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PRACTICE – Final Exam Name: ______________________ The Final Exam is six pages and has 60 questions - 109 points possible = 100 points + 9 Extra Credit 1) Complete the table below to convert between scientific notation and standard form 2 points Standard Form 62.3 g (example) Scientific Notation 6.23 x 101 g 1993 mL 0.0000072 kg 1.993 x 103 mL 7.2 x 10-6 kg Standard Form Scientific Notation 5.300 x 10-3 cm 2.68023 x 102 kg 6.71 x 10-4 L 0.005300 cm 268.023 kg 0.000671 L 2) Use <, >, or = for each of the questions below. 3 points a) 9.8 m _<_ 9800 km 0.0098 km 9,800,000 m b) 1 mL _>_ 0.010 cL 0.1 cL 0.1 mL c) 3.5 g _=_ .0035 kg 0.0035 kg 3.5 g 3) Complete the table below – Note that the particles are not is the same order: 3 points Charge Location AMU 0 In Nucleus 1 Neutron 1Electron Cloud 0 Electron 1+ In Nucleus 1 Proton 4) Draw the Lewis Structures for the following neutral atoms. 3 points C F Si He Ga Ba 6) Fill in the blanks using one of the following elements. Please note that each element may be used once, more than once, or not at all. 10 points K, Ca, Ga, C, As, O, Cl, Kr __Ca___ is an example of metal __ O __ is an example of a nonmetal __ As ___ is an example of a metalloid __ C ____ has 6 total electrons __ O_ ___ has 6 valence electrons __ K ____ has 1 valence electrons __ Ca ___ is an Alkaline Earth Metal __ Kr ___ is a Nobel Gas. __ Cl __ is a Halogen ___ K __is an Alkali Metal 13) Look at each pair of elements below, select (circle) which element has the larger atomic radii: Be or Ca Na or P N or B 2 points 14) Look at each pair of elements below, select (circle) which element has the higher ionization energy: C or Si F or Br N or Li 2 points 15) Look at each pair of elements below, select (circle) which element has the higher electronegativity: O or Se P or Mg N or F 2 points 9-10) Complete the following problems for Magnesium and Phosphorus 5 points Magnesium (Neutral ) e-= 12 112__ Ve- =__2_ __ P+ =_12_ 2 8 2 12 Ve- =_5__ __ e- _15_ P+ =_15_ 2 8 5 12 .Mg . Mg 2+ Magnesium 2+ e-= 10 __ Ve- =_8__ __ P+ = 12__ What must be done to make this atom stable? 3 Phosphorus (Neutral) New Ion Symbol Lewis Structure 12 Lose two electrons New Ion Symbol Lewis Structure .. P.. . P 3- 3 3- Phosphorus Ve- =_8__ __ e-=18_ P+ =_15_ What must be done to make this atom stable? 3 2 8 2 8 8 12 Gain three electrons 3 (A stable atom or ion must have a full valence shell = 8 valence e-) Identify each as either ionic or covalent compounds and provide either the name or formula 5 points You may find these prefixes helpful for the questions below mono- di- tri- tetra- penta hexa- hepta octa- nona- deca- 1 2 3 4 5 6 7 8 9 10 Ionic or Covalent Covalent (remember only covalent compounds have the prefixes above) Ionic Magnesium Fluoride 13) phosphorus trifluoride Covalent PF3 14) sulfur dioxide Covalent SO2 15) N2O5 Covalent Dinitrogen Pentoxide Ionic Ca(NO3)2 Covalent Carbon Monoxide 18) lead (IV) oxide Ionic PbO2 19) FeSO4 Ionic Iron (II) Sulfate 11) dinitrogen trioxide 12) MgF2 16) calcium nitrate 17) CO Name or Formula N2O3 For the following questions, put your answer in the box ___ at the beginning of the question. NOTE: There are no questions like these on the test, but make sure you understand this for other questions. 20) _7a_ Which group of elements in the periodic table is known as the halogens? 21) _4 _ Use the periodic table to determine the number of electrons in a neutral atom of beryllium. 22) _35_ Use the periodic table to determine the number of protons in an atom of bromine. 23) _13_ What is the mass number for a carbon atom that has 7 neutrons in its nucleus? Moving from left-to-right across a period (row) of the periodic table, 24) TRUE or FALSE - the ionization energy of the elements generally decreases 25) TRUE or FALSE - the atomic radius of the elements generally decreases NOTE: There are only 10 multiple choice questions on the test – MOST are SIMILAR to these questions below _D__ 26) Which of the following is true about subatomic particles? a. Electrons have no charge and have almost no mass. b. Protons are negatively charged and the lightest subatomic particle. c. Neutrons have a negative charge and are the lightest subatomic particle. d. Electrons have almost no mass compared to the protons _A__ 27) All atoms are ____. a. neutral, with the number of protons equaling the number of electrons b. neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons c. positively charged, with the number of protons exceeding the number of electrons d. negatively charged, with the number of electrons exceeding the number of protons _B__ 28) The nucleus of all atoms ____. a. always has the same number of neutrons and is considered neutral b. are positively charged because of the positive charge of the protons c. are negatively charged because of the negative charge of the neutrons d. are positively charged and it occupies the vast majority of the volume of the atom. _B__ 29) The sum of the protons and electrons in an atom equals the ____. a. atomic number b. charge of the atom c. atomic mass d. mass number _A__ 30) Isotopes of the same element have different ____. a. numbers of neutrons b. numbers of protons c. numbers of electrons _B__ 31) All atoms of the same element have the same ____. a. number of neutrons b. number of protons c. mass numbers d. atomic numbers d. mass _D__ 32) Which of the following elements is in the same period as krypton? a. helium b. magnesium c. nitrogen d. bromine _B__ 33) Of the elements Fr, Sb, Al, and Rn, which is a metalloid? a. Fr b. Sb c. Al d. Rn _A__ 34) Which of the following statements is NOT true? a. Atoms of the same element must always have the same mass b. Atoms of isotopes of an element have different numbers of neutrons. c. The nucleus of an atom has a positive charge. d. Atoms are mostly empty space. _B__ 35) Which of the following particles are free to drift in metals? a. protons b. electrons c. neutrons d. cations (the electrostatic force is between the e- and the cations) _C__ 36) Which of the following pairs of elements is most likely to form an ionic compound? a. chlorine and oxygen c. aluminum and chlorine (ionic is metal and nonmetal) b. nitrogen and sulfur d. sodium and lithium _A__ 37) What characteristic of metals makes them good electrical conductors? (electricity is a flow of charge) a. They have mobile valence electrons. c. They have mobile cations. b. They have mobile protons. d. Their crystal structures can be rearranged easily. _C__ 38) Which of these elements does not exist as a diatomic molecule? a. H b. F c. Ar d. O (Argon is a noble gas and is stable- will not bond) _C__ 39) How do atoms achieve noble-gas electron configurations in double covalent bonds? a. Two atoms share one electron. c. Two atoms share two pairs of electrons. (one bond = 2 e-) b. Two atoms share two electrons. d. One atom completely loses two electrons to the other atom. _D__ 40) When Group 6A elements form ions, they ____. (6A elements have six valence electrons) a. lose two protons b. gain two protons c. lose two electrons d. gain two electrons _A__ 41) Which of the following is true about the composition of ionic compounds? a. They are composed of anions and cations. c. They are composed of cations only. b. They are composed of anions only. d. They are formed from two or more nonmetallic elements. _A__ 42) Which element, when combined with bromine, would most likely form an ionic compound? a. lithium b. carbon c. phosphorus d. chlorine (Ionic = metal (lithium) and a nonmetal (bromine)) _A__ 43) Which of the following occurs in an ionic bond? (electrostatic forces between charged ions) a. Oppositely charged ions attract. c. Two atoms share more than two electrons. b. Two atoms share two electrons. d. Like-charged ions attract. _A__ 44) Which of the following pairs of elements is most likely to form an ionic compound? a. magnesium and fluorine c. oxygen and chlorine (ionic = metal and nonmetal) b. nitrogen and sulfur d. sodium and aluminum _A__ 45) A bond formed between a calcium atom and an oxygen atom is likely to be ____. a. ionic b. coordinate covalent c. polar covalent d. nonpolar covalent (Ionic = metal (calcium) and nonmetal (oxygen)) _A__ 46) Which of the following covalent bonds is the most polar? (more polar = larger difference in EN) a. H—F b. H—C c. H—H d. H—N (Fluorine has the highest Electronegativity (EN)) _C__ 47) Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen? a. C b. Na c. O d. S (Oxygen has the highest electronegativity (EN)) _B__ 48) Which of the forces of molecular attraction is the weakest? (dispersion is just from the moving e-) a. dipole interaction b. dispersion c. hydrogen bond d. single covalent bond 49) Compare and Contrast Ionic and covalent bonds. 3 points Both allow for stable atoms or ions. They both involve electrons. They are both electrostatic forces between opposite charges. Both may involve nonmetals. a) how are they similar? b) how are they different? Ionic ~ transferring electrons ~ metal & nonmetal ~ attraction between ions Covalent ~ sharing electrons ~ two nonmetals ~ attraction between neutral atoms and the electrons between them. 105) Complete the Lewis Structures for each Compound (there will be two of these) 4 points Cl2 ____________ C2H4 ___________ N2 ____________ Cl – Cl (single bond) N N (triple bond) (NOTE: I will provide you with a copy of the electronegativities of the atoms) Identify each of the Bond Types as either: Nonpolar Covalent, Polar Covalent, or Ionic (Do not forget to include the identification of cations and anions or partial positive and partial negative where appropriate.) (for ionic) (for polar covalent) 4 points 51) HO H 2.2 O 3.5 ΔEN = 52) NaI 1.3 Na 0.9 Polar Covalent 53) HC H 2.2 C 2.5 F 4.0 O 3.5 I 2.5 - ΔEN = 1.6 Ionic ΔEN = 54) H-H 0.3 H 2.2 H 2.2 ΔEN = 0.0 Nonpolar Covalent Nonpolar Covalent 55) FO + ΔEN = 0.5 Polar Covalent 56) HN H 2.2 N 3.0 ΔEN = 0.8 Polar Covalent Identify each of the following as either intermolecular or intramolecular 2 points 57) _ intramolecular__ Polar Covalent Bond 60) _ intramolecular__ Ionic Bond 58) _ intermolecular__ Hydrogen Bond 61) _ intermolecular__ Dipole-Dipole Interact 59) _ intermolecular__ London Dispersion 62) _ intermolecular__ Van der Waals Intramolecular = between Atoms intermolecular = between molecules 63) Explain “why” atoms become partially positive and partially negative in a polar bond. 2 points In a polar bond, the difference between the electronegativities between the two non-metals is greater than 0.4, this difference will result in the shared electrons not being shared equally. This unequal sharing will cause the electrons to move closer to the atom with the higher electronegativity. The negatively charged electrons will result in this higher electronegative atom becoming partial negative, and the other atom becoming partial positive. 1 m3 = 1,000 L 1 mL = 1 cm3 1 inch = 2.54 cm 1 mile = 5280 ft 1 Atm = 101.3 kPa = 760 mmHg = 14.7 PSI 1 km = 1,000 m 1 m = 100 cm = 1,000 mm 1 kg = 1,000 g 1 g = 100 cg = 1,000 mg 1 kL = 1,000 L 1 L = 100 cL = 1,000 mL 1 lb = 454 grams 1oz = 28.35 g 1 lb = 16 oz 1 quart = 0.95 L 1 gallon = 4 quarts 1 quart = 2 pints 1 pint = 2 cups 1 cup = 8 oz. (fl) Perform the following conversions: (Show your work to earn partial credit) Missing units = loss of credit NOTE: There will be five problems like those below (64-71) 64) 147.2 kPa = ____ mmHg x 760 mmHg 101.3 kPa 65) 3.4 Atm = ____ kPa x 101.3 kPa 1 Atm 66) 894.2 cm = ____ km x 1m . 100 cm 67) 287,520 mg = ____ kg x 1g . 1000 mg 68) 97 mL to gallons x 1L . 1,000 mL 69) 133.5 mm to inches x 100 cm . 1,000 mm = 344 kPa x x x = 1104 mmHg x 1 km . 1,000 m = 0.008942 km 1 kg . 1,000 g 1 qt . 0.95 L x = 0.28752 kg 1 gal 4 qt 1 in . 2.54 cm = 0.0255 gallons = 5.256 inches NOTE: You will need to know Avagadro’s Number for the following two questions 70) How many atoms of platinum are in the 4.2 g ring? (From Periodic Table: 1 mole Pt = 195.08 g Pt) 4.2 g x 1 mole . 195.08 g x 6.022 x 1023 atoms 1 mole = 1.3 x 1022 atoms of platinum 71) If there are 5.45 x 1025 atoms of aluminum (Al), how many grams would this be? (1 mole = 26.98g) 5.45 x 1025 atoms x 1 mole . 6.022 x 1023 atoms x 26.98 g . 1 mole = 2442 grams of aluminum 4points 72) TRUE or FALSE: The motion/speed of the particles increases as the temperature of particles decreases. 73) TRUE or FALSE: Because the shape of a solid never changes, the particles of the solid do not move. 74) TRUE or FALSE: Particles can stick together because of the intermolecular forces between the particles. 75-78) Balance the following equations 2 points [3] C + [ 4] H2 [ 1] C3H8 [4] NaI + [1] Pb(SO4)2 [2] Fe(OH)3 [1] Fe2O3 + [3] H2O [1] PbI4 + [2] Na2SO4 [1] H3PO4 + [3] NaBr [3] HBr + [1] Na3PO4 3 points 79) Look at the equations in questions 75-78 above. List each chemical as either a reactant (R) or a product (P). C PbI4 Fe(OH)3 NaBr NaI H2O C3H8 H2 R Prod R R R Prod Prod R 80) How does the Law of Conservation of Mass relate to balancing chemical equations? 2 points The law of conservation of mass states that matter can not be created or destroyed. By balancing a chemical equation the number and type of atoms in the REACTANTS are the EXACT same number and type of atoms in the PRODUCTS. 81-85) Write balanced equations for the following word equations. Indicate the type of reaction on the line to the left of the equation by classifying each reaction as single replacement (SR), double replacement (DR), decomposition (D), synthesis (S), or combustion (C). (NO PHASE LABELS) 4 * 3 points each = 12 points _S_81) phosphorous + oxygen diphosphorous trioxide P + O2 P2O3 (No ions as it is a covalent compound) 4 P + 3 O2 2 P2O3 . 1 point for the type of reaction, 1 point for writing compounds with a net charge of zero, and 1 point for balancing _ DR 82) lithium nitride + barium nitrate lithium nitrate + barium nitride 1+ 32+ 1Li N + Ba NO3 Li1+ NO31+ Ba2+ N32 Li 3N + 3 Ba(NO3 )2 6 LiNO3 + 1 Ba3N2 _ DR 83) sodium bromide + Na1+ Br1+ 2 NaBr + . (make sure you write the names of the products) calcium hydroxide sodium hydroxide + calcium bromide . Ca2+ OH1 Na1+ OH1+ Ca2+ Br11 Ca(OH)2 2 NaOH + 1 CaBr2 _DR 84) Solutions of potassium chloride and silver nitrate are mixed to create solid silver chloride and aqueous potassium nitrate. K1+ Cl 1- + Ag1+ NO31- Ag1+ Cl 1- + K1+ NO31_1_ KCl (aq) + _1_ Ag NO3(aq) _1_ AgCl (s) + _1_ KNO3 (aq) _DR 85) Aqueous ammonium hydroxide reacts with aqueous copper (II) nitrate to produce solid copper (II) hydroxide and a solution of ammonium nitrate. NH41+ OH1- + CU2+ NO31 CU2+ OH1- + NH41+ NO31_2_ NH4OH (aq) + _1_ CU(NO3)2 (aq) _1_ CU(OH)2 (s) + _2_ NH4NO3 (aq) 86) List the seven diatomic elements. 2 points H2 N2 O2 F2 Cl2 Br2 I2 87) How did you know that a chemical reaction occurred when you added the magnesium metal to the solution of hydrochloric acid? 2 points Bubbling occurred, this bubbling was a release of a gas . The production of a gas is one source of evidence that a chemical reaction is occurring. 88) How many grams of lead (II) phosphate will be formed when 85.39 grams of phosphoric acid (H3PO4) react with an excess of lead metal in the following reaction? 5 points _3__ Pb + _2__ H3PO4 _3__ H2 + _1__ Pb3(PO4)2 MM = Pb3(PO4)2 = 3(207.2 g) + 2(30.97 g) + 8(16.00 g) = 811.54 g/mol Pb3(PO4)2 MM = H3PO4= 3(1.01 g) + 1(30.97 g) + 4(16.00 g) = 98.00 g/mol H3PO4 1 mol H3PO4 85.39 g H3PO4 1 mol Pb3(PO4)2 811.54 g Pb3(PO4)2 x ------------------ x ----------------- x -----------------98.00 g H3PO4 2 mol H3PO4 = 353.56 g Pb3(PO4)2 1 mol Pb3(PO4)2 5 points = 1 point for balancing, 2 points for molar masses, and 2 points for final mass (stoichiometry) 89) How many grams of hydrofluoric acid (HF) are required to react completely with 23.68 grams of calcium hydroxide in the following reaction? 5 points _1_ Ca(OH)2 + __2_ HF __1_ CaF2 + __2_H2O MM = HF = 1(1.01 g) + 1(19.00 g) = 20.01 g/mol HF MM = Ca(OH)2 = 1(40.08 g) + 2(16.00 g) + 2 (1.01 g) = 74.10 g/mol Ca(OH)2 1 mol Ca(OH)2 23.68 Ca(OH)2 2 mol HF 20.01 g HF x ------------------ x ----------------- x ------------------ = 12.79 g HF 74.10 g Ca(OH)2 1 mol Ca(OH)2 1 mol HF NOTE: There are eleven more points/questions that are based on reaction rates Final Exam is six pages and has 60 question: 109 points possible = 100 points + 9 Extra Credit You are allowed to use TWO index cards (BOTH SIDES) or ONE SIDE of a piece of paper: a) TWO index cards (front and back) OR b) ONE piece of standard sized typing paper (only ONE SIDE of the paper) Similar to all of my tests and quizzes, the questions on your FINAL EXAM will be similar to these provided on this practice test. I recommend that you look over your old tests, old practice tests, old quizzes, old notes, old homework assignments… to help you prepare for the final exam. I am almost always available for questions.