Video: Carbon, Isomers, and Functional Groups - Vocabulary Flashcards

Vocabulary flashcards covering carbon chemistry, isomers, and functional groups from the lecture.

Carbon

Element with atomic number 6; forms four covalent bonds; central to organic molecules; bonding is typically tetrahedral.

Atomic number

Number of protons in an atom's nucleus; equals the number of electrons in a neutral atom.

Electron shell

Regions around the nucleus where electrons reside; first shell holds 2 electrons, second shell holds more (up to 8).

1s orbital

The lowest-energy orbital in the first electron shell; holds up to 2 electrons.

2s orbital

The s orbital in the second electron shell.

2p orbitals

Three degenerate p orbitals in the second shell that accommodate electrons for bonding.

Hybridization

Mixing of atomic orbitals to form new, equivalent orbitals for bonding.

sp3

Hybridization producing four equivalent orbitals arranged tetrahedrally; enables four covalent bonds.

Tetrahedral

Geometry with four electron groups around a central atom; common for carbon bonding.

Valence

Number of covalent bonds an atom tends to form; carbon valence is four.

Covalent bond

Bond formed by sharing electrons between atoms.

Molecule

Two or more atoms held together by covalent bonds.

Isomer

Compound with the same molecular formula but different three-dimensional arrangement.

Structural isomer

Isomers with different covalent partnerships between atoms.

Cis-trans isomer

Geometric isomer; differs in arrangement around a carbon–carbon double bond.

Enantiomer

Non-superimposable mirror-image isomer.

Asymmetric carbon

Carbon attached to four different substituents; center of chirality.

Hydrophobic

Water-fearing; nonpolar substances that do not dissolve well in water.

Hydrocarbon

Molecule composed only of carbon and hydrogen; typically nonpolar.

Nonpolar

Lack of significant partial charges; weak interactions with water.

Functional group

Atoms or groups attached to a carbon skeleton that participate in chemical reactions.

Hydroxyl group

-OH group; polar; common in alcohols; increases water solubility.

Carbonyl group

C=O; polar; end of chain aldehydes or interior ketones.

Aldehyde

Carbonyl group at the end of a carbon chain.

Ketone

Carbonyl group within a carbon skeleton.

Carboxyl group

-COOH; carbonyl with hydroxyl; acidic; present in carboxylic acids.

Carboxylic acid

Organic acids containing a carboxyl group; donate H+ in solution.

Amino group

-NH2; acts as a base by accepting H+ to form NH3+ in solution.

Amine

Organic compound containing an amino group.

Sulfhydryl group

-SH group; thiols; can form cross-links (disulfide bonds) stabilizing proteins.

Thiol

Alternative name for sulfhydryl group.

Phosphate group

Phosphorus bonded to four oxygens; two negative; high-energy; transfers energy between molecules.

ATP

Adenosine triphosphate; energy currency of the cell; carries three phosphate groups.

Methyl group

-CH3 group; nonpolar; methylation can affect gene activity.

Methylation

Addition of a methyl group to DNA or molecules; influences gene expression.

Polar

Molecules with uneven electron distribution; possess partial charges.

Electronegativity

Attractiveness of an atom for electrons in a covalent bond.

Water solubility

Ability of a substance to dissolve in water; increased by polar groups.

Proton/Hydrogen ion

H+; involved in acid-base chemistry; leaves a molecule upon ionization.

Acid

Substance that donates H+ in solution; carboxyl groups contribute acidity.

Base

Substance that accepts H+; amino groups act as bases (form NH3+ in solution).

Biomolecule

Large organic molecule such as lipids, carbohydrates, nucleic acids, or proteins.

Lipids

Hydrophobic biological molecules; fats and oils; mainly nonpolar.

Carbohydrates

Sugars and polymers; sources of energy and structural components.

Nucleic acids

DNA and RNA; store, transmit, and express genetic information.

Proteins

Polymers of amino acids; perform most cellular functions and catalysis.

Disulfide bond

Covalent bond between two thiol groups that stabilizes protein structure.

Chirality

Property of a molecule having a non-superimposable mirror image.

Ring

Cyclic carbon skeleton; atoms connected to form a closed loop.

Branched

Carbon skeleton with side chains; increases structural diversity.

Methane

CH4; simplest hydrocarbon; tetrahedral geometry around carbon.

Ethane

C2H6; two carbons single-bonded with each carbon bonded to three hydrogens.

Ethene

C2H4; carbon–carbon double bond; planar; leads to cis-trans variability.

Molecular formula

Notation showing the number and types of atoms in a molecule.

Geometric isomer

Isomers differing in arrangement around a double bond (includes cis/trans).

Disulfide bridge

Bond between two thiol groups in proteins, stabilizing 3D structure.

Enzyme relation to chirality

Enantiomeric form can affect binding to a protein receptor or active site.

Renewable plastic concept

Biotechnological aim to make plastic from renewable sources using microbial pathways.

Covalent partnerships

Which atoms are bonded to which in a molecule; determines structural isomer type.

Molecule vs atom

A molecule is a group of atoms bonded together; an atom is a single element.

Isomer criteria

Same molecular formula and different three-dimensional shapes.

Covalent partnerships distinction

Structural isomers differ in which atoms are covalently bonded to what.

Geometric vs structural isomers

Geometric (cis-trans) differ around a double bond; structural differ in connectivity.

Functional group importance

Functional groups determine reactivity, solubility, and overall molecule behavior.

Steric arrangement around C

Positioning of substituents around a carbon center affects reactivity and recognition.

Molecule orientation

How a molecule is arranged in space, affecting interactions with enzymes or receptors.