Ionic bonds and ionic compounds

Introduction

Ion is an atom or group of atoms carrying a positive or negative electric charge resulting in loss or gain of one or more electrons. Positively charged ions are cations and negatively charged ones are anions. Positively charged ions and negatively charged ions attract each other through the electrostatic forces of attraction that exist between them. The forces of attraction that binds these oppositely charged ions are called ionic bonds. Ionic compounds/substances are compounds that are made up of electrically neutral groups of ions that are joined by electrostatic forces. Any ionic compound must have an equal number of cations and anions. A good example of an ionic compound is sodium chloride in which sodium has a single valence electron that can be easily lost in order to attain stability. On the other hand, chlorine requires one electron for it to become stable. Therefore, when sodium and chlorine reacts to form an ionic compound, sodium will donate its valence electron to chlorine atom. In other words, sodium and chlorine atoms combine in a one-to-one ratio hence both ions have stable electron configurations.

Table of Contents

1. Introduction

2. Properties of ionic compounds

3. Co-ordination number

4. X-ray Diffraction Crystallography

 

 

Electron transfer in NaCl

 

In the illustration above, the ionic compound NaCl formed has the lowest whole number ratio of cation Naand anion Cl as seen through the chemical formula. Formation of aluminium bromide can be illustrated as shown below: Aluminum has three valence electrons while bromine has seven valence electrons. Each bromine atom readily gains one additional electron to become stable. Therefore, when aluminium and bromine react, 3 bromine atoms combine with each aluminium atom to form aluminium bromide- AlBr2.

Formation of aluminum bromide

 

Properties of ionic compounds

Ionic compounds are crystalline in nature at room temperature.  The component ions in such structures are arranged in 3D patterns that are repetitive. For instance, in sodium chloride each Na+ ion is surrounded by 6 Cl- ions and each Cl- ion is surrounded by 6 Na+ ions. In this structure, each ion is strongly held to each other and the repulsive forces of attraction are minimal. The structure is very stable due to the large attractive forces that exist between the ions.

Ionic bond between Na and Cl

 

Co-ordination number

Coordination number refers to the number of oppositely charged ions that surrounds the anion in a crystal. From the above diagram, Na+ has a coordination number of 6 because it is surrounded by 6 chloride ions.  Furthermore, each Clion is surrounded by 6 Naions and also has a coordination number of six.

 

X-ray Diffraction Crystallography

X-ray diffraction crystallography is the technique used to determine the internal structure of crystals. In this process, the x-rays are passed through a crystal and results recorded on a film. The pattern on the exposed film shows how ions are deflected by the x-rays. Generally, the pattern is used to calculate the position of the ions in the crystal and can also be used to define the structure of the crystal.

X-ray Diffraction Crystallography

Ionic compounds can conduct an electric current when melted. Melting of sodium chloride makes the crystal structure to breakdown. If a voltage is applied across the molten mass, positively charged ions will migrate towards the cathode while the negatively charged ions will move towards the anode. For a similar reason, ionic compounds also conduct electricity if they are dissolved in water.  If you dissolve sodium chloride in water, the ions are freely moved in the aqueous solution.

 



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