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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 Standard Form Scientific Notation 0.005300 cm 2.68023 x 102 kg 6.71 x 10-4 L 1993 mL 0.0000072 kg 2) Use <, >, or = for each of the questions below. 3 points a) 9.8 m ___ 9800 km b) 1 mL ___ 0.010 cL c) 3.5 g ___ .0035 kg 3) Complete the table below – Note that the particles are not is the same order: 3 points Charge Location AMU Neutron Electron Proton 4) Draw the Lewis Structures for the following neutral atoms. 3 points C F Si He Ga Ba 5) 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 ________ is an example of metal ________ is an example of a nonmetal ________ is an example of a metalloid ________ has 6 total electrons ________ has 6 valence electrons ________ has 1 valence electrons ________ is an Alkaline Earth Metal ________ is a Nobel Gas. ________ is a Halogen ________ is an Alkali Metal 6) 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 7) 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 8) 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- = __ Ve- =___ __ P+ =__ 12 e- = __ Ve- =___ __ P+ =__ 12 3 e- = __ P+ =__ 12 Magnesium What must be done to make this atom stable? Phosphorus (Neutral) Ve- =___ __ New Ion Symbol Lewis Structure New Ion Symbol Lewis Structure 3 Phosphorus Ve- =___ __ e- = __ P+ =__ What must be done to make this atom stable? 12 3 3 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 Ionic or Covalent mono- di- tri- tetra- penta hexa- hepta octa- nona- deca- 1 2 3 4 5 6 7 8 9 10 Name or Formula 11) dinitrogen trioxide 12) MgF2 13) phosphorus trifluoride 14) sulfur dioxide 15) N2O5 16) calcium nitrate 17) CO 18) lead (IV) oxide 19) FeSO4 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) ___ Which group of elements in the periodic table is known as the halogens? 21) ___ Use the periodic table to determine the number of electrons in a neutral atom of beryllium. 22) ___ Use the periodic table to determine the number of protons in an atom of bromine. 23) ___ 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 _____ 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 _____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 _____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. _____ 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 _____ 30) Isotopes of the same element have different ____. a. numbers of neutrons b. numbers of protons c. numbers of electrons _____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 _____ 32) Which of the following elements is in the same period as krypton? a. helium b. magnesium c. nitrogen d. bromine _____ 33) Of the elements Fr, Sb, Al, and Rn, which is a metalloid? a. Fr b. Sb c. Al d. Rn _____ 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 ____ 35) Which of the following particles are free to drift in metals? a. protons b. electrons c. neutrons d. cations ____ 36) Which of the following pairs of elements is most likely to form an ionic compound? a. chlorine and oxygen c. aluminum and chlorine b. nitrogen and sulfur d. sodium and lithium ____ 37) What characteristic of metals makes them good electrical conductors? a. They have mobile valence electrons. c. They have mobile cations. b. They have mobile protons. d. Their crystal structures can be rearranged easily. ____ 38) Which of these elements does not exist as a diatomic molecule? a. H b. F c. Ar d. O ____ 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. b. Two atoms share two electrons. d. One atom completely loses two electrons to the other atom. ____ 40) When Group 6A elements form ions, they ____. a. lose two protons b. gain two protons c. lose two electrons d. gain two electrons ____ 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. ____ 42) Which element, when combined with bromine, would most likely form an ionic compound? a. lithium b. carbon c. phosphorus d. chlorine ____ 43) Which of the following occurs in an ionic bond? a. Oppositely charged ions attract. c. Two atoms share more than two electrons. b. Two atoms share two electrons. d. Like-charged ions attract. ____ 44) Which of the following pairs of elements is most likely to form an ionic compound? a. magnesium and fluorine c. oxygen and chlorine b. nitrogen and sulfur d. sodium and aluminum ____ 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 ____ 46) Which of the following covalent bonds is the most polar? a. H—F b. H—C c. H—H d. H—N ____ 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 ____ 48) Which of the forces of molecular attraction is the weakest? a. dipole interaction b. dispersion c. hydrogen bond 49) Compare and Contrast Ionic and covalent bonds. 3 points a) how are they similar? b) how are they different? d. single covalent bond 50) Complete the Lewis Structures for each Compound (there will be two of these) 4 points Cl2 ____________ C2H4 ___________ N3 ____________ (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.) 4 points 51) HO H O ΔEN = 52) NaI Na I ΔEN = 53) HC H C ΔEN = 54) H-H H H ΔEN = 55) FO F O ΔEN = 56) HN H N ΔEN = Identify each of the following as either intermolecular or intramolecular 2 points 57) _____________ Polar Covalent Bond 60) _____________ Ionic Bond 58) _____________ Hydrogen Bond 61) _____________ Dipole-Dipole Interact 59) _____________ London Dispersion 62) _____________ Van der Waals 63) Explain “why” atoms become partially positive and partially negative in a polar bond. 2 points 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 m3 = 1,000 L 1 mL = 1 cm3 1 inch = 2.54 cm 1 mile = 5280 ft 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 65) 3.4 Atm = ____ kPa 66) 894.2 cm = ____ km 67) 287,520 mg = ____ kg 68) 97 mL to gallons 69) 133.5 mm to 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? 71) If there are 5.45 x 1025 atoms of aluminum (Al), how many grams would this be? 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 [ ] C + [ ] H2 [ ] C3H8 [ ] NaI + [ ] Pb(SO4)2 [ ] Fe(OH)3 [ ] Fe2O3 + [ ] H2O [ ] PbI4 + [ ] Na2SO4 [ ] H3PO4 + [ ] NaBr [ ] HBr + [ ] 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 80) How does the Law of Conservation of Mass relate to balancing chemical equations? 2 points 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 ____81) phosphorous + oxygen diphosphorous trioxide ____ 82) lithium nitride + barium nitrate ____ 83) sodium bromide + lithium nitrate + barium nitride calcium hydroxide ______________________________________. ____ 84) Solutions of potassium chloride and silver nitrate are mixed to create solid silver chloride and aqueous potassium nitrate. ____ 85) Aqueous ammonium hydroxide reacts with aqueous copper (II) nitrate to produce solid copper (II) hydroxide and a solution of ammonium nitrate. . . 86) List the seven diatomic elements. 2 points 87) How did you know that a chemical reaction occurred when you added the magnesium metal to the solution of hydrochloric acid? 2 points 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 ____ Pb + ____ H3PO4 ____ H2 + ____ Pb3(PO4)2 MM = MM = x ------------------ x ----------------- x ------------------ = 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 ____ Ca(OH)2 + ____ HF ____ CaF2 + ____H2O MM = MM = x ------------------ x ----------------- x ------------------ = 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.