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Chapter 9: Problem 17

Use Lewis dot symbols to show the transfer of electrons between the following atoms to form cations and anions: (a) \(\mathrm{Na}\) and \(\mathrm{F},\) (b) \(\mathrm{K}\) and \(\mathrm{S},\) (c) \(\mathrm{Ba}\) and \(\mathrm{O}\), (d) \(\mathrm{Al}\) and \(\mathrm{N}\).

Short Answer

Expert verified
Once the electrons have been transferred, our ion pairs become: (a) \(\mathrm{Na}^+\) and \(\mathrm{F}^-\), (b) \(\mathrm{K}^+\) and \(\mathrm{S}^{2-}\), (c) \(\mathrm{Ba}^{2+}\) and \(\mathrm{O}^{2-}\), (d) \(\mathrm{Al}^{3+}\) and \(\mathrm{N}^{3-}\).

Step by step solution

01

Identify Valence Electrons

Determine the number of valence electrons for each atom based on their position in the periodic table. For instance, 'Na' (Sodium) and 'K' (Potassium) each have one valence electron as they are in group 1; 'F' (Fluorine) and 'O' (Oxygen) have seven and six valence electrons respectively as they are in group 16; 'S' (Sulphur) has six valence electrons; 'Ba' (Barium) has two valence electrons as it is in group 2; and 'Al' (Aluminium) has three valence electrons as it is in group 13 while 'N' (Nitrogen) has five valence electrons as it's in group 15.
02

Draw Lewis Dot Diagram

The Lewis Dot Diagram is a graphical representation of the valence electrons in an atom. An element's symbol is written, and then dots are placed around it to represent its valence electrons. Start drawing the dots from the top and proceed clockwise.
03

Show Electron Transfer

Each atom would want to achieve a stable electron configuration, which is often having eight electrons in its outer shell (octet rule), or two for elements in the first period of the periodic table. In our pairs, the metal will transfer its valence electrons to the non-metal. For example, 'Na' will transfer its one valence electron to 'F', 'K' will transfer its electron to 'S', 'Ba' will transfer its two valence electrons to 'O', and 'Al' will transfer its three electrons to 'N'. After transfer, metals become cations and non-metals become anions.

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Most popular questions from this chapter

The species \(\mathrm{H}_{3}^{+}\) is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. (a) Draw three resonance structures to represent the ion. (b) Given the following information and $$ \begin{aligned} 2 \mathrm{H}+\mathrm{H}^{+} \longrightarrow \mathrm{H}_{3}^{+} & \Delta H^{\circ}=-849 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2} \longrightarrow 2 \mathrm{H} & \Delta H^{\circ}=436.4 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ calculate \(\Delta H^{\circ}\) for the reaction $$ \mathrm{H}^{+}+\mathrm{H}_{2} \longrightarrow \mathrm{H}_{3}^{+} $$

The only known argon-containing compound is HArF, which was prepared in \(2000 .\) Draw a Lewis structure of the compound.

True or false: (a) Formal charges represent actual separation of charges; (b) \(\Delta H_{\mathrm{rxn}}^{\circ}\) can be estimated from bond enthalpies of reactants and products; (c) all second-period elements obey the octet rule in their compounds; (d) the resonance structures of a molecule can be separated from one another.

Give three examples of compounds that do not satisfy the octet rule. Write a Lewis structure for each.

Name five metals and five nonmetals that are very likely to form ionic compounds. Write formulas for compounds that might result from the combination of these metals and nonmetals. Name these compounds.
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