The reaction of barium with bromine is similar to that of magnesium with bromine. Write the balanced chemical equation for the reaction of barium with bromine. Include phase symbols.
The correct answer and explanation is :
Balanced Chemical Equation:
[
\text{Ba}(s) + \text{Br}_2(g) \rightarrow \text{BaBr}_2(s)
]
Explanation:
- Understanding the Reactants
- Barium (Ba) is an alkaline earth metal located in Group 2 of the periodic table. It is a highly reactive metal, especially with nonmetals such as bromine.
- Bromine (Br₂) is a diatomic halogen that exists as a liquid at room temperature but readily vaporizes into a reddish-brown gas.
- Reaction Process
- Barium reacts with bromine in a similar manner to magnesium because both elements belong to Group 2 (alkaline earth metals). This means they share similar chemical properties, such as forming ionic compounds with halogens.
- When barium (Ba) reacts with bromine (Br₂), barium loses two electrons to form a Ba²⁺ ion while each bromine atom gains one electron to form two Br⁻ ions.
- The Ba²⁺ cation and Br⁻ anions combine to form an ionic compound, barium bromide (BaBr₂).
- Balancing the Equation
- Ba donates two electrons, and Br₂ consists of two bromine atoms that each accept one electron.
- The reaction naturally produces one formula unit of BaBr₂, meaning the equation is already balanced.
- Phase Symbols
- Ba (s) → Solid metal.
- Br₂ (g) → Diatomic bromine gas.
- BaBr₂ (s) → The ionic compound barium bromide, a solid at room temperature.
This reaction is exothermic, releasing heat as barium reacts vigorously with bromine gas.
Here is an artistic depiction of the reaction between barium (Ba) and bromine (Br₂). The image illustrates solid barium metal reacting with reddish-brown bromine gas to form white crystalline barium bromide (BaBr₂), along with an electron transfer representation.