Ch. 8 – Ionic Compounds
8.1 Forming Chemical Bonds
Chemical Bond –
May be formed from
1)
2)
Table 8.1: Electron Dot Structures
Group
1A
2A
3a
4a
5a
6a
7a
8a
Diagram
Noble gases show low reactivity because they have…
_____ ionization energies
_____ electron affinities
Stable octet –
Formation of positive ions:
Positive ions are formed by losing ____________ electrons.
Reactivity of metals is based on ________________________________________.
Cation Group 1A forms ______
Group 2A forms ______
Group 3A forms ______
Transition metals commonly lose ______________, but may also lose their ___
electrons forming ____ ions or greater.
Formation of negative ions:
Nonmetals (on the right side) have _________________ for electrons and form a stable outer
electron configuration by ______________________.
Anion –
To name an anion, the ending ___________ is added.
Cl = Chlorine atom
Cl- = ______________ ion
N3- = ______________ ion
Nonmetals gain enough electrons so the total is _______ valence electrons.
_____ = phosphide ion
_______ = oxide ion
8.2 The Formation and Nature of Ionic Bonds
Formation of an Ionic Bond
Na
____ an electron
+
Cl

____ an electron
NaCl
forms because of the attraction between
_____________________
Ionic Bond –
Compounds that contain ionic bonds are _____________________.
Ionic compounds that contain oxygen are called ____________.
Most other Ionic compounds are called ____________.
Binary compounds –
- The number of electrons lost must ____________ the number of electrons _________.
Properties of Ionic Compounds
The _____________ that occur between the atoms in a compound determine many of the
physical properties of the compound.
- ____________________________ are packed into a regular repeating pattern that
balances the forces of attraction and repulsion between the ions.
- The _____________ attraction of positive ions and negative ions in an ionic compound
results in a ____________________.
- Because ionic bonds are __________________, the crystals require
________________________________ to be broken apart.
- Thus …
o Ionic crystals have ____________ melting and boiling points.
o They are also ____________, ______________, and _____________.
- Conductivity:
o In a solid –
o In a liquid –
o In a solution (mixed with water) –
Electrolyte –
Energy and the ionic bond –
Endothermic –
Exothermic –
The formation of ionic compounds from ____________ is always _______________.
Lattice energy Lattice energy is related to
1)
Li vs. K
2)
MgO vs. NaF vs. SrCl2
Ex.
RbF vs. KF – which is more exothermic?
SrCl2 vs. AgCl – which is more exothermic?
8.3 Names and Formulas for Ionic Compounds:
Formulas for Ionic Compounds
Ionic compounds are represented by a formulas that provides ________________________
because ______________________________________.
Formula unit –
The overall charge of a formula unit is ___________.
Determining Charge:
Monatomic ion –
Table 8-4
Group
1A
2A
5A
6A
7A
Atoms that commonly form ions
Charge on Ions
Table 8-5 (some…)
Group
Atoms that commonly form ions
3A
4A
Charge on Ions
Oxidation number – same as charge for ionic compounds – we won’t use this term now.
In writing formulas, subscripts are used to the lower right to indicate _________________.
Ex. 8-2 – What the ionic formula of a compound formed between potassium and oxygen?
Ex. 8-3 – What the ionic formula of a compound formed between aluminum and sulfur?
Compounds that contain polyatomic ions:
Polyatomic ions –
When writing formulas, if more than one polyatomic ion is needed _________________
______________________________________.
Formula for NH4+ and Cl- _____________
Ex. 8-4 – What the ionic formula of a compound formed between calcium ion and phosphate
ion?
Naming Ions and Ionic Compounds:
Oxyanion –
- The ion with more oxygen atoms is named…
- The ion with fewer oxygen atoms is named…
Ex.
-
NO3-
NO2-
SO42-
SO32-
The ion with the greatest number oxygen atoms is named…
The ion with one less oxygen atoms is named…
The ion with two fewer oxygen atoms is named…
The ion with three fewer oxygen atoms is named…
Ex.
ClO4-
ClO3-
ClO2-
ClO-
Naming Ionic Compounds –
1. Name the ___________ first and the ____________ second.
2. _______________________ cations use the _________________ name.
3. ___________________ anions take their name from the ________ of the element name
plus ____________________.
4. Group ________ and _____________ metals have only one oxidation number.
________________ metals and metals on the __________________ of the periodic table
often have ___________________________.
To distinguish between multiple oxidation number of the same element, the name of the
chemical formula must indicate _____________________ of the _____________. The
oxidation number is written as a _______________________ in __________________
after the name of the ___________________.
Ex.
Ex.
Fe2+ and O2- = FeO which is named: ____________________
Fe2+ and O2- = Fe2O3 which is named: ____________________
5. If the compound contains a polyatomic ion, simply __________________________.
Figure 8-8 (Write is space provided if you think it would be helpful.)