Ionic and Metallic Bonding
Chapter 7
Valence Electrons
 The _______________in an atom
 Their arrangement determines the
bonding __________and activities
of an atom
 S-Block– they are the same as the
group number
Na= 1 valence electron
 P-Block–They are the group
number- 10
C= 4 valence electrons
F= 7 valence electrons
Iodine… 7 valence electrons
Electron Dot Notation:
Instead of drawing the orbital
diagram, which can be long
& complex, there is an easier
way to represent the atoms.
_______________________: is an
electron notation in which
only the _______________are
shown, and are represented
by dots around the element’s
symbol.
Lots and lots of examples…
Valence
electrons
Dot
notation
Ions
Ion:______________________________
Cation: atom that has a +ve charge (A+).
i.e. missing an eAnion: atom that has a –ve charge (X-).
i.e. has an extra e-
Do the Lewis structure for Cl, Cl-, Na, Na+
Polyatomic Ions
 An ion that consist of____________, covalently bonded
together and carrying a charge.
 Common Examples…
 OH- (Hydroxide)
 NO3- (Nitrate)
 SO42- (Sulfate)
 PO43- (phosphate)
(draw their Lewis structures)
Ionic Bonding
Most of Earth’s rocks & minerals are made up of compounds held
together by ionic bonds.
________________: consists of positive (cat) & negative (an) ions
that are combined such that the # positives = # negatives.
e.g. Na -> Na+ + e- & Cl + e- -> ClNa+ + Cl- -> NaCl
(#+’s = #-’s)
e.g.2. Mg & Cl
Most ionic compounds exist as a ______________of alternating +’ve
& -’ve ions (NaCl dia)
(Screen 3.9 Coulomb’s law, 3.10 NaCl, 3.10.SB KBr)
Ionic Compounds: Molecular
arrangement
_________________: is
the simplest collection of
atoms from which an ionic
compounds formula can be
established.
Ionic compounds can be
represented by Electron
Dot diagrams.
e.g. NaCl
Ionic Solid Structure
 Ionic crystals combine in an orderly arrangement known as a
_________________
 Crystalline solids at room temperature
Rutile (crystal
and model of
lattice)
Ionic Solids: Characteristics
-high melting/boiling
pts
-_______________
-when molten (or
dissolved in H2O)
they become
good___________
______________
Metallic Bonding:
 Metals have few valence e-’s (1,2or3) which
roam freely as a “sea of electrons” throughout
the metal. They do not belong to any
particular atom
 The atoms themselves are arranged in
a______________________________.
 The bonding between the metal atoms & this
sea of electrons is called_______________.
 It is NOT bonding between different types of
metal atoms.
Metal Solids
Characteristics:
•highly conductive:
electrical & heat
•___________
•___________
•___________
Metals can only come together when they are in their molten state.
A mixture of 2 or more metals called an alloy.
Alloys
____________________: some of the host
metal atoms are replaced by other
similar sized metal atoms.
E.g’s: Brass:
Bronze:
Sterling Silver:
24 Karat Gold:
18 Karat Gold:
Copper (~2/3) & Zinc (~1/3)
Copper (~80%) & Tin (~20%)
Silver (93%) & Copper (7%)
Gold (100%)
Gold (18/24 = 75%) & Silver
_______________: some of the holes
(interstices) between the metal atoms
are filled with small atoms.
Makes the metal harder, tougher and
more durable… better for building
E.g’s: Steel:
Iron &
Carbon (small %)