Light and Electrons Practice Quiz Chem 1
1. How many valence electrons are found in the atom Mg. a) 1 b) 2 c) 5 d) 8
2. How many electrons can the second energy level hold a) 1 b) 2 c) 5 d) 8
3. As it travels through space, electromagnetic radiation a) exhibits wavelike behavior. b) loses energy. c) varies in speed. d) releases photons.
4. If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B the wavelength of A is a) longer. b) shorter. c) equal. d) exactly half the length of B's wavelength.
5. The distance between two successive peaks on a wave is its a) frequency. b) wavelength. c) quantum number. d) velocity.
6. A quantum of electromagnetic energy is called a(n) a) photon. b) electron. c) excited atom. d) orbital.
7. A line spectrum is produced when an electron moves from one energy level a) to a higher energy level. b) to a lower energy level. c) into the nucleus. d) to another position in the same sublevel.

8. A bright-line spectrum of an atom is caused by the energy released when electrons a) jump to a higher energy level. b) fall to a lower energy level c) absorb energy and jump to a higher energy level. d) absorb energy and fall to a lower energy level.
9. Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen a) had no electrons. b) did not release photons. c) released photons of only certain energies. d) could only exist in the ground state.
10. The Bohr model of the atom was an attempt to explain hydrogen's a) density b) flammability. c) mass. d) line-emission spectrum.
11. Bohr's model of the atom works best in explaining a) the spectra of the first ten elements. b) only the spectrum of hydrogen c) only the spectra of atoms with electrons in an "s" orbital. d) the entire visible spectra of atoms.
12. The change of an atom from an excited state to the ground state always requires a) absorption of energy. b) emission of electromagnetic radiation. c) release of visible light. d) an increase in electron energy.
13. Which model of the atom explains why excited hydrogen gas gives off certain colors of light? a) the Bohr model b) the quantum model c) Rutherford's model d) Planck's theory
14. Which model of the atom explains the orbitals of electrons as waves? a) the Bohr model b) the quantum model c) Rutherford's model d) Planck's theory

15. Unlike in an orbit, in an orbital a) an electron's position cannot be known precisely. b) an electron has no energy. c) electrons cannot be found. d) protons cannot be found.
16. 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.
17. The shape of an "s" orbital is: a) spherical b) dumbbell shaped c) donut shaped d) conical shaped e) none of these
18. The shape of a "p" orbital is: a) spherical b) donut shaped c) can hold more than two electrons d) dumbbells e) none of these
19. The maximum number of electrons allowed in each of the "p" orbitals is: a) 2 b) 4 c) 8 d) 18 e) none of these
20. A given set of "d" orbitals consists of ______ orbitals. a) 1 b) 3 c) 5 d) 6 e) none of these
21. The maximum number of electrons allowable in the "d" sublevel of the 3rd principal level is: a) 2 b) 4 c) 8 d) 18 e) none of these

22. The maximum electron capacity of an "f" sublevel is: a) 18 b) 14 c) 10 d) 6 e) 2
23. A "d" sublevel can hold a maximum of a) 5 electrons. b) 10 electrons. c) 14 electrons. d) 32 electrons. e) none of these.
24. The maximum number of electrons allowed in the p sublevel of the 3rd principle level is a) 1 b) 2 c) 3 d) 6 e) 8
25. Sodium has how many electrons in it's outermost principal a) 1 b) 2 c) 6 d) 11 e) 4
26. The number of unpaired electrons in a nitrogen atom is: a) 1 b) 3 c) 5 d) 7 e) nitrogen has no unpaired electrons
27. The electron configuration for the oxygen atom is: a) 1s
2
2s
6 b) 1s
8 c) 1s 2 2s 2 2p 4 d) 1s
1
2s
1 e) 1s
2
2s
2
2p
6
3s
2

28. 1s
2
2s
2
2p
6
3s
2
3p
4
is the electron configuration for which of the following atoms? a) Si b) P c) S d) Cl e) none of these
29. The number of p orbitals in the fourth principal energy level is: a) 6 b) 4 c) 3 d) 1 e) none of these
30. The halogens ( Group 17) contain how many valence electrons? a) 1 b) 7 c) 0 d) 8 e) none of these
31. The maximum number of electrons in the third principal energy level in the atom is: a) 2 b) 6 c) 8 d) 18 e) 32
32. Which element has the largest number of electrons in it's valence shell? a) S b) As c) K d) F e) Fr
33. When moving down a group (family ) in the periodic table, the number of valence electrons a) remains constant b) increases by 2 then by 8 then 18 then 32 c) doubles with each move d) decreases regularly e) changes in as unpredictable manner

34. The Group 13 elements through the group 18 elements form an area of the periodic table where the sublevels being filled are a) p orbitals b) s and p orbitals c) d orbitals d) p and d orbitals e) f orbitals
35. 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
6
is the electron configuration for which of the following a) Ca b) Fe c) Cr d) Ar e) none of these
36. Which electron configuration indicates a transition element? a) 1s
2
2s
2
2p
6
3s
1
3p
6 b) 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
3 c) 1s
2 d) 1s
2
2s
2
2p
5
2s
2
2p
6
3w
2
3p
5
4s
2
3d
10
4p
2 e) none of these
37. What part of the visible light spectrum does a green leaf reflect? a) blue b) green c) red and blue d) all colors
38. If electrons in an atom have the lowest possible energies, the atom is in the a) ground state b) inert state c) excited state d) radiation-emitting state
39. The spin quantum number indicates that the number of possible states for an electron in an orbital is a) 1 b) 2 c) 3 d) 4
40. The total number of orbitals that can exist at the third main energy level is a) 1 b) 5 c) 9 d) 12

41. At n=4 the total number of electrons that could be found is a) 12 b) 22 c) 32 d) 42
42. The number electrons in the highest energy level of Kr atom a) 2 b) 6 c) 8 d) 18
43. The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to a) Mendeleev b) Moseley c) Bohr d) Ramsay
44. A horizontal row of blocks in the periodic table is called a(n) a) group b) family c) period d) octet
45. How many 5p electrons are in the element Antimony (Sb)? a) 1 b) 2 c) 3 d) 4 e) none
46. What element has its last electron 5d
6
? a) Ru b) Xe c) Os d) Ir e) I
47. In period 3 there are 8 elements. What sublevel(s) is (are) being filled? a) s b) s and d c) s and p d) d and f

48. Elements in which the d-sublevel is being filled have the properties of a) metals b) nonmetals c) metalloids d) gases
49. The electron configuration of an element is [Kr]4d
10
5s
1
. To what group does this element belong? a) alkali metals b) alkaline earth metals c) halogens d) transition metals e) noble gases
50. The energy required to remove an electron from an atom is the atom's a) electron affinity b) electron energy c) electronegativity d) ionization energy
51. A negative ion is known as a(n) a) ionic radius b) valence electron c) cation d) anion
52. In a row in the periodic table, as the atomic number increases, the atomic radius generally a) decreases b) remains constant c) increases d) becomes unmeasureable
53. The energy required to remove an electron from an atom ___________ as you move left to right from potassium(K) through iron(Fe). a) generally increases b) generally decreases c) does not change d) varies unpredictably
54. The electrons available to be lost, gained, or shared when atoms form molecules are called a) ions b) valence electrons c) d electrons d) electron clouds

7. (b)
8. (b)
9. (c)
10. (d)
11. (b)
12. (b)
13. (a)
14. (b)
15. (a)
16. (c)
17. (a)
55. Valence electrons are those a) closest to the nucleus b) in the lowest energy level c) in the highest energy level d) combined with protons
56. In Group 2 elements, the valence electrons are in sublevel a) s b) p c) d d) f
57. The number of valence electrons in Group 17 is a) 7 b) 8 c) 17 d) equal to the period number
58. In Groups 13 through 18, valence electrons are in sublevels a) s and d b) s and p c) d and f d) p and d
----------Key----------
1. (b)
2. (d)
3. (a)
4. (a)
5. (b)
6. (a)

32. (d)
33. (a)
34. (a)
35. (b)
36. (b)
37. (b)
38. (a)
39. (b)
40. (c)
41. (c)
42. (c)
43. (a)
44. (c)
45. (c)
46. (c)
47. (c)
48. (a)
49. (a)
50. (d)
51. (d)
52. (a)
53. (a)
54. (b)
55. (c)
56. (a)
57. (a)
58. (b)
18. (d)
19. (a)
20. (c)
21. (e)
22. (b)
23. (b)
24. (d)
25. (a)
26. (b)
27. (c)
28. (c)
29. (c)
30. (b)
31. (d)