2.2- covalent model
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covalent bonding
electrostatic attraction between a shared pair of electrons and positively charged nuclei
whats the definition of the covalent bond iself
electrostatic attraction of the positive nucleii for the region of negatively charged jigh electron density
whats the region of high electron density
space between the atoms where a pair of electrons are shared
atoms forming a covalent bond will achieve a lower energy state by…
sharing electrons and have a full valence shell. This can be doen by either forming single double or triple bond
octet rule
filling of the valence shell to achieve 8 electrons, this rule can in certain circumstances be broken
electronegativity
relative measure of attraction of an atom for a pair of electrons (in a covalent bond)
effective nucleus charge determines
the net positive charge pulling these electrons towards the nucleus electronegativity and ionization energy
whats the hybrid diagram
the one with the lines
lewis diagram
one with the dots
2 electron domains
= linear, andgle= 180 eg. co2
3 electron domains
= triognal planar angle= 120 eg. c2h4 or bf3
3 electron domains 1 lone pair
angle= 104.5 because stronger repulsion from lone pairs, forcing bonding pairs closer together =bent linear eg.so2
4 electron domains
=tetrahedral angle= 109.5 eg. ch4
4 electron domains 1 lone pair
=trigonal pyramidal angle= 107 due to extra repulsion from lone pair eg. Nh3
4 electron domains 2 lone pairs
=bent angle= 104.5 even greater repulsion eg. Oh2
repuslion diagram explain
biggest repulsion is between two pairs oflone pair intermedaite= between lone pai and bonding pair least between 2 bonding pairs
domain geometry
= total number of domains, negatively charged areas with electrons ncluding line pairs
molecular geometry
only bonding pair areas
electronegativity
ability of atom to draw pair of electrons towards itself in a covalent bond
higher value in pauleen scale means
more electronegativ element it is in diatomic molecules electron density shared equally between 2 atoms eg. h2 AS BOTH ATOMS HAVE SAME ELECTRONEGATIVITY VALUE= EQUAL ATTRACTION FOR BODNING PAIR OF ELECTRONS LEADING TO FORMATION OF A COVALENT BOND which is non polar
polar bond
when 2 atoms in a covalent bond have different electronegstivity, covalnt bond= polar, electrons are drawn to more electronegative atom, electron distributions is aysemmetric the less electronegative atom si partially positive charge and more is partially negative harge bigger the differnece in electronegativity between 2 atoms higher polarity of covalent bond
dipole moment
measure of how polar a bond is , arrow points to partilly negative charge
intramoleculer vc inter
intra within molecules inter between seperate moelcules
what are the 3 main intermoleculear forces
london (dispersion) force dipole dipole attraction dipole induced dipole hydrogen bonding