2015 Chemistry Fall Final Exam Review (Major Grade) Name __________________________

Physical or Chemical Change

1. boiling ____

2. burn (combustion)__

3. corrode ____

4. sublimation ____

5. decay ____

6. rust ____

7. dissolve ____

8. freeze ____

9. oxidize ____

Physical or Chemical Property

10. glass is transparent _____

11. Under proper conditions, water will break apart into hydrogen and oxygen gas ____

12. copper conducts electricity _____

13. fumes from ammonia and hydrochloric acid mix to produce a white smoke _____

Intensive or Extensive Property

14. mass of 50 g ____

15. color is green ____

16. density is 2 g/mL ___

17. boils at 100 ◦C ____

18. volume of 4 cm3 ___

19. length of 10 m ____

Atomic Structure

20. Draw a Bohr’s Atom model for Potassium.

21. The mass of which subatomic particle is negligible (too small to matter)? ____________

22. What part of an atom carries most of its mass? _________

23. Match the following:

__________ Who discovered the nucleus was positive and dense?A. protons

__________What experiment was used to discover the electron?B. electrons

__________ Who discovered the electron? C. Rutherford

__________What experiment was used to discover the proton? D. Cathode Ray

__________Who included energy levels in his model? E. Thomson

__________What particle(s) are found inside the nucleus? F. Dalton

__________ What particle(s) are found outside the nucleus? G. Bohr

H. gold foil

Classification of Matter

24. Identify the following as element (e) or compound(c)

a.

b. Sugar (C12H22O11 ) ___

c. b. H2O ___

d. c. Cl2 ___

e. d. potassium ___

f. e. Oxygen ___

25. What are the two types of mixtures?

26. Identify the following as homogeneous (homo) or heterogeneous mixtures (hetero)

a. Steel _______

b. Air _______

c. Salt water ________

d. Sand + water _______

27. How are pure substances different from mixtures?

28. Identify the following as pure substances (p) or mixtures (m)

a.

b. H2O _____ b. Milk _____ c. steel alloy _____ d.F2 _____

29. When would you use physical means (p) or chemical means (c) to separate each of the following?

a.

b. Fe2O3 ____ b.Sugar Water ____c. trail mix ___d. HCl ___

States of Matter

Shape

(definite or indefinite)

Volume

(definite or indefinite)

Compressibility

(compressible or incompressible)

Spread out to take shape of container (Yes or No)

Solid

Liquid

Gas

Isotopes

30. A new element X has recently been discovered and consists of two isotopes. One isotope has a mass of 331 amu and is 35.0 % abundant. The other isotope is 337 amu and is 65.0 % abundant. What is the mass (amu) of X?

31. Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

32. Element Q has two stable isotopes, Q-37 and Q-39. Q-37 has an amu of 36.956 and abundance of 24.23%. The other isotope Q-39 has an amu of 38.944 and 77.77%. What is the average atomic mass of this element?

Alpha, Beta, and Gamma radiation characteristics

1. Complete the following table.

Symbol

Mass

Charge

Shielding Power

Penetrating Power

Alpha

Beta

Gamma

Balanced nuclear equations

Fill in the blank in each of the following decay reactions with the correct decay particle or decayed nucleus that will balance the decay reaction, and also state whether it is alpha or beta decay.

33.

34.

35.

36.

37.

38.

39.

Fission vs Fusion

Write fission or fusion next to each of the descriptions below (55-61)

40. Occurs when the nucleus of an atom splits. __________________

41. Occurs when the nuclei of two small atoms combine to form a larger nucleus. ________

42. Occurs in the core of the sun. _________________

43. Generates a large volume of radioactive waste. ________________

44. Is used to generate power in a nuclear power plant. ________________

45. Atomic bomb reaction. __________________

46. Identify the following equations as fission or fusion

Electron configurations

47. Label the periodic table with the orbital blocks (s,d,p,f).

48. How many electrons can each orbital block hold?

S block: ____p block: ____d block: ____f block: _____

49. Identify the elements based on their electron configurations

a.

b. [Ar] 4s23d7 _______________

c. [Kr] 5s2 __________________

d. 1s22s22p63s1 _______________

e. 1s22s22p63s23p64s2 _________

Ions

50. Circle the word that would make each statement true.

a. Anions have a ( positive / negative) charge.

b. Cations have a (positive / negative) charge.

c. Metals will (gain / lose ) electrons.

d. Nonmetals will (gain / lose ) electrons.

e. Ionic bonds from between cations and (cations / anions).

f. Ionic bonds (transfer / share ) electrons.

51. Complete the table below

Element

Symbol

Valence Electrons

Gain/Lose Electrons

Normal

Lewis Dot Diagrams

Ion Symbol with Charge

Cation or Anion

Sulfur

Barium

Metals and Metallic Bonds Fill in the Blank. Words may be used more than once.

losing

good

cations

left

positive

sea of electrons

malleable

ductile

52. Metals are found to the ___________________ of the zig zag line on the periodic table.

53. Metals are _____________ conductors of heat.

54. Metals are _____________ conductors of electricity because they contain a mobile ________ ________________________.

55. Metals are _______________and ______________, unlike non metals which are brittle.

56. Metals form _____________ions (______________) by ____________electrons.

Ionic and Covalent Compounds and Molecular Geometry

57. Write down the correct name for the following Ionic or Covalent compounds –

1. MnF3 ______________________________________

1. CoCl3 ______________________________________

1. N2O3 ______________________________________

1. MgCl2 _____________________________________

58. Write down the correct formula for the following Ionic or Covalent compound-

a. Calcium Phosphate _____________________

b. Nitrogen triodide _____________________

c. Disulfur decafluoride _____________________

d. Mercury(II) bromide _____________________

59. What is the correct Lewis electron-dot structure for the compound formed between magnesium and fluorine?

C.

D.

B.

A.

60. Draw a Lewis dot structure for the following ionic bonds

Potassium + Oxygen

61. Draw a Lewis dot structure for the following covalent bonds

Covalent Bond

Lewis Dot Structure

VSEPR Shape

(Linear, Bent, trigonal planar, or tetrahedral)

CO2

CH4

H2O

BCl3

62. Which of the following choices shows the correct Lewis electron-dot diagram for a molecule of chlorine, Cl2?

A. B. C. D.

63. Fill in the blank with ionic, covalent, or metallic bond.

a. A __________________ bond forms between a metal and a metal.

b. A __________________ bond forms between a metal and a nonmetal.

c. A __________________ bond forms between a nonmetal and a nonmetal.

64. Which of the following compounds are ionic (I), which are covalent (C)?

a. KCl ____b. SO2 ____ c. C2H4 _____ d. Mn2O3_____

65. Determine whether the image shows a single, double, or triple covalent bond. How many electrons total does each bond have?

a.b. c.

Periodic Table Trends

66. Look at the images below. Determine which image represents ionization energy, electronegativity, atomic radius, and ionic radius.

67. Use the following choices to answer the following questions:

Sulfur Calcium ChlorineStrontium

a. Which element has the lowest electronegativity? _____________

b. Which element has the largest atomic radius? ____________

c. Which element has the highest ionization energy? ____________

d. Which element has the largest ionic radius? _____________

Periodic Table

68.

69. Complete the following table.

Group

Number of valence electrons

Charge

Example of a Lewis Dot structure

1A

2A

3A

4A

5A

6A

7A

8A

70. Which scientists are responsible for creating/organizing the periodic table and why did each scientist organize the periodic table as they did?

Scientist

Organization

Mendeleev

Moseley

71. Fill in the Blank. Words can be used more than once.

Groups

Periods

Halogens

Alkali Metals

Alkaline Earth Metals

Noble Gases

Transition Metals

a. Name of group 1A on periodic table _____________________________________

b. Name of group 2A on periodic table ____________________________________

c. Name of group 7A on periodic table _____________________________________

d. Name of group 8A on periodic table _____________________________________

e. Group that has full outer shells (inert) __________________________________

f. The most active metal group, react violently in water _______________________

g. Share the same physical and chemical properties __________________________

h. Share the same number of electron shells ________________________________

i. Name of the B group on periodic table ___________________________________

Electromagnetic spectrum

72. A helium-neon laser emits light with a wavelength of 6.33 x 10-7 m. SHOW ALL WORK

a. What is the frequency of this light

b. How much energy is emitted by this light?

73. Calculate the energy of a gamma ray photon whose frequency is 5.02 x 1020 Hz.

74. Calculate the frequency of a photon that emits 4.06 X 10-18 J of energy.

75. Label the electromagnetic spectrum with the following: low energy, high energy, low frequency, high frequency, low wavelength, high wavelength.

76. Arrange the following types of electromagnetic radiation in order of increasing wavelength:

a. Ultraviolet light b.Microwaves c. X rays d. Radio waves

77. When sunlight passes through a prism, the different wavelengths separate into spectrum colors (like a rainbow). Correctly organize these colors from lowest to highest energy.

78. As frequency increases, the wavelength __________________ and the energy __________________.

79. Waves with more energy have __________________ wavelengths and __________________ frequencies.