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Chapter 21: Problem 10

Select one of the alkaline earth metals and write a balanced chemical equation for its reaction with oxygen. Is the reaction likely to be exothermic or endothermic? Is the product ionic or molecular?

Short Answer

Expert verified
Mg reacts with O鈧� to form MgO, which is ionic and exothermic.

Step by step solution

01

Select an Alkaline Earth Metal

We will select magnesium (Mg) as our alkaline earth metal for this exercise. Magnesium is a common example of this group and often used to demonstrate reactions with oxygen.
02

Write the Chemical Equation

The chemical equation for the reaction between magnesium and oxygen is written as follows:\[ 2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO} \]This equation shows that two moles of magnesium react with one mole of oxygen gas to produce two moles of magnesium oxide.
03

Balance the Chemical Equation

The chemical equation is already balanced as written in Step 2. There are two magnesium atoms and two oxygen atoms on both the reactant and product sides of the equation, indicating that the equation follows the law of conservation of mass.
04

Determine the Nature of the Reaction (Exothermic or Endothermic)

The reaction between magnesium and oxygen is highly exothermic. It releases a significant amount of energy in the form of heat and light, which is why burning magnesium produces a bright white flame.
05

Identify the Type of Product (Ionic or Molecular)

The product, magnesium oxide (MgO), is ionic. This is because it is formed by the transfer of electrons: magnesium loses two electrons to form Mg虏鈦� ions, and oxygen gains those electrons to form O虏鈦� ions, resulting in the ionic compound MgO.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Magnesium
Magnesium is a key alkaline earth metal found in group 2 of the periodic table. It鈥檚 often used in chemistry due to its reactivity, especially with oxygen.
When studying magnesium, remember these points:
  • Symbol: Mg
  • Atomic number: 12
  • Silvery-white appearance
  • Commonly found in minerals like dolomite and magnesite
Magnesium is not only essential in chemical reactions but also in biological processes. It plays a vital role in helping our body function, particularly in muscle and nerve operations.
Chemical Reactions
Chemical reactions involve the transformation of substances through the breaking and forming of bonds. In the case of magnesium reacting with oxygen, the following process occurs:- Magnesium (Mg) reacts with oxygen (O_2)- The reaction produces magnesium oxide (MgO)The balanced equation is:\[2\text{Mg} + \text{O}_2 \rightarrow 2\text{MgO}\]Balancing chemical equations ensures the law of conservation of mass is obeyed, meaning the same number of each type of atom is present before and after the reaction.
Exothermic Reactions
An exothermic reaction is one that releases energy, usually as heat or light. The reaction between magnesium and oxygen is a prime example.
Here's what to note about exothermic reactions:
  • Release energy to the surroundings
  • Products have less energy than reactants
  • Temperature increase is often noticeable
  • Commonly seen with combustion reactions, like burning magnesium
The bright white flame seen when magnesium burns is due to this energy release, capturing students' attention with its dramatic effect.
Ionic Compounds
Ionic compounds form through the transfer of electrons, resulting in positively and negatively charged ions. Magnesium oxide (MgO) is one such ionic compound.
Here's how it works:
  • Magnesium loses two electrons to become Mg虏鈦�
  • Oxygen gains two electrons to become O虏鈦�
  • These oppositely charged ions attract, forming a strong ionic bond
Ionic compounds like MgO are generally solid at room temperature and have high melting points due to the strong electrostatic forces between ions.

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Most popular questions from this chapter

Calcium reacts with hydrogen gas at \(300-400^{\circ} \mathrm{C}\) to form a hydride. This compound reacts readily with water, so it is an excellent drying agent for organic solvents. (a) Write a balanced equation showing the formation of calcium hydride from Ca and \(\mathrm{H}_{2}\). (b) Write a balanced equation for the reaction of calcium hydride with water (Figure 21.7 ).

(a) Heating barium oxide in pure oxygen gives barium peroxide. Write a balanced equation for this reaction. (b) Barium peroxide is an excellent oxidizing agent. Write a balanced equation for the reaction of iron with barium peroxide to give iron(III) oxide and barium oxide.

Which of the following statements is not correct? (a) The ease of oxidation of the halide ions is \(\mathrm{F}^{-}\) $$ <\mathrm{Cl}^{-}<\mathrm{Br}^{-}<\mathrm{I}^{-} $$ (b) Fluorine is the most abundant halogen in the Earth's crust. (c) \(\mathrm{F}_{2}\) is prepared industrially by electrolysis of aqueous NaF. (d) HF is used to etch glass.

For each of the third-period elements (Na through Ar), identify the following: (a) whether the element is a metal, nonmetal, or metalloid (b) the color and appearance of the element (c) the state of the element \((s, \ell, \text { or } g\) ) under standard conditions

Calcium oxide, \(\mathrm{CaO}\), is used to remove \(\mathrm{SO}_{2}\) from ower plant exhaust. These two compounds react o give solid \(\mathrm{CaSO}_{3} .\) What mass of \(\mathrm{SO}_{2}\) can be emoved using \(1.2 \times 10^{3} \mathrm{kg}\) of \(\mathrm{CaO} ?\)
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