Download Chapter 6 Part II

Chapter 6 Part II
1. Write the subshell notation and the number of orbitals having these quantum numbers
in an atom: (a) n =3, l = 2; (b) n = 1, l =0; (c) n = 6, l =3; (d) n =2, l =1.
2. Identify the values of the principal quantum number, n, and the azimuthal quantum
number, l, for the following subshells: (a) 2p; (b) 5f; (c) 3s; (d) 4d.
3. How many electrons can have the following quantum numbers in an atom: (a) n =2,
l=1; (b) n =4, l =2, ml = -2; (c) n =2; (d) n =3, l =2, ml = +1?
4. Which of the following subshells cannot exist in an atom: (a) 1p; (b) 3 f; (c) 7p; (d)
5d; (e) 2d; (f) 4g?
5. Identify the sets of four quantum numbers {n, l, ml, ms} that cannot exist for an
electron in an atom and explain why not? (a) {2,2,-1,+1/2}; (b) {5, 0, -1, +1/2}; (c)
{4, 4, -1, +1/2}; (d) {4, 2, -1, +1/2}; (e) {5, 4, +5, +1/2}.
6. Identify the possible sets of four quantum numbers {n, l, ml, ms} for the starred
electron in the diagrams below. Select the values of ml by numbering from –l to +l
from left to right.
a) 2p   *
b) 5d    *

c) 5f    *   
7. For the following elements: Na, Mg, Cu, Co, Fe, K, P, La, Au, Cf, Po, Rn, Re, Cs.
(a) Give the name and the family to which the element belongs.
(b) Give the block to which the element belongs.
(c) Write the complete electron configuration.
(d) Write the electron configuration starting with the previous noble gas.
(e) Write the electron diagram for the outer shell.
8. Identify the elements that have the electronic configuration in question 6.