The correct answer is option 1) (iii) 2KBr (aq) + Bal2(aq) → 2Kl(aq) + BaBr2(s)
potassium bromide (KBr) and barium iodide (BaI2) exchange ions to form potassium iodide (KI) and barium bromide (BaBr2). This reaction demonstrates the characteristic exchange of ions between two compounds, making it a double displacement reaction.
- The reactants are potassium bromide (KBr) and barium iodide (BaI2).
- In potassium bromide (KBr), potassium (K+) is the cation, and bromide (Br-) is the anion.
- In barium iodide (BaI2), barium (Ba2+) is the cation, and iodide (I-) is the anion.
- In a double displacement reaction, the cations and anions of the reactants switch partners to form new compounds. In this case:
- The potassium cation (K+) from KBr combines with the iodide anion (I-) from BaI2 to form potassium iodide (KI).
- The barium cation (Ba2+) from BaI2 combines with the bromide anion (Br-) from KBr to form barium bromide (BaBr2).
Ionic equation, focusing on the species that are involved in the chemical change:
2K+(aq) + 2I-(aq) + Ba2+(aq) + 2Br-(aq) → 2K+(aq) + 2I-(aq) + BaBr2(s)
Key Points
- A double-displacement or replacement reaction occurs when parts of two ionic compounds are exchanged, making two new compounds.
- A characteristic of a double-replacement equation is that there are two compounds as reactants and two different compounds as products.
- Double displacement reactions usually occur in an aqueous solution.
- Ions in the compounds are free to move and interact with each other.
- Compounds consist of positively charged ions (cations) and negatively charged ions (anions).
- A double displacement reaction is used to synthesize specific compounds, precipitation reactions, and acid-base reactions.
Additional Information Types of chemical reactions:
- Combination (Synthesis) Reactions:
- Two or more substances combine to form a single product
Example: 2H2(g) + O2(g) → 2H2O(l)
A single compound breaks down into two or more simpler substances.
General form: AB → A + B.
Example: 2H2O(l) → 2H2(g) + O2(g)
- Single Replacement (Displacement) Reactions:
An element replaces another element in a compound, resulting in the formation of a new compound and a free element.
General form: A + BC → AC + B.
Example: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) (zinc displaces hydrogen from hydrochloric acid).
- Double Displacement (Metathesis) Reactions:
The cations and anions of two different compounds exchange places to form new compounds.
General form: AB + CD → AD + CB.
Example: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) (formation of silver chloride and sodium nitrate).
- Redox (Oxidation-Reduction) Reactions:
Electrons are transferred between reactants. One substance loses electrons (oxidation), and another gains electrons (reduction).
Examples:
2Mg(s) + O2(g) → 2MgO(s) (oxidation of magnesium, reduction of oxygen).
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s) (oxidation of copper, reduction of silver ions).
A substance reacts rapidly with oxygen, usually producing heat and light.
Often involves hydrocarbons (compounds of hydrogen and carbon).
Examples:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) (combustion of methane).
C6H12O6(aq) + 6O2(g) → 6CO2(g) + 6H2O(l) (combustion of glucose).
- Acid-Base (Neutralization) Reactions:
An acid reacts with a base to produce salt and water.
General form: Acid + Base → Salt + Water.
Example: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) (neutralization of hydrochloric acid and sodium hydroxide).
Two soluble compounds in aqueous solution react to form an insoluble product (precipitate).
General form: AB(aq) + CD(aq) → AD(s) + CB(aq).
Example: Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq) (formation of lead iodide precipitate).