Final Exam Review HonorsName_________________________

Short Answer- Zushma Date _________________________

Answer all these questions as completely as possible and make sure to look up any information you are unsure of! The questions go in chapter order…

1) You record the following in your lab book: A liquid is thick and has a density of 4.58 g/mL. Which data is qualitative? Which data is quantitative?

2) Express the following in scientific notation:a) 34500______________________b) 2665 _______________________c) 0.9640 ______________________d) 789 _________________________e) 75600 _______________________f) 0.002189 _____________________

3) Convert 65ºC to Kelvins. ________________________________________4) Classify the following mixtures as heterogeneous or homogeneous.

a) salt water___________________________b) vegetable soup_____________________________b) 14- K gold_________________________________c) Concrete __________________________________

5) Are the following changes physical or chemical?a) water boils _______________________________b) a match burns _____________________________c) sugar dissolves in water _________________________________d) sodium reacts with water ________________________________e) ice cream melts ____________________________

6) Round 20.56120 g to three significant figures. _________________________________7) Identify each of the following as either chemical or physical properties of a substance:

a) mercury is a liquid at room temperature ______________________________b) sucrose is a white crystalline solid ___________________________________c) iron rusts when exposed to moist air _________________________________d) paper burns when ignited __________________________________________

8) Identify each of the following as a pure substance or a mixture:

a) distilled water ___________________________________________b) orange juice with pulp ____________________________________c) smog __________________________________________________d) diamond ________________________________________________e) milk ____________________________________________________f) copper metal _____________________________________________

9) Convert the following measurements as indicated (show OUR work):a) 1.1 cm to meters

b) 76.2 pm to mm

c) 11 Mg to kg

d) 7.23 micrograms to kg

10) Determine the correct number of significant figures in each of the following: a) 708.4 mL ___________________________________________b) 1.0050 g _____________________________________________c) 1.000 mg _____________________________________________d) 6.626 * 10-34 s _________________________________________

11) A quarter has a mass of 5.627 g. What is its mass in milligrams?

12) A solution of sugar has a density of 1.05 g/mL. If you have 300 ml of sugar solution, what is the mass of your solution?

13) A substance is said to be volatile if it readily changes from a liquid to a gas at room temperature. Is his a physical change or a chemical change?

14) You are given a liquid of unknown density. The mass of a graduated cylinder containing 2.00 mL of a liquid is 34.68 g. The mass of the empty graduated cylinder is 30.00 g. What is the density of the liquid?

15) Distinguish among a mixture, a solution, and a compound.

16) Identify the following as an element, compound, homogeneous mixture, or heterogeneous mixture:

a) Air _________________________________________b) Salt _______________________________________c) Antimony ____________________________________d) Brass ________________________________________e) Ammonia _____________________________________f) Yellow Mustard ____________________________________g) Tap Water ________________________________________h) Tin __________________________________________

17) An atom of gadolinium has an atomic number of 64 and a mass number of 153 How many electrons, protons and neutrons does it contain?

18) What element has the ground state electron configuration of [Ar] 4s2 3d6?

19) How many electrons, protons and neutrons are there in the following:

a) carbon 13 __________________________________________________________b) chromium 50 _______________________________________________________c) tin 119 ____________________________________________________________

20) Identify which of the following orbitals cannot exist according to quantum theory: 4s, 1p, 3f, 2d. Briefly explain your answer.

21) Distinguish between atomic number and mass number. How do these two numbers compare for isotopes of an element?

22) Write the electron configuration for each of the following atoms:a) fluorine

b) aluminum

c) titanium

d) radon

23) Phosphorus has the atomic number 15 and an atomic mass of 31 amu. How many protons, neutrons and electrons are in a neutral phosphorus atom?

24) Mendeleev left a space on his periodic table for the undiscovered element germanium and in 1886 Winkler discovered it. Write the electron configuration for germanium.

25) Select the atom or ion in each pair that has the larger (atomic or ionic) radius:

a) Cs or Fr

b) Br or As

c) O-2 or O

26) Arrange the following in order of increasing ionization energy: Li, C, Si, Ne.

27) Arrange the following in order of increasing electronegativity: K, Ca, Fr, Mg.

28) Which element has the greater atomic radius: chlorine or carbon? Why?

29) Compare and contrast the way metals and nonmetals form ions and explain why they are different.

30) What are transition elements?

31) Write the symbol and name of the element that fits each description:

a) the second lightest of the halogens ______________________________b) the metalloid with the lowest period number ______________________c) the only group 6A element that is a gas at room temperature

__________________________d) the heaviest of the noble gases _________________________________

32) Write the correct chemical formula or name the following compounds:a) NaI _____________________________________________b) Calcium Carbonate ________________________________c) Fe(NO3)3 _________________________________________d) Sr(OH)2 __________________________________________e) Potassium Chlorate __________________________________f) Copper (II) Sulfate __________________________________g) CoCl2_____________________________________________h) Ammonium Phosphate _______________________________i) Silver Acetate ______________________________________j) Mg(Br)2 __________________________________________

33) Write the formula for the compounds made from each of the following pairs of ions:

a) copper (I) and sulfite ____________________________________________b) tin (IV) and fluoride ____________________________________________c) gold (III) and cyanide ___________________________________________d) lead (II) and sulfide _____________________________________________

34) You are given two clear, colorless aqueous solutions. You are told that one solution contains an ionic compound and one contains a covalent compound. How could you determine which is an ionic and which is a covalent solution?

35) Name the following compounds:a) NaBr _______________________________________________b) Pb(NO3)2 _______________________________________

c) (NH4)2CO3 __________________________________________

36) Identify if the following are polar or nonpolar: (you must draw Lewis structures first)a) SiH4

b) NO2+

c) H2S

d) NCl3

37) Name the following molecular compounds:

a) S2Cl2 __________________________________________________b) CS2 ____________________________________________________c) SO3 ____________________________________________________d) P4O10 __________________________________________________

38) Write the balanced chemical equation for the following reactions:

a) solid barium and oxygen gas react to produce solid barium oxide

b) aqueous carbonic acid reacts to produce liquid water and gaseous carbon dioxide

c) Calcium carbonate decomposes to produce calcium oxide and carbon dioxide

d) solid copper (II) sulfide reacts with aqueous sodium chloride to produce aqueous copper (II) chloride and aqueous sodium sulfide.

39) Write a complete and net ionic equation for the following: aqueous solutions of copper (I) nitrate and potassium sulfide are mixed to form insoluble copper (I) sulfide and one other aqueous product.

40) Calculate the molar mass of phosphoric acid. (first you have to find the formula of an acid!)

41) Calculate the mass of 42.5 mole of potassium cyanide.

42) Calculate the number of moles in 5.67g potassium hydroxide.

43) What mass of sodium hydroxide contains 4.58 * 1023 atoms?

44) A colorless liquid was found to contain 39.12%C, 8.76%H and 52.12%O. Determine the empirical formula of the substance.

45) When 25g of a hydrate of nickel (II) chloride was heated, 11.37g of water was released. Determine the name and formula of the hydrate.

46) Write and balance the equation for the formation of magnesium hydroxide and hydrogen from water and magnesium. 47) Given the following equation: 2SO2 + 2H2O + O2 → 2H2SO4. Determine the mass of sulfuric acid formed from 3.2 moles of sulfur dioxide.

48) Given the following equation: Cl2 + C6H6 → C6H5Cl + HCl. Determine the limiting reactant if 45g of benzene reacts with 45 g of chlorine. Determine the mass of hydrochloric acid produced.

49) Tin (IV) iodide is prepared by reacting tin with iodine. Write the balanced chemical equation for the reaction. Determine the theoretical yield if a 5g sample of tin reacts in an excess of iodine. Determine the percent yield if the experimental yield is 28g of SnI4.

50) The volume of a sample of hydrogen gas at 0.997atm is 5L. What will be the new volume if the pressure is decreased to 0.956atm?

51) A gas at 55ºC occupies a volume of 3.6L. What volume will it occupy at 30ºC?

52) The pressure in a bicycle tire is 1.34atm at 33ºC. At what temperature will the pressure inside the tire be 1.6atm?

53) How many moles of air are in 6.06L tire at STP?

54) Calculate the mass of hydrogen peroxide needed to obtain 0.46L of oxygen gas at STP using the following equation: 2H2O2 → 2H2O + O2.

55) Given the following phase diagram of carbon dioxide:

a) What is the triple point? _____________________________b) What is the critical point? ____________________________c) At 10atm what is the melting point? ____________________d) At 10atm what is the boiling point? ____________________

56) What is the molarity of the following solutions?a) 0.96g MgCl2 in 500 mL of solution

b) 9.33g Na2S in 450 mL solution

c) 2.48g CaF2 in 375mL of solution

57) Calculate the molality of 34.2g NaOH in 845.4g H2O.

58) Calculate the pH of solutions having the following ion concentrations at 298K:a) [H+] = 1 * 10-2M

b) [OH-] = 8.2 * 10-6M

59) Calculate the [H+] and [OH-] from the following pH:

a) pH = 11.05

b) pH = 2.37

60) A solution of 0.6M HCl is used to titrate 15ml of KOH solution. The endpoint of the titration is reached after the addition of 27.13mL. What is the concentration of the KOH solution?

61) Determine the oxidation number of the bold element in each of the following examples:

a. OF2 ___________________________b. Fe2O3 _________________________c. RuO4 __________________________d. UO2+2 _________________

62) Is the following reaction an example of a redox reaction? Why or why not? LiOH + HNO3 → LiNO3 + H2O

63) Write the half reactions and balance the following redox equation: Al + I2 → Al+3 + I-

Final Exam Review Multiple Choice- ZushmaAnswer the following multiple choice questions with the BEST answer available. You might want to make notes to help yourself study!

1) Matter is defined as anything that_________a. Exists in natureb. Is solid to the touchc. Is found in the universed. Has mass and takes up space

2) Which of the following is NOT equivalent to the others?a. 500 meters

b. 0.5 kilometersc. 5000 centimetersd. 5 * 1011 nanometers

3) The correct representation of 702.0g using scientific notation is __________?a. 7.02 * 103 gb. 70.20 * 101 gc. 7.020 * 102 gd. 70.20 * 102 g

4) How many significant figures are there in a distance measurement of 20.070km?a. 2b. 3c. 4d. 5

5) All of the following are physical properties of table sugar (sucrose) EXCEPT ___?a. Forms solid crystals at room temperatureb. Appears as white crystalsc. Breaks down into carbon and water vapor when heatedd. Tastes sweet

6) Which is a chemical change?a. evaporating alcoholb. melting ice cubesc. burning butterd. forming fog

7) Which statement describes a chemical property of bromine?a. bromine is soluble in waterb. bromine has a reddish brown colorc. bromine combines with aluminum to produce AlBr3d. bromine changes from a liquid to a gas at 332K and 1 atm

8) Which is a mixture?a. HCl (aq)b. NaCl (s)c. O2 (g)d. H2O (l)

9) A sample of material which has a definite shape but no definite volume is:a. a solidb. a gasc. a liquidd. does not exist

10) Na, K, Li, and Cs all share very similar chemical properties. In the periodic table of elements, they most likely belong to the same __________?

a. Rowb. Period

c. Groupd. Element

11) Which substance can not be decomposed by a chemical change?a. ammoniab. copperc. propanold. water

12) The percent by mass of sulfur in sulfuric acid, H2SO4, is ____?a. 32.69%b. 64.13%c. 16.31%d. 48.57%

13) Which of the following is not a chemical reaction?a. Dissolving of sodium chloride in waterb. Combustion of gasolinec. Fading of wallpaper by sunlightd. Curdling of milk

14) Neptunium’s only naturally occurring isotope, 23793Np, decays by alpha radiation. What is the new atom formed by this decay?

a. 23392Ub. 23390Thc. 23391Pad. 24193Np

15) 12652Te has ___________ a. 126 neutrons, 52 protons, and 52 electrons b. 74 neutrons, 52 protons, 52 electrons c. 52 neutrons, 74 protons, 74 electrons d. 52 neutrons, 126 protons, 126 electrons

16) The hypothetical element X has these isotopes:Isotope Mass Abundanc

e40X 39.997 30.1%45X 44.995 69.9%

What is the average atomic mass of element X?a. 45 amub. 42.5 amuc. 43.5 amud. 40.0 amu

17) In an atom of argon-40, the number of protons:a. equals the number of electronsb. equals the number of neutronsc. is less than the number of electronsd. is greater than the number of electrons

18) The volume of an atom is made up mostly of __________

a. Protonsb. Neutronsc. Electronsd. Empty space

19) Assume the following three isotopes of Q exist: 248Q, 252Q and 259Q. If the atomic mass of Q is 258.63 which of its isotopes is the most abundant?

a. 248 Qb. 252 Qc. 259 Qd. They are equally abundant

20) The element that has the ground state electron configuration [Xe] 6s24f145d6 is ____?

a. Lab. Tic. Wd. Os

21) An atom of aluminum in the ground state and an atom of gallium in the ground state have the same:

a. massb. electronegativityc. total number of protonsd. total number of valence electrons

22) Periodic law states that elements show a _______?a. Repetition of their physical properties when arranged by increasing atomic numberb. Repetition of their chemical properties when arranged by increasing atomic numberc. Periodic repetition of their properties when arranged by increasing atomic numberd. Periodic repetition of their properties when arranged by increasing atomic mass

23) Elements in the same group of the periodic table have the same ____?a. Number of valence electronsb. Physical propertiesc. Number of electronsd. Electron configuration

24) An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of t he atom:

a. absorbing energyb. releasing energyc. gaining an electrond. losing an electron

25) Moving down a group on the periodic table, which two atomic properties follow the same trend?

a. atomic radius and ionization energyb. ionic radius and atomic radiusc. ionization energy and electronegativityd. ionic radius and electronegativity

26) Niobium (Nb) is a(n) ____?a. nonmetalb. transition metalc. alkali metald. halogen

27) It can be predicted that element 118 would have properties similar to a(n) ___?a. alkali earth metalb. halogenc. metalloidd. noble gas

28) Yttrium, a metallic element with atomic number 39, will form___?a. positive ionsb. negative ionsc. both positive and negative ionsd. no ions at all

29) What is the correct chemical formula for the ionic compound formed by the calcium ion and the fluoride ion?

a. CaF2b. CaF8c. (Ca)2Fd. CaF

30) What is the correct name for the compound with the formula RbNO3?a. rubidium nitrogen oxideb. rubidium nitride trioxidec. rubidium nitrated. rubidium nitrite

31) What is the formula for diarsenic trioxide?a. As2(O2)3b. As2O3c. As3(O2)2d. As3O2

32) The anion in AlPO4 has a charge of _____?a. +2b. +3c. -2d. -3

33) The common name of SiI4 is tetraiodosilane. What is the molecular compound name?

a. silane tetraiodideb. silane tetraiodinec. silicon iodided. silicon tetraiodide

34) Which represents a molecular compound?a. HIb. KIc. KCld. LiCl

35) Which is the strongest type of intermolecular force?a. ionic bondb. dipole-dipole forcec. dispersion forced. hydrogen bond

36) All of the following compounds have bent molecular shapes except___? (Draw these)

a. BeH2b. H2Sc. H2Od. SeH2

37) Which of the following is not polar? (Draw these)a. H2Sb. CCl4c. SiH3Cld. AsH3

38) What is the formula of the missing product in this reaction? 2HNO3 + Mg(OH)2 → _____ + 2H2O

a. Mg3N2b. Mg(NO3)2c. MgNO3d. Mg(NO2)2

39) What type of reaction is described by the following equation?Cs(s) + (H2O) (l) → CsOH (aq) + H2(g)

a. synthesisb. combustionc. decompositiond. replacement

40) What is the product of this synthesis reaction? Cl2 + 2NO → ?a. NCl2b. 2NOClc. N2O2d. 2ClO

41) The combustion of ethanol, C2H6O, produces carbon dioxide and water vapor. The equation that best describes this process is_________?a. C2H6O + O2 → CO2 + H2Ob. C2H6O →2CO2 + 3H2Oc. C2H6O + 3O2 → 2CO2 + 3H2Od. C2H6O → 3O2 + 2CO2 + 3H2O

42) What is the coefficient for oxygen gas when the equation below is balanced?___ C2H5OH + __ O2 → __CO2 + __H2O

a. 1b. 3c. 5d. 7

43) If the experimental molar mass of butanoic acid is 88.1g/mol and the empirical formula is C2H4O, what is the molecular formula?a. CH2Ob. C2H4Oc. C6HO2d. C4H8O2

44) How many atoms are in 0.625 moles of Ge?a. 2.73 * 1025 atomsb. 6.99 * 1025 atomsc. 3.76 * 1023 atomsd. 9.63 * 1023 atoms

45) The molar mass of fluorapatite [Ca5(PO4)3F] is _______?a. 314 g/moleb. 344 g/molec. 442 g/moled. 504 g/mole

46) How many moles of cobalt (III) titanate (Co2TiO4) are in 7.13g of the compound?a. 2.39 * 101 moleb. 3.14 * 10-2 molec. 3.22 * 101 moled. 4.17 * 10-2 mole

47) Stoichiometry is based on the law of __?a. constant mole ratiosb. Avogadro’s constantc. Conservation of energyd. Conservation of mass

48) Magnesium sulfate is often added to water insoluble liquid products of chemical reactions to remove any unwanted water. Magnesium sulfate hydrate contains 13.0% water and 87.0% magnesium sulfate. What is the name of this hydrate? (This requires MATH!)a. magnesium sulfate monohydrateb. magnesium sulfate dihydratec. magnesium sulfate hexahydrated. magnesium sulfate heptahydrate

49) Na2CO3 + Ca(OH)2 → 2NaOH + CaCO3 The LeBlanc process shown above is the traditional method of making sodium hydroxide. If you have 500g of sodium carbonate how many moles of NaOH can you make?

a. 4.05 moles c. 8.097 molesb. 4.72 moles d. 9.43 moles

50) Water has an extremely high boiling point compared to other compounds of similar molar mass because:

a. Hydrogen bondingb. Adhesive forcesc. Covalent bondingd. Dispersion forces

51) The solid phase of a compound has a definite shape and volume because its particles _____.

a. Are not in constant motionb. Are always packed more tightly than particles in a compounds liquid phasec. Can only vibrate around fixed pointsd. Are held together by strong intermolecular forces

52) Which of the following does not affect the viscosity of a liquid?a. Intermolecular attractive forcesb. Size and shape of moleculesc. Temperature of liquidd. Capillary action

53) A sealed flask contains neon, argon, and krypton gas. The total pressure in the flask is 3.782 atm and the partial pressure of neon is 0.435 atm and krypton’s partial pressure is 1.613 atm. What is the partial pressure of argon?

a. 2.048 torrb. 1.734 torrc. 1556 torrd. 1318 torr

54) What volume will 0.875 moles of SF4 occupy at STP?a. 19.6 Lb. 21.4Lc. 22.4Ld. 32.7L

55) While it is on the ground a blimp is filled with 5.66 * 106L of He gas. The pressure inside the grounded

blimp, where the temperature is 25ºC, is 1.10atm. Modern blimps are non-rigid which means that their

volume is changeable. If the pressure inside the blimp remains the same what will the volume of the

blimp be at a height of 2300m where the temperature is 12ºC?a. 5.66 * 106 Lb. 2.72 * 106 Lc. 5.4 * 106 Ld. 5.92 * 106 L

56) The reaction that provides blowtorches with their intense flame is the combustion of acetylene (C2H2) to form carbon dioxide and water vapor. Assuming that the pressure and temperature of the reactants are the same, what volume of oxygen gas is required to completely burn 5.60L of acetylene? (Gas Stoichiometry!)

a. 2.24 Lb. 5.60 Lc. 11.2 Ld. 14.0 L

57) Assuming ideal behavior how much pressure will 0.0468g of ammonia (NH3) gas exerts on the walls of a 4L at 35ºC?

a. 0.0174 atmb. 0.296 atmc. 0.00198 atmd. 0.278 atm

58) How much water must be added to 6ml of a 0.05M stock solution to dilute it to 0.020M?

a. 15 mLb. 9.0 mLc. 6.0 mLd. 2.4 mL

59) What is the molality of solution containing 0.25g of dichlorobenzene (C6H4Cl2) dissolved in 10g of cyclohexane (C6H12)?

a. 0.17 mole/kgb. 0.014mole/kgc. 0.025 mole/kgd. 0.00017 mole/kg

60) All of the following are colligative properties except:a. boiling point elevationb. freezing point depressionc. vapor pressure increased. osmotic pressure

61) A carbonated soft drink has a pH of 2.5. What is the concentration of H+ ions in the soft drink?

a. 3 *10-12 Mb. 3 * 10-3 Mc. 4.0 * 10-1 Md. 1.1 * 101 M

62) Which of the following is not a characteristic of a base?a. bitter tasteb. ability to conduct electricityc. reactivity with some metalsd. slippery feel

63) A compound that accepts H+ ions is:a. an Arrhenius acidb. an Arrhenius basec. a Bronsted Lowry based. a Bronsted Lowry acid

64) Which of the following acids is the strongest?a. Formic acid (Ka = 1.78 *10-4)b. Cyanoacetic Acid (Ka= 3.55 * 10-3)c. Lutidinic Acid (Ka= 7.08 * 10-3)d. Barbituric Acid (Ka= 9.77 * 10-5)

65) The reducing agent in a redox reaction is all of the following except: ________________

a. The substance oxidizedb. The electron acceptorc. The reducer of another substanced. The electron donor

66) The reaction between sodium iodide and chlorine is shown 2NaI + Cl2 → 2NaCl + I2. The oxidation state of Na remains unchanged because:

a. Na+ is a spectator ionb. Na+ cannot be reducedc. Na is an uncombined elementd. Na+ is a monatomic ion

67) In HBr + H2O → H3O+ + Br-, the H2O is the:

a. Acidb. Basec. Conjugate acidd. Conjugate base

68) Which is the net ionic equation for the following reaction:SrCl2 (aq) + K2SO4 (aq) → SrSO4 (s) + 2KCl (aq)

a. SrCl2 (aq) + SO4-2 (aq) → SrSO4 (s) + 2Cl- (aq)b. Sr+2 (aq) + SO4-2 (aq) → SrSO4 (s)c. Cl2-(aq) + 2K+(aq) → 2KCl (aq)d. Cl-(aq) + K+(aq) → KCl(aq)

Final Exam Review True & False - Zushma

True-False: State whether each statement is true or false. If false, correct the statement so that it is a true statement.

1. Complete combustion has occurred when all the carbon in the product is in the form of carbon dioxide.

2. A single reactant is the identifying characteristic of a decomposition reaction.

3. The only way to determine the products of a reaction is to perform the reaction.

4. All chemical reactions can be classified as one of four general types.

5. With solutions of strong acids and strong bases, the word strong refers to Concentration.

6. A 12 M solution of an acid that is able to ionize completely in solution would be termed concentrated and weak

7. Bitter taste is a property of an acid.

8. Only bases are strong electrolytes

9. A solution which has [H+] of 1.0 x 10-7 M is strongly acidic.

10. A solution that turns red litmus blue is strongly basic.

11. [H+] = 2.0 x 10-7M is an acidic solution

12. [OH-] = 1.0 x 10-8M is a neutral solution.

13. Mg (OH) 2 is an Arrhenius base.

14. NH3 is an Arrhenius base

15. H2CO3 is triprotic

16. In the reaction, HCl + H2O (aq) ↔ Cl- (aq) + H3O+ (aq), H2O is acting as a Bronsted-Lowry acid

17. NH3 + H2O ↔ NH4+ + OH- is a Brønsted-Lowry acid-base reaction.