Answer
362.2k+ views
Hint: Nodal plane is a plane that passes through a nucleus where the probability of finding an electron is almost zero. The number of nodal planes for any orbital is equal to azimuthal quantum number is denoted by “l”.
Complete step by step answer:
- Now, the shell whose principal quantum number is 3, the value of l possible are:
n=3, number of subshell is $l=0\text{ }to\text{ }\left( n-1 \right)$
\[\begin{align}
& l=0\text{ }to\text{ }\left( 3-1 \right) \\
& l=0\text{ }to\text{ }\left( 2 \right) \\
& l=0\text{ }to\text{ }2 \\
\end{align}\]
- We can see that value of l possible are 0, 1, 2, so we can say that 3s , 3p, 3d subshell will be present, out of which there is one orbital present in 3s subshell, 3 orbitals present in 3p subshell that are $\left( 3{{p}_{x}},3{{p}_{y}},3{{p}_{z}} \right)$ and 5 orbitals present in 3d subshell that are $\left( 3{{d}_{xy}},3{{d}_{yz}},3{{d}_{zx}},3{{d}_{{{x}^{2}}-{{y}^{2}}}},3{{d}_{{{z}^{2}}}} \right)$.
- In general, we can say that the number of nodal planes for any orbital is the Azimuthal quantum number (that is denoted by l) of that orbital.
- We can say that, in 3s subshell there is zero nodal plane. In 3p subshell there will be three nodal planes, one from each $\left( 3{{p}_{x}},3{{p}_{y}},3{{p}_{z}} \right)$.
- In 3d , there will be 8 nodal planes, 2 from each $\left( 3{{d}_{xy}},3{{d}_{yz}},3{{d}_{zx}},3{{d}_{{{x}^{2}}-{{y}^{2}}}} \right)$ and there are zero nodal plane in $3{{d}_{{{z}^{2}}}}$this is an exception .
- So, we can write the total nodal planes of the atomic orbitals for the principal quantum number n = 3 as: 0 + 3 + 8 = 11
Hence, we can conclude that the correct option is (C) that 11 nodal planes are there in the atomic orbitals for the principal quantum number n = 3.
Note:
-Nodal planes and Nodal surfaces are different. As we know the number of nodal planes for the orbital is denoted by the value of ‘l’ but in case of nodal surface, the number of nodal surfaces can be determined by the n-l-1 where n = principal quantum number and l = azimuthal quantum number.
- Nodal planes are also called angular nodes while nodal surfaces are also known as radial nodes.
- There are zero nodal planes in $3{{d}_{{{z}^{2}}}}$, this is an exception.
Complete step by step answer:
- Now, the shell whose principal quantum number is 3, the value of l possible are:
n=3, number of subshell is $l=0\text{ }to\text{ }\left( n-1 \right)$
\[\begin{align}
& l=0\text{ }to\text{ }\left( 3-1 \right) \\
& l=0\text{ }to\text{ }\left( 2 \right) \\
& l=0\text{ }to\text{ }2 \\
\end{align}\]
- We can see that value of l possible are 0, 1, 2, so we can say that 3s , 3p, 3d subshell will be present, out of which there is one orbital present in 3s subshell, 3 orbitals present in 3p subshell that are $\left( 3{{p}_{x}},3{{p}_{y}},3{{p}_{z}} \right)$ and 5 orbitals present in 3d subshell that are $\left( 3{{d}_{xy}},3{{d}_{yz}},3{{d}_{zx}},3{{d}_{{{x}^{2}}-{{y}^{2}}}},3{{d}_{{{z}^{2}}}} \right)$.
- In general, we can say that the number of nodal planes for any orbital is the Azimuthal quantum number (that is denoted by l) of that orbital.
- We can say that, in 3s subshell there is zero nodal plane. In 3p subshell there will be three nodal planes, one from each $\left( 3{{p}_{x}},3{{p}_{y}},3{{p}_{z}} \right)$.
- In 3d , there will be 8 nodal planes, 2 from each $\left( 3{{d}_{xy}},3{{d}_{yz}},3{{d}_{zx}},3{{d}_{{{x}^{2}}-{{y}^{2}}}} \right)$ and there are zero nodal plane in $3{{d}_{{{z}^{2}}}}$this is an exception .
- So, we can write the total nodal planes of the atomic orbitals for the principal quantum number n = 3 as: 0 + 3 + 8 = 11
Hence, we can conclude that the correct option is (C) that 11 nodal planes are there in the atomic orbitals for the principal quantum number n = 3.
Note:
-Nodal planes and Nodal surfaces are different. As we know the number of nodal planes for the orbital is denoted by the value of ‘l’ but in case of nodal surface, the number of nodal surfaces can be determined by the n-l-1 where n = principal quantum number and l = azimuthal quantum number.
- Nodal planes are also called angular nodes while nodal surfaces are also known as radial nodes.
- There are zero nodal planes in $3{{d}_{{{z}^{2}}}}$, this is an exception.
Recently Updated Pages
How many sigma and pi bonds are present in HCequiv class 11 chemistry CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Why Are Noble Gases NonReactive class 11 chemistry CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Let X and Y be the sets of all positive divisors of class 11 maths CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Let x and y be 2 real numbers which satisfy the equations class 11 maths CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Let x 4log 2sqrt 9k 1 + 7 and y dfrac132log 2sqrt5 class 11 maths CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Let x22ax+b20 and x22bx+a20 be two equations Then the class 11 maths CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Trending doubts
Fill the blanks with the suitable prepositions 1 The class 9 english CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Which are the Top 10 Largest Countries of the World?
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Write a letter to the principal requesting him to grant class 10 english CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Difference between Prokaryotic cell and Eukaryotic class 11 biology CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Give 10 examples for herbs , shrubs , climbers , creepers
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Fill in the blanks A 1 lakh ten thousand B 1 million class 9 maths CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Change the following sentences into negative and interrogative class 10 english CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Difference Between Plant Cell and Animal Cell
![arrow-right](/cdn/images/seo-templates/arrow-right.png)
Differentiate between homogeneous and heterogeneous class 12 chemistry CBSE
![arrow-right](/cdn/images/seo-templates/arrow-right.png)