Polarity
• Alkanes are not polar, as there is no electronegativity between C-H bonds
• Alcohols and water are polar because they contain –OH bonds, with a difference in electronegativity
• The only force present in hydrocarbons are Van Der Waals
Reactivity
• Alkenes are more reactive than alkanes due to their double bonds which break in the reaction releasing more energy
• Alkanes are not reactive but can be combusted as fuels for engines.
Solubility
• Alkanes are non-polar and therefore do not mix and dissolve into polar liquids such as water. They are unable to form hydrogen bonds between each molecule. Water also has strong hydrogen bonds between each H2O molecule and therefore not want to move apart to allow for the alkane in
Boiling Points
• The increase in the chain of the atoms in an alkane, increases the boiling points as a result of there being more Van der Waal forces between each molecule. (A CH4 molecule has a boiling point of -161.5 °C, where are C10H22
Polarity
• Alkanes are not polar, as there is no electronegativity between C-H bonds
• Alcohols and water are polar because they contain –OH bonds, with a difference in electronegativity
• The only force present in hydrocarbons are Van Der Waals
Reactivity
• Alkenes are more reactive than alkanes due to their double bonds which break in the reaction releasing more energy
• Alkanes are not reactive but can be combusted as fuels for engines.
Solubility
• Alkanes are non-polar and therefore do not mix and dissolve into polar liquids such as water. They are unable to form hydrogen bonds between each molecule. Water also has strong hydrogen bonds between each H2O molecule and therefore not want to move apart to allow for the alkane in
Boiling Points
• The increase in the chain of the atoms in an alkane, increases the boiling points as a result of there being more Van der Waal forces between each molecule.
Polarity
• Alkanes are not polar, as there is no electronegativity between C-H bonds
• Alcohols and water are polar because they contain –OH bonds, with a difference in electronegativity
• The only force present in hydrocarbons are Van Der Waals
Reactivity
• Alkenes are more reactive than alkanes due to their double bonds which break in the reaction releasing more energy
• Alkanes are not reactive but can be combusted as fuels for engines.
Solubility
• Alkanes are non-polar and therefore do not mix and dissolve into polar liquids such as water. They are unable to form hydrogen bonds between each molecule. Water also has strong hydrogen bonds between each H2O molecule and therefore not want to move apart to allow for the alkane in
Name of Alkene |
Number of Carbons |
Chemical Formula |
Boiling Point in °C |
State at “Room Temperature” (20°C) |
Melting Point in °C |
Ethene |
2 |
C2H4 |
-104 |
gas |
-169 |
Propene |
3 |
C3H6 |
-47 |
gas |
-185 |
Z-Butene |
4 |
C4H8 |
0.9 |
gas |
-138.9 |
E-Butene |
4 |
C4H8 |
3.7 |
gas |
-139.7 |
1-Pentene |
5 |
C5H10 |
30 |
gas |
-165 |
Z-2-Pentene |
5 |
C5H10 |
36 |
gas |
-135 |
E-2-Pentene |
5 |
C5H10 |
37 |
gas |
-180 |
1-hexene |
6 |
C6H12 |
63 |
liquid |
−139.8 |
1-Heptene |
7 |
C7H14 |
115 |
liquid |
-119 |
3-octene |
8 |
C8H16 |
122 |
liquid |
-101.9 |
3-nonene |
9 |
C9H18 |
147 |
liquid |
-84.4 |
5-decene |
10 |
C10H20 |
170 |
liquid |
-66.3 |
Name of Alkane |
Number of Carbons |
Chemical Formula |
Boiling Point in °C |
State at “Room Temperature” (20°C) |
Melting Point in °C |
Methane |
1 |
C H4 |
-162 |
gas |
-183 |
Ethane |
2 |
C2H6 |
-89 |
gas |
-172 |
Propane |
3 |
C3H8 |
-42 |
gas |
-188 |
Butane |
4 |
C4H10 |
0 |
gas |
-138 |
Pentane |
5 |
C5H12 |
36 |
liquid |
-130 |
Hexane |
6 |
C6H14 |
69 |
liquid |
-95 |
Heptane |
7 |
C7H16 |
98 |
liquid |
-91 |
Octane |
8 |
C8H18 |
126 |
liquid |
-57 |
Nonane |
9 |
C9H20 |
151 |
liquid |
-54 |
Decane |
10 |
C10H22 |
174 |
liquid |
-30 |