Honors Final Exam Review Name: ___________________________________Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must answer every questions in order to receive the bonus points. All answer must be hand written and you MUST show ALL work.

UNIT 1 and 2: Chemical Math, Matter, Energy, Lab Safety1. Study the lab safety rules.2. Know what the following glass wear is and what it is used for: beaker, graduated cylinder, watch plate,

evaporating dish, Erlenmeyer flask. 3. Describe the proper way to smell an unknown chemical in lab. 4. What is chemistry? 5. What is qualitative data?6. What is quantitative data?7. What are the SI base units for mass, length, and volume?8. How does one determine the number of significant digits in a number? 9. How many sig figs are in each of the following?

a. 0.000343 d. 0.000030340 b. 34030000 e. 3200 c. 3200.0 f. 32.002

10. What is precision?11. What is accuracy? 12. Model each of the following on a bull’s eye target:

a. Accurate and Preciseb. Accurate and NOT precisec. Precise but NOT accurated. Neither precise nor accurate

13. Convert the following using dimensional analysis: a. 5000cm km c. 32304 mL DL b. 8324 cg g d. 325.6 dm Dm

14. Convert the following using dimensional analysis: a. 19.0 ft into miles b. 37 hours into days c. 4.23 cm into inches

15. What is a physical property?16. Give 4 examples of physical properties.17. What is a chemical property?18. Give 3 examples of chemical properties.19. What is a physical change?20. How do you know if a physical change has occurred?21. What is a chemical change?22. How do you know if a chemical change has occurred?23. Label the following as chemical or physical change.

a. Silver tarnishing b. Ice melting c. Evaporating water from a salt water solution d. Burning e. Rusting f. Cutting

24. What are the six phase changes of matter?25. Define each phase change of matter. 26. Define temperature.

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Honors Final Exam Review Name: ___________________________________27. Define element.28. Define compound.29. Define mixture.30. What is the difference between a compound and a mixture?31. Label each of the following as element, compound, or mixture:

a. Water f. salad dressingb. Liquid bromine h. carbon dioxidec. Carbon i. Kool-Aidd. Salt water j. Gatorade

32. What is the formula for density? 33. What are the units of density?

UNIT 3: The Periodic Table34. Be able to label the following on a periodic table: Families/groups, periods, alkali metals, alkaline earth metals,

transition metals, halogens, noble gases, lanthanides, actinides, inner transition metals, metals, non-metals, metalloids, charges of families, valence electrons of families, elements that are liquid at room temperature, elements that are gases at room temperature

35. Write the long hand electron configuration, short hand electron configuration, and the orbital diagram for the following:

a. Magnesium d. Phosphorousb. Selenium e. Xenonc. Calcium f. Oxygen

36. List the 7 diatomic molecules.37. What element ends in 3p3?38. What element ends in 6s1?39. How many valance electrons are in the p orbital of Kr?40. How many valance electrons are in the s orbital of Rb?41. What is group 1? What are some characteristics of group 1?42. What is the possible charge of group 1?43. What is group 2? What are some characteristics of group 2?44. What is the charge on group 2?45. What are groups 3-12 called? And what are some characteristics of these groups?46. What is group 17 group 7A? What are some characteristics of group 7A?47. What is the charge on group 17?48. What is group 18/group 8A? What are some characteristics of group 8A?49. What are the two sections at the bottom of the periodic table called? 50. Where are the radioactive elements located on the periodic table?51. What is a cation?52. What is an anion?53. What is atomic radius?54. What are the group and periodic trends of atomic radius?55. What is ionization energy?56. What are the group and periodic trends of ionization energy?57. What is electronegativity?58. What are the group and periodic trends of electronegativity?59. What element has the highest electronegativity?60. What are metalloids?61. What is the law of conservation of mass?

UNIT 4: Atomic Theory62. ____________________________ said there were 4 elements: Earth, Air, Fire, and Water.63. What equipment did J. J. Thomson use to discover the electron? 64. Explain Thomson’s Plum Pudding Model of the Atom. Draw a picture to support your explanation.

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Honors Final Exam Review Name: ___________________________________65. ________________________________ is credited with discovering the charge and mass of the electron using his

famous experiment called the ____________________________________________________________.66. ______________________________ used the Gold Foil Experiment to discover the proton and develop the idea

of a _______________________________ which contains most of an atom’s mass. 67. What contributes the most to an atom’s volume? ______________________________.68. Explain Rutherford’s Nuclear Model of the Atom. Draw a picture to support your explanation. 69. Chadwick discovered the __________________________________.70. Explain the Bohr Model of the Atom. Draw a picture to support your explanation. 71. Is the Bohr Model an accurate model of the atom? Explain. 72. Explain how Schrodinger expanded upon the Bohr model of the atom. 73. What is Heisenberg’s uncertainty principle?74. What is the law of definite proportions?75. What are vertical columns called on the periodic table?76. What are rows called on the periodic table?77. What is an isotope?78. What do isotopes have in common?79. How do isotopes of the same element differ?80. How do you find the mass number? 81. How do you find the number of neutrons?82. How do you determine the number of protons?83. How do you determine the number of electrons?84. What determines an element’s identity?85. What determines an element’s behavior?86. What have more in common: elements in the same period or elements in the same family?87. What are the sub atomic particles of an atom?88. What is the charge on each sub atomic particle in an atom?89. Where is each sub atomic particle in the atom?90. How many protons, neutrons, and electrons are in C-4? 91. How many protons are present in a titanium atom with a mass of 48 g/mol? 92. Where are the metals, non-metals and metalloids on the periodic table?93. What are valance electrons?94. How many valance electrons does each family on the periodic table contain?95. What is a nuclear symbol? (Draw and label one)96. How many protons, neutrons, and electrons are in the following?

97. List the electron configuration/noble gas configuration/orbital notation for the following elements: Mg, Ca, F, Se, Si, P, S, As

98. What is Hund’s rule?99. Draw an orbital diagram that violates Hund’s rule.100. What is Aufbau’s principle?101. Draw an orbital diagram that violates Aufbau’s principle.102. What is Pauli’s exclusion principle?103. Draw and orbital diagram that violates Pauli’s exclusion principle. 104. What are the 4 quantum numbers?105. What does the quantum number “n” represent?106. What does the quantum number “l” represent?107. What does the quantum number “ml” represent?

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Honors Final Exam Review Name: ___________________________________108. What does the quantum number “ms” represent?109. What is the electromagnetic spectrum?110. What does ROY G BIV represent?111. What color of visible light has the lowest energy? ______________________________112. What color of visible light has the highest energy? ______________________________113. What is a ground state?114. How do electrons reach an excited state?115. What happens when electrons in the excited state fall back to their ground state?116. Which of the following is closer to the nucleus: 2s or 3s? ___________________________117. Which of the following has more energy: 2s or 3s? ________________________________118. Write the set of 4 quantum numbers (or ranges of quantum numbers) for the following:

a. Magnesium’s valance electron: ________________________________________________b. Lithium’s valance electrons: __________________________________________________c. The last electron in copper: ___________________________________________________d. The last electron in oxygen: _______________________________________________e. The circled electron below: __________________________________________________

f. The circled electron below: __________________________________________________

UNIT 5 and 6: Bonding and Nomenclature119. What are ionic compounds composed of? 120. What are covalent molecules composed of? 121. What are acids composed of? 122. What are bases composed of?123. How are ionic bonds formed? 124. How are covalent bonds formed? 125. What are properties of ionic compounds? 126. What are properties of covalent compounds? 127. How do you name ionic compounds? 128. When do you use roman numerals and what do the roman numerals represent? 129. How do you name covalent compounds? 130. What are the 8 prefixes? 131. What do the prefixes in the name represent? 132. What is a lewis structure? 133. How do you draw a lewis structure?134. What is a single bond?135. What is a double bond? 136. What is a triple bond? 137. Be able to draw Lewis structures. 138. What is a binary acid? 139. What is a ternary acid? 140. What is the difference among a nonpolar and polar bond? 141. How many oxygen atoms are in aluminum hydroxide?142. How many iron atoms are in Iron (II) sulfate? 143. What is the formula for hydrofluoric acid?

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Honors Final Exam Review Name: ___________________________________144. What is the formula for chloric acid? 145. What is the formula for perchloric acid? 146. How many lead atoms are in Lead (IV) Sulfate? 147. How many lone pairs on the central atom of Carbon tetrahydride. 148. Draw the Lewis structure of nitrogen trifluoride? 149. Draw the Lewis structure of water.150. Be able to calculate molar mass. 151. What are the units of molar mass? 152. List two different ways you can tell if a compound is ionic, covalent, or an acid.153. What does VSEPR stand for?154. What is VSEPR used for?155. What is the difference between bond polarity and molecular polarity?156. What is a dipole? What shape is used to show a dipole moment?157. How do you determine bond polarity?158. How do you determine molecular polarity? 159. What does “like dissolves like” mean?

UNIT 7: Chemical Reactions160. What is a reactant?161. What is a product?162. What is the law of conservation of mass? 163. Why do we balance equations? 164. What is evidence of a chemical change? 165. What is a redox reaction?166. How can you determine if a reaction is a redox reaction or not?167. What types of reactions are redox reactions?168. What type of reaction is NOT a redox reaction?169. What does the saying “Leo the lion says ger” mean?170. What are precipitation reactions?171. What are neutralization reactions?172. What are the requirements for single displacement?173. What are the requirements for double displacement? 174. What type can be predicted using the activity series? 175. What does soluble mean? 176. What does insoluble mean? 177. What is aqueous? 178. What is a precipitate?

UNIT 8: The Mole179. What is the mole (definition and value)?180. How are a mole and a dozen similar?181. What is Avogadro’s number?182. Why do scientists use the mole?183. What is the formula for percent composition?

184. What conversion factor is used to convert between mass and moles?185. When converting between particles and moles, what conversion factor would you use?186. When converting between volume and moles, what conversion factor is used?187. What does STP stand for?188. What is standard temperature?

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Honors Final Exam Review Name: ___________________________________189. What is standard pressure?190. What is the difference between empirical and molecular formulas?191. Can the empirical formula be the same as the molecular formula?192. Know the steps to determining the empirical formula and the molecular formula.

PROBLEMS:Measuring Accurately:

1) Measure each of the following using correct significant figures. Include units in your answers.

a. __________________________b. __________________________ c. __________________________d. __________________________

e. __________________________f. __________________________g. __________________________h. __________________________

Use the graph to the right to

answer questions 2-5.2) Is this reaction endothermic or exothermic?

____________________________________3) What is the energy of the reactants? ____________________________________4) What is the energy of the products? _____________________________________5) How much energy did this reaction gain/lose? _____________________________________

Use the graph to the right to answer question 6-7.6) Label the following: solid phase, liquid phase, gas phase,

critical point, triple point, equilibrium between solid and liquid, equilibrium between solid and gas, equilibrium between liquid and gas.

7) What substance is represented in this phase diagram and how do you know?

Use the following graph to answer questions 7-13. 8) Which letter represents the solid phase? __________9) Which letter represents the liquid phase? __________10) Which letter represents the gas phase? __________11) Which letter represents melting? __________12) Which letter represents evaporation? __________13) What is the melting point? _____________14) What is the boiling point? _____________

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Honors Final Exam Review Name: ___________________________________

15) Determine if the following are Elements (E), Compounds (C), or a Mixture (M)

16) Use the chart below to describe each phase of matter.

17) Fill in the chart: Nuclear Symbol Mass Number Atomic Number # Protons # Neutrons # Electrons

35 17 17

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+159Ni28

Honors Final Exam Review Name: ___________________________________

32 16 18

Give the number of significant figures:18) 420.0 _____19) 7589 _____20) 432506.43 _____21) 0.0000476 _____

22) 0.03 _____23) 35.17 _____24) 0.00004 _____25) 8671.5 _____

Express your answer to the following with the appropriate number of significant figures:26) 2.21 x 0.3= 27) 789.234 ÷ 47.36 =28) 2.90 x 0.01733 x 920=

29) 2.02 x 4.113 =30) (72) (4.022) =

9.03Convert the following:

31) 34 m = _____ cm32) 0.15 mg = _____ g33) 32.98 L = _____ mL34) 1286 m = _____ km

35) 72 cm = _____ m36) 948 mm = _____ cm37) 32 Dm = _____ m38) 87 km = _____ Hm

Place the following in scientific notation:39) 0.000 000 11040) 0.000 02741) 6 220 000 000

42) 77 000 000 000 43) 410 00044) 0.000 000 011

Place the following in standard form:45) 4.3 x 108

46) 2.5 x 10-10

47) 1.2 x 10-4

48) 6.2 x 1011

49) 4.4 x 10-6

50) 1.3 x 105

Perform the following calculations:51) ( 1.10 x 103 ) ( 3.922 x 106 )52) ( 2.377 x 106 ) (1.81 x 109 )53) (6.30 x 108 ) ÷ ( 2.50 x 103 )54) ( 7.64 x 106 ) ÷ (1.343 x 108 )

Density: D=m/V55) Given that the density of iron is 11.35 g/cm3, what would be the volume of a 5.7 gram piece of iron?56) What is the density of 37.72 g of water whose volume is 6.80 cm3?57) The density of Aluminum is 2.70 g/cm3. The volume of a solid piece of Al is 1.50 cm3. What is the mass of this

piece?Bohr Model: Draw the Bohr model of the following:

58) Oxygen ion: 59) Lithium ion: 60) Carbon atom:

Use the following to calculate the average atomic mass:61) Copper is made up of two isotopes, Copper- 63 and Copper-65. Cu-63 is 69.16% abundant. Calculate the average

atomic mass.62) A sample of naturally occurring Silicon consists of Si-28, Si-29, and Si-30. Si-28 is 92.23% abundant, Si- 29 is

4.67% and the remainder is Si-30. Calculate the average atomic mass of silicon.63) Nitrogen is composed of two common isotopes, Nitrogen-14 (which is 99.3% abundant) and Nitrogen-15 (which

is 0.7% abundant). What is the average atomic mass for nitrogen.

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+11H1

Honors Final Exam Review Name: ___________________________________Trends: Circle the element described

64) N P As smallest ionization energy65) O C N highest ionization energy66) Al Si P most electronegative67) Cl Br I least electronegative68) Na K Li largest atomic radius69) Na Mg Al smallest atomic radius

Bonding and Nomenclature: Write the name or the formula for the following substances. Indicate if the substance is (I) Ionic, (C) Covalent, or (A) Acid.

70) _____Copper (I) oxide ____________________________________71) _____Aluminum phosphide ____________________________________72) _____Calcium bromide ____________________________________73) _____Lead (IV) chloride ____________________________________74) _____Hydroiodic acid ____________________________________75) _____Mercury (II) hydroxide ____________________________________76) _____Dinitrogen pentaoxide ____________________________________77) _____Carbon tetrahydride ____________________________________78) _____Dihydrogen monoxide ____________________________________79) _____Ammonium chloride ____________________________________80) _____Hydrocyanic acid ____________________________________81) _____Sulfurous acid ____________________________________82) _____Copper (I) sulfate ____________________________________83) _____Sodium phosphate ____________________________________84) _____nickel(II) nitrate ____________________________________85) _____Hydrogen gas ____________________________________86) _____silver perchlorate ____________________________________ 87) _____H3P ________________________________________________________88) _____FeO ________________________________________________________89) _____CuCl2 ________________________________________________________90) _____NO2 ________________________________________________________91) _____CO ________________________________________________________92) _____O2 ________________________________________________________93) _____C2H6 ________________________________________________________94) _____Al2(SO4)3 ________________________________________________________95) _____HF ________________________________________________________96) _____Pb3(PO4)2 ________________________________________________________97) _____H2CO3 ________________________________________________________98) _____P2O5 ________________________________________________________99) _____H2O _______________________________________________________

Name the following molecules AND calculate their molar mass:100) CO2

101) CCl4

102) PCl5

103) SeF6

104) As2O5

105) SO3

106) ICl3

107) PBr5

Determine what type of bond will exist between the following pairs of atoms based on electronegativity values (Ionic, Covalent, Acid):

108) H and I109) Se and S110) Li and F

111) S and O112) C and H113) Cu and S

114) K and Br115) Ca and Cl116) I and Br

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Honors Final Exam Review Name: ___________________________________Draw the Lewis structure and predict the bond polarity AND molecular polarity for the following molecules:

117) CI4

118) BCl3

119) Cl2O120) PI3

121) Fill out the following chart regarding VSEPR:

Shape Picture # of Electron Domains (#Bonds and #LP)

Bond Angle

Linear

Trigonal Planar

V shape with 3 domains

Tetrahedral

Trigonal Pyramidal

Bent with 4 domains

Determine the state of matter of the following:122) AgCl 123) CH4

124) NH3

125) Na2SO4 126) NH4NO3 127) Al(ClO4)3

128) Sr3(PO4)2 129) K2SO4 130) HCl131) Br2

132) FeBr3 133) NaCl

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Honors Final Exam Review Name: ___________________________________Determine the oxidation number of each element in the following compounds:

134) Al2O3 ____________________135) CO2 _____________________136) H2O _____________________

137) Na ______________________138) Br2 ______________________139) LiOH _____________________

Determine if the following reactions are redox or not. If they are determine which substance is oxidized and which substance is reduced.

140) ____ C2H6 + ____ O2 ____ CO2 + ____ H2O ______________________________________________________________________________

141) ____ Li2S + ____ AlP ____ Al2S3 + ____ Li3P ______________________________________________________________________________

142) ____ K2S + ____ PbO2 ____ K2O + ____ PbS2 _____________________________________________________________________________

143) ____ K + ____ H2O ____ KOH + ____H2 ______________________________________________________________________________

Using the activity series, determine if the following reactions will occur. If they do, you must balance and write the produces.

144) ___Na + ___AlBr3 145) ___Li + ___CuSO4 146) ___Al + ___CuSO4 147) ___Mg + ___LiNO3 148) ___Br2 + ___HCl

Write the balanced reactions indicating states of matter. If the reaction will not occur write NR after the reaction arrow.

149) Nickel (I) carbonate reacts with sodium bromide ______________________________________________________________________________

150) Hydrosulfuric acid reacts with copper (III) oxide ______________________________________________________________________________

151) Calcium perchlorate reacts with potassium sulfate _____________________________________________________________________________

152) Potassium hydroxide reacts with lithium bromide _____________________________________________________________________________

Balance AND identify the type of reaction for the following reactions:153) ___Mg + ___Zn(NO3)2 ___Zn + ___Mg(NO3)2 _______________154) ___MgO ___Mg + ___ O2 _______________155) ___K + ___Cl2 ___KCl _______________156) ___HI ___H2 + ___I2 _______________157) ___C2H6 + ___O2 ___CO2 + ___H2O _______________158) ___Li2S + ___AlP ___Al2S3 + ___Li3P _______________159) ___K2S + ___PbO2 ___K2O + ___PbS2 _______________160) ____ Al + ____ CuSO4 ____ Al2(SO4)3 + ____ Cu _______________161) ____ Pb(NO3)2 + ____ NaI ____ PbI2 + ____ NaNO3 _______________

Calculate the following using your knowledge of the mole:162) A 9.14g sample contains 4.77 g of carbon, 1.19 g of hydrogen, and 3.18g of oxygen. What is the percent

composition of hydrogen in the sample?

163) What is the percent composition of oxygen in the following: a. CuMnO4

b. Fe(NO3)2

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Honors Final Exam Review Name: ___________________________________c. Mn2(SO4)3

164) What is the mass of 3.11 moles of SiH4?165) How many moles of water are present in 15.6 g of H2O?166) How many moles of gas are present in 0.980 L of hydrogen gas at STP?167) What volume does 120 moles of water vapor occupy at STP?168) How many moles are in 3.33 x 1030 molecules of carbon dioxide?169) How many atoms are in 0.895 moles of tin?170) How many atoms of gold does it take to make 1 gram of gold?171) If a balloon contains 3.4 x 1019 atoms of helium, what is the volume of the balloon at STP?172) A sample of sulfur has a mass of 5.37g. How many moles in the sample? How many atoms?173) How many grams of zinc are in 1.16x1022 atoms of zinc?174) How many liters are in 3.68 moles of oxygen gas at STP?175) What is the mass of 4.28x1022 molecules of water?176) How many liters of sulfur dioxide are in 4.8x1020 molecules of sulfur dioxide?177) How many atoms of oxygen are present in 2 moles of sodium phosphate?178) How many atoms of chlorine 5.8 grams of calcium chloride?179) A compound was analyzed and found to contain 13.5g Ca, 10.8g O, and 0.675g H. What is the empirical formula

for the compound?180) A compound has the following composition: 32.4% sodium, 22.5% sulfur, and 45.1% oxygen. What is the

empirical formula of the compound?181) A compound is 64.9% carbon, 13.5% hydrogen, and 21.6% oxygen. Its molar mass is 74.14g/mol. What is its

molecular formula?182) The empirical formula for a compound of CH2 has a molar mass of 70.00 g/mole. What is the molecular

formula?183) Determine the empirical formula from the molecular formulas:

a. C6H6

b. C6H12O6

c. Fe3(CO)9

d. Na2SO4

e. C6H5Nf. LiCl

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Honors Final Exam Review Name: ___________________________________

Electronegativity Values:

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