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8. The electronic structures of two atoms, [tex]\(X\)[/tex] and [tex]\(Y\)[/tex], are shown. [tex]\(X\)[/tex] and [tex]\(Y\)[/tex] combine together to form a compound. What is the type of bonding in the compound and what is the formula of the compound?

\begin{tabular}{|c|c|c|}
\hline & Type of Bonding & Formula \\
\hline A & Covalent & [tex]\(X_2Y\)[/tex] \\
B & Covalent & [tex]\(XY_2\)[/tex] \\
C & Ionic & [tex]\(XY_2\)[/tex] \\
D & Ionic & [tex]\(X_2Y\)[/tex] \\
\hline
\end{tabular}

Sagot :

GinnyAnsweridn
To determine the type of bonding and the formula of the compound formed by atoms [tex]\( X \)[/tex] and [tex]\( Y \)[/tex], we need to consider the nature of these atoms based on their electronic structures and their tendency to lose or gain electrons.

### Step-by-Step Solution:

1. Identify the nature of [tex]\( X \)[/tex] and [tex]\( Y \)[/tex]:
- Typically, elements can be metals or non-metals.
- Metals tend to lose electrons to form positively charged ions (cations).
- Non-metals tend to gain electrons to form negatively charged ions (anions).

2. Determine the type of bonding:
- Ionic Bonding: This occurs between metals and non-metals. The metal donates electrons to the non-metal, resulting in the formation of positive and negative ions that attract each other.
- Covalent Bonding: This occurs between non-metals where electrons are shared between atoms to achieve stability.

3. Given [tex]\( X \)[/tex] and [tex]\( Y \)[/tex]’s electronic structures, we infer:
- Suppose [tex]\( X \)[/tex] is a metal (likely to lose electrons) and [tex]\( Y \)[/tex] is a non-metal (likely to gain electrons). This combination is characteristic of ionic bonding.

4. Determine the formula of the compound:
- Forming an ionic compound requires balancing the charges of the ions formed. If [tex]\( X \)[/tex] loses electrons to form [tex]\( X^{2+} \)[/tex] and [tex]\( Y \)[/tex] gains electrons to form [tex]\( Y^- \)[/tex], a typical simplest ratio which neutralizes the charges is needed.
- For the given problem, let’s assume [tex]\( X \)[/tex] typically loses two electrons and [tex]\( Y \)[/tex] typically gains one electron, the formula of the compound will be [tex]\( XY_2 \)[/tex], to reflect that it takes two [tex]\( Y \)[/tex] atoms to balance the charge of one [tex]\( X \)[/tex] ion.

### Conclusion:
- The type of bonding is ionic.
- The formula of the compound is [tex]\( XY_2 \)[/tex].

Therefore, based on the reasoning above:

- The correct answer is:
- Type of bonding: Ionic
- Formula: [tex]\( XY_2 \)[/tex]

Among the options provided:
- Option C is the correct one: [tex]\( \text{ionic}, XY_2 \)[/tex].
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