Download ExamView - Chapter 4 Test.tst

Name: ________________________ Class: ___________________ Date: __________
ID: A
Chapter 4 Test
Matching - 2pts each
Match each item with the correct statement below.
a. proton
d. electron
b. nucleus
e. neutron
c. atom
____
____
____
____
____
1.
2.
3.
4.
5.
the smallest particle of an element that retains the properties of that element
a positively charged subatomic particle
a negatively charged subatomic particle
a subatomic particle with no charge
the central part of an atom, containing protons and neutrons
Match each item with the correct statement below.
a. mass number
d. atomic mass
b. atomic mass unit
e. isotope
c. atomic number
____ 6.
____ 7.
____ 8.
____ 9.
____ 10.
atoms with the same number of protons, but different numbers of neutrons in the nucleus of an atom
the total number of protons and neutrons in the nucleus of an atom
the number of protons in the nucleus of an element
the weighted average of the masses of the isotopes of an element
one-twelfth the mass of a carbon atom having six protons and six neutrons
Multiple Choice - 2pts each
Identify the choice that best completes the statement or answers the question.
____ 11. Who was the man who lived from 460B.C.–370B.C. and was among the first to suggest the idea of atoms?
a. Atomos
c. Democritus
b. Dalton
d. Thomson
____ 12. Which of the following was NOT among Democritus’s ideas?
a. Matter consists of tiny particles called atoms.
b. Atoms are indivisible.
c. Atoms retain their identity in a chemical reaction.
d. Atoms are indestructible.
____ 13. The smallest particle of an element that retains the properties of that element is a(n) ____.
a. atom
c. proton
b. electron
d. neutron
____ 14. Which of the following is NOT a part of Dalton's atomic theory?
a. All elements are composed of atoms.
b. Atoms are always in motion.
c. Atoms of the same element are identical.
d. Atoms that combine do so in simple whole-number ratios.
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Name: ________________________
ID: A
____ 15. 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.
____ 16. 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
____ 17. 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
____ 18. The nucleus of an atom is ____.
a. the central core and is composed of protons and neutrons
b. positively charged and has more protons than neutrons
c. negatively charged and has a high density
d. negatively charged and has a low density
____ 19. 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
____ 20. The sum of the protons and neutrons in an atom equals the ____.
a. atomic number
c. atomic mass
b. nucleus number
d. mass number
____ 21. All atoms of the same element have the same ____.
a. number of neutrons
c. mass numbers
b. number of protons
d. mass
____ 22. Isotopes of the same element have different ____.
a. numbers of neutrons
c. numbers of electrons
b. numbers of protons
d. atomic numbers
____ 23. Which of the following statements is NOT true?
a. Atoms of the same element can have different masses.
b. Atoms of isotopes of an element have different numbers of protons.
c. The nucleus of an atom has a positive charge.
d. Atoms are mostly empty space.
____ 24. 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.
____ 25. In which of the following is the number of neutrons correctly represented?
a. 199 F has 0 neutrons.
c. 24
Mg has 24 neutrons.
12
b.
75
As
33
has 108 neutrons.
d.
2
238
U
92
has 146 neutrons.
Name: ________________________
ID: A
____ 26. 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
____ 27. Which of the following isotopes has the same number of neutrons as phosphorus-31?
P
c. 29
Si
a. 32
15
14
b.
32
S
16
d.
28
Si
14
____ 28. What unit is used to measure weighted average atomic mass?
a. amu
c. angstrom
b. gram
d. nanogram
____ 29. Which of the following equals one atomic mass unit?
a. the mass of one electron
b. the mass of one helium-4 atom
c. the mass of one carbon-12 atom
d. one-twelfth the mass of one carbon-12 atom
____ 30. Why do chemists use relative masses of atoms compared to a reference isotope rather than the actual masses
of the atoms?
a. The actual mass of an electron is very large compared to the actual mass of a proton.
b. The actual masses of atoms are very small and difficult to work with.
c. The number of subatomic particles in atoms of different elements varies.
d. The actual masses of protons, electrons, and neutrons are not known.
Short Answer - 5pts each
31. List the number of protons, neutrons, and electrons in
13
C.
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32. Chlorine has two naturally occurring isotopes, Cl-35 and Cl-37. The atomic mass of chlorine is 35.45. Which
of these two isotopes of chlorine is more abundant?
33. The element chromium has four naturally occurring isotopes. Use the relative abundance of each to calculate
the average atomic mass of chromium.
50
Cr = 4.34%,
52
Cr = 83.79%,
53
Cr = 9.50%,
54
Cr = 2.37%.
Figuring Out the Atom - 1pt each
34. Fill in the following table with the correct numbers or elements:
Element
Mass Number
Protons
Electrons
Carbon
Neutrons
13
15
7
Sulfur
20
22
25
37
17
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Name: ________________________
ID: A
Essay - 10pts (1 for having 3 sentences, 1 for spelling/grammar, 8 for the correct response)
35. In what way are two isotopes of the same element different? Explain why isotopes of the same element have
the same chemical behavior.
Bonus - 10pts (no partial credit)
36. Chlorine has two naturally occuring isotopes. Chlorine-35 has an atomic mass of 34.969 amu. Chlorine-37
has an atomic mass of 36.966 amu. If the average atomic mass of chlorine is 35.453 amu, what is the natural
abundance of chlorine-37?
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