## How many electrons can be accommodated in a subshell for which N 3 L 2?

10 electrons

– Means the respective orbital where n = 3, l = 2 will be ‘3d’ because 3d orbitals contain five subshells and the principal quantum number is 3. – We know that 3d orbital can accommodate 10 electrons (each subshell can accommodate two electrons). – Therefore the number of electrons are in n = 3, l = 2 are 10.

### What type of orbital is occupied by an electron with n 3 and L 2?

Therefore, a maximum number of 10 electrons can share these two quantum numbers in an atom. These electrons are located on the third energy level, in the 3d subshell.

#### When N 3 and L 2 What are the allowed values of ML?

For n = 3, l = 0, 1, 2 For l = 0 ml = 0 For l = 1 ml = -1, 0, or +1 For l = 2 ml = -2, -1, 0, +1, or +2 There are 9 ml values and therefore 9 orbitals with n = 3.

**What is the subshell for N 3 L 1?**

The principal quantum number can be used to determine the energy level, and the subshell can be determined by the value of the angular momentum quantum number. Here, l is 1 and corresponds to the p-subshell. Hence, the subshell for the given quantum numbers is 3p.

**How many Subshells are in the N 3 shell?**

three subshells

The n = 3 shell, for example, contains three subshells: the 3s, 3p, and 3d orbitals.

## How many electrons can fit into the subshell for which N 3?

So, n=3 and l = 1 indicates electrons are present in the 3p subshell. The p subshell has a maximum of 3 orbitals and each orbital contains a maximum of 2 electrons. Hence, the correct option is (D) 6.

### How many Subshells are in the N 2 shell?

two subshells

After looking at the examples above, we see that the value of n is equal to the number of subshells in a principal electronic shell: Principal shell with n = 1 has one subshell. Principal shell with n = 2 has two subshells.

#### What is the correct representation for the subshell with N 2 and L 1?

The subshell with n=2 and l=1 is the 2p subshell; if n=3 and l=0, it is the 3s subshell, and so on. The value of l also has a slight effect on the energy of the subshell; the energy of the subshell increases with l (s < p < d < f).

**How many orbitals are there in N 2?**

four orbitals

There are four orbitals in the n = 2 shell. There is only one orbital in the 2s subshell.

**What are the Subshells in shell 3?**

The third shell has three subshells, labeled s, p, and d. The d subshell can hold a maximum of 10 electrons.

## What Subshells are possible in n 3?

The n = 3 shell, for instance, contains three subshells: the 3s, 3p, and 3d orbitals.

### How many Subshells are in the N 3?

#### How to find subshells?

subshell lies along the Xand Yaxes and is called the 3dx2-y2orbital. Most of the space occupied by the fifth orbital lies along the Zaxis and this orbital is called the 3dz2orbital. The number of orbitals in a shell is the square of the principal quantum number: 12= 1, 22= 4, 32= 9.

**What is the difference between Shell, subshell, and orbital?**

The main difference between shell subshell and orbital is that shells are composed of electrons that share the same principal quantum number and subshells are composed of electrons that share the same angular momentum quantum number whereas orbitals are composed of electrons that are in the same energy level but have

**How many orbitals make up the 4d subshell?**

The 4th shell has 4 subshells: the subshell, which has 1 orbital with 2 electrons,the subshell that has 3 orbitals and 6 electrons, the subshell which has 5 orbitals and 10 electrons, and the subshell which has 7 orbitals and 14 electrons for a total of 16 orbitals and 32 electrons.

## What are shells and subshells?

What are shells and subshells in chemistry? Shells are a collection of subshells with the same principle quantum number, and subshells are a collection of orbitals with the same principle quantum number and angular momentum quantum number.. what is an orbital in chemistry? Orbital Definition. In chemistry and quantum mechanics, an orbital is a mathematical function that describes the wave-like