INTRODUCTION TO ORGANIC CHEMISTRY
Organic chemistry focuses on organic compounds. compounds that contain carbon atoms.
elements in the first group of the periodic table like hydrogen they like to form one bond. Beryllium
for example likes to form two bonds boron which has three valence electrons it likes to form three
bonds, carbon has four valence. electrons carbon likes to have four bonds. elements like fluorine
and the other halogens. chlorine ,bromine, iodine they like to form seven bonds.
A polarized object is an object that is neutral overall but has charge separation. that is one
side is positive and the other side is negative so this is a polar object the bond is polar because
fluorine carries a partial negative charge due to the fact that it 's more electronegative than carbon
so it pulls electrons toward itself. The carbon hydrogen bond that 's a nonpolar covalent bond is
non-polar bonds. We 're going to spend some time drawing lewis structures of certain organic
compounds but before we do let's talk about some common names of alkanes. alkanes are saturated
organic compounds meaning that the carbon atoms are filled with hydrogen atoms. methane is a
one carbon alkane it 's m e t h a n e a two carbon alkanes c two h six this is known as ethane C3H8
this is called propane C4 H10 this is butane.
Carbon likes to form four bonds so the only way this is going to happen is if we put a
double bond between the two carbon atoms. Alkenes contain at least one double bond and alkanes
do not contain double bonds. The length of the carbon-carbon single bond is 154 picometers which
is 1. 54 angstroms. A triple bond is stronger than a sigma bond or a pi bond but triple bonds are
stronger than single bonds. Bond order is the bond order for a single bond a double bond and a
triple bond. hybridization is the hybridization of the atoms that are connected to those bonds. How
you can determine the number of sigma and pi bonds in an organic compound feel free to pause
the video and try. The next topic of discussion is how to calculate the formal charge of an element
so we could say that it has a positive formal charge. The formal charge is equal to the valence
electrons of the element minus the bonds and dots attached to that element.
The formal charge of an element is going to be the number of valence electrons minus the
sum of the bonds and dots around that element. For nitrogen in the ammonium ion nitrogen has
five valence. electrons it's in group 5a of the periodic table in this structure it has four bonds no
dots so 5 minus four is one so this particular nitrogen atom has a plus one or a one plus formal
charge. i 'maintains that a lone pair represents a pair of non-bonding electrons that are only attached
to one atom. One lone pair is equal to two nonbonding electron in a bond and one bond equates to
Organic chemistry focuses on organic compounds. compounds that contain carbon atoms.
elements in the first group of the periodic table like hydrogen they like to form one bond. Beryllium
for example likes to form two bonds boron which has three valence electrons it likes to form three
bonds, carbon has four valence. electrons carbon likes to have four bonds. elements like fluorine
and the other halogens. chlorine ,bromine, iodine they like to form seven bonds.
A polarized object is an object that is neutral overall but has charge separation. that is one
side is positive and the other side is negative so this is a polar object the bond is polar because
fluorine carries a partial negative charge due to the fact that it 's more electronegative than carbon
so it pulls electrons toward itself. The carbon hydrogen bond that 's a nonpolar covalent bond is
non-polar bonds. We 're going to spend some time drawing lewis structures of certain organic
compounds but before we do let's talk about some common names of alkanes. alkanes are saturated
organic compounds meaning that the carbon atoms are filled with hydrogen atoms. methane is a
one carbon alkane it 's m e t h a n e a two carbon alkanes c two h six this is known as ethane C3H8
this is called propane C4 H10 this is butane.
Carbon likes to form four bonds so the only way this is going to happen is if we put a
double bond between the two carbon atoms. Alkenes contain at least one double bond and alkanes
do not contain double bonds. The length of the carbon-carbon single bond is 154 picometers which
is 1. 54 angstroms. A triple bond is stronger than a sigma bond or a pi bond but triple bonds are
stronger than single bonds. Bond order is the bond order for a single bond a double bond and a
triple bond. hybridization is the hybridization of the atoms that are connected to those bonds. How
you can determine the number of sigma and pi bonds in an organic compound feel free to pause
the video and try. The next topic of discussion is how to calculate the formal charge of an element
so we could say that it has a positive formal charge. The formal charge is equal to the valence
electrons of the element minus the bonds and dots attached to that element.
The formal charge of an element is going to be the number of valence electrons minus the
sum of the bonds and dots around that element. For nitrogen in the ammonium ion nitrogen has
five valence. electrons it's in group 5a of the periodic table in this structure it has four bonds no
dots so 5 minus four is one so this particular nitrogen atom has a plus one or a one plus formal
charge. i 'maintains that a lone pair represents a pair of non-bonding electrons that are only attached
to one atom. One lone pair is equal to two nonbonding electron in a bond and one bond equates to
