orgo ch2

octet rule

atoms share e to complete octet

formal charge

valence electrons minus number of bonds minus number of lone pairs

two groups of electrons

linear

three groups of electrons

trigonal planar

four groups of electrons

tetrahedral

4 groups of electrons: 3 bonds and 1 lone pair

trigonal planar

4 groups of electrons:2 bonds and 2 lone pairs

bent

bond polarity

difference in electronegativity between bonded atoms and polarizability of atoms

non polar bonds

electrons are shared equally between atoms with same electronegativity

polar bonds

form between atoms of different electronegativity

electronegativity trend

increase left to right, increase bottom to top

c-h bond

nonpolar

molecular polarity for polar diatomic molecules

bond dipoles where polyatomic molecules are the vector of sum of individual bond dipoles

molecular polarity for nonpolar

the individual bond dipoles cancel each other out

2 hybrid orbitals

sp, linear, 180

3 hybrid oribitals

sp2, trigonal planar, 120

4 hybrid orbitals

sp3, tetrahedral, 109.5

sigma bonds

formed by hybridized orbitals

pi bonds

formed by unhybridized p orbitals

resonance structures

redistributing of shared pi electrons and unshared lone pair electrons

molecular orbital theory

the formation of molecular orbitals by interaction of atomic orbitals of different atoms in a molecule

ion ion

between two ionic groups of opposite charge

ion dipole

between ion and polar molecule with net dipole moment

dipole dipole

between polar molecules with net dipole moment

dispersion forces

between nonpolar groups

hydrogen bonds

between h and n,o,f