Kurdistan regional governmentMinistry of higher education & scientific researchUniversity scientificPart chemistry

Ionic Bond

Kosary Yasin AhmadMohammad Nasih

Prepared by

Dr. Kafia

Supervised by

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Thank God that His grace is righteous, praise be to God who created the earth and the heavens, praise be to God, who knew the pitfalls, he may praise fill the coffers of blessings, and praise what Successive heart pulses, and the number of atoms of the air in the earth and the heavens, and the number of movements, Hostels.

In the name of God the Merciful

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Introduction Some Information & Properties about Ionic Bonding Write Chemical Formula about this substance Atoms gain or lose Formation of Ions from Metals Ions from Nonmetal Ions Some Typical Ions with Positive Charges

(Cations)

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Overview:

a bond is a force of attraction between two atoms

Ionic bond between atoms of metals and nonmetals Bonds that are formed by transfer of electrons

from one element to the other.

Produce charged ions all states. Conductors and have high melting point.

Examples; NaCl, CaCl2, K2O

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Introduction:

Some Information & Properties about Ionic Bonding generally occurs in compounds of metals and

non-metals .

It is the result of the attraction of oppositely charged ions.

The structures formed are very orderly and are given the name crystal lattice.

Ionic solids are called crystals.

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Ionic Bonds

No sharing of electrons occurs between the ions in the crystal lattice.

As a result, ionic solids are brittle.

Ionic solids conduct electricity only in the molten state, and not very well.

Ionic solids are characterized by very high

melting and boiling points.

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Ionic bonds are much stronger if the ions have a large charge.

Ionic solids do not conduct electric current because the ions are held together in a rigid structure.

Ionic substances that are dissolved in water are good conductors because the charged ions are free to move in the solution.

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Ionic bonds have an electronegativity difference between 1.7 and 3.3

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Group IonicBonds

1 1( 1)+2 2( 2)+

13 3( 3)+14 -15 3( 3)-16 2( 2)-17 1( 1)-18 0

1electron promotion 2valence level expansion

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Strength of Attraction(London dispersion) 1 to 50

(hydrogen bonding) 15

Ionic 50

Metallic 20 to 80

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Melting and Boiling Point(London dispersion) very low (nitrogen boils

at - 196 C) VARIABLE

Molecular (hydrogen bonding)

medium (H2O boils at +100 C)

Ionic high (NaCl boils at +1413 C)

Metallic variable (Hg @ +357 C, W @ +5660 C)

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A representation of the kinds and number of atoms in a substance.

A chemical formula that shows the lowest whole number ratio of the atoms (ions) in an ionic compound.

Example: KCl, Mg Cl2

Write Chemical Formulaabout this substance

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Writing formulas

What is the formula of potassium sulfate?

K+ SO42- 12

K2SO4

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Writing formulas with the stock system

What is the formula of copper (II) nitrate?

Cu2+ NO3-

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Cu(NO3)2

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Which ball represents

the Na?

The formula unit is used because ionic compounds have a lattice arrangement of ions. Ex: NaCl

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Atoms gain or lose electrons to arrive at a full set of valence electrons.

When atoms gain or lose electrons they become ions.

Ions are attracted to ions of opposite charge and repelled by ions of the same charge.

This type of bonding is called ionic bonding

Atoms become ionic by losing or gaining electrons from the atom it is bonding with

Atoms gain or lose

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•The electrical force of attraction between oppositely charged ions.

For Example:

The Ionic Bond

Na+ F−

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Formation of Ions from Metals

Ionic compounds result when metals react with nonmetals

Metals lose electrons to match the number of valence electrons of their nearest noble gas

Positive ions form when the number of electrons are less than the number of protons

Group 1 metals ion 1+

Group 2 metals ion 2+

Group 13 metals ion 3+

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Formation of Sodium Ion

Sodium atom Sodium ion

Na – e Na +

11e - 1e = 10e

11 p+ 11 p+

11 e- 10 e-

0 1+

2

2 6

1

1

2 2

3

s

s p

s

2

2 6

1

2 2

s

s p

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Na + , 10e

Na , 11 e

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Chlorine Atom Chlorine Ion

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For example:

Na=11e→10e CL=17e → 18ein Group:1 in Group:17

2

2 6

1

1

2 2

3

s

s p

s

2

2 6

2 5

1

2 2

3 3

s

s p

s p

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Ionic Bonds: One Big Greedy Thief Dog!

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Ions from Nonmetal Ions

In ionic compounds, nonmetals in

15, 16, and 17 gain electrons from

metals

Nonmetal add electrons to achieve

the octet arrangement

Nonmetal ionic charge:

3-, 2-, or 1- 26

Fluoride Ion

unpaired electron octet 1 - : F + e : F :

9 p+ 9 p+

9 e- 10 e- 0 1 -

ionic charge

2 2s

2

2 5

1

2 2

s

s p

2

2 6

1

2 2

s

s p

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Some Typical Ions with Positive Charges (Cations)

Group 1Group 2Group 13

H+Mg2+Al3+

Li+Ca2+

Na+Sr2+

K+Ba2+

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1). Ionic bond – electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes (Na+) and the Cl becomes (Cl-), charged particles or ions.

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Reffrence:

http://www.worldofteaching.com Ionic Bonds-Chemistry By:Mrs. Coyle http://www.youtube.com/watch?v=Kj3o0Xvh

VqQ&NR=1 http://www.youtube.com/watch?v=M89o9X8

hVq37N0=1 Inorganic Chemistry by Shriver &

Atkins C-110, Department of Chemistry

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Blessings and peace upon our Prophet Muhammad, his family and him.