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Ionic Compounds Review
• Ionic compounds are the combination of ions. E.g. Na+ + Cl- NaCl.
• This formula represents the __________ of sodium ions and chloride ions not the exact number of them.
• They are composed of a ___________________ and form a crystal structure (e.g. NaCl and CaCl2 which are both salts)
Molecular Compounds
• Consist of atoms covalently bonded together
• The elements involved are all __________
Some examples
• N2O _____________ = Gas used at the dentist to relax patients
• NO2 _____________ = poisonous toxin emitted from car exhaust
More Examples
• H2O ______
• CO2 ____________ = Gas
exhaled and created during combustion reactions• CO ____________________= Lethal
gas created during incomplete combustion
Recall
• In ionic compounds, the non-metal rips away the electron(s) from the metal because the metals loosely hold their electrons
• This creates a positive and negative ion which attract each other making them stick together (opposites attract)
Molecular Compounds• made up of a non-metal and a non-metal.
• also called _____________
Molecular Compounds• ________ electrons (e-) to
form a ________________.
• Neg. e- are attracted to the Pos. nuclei of both atoms
Molecular CompoundsMolecular compounds are formed
when non metals share electrons to fill their outer electron orbit (shell).
If we draw the Lewis Structure for Fluorine,
We can see that it needs ________
It wants to share one electron with another atom.
If it bonds with another fluorine atomWe draw the shared pair of
electrons between the two atoms.
F F
F F
Shared electron pair ______
Molecular CompoundsMany molecular compounds are
predictable. How will Oxygen bond with
Hydrogen to form a molecule.Draw the Lewis Structure of both
Atoms.________________________
Clearly we need another Hydrogen atom
Putting the shared electrons between the atoms.
The molecule is H2O
H OH
H O
H
**The Oxygen atom has 8 valence electrons (full) and the Hydrogen has 2 valence electrons (full)
Molecular CompoundsNot all molecular compounds are as
predictable.How will Oxygen bond with Carbon?Draw the Lewis Structures of each
atom. ___________________________
If we add one more Oxygen, each oxygen can share two.
However, if Oxygen will share two and donate one of its other electrons pairs, Oxygen can bond with just on Carbon atom.
OC
OCO
C O
_____________
_____________
Types of Bonds
OCO
Carbon Monoxide – Triple Bond because _______pairs of electrons are shared
H O
H
Water – Single bond because ______ pair of electrons are shared
Carbon Dioxide – Double bond because _______pairs of electrons are shared
C O
Molecular Compounds – Naming
So Oxygen can form CO or CO2
We need a more flexible naming system for covalent compounds to reflect the many different bonding possibilities.
To name a covalent compound,1. Starting with the atom that is
to the left in the periodic table, (or lower)
2. Write the name of the atoms with the prefix indicating the number of that atom in the compound.
3. Change the ending of the last atom to – ide.
The prefixes are,1 _______2 _______ 3 _______4 _______5 _______6 _______7 _______
Note, the mono is omitted on the first atom.
CO _____________
CO2 _____________
Memorize me!
Number Prefix Number Prefix
1 mono 6 _________
2 _________ 7 hepta
3 tri 8 _________
4 _________ 9 nona
5 penta 10 _________
Naming Example
• P4O10
Phosphorus - use prefix tetra (4)Oxygen – change ending – OxideOxide – use prefix deca (10)
= _________
Molecular Compounds - NamingName the following compounds
CF4
_________
H2O
_________
PF5
_________
Write the chemical formula for,
Sulphur Dioxide
_________
DiCarbon Tetrahydride
_________
Molecular Compounds – Diatomic Gases
Molecular compounds show an incredible variety in structure, physical and chemical properties.
There are categories that further divide covalent compounds into categories with common properties.
Diatomic Gases – _________
The Halogens, Oxygen, Nitrogen and Hydrogen form diatomic gases.
H2 is called Hydrogen Gas not Dihydrogen.
Writing Formulas
left-most element goes 1st
Carbon monoxide
- Carbon (C) no prefix therefore = C- Monoxide – Mono = 1 therefore, 1 oxygen
atom = O= _________
Writing Formulas
• Nitrogen dioxide
- Nitrogen (N) no prefix therefore = N- Dioxide – Di = 2 therefore, 2 oxygen
atoms = O2
= _________
Writing Formulas
DiCarbon Tetrahydride
- Dicarbon (C) Di = 2 therefore = C2
- Tetrahydride (H) Tetra = 4 therefore, 4 Hydrogen atoms = H4
= _________