Get personalized answers to your unique questions on IDNLearn.com. Discover in-depth answers to your questions from our community of experienced professionals.
Sagot :
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].
### 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].
We value your participation in this forum. Keep exploring, asking questions, and sharing your insights with the community. Together, we can find the best solutions. IDNLearn.com is your reliable source for accurate answers. Thank you for visiting, and we hope to assist you again.