Download What is the smallest particle of an element that retains the properties

CHAPTER 3 TEST REVIEW
NAME______________________________
1. What is the smallest particle of an element that retains the properties of that element?
2. What particles form the nucleus of an atom?
3. T or F. Electrons are positively charged and are the lightest of the three subatomic particles.
4. Which subatomic particle has a +1 charge? Which has a 0 charge?
5. In Rutherford’s gold foil experiment, most of the positively charged particles which he shot at the foil
________________, while a very small percentage of the positively charged particles _________________.
a) passed right through the foil / were deflected
b) were deflected / passed right through the foil
6. Rutherford’s gold foil experiment confirmed the existence of...
a) a massive negatively charged nucleus
b) massive positively charged electrons
c) a massive positively charged nucleus
d) all of these
9. Thomson first suggested the existence of _______________, while Bohr first suggested the idea of
______________.
a) energy levels, electrons
b) electrons, energy levels
c) the nucleus, neutrons
11. A neutral atom always has the same number of ___________ and ___________.
12. The atomic number is the total number of which particles in the nucleus?
13. High energy light has a _________ frequency.
a) low
b) high
c) inconsistent
14. Light which has a very high energy has a very _______ wavelength and _______ frequency.
a) short/low b) long/low c) short/high d) long/high
15. The oxide ion has a charge of –2. Therefore it has 8 protons and ______ electrons.
a) 9
b) 8
c) 10
d) 12
e) 7
f) 6
16. An atom of helium-4 contains…
a) one proton
b) 2 electrons
c) no neutrons
d) all of these
17. The number “16” in oxygen-16 represents the…
18. Average atomic mass is measured in…
19. All atoms of the same element have the same…
a) number of neutrons
b) mass numbers
c) masses
d) number of protons
20. By definition, the atomic mass unit is based on what isotope?
a) carbon-14
b) carbon-13
c) carbon-12
d) oxygen-16
24. Phosphorus-31 has ______ neutrons.
25. T or F. As a whole, the atom is primarily made up of empty space.
e) hydrogen-1
26. Element Z has 2 naturally occurring isotopes with the following percent abundances: the isotope with a
mass of 20.0 amu is 75% abundant, while the isotope with a mass of 22.0 amu is 25% abundant. What is the
average atomic mass for element Z?
a) 20.0 amu
b) 20.5 amu
c) 21.0 amu
d) 21.5 amu
e) 22.0 amu
27. Which subatomic particle is most important in determining the chemical properties of an element?
a) electrons
b) neutrons
c) protons
d) croutons
MATCHING: NUMBERS 28 - 31
28. Orbital
a) a depiction of the electron arrangement of an atom
29. Aufbau Principle
b) a region where an electron is located
30. Electron Configuration
c) each orbital can contain 2 electrons at most
31. Pauli Exclusion Principle
d) tendency of electrons to enter orbitals of lowest energy first
32. Which of the following elements is in the same period as Cl on the periodic table?
a) C
b) Mg
c) N
d) O
e) Bi
33. Which of the following elements is in the same group as As on the periodic table?
a) C
b) Mg
c) N
d) O
e) Ar
35. T or F. Neon lights give off light when electrons rise from lower energy levels to higher energy levels.
36. How might you excite electrons of an element so that they move up to higher energy levels?
a) heat the element
b) pass an electrical current over the element
c) both a & b
37. T or F. Electrons travel around the nucleus in well defined paths called orbits, much like the earth
travels around the sun.
39. Outer electron configurations (battleship configurations) show only the electrons in the _____________
energy levels.
40. In the orbital diagram of Boron (B), how many electrons are unpaired in the 2p sublevel?
a) 1
b) 2
c) 3
d) 4
e) 0
42. What sublevels are present in the third energy level?
a) s only
b) s and p only
c) s, p, and d only
d) s, p, d, and f
43. The noble gases are found in group ___ on the periodic table.
44. How many electrons can fit into any “f” orbital?
45. How many electrons can fit into any “d” sublevel?
46. T or F. Stable electron configurations are likely to include completely filled outer electron
configurations, like those present in noble gases.
47. If an atom of phosphorus were to gain 3 electrons, its new electron configuration would match the
configuration of______________________.
48. How many electrons would Mg have to lose in order to have an electron configuration identical to its
nearest noble gas?
53. The elements of group 17 tend to attain what charge when they form ions?
54. The elements of group 18 tend to attain what charge when they form ions?
55. When elements in the s and p blocks form ions by gaining or losing electrons, they attain the same
electron configuration as the nearest…
59. Magnetic metals have unpaired electrons. Which of the following metals would be least magnetic?
a) K
b) Zn
c) Na
d) Mn
60. What would have to happen in order to change an atom of Aluminum-27 into an atom of
Magnesium-24?
61. What is the shorthand configuration of At?
62. What is the valence configuration of At?
63. What element has the valence configuration 4s2 4p5?
64. What is the name of the particles that make up protons and neutrons?
65. In modern atomic theory, what does the term fundamental mean?
66. Which particles are fundamental? (choose more than one if necessary)
a) atoms
b) protons
c) neutrons
d) electrons e) quarks
67. Write a short paragraph describing the atom in detail. Use the words in the word bank at least once, and
underline them as you use them.
(HINT: This question will appear on the free response test word for word as it appears right here!!!)
Word bank:
atom nucleus
orbital quarks
proton neutron
electron
positive charge
mass number atomic number charge
negative charge
energy level