Ionic Bonding

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Show the ion formation of Lithium

Some Typical Ions with Positive
Charges (Cations)

Group 1

Group 2

Group 3

H+

Mg2+

Al3+

Li+

Ca2+

Na+

Sr2+

K+

Ba2+

Open Ended

This ion forms a negative charge.

Anions are negative ions that are formed when a nonmetal atom gains one or more electrons.

Anion

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-

Fluoride Ion

unpaired electron

octet

• •

• •1 -

: F •
+ e−

: F :

• •

• •

2-7

2-8 (= Ne)

9 p+

9 p+

9 e-

10 e-

0

1 -

ionic charge

Chlorine Ion

octet

• •1 -

: Cl :

• •

2-8 (= Ne)

9 p+

10 e-

1 -

Draw

Draw the ion formation of oxygen.

Review

• Ions
• Positive Ions
• Negative Ions
• Formation of ions in Metals
• Formation of ions in Non Metals

Open Ended

Where do electrons go? (lost)

Open Ended

Where do electrons come from? (Gained)

IONIC BOND

formed between
two ions by the transfer of electrons

Ionic Compounds

• Since ions have

positive or negative
charges, they can
attract to each other
and form chemical
bonds called ionic
bonds.

Ionic Bond

• Between atoms of metals and nonmetals
• Bond formed by transfer of electrons
• Produce charged ions all states. Conductors and have high

melting point.

• Examples; NaCl, CaCl2, K2O

Ionic Bonds: One Big Greedy Thief Dog!

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.

Example:
Formation of Lithium Fluoride

.

..

Li. + : F :

→

Li+: F -:

..

..

Formation of Ionic Bond

METALLIC BOND

found in

metals; holds metal

atoms together

very strongly

Metallic Bond

• Formed between atoms of metallic elements
• Electron cloud around atoms
• Good conductors at all states, lustrous, very high melting points
• Examples; Na, Fe, Al, Au, Co

Metallic Bonds: Mellow dogs with plenty

of bones to go around.

Properties

Explanation

Metals are dense

The particles present in metals are tightly packed in a lattice (3D structure);
Greater atomic attraction in metals leads to higher density, since more
particles occupy a small volume.

Metals have high melting
and boiling points

Strong forces of attraction exist between particles. A large amount of
thermal energy is required to overcome this attraction between the positive
ions and delocalized electrons. These forces operate throughout the lattice.
Tungsten has one of the highest melting point of 3380 ⁰C, and iron 1535 ⁰C.

Metals are good
conductors of heat

Delocalized electrons transmit the energy of vibrations of a positive ion to its
neighbors.

Metals are good
conductors of electricity.

Electrons are delocalized within the lattice. Electrons flow from one end to
the other end.

Metals are malleable and
ductile

The distortion (caused by reshaping the metal) does not disrupt metallic
bonding

Metals are lustrous

The presence of free electrons causes most metals to reflect light.
(Nonmetals are transparent)

Metallic Bond, A Sea of Electrons

Metals Form Alloys

Metals do not combine with metals. They form
Alloys which is a solution of a metal in a metal.
Examples are steel, brass, bronze and pewter.

Draw

Draw the bond formation between Beryllium and Oxygen

Open Ended

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