atomic numbers and electron configurations (practice)

For the n = 3 electron shell, which of the following quantum numbers are valid? Check all that apply. l = 3 m = 3 l = 0 m = -2 l = -1 m = 2

l=0 m= -2 m=2

Which of the following is not a valid set of quantum numbers? n = 2, l = 1, m = 0 n = 1, l = 0, m = 0 n = 3, l = 3, m = 3

n = 3, l = 3, m = 3

Which of the following sets of quantum numbers describe valid orbitals? Check all that apply. n = 1, l = 0, m = 0 n = 2, l = 1, m = 3 n = 2, l = 2, m = 2 n = 3, l = 0, m = 0 n = 5, l = 4, m = -3 n = 4, l = -2, m = 2

n=1, l=0, m=0 n=3, l=0, m=0 n=5, l=4, m=-3

Which of the following gives the correct possible values of l for n = 4? 0, 1, 2, 3 -4, -3, -2, -1, 0, 1, 2, 3, 4 0, 1, 2, 3, 4

0, 1, 2, 3

Which is the correct electron configuration for sodium (Na)? 1s^2 2s^2 2p^6 2d^1 1s^2 2s^2 2p^6 3s^1 1s^2 2p^6 3d^3

1s^2 2s^2 2p^6 3s^1

Which of the following is the correct electron configuration for titanium (Ti)? 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2 1s^2 2s^2 2p^6 3s^2 3p^6 3d^4 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^2

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2

What is the correct representation for the subshell with n = 2 and l = 1? 2p 1p 1d 2d

2p

1: n = 2, l = 0 2p: 2: n = 3, l = 2 3d: 3: n = 1, l = 0 2s: 4: n = 2, l = 1 4f: 5: n = 4, l = 3 1s:

2p=4 3d=2 2s=1 4f=5 1s=3

How many subshells are in the n = 4 shell? How many orbitals does the n = 4 shell have? What is the maximum number of electrons the n = 4 shell can contain?

4 16 32

n = 5 shell: n = 2 shell: n = 2, l = 0 subshell: n = 2, l = 1 subshell: 3d subshell: 2s subshell: 5f subshell

50 8 2 6 10 2 14