Table of Contents

## How many different values of ML are possible for n 5?

There are **16 different values** of ml when the principal quantum number is n = 5. The fifth energy level is the fifth row on the periodic table which…

## How many electrons can be found at the principal quantum number 5?

SImply put two electrons of opposite spins can share one orbital (given by ml=1 ) per subshell (given by l ). Therefore total of **8 electrons** that can share those two quantum numbers.

## What are all possible quantum numbers for when n 5?

Answer: For n=5 we can have **l=4 3 2 1 and 0**.

## What are the possible values of the principal quantum number n What are the possible values of the principal quantum number n?

**1 2 3 4**and so on. The angular quantum number (l) can be any integer between 0 and n – 1.

## How many different values of ML are possible?

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.

## How many different values of ML are possible when the principal quantum number is N 4?

Indicate the number of subshells the number of orbitals in each subshell and the values of l and ml for the orbitals in the n = 4 shell of an atom. For n = 4 l can have values of **0 1 2 and 3**. Thus s p d and f subshells are found in the n = 4 shell of an atom.

## How many electrons does n 5 have?

Energy Level (Principal Quantum Number) | Shell Letter | Electron Capacity |
---|---|---|

3 | M | 18 |

4 | N | 32 |

5 | O | 50 |

6 | P | 72 |

## How many possible orbitals and how many electrons can inhabit the energy level n 5?

**5**and so on. To calculate the maximum number of electrons in each energy level the formula 2n

^{2}= 25 orbitals^{2}can be used where n is the principal energy level (first quantum number).

## What are the allowed values of L when the principal quantum number is N 5?

So n=5 means it is the fifth electron shell. ‘l’ is the azimuthal quantum number and it describes electron subshell (s p d etc.). Basically l=0 corresponds to s orbital l=1 – p orbital l=2 – d orbital and **l=3 – f orbital**. So the final notation is 5f.

## What are the possible orbitals for n 5?

We are given principal quantum number n = 5. The possible subshells are s p d f g. **g = 9 orbitals**.

## What are the possible values of quantum number L when n 3?

Because n=3 the possible values of **l = 0 1 2** which indicates the shapes of each subshell.

## What are the values of n and l for the subshells 3s?

**if n=3 and l=0**it is the 3s subshell and so on.

## What are the possible values of the principal quantum number n chegg?

**all the positive integers: 1 2 3 etc.**

## Which is a possible value for the principal quantum number n quizlet?

The principal quantum number n gives the overall energy level and size of the electron’s path. The allowed values of n are the positive integers: **1 2 3** ….

## How many different values of L are possible in the third principal energy level?

n – the principal quantum number the ones that gives the energy level. distinct orbitals. So if each electron is described by an unique set of quantum numbers you can conclude that **18 sets** of quantum numbers are possible for the third energy level.

## How many possible values of ML would there be if l 20?

The possible values for m_{l} is the range of l: –l to +l. There are **41 m _{l} values** when l = 20.

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

The possible values of l is from **0 to n-1**. The possible values of ml is from 0 to l both positive and negative values.

## How many possible combinations are there for the values of L and ML when N 2?

**four possible combinations**for values of l and ml for n = 2. The n = 2 principal energy level includes an s orbital and a p orbital.

## How many possible ML values are there for N 4?

For n = 4 l can have values of 1 2 and 3. Thus s p d and f subshells are found in the n = 4 shell of an atom. For l = 0 (the s subshell) m_{l} can only be 0.

## How many values of ML are possible for an electron with orbital quantum number L 3?

If l = 3 then ml = -3 -2 -1 0 1 2 3 (**7 possible values**) and ms = -1/2 1/2 (2 possible values). 2 × 7 = 14 – it is the number of electrons can be held in a sublevel l = 3.

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

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

## 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.

## 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 orbitals are in the N 5th shell?

**25 orbitals**in 5th shell.

## How many possible orbitals and how many electrons can inhabit the energy level n 4?

**16 orbitals**and a maximum of 32 electrons.

## What is the maximum number of electrons that can exist in each orbital Be sure to explain your answer?

**two electrons**. When in a magnetic field the two electrons in a particular orbital differ very slightly in energy because of a property called electron spin.

## What are the possible Subshells when n 4 How many orbitals are contained by each of these Subshells?

Therefore in n=4 number of subshells=4 orbitals=**16** and number of electrons =32.

## What will be the sum of all possible values of L and M for N is equal to 5?

For any value of l the value of n ranges from -l to +l. In this case the value of n can range from -4 to +4. Therefore the sum of all possible values of l and m for n= 5 is **10**.

## What values of ML are possible for L 2?

Since the value of l is 2 the allowed values of ml **= -2 -1 0 1 2**. Therefore there are five spatial orbitals which can hold electrons in this subshell.

## When n 5 What is the value of L?

The n and l quantum numbers of an electron of an element are n=**5 and l=1**.

## What are all the possible subshells associated with the principal quantum number n if’n 6?

**6s 6p 6d 6f 6g 6h**and the orbitals associated with them are 1 3 5 7 9 11.

## How many orbitals have the following quantum numbers n 5 L 3?

Re: n=5 l=3 ml=-1

n=5 tells you that your quantum number is 5. l=3 tells you that it is 5f. (0-s 1-p 2-d 3-f). ml=-1 is telling you that it will only take the -1 orbital out of the 7 listed above therefore it can only hold 2 electrons.

## How many total orbitals are in the 5th energy level?

**25**.

## What are the possible values for mell when the principal quantum number n is 3 and the angular momentum quantum number ell is 2?

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