## How many electrons can be held in a 3d orbital?

The 3d, 4d etc., can each hold **ten electrons**, because they each have five orbitals, and each orbital can hold **two electrons** (5*2=10).

## Why is 3rd shell 8 or 18?

In this sense the **third shell** can hold **8** electrons. In this sense the **third shell** can hold a total of **18** electrons. So the **third shell** can be considered to hold **8 or 18** electrons but in total the **third shell** can hold **18** electrons.

## How many electrons can 4s hold?

Maximum number of electron in an energy level (2n2)

Principal Energy Level (n) | sublevels | total electrons |
---|---|---|

2 | 2s 2p | 8 |

3 | 3s 3p 3d | 18 |

4 | 4s 4p 4d 4f |
32 |

5 | 5s 5p 5d 5f 5g | 50 |

## What is the maximum number of electrons in 3d sublevel?

The s **sublevel** has just one orbital, so can contain 2 **electrons** max. The p **sublevel** has 3 orbitals, so can contain 6 **electrons** max. The d **sublevel** has 5 orbitals, so can contain 10 **electrons** max. And the 4 **sublevel** has 7 orbitals, so can contain 14 **electrons** max.

## Why is 3d higher energy than 4s?

The **3d** orbitals have a slightly **higher energy than** the **4s** orbitals. So because the **4s** orbitals has the lower **energy**, it gets filled first. When **3d** orbitals are filled, **4s** is no longer lower in **energy**.

## Why does the third shell have 8 electrons?

The **electron** capacity of the **third shell** is **8**, when there are no **shells** above it. And that is the case for all elements in the **third** period. It is only when there are outer **shells** surrounding it that the **third** (or higher) **shell has** a higher capacity.

## What is the 2 8 8 rule in chemistry?

There is a **2**–**8**–**8 rule** for these elements. The first shell is filled with **2** electrons, the second is filled with **8** electrons, and the third is filled with **8**. You can see that sodium (Na) and magnesium (Mg) have a couple of extra electrons. They, like all atoms, want to be happy.

## Why does the third period contain 8 elements but not 18?

According to the 2n^{2} rule, the maximum number of electrons in the **third period** = 2 x (3)^{2} = **18**. But, the last shell cannot accommodate more than **8** electrons so, the number of electrons in **third period** is **8**. Hence, the number of **elements** is also **8**.

## Why are the shells named KLMN?

The **names** of the electron **shell** were given by a spectroscopist **named** Charles G Barkla. He **named** the innermost **shell** has k **shell** because he noticed that the X-rays emitted two types energies. These energies were **named** as type A that is higher energy X-ray and type B that is lower energy X-ray.

## What is meant by 3p 3?

#33 **what is meant by 3p3**? **3rd** orbital in p sublevel **3** electrons. #34a give the electron configuration for Na. 1s2 2s2 2p6 3s1.

## How many electrons are in a shell?

Each shell can contain only a fixed number of electrons: The first shell can hold up to **two electrons**, the second shell can hold up to eight (2 + 6) electrons, the third shell can hold up to **18** (2 + 6 + 10) and so on. The general formula is that the nth shell can in principle hold up to 2(n^{2}) electrons.

## How many electrons can 5s hold?

5s (which holds **2 electrons**), 5p (which holds 6), 5d (holds 10), and 5f (holds 14) for a total of 32 electrons. After that, the fifth, sixth, and seventh energy levels also have four sublevels each. 6. Sublevels are designated or symbolized, by the letters s, p, d, and f.

## Which element has 3 electrons in the n 4 energy level?

Element | Element Number | Number of Electrons in each Level |
---|---|---|

Sodium | 11 | 1 |

Magnesium | 12 | 2 |

Aluminum | 13 | 3 |

Silicon |
14 | 4 |

## What sublevels do not exist?

The answer is (b) 2d. The third energy level, the electrons are located only in the s and p subshell so 2d subshell **do not exist**. For the s subshell, the lowest energy level is 1 (1s).

## Which element has 3 electrons in the 2p sublevel?

**Lithium** has 3 electrons; 2 of the 3 electrons occupy the **s** sublevel in principal energy level 1.

3G – Electron Configuration Notations.

Name | Atomic Number |
Electron Configuration |
---|---|---|

Phosphorus | 15 | 1s^{2} 2s^{2}2p^{6}3s^{2}3p^{3} |

Sulfur |
16 | 1s^{2} 2s^{2}2p^{6}3s^{2}3p^{4} |

Chlorine | 17 | 1s^{2} 2s^{2}2p^{6}3s^{2}3p^{5} |

Argon |
18 | 1s^{2} 2s^{2}2p^{6}3s^{2}3p^{6} |