Atom and Periodic Table Review

27

EOC Exam Review

Name:_____________________

page 11 of 17

This semester review was compiled using the NC Standard Course of Study for Chemistry. You need to answer each question. This semester review is due by January 6, 2015. This packet will count as two tests and two labs. This will significantly affect your grade!!! Answers will be provided before school beginning December 1. Use your green/yellow “reference packets” as needed. You will provide me with the work you have completed and I will allow you to check your answers for those problems. You turn in questions in consecutive order (1, 2, 3, 4…) on notebook paper. (If you want to work out of order, begin a new sheet of paper each time you skip ahead.)

Atom and Periodic Table Review

1. Sketch a PT similar to the one to the right and then, label metals, nonmetals and metalloids (or semi-metals).

2. Sketch a PT similar to the one to the right and then, label periods and groups.

3. Sketch a PT similar to the one to the right and then, label s, p, d, and f blocks.

4. List the five major properties of metals.

5. Describe the five major properties of nonmetals

6. What are semi-metals/metalloids?

7. Sketch and complete a table similar to the one below.

Particle

Location

Charge

Relative mass

(compared with one another)

8. What does the atomic number and mass number tell us about the atom?

9. What symbol is used for atomic number? Mass number?

10. Draw the Bohr model for the Al atom. Fill in the number of protons, neutrons and electrons. It is an aluminum atom with a mass number of 27.

11. Who discovered the proton?

12. Who discovered the electron?

13. Who discovered the neutron?

14. Convert 125 °C to K.

15. The “plum-pudding” model was created by

16. Who performed the “gold foil” experiments?

17. How many protons are there in zinc?

18. How many neutrons are there in mercury?

19. Air is best classified as a(n)

20. Gold is best described as a(n)

21. Water is best classified as a

22. Give 5 examples of a chemical change.

23. Give 5 examples of a physical change.

24. Give 5 examples of a physical property

25. Give 5 examples of a chemical property.

26. State the rule of thumb to determine if a chemical change has occurred.

27. What is difference between a substance and a mixture?

28. Complete the following table.

Name

Nuclear/ Isotopic Symbol

Atomic Number

Mass Number

Average atomic mass

Protons

Electrons

Neutrons

Ion Isotope Neutral

Charge

(if applicable)

11

10

12

Fluorine -18

9

Oxygen - 14

-2

126C

29. Calculate the average atomic mass of the following isotopes (show work):

a. 15% 55Fe, 85% 56Fe

b. 95% 14N, 3% 15N, 2% 16N

30. Using the Bohr model for Hydrogen, determine the energy (wavelength and section of electromagnetic spectrum) that is produced when an electron falls from the 3rd to the 1st energy level?

31. Red light would be produced when an electron “drops” between which energy levels according to the Bohr model of the Hydrogen Atom?

32. What is a quanta? Photon?

33. Describe the current model of the atom.

34. List the number of electrons in the following energy levels:

1st (_____________________________

2nd (_____________________________

3rd (_____________________________

4th (_____________________________

35. Construct the longhand, short hand, and orbital e- configurations for the following elements.

a. K

b. U

c. Ar

d. As

36. Given the electron configuration below, identify the element, valence electrons, oxidation number and/or number of electrons gained or lost.

a. 1s22s22p1element:__________________________

b. 1s22s22p63s2oxidation number: _____________________________

c. 1s22s22p63s23p5valence electrons:_____________________________

d. 1s22s22p63s23p54s23d104p4

oxidation number: ______________why?

37. Name the following families on the Periodic Table and identify as representative/main (A) or transition(B) :

Group

Name

A or B “elements”

1

18

2

17

3-12

38. Match the property to its proper group. (Use the #’s given for each group when matching.)

[Note: Some choices will be used more than once.]

Alkali Metals ( 1

Alkaline-earth Metals ( 2

Transition Metals ( 3

Halogens ( 4

Noble Gases ( 5

a. Form “salts” when reacted with metals.

_____________

b. Least reactive of all elements.

_____________

c. Very reactive with water.

_____________

d. Most reactive group of all non-metals

_____________

e. Contain elements that are free in nature

_____________

f. Contain the hardest and densest metals

_____________

g. Have a +2 charge when they become an ion

_____________

h. Have to be shipped in oil when free

_____________

i. Considered to be inert

_____________.

39. Define: ATOMIC RADIUS

In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest

a.

Mn

Br

Ga

K

b.

Mg

Ar

S

Cl

c.

Bi

N

P

As

Justify your answers

40. Identify the smaller ion of the two listed and justify your answer.

a. N-3NJustify

b. Be+2Be Justify

41. Define: Ionization Energy

In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest

a.

Mn

Br

Ga

K

b.

Mg

Ar

S

Cl

c.

Bi

N

P

As

Justify your answers

42. Define: Electronegativity / Electron Affinity

In the following, number the elements 1 – 4, with 1 being the smallest and 4 being the largest.

a.

Mn

Br

Ga

K

b.

Mg

Ar

S

Cl

c.

Bi

N

P

As

Justify your answers

Formulas and Atomic Stoichiometry Review

43. Write the chemical formula that would exist between the following elements, then draw the Lewis structure that confirms the formula.

a. Zn & F ( _______________

b. Al & O ( _______________

c. Ca & S ( _______________

d. K & Br ( _______________

44. Name each of the following compounds.

a. AlCl3 ( _________________________________

b. CO2 ( _________________________________

c. LiNO3 ( _________________________________

d. Fe2O3 ( _________________________________

e. Na2CO3 ( _________________________________

f. P2O5 ( _________________________________

g. SO3 ( _________________________________

h. Ba(C2H3O2)2 ( ____________________________

i. NH4OH ( _________________________________

j. ZnS ( _________________________________

45. Write the chemical formula from the following names:

a. Potassium nitrate ( _________________________

b. Carbon monoxide ( _________________________

c. Silver oxide ( ______________________________

d. Copper (II) chloride ( _______________________

e. Nitrogen dioxide ( __________________________

f. Aluminum sulfate ( _________________________

46. Calculate the GFM of the following compounds:

a. NaBr ( _______________

c. Al2(S2O3)3 ( _______________

b. Mn3(PO4)2 ( _______________

d. Ag2SO3 ( _______________

47. Make the following conversions.

a. 3.65 moles H2CO3 = ____________________ g H2CO3

b. 5.10 x 1028 molecules CO2 = ____________________ moles CO2

c. 37.9 g K2S = ____________________ moles K2S

d. 195 g Ca(OH)2 = ____________________ molecules Ca(OH)2

48. What is the % composition of each element in the following compounds:

a. Li2SO4

b. Ca(NO2)2

49. Calculate the empirical formula for the following.

a. 32.38 % Na, 22.65 % S, and 44.99 % O

b. 66% Ca and 34 % P

50. Calculate the molecular formula for:

a. A compound made of 25.3% copper, 12.9% sulfur, 25.6% oxygen, and water, with an molecular mass of 249.7 g/mol.

b. The empirical formula of a compound is CH2. Its molecular mass is 70 g/mol. What is its molecular formula?

c. A compound is found to be 40.0% carbon, 6.7% hydrogen, and 53.5% oxygen. Its molecular mass is 60.0 g/mol. What is its molecular formula?

Reaction Stoichiometry Review

I. Chemical Reactions

51. Balance the following reactions and then classify them.

a. __HCl + ____Al ( ____AlCl3 + ____H2

Classification (

b. ____Zn + ____O2 ( ____ZnO

Classification (

c. ___CH4 + ____O2 ( ____CO2 + ____H2OClassification (

d. __Mg(NO3)2 + ____Cu3PO4 ( ____Mg3(PO4)2 + ___CuNO3 Classification (

e. ___H2O2 ( ____H2O + ____O2

Classification (

52. Predict the products and balance the reaction for the following.

a. ____Al + ____O2 (

b. ____H2O (

c. ____C2H6 + ____O2 (

d. ____Ag2SO4 + ____Ba3N2 (

e. ____FeCl3 + ____F2 (

53. Answer the following questions that involve experimentation.

a. The “pop” test is used to check for ___________________________________________________.

b. If a glowing splint reignites __________________________ was present

c. When a student places a glowing/burning splint into a test tube containing a gas, the splint is immediately extinguished (goes out); therefore ________________________ was present.

d. The process in which an electrical current is passed through an object in order for it to decompose is called

________________________________________________________________.

e. What must be present in order for something to burn? _________________

54. Use the activities series to decide if the following reactions will occur.

a. Pb2O3 + Li ( ????______________

D. Al + HCl ( ???? ________________

b. ZnF2 + Cu ( ????______________

E. Fe + MgSO ( ???? ______________

c. H2S + Hg ( ????______________

F. Cr + AuI3 ( ???? ________________

55. What are three possible categories of products in a double replacement reaction?

II. Stoichiometry

56. How many grams of NH3 are produced when excess N2 reacts with 11.7 g of H2?

N2 + 3H2 ( 2NH3

57. When 15.4 grams of Al is added to HCl, how much HCl is needed to react completely with the Al?

2Al + 6HCl ( 2AlCl3 + 3H2

58. What mass of Cu could be produced when 4.77 g of K reacts with excess CuSO4?

59. How much O2 is needed to react completely with 31.9 g of C2H6?

60. How much Al2(SO4)3 is produced when 6.55 g of Na2SO4 reacts with excess Al(OH)3?

Energy in reactions

61. A fire is what type of energy reaction?

_________________________________________

62. A first aide cold pack is what type of energy reaction?_________________________________________

63. What type of energy reaction is the diagram A?

_________________________________________

64. What type of energy reaction is the diagram B?

____________________________________

65. What is the minimum amount of energy required for a reaction to start?____________________________

The graph below is a potential energy diagram of a compound which is formed from its elements.

66. Which interval represents the heat of reaction? _______________

67. Which interval represents the activation energy of the forward reaction?_______________

68. What would change if a catalyst was added? What is a catalyst?

69. Where is the activated complex found?

70. Explain the collision theory?

Phases Review

PHASE CHANGES

71. Define the following phase changes and describe the change in kinetic energy.

a. Solid ( Liquid ( _________________________________________KE ( ______________

b. Solid ( Gas ( ___________________________________________KE ( ______________

c. Gas ( Liquid ( __________________________________________KE ( ______________

d. Liquid ( Solid ( _________________________________________KE ( ______________

e. Liquid ( Gas ( __________________________________________KE ( ______________

f. Gas ( Solid ( ___________________________________________KE ( ______________

72. Label the following chart according to a phase change from ice to steam

E

140 oC

D

C

B

10 oC

A

Energy

73. From the above chart, answer the following questions:

a. What is the boiling point of the substance?

b. Which letter represent where vaporization and condensation occur?

c. Which letter(s) show a change in kinetic energy?

d. Which letter shows where crystallization can occur?

e. What is the melting point of the substance?

f. Which letter(s) show a change in potential energy?

74. How much energy is required to raise 16.7 g of ice at –27 oC to steam at 162 oC?

75. How much energy is lost when 14.7grams of liquid water freezes?

76. If you fill a sauce pan with 1000grams of water and heat the water from 21.70C to 98.0oC, how much heat is required?

77. What mass of water was boiled if 340 000J of heat was required?

Phase Diagrams

B

760

I

II

III

220

A

55 70

165 190

Temperature (oC)

a. What section represents the gaseous phase? __________________________________

b. What is the substances normal boiling point? _________________________________

c. What is point B called? __________________________________________________

d. Is the solid more or less dense than the liquid? ________________________________

e. Would an increase of pressure favor melting or freezing? _________________________________________

f. What section represents the solid phase? _____________________________________

g. What is the substances normal melting point? _________________________________

h. What is the critical temperature? ____________________________________________

i. What does point A represent? ______________________________________________

j. What section represents the liquid phase? _____________________________________

k. What pressure and temperature would all three states of matter coexist? _____________________________

KMT Review

Gas Laws Review:

78. Which of the following gas laws match up to the following descriptions:

a. relationship between temperature and pressure ( __________________________________

b. our atmospheric pressure is a practical example ( _________________________________

c. explains how a hot air balloon works ( __________________________________________

d. relationship between volume and pressure ( ______________________________________

79. A tire has an air pressure reading of 35.1 psi on a day when it is 30 °C. What would be the air pressure of this tire on a day when it is 0 °C?

80. A hot air balloon can rise only when its air volume is 2560 L. If air inside an air balloon has a volume of

1100 L at 130 °C, what must the temperature become in order for the balloon to be able to fly?

81. NH3 will occupy a volume of 1.45 L under 165 kPa. What must the pressure be if the volume of NH3 rises to 6.01 L?

82. A certain gas occupies a volume of 25.1 cm3 at STP. What would be the volume of this gas if the pressure was 175 torr and the temperature was 147 °C?

83. How many times faster will oxygen gas diffuse compared to argon gas?

84. A gas with a volume of 48.7 L exerts a pressure of 187 mm Hg. The gas is composed of 24.1 L of methane, 11.1 L of carbon monoxide, and 13.5 L of ammonia. What is the pressure of the carbon monoxide?

85. Air will leak out of a punctured tire due to ________________________________.

86. What kind of gas will diffuse the fastest?

Answer ( ____________________________________

Molar Volume and the Ideal Gas Law

87. What is the value of molar volume according to Avogardro’s principle? _____________________________

88. What is the formula for the ideal gas law?________________________________________________

89. What value of R corresponds to the following pressures:

a. atm ( ______________________

c. mm Hg ( _______________________

b. torr ( ______________________

d. kPa ( __________________________

90. What volume of steam would there be in 4.87 moles at STP?_________________________________

91. How many liters of O2 are there in 2.09 moles at 2.88 atm and 42 oC? _______________________________

92. How many molecules are found in 5.33 L of Cl2 at STP? _________________________________________

93. What mass of CO2 has a volume of 9.94 L at STP?________________________________________

94. What pressure is exerted on 37.4 g of KOH with a volume of 1.87 L at 26 oC?

95. How many moles would make up a sample of Br2 taking up 3.18 L of space under 24.7 kPa and 28 oC?

96. What is the temperature of 3.09 x 1024 molecules of some gas taking up 4.22 L at 1.87 atm?

Gas Stoichiometry

97. What volume of CO2 is produced when 19.3 L of C2H6 reacts with excess O2 at STP?

____C2H6 + ____O2 ( ____CO2 + ____H2O

98. How many grams of Ni3PO4 are produced when 2.11 L of NiOH reacts with excess Zn3(PO4)2 at STP?

____NiOH + ____Zn3(PO4)2 ( ____Ni3PO4 + ____Zn(OH)2

99. How many liters of Li2SO4 are needed to react completely with 1.95 g of AgOH at STP?

____Li2SO4 + ____AgOH ( ___LiOH + ____Ag2SO4

Limiting Reagents

100. What mass of KI can be produced when 16.7 g of BaI2 reacts with 11.8 g of KOH?

____BaI2 + ____KOH ( ____Ba(OH)2 + ____KI

101. What mass of Ca(NO3)2 can be produced from 6.77 g of Al(NO3)3 reacting with 16.7 L of Ca(CN)2 at STP?

____Al(NO3)3 + ____Ca(CN)2 ( ____Al(CN)3 + ____Ca(NO3)2

102. In closed container, 13.8 L of CH4 reacts with 19.7 L of O2. What is the limiting reagent if the desired product to be measured is grams of H2O?

____CH4 + ____O2 ( ____CO2 + ____H2O

103. How many grams of NH3 can be produced when 1.33 L of N2 reacts with 8.97 g of H2 at STP?

____N2 + ____H2 ( ____NH3

Bonding Review

104. What is the strongest possible bond?_________________________

105. A bond formed by the sharing of electrons is called _________________________.

106. Describe each type of bond.

a. Ionic bonding ( _______________________________________________________

b. metallic ( ________________________________________

c. Covalent bonding ( _______________________________________

107. Classify the following compounds as containing an ionic or covalent bond. If the compound contains both types of bonds, be sure to write both for the answer.

a. NO2 __________________

i. CO ____________________

b. H2O __________________

j. MgF2 __________________

c. KF __________________

k. O2 ____________________

d. NaNO3 _______________

l. CaCO3 _________________

e. Fe2O3 _________________

m. HCl ____________________

f. NaCl ( _________________

n. NH3 ( ______________________

g. SO3 ( __________________

o. Ba(NO2)2 ( __________________

h. K2CO3 ( ________________

108. A (+) ion is called a(n) ________________ and a (-) ion is called a(n) __________________.

109. An ionic compound will dissolve in water and carry an electrical current. This compound is a(n) ______________.

110. Circle the compound with the highest melting point.

CO2

N2

NaF

H2

SI3

111. Circle the compound with the strongest bond.

CO2

N2

NaF

H2

SI3

112. Circle the compounds which contain at least one polar bond.

H2

H2O

NH3

CO

MgCl2

O2

113. Circle the compound that would conduct electricity in its aqueous solution.

H2

H2O

NH3

CO

MgCl2

O2

114. Circle the compound that would conduct electricity in its molten state.

N2

HBr

SO3

H2

Al2O3

SiF4

115. Draw the molecular structures for the following. Don’t forget to draw the lone pair electrons.

a. NH3

Shape ( ________________________________

b. N2

Shape ( ________________________________

c. H2

Shape ( ________________________________

d. CO2

Shape ( ________________________________

e. Cl2

Shape ( ________________________________

f. H2O

Shape (________________________________

g. F2

Shape ( ________________________________

h. Br2

Shape ( ________________________________

i. O2

Shape ( ________________________________

116. Complete the following chart.

Compound

Name

Shape

Polar / Non-Polar

H2O

CO2

NCl3

H2SO4

PF3

SBr2

CS2

O2

CH4

Solutions Review

117. Circle the following compounds that are electrolytes in solution :

Table Salt Methyl AlcoholFructose

Sulfuric Acid

Ammonia

118. Label the following as a suspension, colloid, or soluiton.

a. particle size less than 1 nm = ________________________________________

b. particle size greater than 100 nm = ____________________________________

c. between 1 nm & 100 nm = __________________________________________

d. does not exhibit the Tyndall Effect = __________________________________

e. muddy water = ___________________________________________________

f. glue = ___________________________________________________________

g. dusty air = _______________________________________________________

h. kool aid = ________________________________________________________

i. milk = ___________________________________________________________

119. The part of a solution that gets dissolved is called the ________________________ and the part that

does the dissolving is called the _________________________________.

120. The nature of the solute and solvent is the predominating factor of whether or not a solution can be formed. What are the three factor that affect the rate at which a solution can form?

___________________________________________________________________

121. If two liquids will not form a solution, they are said to be ____________________________.

122. How does pressure affect the solubility of a gas? ___________________________________

123. How does temperature affect the solubility of a gas? ________________________________

124. The rapid escape of a gas from a liquid in which it was dissolved is called ______________________.

125. If we add 5.0 g of sugar to a sugar solutiona. if it doesn’t dissolve, the solution is ___________________

b. if it dissolves, the solution is ___________________c. if 7 g falls out, the solution is ________________

126. What kind of mixture are suspensions?____________________

Use the solubility curve to answer questions 127 – 135.

127. At 60 °C, how much KNO3 will dissolve in 100 g of H2O? __________________________________________

128. Which of these compounds shows the least change in solubility with temperature?_____________________

129. At 80 °C, a solution contains 35 g of NaCl in 100 g of H2O. This solution is said to be ____________________

130. How many grams of NH4Cl will dissolve in 300 g of H2O at 80 °C? __________________________________

131. Circle the salt in the following list that is the most soluble at 50 °C.

NH4Cl

NaCl

KClO4

NaNO3

KNO3

132. At 100 °C a solution contains 100 g of KClO3 in 100 g of water. This solution is said to be ________________

133. Which compound is the least soluble at 100 °C?__________________________________________________

134. At 40 °C, a solution is composed of 90 g of NaNO3 dissolved in 100 g of H2O. This solution is ____________

135. Which of these compounds shows the greatest change in solubility with temperature?____________________

136. What is the molarity of a solution in which 11.5 g of Al(OH)3 are dissolved in 678 mL of solution?

137. If 36.4 g of sodium hydroxide are dissolved in 255 mL of solution, calculate its molarity.

138. How many grams of barium chloride are needed to make 1.06 L of 2.01 M barium chloride?

139. Explain what would happen to the following if salt were to be added:

a boiling point ______________________

b. freezing point ________________________

Equilibrium and Energy Review

140. The minimum amount of energy that colliding particles must have in order to react is called __________________.

141. What are five factors which increase reaction rate?

142. Determine if the following reactions would have an increase or decrease in entropy.

a. HCl(g) + NaOH(aq) ( NaCl(aq) + H2O(l)

b. MgSO4(aq) + 2LiCl(aq) ( MgCl2(aq) + Li2SO4(aq)

c. C(s) + O2(g) ( CO2(g)

143. __________________________ is a measure of disorder within a chemical reaction system.

144. An enzyme in the body helps speed up reactions at low temperatures. An enzyme is an example of a(n)

_____________________________________.

145. Which state of matter has the greatest entropy?__________________________________________________

146. What direction would the equilibrium shift toward in the reactions in questions of #143 if the following occurred:

Change

Rxn a

Rxn b

Rxn c

Rxn d

Rxn e

[Reactants] Increases

Pressure Increases

[Products] Increases

147. Fill in the chart for the following reaction: H2O(g) + NaCl(aq) + 126 kcal (( HCl (g) + NaOH(g)

Change

[H2O]

[NaCl]

[HCl]

[NaOH]

Keq

Pressure decreases

[HCl] decreases

[NaCl] increases

Temperature decreases

[H2O] increases

[NaOH] increases

Pressure increases

Temperature increases

Acid and Base Review

148. For the following compounds, determine if the compound is an acid, base, or salt. Name the compound and then determine its relative strength.

Compound

Acid / Base / Salt

Name

Relative Strength

NH3

H2SO4

K2CO3

LiCl

HCl

Zn(OH)2

Ca(OH)2

HNO3

NH4C2H3O2

MgCO3

AgOH

HClO3

NaOH

Bronsted – Lowry Acid / Base Theory

149. For each of the following reaction, label each compound as acid, base, conjugate acid, or conjugate base.

a. NH3

+ HCl ( NH4+

+ Cl-

____

____

____

____

b. BaSO4

+2HF(H2SO4

+BaF2

____

____

____

____

c. HC3H3O3+LiBr(LiC3H3O3+HBr

____

____

____

____

d. HSO3-

+H2O(SO3-2

+H3O+

____

____

____

____

pH

150. Answer the following questions.

Acid or Base

Color of indicator

a. pOH = 2.89

[H+] = _______________________________blue litmus_____________

b. [NaOH] = 5.99 x 10-8 M

pH = ________________________________red litmus _____________

c. [H3O+] = 8.67 x 10-6 M

[OH-] = ______________________________universal ______________

d. [H+] = 1.88 x 10-10 M

pH = ________________________________blue litmus_____________

e. [HCl] = 8.11 x 10-2 M

pOH = ______________________________red litmus _____________

f. [KOH] = 5.33 x 10-7 M

[H+] = _______________________________pheonothalein___________

g. pH = 2.08

[H+] = _______________________________universal ______________

h. [OH-] = 3.44 x 10-9 M

pOH = ______________________________blue litmus_____________

i. pH = 8.23

[H+] = _______________________________pheonothalein___________

Dilution

151. How much concentrated 18M sulfuric acid is needed to prepare 250 mL of a 6.0 M solution?

152. To approximately how much water should 50.mL of 12M hydrochloric acid be added to produce a 4.0M solution?

Titrations

153. Describe the graph to the right.

154. Answer the following questions about titrations.

a. The solution of known concentration is called the ____________________________.

b. The solution of known concentration is placed in the _________________ during a titration.

c. 36.7 mL of 6.72 M NaOH is used to neutralize 61.8 mL of H2CO3. What is the molarity of the H2CO3?

d. 206 mL of 3.92 M Mg(OH)2 can be used to neutralize how much 1.77 M HCl?

Precipitation Reactions

155. Balance the following reactions and determine the precipitate.

a. ___K2SO4 + ___Ba(NO3)2 ( ___KNO3 + ___BaSO4

Precipitate ( _________________

b. ___BaCl2 + ___Na2SO3 ( ___BaSO3 + ___NaCl

Precipitate ( _________________

c. ___Zn(NO3)2 + ___(NH4)2S ( ___ZnS + ___NH4NO3

Precipitate ( _________________

d. ___HgCl2 + ___K2S ( ___HgS + ___KCl

Precipitate ( _________________

e. ___Na2CO3 + ___CaCl2 ( ___NaCl + ___CaCO3

Precipitate ( _________________

f. ___CuCl2 + ___(NH4)3PO4 ( ___Cu3(PO4)2 + ___NH4Cl

Precipitate ( __________________

Nuclear Review

156. What are three types of radiation?

157. What are fission and fusion? Give common examples of how they are used or where they are found.

158. For the following statements, determine the type of radiation that best fits the description.

a. most dangerous ( ________________________________

b. no mass ( ______________________________________

c. shielded by aluminum foil ( ________________________

d. mass is equivalent to that of an electron ( _____________

e. largest form of radiation ( _________________________

f. double positive charge ( ___________________________

g. (-1) charge ( ____________________________________

h. most penetrating ( _______________________________

i. shielded by skin ( ________________________________

j. shielded by several inches of lead ( __________________

159. Complete the following nuclear reactions:

23892U ( 42He + _________________

d. 6430Zn + 0-1e ( ______________

3719K + 0+1e ( ___________________

e. 15763Eu ( 11H + ______________

3115P + 42He ( 10n + ______________

f. 23190Th + 10n ( 0-1e + _________

160. _________________________ is the splitting of nuclei and ___________________ is the combining of nuclei.

161. Name three devices used to detect radiation.

162. _____________ occurs in nuclear bombs and in nuclear power plants. ____________________ occurs in the sun.

163. Phosphorous – 32 has a half-life of 14.3 years. How many grams will remain after 57.2 years of a 4.0 g sample of Phosphorous – 32?

164. Sketch the table below, label the areas mentioned in question 37. Then identify the number of valence electrons and oxidation number for each family.

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Potential Energy

D

E

C

B

A

Reaction

A.

B.

C.

D.

E.

Pressure (torr)