properties of alkanes

• alkanes bonds are non polar because carbon and hydrogen have similar electronegativity
• shape and angle of an alkane is tetrahedral 109.5 degrees
• sigma bond is a covalent bond which has a direct overlap of electron clouds of the bonding atoms
• alkanes have London forces -> induced dipole-dipole interaction, because bonds are non-polar
• boiling point increasees as alkane chain length increases because more surface area + so more number of induced dipole-dipole interaction

  -> therefore more energy required to overcome the attraction
• branched molecules have lower boiling points because they have fewer surface area + hence less induced dipole-dipole interactions
• alkanes are insoluble in water because hydrogen bonds in water are stronger than alkanes' London forces of attraction