Question

Number of radial nodes orbitals in 3s and 2p

Answer 1

Answer:

The Formula to find the radial nodes is,

$\blue{\large{\boxed{\sf Number \;of\; radial\; nodes = n-l-1}}}$

where,

$\sf n$ = principal quantum number

$l$ = azimuthal quantum number

For 3s orbital, number of radial nodes = $3 - 0 - 1 = 2$

For 2p orbital, number of radial nodes = $2-1-1=0$

Hence, The number of radial nodes orbitals in 3s and 2p orbitals are 2 and 0 respectively.

Answer 2

★$\color{darkblue}\underline{\underline{\sf To \: Find-}}$

• Number of radial nodes orbital in 3s and 2p

★$\color{darkblue}\underline{\underline{\sf Solution-}}$

$\large\underline{\sf Node-}$

It is point / line / plane / surface in which probability of finding electrons is zero

They are of two type

• Radial Node
• Angular Node

To find number of radial Node we use -

$\color{violet}\bullet\underline{\boxed{\sf No. \: of \: radial \: nodes = n - \ell - 1}}$

Here ,

n = Principal Quantum Number

$\ell$ = Azimuthal Quantum Number

Now , in our Question

We have to find radial Node of 3s and 2p

$\underline{\sf For \: 3s-}$

$\implies{\sf no. \: of \: radial \: nodes = n-\ell - 1 }$

$\implies{\sf 3-0-1}$

$\color{red}\implies{\sf no.\; of \: radial \: node= 2}$

$\underline{\sf For \: 2p-}$

$\implies{\sf no.\: of \: radial \: node = n-\ell-1}$

$\implies{\sf 2-1-1 }$

$\color{red}\implies{\sf no. \: of \: radial \: node = 0 }$

★$\color{darkblue}\underline{\underline{\sf Answer-}}$

No. of radial Node in 3s is $\color{red}{\sf 2}$

No. of radial Node in 2p is $\color{red}{\sf zero}$

★$\Large\underline{\sf Extra \: Information -}$

Azimuthal Quantum Number $(\ell)$ for -

$</p><p>\begin{tabular}{c | 1}</p><p></p><p>Orbital & Azimuthal \: Quantum \: Number \: (\ell) \\</p><p></p><p>\cline {1-2}</p><p></p><p>s & 0 \\</p><p>p & 1 \\</p><p>d & 2 \\</p><p>f & 3 \\</p><p></p><p></p><p>\end{tabular}</p><p>$