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Chapter 9: Problem 6

Explain what an ionic bond is.

Short Answer

Expert verified
An ionic bond is a type of chemical bond formed through the transfer of electrons from one atom (usually a metal) to another (usually a nonmetal). This results in one atom becoming a positively charged ion and the other a negatively charged ion. The attraction between these oppositely charged ions constitutes the ionic bond. An example is the formation of table salt (NaCl) from sodium (Na) and chlorine (Cl).

Step by step solution

01

Define Ionic Bond

An ionic bond is a type of chemical bond that occurs when an atom transfers an electron to another atom. This results in one atom becoming positively charged (cation) and the other becoming negatively charged (anion). The attraction between these oppositely charged ions forms the ionic bond.
02

Explain How Ionic Bonds Form

Ionic bonds form through the transfer of electrons between atoms. This usually occurs between a metal and a nonmetal. The metal, which has a tendency to lose electrons and form a positively charged ion, will transfer its electron(s) to the nonmetal. This nonmetal tends to gain electrons and form negatively charged ions. The opposite charges of these ions attract each other, forming an ionic bond.
03

Provide an Example

An example of an ionic bond is the bond between sodium (Na) and chlorine (Cl) to form table salt (NaCl). In this reaction, the sodium atom loses one electron to become Na+ (a cation), and the chlorine atom gains that electron to become Cl- (an anion). The resulting attraction between Na+ and Cl- forms the ionic bond within NaCl

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Most popular questions from this chapter

Write Lewis structures for these ions: (a) \(\mathrm{O}_{2}^{2-}\), (b) \(\mathrm{C}_{2}^{2-},\) (c) \(\mathrm{NO}^{+}\), (d) \(\mathrm{NH}_{4}^{+}\). Show formal charges.

Explain how the lattice energy of an ionic compound such as \(\mathrm{KCl}\) can be determined using the Born-Haber cycle. On what law is this procedure based?

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.

Draw three reasonable resonance structures for the \(\mathrm{OCN}^{-}\) ion. Show formal charges.
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