SI Worksheet 4
1. Which of the following is NOT a part of Dalton’s Atomic Theory?
a. Atoms cannot be created or destroyed.
b. Atoms of one element are different from atoms of any other element.
c. Atoms are composed of protons, neutrons, and electrons.
d. Atoms of one element may combine with atoms of other elements to form
chemical compounds.
2. Which subatomic particle of an atom contains a negative charge?
a. Proton
b. Neutron
c. Electron
d. Both B and C
3. Which subatomic particles mainly account for the atom’s mass and are located in the
nucleus of the atom?
a. Protons and neutrons
b. Neutrons and electrons
c. Electrons and protons
d. Protons, neutrons, and electron
4. Atoms become ions when they:
a. Lose or gain electrons
b. Lose or gain protons
c. Lose or gain neutrons
d. Lose or gain kinetic energy
5. On a periodic table, columns are ____ and rows are ____.
a. Periods; groups
b. Metal; nonmetal
c. Nonmetal; metal
d. Groups; periods
6. Cadmium (Cd) is a(n) ______.
a. Alkali metal
b. Alkaline-earth metal
c. Transition element
d. Noble gas
7. Where are the halogens located on the periodic table?
a. Group 2A
b. Group 7A
c. Period 2
d. Period 7
8. According to Thompson’s “plum pudding” model of the atom, what where the charges of
the different parts?
a. Negative “plums” and positive “pudding”
b. Neutral “plums” and negative “pudding”
c. Positive “plums” and neutral “pudding”
d. Positive “plums” and negative “pudding”
9. What is the difference between Thompson’s “plum pudding” model and Rutherford’s
atomic model?
a. Thompson’s model contains a nucleus, while Rutherford’s does not.
b. Rutherford’s model contains proton “plums” dispersed throughout an electron
“pudding”, while Thompson’s was the opposite.
c. The nucleus contained a majority of the atom’s volume in Rutherford’s model.
d. Electrons are randomly distributed in Thompson’s model, unlike Rutherford’s.
10. The atomic number of Bismuth is 83, and its mass number is 209. How many protons,
neutrons, and electrons does it contain?
a. 83 p, 83 n, 83 eb. 83 p, 126 n, 83 ec. 83 p, 83 n, 126 ed. 126 p, 83 n, 126 e11. Isotopes have a different _____ number because of a change in the number of _____.
a. Mass; protons
b. Atomic; electrons
c. Atomic; neutrons
d. Mass; neutrons
12. Which nuclear symbol and name is correct for an isotope of potassium with 22 neutrons?
a. 41P; potassium-41
b. 41K; potassium-41
c. 22K; potassium-22
d. 19K; potassium-41
13. What is the nuclear symbol for an atom with 74 p, 112 n, and 74 e-?
a. 112W
b. 186Th
c. 74W
d. 186W
14. One carbon-12 atom equals how many amu?
a. 1 amu
b. 12 amu
c. 6 amu
d. 100 amu
15. What is the formula for finding the atomic mass of an atom?
a. Σ[(Mass number of isotope) x (% abundance)]
b. Σ[(Atomic number of isotope) x (Mass number of isotopes)]
c. Σ[(Atomic mass of isotope) x (% abundance)]
d. y = mx + b
16. Selenium has the naturally occurring isotopes 74Se at 0.89% (73.9225 amu), 76Se at
9.37% (75.9192 amu), 77Se at 7.63% (76.9192 amu), 78Se at 23.77% (77.9173 amu), 80Se
at 49.61% (79.9165 amu), and 82Se at 8.73% (81.9167 amu). What is the atomic mass of
selenium?
a. 78.96 amu
b. 7896 amu
c. 79.86 amu
d. 77.75 amu
17. On an EM spectrum, the _____ the energy, the _____ the wavelength.
a. Lower; shorter
b. Brighter; more unpredictable
c. Colder; shorter
d. Higher; shorter
18. What is the order of the colors of the rainbow from highest energy to lowest?
a. Red, orange, yellow, green, blue, indigo, violet
b. Violet, blue, yellow, red, indigo, green, orange
c. Violet, indigo, blue, green, yellow, orange, red
d. White, red, orange, yellow, green, blue, indigo, violet, black
19. Which does not describe electron energy levels?
a. Energy levels decrease in energy as n increases.
b. Electrons with the lowest energy level are closest to the nucleus.
c. Space between energy levels decreases with each higher level.
d. Energy levels are labeled n = 1, n = 2, n = 3, and so on.
20. What is the maximum number of electrons the d sublevel can contain?
a. 6
b. 2
c. 10
d. 14
21. List the sublevels in order of highest to lowest energy.
a. S, p, d, f
b. F, d, s, p
c. A, b, c, d
d. F, d, p, s
22. How many electrons can an orbital hold?
a. 2
b. 3
c. 5
d. 8
23. Which orbital has a two-lobed shape and can be arranged on the x, y, and z axes around
the nucleus (3 maximum)?
a. S orbital
b. P orbital
c. D orbital
d. F orbital
24. What is the electron configuration of copper?
a. 1s2 2s2 2p6 3s2 3p6 4s1 3d10
b. 1s2 2s2 2p2
c. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p2
d. 1s2 2s2 3s2
25. How many electrons are unpaired in the electron configuration of copper?
a. 0
b. 1
c. 2
d. 3
26. What is the abbreviated configuration for copper?
a. 1s2 2s2 2p6 3s2 3p6 4s1 3d10
b. [Ar] 4s2 3d9
c. [Ne] 3s2 3p6 3d8 4s2
d. [Ar] 4s1 3d10
27. How many valence electrons does lead have?
a. 4
b. 5
c. 2
d. 8
28. How many of those electrons are paired (on the same side)?
a. 0
b. 1
c. 2
d. 3
29. Atomic size _____ across a period and _____ down a group.
a. Increases; increases
b. Increases; decreases
c. Decreases; decreases
d. Decreases; increases
30. Ionization energy _____ across a period and _____ down a group.
a. Increases; increases
b. Increases; decreases
c. Decreases; decreases
d. Decreases; increases