Chlorine And Oxygen Ionic Compound

half dozen.iv Ionic bonding (ESABW)

The nature of the ionic bond (ESABX)

When electrons are transferred from one atom to another information technology is called ionic bonding.

Electronegativity is a property of an atom, describing how strongly information technology attracts or holds onto electrons. Ionic bonding takes identify when the departure in electronegativity between the two atoms is more than than \(\text{1,7}\). This commonly happens when a metal cantlet bonds with a non-metal cantlet. When the difference in electronegativity is large, ane cantlet will attract the shared electron pair much more than strongly than the other, causing electrons to be transferred to the atom with higher electronegativity. When ionic bonds grade, a metal donates i or more electrons, due to having a low electronegativity, to form a positive ion or cation. The non-metal atom has a high electronegativity, and therefore readily gains electrons to class a negative ion or anion. The two ions are then attracted to each other by electrostatic forces.

Ionic bond: An ionic bond is a type of chemic bond where ane or more electrons are transferred from one atom to another.

Example 1:

In the case of \(\text{NaCl}\), the difference in electronegativity between \(\text{Na}\) (\(\text{0,93}\)) and \(\text{Cl}\) (\(\text{3,16}\)) is \(\text{2,1}\). Sodium has only ane valence electron, while chlorine has seven. Because the electronegativity of chlorine is college than the electronegativity of sodium, chlorine will attract the valence electron of the sodium atom very strongly. This electron from sodium is transferred to chlorine. Sodium loses an electron and forms an \(\text{Na}^{+}\) ion.

Chlorine gains an electron and forms a \(\text{Cl}^{-}\) ion.

Chlorine is a diatomic molecule and then for it to take part in ionic bonding, it must beginning break up into two atoms of chlorine. Sodium is office of a metallic lattice and the individual atoms must beginning suspension abroad from the lattice.

The electron is therefore transferred from sodium to chlorine:

Figure vi.1: Ionic bonding in sodium chloride

The balanced equation for the reaction is:

\[2\text{Na} + \text{Cl}_{two} \rightarrow two\text{NaCl}\]

Example 2:

Another instance of ionic bonding takes identify between magnesium \((\text{Mg})\) and oxygen \((\text{O}_{2})\) to form magnesium oxide \((\text{MgO})\). Magnesium has ii valence electrons and an electronegativity of \(\text{one,31}\), while oxygen has 6 valence electrons and an electronegativity of \(\text{3,44}\). Since oxygen has a higher electronegativity, information technology attracts the two valence electrons from the magnesium atom and these electrons are transferred from the magnesium atom to the oxygen atom. Magnesium loses ii electrons to course \(\text{Mg}^{2+}\), and oxygen gains two electrons to class \(\text{O}^{ii-}\). The bonny forcefulness betwixt the oppositely charged ions is what holds the chemical compound together.

The balanced equation for the reaction is:

\[two\text{Mg} + \text{O}_{2} \rightarrow 2\text{MgO}\]

Because oxygen is a diatomic molecule, two magnesium atoms volition be needed to combine with i oxygen molecule (which has two oxygen atoms) to produce two units of magnesium oxide \((\text{MgO})\).

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The crystal lattice structure of ionic compounds (ESABY)

Ionic substances are really a combination of lots of ions bonded together into a behemothic molecule. The arrangement of ions in a regular, geometric structure is called a crystal lattice. So in fact \(\text{NaCl}\) does not contain one \(\text{Na}\) and ane \(\text{Cl}\) ion, but rather a lot of these two ions arranged in a crystal lattice where the ratio of \(\text{Na}\) to \(\text{Cl}\) ions is one:1. The structure of the crystal lattice is shown below.

Figure 6.2: The crystal lattice organization in \(\text{NaCl}\)

Effigy 6.3: A space filling model of the sodium chloride lattice

Properties of ionic compounds (ESABZ)

Ionic compounds have a number of properties:

Ions are arranged in a lattice construction
Ionic solids are crystalline at room temperature
The ionic bond is a strong electrostatic attraction. This ways that ionic compounds are often hard and have loftier melting and humid points
Ionic compounds are brittle and bonds are broken forth planes when the chemical compound is put under force per unit area (stressed)
Solid crystals practice not conduct electricity, only ionic solutions do

Ionic compounds

Textbook Practice 6.3

Explain the divergence between a covalent and an ionic bond.

Solution not yet available.

Magnesium and chlorine react to course magnesium chloride.

What is the divergence in electronegativity between these ii elements?
Give the chemic formula for:
1. a magnesium ion
2. a chloride ion
3. the ionic compound that is produced during this reaction
Write a balanced chemical equation for the reaction that takes identify.