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Sagot :
To identify the elements that are diatomic, we follow these steps:
1. List of Diatomic Elements: Diatomic elements are those that form molecules consisting of two atoms bonded together. The commonly known diatomic elements are:
- Hydrogen (H2)
- Nitrogen (N2)
- Oxygen (O2)
- Fluorine (F2)
- Chlorine (Cl2)
- Bromine (Br2)
- Iodine (I2)
2. Periodic Table Locations: Locate each of these diatomic elements on the periodic table using their atomic numbers:
- Hydrogen (H) with atomic number 1
- Nitrogen (N) with atomic number 7
- Oxygen (O) with atomic number 8
- Fluorine (F) with atomic number 9
- Chlorine (Cl) with atomic number 17
- Bromine (Br) with atomic number 35
- Iodine (I) with atomic number 53
3. Mapping to Periodic Table Image: Using the information in the table provided:
- Hydrogen (H) is located in the first row, atomic number 1.
- Nitrogen (N) is located in the second row, atomic number 7.
- Oxygen (O) is located in the second row, atomic number 8.
- Fluorine (F) is located in the second row, atomic number 9.
- Chlorine (Cl) is located in the third row, atomic number 17.
- Bromine (Br) is located in the fourth row, atomic number 35.
- Iodine (I) is located in the fifth row, atomic number 53.
Now, let's highlight the correct locations in the periodic table provided:
4. Highlighting the Elements: The positions of the diatomic elements on the periodic table are:
- 1: H
- 7: N
- 8: O
- 9: F
- 17: Cl
- 35: Br
- 53: I
Highlighting these locations:
```plaintext
\begin{tabular}{|c|c|}
\hline 1 & \\
[tex]$H$[/tex] & \\
\hline 3 & 4 \\
[tex]$Li$[/tex] & [tex]$Be$[/tex] \\
\hline 11 & 12 \\
[tex]$Na$[/tex] & [tex]$Mg$[/tex] \\
\hline 19 & 20 \\
[tex]$K$[/tex] & [tex]$Ca$[/tex] \\
\hline 37 & 38 \\
[tex]$Rb$[/tex] & [tex]$Sr$[/tex] \\
\hline 55 & 56 \\
[tex]$Cs$[/tex] & [tex]$Ba$[/tex] \\
\hline 87 & 88 \\
[tex]$Fr$[/tex] & [tex]$Ra$[/tex] \\
\hline
\end{tabular}
\begin{tabular}{|c|c|c|c|c|c|}
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 5 \\
\hline \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
C
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
7 \\
[tex]$N$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
8 \\
0
\end{tabular}
\end{tabular} & \begin{tabular}{l}
F
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
10 \\
[tex]$Ne$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 13 \\
Al \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
14 \\
[tex]$Si$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
15 \\
[tex]$P$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
16 \\
[tex]$S$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
17 \\
[tex]$Cl$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
18 \\
[tex]$Ar$[/tex]
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{r}
31 \\
[tex]$Ga$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
32 \\
[tex]$Ge$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
33 \\
As
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
34 \\
Se
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
35 \\
[tex]$Br$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
36 \\
[tex]$Kr$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{l}
In \\
In
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
50 \\
[tex]$Sn$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{|l}
51 \\
Sb
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
52 \\
[tex]$Te$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
53
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
54 \\
[tex]$Xe$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 81 \\
\hline [tex]$TI$[/tex] \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
82 \\
[tex]$Pb$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{|l}
83 \\
[tex]$Bi$[/tex] \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
84 \\
Po
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
85 \\
At
\end{tabular}
\end{tabular} & \begin{tabular}{l}
86 \\
[tex]$Rn$[/tex]
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{l}
113 \\
[tex]$Nh$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{c}
114 \\
FI
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
115 \\
Mc
\end{tabular}
\end{tabular} & \begin{tabular}{l}
116 \\
[tex]$Lv$[/tex]
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
117 \\
Ts
\end{tabular}
\end{tabular} & \\
\hline
\end{tabular}
```
Therefore, H, N, O, F, Cl, Br, and I are identified as the diatomic elements located on the periodic table.
1. List of Diatomic Elements: Diatomic elements are those that form molecules consisting of two atoms bonded together. The commonly known diatomic elements are:
- Hydrogen (H2)
- Nitrogen (N2)
- Oxygen (O2)
- Fluorine (F2)
- Chlorine (Cl2)
- Bromine (Br2)
- Iodine (I2)
2. Periodic Table Locations: Locate each of these diatomic elements on the periodic table using their atomic numbers:
- Hydrogen (H) with atomic number 1
- Nitrogen (N) with atomic number 7
- Oxygen (O) with atomic number 8
- Fluorine (F) with atomic number 9
- Chlorine (Cl) with atomic number 17
- Bromine (Br) with atomic number 35
- Iodine (I) with atomic number 53
3. Mapping to Periodic Table Image: Using the information in the table provided:
- Hydrogen (H) is located in the first row, atomic number 1.
- Nitrogen (N) is located in the second row, atomic number 7.
- Oxygen (O) is located in the second row, atomic number 8.
- Fluorine (F) is located in the second row, atomic number 9.
- Chlorine (Cl) is located in the third row, atomic number 17.
- Bromine (Br) is located in the fourth row, atomic number 35.
- Iodine (I) is located in the fifth row, atomic number 53.
Now, let's highlight the correct locations in the periodic table provided:
4. Highlighting the Elements: The positions of the diatomic elements on the periodic table are:
- 1: H
- 7: N
- 8: O
- 9: F
- 17: Cl
- 35: Br
- 53: I
Highlighting these locations:
```plaintext
\begin{tabular}{|c|c|}
\hline 1 & \\
[tex]$H$[/tex] & \\
\hline 3 & 4 \\
[tex]$Li$[/tex] & [tex]$Be$[/tex] \\
\hline 11 & 12 \\
[tex]$Na$[/tex] & [tex]$Mg$[/tex] \\
\hline 19 & 20 \\
[tex]$K$[/tex] & [tex]$Ca$[/tex] \\
\hline 37 & 38 \\
[tex]$Rb$[/tex] & [tex]$Sr$[/tex] \\
\hline 55 & 56 \\
[tex]$Cs$[/tex] & [tex]$Ba$[/tex] \\
\hline 87 & 88 \\
[tex]$Fr$[/tex] & [tex]$Ra$[/tex] \\
\hline
\end{tabular}
\begin{tabular}{|c|c|c|c|c|c|}
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 5 \\
\hline \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
C
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
7 \\
[tex]$N$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
8 \\
0
\end{tabular}
\end{tabular} & \begin{tabular}{l}
F
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
10 \\
[tex]$Ne$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 13 \\
Al \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
14 \\
[tex]$Si$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
15 \\
[tex]$P$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
16 \\
[tex]$S$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
17 \\
[tex]$Cl$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
18 \\
[tex]$Ar$[/tex]
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{r}
31 \\
[tex]$Ga$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
32 \\
[tex]$Ge$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
33 \\
As
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
34 \\
Se
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
35 \\
[tex]$Br$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
36 \\
[tex]$Kr$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{l}
In \\
In
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
50 \\
[tex]$Sn$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{|l}
51 \\
Sb
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
52 \\
[tex]$Te$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
53
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{r}
54 \\
[tex]$Xe$[/tex]
\end{tabular}
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{|l|}
\hline 81 \\
\hline [tex]$TI$[/tex] \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
82 \\
[tex]$Pb$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{|l}
83 \\
[tex]$Bi$[/tex] \\
\hline
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
84 \\
Po
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
85 \\
At
\end{tabular}
\end{tabular} & \begin{tabular}{l}
86 \\
[tex]$Rn$[/tex]
\end{tabular} \\
\hline \begin{tabular}{l}
\begin{tabular}{l}
113 \\
[tex]$Nh$[/tex]
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{c}
114 \\
FI
\end{tabular}
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
115 \\
Mc
\end{tabular}
\end{tabular} & \begin{tabular}{l}
116 \\
[tex]$Lv$[/tex]
\end{tabular} & \begin{tabular}{l}
\begin{tabular}{l}
117 \\
Ts
\end{tabular}
\end{tabular} & \\
\hline
\end{tabular}
```
Therefore, H, N, O, F, Cl, Br, and I are identified as the diatomic elements located on the periodic table.
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