Question

activity c (continued from previous page)
8 make a rule next to subshells ordered by, select number the diagonal rule at right shows which subshell will be filled next. to follow the rule, move down along an arrow until you reach the end of the arrow. then move to the start of the next arrow to the right.
a which subshell is filled after 4p?
b which subshell is filled after 6s?
c which subshell is filled after 5d?
9 practice determine the electron configurations of the following elements. use the gizmo to check your work. (note: in some cases, the diagonal rule doesnt work perfectly. if you submit a theoretically correct configuration, the gizmo will give you the actual configuration.)
element atomic number electron configuration
cobalt (co) 27
germanium (ge) 32
neodymium (nd) 60
gold (au) 79
10 infer select the periodic table tab. earlier you saw that the transition metals represent the filling of the d subshells. now locate the purple lanthanides and actinides on the bottom rows of the periodic table.
a how many elements are in the lanthanides series?
b which subshell is represented by the lanthanides series?
c which subshell is represented by the actinides series?
d in general, how does the shape of the periodic table relate to electron configuration?

Explanation:

Step1: Recall diagonal - rule for electron - filling

The diagonal rule is used to determine the order of filling of sub - shells. We follow the arrows in the diagonal pattern.

Step2: Answer question 8A

Moving along the diagonal arrows, after 4p, the next sub - shell is 5s.

Step3: Answer question 8B

After 6s, the next sub - shell is 4f.

Step4: Answer question 8C

After 5d, the next sub - shell is 6p.

Step5: Determine electron configuration of Cobalt (Co)

Cobalt has an atomic number of 27. Using the diagonal rule, the electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d⁷.

Step6: Determine electron configuration of Germanium (Ge)

Germanium has an atomic number of 32. Its electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p².

Step7: Determine electron configuration of Neodymium (Nd)

Neodymium has an atomic number of 60. Its electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f⁴.

Step8: Determine electron configuration of Gold (Au)

Gold has an atomic number of 79. Its electron configuration is 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d¹⁰.

Step9: Answer question 10A

The lanthanides series has 14 elements.

Step10: Answer question 10B

The lanthanides series represents the filling of the 4f sub - shell.

Step11: Answer question 10C

The actinides series represents the filling of the 5f sub - shell.

Step12: Answer question 10D

The shape of the periodic table is related to electron configuration as elements in the same group have the same number of valence electrons, and the periods correspond to the principal energy levels being filled. The s - block elements are in groups 1 and 2, the p - block elements are in groups 13 - 18, the d - block elements are the transition metals, and the f - block elements are the lanthanides and actinides.

Answer:

8A. 5s
8B. 4f
8C. 6p

1. Cobalt (Co): 1s²2s²2p⁶3s²3p⁶4s²3d⁷

Germanium (Ge): 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²
Neodymium (Nd): 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²4f⁴
Gold (Au): 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d¹⁰
10A. 14
10B. 4f
10C. 5f
10D. The shape of the periodic table is related to electron configuration as elements in the same group have the same number of valence electrons, and the periods correspond to the principal energy levels being filled. The s - block elements are in groups 1 and 2, the p - block elements are in groups 13 - 18, the d - block elements are the transition metals, and the f - block elements are the lanthanides and actinides.