3B.1 covelant bonding
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what is covalent bondingg
it is the electrostatic attraction between the nuclei of the bond atoms and the pair of electrons shared between them
what leads to a sigma bond formation
any end-on overlap leads to a formation of a sigma bond
what is a sigma bond
a type of covalent bond that forms a single covalent bond between two atoms
what leads to a pi bond formation
a sideways overlap of two p-orbitals
why is a pi bond only double or triple bond s
a pi bond cannot form until a sigma bond is formed
what does a pi bond result in
high electrons density both above and below the molecule
what is an example of a pi bond
• in an ethene molecule, one of the carbon bonds is a sigma bond; the other is a pi bond. • the triple bond in a nitrogen molecule is made up of one sigma bond and two pi bonds
why are alkenes more reactive than alkane s
it is because alkenes have 1 sigma bond that is stronger than 1 pi bond
what are examples of a sigma bond
• hydrogen s orbitals would overlap to form a new molecular orbital. the 2 electrons would exist in a new orbital, the highest electron density is between the two nuclei • chlorine p orbitails would overlap each other
what is the bond length
it is the distance between nuclei of two atoms that are covalently bonded together.
the strength of a covalent bond
is the energy required to break a single mole of the bond length in a gaseous state
what is the general relationship between bond length and bond strength
the shorter the bond the stronger the bond length
The stronger the bond length the stronger the…
electrostatic attraction between the two nuclei and the overlapping shared pair of electrons