Alkanes and Alkenes

• Alkanes are hydrocarbons that consist entirely of single-bonded carbon and hydrogen atoms.
• Organic compounds can involve covalent bonding, ionic bonding, or a combination of both.
• Carbon atoms can bond together to form very long, durable chains.
• Carbon atoms can form strong bonds, sealed off by hydrogen atoms.
• Carbon atoms can bond with many different elements.
• Alkanes are saturated hydrocarbons that consist of C and H atoms.
• Alkanes can be represented by the formula CnHz + 2.
• The longest possible chain is represented as CH-2H-CH-CH-CH-CH=GCs.
• The chain can be identified and named by attaching groups to this chain.
• The chain can be started at any point.
• Alkanes can be represented by structural formulas, which show how the atoms are bonded together.
• The general formula for alkanes is CnH2n+2, where n represents the number of carbons in the molecule.
• Alkenes are unsaturated hydrocarbons that contain at least one carbon-to-carbon double bond.
• Alkanes are saturated hydrocarbons that contain only single bonds between carbon atoms.
• Alkenes are unsaturated hydrocarbons with one or more double bonds between carbon atoms.
• Alkanes are named using the prefixes meth-, eth-, prop-, but-, pent-, hex-, hept-, oct-, non-, dec-, undec-, dodec-, tridec-, tetradec-, pentadec-, and hexadec-. The suffix -ane indicates an alkane.
• Alkenes are named using the suffix "-ene" and their common names include ethene (C2H4), propene (C3H6), butene (C4H8), pentene (C5H10), hexene (C6H12), heptene (C7H14), octene (C8H16), nonene (C9H20), decene (C10H22).
• Intermolecular forces, also known as Van der Waals forces, are attractive forces between molecules.
• Hydrocarbons, although typically non-polar, experience temporary fluctuations in electron distribution that create temporary dipoles, leading to another molecule being attracted, a process known as dipole-dipole.
• In the context of hydrocarbons, such as alkanes, which consist of carbon and hydrogen, the length of carbon chains is relevant due to increased surface area.
• The bigger the surface area, the greater the force.
• Alkenes have names ending in "-ene".
• Alkenes with multiple double bonds are numbered starting from the end closest to the first double bond.