Chemical Bonding
and Nomenclature
Bonding Basics, Ionic
Bonding, Formula Writing
and Naming
What is a bond?
• Bond –
- formed when electrons are __________ or ______
between atomic nuclei.
- All bonds occur b/c of _______________________.
(+ / - attract one another)
Intramolecular forces –
– Covalent
– Ionic
What electrons and How?
• ___________ electrons are used in bonding.
- Stable elements want to _____________ similar
to the noble gases.
- If the element is a ______ it wants to achieve the
noble gas configuration for the noble gas ________.
Metals ____________ to achieve this. (______)
- If the element is a ________ it wants to achieve
the noble gas configuration for the noble gas ______.
Nonmetals ____________ to achieve this. (_____)
Ionic Bonding
• Between ionic compounds which contain a _____ and a
__________
• Atoms that lose electrons relatively easily (______)
react with an atom that has a high affinity for
electrons (_________)
• __________ of electrons
• Electrostatic attraction between + and –
metals
nonmetals
Lewis Structure
• _____________________________
• shows how the ________________
are arranged among the atoms in the
molecule
• can be used for Ionic or Covalent
Bonding
Lasso and Arrow Technique
• ______________________________
______________________________
• Metals should generally lose all of their
valence e- and nonmetals will gain to
have a full shell.
• Shows the _______ (__ valence e-)
Lights on for some examples!!!!
Naming Ionic Compounds
• Binary compounds –
1)
2)
• Naming Compounds That Contain a Metal and a Nonmetal
• Binary ionic compound –
• Type 1 Compounds –
• Type II Compounds –
Naming Type I Ionic
Rules 1. Cation is always named first and the anion second
2. Cation takes its name from the name of the
element
3. Anion takes its name from the root of the
element name and changing the ending to –ide
Example: Name the following Type I Ionic Compounds.
a) AlCl3
b) MgI2
c) SrI2
d) K2S
Naming Type II Ionic
1. Determine the charge of the anion.
2. Assign a charge to the cation, that will give the ionic compound a net
charge of zero.
3. Name the cation with the name of the element.
4. Put the charge of the cation, as a Roman Numeral in parentheses,
after the name of the cation
5. Follow the Roman Numeral, with the name of the anion, take the root
of the elements name and change the ending to –ide
Example : Name the following Type II Ionic Compounds
a) CuCl
b) MnO2
c) Fe2O3
d) PbCl2
Example : Name the following Type I and II Ionic Compounds
a) CoBr2
b) CaCl2
c) Al2O3
d) CrCl3
Naming Compounds That Contain
Polyatomic Ions
polyatomic ions –
To name use the rules for naming Type I Ionic or
Type II Ionic. Name the polyatomic ion with its
full name, do not change the ending.
Example:
a) Na2SO4
Name these compounds that contain polyatomic ions.
b) K3PO4
c) Fe(NO3)3 d) Mn(OH)2
Writing Formulas for Ionic Compounds
Rules1. Write the symbols for the elements.
2. Label the symbols with the appropriate charge
Remember the Roman Numeral is the charge.
3. Add subscripts so the charges will equal zero.
Examples: Write the formula.
a) potassium hydroxide
b) sodium carbonate
c) iron (III) oxide
d) cobalt (III) nitrate
e) calcium chloride
f) lead (IV) oxide
g) ammonium sulfate