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poizon [28]
3 years ago
10

Select the correct location on the image

Chemistry
2 answers:
Lubov Fominskaja [6]3 years ago
8 0

Answer: 3p4, the first box of the 3p orbital

Explanation:

Lera25 [3.4K]3 years ago
7 0

The orbital filled by the last electron from the S element is 3p

<h3>Further explanation </h3>

In an atom there are levels of energy in the skin and sub skin.

This energy level is expressed in the form of electron configurations.

Writing electron configurations starts from the lowest to the highest sub-shell energy level. There are 4 sub skins in the skin of an atom, namely s, p, d and f. The maximum number of electrons for each sub skin is

• s: 2 electrons

• p: 6 electrons

• d: 10 electrons and

• f: 14 electrons

Charging electrons in the sub skin uses the following sequence:

<em>1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc. </em>

Each sub-skin also has an orbital depicted in the form of a square in which there are electrons symbolized by half arrows.

Each orbital in an atom consists of 4 quantum numbers:

  • n is the principal quantum number.
  • l is the angular momentum / azimuthal quantum number
  • ml, the magnetic quantum number
  • ms, the electron-spin quantum number

Value of n: positive integer

value of l: s = 0, p = 1, d = 2, f = 3, ... (n-1)

ml value: between -l to + l

ms value: +1/2 or -1/2

An sulfur atom (S) has 16 electrons means having an electron configuration as follows:

1s², 2s², 2p⁶, 3s², 3p⁴

or we can write with the noble gas symbol

[Ne] 3s² 3p⁴

From this configuration, it has been seen that the last electron (16th electron) occupies a 3p orbital (3p⁴) orbital with a downward symbol

The quantum number:

n = 3

l = 1

ml = -1

ms = -1/2

<h3>Learn more </h3>

electron transitions

brainly.com/question/2079874

the locations and properties of two electrons

brainly.com/question/2292596

It's sublevel

brainly.com/question/4520082

a possible full set of quantum numbers

brainly.com/question/5389767

Keywords: orbitals, subshells, quantum numbers

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