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Chapter 8: Problem 13

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

Short Answer

Expert verified
Using Lewis symbols, the reaction between magnesium and oxygen atoms to form MgO is illustrated as: Mg: Mg 鈥⑩�� O: O 鈥⑩�� |鈥⑩� Mg 鈥⑩�� + O 鈥⑩�� |鈥⑩� 鈫� Mg O 鈫掆啋 Mg虏鈦� O虏鈦� Mg虏鈦� + O虏鈦� 鈫� MgO In this reaction, magnesium loses its 2 valence electrons to oxygen, forming Mg虏鈦� and O虏鈦� ions that attract each other and create the ionic compound magnesium oxide (MgO).

Step by step solution

01

Understand Lewis symbols

Lewis symbols are a way to represent atoms and their valence electrons using symbols. The symbol of the element is written, and around it, dots are added to represent the valence electrons. Valence electrons are the electrons in the outermost energy level of an atom and are involved in chemical bonding. For example, Magnesium (Mg) has 2 valence electrons, so its Lewis symbol would be Mg with 2 dots around it, like this: Mg 鈥⑩��
02

Write the Lewis symbols for magnesium and oxygen atoms

Now that we understand what Lewis symbols are, let's write them for magnesium and oxygen atoms. As mentioned earlier, magnesium has 2 valence electrons, while oxygen has 6 valence electrons. Their Lewis symbols are written as: Mg: Mg 鈥⑩�� O: O 鈥⑩�� |鈥⑩�
03

Show the electron transfer

In the reaction to form MgO, magnesium loses its 2 valence electrons to oxygen. This transfer of electrons leads to the formation of a positively charged magnesium ion (Mg2+) and a negatively charged oxygen ion (O2鈭�). The electron transfer can be illustrated as follows: Mg 鈥⑩�� + O 鈥⑩�� |鈥⑩� 鈫� Mg O 鈫掆啋 Mg虏鈦� O虏鈦�
04

Demonstrate the formation of MgO

Now that we have shown the electron transfer and formation of Mg虏鈦� and O虏鈦� ions, we can demonstrate the formation of MgO. The positive Mg虏鈦� ion and the negative O虏鈦� ion will attract each other due to electrostatic forces, forming an ionic bond. This leads to the formation of the ionic compound magnesium oxide (MgO): Mg虏鈦� + O虏鈦� 鈫� MgO In conclusion, we have used Lewis symbols to illustrate the electron transfer and formation of the MgO ionic compound. Magnesium loses its 2 valence electrons to oxygen, resulting in a positively charged Mg虏鈦� ion and a negatively charged O虏鈦� ion. These ions attract each other, forming an ionic bond and the ionic compound magnesium oxide (MgO).

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Most popular questions from this chapter

Using bond enthalpies (Table 8.4), estimate \(\Delta H\) for each of the following reactions: (a) \(2 \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{CH}_{3} \mathrm{OH}(g)\) (b) \(\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow 2 \mathrm{HBr}(g)\) (c) \(2 \mathrm{H}_{2} \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{O}_{2}(g)\)

(a) Write a Lewis structure for the phosphorus trifluoride molecule, \(\mathrm{PF}_{3}\). Is the octet rule satisfied for all the atoms in your structure? (b) Determine the oxidation numbers of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms. (c) Determine the formal charges of the \(\mathrm{P}\) and \(\mathrm{F}\) atoms. (d) Is the oxidation number for the \(\mathrm{P}\) atom the same as its formal charge? Explain why or why not.

(a) Using average bond enthalpies, predict which of the following reactions will be most exothermic: (i) \(\mathrm{C}(\mathrm{g})+2 \mathrm{~F}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CF}_{4}(\mathrm{~g})\) (ii) \(\mathrm{CO}(\mathrm{g})+3 \mathrm{~F}_{2} \longrightarrow \mathrm{CF}_{4}(g)+\mathrm{OF}_{2}(g)\) (iii) \(\mathrm{CO}_{2}(g)+4 \mathrm{~F}_{2} \longrightarrow \mathrm{CF}_{4}(g)+2 \mathrm{OF}_{2}(g)\) (b) Explain the trend, if any, that exists between reaction exothermicity and the extent to which the carbon atom is bonded to oxygen.

(a) Use bond enthalpies to estimatethe enthalpy change for the reaction of hydrogen with ethene: $$\mathrm{H}_{2}(\mathrm{~g})+\mathrm{C}_{2} \mathrm{H}_{4}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)$$ (b) Calculate the standard enthalpy change for this reaction, using heats of formation. Why does this value differ from that calculated in (a)?

For the following collection of nonmetallic elements, \(\mathrm{O}\), \(\mathrm{P}, \mathrm{Te}, \mathrm{I}, \mathrm{B},(\mathrm{a})\) which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which two would be likely to form a compound of formula \(\mathrm{XY}_{2}\) ? (d) Which combinations of elements would likely yield a compound of empirical formula \(\mathrm{X}_{2} \mathrm{Y}_{3} ?\) In each case explain your answer.
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