Chemical Bonding Geometry
by Owen Borville
October 25, 2022
Chemistry
Lewis structures don’t show all information about chemical bonds.
Valence Bond theory=
Covalent=both atoms acquire electrons that fill orbital
Sigma Bond 1s orbital
Pi Bond=p orbitals=single, double, and triple bonds, weaker than sigma bonds
Molecular Resonance=Lewis structure does not totally describe the distribution of electrons and bonds are of intermediate character=electrons have multiple locations and partial bonds
Octet Rule Exceptions=not having 8 electrons in outer shell
Some molecules have an odd number of valence electrons to share
Some molecules can feature less or more than 8 electrons shared.
Valence bond theory does not explain chemical bonding totally
Orbitals are replaced with new orbitals in an atom when a molecule forms
There are bonding and antibonding orbitals=when orbitals in atoms either reinforce each other or interfere against each other.
VSEPR=Valence shell electron pair repulsion theory=electrons repel each other until they are as far apart as is geometrically possible=Geometric structures=tetrahedral, trigonal planar, and linear
Orbital Hybridization=how carbon bonds=s and p orbitals combine into a single valence energy level=sp3 (one s and three p orbitals combine)
Other orbital hybridization possibilities=BF3, sp2
Examples=CH4 (methane)=tetrahedral
NH3 (ammonia)=only 3 bonding pairs and pyramidal
H2O (water)=only 2 bonding pairs=bent
HF= (hydrogen fluoride)=single bond= linear
Diatomic molecule bonds=share electrons equally=same electronegativities
Unequal sharing of electrons=different electronegativities=Polar Covalent bonds
Polar covalent bonds=greater difference in electronegativity=higher polarity
Ionic bonds=very polar
Polar covalent bonds=symbolized with a directional arrow toward the more polar atom in the Lewis structure.
All compounds of different elements are polar to some degree
Dipole moment=measure of the amount of polarity (unequal sharing) of electrons in a compound=vector sum
Non-polar=molecule is symmetrical=All outer electronegativities are equal
by Owen Borville
October 25, 2022
Chemistry
Lewis structures don’t show all information about chemical bonds.
Valence Bond theory=
Covalent=both atoms acquire electrons that fill orbital
Sigma Bond 1s orbital
Pi Bond=p orbitals=single, double, and triple bonds, weaker than sigma bonds
Molecular Resonance=Lewis structure does not totally describe the distribution of electrons and bonds are of intermediate character=electrons have multiple locations and partial bonds
Octet Rule Exceptions=not having 8 electrons in outer shell
Some molecules have an odd number of valence electrons to share
Some molecules can feature less or more than 8 electrons shared.
Valence bond theory does not explain chemical bonding totally
Orbitals are replaced with new orbitals in an atom when a molecule forms
There are bonding and antibonding orbitals=when orbitals in atoms either reinforce each other or interfere against each other.
VSEPR=Valence shell electron pair repulsion theory=electrons repel each other until they are as far apart as is geometrically possible=Geometric structures=tetrahedral, trigonal planar, and linear
Orbital Hybridization=how carbon bonds=s and p orbitals combine into a single valence energy level=sp3 (one s and three p orbitals combine)
Other orbital hybridization possibilities=BF3, sp2
Examples=CH4 (methane)=tetrahedral
NH3 (ammonia)=only 3 bonding pairs and pyramidal
H2O (water)=only 2 bonding pairs=bent
HF= (hydrogen fluoride)=single bond= linear
Diatomic molecule bonds=share electrons equally=same electronegativities
Unequal sharing of electrons=different electronegativities=Polar Covalent bonds
Polar covalent bonds=greater difference in electronegativity=higher polarity
Ionic bonds=very polar
Polar covalent bonds=symbolized with a directional arrow toward the more polar atom in the Lewis structure.
All compounds of different elements are polar to some degree
Dipole moment=measure of the amount of polarity (unequal sharing) of electrons in a compound=vector sum
Non-polar=molecule is symmetrical=All outer electronegativities are equal