activity: punny configurations
part 1: go through the following electron configurations and determine which element each represents. fill in
the chemical symbol in the blank to the right of the configuration. if any of the electron configurations are not
valid for any element, write \invalid\ in the space.
1. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 3 } )
2. ( 1 s ^ { 2 } )
3. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 5 } )
4. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 4 } )
5. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 1 } )
6. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 4 } 3 s ^ { 1 } ) invalid
7. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 6 } 6 s ^ { 2 } )
8. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } )
9. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 d ^ { 3 } ) invalid
10. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 6 } 6 s ^ { 2 } 4 f ^ { 1 4 } 5 d ^ { 1 0 } 6 p ^ { 6 } 7 s ^ { 2 } 5 f ^ { 7 } 6 d ^ { 1 } )
*hint: it gets tricky with 5f and 6d, so after ( 7 s ^ { 2 } ), see that i have 8 more e-, and count down the row to 8 to find me.
11. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 6 } 6 s ^ { 2 } 4 f ^ { 1 4 } 5 d ^ { 1 0 } 6 p ^ { 6 } 7 s ^ { 2 } 5 f ^ { 1 4 } ) no
12. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 2 } )
13. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 6 } 6 s ^ { 2 } 4 f ^ { 1 4 } 5 d ^ { 1 0 } 6 p ^ { 6 } 7 s ^ { 2 } 6 d ^ { 1 } )
14. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 4 d ^ { 1 0 } 4 p ^ { 3 } )
15. ( 1 s ^ { 2 } 2 s ^ { 2 } 2 p ^ { 6 } 3 s ^ { 2 } 3 p ^ { 6 } 4 s ^ { 2 } 3 d ^ { 1 0 } 4 p ^ { 6 } 5 s ^ { 2 } 4 d ^ { 1 0 } 5 p ^ { 6 } 6 s ^ { 2 } 4 f ^ { 1 4 } 5 d ^ { 5 } ) re

Question

Accepted Answer

# Brief Explanations:
To determine the element from the electron configuration, we count the total number of electrons. The number of electrons is equal to the atomic number of the element.
1. For $1s^{2}2s^{2}2p^{3}$, the total number of electrons $=2 + 2+3=7$. The element with atomic number $7$ is $N$ (Nitrogen).
2. For $1s^{2}$, the total number of electrons $= 2$. The element with atomic number $2$ is $He$ (Helium).
3. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{5}$, the total number of electrons:
$$
\begin{align*}
&2+2 + 6+2+6+2+10+6+2+10+5\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+5)\
=&4+14+18+17\
=&53
\end{align*}
$$
The element with atomic number $53$ is $I$ (Iodine).
4. For $1s^{2}2s^{2}2p^{4}$, the total number of electrons $=2+2 + 4=8$. The element with atomic number $8$ is $O$ (Oxygen).
5. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}$, the total number of electrons $=2+2+6+2+6 + 1=19$. The element with atomic number $19$ is $K$ (Potassium).
6. $1s^{2}2s^{2}2p^{4}3s^{1}$ is invalid because according to the Aufbau principle, after filling $2p$ (which can hold a maximum of $6$ electrons), we should fill $3s$ only when $2p$ is completely filled or half - filled (in some cases of stability, but here $2p$ is not full).
7. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}$, the total number of electrons:
$$
\begin{align*}
&2+2+6+2+6+2+10+6+2+10+6+2\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+6)+2\
=&4+14+18+18+2\
=&56
\end{align*}
$$
The element with atomic number $56$ is $Ba$ (Barium).
8. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}$, the total number of electrons $=2+2+6+2+6=18$. The element with atomic number $18$ is $Ar$ (Argon).
9. $1s^{2}2s^{2}2p^{6}3s^{2}3d^{3}$ is invalid. After filling $3s$ ($3s^{2}$), we should fill $3p$ before $3d$ according to the Aufbau principle ($n + l$ rule: for $3p$, $n + l=3 + 1 = 4$; for $3d$, $n + l=3+2 = 5$).
10. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{7}6d^{1}$, the total number of electrons:
$$
\begin{align*}
&2+2+6+2+6+2+10+6+2+10+6+2+14+10+6+2+7+1\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+6)+(2+14+10+6)+(2+7+1)\
=&4+14+18+18+32+10\
=&86 + 10\
=&96
\end{align*}
$$
The element with atomic number $96$ is $Cm$ (Curium).
11. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{14}$, the total number of electrons:
$$
\begin{align*}
&2+2+6+2+6+2+10+6+2+10+6+2+14+10+6+2+14\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+6)+(2+14+10+6)+14\
=&4+14+18+18+32+14\
=&100
\end{align*}
$$
The element with atomic number $100$ is $Fm$ (Fermium).
12. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{2}$, the total number of electrons $=2+2+6+2+6+2+2=22$. The element with atomic number $22$ is $Ti$ (Titanium).
13. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}6d^{1}$, the total number of electrons:
$$
\begin{align*}
&2+2+6+2+6+2+10+6+2+10+6+2+14+10+6+2+1\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+6)+(2+14+10+6)+(2 + 1)\
=&4+14+18+18+32+3\
=&89
\end{align*}
$$
The element with atomic number $89$ is $Ac$ (Actinium).
14. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}4d^{10}4p^{3}$, the total number of electrons $=2+2+6+2+6+2+10+3=33$. The element with atomic number $33$ is $As$ (Arsenic).
15. For $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{5}$, the total number of electrons:
$$
\begin{align*}
&2+2+6+2+6+2+10+6+2+10+6+2+14+5\
=&(2 + 2)+(6+2+6)+(2+10+6)+(2+10+6)+(2+14+5)\
=&4+14+18+18+21\
=&65
\end{align*}
$$
The element with atomic number $65$ is $Tb$ (Terbium).

# Answer:
1. $N$
2. $He$
3. $I$
4. $O$
5. $K$
6. $invalid$
7. $Ba$
8. $Ar$
9. $invalid$
10. $Cm$
11. $Fm$
12. $Ti$
13. $Ac$
14. $As$
15. $Tb$

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Answer: