Chemistry Unit 4 AOS 1

Organic Compounds

Carbon-based compounds with diverse structures and functions.

Molecular Formula

Shows number and type of atoms in a compound.

Structural Formula

Illustrates the arrangement of atoms in a molecule.

Skeletal Formula

Simplified representation of organic compounds.

Isomers

Compounds with the same formula but different structures.

Hydrocarbons

Compounds consisting only of carbon and hydrogen.

Alkanes

Saturated hydrocarbons with single carbon bonds.

Alkenes

Unsaturated hydrocarbons with at least one double bond.

Cyclohexane

Cyclic alkane with six carbon atoms.

Degree of Unsaturation

Indicates number of rings and double bonds present.

Haloalkanes

Alkanes with halogen substituents like F, Cl, Br, I.

Alcohols

Organic compounds with hydroxyl (-OH) functional group.

Primary Alcohols

One alkyl group attached to carbon with -OH.

Secondary Alcohols

Two alkyl groups attached to carbon with -OH.

Tertiary Alcohols

Three alkyl groups attached to carbon with -OH.

Carbonyl Group

Functional group with a carbon double-bonded to oxygen.

Aldehydes

Contain carbonyl (CHO) group at the end of the molecule.

Ketones

Contain carbonyl (CO) group not at the end of the molecule.

Carboxylic Acids

Contain carboxyl group (-COOH) at the end.

Esters

Formed from reaction of alcohol and carboxylic acid.

Primary Amines

Contain amino group (-NH2) attached to carbon.

Condensation Reaction

Reaction that produces water as a byproduct.

Hydrolysis

Splitting molecules using water, often enzyme-catalyzed.

Atom Economy

Percentage of reactant atoms in desired product.

Percentage Yield

(Actual yield/Theoretical yield) x 100.

Intermolecular Forces

Forces between molecules affecting physical properties.

Dispersion Forces

Weakest intermolecular forces present in all compounds.

Dipole-Dipole Forces

Attractive forces between polar molecules.

Hydrogen Bonds

Strong bonds between H and O, N, or F.

Polypeptides

Chains of amino acids linked by peptide bonds.

Dipeptides

Formed from two amino acids via condensation.

Monosaccharides definition

Simplest carbohydrates, e.g., glucose, fructose.

Disaccharides definition

Two monosaccharides linked by glycosidic bond.

Polysaccharides definition

Long chains of monosaccharides, e.g., starch, cellulose.

Saturated Fatty Acids

Only single carbon-carbon bonds in hydrocarbon chain.

Unsaturated Fatty Acids

Contain one or more double bonds in hydrocarbon chain.

Boiling point

temperature at which a substance changes from a liquid to a

gas at a specific pressure.

how does Molecular Size influence boiling point

makes a higher boiling points because they have a greater number of electrons, leading to stronger van der Waals forces between molecules

how does molecular mass influence boiling point

Heavier molecules with greater mass typically have

higher boiling points due to the increased number of electrons and stronger London dispersion forces.

how does hydrogen bonding influence boiling point

Molecules capable of forming hydrogen bonds,

typically those with -OH, -NH2, or -COOH groups, have significantly higher boiling points because of the strong hydrogen bonds between molecules

how does polarity influence boiling point

Polar molecules with permanent dipoles, such as those containing electronegative atoms, have higher boiling points

due to stronger dipole-dipole interactions

viscosity

the resistance of a liquid to flow

how does molecular size and shape influence viscosity

Larger and more complex molecules tend to

have higher viscosities because they have more extensive molecular interactions. Highly branched or irregularly shaped molecules may have

lower viscosities.

how does polarity influence viscosity

Polar molecules exhibit higher viscosities compared to non polar molecules of similar size due to stronger intermolecular forces.

how does temperature influence viscosity

Viscosity generally decreases with increasing temperature because higher temperatures provide molecules with more kinetic energy to

overcome intermolecular forces, making the liquid flow more easily.

flashpoint

the lowest temperature at which a substance's vapour can ignite when exposed to an open flame or spark.

how does volatility influence flashpoint

Highly volatile compounds with low boiling points tend to have lower flashpoints because they can vaporise easily.

how does chemical structure influence flashpoint

Some functional groups, such as alkyl groups (-CH3), can lower flashpoints because they promote vaporisation. Conversely, polar

or functional groups may increase flashpoints.

how does ignition sources influence flashpoint

The presence of ignition sources, such as open flames or sparks, can lower the effective flashpoint of a substance by providing the

necessary energy for ignition.

esterfication reaction

carboxylic acid + alcohol --> ester + water

addition reaction

a chemical reaction in which two or more substances combine to form a new compound (c=c)

substitution reaction

a reaction in which one or more atoms replace another atom or group of atoms in a molecule (c-c)

hydrolysis reaction

water is used to break down a polymer (protein)

condensation reaction

monomers join to form polymers (proteins) and water molecules are also formed

oxidation reaction

a reactant loses one or more electrons, thus becoming more positive in charge (Cr2O7 or MnO4)

examples of monosaccharides

glucose, fructose galactose (C612O6)

Disaccharides

carbohydrates formed from the reaction of two monosaccharides via a condensation reaction between the hydroxyl groups forming an ether

Polysaccharides

generally insoluble in water and have no taste

Triglycerides

made from a condensation reaction between a glycerol molecule and three fatty acids

Polyunsaturated fatty acids

a type of fat characterized by having two or more carbon-carbon double bonds in their chemical structure

how does chain length influence solubility

As the length of the hydrocarbon chain increases, the non-polar hydrocarbon part of the molecule starts to become more important and the solubility decreases.

how does pressure affect solubility

As you increase the pressure of a gas, the collision frequency increases and thus the solubility goes up, as you decrease the pressure, the solubility goes down

how does temperature affect solubility

According to Le Chatelier's Principle, the system adjusts to this increase in the heat by promoting the dissolution reaction to absorb the added heat energy. Increasing the temperature, therefore, increases the solubility of the solute.

how to test for a carbon to carbon double bond

Add bromine or iodine. The double bond is broken and there is an addition reaction

how to test for carboxylic acids

litmus paper, add alcohol, add a base, universal indicator

general formula for making esters

RCOOH (aq) + ROH (l) -> RCOOR(l) + H2O(l)