Consider the following Lewis symbols for elements X and Y:

c. What ions would be formed by X and Y?

Guida verificata passo dopo passo

Step 1: Analyze the Lewis symbols provided in the image. The element 'M' has six valence electrons, represented by six dots around the symbol. The element 'N' has one valence electron, represented by a single dot around the symbol.

Step 2: Determine the electron configuration and stability of each element. Element 'M' needs two more electrons to complete its octet (8 valence electrons), while element 'N' needs to lose one electron to achieve a stable electron configuration.

Step 3: Predict the type of ions formed based on the electron transfer. Element 'M' will likely gain two electrons to form an anion with a charge of -2 (M²⁻), while element 'N' will lose one electron to form a cation with a charge of +1 (N⁺).

Step 4: Write the chemical symbols for the ions formed. The anion formed by 'M' is represented as M²⁻, and the cation formed by 'N' is represented as N⁺.

Step 5: Confirm the charges and stability of the ions. The transfer of electrons between 'M' and 'N' ensures that both achieve stable electron configurations, satisfying the octet rule for 'M' and the empty valence shell for 'N'.

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