Download CHEMISTRY Test 3: Atomic Structure

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CHEMISTRY Test 3: Atomic Structure
Multiple Choice (1.6 points each) Identify the letter of the choice that best completes the statement or answers the
question.
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1. According to the law of definite proportions, any two samples of KCl have
a. the same mass.
c. the same melting point.
b. slightly different molecular structures.
d. the same ratio of elements.
____
2. Which of the following statements is true?
a. Atoms of the same element may have different masses.
b. Atoms may be divided in ordinary chemical reactions.
c. Atoms can never combine with any other atoms.
d. Matter is composed of large particles called atoms.
____
3. A positively charged particle with mass 1.673 × 10–24 g is a(n)
a. proton.
c. electron.
b. neutron.
d. positron.
____
4. 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.
____
5. The nucleus of an atom has all of the following characteristics EXCEPT that it
a. is positively charged.
c. contains nearly all of the atom's mass.
b. is very dense.
d. contains nearly all of the atom's volume.
____
6. The mass of a neutron is
a. about the same as that of a proton.
b. about the same as that of an electron.
c.
d.
double that of a proton.
double that of an electron.
7. The nucleus of most atoms is composed of
a. tightly packed protons.
b. tightly packed neutrons.
c.
d.
tightly packed protons and neutrons.
loosely connected protons and electrons.
8. Protons have
a. negative charges.
b. an attraction for neutrons.
c.
d.
no charges.
no mass.
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____
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9. 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.
____ 10. Most of the volume of an atom is occupied by the
a. nucleus.
c.
b. nuclides.
d.
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electron cloud.
protons.
ID: A
____ 11. The charge on the electron cloud
a. prevents compounds from forming.
b. balances the charge on the nucleus.
c. attracts electron clouds in other atoms to form compounds.
d. does not exist.
____ 12. The smallest unit of an element that can exist either alone or in combination with other such particles of the
same or different elements is the
a. electron.
c. neutron.
b. proton.
d. atom.
____ 13. Isotopes are atoms of the same element that have different
a. principal chemical properties.
c. numbers of protons.
b. masses.
d. numbers of electrons.
____ 14. Atoms of the same element that have different masses are called
a. moles.
c. nuclides.
b. isotopes.
d. neutrons.
____ 15. Isotopes of an element contain different numbers of
a. electrons.
c. neutrons.
b. protons.
d. nuclides.
____ 16. All isotopes of hydrogen contain
a. one neutron.
b. two electrons.
c.
d.
one proton.
two nuclei.
____ 17. Helium-4 and helium-3 are
a. isotopes.
b. different elements.
c.
d.
compounds.
nuclei.
____ 18. The atomic number of oxygen, 8, indicates that there are eight
a. protons in the nucleus of an oxygen atom.
b. oxygen nuclides.
c. neutrons outside the oxygen atom's nucleus.
d. energy levels in the oxygen atom's nucleus.
____ 19. 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.
____ 20. As the mass number of the isotopes of an element increases, the number of protons
a. decreases.
b. increases.
c. remains the same.
d. doubles each time the mass number increases.
____ 21. All atoms of the same element have the same
a. atomic mass.
c.
b. number of neutrons.
d.
2
mass number.
atomic number.
ID: A
____ 22. Atoms of the same element can differ in
a. chemical properties.
b. mass number.
c.
d.
atomic number.
number of protons and electrons.
____ 23. The relative atomic mass of an atom can be found by comparing the mass of the atom to the mass of
a. one atom of carbon-12.
c. a proton.
b. one atom of hydrogen-1.
d. uranium-235.
____ 24. The average atomic mass of an element is the average of the atomic masses of its
a. naturally occurring isotopes.
c. nonradioactive isotopes.
b. two most abundant isotopes.
d. artificial isotopes.
____ 25. The average atomic mass of an element
a. is the mass of the most abundant isotope.
b. may not equal the mass of any of its isotopes.
c. cannot be calculated.
d. always adds up to 100.
____ 26. The atomic mass listed in the periodic table is the
a. average atomic mass.
b. relative atomic mass of the most abundant isotope.
c. relative atomic mass of the most stable radioactive isotope.
d. mass number of the most abundant isotope.
____ 27. An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a. 13.
c. 27.
b. 14.
d. 40.
____ 28. Zn-66 (atomic number 30) has
a. 30 neutrons.
b. 33 neutrons.
c.
d.
36 neutrons.
96 neutrons.
____ 29. Ag-109 has 62 neutrons. The neutral atom has
a. 40 electrons.
c.
b. 47 electrons.
d.
53 electrons.
62 electrons.
____ 30. Carbon-14 (atomic number 6), the radioactive nuclide used in dating fossils, has
a. 6 neutrons.
c. 10 neutrons.
b. 8 neutrons.
d. 14 neutrons.
____ 31. Silicon-30 contains 14 protons. It also contains
a. 16 electrons.
c.
b. 16 neutrons.
d.
30 neutrons.
44 neutrons.
____ 32. Neon-22 contains 12 neutrons. It also contains
a. 12 protons.
c.
b. 22 protons.
d.
22 electrons.
10 protons.
____ 33. The part of the atom where the electrons CANNOT be found is the
a. area surrounding the nucleus.
c. electron cloud.
b. nucleus.
d. orbitals.
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ID: A
____ 34. How many quantum numbers are needed to describe the energy state of an electron in an atom?
a. 1
c. 3
b. 2
d. 4
____ 35. The possible values of an electron's spin quantum number are
a. –1, 0, or 1.
c. +1 or –1.
b.
1
1
+ 2 or − 2
d.
0 or 1.
____ 36. The number of sublevels within each energy level of an atom is equal to the value of the
a. principal quantum number.
c. magnetic quantum number.
b. angular momentum quantum number.
d. spin quantum number.
____ 37. What values can the angular momentum quantum number have when n = 2?
1
1
a.
+ 2 ,− 2
b.
− 2 ,− 1,− 2
1
c.
0, 1, 2
d.
0, 1
____ 38. The spin quantum number indicates that the number of possible states for an electron in an orbital is
a. 1.
c. 3.
b. 2.
d. 5.
____ 39. The spin quantum number of an electron can be thought of as describing
a. the direction of electron spin.
b. whether the electron's charge is positive or negative.
c. the electron's exact location in orbit.
d. the number of revolutions the electron makes about the nucleus per second.
____ 40. The set of orbitals that are dumbbell-shaped and directed along the x, y, and z axes are called
a. d orbitals.
c. f orbitals.
b. p orbitals.
d. s orbitals.
____ 41. A spherical electron cloud surrounding an atomic nucleus would best represent
a. an s orbital.
c. a combination of p x and p y orbitals.
b. a p x orbital.
d. a combination of an s and a p x orbital.
____ 42. The major difference between a 1s orbital and a 2s orbital is that
a. the 2s orbital can hold more electrons.
b. the 2s orbital has a slightly different shape.
c. the 2s orbital is at a higher energy level.
d. the 1s orbital can have only one electron.
____ 43. The p orbitals are shaped like
a. electrons.
b. circles.
c.
d.
dumbbells.
spheres.
____ 44. An orbital that could never exist according to the quantum description of the atom is
a. 3d.
c. 6d.
b. 8s.
d. 3f.
____ 45. The number of possible orbital shapes for the third energy level is
a. 1.
c. 3.
b. 2.
d. 4.
4
ID: A
____ 46. The number of orbitals for the d sublevel is
a. 1.
b. 3.
c.
d.
____ 47. For n = 4, the number of possible orbital shapes is
a. 1.
c.
b. 4.
d.
5.
7.
16.
32.
____ 48. How many orientations can an s orbital have about the nucleus?
a. 1
c. 3
b. 2
d. 5
____ 49. How many electrons can occupy the s orbitals at each energy level?
a. two, if they have opposite spins
c. one
b. two, if they have the same spin
d. no more than eight
____ 50. If n is the principal quantum number of a main energy level, the number of electrons in that energy level is
a. n.
c. n 2 .
b. 2n.
d. 2n 2 .
____ 51. How many electrons are needed to completely fill the fourth energy level?
a. 8
c. 32
b. 18
d. 40
____ 52. The atomic sublevel with the next highest energy after 4p is
a. 4d.
c. 5p.
b. 4f.
d. 5s.
____ 53. The element with electron configuration 1s2 2s2 2p 6 3s2 3p 2 is
a. Mg (Z = 12).
c. S (Z = 16).
b. C (Z = 6).
d. Si (Z = 14).
____ 54. The electron configuration for the carbon atom (C) is 1s2 2s2 2p 2 . The atomic number of carbon is
a. 3.
c. 11.
b. 6.
d. 12.
____ 55. What is the electron configuration for nitrogen, atomic number 7?
a. 1s2 2s2 2p 3
c. 1s2 2s3 2p 1
b. 1s2 2s3 2p 2
d. 1s2 2s2 2p 2 3s1
____ 56. The electron notation for aluminum (atomic number 13) is
a. 1s2 2s2 2p 3 3s2 3p 3 3d 1 .
c. 1s2 2s2 2p 6 3s2 3p 1 .
2
2
6
2
1
b. 1s 2s 2p 3s 2d .
d. 1s2 2s2 2p 9 .
____ 57. If the s and p orbitals of the highest main energy level of an atom are filled with electrons, the atom has a(n)
a. electron pair.
c. ellipsoid.
b. octet.
d. circle.
____ 58. These subatomic particles determine how the atoms of an element will behave chemically
a. proton
c. electron
b. neutron
d. valence electron
5
ID: A
____ 59. This subatoic particle that determines which isotope of an element the atom is:
a. proton
c. electron
b. neutron
d. valence electron
____ 60. How is an electron's principal quantum number symbolized?
a. s
c. n
b. p
d. d
6
ID: A
CHEMISTRY Test 3: Atomic Structure
Answer Section
MULTIPLE CHOICE
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