BO101 Biochemistry of Life - Lecture 1: Chemistry of Life Flashcards

Vocabulary practice flashcards covering fundamental chemistry concepts from Lecture 1 of BO101 Biochemistry of Life.

Trace Elements

Essential chemical elements required by organisms in minute quantities (less than $0.01\%$ of body mass), such as iron ($\text{Fe}$) and zinc ($\text{Zn}$).

Electronegativity

The degree of attraction or 'pull' that an atom exerts on shared electrons within a chemical bond.

Non-polar Covalent Bond

A strong chemical bond formed when two atoms with equal electronegativity share electrons equally (e.g., $\text{H}_2$).

Polar Covalent Bond

A strong chemical bond formed when electrons are shared unequally due to differing electronegativity between atoms, generating partial positive ($\delta+$) and partial negative ($\delta-$) charges.

Ionic Bond

A non-covalent bond resulting from the complete transfer of one or more valence electrons from one atom to another, forming oppositely charged ions.

Cation

A positively charged ion formed when an atom gives up one or more electrons (e.g., $\text{Na}^+$).

Anion

A negatively charged ion formed when an atom gains one or more electrons (e.g., $\text{Cl}^-$).

Hydrogen Bond

A weak non-covalent interaction formed between a partial positive charge on a hydrogen atom of one molecule and a partial negative charge on an atom in another molecule.

Van der Waals Interactions

Weak non-covalent bonding interactions caused by transient dipoles, where temporary regions of positive and negative charge attract adjacent molecules.

Hydration Shell

A sphere of water molecules surrounding a dissolved ion or polar molecule, oriented according to partial electrical charges.

Acid

A substance that increases the hydrogen ion concentration of a solution by donating protons ($\text{H}^+$) in aqueous solutions.

Base

A substance that reduces the hydrogen ion concentration of a solution by accepting protons ($\text{H}^+$) or donating hydroxide ions ($\text{OH}^-$) in aqueous solutions.

pH Scale

A logarithmic measure of acidity and basicity ranging from $0$ to $14$, calculated as $\text{pH} = -\log[\text{H}^+]$.

Buffer

A chemical substance that minimizes changes in pH by accepting $\text{H}^+$ ions when they are in excess and donating $\text{H}^+$ ions when they are depleted.

Organic Chemistry

The scientific study of carbon-containing compounds and their structures, properties, and reactions.

Carbon Skeleton

The chain or ring framework of carbon atoms that forms the structural foundation of organic biomolecules.

Enantiomers

Isomers that are non-superimposable mirror images of each other due to differing spatial arrangements around an asymmetric carbon atom.

Functional Groups

Specific chemical arrangements decorated on carbon skeletons that participate in biological interactions and determine molecular properties.

Estradiol and Testosterone

Steroid sex hormones that share a common carbon skeleton but differ in attached functional groups, leading to distinct biological functions.

Double Bond

A covalent bond formed when two atoms share two pairs of valence electrons (4 electrons total), such as in $\text{O}_2$ or ethene ($\text{C}_2\text{H}_4$).