## What are the possible values of quantum number L when n 4?

For n = 4, l can have values of **0, 1, 2, and 3**.

## How many values of ML are possible for an electron with orbital quantum number L 4?

Answer and Explanation: **Nine** values of ml are possible for an electron with orbital quantum number l = 4.

## How many values of ML are possible for an electron with orbital quantum number L 2?

Therefore, given l=2 , the possible ml values are **−2,−1,0,1,2** .

## How many values of ML are possible for an electron with orbital quantum number L 1 Express your answer as an integer?

The values of the magnetic quantum number range from -l to l so the possible values of ml for the 4d orbital are **-2 -1 0 1 and 2**.

## What are the possible values of L if’n 4 quizlet?

Therefore, for n = 4 n = 4 n=4, the possible values of l l l are **0, 1, 2, 3**.

## What are the possible values of L?

The Orbital Angular Momentum Quantum Number (l) If n=7, what are the possible values of l? Since l can be zero or a positive integer less than (n−1), it can have a value of **0, 1, 2, 3, 4, 5 or 6**.

## How many possible values are there for the principal quantum number?

The principal quantum number (n) **cannot be zero**. The allowed values of n are therefore 1, 2, 3, 4, and so on. The angular quantum number (l) can be any integer between 0 and n – 1. If n = 3, for example, l can be either 0, 1, or 2.

## What are the possible values for the quantum numbers n L and ML?

Follow the rules for allowable quantum numbers found in the text. **l values can be integers from 0 to n-1; ml can be integers from -l through 0 to + l**. 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 are the possible values of quantum number L when n-1?

When n = 1, **l= 0** (l takes on one value and thus there can only be one subshell)

## What are the possible values for the magnetic quantum number ml when the principal quantum number n is 3 and the angular quantum number L is 1?

Possible values for ml=**−2,−1,0,+1,+2**.

## What are possible values of L for each of the following values of n?

**Answer:**

- The possible values of l is from 0 to n-1. So, when n=1, l=0. when n=2, l=0, 1. when n=3, l=0, 1, 2. when n=4, l=0, 1, 2, 3.
- The possible values of ml is from 0 to l, both positive and negative values. So, when l=0, ml=0. when l=1, ml= 0, 1, -1. when l=2, ml= 0, 1, -1, 2, -2. when l=3, ml= 0, 1, -1, 2, -2, 3, -3. Home.

Mar 13, 2018

## What values of L are possible for n 5?

Solution: The principle quantum number(n), describe the energy level in which the electron an be found. Therefore, the possible values of l if n = 5 are **0, 1, 2 , 3, 4**.

## What is the L quantum number?

The angular momentum quantum number is symbolized by l. **l indicates the shape of the orbital**. This will tell us the shape of the orbital. Values for l are dependent on n, so the values for l go from zero all the way up to n minus one, so it could be zero, one, two, or however values there are up to n minus one.

## What are the L values for n 5?

The principle quantum number(n), describe the energy level in which the electron an be found. Therefore, the possible values of l if n = 5 are **0, 1, 2 , 3, 4**.

## What are possible values of L?

It describes the shape of orbitals and is in a relationship with principal quantum number (n). For a given value of n, l can be determined as **l = 0 to n – 1**. If, l = 0 corresponds to an s-subshell, l = 1 corresponds to a p-subshell, l = 2 corresponds to a d-subshell, l = 3 corresponds to an f-subshell, and so on.

## How many Subshells are in the n 4 shell?

four sub-shells Solution. The **four** sub-shells are associated with n = 4, which are s, p, d and f. The number of orbitals = 16.

## Which values of ML are possible within the 4s subshell?

These two quantum numbers correspond to an electron located on the fourth energy level, in the 4s-subshell. In this particular case, ml can only take one possible value, **ml=0** . This means that you electron will be located in the 4s orbitals.

## What are the possible values of n and ML for an electron in a 4f orbital?

Solution : The possible values of n, l `and m _(l)` quantum numbers for 4 f orbital are : <br> `**n = 4, L =3 , m _(l ) =-3, -2, -1, 0, + 1, + 2, + 3**. `

## What are the possible values of quantum number L when n 2?

When n = 2, l= **0, 1** (l takes on two values and thus there are two possible subshells)

## How many possible values for L and ML are there for?

**l values can be integers from 0 to n-1; ml can be integers from -l through 0 to + l**. 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 are the possible values of ML when L 1?

Answer: the possible values of ml are **-1, 0 and +1** because the range of values are from -l to +l.

## How do you find quantum number L?

0:004:24How To Determine The 4 Quantum Numbers From an Element or a …YouTube

## What are the 4 quantum numbers?

In atoms, there are a total of four quantum numbers: **the principal quantum number (n), the orbital angular momentum quantum number (l), the magnetic quantum number (ml), and the electron spin quantum number (ms)**.

## What are the possible values of L for each value of n?

l values can be **integers from 0 to n-1**; ml can be integers from -l through 0 to + l. 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 values of L are possible for n 3?

The angular quantum number (l) can be any integer between 0 and n – 1. If n = 3, for example, l can be either **0, 1, or 2**.

## How many possible states are there for the L 4 state?

18 possible states l = 4: 9 m values are possible, 2 ms values are possible. There are 9*2 = **18** possible states.

## What is quantum number L?

The angular quantum number (l) **describes the shape of the orbital**. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2).

## How many values of the quantum number L are possible when?

The angular quantum number (l) can be **any integer between 0 and n – 1**. If n = 3, for example, l can be either 0, 1, or 2.

## What are the orbitals for n 4?

Orbitals and Electron Capacity of the First Four Principle Energy Levels | ||
---|---|---|

Principle energy level (n) | Type of sublevel | Number of orbitals per level(n2) |

4 | s | 16 |

p | ||

d |

## How many Subshells are in L shell?

two subshells The first K shell has one subshell, called '1s'; the L shell has **two subshells**, called '2s' and '2p'; the third shell has '3s', '3p', and '3d'; and so on. A subshell is the set of states defined by azimuthal quantum number, l, within a shell.