IOC Lab and Lec (1)

Organic Chemistry

The branch of science that studies naturally occurring compounds derived from living and non-living things.

Inorganic Chemistry

The branch of science that studies compounds that do not contain carbon atoms.

Organic Compounds

Compounds that contain carbon atoms and are derived from living organisms.

Inorganic Compounds

Compounds that do not contain carbon atoms and are obtained from natural processes or human experiments.

Carbon-Hydrogen Bond

A bond between a carbon atom and a hydrogen atom, commonly found in organic compounds.

Covalent Bond

A type of chemical bond formed by the sharing of electrons between atoms, commonly found in organic compounds.

Ionic Bond

A type of chemical bond formed by the transfer of electrons between atoms, commonly found in inorganic compounds.

Volatility

The tendency of a substance to vaporize or evaporate.

Inflammable

Capable of catching fire and burning easily.

Solubility

The ability of a substance to dissolve in a solvent.

Conductivity

The ability of a substance to conduct heat or electricity.

Hydrocarbons

Organic compounds composed of only carbon and hydrogen atoms.

Functional Groups

Specific groups of atoms in a molecule that impart specific chemical and physical properties to the molecule.

Saturated Hydrocarbons

Hydrocarbons that contain only single bonds between carbon atoms.

Unsaturated Hydrocarbons

Hydrocarbons that contain double or triple bonds between carbon atoms.

Aromatics

Hydrocarbons that contain one or more benzene rings.

Chlorinated Hydrocarbons

Hydrocarbons in which one or more hydrogen atoms are replaced by chlorine atoms.

CFCs

Chlorofluorocarbons, a subfamily of chlorinated hydrocarbons that were banned due to their role in ozone destruction.

Alcohols

Organic compounds that contain the -OH functional group.

Aldehydes

Organic compounds that contain the carbonyl group (C=O) at the end of a carbon chain.

Ketones

Organic compounds that contain the carbonyl group (C=O) within the carbon chain.

Carboxylic Acids

Organic compounds that contain the carboxyl group (COOH).

Ester

Organic compounds that contain the ester functional group (RCOOR).

Ethers

Organic compounds that contain the ether functional group (ROR).

Amines

Organic compounds that contain the amino functional group (NH2).

Gen Formula

NR3:A general formula representing a compound that contains nitrogen and has three R groups attached to it.

Odor

A property of a substance that can be perceived by the sense of smell.

R groups

Organic groups or substituents that are attached to a molecule.

-amine

A suffix used to name compounds that contain an amino group (NH2).

Atomic Orbital

A region of space around the nucleus where an electron is most likely to be found.

s-orbital

An atomic orbital with a spherical shape that can hold a maximum of 2 electrons.

p-orbital

An atomic orbital with a dumbbell shape that can hold a maximum of 6 electrons.

d-orbital

An atomic orbital with a clover leaf shape that can hold a maximum of 10 electrons.

f-orbital

An atomic orbital with a double clover leaf shape that can hold a maximum of 14 electrons.

Electron configuration

The arrangement of electrons in an atom or molecule, represented by a series of numbers and letters indicating the energy levels and sublevels occupied by the electrons.

Valence Electron

An electron in the outermost energy level of an atom.

Core electrons

Electrons in the inner energy levels of an atom.

Covalent Bond

A chemical bond formed by the sharing of electron pairs between atoms.

Lewis Dot Structure

A representation of the valence electrons of an atom using dots around the atomic symbol.

Sigma (σ) bond

A covalent bond formed by the overlap of atomic orbitals along the internuclear axis.

Pi (π) bond

A covalent bond formed by the overlap of atomic orbitals above and below the internuclear axis.

Formal charge

The difference between the number of valence electrons an atom contributes to a molecule and its typical valence.

Main Group Elements

Elements in groups 1, 2, and 13-18 of the periodic table.

Transition Metals

Elements in groups 3-12 of the periodic table that have partially filled d orbitals in addition to their valence electrons.

Noble Gases

Elements in group 18 of the periodic table that have full valence electron shells and are chemically inert.

Octet Rule

The tendency of atoms to gain, lose, or share electrons in order to achieve a stable electron configuration with 8 valence electrons.

Molecular Orbital Theory

A theory that describes the behavior of electrons in entire molecules using molecular orbitals formed by the combination of atomic orbitals.

Hybridization Theory

A theory that explains the formation of molecular orbitals through the mixing of atomic orbitals.

Hydrocarbons

Organic compounds composed of hydrogen and carbon atoms.

Alkanes

Hydrocarbons with single bonds between carbon atoms.

Alkenes

Hydrocarbons with double bonds between carbon atoms.

Alkynes

Hydrocarbons with triple bonds between carbon atoms.

Propyne

C3H4

Butyne

C4H6

Hexyne

C6H10

Heptyne

C7H12

Octyne

C8H14

Nonyne

C9H16

Decayne

C10H18

Condensed Formula

A formula that shows the atoms and their connectivity in a molecule without explicitly showing all the bonds.

Acyclic or Open Chain Compounds

Organic compounds with branched or straight chain structures.

Alicyclic or Closed Chain or Ring Compounds

Homocyclic compounds that contain carbon atoms connected to each other in a ring.

Aromatic Compounds

Compounds that contain benzene or other ring-related compounds.

Alkyl Halides

Organic compounds with a halogen atom bonded to an alkyl group.

Aryl Halides

Organic compounds with a halogen atom bonded to an aryl group.

Primary Alkyl Halide

Alkyl halide with one carbon group attached to a C-X bond.

Secondary Alkyl Halide

Alkyl halide with two carbon groups attached to a C-X bond.

Tertiary Alkyl Halide

Alkyl halide with three carbon groups attached to a C-X bond.

Carbon-Halogen Bond

The bond between carbon and a halogen atom in alkyl halides.

Polarizability

The ease with which the electron distribution around an atom is distorted by a nearby electric field.

Solubility

The ability of a substance to dissolve in a solvent.

Density

The mass per unit volume of a substance.

Alcohols

Compounds containing the hydroxyl (–OH) functional group bonded to an alkyl group.

Primary Alcohol

Alcohol with the hydroxyl group bonded to a primary carbon.

Secondary Alcohol

Alcohol with the hydroxyl group bonded to a secondary carbon.

Tertiary Alcohol

Alcohol with the hydroxyl group bonded to a tertiary carbon.

Fermentation

The process of converting sugars and starches into alcohol, catalyzed by the enzyme zymase found in yeast.

Zymase

An enzyme found in yeast that catalyzes the fermentation of sugars and starches into alcohol.

Primary alcohols

Alcohols that can be oxidized to aldehydes.

Secondary alcohols

Alcohols that can be oxidized to ketones.

Tertiary alcohols

Alcohols that are resistant to oxidation due to the absence of an alpha hydrogen.

Chromic acid test

A test used to distinguish between primary, secondary, and tertiary alcohols based on their oxidation reactions.

Lucas test

A test used to distinguish between primary, secondary, and tertiary alcohols based on the formation of an immiscible upper layer of alkyl chloride.

SN1 mechanism

The reaction mechanism involved in the oxidation of tertiary and secondary alcohols.

Monohydroxy alcohols

Alcohols with one hydroxyl (OH) group.

Polyhydroxy alcohols

Alcohols with multiple hydroxyl (OH) groups.

Glycerol

A polyhydroxy alcohol used as a moisturizing agent in cosmetics, tobacco products, and food.

Acrolein test

A test used to detect the presence of glycerol by its dehydration to form propenal (acrolein).

Physical properties of alcohols

The properties of alcohols determined by intermolecular forces, such as hydrogen bonding.

Boiling point

The temperature at which a liquid changes into a gas.

Molar mass

The mass of one mole of a substance.

Hydrogen bonding

The attractive force between the hydrogen atom of one molecule and the oxygen, nitrogen, or fluorine atom of another molecule.

Solubility

The ability of a substance to dissolve in a solvent.

Hydration

The addition of water to a compound.

Methanol

A toxic alcohol used as a solvent and automotive fuel.

Ethanol

The alcohol found in alcoholic beverages, produced by the hydration of ethylene.

Isopropyl alcohol

A rubbing alcohol used as a disinfectant, produced by the addition of water to propene.

Toxicity

The degree to which a substance can cause harm to living organisms.

Dehydration

The removal of water from a compound.

Alkene

A hydrocarbon with a carbon-carbon double bond.