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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 that involves a complete transfer of valence electrons between atoms and produces oppositely charged ions. An example is NaCl (Sodium Chloride), where Sodium gives up an electron to Chlorine, forming an ionic bond.

Step by step solution

01

Define Ionic Bond

An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. Ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions.
02

Understand the Formation of Ions

During Ionic Bonding, atoms that lose electrons during this process become positively charged ions known as cations, while atoms that gain electrons become negatively charged ions known as anions.
03

Explain Examples of Ionic Bonds

A common example of an ionic bond is NaCl (Sodium Chloride), where Sodium (Na) gives up an electron to Chlorine (Cl), and they bond to form NaCl.

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Most popular questions from this chapter

Which of the following are ionic compounds? Which are covalent compounds? \(\mathrm{RbCl}, \mathrm{PF}_{5}, \mathrm{BrF}_{3},\) \(\mathrm{KO}_{2}, \mathrm{CI}_{4}\)

When irradiated with light of wavelength \(471.7 \mathrm{nm}\) the chlorine molecule dissociates into chlorine atoms. One \(\mathrm{Cl}\) atom is formed in its ground electronic state while the other is in an excited state that is \(10.5 \mathrm{~kJ} / \mathrm{mol}\) above the ground state. What is the bond enthalpy of the \(\mathrm{Cl}_{2}\), molecule?

Draw Lewis structures for the following organic molecules: (a) tetrafluoroethylene \(\left(\mathrm{C}_{2} \mathrm{~F}_{4}\right),\) (b) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right),(\mathrm{c})\) butadiene \(\left(\mathrm{CH}_{2} \mathrm{CHCHCH}_{2}\right),\) (d) propyne \(\left(\mathrm{CH}_{3} \mathrm{CCH}\right),(\mathrm{e})\) benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right) .\) (To draw \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH},\) replace a \(\mathrm{H}\) atom in benzene with a COOH group.)

Draw three resonance structures for the chlorate ion, \(\mathrm{ClO}_{3}^{-}\). Show formal charges.

Write Lewis structures for \(\mathrm{SeF}_{4}\) and \(\mathrm{SeF}_{6}\). Is the octet rule satisfied for Se?
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