Predict the products and write a balanced equation for each...

Predict the products and write a balanced equation for each of the following: $(8.1,8.2,8.3)$ Electicity a. decomposition: $\mathrm{NaCl}(s)$ $\stackrel{\text { Electricity }}{\longrightarrow}$ ______ $+$______ b. combination: $\mathrm{Ca}(s)+\mathrm{Br}_{2}(l) \longrightarrow$______ c. combustion: $\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow}$______ $+$______ d. double replacement: $\mathrm{NiCl}_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow$______ $+$______

Predict the products and write a balanced equation for each of the following: $(8.1,8.2,8.3)$ Electicity
a. decomposition: $\mathrm{NaCl}(s)$ $\stackrel{\text { Electricity }}{\longrightarrow}$ ______ $+$______
b. combination: $\mathrm{Ca}(s)+\mathrm{Br}_{2}(l) \longrightarrow$______
c. combustion:
$\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow}$______ $+$______
d. double replacement:
$\mathrm{NiCl}_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow$______ $+$______

Key Concepts

Electrolysis

Electrolysis is a process that uses electrical energy to drive a non-spontaneous chemical reaction, often leading to the decomposition of compounds into their elemental components. This concept is essential in topics where external energy sources, such as electricity, are used to initiate and sustain chemical transformations.

Double Replacement Reactions

Double replacement reactions involve the exchange of ions between two compounds, resulting in the formation of two new compounds. These reactions typically occur in aqueous solutions and often lead to the formation of a precipitate, a gas, or a weak electrolyte, illustrating the principle of ion exchange in chemical processes.

Balancing Chemical Equations

Balancing chemical equations is the method of ensuring that the number of atoms for each element is the same on both sides of the reaction. This process is critical for upholding the law of conservation of mass and accurately representing chemical reactions in quantitative terms.

Combination Reactions

Combination reactions, also known as synthesis reactions, occur when two or more reactants combine to form a single, more complex product. These reactions are typically exothermic and are fundamental in showing how simple substances can combine to create more complex compounds during chemical processes.

Decomposition Reactions

Decomposition reactions involve breaking a single compound into two or more simpler substances. These reactions often require the input of energy in the form of heat, light, or electricity, and they are essential for understanding how complex compounds can be broken down into their constituent elements or simpler compounds under certain conditions.

Combustion Reactions

Combustion reactions are a type of redox reaction where a substance reacts rapidly with oxygen, releasing energy in the form of heat and light. They are characterized by the production of common byproducts such as carbon dioxide and water when organic compounds are burned, and they play a significant role in both energy production and various industrial processes.

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