Chapter 7 PPT
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Transcript Chapter 7 PPT
Chapter 7
IONIC AND METALLIC BONDING
Objectives
You WILL be able to…
Determine number of valence electrons in an atom of a
representative element
Explain how the octet rule applies o atoms of metallic
and nonmetallic elements
Describe how cations form
Explain how anions form
Explain the electrical charge of an ionic compound
Describe 3 properties of ionic compounds
Model the valence electrons of metal atoms
Describe the arrangement of atoms in metal
Explain the importance of alloys
Ions
Valence Electrons – Electrons in the highest
occupied energy level of an element’s atoms
The number of valence electrons determines an
element’s properties
Group number indicates the number of valence e-
The Octet Rule- the achievement of 8 electrons in the
highest energy level of an atom
Done by losing, gaining, or sharing valence electrons
Formation of Cations
Cations form when atoms lose valence electrons
Metals usually do this because they only have a few
valence electrons and they have low ionization energies
The loss of valence electrons makes the cation more
stable than the atom because there is an complete octet
in the valence shell
For example:
Na = 1s22s22p63s1 and Na + = 1s22s22p6
Monatomic cations are named using the name of the
element (ie sodium ion, magnesium ion)
Some metals that easily give up valence electrons are…
Alkali metals (+1 charge)
Alkali Earth Metals (+2 charge)
Aluminum (+3 charge)
Heavier group IV and V elements (Sn +2 or +4; Pb +2 or
+4; Bi +3)
Most transition and inner transition elements (Ag+1, Zn
+2, Cr +3; most rare earth metals +3)
Some transition metals have cations with varying charge
depending on what they are bonded with (ie Fe +3 and
Fe+2)
Formation of Anions
Anions form when atoms gain valence electrons
The gain of valence electrons makes the anion more
stable than the atom because there is now a complete
octet in the valence shell
For example:
Cl = 1s22s22p63s23p5
and Cl - =1s22s22p63s23p6
Anions are named using the root of the element’s
name plus the ending –ide (ie. bromide, chloride)
Some nonmetals easily acquire electrons…
Halogens (-1 charge)
Chalcogens (-2 charge)
Nitrogen (-3 charge)
Polyatomic Ions are comprised of two or more atoms
covalently bonded that can be considered as acting
as a single particle
Ionic Bonds and Ionic Compounds
Ionic bonds are formed when the charges on positive
ions balance the charges on the negative ions
through electrostatic attraction
Formula units are the lowest whole number ratio of
ions in an ionic compound.
Chemical formulas are shorthand ways of showing
the amounts and the types of elements in the
smallest representative unit
Example: NaCl, CaBr2, AlI3 (salts)
Electron Dot Formulas-Open and closed circles or x’s
Ionic attractions are so strong that almost all ionic
compounds are solid with unique crystalline
structures
The strength of the bonds also leads to high melting
points and boiling points
Ionic bonds almost always occur between metals and
nonmetals
Ionic compounds are also good conductors of
electricity if dissolved in water or molten
Ionic compounds are electrically neutral, therefore
the number of positive charges is the same as the
number of negative charges.
Colors of Ionic Compounds
Transition metal ions having partially filled d
orbitals usually have a color.
For example…
NiSO4
FeCl3
CuSO4
Metal cations that have no d electrons or completely
filled d orbitals are usually not colored.
NaCl
MgSO4
CaCl2
ZnCl2
Metals in Bonding
Metals have loosely held valence electrons
When metal atoms exist in the solid form of a metal
all the nuclei share all the valence electrons of all the
atoms in the sample
“Electron Sea”
The “sea of electrons” explains physical properties
such as conductivity, malleability, and ductility
Metals are arranged in compact and orderly patterns
Alloys
Mixtures of two or more elements where at least one
is a metal
Steel, brass (Cu and Zn), bronze
Mixing alloys will result in a metal with superior
properties than those of the component materials
Them’s
22’s son!!!