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CHEMICAL BONDING
VSEPR Theory
Objectives
◻ Predict the shape of a molecule based on the VSEPR theory.
Warm-Up: Draw Lewis Structures for the following:
IONIC COVALENT
MgI2 CF4
HOMEWORK CHECK
VSEPR
Stands for:
⬜ V-Valence
⬜ S-Shell
⬜ E-Electron
⬜ P-Pair
⬜ R-Repulsion
Basically Electrons don’t like each other very much!
A Few Important Terms:
Central Atom:
Lone Pairs: centralatom
Bonds:
VSEPR: Valence Shell ElectronPair Repulsion
Atoms Attached to the
Central Atom
Lone Pairs on
Central Atom
Shape
4 0 Tetrahedral
3 1 Trigonal Pyramidal
3 0 Trigonal Planar
2 1 or 2 Bent
2
OR a 2 atom molecule
0
H2, N2, HCl for example
Linear
IONIC COMPOUND --------- Lattice (Salt)
Lone pairs = unshared electrons
What About Ionic Structures????
◻ Lattice- Ionic Compounds form a 3D lattice structure when the cations and anions come together via electrostatic attraction.
◻ The Lattice has a repeating structure - NaCl
MOLECULAR GEOMETRY EXPLORATION
CH4Step 1: Draw Lewis Structure
Step 2: Examine Central Atom
Step 3: Count # of atoms bonded around central atom
Step 4: Count # of lone pairs around central atom
Step 5: Determine the Geometry
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ H2O
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ H2O
Atoms bonded = 2
Lone pairs = 2
BENT
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ NH3
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ NH3
Atoms Bonded = 3
Lone Pairs = 1
TRIGONAL PYRAMIDAL
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ CH4
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ CH4
Atoms bonded = 4
Lone pairs = 0
TETRAHEDRAL
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ SO3
Example
◻ Draw the Lewis Structure. Predict the shape.
◻ SO3***** Sulfur is the CENTRAL ATOM
Trigonal Planar
3 atoms bonded to Sulfur
0 lone pairs on Sulfur
You Try
Draw the Lewis Structure &
Predict the Shape of the Following:
◻ AsH3
◻ SiF4
◻ CO2
You Try
Draw the Lewis Structure &
Predict the Shape of the Following:
◻ PF3
◻ SiF4
◻ CO2
Molecule or Ion_______________
# valence
electrons
Lewis Dot
Structure
# Lone
Pairs
# of atoms
Bonded to
central atom
VSEPR
Shape
Are there Ionic
Bonds in the
structure?
Is the molecule or
ion polar? Why?
CH44 + 1 + 1 + 1 + 1=8
0 4 Tetrahedral Yes No. No lone pairs.
All atoms bonded
are identical
CH2F2
NH3Trigonal Pyramidal Yes Yes. There is a
lone pair on the
central atom
AsI33
HCNLinear
N2- - - - - - - - - - - - - - No No. Atoms are
Identical
H2OBent
SCl22
SO3Trigonal Planar
CF2O3
Molecule or Ion_______________
# valence
electrons
Lewis Dot
Structure
# Lone
Pairs
# of atoms
Bonded to
central atom
VSEPR
Shape
Are there Ionic
Bonds in the
structure?
Is the molecule or
ion polar? Why?
HBr- - - - - - - - - - - - - -
SiCl4
CH2O
NO2-1
CO3-2
OH-1- - - - - - - - - - - - - -
SO4-2
CO2
NO3-1
NH4+
Six Shapes Practice
A B C
DE
F
Six Shapes
A B C
DE
F
TRIGONAL PLANARTETRAHEDRAL TRIGONAL PYRAMIDAL
LINEAR
IONIC – LATTICE/SALT
BENT
Try This !!
Exit Ticket
(1) Draw the Lewis Structure for Carbon Dioxide (CO2)
(2) Predict the geometric shape of carbon dioxide
(3) How many lone pairs of electrons are on the central
atom?
(4) Describe the bond(s) between the carbon atom and
the two oxygen atoms.
(5) How many atoms of each type are in 8 Pb(NO3)2 ?
HOMEWORK:
Finish Molecular Geometry Exploration
Quiz: Tuesday 10/8/18
Lewis Structures & VSEPR
Unit 4 TEST Friday 10/12/18