IDNLearn.com is the perfect place to get answers, share knowledge, and learn new things. Ask any question and receive accurate, in-depth responses from our dedicated team of experts.
Sagot :
To determine the compounds that aluminum (Al) can form to dissolve in water, we will consider aluminum combining with each of the given ions: oxide ([tex]\( O^{2-} \)[/tex]), sulfide ([tex]\( S^{2-} \)[/tex]), and nitrate ([tex]\( NO_3^{-} \)[/tex]).
Aluminum typically forms a [tex]\( Al^{3+} \)[/tex] ion. We must combine this [tex]\( Al^{3+} \)[/tex] ion with each of the given anions to predict the resulting compounds.
### Combining Aluminum with Oxide ([tex]\( O^{2-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The oxide ion has a charge of [tex]\( -2 \)[/tex] (i.e., [tex]\( O^{2-} \)[/tex]).
To balance the charges, we need a total positive charge and total negative charge that are equal. The least common multiple of 3 and 2 is 6. Therefore:
- Two [tex]\( Al^{3+} \)[/tex] ions will provide a total positive charge of [tex]\( 2 \times (+3) = +6 \)[/tex].
- Three [tex]\( O^{2-} \)[/tex] ions will provide a total negative charge of [tex]\( 3 \times (-2) = -6 \)[/tex].
Thus, the compound formed is [tex]\( Al_2O_3 \)[/tex] (Aluminum oxide).
### Combining Aluminum with Sulfide ([tex]\( S^{2-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The sulfide ion has a charge of [tex]\( -2 \)[/tex] (i.e., [tex]\( S^{2-} \)[/tex]).
As with the oxide ion, we need to balance the charges. Using the least common multiple of 3 and 2, which is 6:
- Two [tex]\( Al^{3+} \)[/tex] ions will give a total positive charge of [tex]\( 2 \times (+3) = +6 \)[/tex].
- Three [tex]\( S^{2-} \)[/tex] ions will give a total negative charge of [tex]\( 3 \times (-2) = -6 \)[/tex].
Thus, the compound formed is [tex]\( Al_2S_3 \)[/tex] (Aluminum sulfide).
### Combining Aluminum with Nitrate ([tex]\( NO_3^{-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The nitrate ion has a charge of [tex]\( -1 \)[/tex] (i.e., [tex]\( NO_3^{-} \)[/tex]).
For the charges to balance:
- One [tex]\( Al^{3+} \)[/tex] ion will require three [tex]\( NO_3^{-} \)[/tex] ions to balance out its [tex]\( +3 \)[/tex] charge.
Thus, the compound formed is [tex]\( Al(NO_3)_3 \)[/tex] (Aluminum nitrate).
### Conclusion
The compounds that aluminum (Al) forms to dissolve in water with the given ions are:
- Aluminum oxide: [tex]\( Al_2O_3 \)[/tex]
- Aluminum sulfide: [tex]\( Al_2S_3 \)[/tex]
- Aluminum nitrate: [tex]\( Al(NO_3)_3 \)[/tex]
Aluminum typically forms a [tex]\( Al^{3+} \)[/tex] ion. We must combine this [tex]\( Al^{3+} \)[/tex] ion with each of the given anions to predict the resulting compounds.
### Combining Aluminum with Oxide ([tex]\( O^{2-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The oxide ion has a charge of [tex]\( -2 \)[/tex] (i.e., [tex]\( O^{2-} \)[/tex]).
To balance the charges, we need a total positive charge and total negative charge that are equal. The least common multiple of 3 and 2 is 6. Therefore:
- Two [tex]\( Al^{3+} \)[/tex] ions will provide a total positive charge of [tex]\( 2 \times (+3) = +6 \)[/tex].
- Three [tex]\( O^{2-} \)[/tex] ions will provide a total negative charge of [tex]\( 3 \times (-2) = -6 \)[/tex].
Thus, the compound formed is [tex]\( Al_2O_3 \)[/tex] (Aluminum oxide).
### Combining Aluminum with Sulfide ([tex]\( S^{2-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The sulfide ion has a charge of [tex]\( -2 \)[/tex] (i.e., [tex]\( S^{2-} \)[/tex]).
As with the oxide ion, we need to balance the charges. Using the least common multiple of 3 and 2, which is 6:
- Two [tex]\( Al^{3+} \)[/tex] ions will give a total positive charge of [tex]\( 2 \times (+3) = +6 \)[/tex].
- Three [tex]\( S^{2-} \)[/tex] ions will give a total negative charge of [tex]\( 3 \times (-2) = -6 \)[/tex].
Thus, the compound formed is [tex]\( Al_2S_3 \)[/tex] (Aluminum sulfide).
### Combining Aluminum with Nitrate ([tex]\( NO_3^{-} \)[/tex])
1. Aluminum has a charge of [tex]\( +3 \)[/tex] (i.e., [tex]\( Al^{3+} \)[/tex]).
2. The nitrate ion has a charge of [tex]\( -1 \)[/tex] (i.e., [tex]\( NO_3^{-} \)[/tex]).
For the charges to balance:
- One [tex]\( Al^{3+} \)[/tex] ion will require three [tex]\( NO_3^{-} \)[/tex] ions to balance out its [tex]\( +3 \)[/tex] charge.
Thus, the compound formed is [tex]\( Al(NO_3)_3 \)[/tex] (Aluminum nitrate).
### Conclusion
The compounds that aluminum (Al) forms to dissolve in water with the given ions are:
- Aluminum oxide: [tex]\( Al_2O_3 \)[/tex]
- Aluminum sulfide: [tex]\( Al_2S_3 \)[/tex]
- Aluminum nitrate: [tex]\( Al(NO_3)_3 \)[/tex]
Thank you for using this platform to share and learn. Don't hesitate to keep asking and answering. We value every contribution you make. Find precise solutions at IDNLearn.com. Thank you for trusting us with your queries, and we hope to see you again.
