Welcome to Westonci.ca, your one-stop destination for finding answers to all your questions. Join our expert community now! Get immediate and reliable answers to your questions from a community of experienced professionals on our platform. Get precise and detailed answers to your questions from a knowledgeable community of experts on our Q&A platform.
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.
Thank you for your visit. We're committed to providing you with the best information available. Return anytime for more. We hope you found what you were looking for. Feel free to revisit us for more answers and updated information. Thank you for visiting Westonci.ca, your go-to source for reliable answers. Come back soon for more expert insights.