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Name: _____________________________________ Class: _____ Date: ________________
FALL 2013 SEMESTER FINAL EXAM REVIEW
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
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1. MATTER - Properties and Changes
The study of matter and changes in matter best describes the science of
a. biology.
c. microbiology.
b. physics.
d. chemistry.
2. A physical property may be investigated by
a. melting ice.
c. allowing silver to tarnish.
b. letting milk turn sour.
d. burning wood.
3. A chemical property is
a. description of observations and measurements.
b. description of a chemical’s reactivity.
c. when the composition of a substance is unchanged, only change appearance.
d. when the composition of a substance is changed, creating something new.
4.
What type of substance is shown in the picture above?
a. element
c. mixture of elements
b. compound
d. mixture of elements and compounds
5. In water, there are always 2 hydrogen atoms for every 1 oxygen atom. The elements cannot be
separated by physical means. What type of matter is the material?
a. element
c. heterogeneous mixture
b. compound
d. homogeneous mixture
6. What is an alloy?
a. an element
c. a mixture of two metals
b. a compound
d. a mixture of two compounds
7. An example of an extensive physical property is
a. mass.
c. color.
b. density.
d. boiling point.
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8.
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9. Which of the following is an intensive physical property?
a. volume
c. color
b. length
d. mass
What type of substance is shown in the picture above?
a. element
c. mixture of elements
b. compound
d. mixture of compounds
____ 10. A chemical change occurs when
a. ice melts to water.
b. paper rips in half.
c. sugar is dissolved in a solution.
d. an unexpected color change occurs.
____ 11. Which sign does NOT indicate that a chemical change has occurred?
a. color change.
c. energy absorbed or released.
b. dissolving in a solution.
d. gas produced.
____ 12. A physical change occurs when
a. milk sours.
c. a bracelet turns your wrist green.
b. a copper bowl tarnishes.
d. steam condenses to water on a mirror.
____ 13. The particles in a solid are
a. packed closely together.
c. constantly in motion.
b. very far apart.
d. able to slide past each other.
____ 14. Physical means can be used to separate
a. elements.
c. mixtures.
b. pure substances.
d. compounds.
____ 15. MEASUREMENT AND LAB TECHNIQUES/SAFETY
You are heating a substance in a test tube. Always point the open end of the tube
a. toward yourself.
c. toward another classmate.
b. toward your lab partner.
d. away from all people.
____ 16. When measuring liquids, it is best to use which of the following to measure the volume?
a. beaker
c. graduate cylinder
b. test tube
d. beaker and graduate cylinder
____ 17. What is an observation?
a. A hypothesis
c. An inference
b. A description using 5 senses
d. A type of conclusion.
____ 18. Which type of investigation would be used to answer this question:
“Which vegetable shows the greatest reaction with hydrogen peroxide?”
a. Descriptive
c. Experimental
b. Comparative
d. Investigatory
____ 19. What step of the Scientific Method is shown in the following example:
“SpongeBob notices that Gary is giving off a horrible odor. How can Gary get rid of this odor?”
a. Develop a Hypothesis
c. Choose a Problem
b. Research the Problem
d. Draw Conclusions
____ 20. These values were obtained as the mass of products from the same reaction: 8.83 g; 8.84 g; 8.82
g. The known mass of products from that reaction is 8.60 g. The values are
a. accurate, but not precise.
c. both accurate and precise.
b. precise, but not accurate.
d. neither accurate nor precise.
____ 21. Convert 125 mm to dm.
a. 0.0125
c. 1.25
b. 0.125
d. 12.5
____ 22. When comparing the volume of a liquid, the most accurate instrument to use to measure the
volume is
a. the beaker.
c. the buret.
b. the graduate cylinder.
d. the flask.
____ 23. Which of the following observations is quantitative?
a. The precipitate is white.
c. The liquid tastes bitter.
b. The liquid boils at 100ºC.
d. The liquid is cloudy.
____ 24. Convert 120 km to meters.
a. 0.120
c. 0.0120
b. 12,000
d. 120,000
____ 25. Which of the following observations is qualitative?
a. A chemical reaction is complete in 2.3 seconds.
b. The solid has a mass of 23.4 grams.
c. The pH of a liquid is 5.
d. Salt deposits form from an evaporated liquid.
____ 26. The symbol for the metric unit used to measure mass is
a. m.
c. g.
b. mm.
d. L.
____ 27. A researcher is studying the effects of climate on freshwater life. She sets up an experiment where
she will count the number of microscopic organisms that survive at a given temperature. In this
experimental investigation, what is the independent variable?
a. Amount of freshwater
c. Number of organisms that survive
b. Temperature
d. none of the above
____ 28. A measure of the quantity of matter is
a. density.
c. volume.
b. weight.
d. mass.
____ 29. To calculate the density of an object,
a. multiply its mass and its volume.
c. divide its volume by its mass.
b. divide its mass by its volume.
d. divide its mass by its area.
3
____ 30. The mass of a 5.00 cm sample of gold is 96.5 g. The density of gold is
a. 0.0518 g/cm3.
c. 101.5 g/cm3.
b. 19.3 g/cm3.
d. 483 g/cm3.
____ 31. The volume of pure diamond is 0.071 cm3. The mass of a diamond is 0.25 g. Find its density.
a. 0.0178 cm3
c. 3.5 cm3
3
b. 0.179 cm
d. 0.284 cm3
____ 32. The number of significant figures in the measurement 0.000 305 kg is
a. 3.
c. 5.
b. 4.
d. 6.
____ 33. The number of significant figures in the measured value 0.003 20 g is
a. 2.
c. 5.
b. 3.
d. 6.
____ 34. The measurement that has been expressed to three significant figures is
a. 0.052 g.
c. 3.065 g.
b. 0.202 g.
d. 5000 g.
____ 35. The number of significant figures in the measurement 170.040 km is
a. 3.
c. 5.
b. 4.
d. 6.
____ 36. When should an MSDS (Material Safety Data Sheet) be consulted?
a. In case of fire or explosion.
c. In the event of a spill.
b. Before working with a chemical.
d. For all of the above.
____ 37. The number of significant figures in the measurement 210 cm is
a. 1.
c. 3.
b. 2.
d. 4.
____ 38. Written in scientific notation, the measurement 0.000 065 cm is
a. 65 x 10–4 cm.
c. 6.5 x 10–6 cm.
–5
b. 6.5 x 10 cm.
d. 6.5 x 10–4 cm.
____ 39. The measurement 0.020 L is the same as
a. 2.0 x 10–3 L.
c. 2.0 x 10–2 L.
2
b. 2.0 x 10 L.
d. 2.0 x 10–1 L.
____ 40. Expressed in scientific notation, 0.0930 m is
a. 93 x 10–3 m.
c. 9.30 x 10–2 m.
b. 9.3 x 10–3 m.
d. 9.30 x 10–4 m.
____ 41. ATOMIC STRUCTURE
According to Dalton's atomic theory, atoms
a. are destroyed in chemical reactions.
b. can be divided.
c. of each element are identical in size, mass, and other properties.
d. of different elements cannot combine.
____ 42. Who discovered the nucleus by bombarding gold foil with positively charged particles and noting
that some particles were widely deflected?
a. Rutherford
c. Chadwick
b. Dalton
d. Bohr
____ 43. With the use of your periodic table, the atomic number for aluminum is
a. 13
c. 26.98
b. 14
d. 26.9815
____ 44. Rutherford's experiments led to the discovery of the
a. electron.
c. nucleus.
b. cathode ray.
d. neutron.
____ 45. With the use of your periodic table, a neutral atom of silicon contains
a. 14 electrons
c. 16 electrons
b. 28.09 electrons
d. 38 electrons
____ 46. A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called
a(n)
a. nuclide.
c. electron.
b. neutron.
d. isotope.
____ 47. The nucleus of most atoms is composed of
a. tightly packed protons.
c. tightly packed protons and neutrons.
b. tightly packed neutrons.
d. tightly packed protons and electrons.
____ 48. Protons have
a. negative charges.
c. no charges.
b. positive charges.
d. no mass.
____ 49. An atom is electrically neutral because
a. neutrons balance the protons and electrons.
b. nuclear forces stabilize the charges.
c. the numbers of protons and electrons are equal.
d. the numbers of protons and neutrons are equal.
____ 50. Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
____ 51. The atomic number of oxygen, 8, indicates that there are
a. 8 energy levels.
b. 8 protons in the nucleus.
c. 4 protons and 4 neutrons in the nucleus.
d. 4 protons and 4 electrons in the nucleus.
____ 52. Isotopes of an element contain different numbers of
a. electrons.
c. neutrons.
b. protons.
d. nuclides.
____ 53. The total number of protons and neutrons in the nucleus of an atom is its
a. atomic number.
c. mass number.
b. Avogadro constant.
d. number of neutrons.
____ 54. All atoms of the same element have the same
a. atomic mass.
c. mass number.
b. number of neutrons.
d. atomic number.
____ 55. An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a. 13.
c. 27.
b. 14.
d. 40.
____ 56. An atom of potassium has 19 protons and 20 neutrons. What is its mass number?
a. 19
c. 39
b. 20
d. 10
____ 57. Zn-66 (atomic number 30) has
a. 30 neutrons.
c. 36 neutrons.
b. 33 neutrons.
d. 96 neutrons.
____ 58. Chlorine has atomic number 17 and mass number 35. It has
a. 17 protons, 17 electrons, and 18 neutrons.
b. 35 protons, 35 electrons, and 17 neutrons.
c. 17 protons, 17 electrons, and 52 neutrons.
d. 18 protons, 18 electrons, and 17 neutrons.
____ 59. Nickel-60 (atomic number 28) has
a. 28 neutrons.
c. 60 neutrons.
b. 32 neutrons.
d. 88 neutrons.
____ 60. Silicon-30 contains 14 protons. It also contains
a. 16 electrons.
c. 30 neutrons.
b. 16 neutrons.
d. 44 neutrons.
____ 61. Calcium-48 (atomic number 20) contains
a. 20 electrons.
c. 20 neutrons.
b. 48 protons.
d. 28 protons.
____ 62. An electrically neutral atom of mercury (atomic number 80) has
a. 80 neutrons and 80 electrons.
c. 80 protons and 80 neutrons.
b. 40 protons and 40 electrons.
d. 80 protons and 80 electrons.
____ 63. Henry Jenkins’ 2nd favorite element is iodine. There are 3 isotopes of iodine: 80% 127I, 17% 126I,
and 3% 128I. What is the average atomic mass of iodine?
a. 126.86 amu
c. 76.34 amu
b. 161.42 amu
d. 127 amu
____ 64. Henry Jenkins’ favorite element is nitrogen. There are 3 isotopes of nitrogen: 95% 14N, 3%
2% 16N. What is the average atomic mass of nitrogen?
a. 469 amu
c. 21 amu
b. 12.53 amu
d. 14.07 amu
____ 65. PERIODIC TABLE
Group ____ contains only metals.
a. 2
c. 17
b. 13
d. 18
____ 66. Which element has properties most similar to those of sodium?
a. boron
c. sulfur
b. calcium
d. nitrogen
____ 67. A horizontal row of blocks in the periodic table is called a(n)
a. group.
c. family.
b. period.
d. octet.
____ 68. The person whose work led to a periodic table based on increasing atomic number was
a. Moseley.
c. Rutherford.
b. Mendeleev.
d. Cannizzaro.
15
N, and
____ 69. Elements in a group or column in the periodic table can be expected to have similar
a. atomic masses.
c. numbers of neutrons.
b. atomic numbers.
d. properties.
____ 70. The elements that have properties of both metals and nonmetals are
a. inactive.
c. metalloids.
b. semi-metals.
d. nonmetals.
____ 71. To which group do lithium and potassium belong?
a. alkali metals
c. halogens
b. transition metals
d. noble gases
____ 72. To which group do fluorine and chlorine belong?
a. alkaline-earth metals
c. halogens
b. transition elements
d. actinides
____ 73. Which element has a larger atomic radius?
a. magnesium
c. rubidium
b. nitrogen
d. calcium
____ 74. A positive ion is known as a(n)
a. ionic radius.
c. cation.
b. valence electron.
d. anion
____ 75. The electrons available to be given away or stolen are called
a. ions.
c. d electrons.
b. valence electrons.
d. electron clouds.
____ 76. The elements that have properties of both metals and non-metals are
a. inactive.
c. metalloids.
b. semi-metals.
d. non-metals.
____ 77. What is the oxidation number for chlorine?
a. +1
c. +7
b. -1
d. -7
____ 78. What is the oxidation number for aluminum?
a. +3
c. +5
b. -3
d. -5
____ 79. What is the oxidation number for sulfur?
a. +2
c. +6
b. -2
d. -6
____ 80. The number of valence electrons for potassium is
a. 1.
c. 7.
b. 2.
d. 8.
____ 81. Which element requires less energy to remove valence electrons?
a. carbon
c. fluorine
b. sodium
d. boron
____ 82. Argon, krypton, and xenon are
a. alkaline earth metals.
c. actinides.
b. noble gases.
d. lanthanides.
____ 83. ELECTRON CONFIGURATION
The “p” orbitals are shaped like
a. flowers.
c. propellers.
b. circles.
d. spheres.
____ 84. The number of orbitals for the “d” sublevel is
a. 1.
c. 5.
b. 3.
d. 7.
____ 85. For the “f” sublevel, the TOTAL number of electrons is
a. 5.
c. 10.
b. 7.
d. 14.
____ 86. How many electrons can occupy the “s” orbitals at each energy level?
a. two, in opposite directions 
c. one 
b. two, in same direction 
d. no more than eight
____ 87. The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
a. Mg.
c. S.
b. C.
d. Si.
____ 88. What is the electron configuration for nitrogen?
a. 1s2 2s2 2p3
c. 1s2 2s3 2p1
2
3
2
b. 1s 2s 2p
d. 1s2 2s2 2p2 3s1
____ 89. Elements in which the “d” sublevel is being filled have the properties of
a. transition metals.
c. metalloids.
b. nonmetals.
d. halogens.
____ 90. Strontium's highest occupied energy level is 5s2. To what group does strontium belong?
a. Alkali Metals
c. Transition Metals
b. Alkaline Earth Metals
d. Halogens
____ 91. What is given off when an electron falls back down to a lower energy level?
a. electrons
c. protons
b. light
d. elements
____ 92. Based on the location of the element, nitrogen, how many more electrons does nitrogen need to be
stable like the noble gases?
a. 1
c. 5
b. 3
d. 8
____ 93. COVALENT BONDING
Name the compound CF4.
a. calcium fluoride
c. carbon tetrafluoride
b. carbon fluoride
d. monocarbon quadrafluoride
____ 94. What is the formula for diphosphorous pentoxide?
a. P2PeO5
c. P2O4
b. PO5
d. P2O5
____ 95. What is the formula for silicon dioxide?
a. SO2
c. Si2O
b. SiO2
d. S2O
____ 96. Draw the Lewis Dot Sharing for PBr3. What type of bonds are formed in this compound?
a. 2 single bonds
c. 1 triple bond
b. 3 single bonds
d. 3 triple bonds
____ 97. Draw the Lewis Dot Sharing for O2. What type of bonds are formed in this compound?
a. 2 single bonds
c. 1 double bond
b. 1 triple bond
d. 2 double bonds
____ 98. Name the compound N2O4.
a. binitrogen tetraoxide.
c. dinitrogen quadraoxide.
b. dinitride tetraoxide.
d. dinitrogen tetraoxide
____ 99. Name the compound P3Cl6.
a. triphosphorus heptachloride
c. triphosphide hexachloride
b. triphosphorus hexachloride
d. triphosphorus pentachloride
____100. Which of the following statements is an observation?
a. It was raining while Henry Jenkins was at the movies.
b. Henry Jenkins liked the movie he watched at the theater.
c. Henry Jenkins leaves the movie theater and sees that the ground is wet.
d. The sprinklers flooded the street while Henry Jenkins was at the movies.