Download CHEMISTRY TEST #1 REVIEW FALL 2012

CHEMISTRY TEST #1 REVIEW
FALL 2012
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
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1. Which of the following is true about subatomic particles?
a. Electrons are negatively charged and are the heaviest subatomic particle.
b. Protons are positively charged and the lightest subatomic particle.
c. Neutrons have no charge and are the lightest subatomic particle.
d. The mass of a neutron nearly equals the mass of a proton.
2. All atoms are ____.
a. positively charged, with the number of protons exceeding the number of electrons
b. negatively charged, with the number of electrons exceeding the number of protons
c. neutral, with the number of protons equaling the number of electrons
d. neutral, with the number of protons equaling the number of electrons, which is equal to the
number of neutrons
3. The atomic number of an element is the total number of which particles in the nucleus?
a. neutrons
c. electrons
b. protons
d. protons and electrons
4. What does the number 84 in the name krypton-84 represent?
a. the atomic number
c. the sum of the protons and electrons
b. the mass number
d. twice the number of protons
5. Isotopes of the same element have different ____.
a. numbers of neutrons
c. numbers of electrons
b. numbers of protons
d. atomic numbers
6. In which of the following sets is the symbol of the element, the number of protons, and the number of
electrons given correctly?
a. In, 49 protons, 49 electrons
c. Cs, 55 protons, 132.9 electrons
b. Zn, 30 protons, 60 electrons
d. F, 19 protons, 19 electrons
7. Using the periodic table, determine the number of neutrons in O.
a. 4
c. 16
b. 8
d. 24
8. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125
contain?
a. 50 protons, 50 electrons, 75 neutrons
c. 120 neutrons, 50 protons, 75 electrons
b. 75 electrons, 50 protons, 50 neutrons
d. 70 neutrons, 75 protons, 50 electrons
9. If E is the symbol for an element, which two of the following symbols represent isotopes of the same
element?
1. E
2. E
3. E
4. E
a. 1 and 2
c. 1 and 4
b. 3 and 4
d. 2 and 3
____ 10. Which of the following sets of symbols represents isotopes of the same element?
a.
c.
J
J
J
M
M
M
b.
d.
L
L
L
Q
Q
Q
____ 11. How is the number of neutrons in the nucleus of an atom calculated?
a. Add the number of electrons and protons together.
b. Subtract the number of electrons from the number of protons.
c. Subtract the number of protons from the mass number.
d. Add the mass number to the number of electrons.
____ 12. In which of the following is the number of neutrons correctly represented?
a.
c.
F has 0 neutrons.
Mg has 24 neutrons.
b.
d.
As has 108 neutrons.
U has 146 neutrons.
____ 13. Which of the following isotopes has the same number of neutrons as phosphorus-31?
a.
c.
P
Si
b.
d.
S
Si
____ 14. The atomic mass of an element depends upon the ____.
a. mass of each electron in that element
b. mass of each isotope of that element
c. relative abundance of protons in that element
d. mass and relative abundance of each isotope of that element
____ 15. The particles that are found in the nucleus of an atom are ____.
a. neutrons and electrons
c. protons and neutrons
b. electrons only
d. protons and electrons
____ 16. An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the
element are ____.
a. 152 protons and 76 electrons
c. 38 protons and 38 electrons
b. 76 protons and 0 electrons
d. 76 protons and 76 electrons
____ 17. The sum of the protons and neutrons in an atom equals the ____.
a. atomic number
c. atomic mass
b. nucleus number
d. mass number
____ 18. All atoms of the same element have the same ____.
a. number of neutrons
c. mass numbers
b. number of protons
d. mass
____ 19. Isotopes of the same element have different ____.
a. positions on the periodic table
c. atomic numbers
b. chemical behavior
d. mass numbers
____ 20. The mass number of an element is equal to ____.
a. the total number of electrons in the nucleus
b. the total number of protons and neutrons in the nucleus
c. less than twice the atomic number
d. a constant number for the lighter elements
____ 21. Which of the following elements is in the same period as phosphorus?
a. carbon
c. nitrogen
b. magnesium
d. oxygen
____ 22. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. Pt
c. Li
b. V
d. Kr
____ 23. Which of the following elements is a transition metal?
a. cesium
c. tellurium
b. copper
d. tin
____ 24. The elements in Groups 3 through 12 of the periodic table are the ____.
a. actinides
c. transition elements
b. alkaline earth metals
d. halogens
____ 25. Three transition elements in Group 12 of the periodic table are ____.
a. copper, silver, and gold
c. mercury, zinc, and cadmium
b. iron, nickel, and cobalt
d. neon, helium, and xenon
____ 26. The noble gases are in ____.
a. Group 18
c. Group 13
b. Group 1
d. Group 2
____ 27. Elements that lie along the stair-step line of the periodic table are ____.
a. liquids
c. metalloids
b. metals
d. radioactive
____ 28. In Bohr's model of the atom, where are the electrons and protons located?
a. The electrons move around the protons, which are at the center of the atom.
b. The electrons and protons move throughout the atom.
c. The electrons occupy fixed positions around the protons, which are at the center of the
atom.
d. The electrons and protons are located throughout the atom, but they are not free to move.
____ 29. In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a. position
b. color
c. energy
d. size
____ 30. How does the energy of an electron change when the electron moves closer to the nucleus?
a. It decreases.
b. It increases.
c. It stays the same.
d. It doubles.
____ 31. Dalton's atomic theory included which idea?
a. All atoms of all elements are the same size.
b. Atoms of different elements always combine in one-to-one ratios.
c. Atoms of the same element are always identical.
d. Individual atoms can be seen with a microscope.
____ 32. Which of the following was originally a part of Dalton's atomic theory, but had to be revised about a century
ago?
a. Atoms of different elements are different.
b. Atoms of the same element are identical.
c. Compounds are made by combining atoms.
d. Atoms of different elements can combine with one another in simple whole number ratios.
Short Answer
33. List the number of protons, neutrons, and electrons in
C.
34. Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the
isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0%
abundant. What is the average atomic mass for element Z?
35. A fictitious element X is composed of 10.0 percent of the isotope
, 20.0 percent of the isotope
70.0 percent of the isotope
. Estimate the atomic mass of element X.
, and
36. The element chromium has four naturally occurring isotopes. Use the relative abundance of each to calculate
the average atomic mass of chromium.
Cr = 4.34%,
Cr = 83.79%,
Cr = 9.50%,
Cr = 2.37%.
37. Which group of elements in the periodic table is known as the alkali metals?
38. Which group in the periodic table is known as the noble gases?
Numeric Response
39. Use the periodic table to determine the number of electrons in a neutral atom of lithium.
40. Use the periodic table to determine the number of protons in an atom of barium.
41. How many protons are present in an atom of Be-9?
42. What is the total number of subatomic particles in the nucleus of an atom of
Bi?
43. Determine the number of electrons in an atom of iridium.
44. What is the atomic number for an element with 41 neutrons and a mass number of 80?
45. How many electrons are in an atom of gold?
46. What is the mass number for an oxygen atom that has 10 neutrons in its nucleus?
47. How many protons are present in the nuclei of the three known isotopes of hydrogen?
48. Use the periodic table to determine the number of neutrons in nitrogen-14.
49. How many neutrons are present in an atom of the isotope
50. Calculate the number of neutrons in
Pb.
U?