PS 6.1 Notes: Ionic Bonding

6.1 Ionic Bonding

When is an atom unlikely to react?

Stable Electron Configurations

When the highest occupied energy level of
an atom is filled with electrons, the atom is
stable and not likely to react.

6.1 Ionic Bonding

The chemical properties of an element depend
on the number of valence electrons. An
electron dot diagram is a model of an atom in
which each dot represents a valence electron.
The symbol in the center represents the
nucleus and all the other electrons in the atom.

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Stable Electron Configurations

6.1 Ionic Bonding

Noble gases are the most stable elements.

• The highest occupied energy level of a noble gas

atom is completely filled.

• The noble gases have stable electron

configurations with eight valence electrons (two
electrons in the case of helium).

• Elements tend to react to achieve electron

configurations similar to those of noble gases.

Stable Electron Configurations

6.1 Ionic Bonding

What is one way in which elements can
achieve stable electron configurations?

Ionic Bonds

Some elements achieve stable electron
configurations through the transfer of
electrons between atoms.

6.1 Ionic Bonding

Transfer of Electrons

• A chlorine atom has one electron fewer than an argon

atom. Adding one electron would give chlorine a
stable configuration.

• A sodium atom has one more electron than a neon

atom. Removing one electron would give sodium a
stable configuration.

Ionic Bonds

6.1 Ionic Bonding

When sodium reacts with chlorine, an electron is
transferred from each sodium atom to a chlorine
atom. Each atom ends up with a more stable
electron arrangement than it had before the
transfer.

Ionic Bonds

6.1 Ionic Bonding

When sodium reacts with chlorine, an electron is
transferred from each sodium atom to a chlorine
atom. Each atom ends up with a more stable
electron arrangement than it had before the
transfer.

Ionic Bonds

6.1 Ionic Bonding

When sodium reacts with chlorine, an electron is
transferred from each sodium atom to a chlorine
atom. Each atom ends up with a more stable
electron arrangement than it had before the
transfer.

Ionic Bonds

6.1 Ionic Bonding

When sodium reacts with chlorine, an electron is
transferred from each sodium atom to a chlorine
atom. Each atom ends up with a more stable
electron arrangement than it had before the
transfer.

Ionic Bonds

6.1 Ionic Bonding

Formation of Ions
When an atom gains or loses an electron, the
number of protons is no longer equal to the
number of electrons.

• The charge on the atom is not balanced, and the

atom is not neutral.

• An atom that has a net positive or negative electric

charge is called an ion.

• The charge on an ion is represented by a plus or a

minus sign.

Ionic Bonds

6.1 Ionic Bonding

The ion that forms when a chlorine atom gains an
electron has 17 protons and 18 electrons.

• This ion has a charge of 1–.
• The symbol for the ion is written Cl1–, or Cl– for short.
• An ion with a negative charge is an anion.
• Anions like the Cl– ion are named by using part of the

element name plus the suffix –ide. Thus, Cl– is called
a chloride ion.

Ionic Bonds

6.1 Ionic Bonding

A sodium ion has 11 protons and 10 electrons.

• The sodium ion has a charge of 1+.
• The symbol for the ion is written Na1+, or Na+ for

short.

• An ion with a positive charge is a cation.
• A cation uses the element name, as in the sodium

ion.

Ionic Bonds

6.1 Ionic Bonding

Formation of Ionic Bonds
A particle with a negative charge will attract a
particle with a positive charge.

• A chemical bond is the force that holds atoms or

ions together as a unit.

• An ionic bond is the force that holds cations and

anions together. An ionic bond forms when electrons
are transferred from one atom to another.

Ionic Bonds

6.1 Ionic Bonding

Ionization Energy
Cations form when electrons gain enough energy
to escape from atoms. The energy allows
electrons to overcome the attraction of the protons
in the nucleus.
The amount of energy used to remove an electron
is called ionization energy. The lower the
ionization energy, the easier it is to remove an
electron from an atom.

Ionic Bonds

6.1 Ionic Bonding

This figure shows two trends for ionization energy.

Ionic Bonds

6.1 Ionic Bonding

Ionic Puzzle Piece Activity

Ionic Bonds

6.1 Ionic Bonding

Compounds that contain ionic bonds are ionic
compounds, which can be represented by
chemical formulas.

• A chemical formula is a notation that shows what

elements a compound contains and the ratio of the
atoms or ions of those elements in the compound.

• The chemical formula for sodium chloride, NaCl,

indicates one sodium ion for each chloride ion in
sodium chloride.

Ionic Compounds

6.1 Ionic Bonding

What is the chemical formula for magnesium chloride?
Ionic Compounds

6.1 Ionic Bonding

What is the chemical formula for magnesium chloride?
Ionic Compounds

6.1 Ionic Bonding

What is the chemical formula for magnesium chloride?
Ionic Compounds

6.1 Ionic Bonding

What is the chemical formula for magnesium chloride?

A magnesium atom cannot reach a stable electron configuration by
reacting with just one chlorine atom. It must transfer electrons to two
chlorine atoms. After the transfer, the charge on the magnesium ion is
2+ and its symbol is Mg2+.

Ionic Compounds

6.1 Ionic Bonding

The formula for magnesium
chloride is MgCl2. The 2
written to the right and slightly
below the symbol for chlorine
is used to show the relative
numbers of atoms of the
elements present.
Magnesium chloride is used
to control dust on unpaved
roads.

Ionic Compounds

6.1 Ionic Bonding

How does the structure of an ionic
compound affect its properties?
Solids whose particles are arranged in a lattice
structure are called crystals.

Ionic Compounds

The properties of an ionic compound can be
explained by the strong attractions among
ions within a crystal lattice.

6.1 Ionic Bonding

Crystal Lattices
A chemical formula for an ionic compound tells
you the ratio of the ions in the compound, but not
how the ions are arranged.
If you looked at a sample of sodium chloride with
a hand lens or microscope, you would be able to
see that the pieces of salt are shaped like cubes.
The crystal shape is a clue to how the sodium
and chloride ions are arranged in the compound.

Ionic Compounds

6.1 Ionic Bonding

Ions in sodium chloride are arranged in an
orderly, three-dimensional structure.

• Each chloride ion is surrounded by six sodium

ions, and each sodium ion is surrounded by six
chloride ions.

• Each ion is attracted to all the neighboring ions

with an opposite charge.

• This set of attractions keeps the ions in fixed

positions in a rigid framework, or lattice.

Ionic Compounds

6.1 Ionic Bonding

The structure and shape of a crystal are related:

A In a sodium chloride crystal, each ion is surrounded
by six oppositely charged ions.
B Sodium chloride crystals are shaped like cubes

Ionic Compounds

6.1 Ionic Bonding

The shape of an ionic crystal, for example, the
cubic shape of a sodium chloride crystal,
depends on the arrangement of ions in its
lattice.
The arrangement of the ions depends on the
ratio of ions and their relative sizes. Crystals
are classified into groups based on the shape
of their crystals.

Ionic Compounds

6.1 Ionic Bonding

Properties of Ionic Compounds
The properties of sodium chloride are typical of
ionic compounds.

• Sodium chloride has a high melting point (801°C).
• Solid sodium chloride is a poor conductor of electric

current. When melted, it is a good conductor of
electric current.

• Sodium chloride crystals shatter when struck with a

hammer.

Ionic Compounds

6.1 Ionic Bonding

The arrangement of particles in a substance is
the result of two opposing factors: the
attractions among particles in the substance
and the kinetic energy of the particles.

• The stronger the attractions among the particles,

the more kinetic energy the particles must have
before they can separate.

• Ionic compounds have strong attractions

between particles and high melting points.

Ionic Compounds

6.1 Ionic Bonding

For an electric current to flow, charged
particles must be able to move from one
location to another.

• Ions in a solid crystal lattice have fixed positions.

Solid sodium chloride is a poor conductor of
electric current.

• When the solid melts, the lattice breaks apart,

and the ions are free to flow. Molten sodium
chloride is an excellent conductor of electric
current.

Ionic Compounds

6.1 Ionic Bonding

When an ionic crystal is struck,
ions are moved from their fixed
positions. Ions with the same
charge repel one another and
the crystal shatters.

Ionic Compounds

Hammer strikes crystal

Ionic crystal
shatters when
struck.

6.1 Ionic Bonding

Assessment Questions

1.

When is an atom stable?

a.

when its electrons are evenly distributed through its
energy levels

b.

when its lowest occupied energy level is filled with
electrons

c.

when its highest unoccupied energy level is filled with
electrons

d.

when its highest occupied energy level is filled with
electrons

6.1 Ionic Bonding

Assessment Questions

1.

When is an atom stable?

a.

when its electrons are evenly distributed through its
energy levels

b.

when its lowest occupied energy level is filled with
electrons

c.

when its highest unoccupied energy level is filled with
electrons

d.

when its highest occupied energy level is filled with
electrons

ANS: D

6.1 Ionic Bonding

Assessment Questions

2.

Which description applies to an element that has
two valence electrons?

a.

reactive metal

b.

nonreactive metal

c.

reactive nonmetal

d.

nonreactive nonmetal

6.1 Ionic Bonding

Assessment Questions

2.

Which description applies to an element that has
two valence electrons?

a.

reactive metal

b.

nonreactive metal

c.

reactive nonmetal

d.

nonreactive nonmetal

ANS: A

6.1 Ionic Bonding

Assessment Questions

3.

How do sodium and chlorine both achieve stable
electron configurations when they react?

a.

An electron is transferred from the sodium atom to the
chlorine atom.

b.

An electron is transferred from the chlorine atom to the
sodium atom.

c.

Both atoms gain one electron.

d.

Both atoms lose one electron.

6.1 Ionic Bonding

Assessment Questions

3.

How do sodium and chlorine both achieve stable
electron configurations when they react?

a.

An electron is transferred from the sodium atom to the
chlorine atom.

b.

An electron is transferred from the chlorine atom to the
sodium atom.

c.

Both atoms gain one electron.

d.

Both atoms lose one electron.

ANS: A

6.1 Ionic Bonding

Assessment Questions

4.

Why do ionic compounds tend to have high melting points?

a.

Ionic compounds contain more than one element, which causes a
high melting point.

b.

Ionic compounds cannot absorb energy efficiently because they
contain ions.

c.

An ionic compound contains metal atoms that raise its melting
point.

d.

A strong electrical attraction means ions require a lot of energy to
move apart.

6.1 Ionic Bonding

Assessment Questions

4.

Why do ionic compounds tend to have high melting points?

a.

Ionic compounds contain more than one element, which causes a
high melting point.

b.

Ionic compounds cannot absorb energy efficiently because they
contain ions.

c.

An ionic compound contains metal atoms that raise its melting
point.

d.

A strong electrical attraction means ions require a lot of energy to
move apart.

ANS:

D

6.1 Ionic Bonding

Assessment Questions

1.

The ratio of aluminum ions to chloride ions in
aluminum chloride (AlC13) is 3:1.

True
False

6.1 Ionic Bonding

Assessment Questions

1.

The ratio of aluminum ions to chloride ions in
aluminum chloride (AlC13) is 3:1.

True
False

ANS:F, 1:3

6.1 Ionic Bonding

Ionic Bonds

Formation of Ions
Scientists use atomic radii to compare the sizes of
atoms of different elements. The radius of a
sphere is the distance from the center of the
sphere to its outer edge–half the diameter of the
sphere.
Atomic radii are extremely small. They are
expressed in units of picometers (pm). There are
one billion (109) picometers in a millimeter.

6.1 Ionic Bonding

Ionic Bonds

This table shows the
atomic radius and ionic
radius for six metals
and six nonmetals. You
will use the data to
relate the size of an
element’s atoms to the
element’s location on
the periodic table and
to compare the sizes of
atoms and their ions.

6.1 Ionic Bonding

Ionic Bonds

1. Using TablesWithin a

period, what happens to the
atomic radius as the atomic
number of the elements
increases?

6.1 Ionic Bonding

Ionic Bonds

1. Using TablesWithin a

period, what happens to the
atomic radius as the atomic
number of the elements
increases?

Answer: Within a period,
the atomic radius
decreases as the atomic
number increases.

6.1 Ionic Bonding

Ionic Bonds

2. Using TablesWithin

Groups 1A, 2A, 6A, and
7A, what happens to
the atomic radius of
elements as the atomic
number increases?

6.1 Ionic Bonding

Ionic Bonds

2. Using TablesWithin

Groups 1A, 2A, 6A, and
7A, what happens to
the atomic radius of
elements as the atomic
number increases?
Answer: Within these
groups, the atomic
radius increases as the
atomic number
increases.

6.1 Ionic Bonding

Ionic Bonds

3. InferringHow does adding

an occupied energy level
affect the atomic radius?
(Hint: Lithium is a Period 2
element and sodium is a
Period 3 element.)

6.1 Ionic Bonding

Ionic Bonds

3. InferringHow does adding

an occupied energy level
affect the atomic radius?
(Hint: Lithium is a Period 2
element and sodium is a
Period 3 element.)
Answer: When the next
higher energy level is
occupied, there is a
significant increase in
atomic radius.

6.1 Ionic Bonding

Ionic Bonds

4. Comparing and

ContrastingCompare the
atomic and ionic radii for
potassium (K), and for
bromine (Br).

6.1 Ionic Bonding

Ionic Bonds

4. Comparing and

ContrastingCompare the
atomic and ionic radii for
potassium (K), and for
bromine (Br).

Answer: The ionic radius for
potassium is much smaller
than its atomic radius. The
ionic radius for bromine is
much larger than its atomic
radius.

6.1 Ionic Bonding

Ionic Bonds

5. Making Generalizations

What happens to the radius
of an atom when the atom
loses electrons? When the
atom gains electrons?

6.1 Ionic Bonding

Ionic Bonds

5. Making Generalizations

What happens to the radius
of an atom when the atom
loses electrons? When the
atom gains electrons?

Answer: With the loss of
valence electrons, the
radius decreases. With the
addition of valence
electrons, the radius
increases.

6.1 Ionic Bonding

Ionic Bonds

6. Relating Cause and

Effect Explain the
difference in size
between a metal atom
and its cation.

6.1 Ionic Bonding

Ionic Bonds

6. Relating Cause and

Effect Explain the
difference in size
between a metal atom
and its cation.

Answer: An energy
level that was occupied
is no longer occupied,
and the size decreases.