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Q of the Day. Day 2 3-30. Write the formula for magnesium chloride. Draw the dot structure for magnesium chloride. Valence-Shell, Electron-Pair Repulsion VSEPR theory. Repulsion between sets of valence-level electrons, causes them to be oriented as far apart as possible. VSEPR THEORY. - PowerPoint PPT PresentationTRANSCRIPT
1. Write the formula for magnesium chloride.
2. Draw the dot structure for magnesium chloride.
Day 2 3-30
Valence-Shell, Electron-Pair Repulsion
VSEPR theory
Repulsion between sets of valence-level electrons, causes them to be oriented as far apart as possible
What do electrons do to other electrons?
VSEPR theory – in a small molecule, the pairs of valence electrons are arranged as far apart from each other as possible
Build:
O2
CO2
*BCl3
CH4
*NH3
H2O
Linear
Trigonal planar
Tetrahedral
Pyramidal Bent
Reds = oxygen short “bonds” = single bonds
Blacks = carbon long “bonds” = double bonds
Whites = hydrogen
Greens = chlorine
Blue = nitrogen
1st & 5th pd stopped
3rd pd stopped
Number of atoms bonded to central atom
# of lone pair electrons
Shape Example(s)
1 0, 1, 2, 3 _________ NaCl, O2
2 0 _________ CO2
2 2 _________ H2O
3 0 __________________
BCl3
3 1 _________ NH3
4 0 _________ CH4
LINEAR
LINEAR
BENT
TRIGONAL
PLANAR
PYRAMIDAL
TETRAHEDRAL
Carbon compounds form 3 shapes, what are they?
WHY? ______________________
____________________________
____________________________
Read Section 8.4 (pages 261-264 AND complete #s 61, 63, 64, 66 (only molecular shape not hybrid orbitals) AND # 60 = an optional bonus –
must be correct
Going back: How did we name orbitals?
2p
Energy level
Shape
As atoms come together and bond, orbitals come together, overlap, and mix … hybridization
As atoms come together and bond, orbitals come together, overlap, and mix … hybridization
Hybrid orbitals – mixed orbitals – combo. of properties of the atomic orbitals that formed them
Intermolecular ForcesForces of attraction between molecules
Intramolecular ForcesForces of attraction within molecules
OH
H
Intermolecular ForcesForces of attraction between molecules
Hydrogen Bonding
OH
H(-) (+)O
H
H(-) (+) O
H
H(-) (+)
PERIODS 3 & 6 – 2-18
Hydrogen bonding is a direct result of water’s polar nature and leads to …
Water sticking to water
Water sticking to something else
… cohesion … adhesion
Does a polar bond mean you have a polar molecule?
Polar molecules unequal charge
distribution …2 factors are molecular shape and bonds (polar
vs. nonpolar)
Linear
VSEPR theory
Intermolecular force
Cohesion
H2SO4
Hydrogen bonding
Bent
Adhesion
Intracellular
Octet rule
Number of atoms bonded to central atom
# of lone pair electrons
Shape Example(s)
1 0, 1, 2, 3
_________
NaCl, O2
2 0
_________
CO2
2 2
_________
H2O
3 0 _________
_________
BCl3
3 1
_________
NH3
4 0 _________
CH4