what is the formula of the ion formed when potassium achieves noble gas electron configuration?
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To determine the ion formed when potassium achieves noble gas electron configuration, we need to first identify the noble gas with a similar electron configuration as potassium.
Potassium (K) has the electron configuration [Ar] 4s1, where [Ar] represents the electron configuration of the noble gas argon. Argon has the electron configuration [Ne] 3s2 3p6.
When potassium achieves noble gas electron configuration, it will lose one electron from its outermost energy level (4th energy level).
Hence, the ion formed when potassium achieves noble gas electron configuration will be K+, as it loses one electron and becomes a positively charged ion.
To determine the formula of the ion formed when potassium achieves noble gas electron configuration, we need to understand the electron configuration of potassium and the concept of noble gases.
The electron configuration of potassium is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹. Noble gases are a group of elements in the periodic table that have completely filled electron shells, making them stable and chemically unreactive.
To achieve a noble gas electron configuration, an atom must either lose or gain electrons to reach the electron configuration of the nearest noble gas. In the case of potassium (K), which has one electron in the outermost shell (4s¹), it is easier for this atom to lose its outermost electron rather than gain seven more electrons to reach the electron configuration of argon (the nearest noble gas).
By losing this one electron, potassium forms a positive ion with a charge of +1, represented as K⁺. The formula of the ion formed is simply the symbol of the element (K) followed by the charge written as a superscript (+1).
Therefore, the formula of the ion formed when potassium achieves noble gas electron configuration is K⁺.