Chem 111 - Quiz 5E - Fall, 2003
1. Which of the following has a negative charge?
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:
3. Which two subatomic particles have approximately the same mass?
4. The number of electrons in a neutral atom of an element is always equal to the _______ of the element.
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%)?
6. Which statement about electromagnetic radiation is FALSE?
7. What is the wavelength of yellow light having a frequency of 5.17 x 1014 Hz?
8. What is the energy in joules of a photon of light of wavelength 3.75 x 103 Å?
9. The difference between the mass number of an atom and the atomic number of the atom is always equal
10. Isotopes are atoms of the same element that:
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 _____.
12. Give the number of protons, neutrons, and electrons in an atom of the 90Sr isotope.
13. Give the number of protons, neutrons, and electrons in the
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)
15. The Heisenberg Uncertainty Principle states that ________.
16. A(An) ______ is a region of space in which there is a high probability of finding an electron in an
17. Which quantum number is often designated by the letters s, p, d and f?
18. What is the total number of orbitals in the fourth energy level (n = 4.)
19. The maximum number of electrons that can occupy an energy level or shell (n = principle quantum
number) is _____.
20. Which of the following is not a valid magnetic quantum number for the 3d set of orbitals?
21. No two electrons in the same atom can have the same set of four quantum numbers is a statement of
22. All orbitals of a given degenerate set must be singly occupied before pairing begins in that set is a
statement of _____.
23. The electron configuration
4s23d6 represents the element _____.
24. Which of the following is the electron configuration of O2-?
25. What is the electron configuration of tin, Sn?
26. Which one of the following electron configurations is INCORRECT?
27. Which element has the following electron configuration?
28. What is the electron configuration of the iron(III) ion?
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
30. Which statement is FALSE?
31. The TOTAL number of electrons in p orbitals in a palladium atom (atomic number = 46) in
its ground state is _____.
32. An element with the outermost electron configuration ns2np3 would be in
33. An element that has four electrons in its outer shell in its ground state is _____.
34. The number of electrons present in the p orbitals in the outermost electron shell (major energy level,
n) of the halogen atoms is _______.
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