TTU General Chemistry


Chem 111 - Quiz 5E - Fall, 2003
Chapter V

1. Which of the following has a negative charge?

a) nucleus
b) neutron
c) proton
d) electron
e) alpha particle

2. In the Rutherford gold foil experiment, the fact that most of the alpha particles were NOT deflected as they passed through the gold foil indicates that:

a) the nucleus is positively charged.
b) the atom is mostly empty space.
c) atoms are solid spheres touching each other in the solid state.
d) gold is very dense.

3. Which two subatomic particles have approximately the same mass?

a) protons and neutrons
b) protons and electrons
c) electrons and nuclei
d) neutrons and electrons
e) protons and alpha particles

4. The number of electrons in a neutral atom of an element is always equal to the _______ of the element.

a) mass number
b) atomic number
c) atomic mass unit
d) isotope number
e) Avogadro's number

5. What is the atomic weight of a hypothetical element consisting of two isotopes, one with mass = 64.23 amu (26.00%), and one with mass = 65.32 amu(74.00%)?

a) 65.16 amu
b) 64.37 amu
c) 64.96 amu
d) 65.04 amu
e) 64.80 amu

6. Which statement about electromagnetic radiation is FALSE?

a) As frequency increases, wavelength decreases.
b) As wavelength increases, energy increases.
c) As wavelength increases, frequency decreases.
d)Wavelength and frequency are inversely proportional.
e) Wavelength and energy are inversely proportional.

7. What is the wavelength of yellow light having a frequency of 5.17 x 1014 Hz?

a) 3.60 x 10-10 m
b) 1.55 x 1023 m
c) 6.45 x 10-28 m
d) 5.80 x 10-7 m
e) 2.72 x 10-6 m

8. What is the energy in joules of a photon of light of wavelength 3.75 x 103 ?

a) 3.30 x 10-13 J
b) 5.30 x 10-19 J
c) 1.10 x 10-17 J
d) 1.38 x 10-14 J
e) 2.22 x 10-11 J

9. The difference between the mass number of an atom and the atomic number of the atom is always equal to __________.

a) 6.02 x 1023.
b) the atomic number of the element.
c) the atomic mass unit.
d) the number of protons in the nucleus.
e) the number of neutrons in the nucleus.

10. Isotopes are atoms of the same element that:

a) have different numbers of electrons.
b) have different numbers of protons.
c) have different atomic numbers.
d) have different numbers of neutrons.
e) have different nuclear charges.

11. The atomic number of a certain element is 19, and its atomic weight is 39. An atom of the element contains _____ protons, _____ neutrons, and the chemical symbol for the element is _____.

a) 19, 19, F
b) 19, 20, F
c) 19, 20, K
d) 20, 19, K
e) none of these

12. Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope.

a) 38 p, 38 n, 38 e
b) 38 p, 90 n, 38 e
c) 52 p, 38 n, 52 e
d) 38 p, 52 n, 38 e
e) 90 p, 38 n, 90 e

13. Give the number of protons, neutrons, and electrons in the 2141Sc3+ ion.

a) 21 p, 20 n, 21 e
b) 21 p, 20 n, 18 e
c) 21 p, 20 n, 24 e
d) 20 p, 21 n, 17 e
e) 21 p, 41 n, 18 e

14. When an electron of an excited hydrogen atom falls from level n = 2 to level n = 1, what wavelength of light is emitted? (R = 1.097 x 107 m-1)

a) 18.2
b) 970
c) 4800
d) 1215
e) 1820

15. The Heisenberg Uncertainty Principle states that ________.

a) no two electrons in the same atom can have the same set of four quantum numbers.
b) two atoms of the same element must have the same number of protons.
c) it is impossible to determine accurately both the position and momentum of an electron simultaneously.
d) electrons of atoms in their ground states enter energetically equivalent sets of orbitals singly before they pair up in any orbital of the set.
e) charged atoms (ions) must generate a magnetic field when they are in motion.

16. A(An) ______ is a region of space in which there is a high probability of finding an electron in an atom.

a) shell
b) atomic orbital
c) core
d) major energy level
e) nucleus

17. Which quantum number is often designated by the letters s, p, d and f?

a) n
b) l
c) ml
d) ms
e) y

18. What is the total number of orbitals in the fourth energy level (n = 4.)

a) 4
b) 24
c) 16
d) 9
e) 18

19. The maximum number of electrons that can occupy an energy level or shell (n = principle quantum number) is _____.

a) n
b) 2n
c) n+1
d) n-1
e) 2n2

20. Which of the following is not a valid magnetic quantum number for the 3d set of orbitals?

a) 1
b) 2
c) 0
d) -2
e) -3

21. No two electrons in the same atom can have the same set of four quantum numbers is a statement of _____.

a) the Aufbau Principle
b) the Pauli Exclusion Principle
c) Dalton's Theory
d) Hund's Rule
e) the Heisenberg Uncertainty Principle

22. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a statement of _____.

a) the Heisenberg Uncertainty Principle
b) the Bohr Theory
c) the Aufbau Principle
d) Planck's Theory
e) Hund's Rule

23. The electron configuration 1s22s22p63s23p6 4s23d6 represents the element _____.

a) Mn
b) Se
c) Fe
d) Co
e) Kr

24. Which of the following is the electron configuration of O2-?

a) 1s22s22p6
b) 1s22s22p4
c) 1s22s22p33s23p6
d) 1s22s22p1
e) 1s22s22p43s23p4

25. What is the electron configuration of tin, Sn?

a) [Kr]5s23d103f145p4
b) [Kr]5s23d104d145p4
c) [Kr]5s23d104f145p2
d) [Kr]5s24d105p2
e) [Xe]5s24d105p2

26. Which one of the following electron configurations is INCORRECT?

a) Cl-; 1s22s22p63s23p6
b) Ge; [Ar]3d104s23p3
c) Sc; [Ar]3d14s2
d) O; [He]2s22p4
e) N3-; 1s22s22p6

27. Which element has the following electron configuration?

a) Na
b) Mg
c) Cl
d) Br
e) P

28. What is the electron configuration of the iron(III) ion?

a) Fe3+[Ar]4s23d3
b) Fe3+[Ar]3d5
c) Fe2+[Ar]4s23d3
d) Fe2+[Ar]3d5
e) Fe3+[Kr]3d5

29. Which of the following sets of quantum numbers COULD represent the "last" electron added to complete the electron configuration for a ground state atom of Br according to the Aufbau Principle. n; l; ml; ms

a) 4; 0; 0; -1/2
b) 4; 1; 1; -1/2
c) 3; 1; 1; -1/2
d) 4; 1; 2; +1/2
e) 4; 2; 1; -1/2

30. Which statement is FALSE?

a) If an electron has quantum number n = 3, the electron could be in a d sublevel.
b) If an electron has quantum number l = 2, the only possible values of ml are 0 and 1.
c) If an electron has ml = 1, it might be in a p, d, or f sublevel but not in an s sublevel.
d) An electron that has n = 3 cannot be in an f sublevel.
e) An electron that has n = 5 could be in an s, p, d, or f sublevel.

31. The TOTAL number of electrons in p orbitals in a palladium atom (atomic number = 46) in its ground state is _____.

a) 6
b) 12
c) 18
d) 24
e) 30

32. An element with the outermost electron configuration ns2np3 would be in Group

b) IIA
e) VA

33. An element that has four electrons in its outer shell in its ground state is _____.

a) Nb
b) Cr
c) Sn
d) Ti
e) O

34. The number of electrons present in the p orbitals in the outermost electron shell (major energy level, n) of the halogen atoms is _______.

a) one
b) two
c) six
d) seven
e) five


1)d 2)b 3)a 4)b 5)d 6)b 7)d 8)b 9)e 10)d 11)c 12)d 13)b 14)d 15)c 16)b 17)b 18)c 19)e 20)e 21)b 22)e 23)c 24)a 25)d 26)b 27)e 28)b 29)b 30)b 31)c 32)e 33)c 34)e