Respuesta :
Answer:
- The spectator ions are Rb⁺ and Cl⁻
Explanation:
Spectator ions are the ions that do not take part of the reaction and, so, you do not show them in the net ionic equation.
1) Molecular equation:
You must show the phases
- Rb₂O (aq) + CaCl₂(aq) --> CaO(s) + 2RbCl (aq)
You are told both Rb₂O and CaCl₂ are in aqueous solutions, so you know their phases and you can write their ionization equations.
2) Ionization
- Rb₂O (aq) → 2Rb⁺ + O⁻, and
- CaCl₂(aq) → Ca²⁺ + 2Cl⁻
- CaO: as per solubility rules most oxides are usually insoluble. CaO, is slightly soluble. Then, for this exercise you can consider that most CaO is a precipitate (solid phase)
- RbCl: as per solubility rules msot chlorides are soluble and RbCl is not an exception, so you get:
RbCl(aq) → Rb⁺ (aq) + Cl⁻ (aq)
3) Total ionic equation:
Now you can write the ionic equation:
2Rb⁺(aq) + O⁻ (aq) + Ca²⁺ (aq) + 2Cl⁻ (aq) → CaO(s) + 2Rb⁺(aq) + 2Cl⁻(aq)
4) Net ionic equation:
Cancel the ions that appear in the same form in the reactant and product sides:
- O⁻ (aq) + Ca²⁺ (aq) → CaO(s)
So, you canceled 2Rb⁺ and 2Cl⁻ because they are the spectator ions.
The study of chemicals and bonds is chemistry. There are different types of elements and these are metals and nonmetals.
The correct answer is The spectator ions are[tex]Rb^+ \ and\ Cl^-[/tex].
What are ions?
The elements which will gain electrons or donate electrons to full fill its outer shell are called ions.
The molecule equation will be:-
The Molecular equation will be
[tex]Rb_2O (aq) + CaCl_2(aq) --> CaO(s) + 2RbCl (aq)[/tex]
You are told both Rb₂O and CaCl₂ are in aqueous solutions, so you know their phases and you can write their ionization equations.
The Ionization process will be:-
[tex]Rb_2O (aq) ---> 2Rb^+ + O^-\\CaCl_2(aq) ---> Ca^{2+} + 2Cl^-[/tex]
- CaO: as per solubility rules most oxides are usually insoluble. Cao is slightly soluble. Then, for this exercise, you can consider that most CaO is a precipitate (solid phase)
- RbCl: as per solubility rules most chlorides are soluble and RbCl is not an exception, so you get:
[tex]RbCl(aq) ---> Rb^+ (aq) + Cl^- (aq)[/tex]
The ionic equation will be:
[tex]2Rb^{2+}(aq) + O^- (aq) + Ca^{2+} (aq) + 2Cl^- (aq) ---> CaO(s) + 2Rb^+(aq) + 2Cl^-(aq)[/tex]
The Net ionic equation will be:-
[tex]O^- (aq) + Ca^{2+} (aq) ----> CaO(s)[/tex]
So, you canceled 2Rb⁺ and 2Cl⁻ because they are the spectator ions.
For more information about the ions, refer to the link;-
https://brainly.com/question/1388366
