## How Many Degenerate Orbitals Are Needed To Contain Six Electrons With Two Of Them Unpaired??

## What are the number of degenerate orbitals?

Firstly degenerate orbitals in an atom are those which have the same energy. For example the “p” subshell has three degenerate orbitals “**d” subshell has five** and “f” subshell has seven.

## How many degenerate orbitals are in 2p?

**three degenerate 2p orbitals**(m

_{l}= −1 0 +1) and the electron can occupy any one of these p orbitals.

## What does it mean for two or more orbitals to be degenerate?

Two or more orbitals are degenerate **if they have the same energy**. … Degenerate means that they have the same energy. ns orbitals cannot be degenerate with respect to themselves because there is only one ns orbital for a given n .

## Are 2s and 2p orbitals degenerate?

The 2s and 2p orbitals have the same energy for hydrogen. They are said to be **degenerate energy levels** all the same. … When the electron is held in the 1s orbital it is said to be in its ground state its lowest energy state. When the electron is a higher energy orbital it is said to be in an excited state.

## How do you calculate the number of degenerate orbitals?

It is calculated **on the basis of QUANTUM numbers**. The total no of orbitals equal to total no of magnetic quantum numbers a subshell can possess. The total no of magnetic no a subshell can possess is given by total nos from -l to +l or mathematically 2l+1. Hence it has 5 degenerate orbitals.

## What are degenerate orbitals 10?

**Electron orbitals having the same energy levels** are called degenerate orbitals. As per the Aufbau principle the lower energy levels are filled before higher energy levels. As per Hund’s rule degenerate orbitals are filled evenly before electrons are filled into higher energy levels.

## Which atomic orbital can accommodate a maximum of six electrons?

**called the p sublevel**can hold a maximum of six electrons.

## Which of the following set of orbitals are degenerate?

Explanation: Orbitals having nearly same energy are called degenerate orbitals. Among the given **π 2px and π 2py orbitals** are of eqouivalent energy thus are called degenerate orbitals.

## What are degenerate orbitals according to Hund’s rule How are degenerate orbitals occupied?

According to Hund’s rule how are degenerate orbitals occupied? Degenerate orbitals **are orbitals of the same energy**. In a multi-electron atom the orbitals in a sub-levels are degenerate. Hund’s rule states that when filling degenerate orbitals electrons fill them singly first with parallel spins.

## What are degenerate orbitals?

Degenerate orbitals are **orbitals that have the same energy**. Each atomic orbital can have maximum of two electrons. There are only two electrons in the first shell as it has only s atomic orbitals.

## How many degenerate orbitals are present in a subshell?

**Three degenerate orbitals**. The number of degenerate orbitals is same as the subshell which has orbital magnetic moment μL=3.46 BM.

## How many degenerate orbitals are there in the N 3 shell of the hydrogen atom?

nine orbitals

There are nine orbitals in the n = 3 shell. There is one orbital in the 3s subshell and three orbitals in the 3p subshell.

## How do you calculate degenerate energy levels?

So the degeneracy of the energy levels of the hydrogen atom is **n ^{2}**. For example the ground state n = 1 has degeneracy = n

^{2}= 1 (which makes sense because l and therefore m can only equal zero for this state).

## What are degenerate orbitals give examples?

Degenerate Orbitals Example

Example: **An atom has four orbitals namely s p d and f**. The p orbital has three orbitals px py and pz. All these three orbitals have similar energy belonging to the same orbital (p) hence are called degenerate molecular orbitals.

## What are non degenerate orbitals?

**When you apply a magnetic field the electrons in the same orbital**are not degenerate.

## What is the difference between DXY and dx2 y2 orbitals?

Difference: The **four** lobes of dxy lie in xy plane at an angle with the x and y axes whereas dx^-y^2 has all four lobes along the x and y axes. Quantum mechanically dxy belongs to the “t2g” set of d orbitals but dx^2-y^2 belongs to the “eg” set of d orbitals.

## Which quantum number is same for degenerate orbitals?

So we can say that degenerate orbitals have the **same principal quantum number** and azimuthal quantum number. As we can see from the above example that the principal quantum number for all 2p subshell is 2 and for all 2p subshell azimuthal quantum number is 1.

## How many orbitals can n 4 have?

l = 3 m_{1} = –3 –2 –1 0 1 2 3 seven 4f orbitals. Hence the number of possible orbitals when n = 4 are **sixteen**.

## How many electrons can NL 4 have in an atom?

In an atom both 4s (n = 4 l = 0) and (n = 3 l = 1) orbitals can have n + l =4. Since four orbitals are involved they can have maximum of **eight electrons**.

## Why do orbitals only have 2 electrons?

**no two electrons in the same atom can have identical values for all four of their quantum numbers**. In other words (1) no more than two electrons can occupy the same orbital and (2) two electrons in the same orbital must have opposite spins (Figure 46(i) and (ii)).

## What does degenerate mean in chemistry?

**are of equal energy**.

## Which atomic orbital can accommodate a maximum?

**S orbital**can only accommodate a max of 2 electrons. P orbitals on the other hand can accommodate 6 electrons. D orbitals can have up to 10 electrons and F orbitals can carry 14 electrons.

## How many electrons can each of the following orbitals hold?

Any orbital can hold a maximum of **2 electrons** with opposite spin. The first shell has one 1s orbital and holds 2 electrons. The second shell holds 8 electrons 2 in a 2s orbital and 6 in three 2p orbitals. The third shell holds 18 electrons 2 in a 3s orbital 6 in three 3p orbitals and 10 in five 3d orbitals.

## In which of the following five 3d orbitals are degenerated?

In **a 3d subshell** all the five orbitals are degenerate.

## Which of the following orbitals are degenerate in 3dxy II 4dxy III 3dyz?

Answer: **3dxy** and are degenerate.

## Which of the following set of quantum number represents degenerate orbitals?

Answer and Explanation: The greatest number of degenerate orbitals is found in B. **n = 4 l = 3**.

## Which orbitals are degenerate in a Multielectron atom?

**Multielectron Atoms**

- Electron shell: All the orbitals with the same value of n.
- Electron subshell: All the orbitals with the same value of n and ℓ. Electrons in the same subshell are degenerate (i.e. have same energies).

## Which electron configuration violates Hunds?

Here in **p orbital one subshell is vacant but one subshell is doubly filled or full filled**. This type of electronic configuration violated the Hund’s rule.

## What is Hund’s rule of maximum multiplicity explain with suitable example?

Hund’s rule of maximum multiplicity is a **rule based on observation of atomic spectra** which is used to predict the ground state of an atom or molecule with one or more open electronic shells. For example for boron through neon the electron filling order of the 2p orbitals follows Hund’s Rule.

## How many degenerate orbitals are present in a subshell if electron present in that Subshell possesses orbital angular momentum equal to?

Number of degenerated orbitals are same as in subshell which possesses μL=**3**.

## How many degenerate orbitals are present in ethane?

The ethane molecule has fourteen valence electrons that are distributed across seven bonding molecular orbitals. **Four molecular orbitals** exist as degenerate pairs.

## How many degenerate orbitals are in the 5d Subshell?

The total number of degenerate atomic orbitals of d sub-shell is **5** ( -2 -1 0 +1 +2 ).

## How many orbitals does n 6 have?

The quantum number n represents the shell number and n = 6 represents the 6th shell (and sixth period on the periodic table). The quantum number l represents the subshell number and l = 3 represents f-orbitals so there will be **7 orbitals** in a 6f subshell.

## Practice Exercise p 231 Electron Configuration and Unpaired Electrons

## Aufbau’s Principle Hund’s Rule & Pauli’s Exclusion Principle – Electron Configuration – Chemistry

## How To Determine The Number of Paired and Unpaired Electrons

## CHM122 2_4_4 Degenerate Orbitals