copper with a mass of 2.25 mg. The density of copper is known to be 8.96 g/cm 3. a) g/cm 3 b) 3.98 g/cm 3 c) 20.2 g/cm 3 d) g/cm 3 5) How many protons, neutrons, and electrons are present in 27 Al 3+? a) p = 13, n = 27, e = 10 b) p = 13, n = 14, e = 10 c) p = 14, n = 13, e = 10 d) p = 27, n = 13, e = 24 6) Which group of the periodic table contains the element magnesium? a) Alkali metal b) Alkaline earth c) Halogen d) Noble gas 7) How many electrons are in the calcium ion? a) 18 b) 19 c) 20 d) 21 8) Which of the following atoms or ions does not possess a noble gas configuration? a) Mg 2+ b) Cs + c) Xe d) Br 9) When aluminum reacts with chlorine, the formula of the expected compound is a) AlCl 2 b) AlCl c) AlCl 3 d) Al 3 Cl 10) Which is the correct formula for ammonium nitrate? a) NH 3 NO 2 b) NH 4 (NO 3 ) 2 c) NH 3 NO 3 d) NH 4 NO 3 11) Which of the following formula-name pairs are correct? A) K 2 SO 4 potassium sulfate B) Ca(NO 3 ) 2 calcium nitrate C) PF 3 phosphorus fluoride a) A and B b) A and C

2 c) B and C d) A, B, and C (all) are correct 12) The specific heat of aluminum is 0.89 J/gºC. If a 45 g piece of aluminum foil at room temperature (25ºC) is placed over a dish, what temperature will the foil be after it absorbs 6000 J of heat? a) 119ºC b) 240ºC c) 175ºC d) 150ºC 13) Calculate the mass of mol of MgSO 4. a) 18.1 g b) 72.4 g c) 30.1 g d) 3.00 g 14) Calculate the number of moles in 1.00 g of Ca 3 (PO 4 ) 2. a) mol b) mol c) mol d) mol 15) If the mass percentages of each element are as follows, what is the empirical formula of formaldehyde? (Elemental analysis: 40.0%C 6.7%H 53.3%O) a) CHO b) CHO 2 c) C 2 HO d) CH 2 O 16) Which of the following empirical formulas for ionic compounds is not correct? a) KBr b) MgO c) Na 2 S d) CaF 17) Which of the following ionic compounds has the largest lattice energy? a) K 2 S b) Al 2 O 3 c) KBr d) CaBr 2 18) The ground state electron configuration of Br is: a) [Ar]4s 2 4d 10 4p 5 b) [Ar]4s 2 3d 10 4p 5 c) [Ar]3s 2 3p 5 d) [Ar]4s 2 3d 10 4p 6 19) How many orbitals are in the third shell of a many-electron atom? a) 3 b) 8 c) 9 d) 18 20) Calculate the mass percent of aluminum in Al 2 O 3 3H 2 O. a) 35% b) 17% c) 65% d) None is within 5% 21) The reaction of chlorine with aluminum should have the following stoichiometry. a) Al + 3 Cl AlCl 3 b) 2 Al + 3 Cl 2 2 AlCl 3 c) Al + Cl 2 AlCl 2 d) Al + 2 Cl AlCl 2 22) How many grams of H 2 O are required to produce 13 g of C 2 H 2 according to the following equation? CaC H 2 O Ca(OH) 2 + C 2 H 2 a) 36 g b) 18 g

3 c) 26 g d) 9.0 g 23) Calculate the theoretical yield of CaBr 2 when 5.44 g of CaSO 4 and 7.62 g of KBr react according to the following equation? CaSO KBr CaBr K 2 SO 4 a) 2.00 g b) 3.20 g c) 1.00 g d) 6.40 g 24) Calculate the molarity of a solution prepared by dissolving 14.7 g of solid NaOH in enough water to make 1.50 L of solution. a) 9.80 M b) M c) 22.0 M d) M 25) Identify the spectator ion(s) in the following reaction: Na 2 CO 3 (aq) + Ca(NO 3 ) 2 (aq) CaCO 3 (s) + 2 NaNO 3 (aq) a) Na + (aq) only 2 b) CO 3 (aq) only c) Na + (aq) and NO 3 (aq) d) Ca 2+ 2 (aq) and CO 3 (aq) 26) Calculate the energy of a photon of light with a wavelength of 532 nm. a) J b) J c) J d) J 27) Which one of the following bonds would you expect to be the most polar bond? a) O-H b) N-C c) O-S d) C-B 28) The properties of a real gas are most likely to deviate from the properties predicted for an ideal gas when: a) Pressure is low b) Temperature is high and pressure is low c) Temperature is high d) Temperature is low and pressure is high 29) What is the volume of 4.7 moles of H 2 at 22ºC and 0.90 atm? a) 126 L b) 215 L c) 7.6 L d) 115 L 30) A balloon filled with helium has a volume of 1.60 L at 1.00 atm and 25ºC. What will be the volume after cooling in liquid nitrogen to 196ºC while maintaining a pressure of 1.00 atm? a) 6.19 L b) L c) 12.5 L d) 7.84 L

4 True / False more review content (all multiple choice on final exam) 31) Metallic elements tend to be hard and brittle. 32) Fluorine is the most reactive nonmetallic element. 33) Condensation is an exothermic process. 34) The boiling point of an aqueous salt solution is higher than the boiling point of pure water. 35) An exothermic process involves the transfer of heat from the surroundings to the system. 36) A photon of 233 nm light has more energy than a photon of 617 nm light. 37) A photon of 15 nm light has a higher frequency than a photon of 15 m light. 38) Ultraviolet light has less energy per photon than infrared light. 39) The molar mass of a gas is directly proportional to its density. 40) All strong acids and strong bases are strong electrolytes. 41) The ph of a solution of the strong base, NaOH, would be expected to be less than seven (7). 42) Oxidation involves the loss of electrons. 43) Salts of metals can be oxidized to form the pure elemental metal. 44) Rutherford s gold foil experiment demonstrated the existence of neutrons. 45) The Lewis structure of ammonia, NH 3, contains 3 lone pairs (non-bonding pairs) of electrons. Key 1) a 2) b 3) c 4) a 5) b 6) b 7) a 8) d 9) c 10)d 11)a 12)c 13)c 14)a 15)d

5 16)d 17)b 18)b 19)c 20)a 21)b 22)b 23)d 24)d 25)c 26)c 27)a 28)d 29)a 30)b 31)F 32)T 33)T 34)T 35)F 36)T 37)T 38)F 39)T 40)T 41)F 42)T 43)F 44)F 45)F 46)F

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided