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Chapter 8: Problem 15

Using Lewis symbols, diagram the reaction between magnesium and oxygen atoms to give the ionic substance \(\mathrm{MgO}\).

Short Answer

Expert verified
Magnesium (Mg) has 2 valence electrons and oxygen (O) has 6 valence electrons. Magnesium transfers its 2 valence electrons to oxygen to achieve a full electron shell configuration: Mg^(2+) and O^(2-). This results in the formation of the ionic compound MgO: \(\mathrm{MgO}\).

Step by step solution

01

Identify the number of valence electrons for each atom

Magnesium (Mg) is in group 2 of the periodic table, which means that it has 2 valence electrons. Oxygen (O) is in group 16, which means that it has 6 valence electrons.
02

Represent the Lewis symbols for the atoms

A Lewis symbol represents an atom with the chemical symbol surrounded by dots representing its valence electrons. For magnesium, this would be: Mg: 鈥⑩�� For oxygen, this would be: O: 鈥⑩�� 鈥⑩�� 鈥⑩��
03

Show the interaction between the atoms

Magnesium can achieve a full electron shell by losing its 2 valence electrons, while oxygen can achieve a stable electron configuration by gaining 2 electrons. In this reaction, magnesium will transfer its 2 valence electrons to oxygen to form the ionic compound.
04

Indicate the transfer of electrons

By transferring the 2 electrons from magnesium to oxygen, we obtain the following new Lewis symbols which represent a complete electron shell configuration: Mg: O: 鈥⑩�� 鈥⑩�� 鈥⑩�� 鈥⑩�� Here, the magnesium atom donates its two valence electrons to the oxygen atom. This changes both of them to ion forms. Magnesium loses electrons and becomes a cation and oxygen gains electrons and becomes an anion.
05

Show the formation of the ionic compound

After the interaction that occurred in the previous step, magnesium becomes a cation with a charge of \(+2\) and oxygen becomes an anion with a charge of \(-2\). The attractive force between these oppositely charged ions results in the formation of the ionic compound MgO. The final result of the reaction is: Mg^(2+) O^(2-): \(\mathrm{MgO}\) This shows the Lewis symbols representing the formation of the ionic substance MgO from magnesium and oxygen atoms.

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Key Concepts

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

Valence Electrons
Valence electrons are the electrons present in the outermost shell of an atom. They play a pivotal role in chemical bonding, as they are the electrons that are involved in the formation of chemical bonds. Understanding valence electrons is crucial when exploring ionic bonding and compound formation.

For example, magnesium (Mg), which falls under group 2 of the periodic table, has 2 valence electrons. These valence electrons are represented in Lewis symbols by dots around the element's symbol. Similarly, oxygen (O), from group 16, has 6 valence electrons, which are also depicted as dots in its Lewis symbol.

Why Valence Electrons Matter

These outer electrons dictate how an element will interact with other elements. The ultimate goal for an atom, based on the octet rule, is to have a full set of valence electrons, usually eight, to attain a stable electronic configuration similar to that of the noble gases.
Electron Transfer Process
During the formation of an ionic compound, atoms undergo an electron transfer process. This process involves the movement of electrons from one atom to another, enabling each to reach a state of electric stability.

In the interaction between magnesium and oxygen, magnesium donates its 2 valence electrons to oxygen. Such a transfer alters the electron configurations of both atoms: magnesium loses electrons and transforms into a positively charged ion, or cation, while oxygen gains electrons to become negatively charged, or an anion.

Understanding Electron Traffic

Depicted in Lewis symbols, we can visualize this traffic of electrons. Post transfer, magnesium鈥檚 Lewis symbol has no dots, symbolizing a full outer shell, whereas oxygen鈥檚 Lewis symbol shows eight dots, illustrating its new full shell attained through the gained electrons.
Ionic Compound Formation
The culmination of the electron transfer process is the formation of an ionic compound. When atoms like magnesium and oxygen undergo electron transfer, the resulting ions oppositely charge and attract one another, forming a strong electrostatic bond.

In our example, magnesium becomes Mg虏鈦� and oxygen becomes O虏鈦�. The ionic bond forms because the positively charged magnesium cation is attracted to the negatively charged oxygen anion.

Final Compounds as Ionic Puzzles

This attraction results in the ionic compound MgO, where each magnesium ion pairs with an oxygen ion. The balance of charges (2+ and 2-) ensures overall neutrality of the compound. Ionic compounds are usually crystalline solids at room temperature, and they tend to have high melting and boiling points due to the strength of the ionic bonds.

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Most popular questions from this chapter

The chlorine oxides, in which a chlorine atom is bonded to one or more oxygen atoms, are important molecules in the chemistry of the atmosphere. Will any of the chlorine oxides obey the octet rule? Why or why not?

(a) What is meant by the term electronegativity? (b) On the Pauling scale what is the range of electronegativity values for the elements? (c) Which element has the greatest electronegativity? (d) Which element has the smallest electronegativity?

The electron affinity of oxygen is \(-141 \mathrm{~kJ} / \mathrm{mol}\), corresponding to the reaction $$ \mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g) $$ The lattice energy of \(\mathrm{K}_{2} \mathrm{O}(s)\) is \(2238 \mathrm{~kJ} / \mathrm{mol}\). Use these data along with data in Appendix \(\mathrm{C}\) and Figure 7.9 to calculate the "second electron affinity" of oxygen, corresponding to the reaction $$ \mathrm{O}^{-}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g) $$

By referring only to the periodic table, select (a) the most electronegative element in group \(6 \mathrm{~A} ;\) (b) the least electronegative element in the group \(\mathrm{Al}, \mathrm{Si}, \mathrm{P} ;(\mathbf{c})\) the most electronegative element in the group \(\mathrm{Ga}, \mathrm{P}, \mathrm{Cl}, \mathrm{Na} ;\) (d) the element in the group \(\mathrm{K}, \mathrm{C}, \mathrm{Zn}, \mathrm{F}\) that is most likely to form an ionic compound with \(\mathrm{Ba}\).

Energy is required to remove two electrons from Ca to form \(\mathrm{Ca}^{2+}\) and is required to add two electrons to \(\mathrm{O}\) to form \(\mathrm{O}^{2-}\). Why, then, is \(\mathrm{CaO}\) stable relative to the free elements?
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