Metals and nonmetals can react with each other to form ions. complete these statements.
a potassium atom gain or loses(electrons/protons/neutrons)an d to form how many ion?
a sulfuratom gain or loses (electrons/protons/neutrons) and to form how many ion?

A potassium atom loses (electrons) to form K⁺ ions

A sulfur atom gain (electrons) to form S²⁻ ions

Atoms have different stability. Unstable atomic atoms will try to form stable electron configurations like those of noble gases. Where noble has the number of outer electrons 2 or 8

The formation of electron configurations can be done by forming shared ions or electron pairs

atoms that have low ionization energy (easily release electrons) forms cations, and these electrons are bound to have large affinity energy (easily pulling electrons) that form anions

Metal elements have low ionization energy and non-metallic elements have a high electron affinity

The location of the element group is the number of valence electrons that fill the last sub-skin

The element period is determined from the valence shell (the largest main quantum number (n))

The chemical element of the group is divided into two, namely:

Group A, occupies sub skin and p

Group B, sub skin occupies d

The electron configuration of noble gases is:

He: 1s²

Ne: [He] 2s² 2p⁶

Ar: [Ne] 3s² 3p⁶

Cr: [Ar] 3d¹⁰ 4s² 4p⁶

Let's look at the statement

Electron configuration

[Ar] 4s¹

The K element is closestto the configuration of the Ar element releasing 1 electron to be stable, becoming K⁺

Electron configuration

[Ne] 3s² 3p⁴

The S element is closest to the configuration of the Ar element by binding 2 electrons to be stable, becoming S²⁻

the chemical bond holds the Na⁺ and Cl⁻ ions

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Identify the group number

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ionic bonding

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Keywords: noble gas, stable, electron configuration

a