Question

data analysis
for each sect of reactions below, write a balanced molecular, total ionic, and net ionic chemical reactions. use your observations to guide your responses. if no reaction occurs, no reaction is a valid response. if a solid forms, you should have a solid as a product. if a gas evolves, you should have a gas as a product.
a
mg (s) + hcl (aq)
molecular
total ionic
net ionic
b
mg (s) + cuso₄ (aq)
molecular
total ionic
net ionic
c
mg (s) + agno₃ (aq)
molecular
total ionic
net ionic
d
cu (s) + mgso₄ (aq)
molecular
total ionic
net ionic

Explanation:

Step1: Write balanced molecular equation for Mg + HCl

Magnesium reacts with hydrochloric acid to form magnesium chloride and hydrogen gas. The balanced molecular equation is $Mg(s)+2HCl(aq)
ightarrow MgCl_2(aq) + H_2(g)$.

Step2: Write total - ionic equation for Mg + HCl

Break the aqueous compounds into ions. $Mg(s)+2H^{+}(aq)+2Cl^{-}(aq)
ightarrow Mg^{2 +}(aq)+2Cl^{-}(aq)+H_2(g)$.

Step3: Write net - ionic equation for Mg + HCl

Cancel out the spectator ions ($Cl^{-}$). The net - ionic equation is $Mg(s)+2H^{+}(aq)
ightarrow Mg^{2 +}(aq)+H_2(g)$.

Step4: Write balanced molecular equation for Mg + CuSO₄

Magnesium reacts with copper(II) sulfate to form magnesium sulfate and copper. The balanced molecular equation is $Mg(s)+CuSO_4(aq)
ightarrow MgSO_4(aq)+Cu(s)$.

Step5: Write total - ionic equation for Mg + CuSO₄

Break the aqueous compounds into ions. $Mg(s)+Cu^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Mg^{2 +}(aq)+SO_4^{2 -}(aq)+Cu(s)$.

Step6: Write net - ionic equation for Mg + CuSO₄

Cancel out the spectator ions ($SO_4^{2 -}$). The net - ionic equation is $Mg(s)+Cu^{2 +}(aq)
ightarrow Mg^{2 +}(aq)+Cu(s)$.

Step7: Write balanced molecular equation for Mg + AgNO₃

Magnesium reacts with silver nitrate to form magnesium nitrate and silver. The balanced molecular equation is $Mg(s)+2AgNO_3(aq)
ightarrow Mg(NO_3)_2(aq)+2Ag(s)$.

Step8: Write total - ionic equation for Mg + AgNO₃

Break the aqueous compounds into ions. $Mg(s)+2Ag^{+}(aq)+2NO_3^{-}(aq)
ightarrow Mg^{2 +}(aq)+2NO_3^{-}(aq)+2Ag(s)$.

Step9: Write net - ionic equation for Mg + AgNO₃

Cancel out the spectator ions ($NO_3^{-}$). The net - ionic equation is $Mg(s)+2Ag^{+}(aq)
ightarrow Mg^{2 +}(aq)+2Ag(s)$.

Step10: Analyze reaction for Cu + MgSO₄

Copper is less reactive than magnesium, so no reaction occurs. The molecular, total - ionic, and net - ionic equations are: Molecular: $Cu(s)+MgSO_4(aq)
ightarrow No\ reaction$. Total ionic: $Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)$. Net ionic: $Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)$ (no reaction).

Answer:

a. Molecular: $Mg(s)+2HCl(aq)
ightarrow MgCl_2(aq) + H_2(g)$
Total Ionic: $Mg(s)+2H^{+}(aq)+2Cl^{-}(aq)
ightarrow Mg^{2 +}(aq)+2Cl^{-}(aq)+H_2(g)$
Net Ionic: $Mg(s)+2H^{+}(aq)
ightarrow Mg^{2 +}(aq)+H_2(g)$
b. Molecular: $Mg(s)+CuSO_4(aq)
ightarrow MgSO_4(aq)+Cu(s)$
Total Ionic: $Mg(s)+Cu^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Mg^{2 +}(aq)+SO_4^{2 -}(aq)+Cu(s)$
Net Ionic: $Mg(s)+Cu^{2 +}(aq)
ightarrow Mg^{2 +}(aq)+Cu(s)$
c. Molecular: $Mg(s)+2AgNO_3(aq)
ightarrow Mg(NO_3)_2(aq)+2Ag(s)$
Total Ionic: $Mg(s)+2Ag^{+}(aq)+2NO_3^{-}(aq)
ightarrow Mg^{2 +}(aq)+2NO_3^{-}(aq)+2Ag(s)$
Net Ionic: $Mg(s)+2Ag^{+}(aq)
ightarrow Mg^{2 +}(aq)+2Ag(s)$
d. Molecular: $Cu(s)+MgSO_4(aq)
ightarrow No\ reaction$
Total Ionic: $Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)$
Net Ionic: $Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)
ightarrow Cu(s)+Mg^{2 +}(aq)+SO_4^{2 -}(aq)$