Daily Science
 Name the following compounds that contain a
TRANSITION METAL:



Zn2O3
ZrF2
CuN
Metallic and Covalent Bonds
PG. 53
Metallic Bonds
 Between a metal and a metal
 Outer energy levels form a ‘sea of electrons’
 High melting and boiling points
 Good conductors
 Can make alloys (mixture of elements that have
metallic properties)
 Ex. Brass and bronze
Covalent Bonds
 Non-metal and non-metal
 Valence electrons are shared
 Form molecules (2 or more atoms covalently
bonded)
 Use Lewis Structures to show covalent bonds
Lewis Structures and Covalent Bonding
 The shared electrons are called bonding pairs
 Unshared electrons are called lone pairs
 Single bonds in a Lewis structure are called sigma
bonds (σ)
 Double and triple bonds are called pi bonds (π)
 When bonds are broken they either release energy or
take in energy


Exothermic- energy is released (feel heat)
Endothermic- Energy is absorbed ( feels cold)
Naming Covalent Bonds
 Name the first element first using the whole name
 If there is only one of the element name is regularly
 If there is more than one of the element use a prefix
 The second element ALWAYS gets a prefix and the
ending drops and you add –ide
 Neither one is capitalized
Number of atoms
Prefix
1
mono-
2
di-
3
tri-
4
tetra-
5
penta-
6
hexa-
7
hepta-
8
octa-
9
nona-
10
deca-
Examples
 CCl4
 As2O3
 CO
 SO2
 NF3
Naming Acids
 Always has a Hydrogen attached to it and is always
dissolved in water
 Naming binary acids:



Only 2 elements
Has a hydrogen atom
Hydro- element or polyatomic ion- ic acid
 Naming oxyacids:
 A polyatomic ion that contains an oxygen
 If the ion ends in –ate change it to –ic
 If the ion ends in –ite change it to –ous
Examples
 HBr
 HCN
 HNO3
 HNO2