Biological Systems and Chemical Bonds

These flashcards cover essential vocabulary related to biological systems and chemical bonds, crucial for understanding concepts in biology.

DNA

Deoxyribonucleic Acid, a molecule that carries genetic instructions.

RNA

Ribonucleic Acid, involved in protein synthesis and gene expression.

Protein

Molecules made up of amino acids, important for structure and function in living organisms.

Periodic Table

A table organizing all known chemical elements based on their properties.

Biological System

A complex network of biologically relevant entities encompassing living organisms and their interactions.

Chemical Bonds

Forces that hold atoms together in molecules; include covalent and ionic bonds.

Covalent Bond

A strong bond formed when two atoms share electrons.

Ionic Bond

A bond formed through the transfer of electrons from one atom to another, resulting in charged ions.

Hydrogen Bond

A weak bond between a hydrogen atom and an electronegative atom.

Electronegativity

The ability of an atom to attract electrons toward itself.

Hydrophilic

Substances that can interact with or dissolve in water.

Hydrophobic

Substances that do not interact with water or are repellent to it.

Homeostasis

The maintenance of stable internal conditions in a living organism.

Molecule

Two or more atoms bonded together, representing the smallest fundamental unit of a chemical compound.

Macromolecule

Large complex molecules, including proteins, nucleic acids, carbohydrates, and lipids.

Amphipathic

Molecules that possess both hydrophilic and hydrophobic regions.

Capillary Action

The ability of water to flow in narrow spaces without external forces, due to its cohesive and adhesive properties.

Polarity

A property of molecules that have a partial positive charge on one side and a partial negative charge on the other.

Sodium Chloride (NaCl)

An ionic compound formed from sodium and chloride ions.

Stable Conformation

The arrangement of atoms in a molecule that has the lowest potential energy.

Valence Electrons

Electrons in the outermost shell of an atom that are involved in forming bonds.

Octet Rule

A principle stating that atoms tend to bond in a way that gives them eight electrons in their valence shell.

Bond Strength

A measure of how much energy is required to break a bond between two atoms.

Low Energy State

A state where energy is minimized, making the system more stable.

Intermolecular Forces

Forces that exist between molecules, including hydrogen bonds, dipole-dipole interactions, and Van der Waals forces.

Carbon Compounds

Organic molecules that contain carbon and are fundamental to life.

Biological Macromolecules

Large molecules necessary for life, including carbohydrates, lipids, proteins, and nucleic acids.

Electrolytes

Ionic substances that dissociate into ions in solution and can conduct electricity.

Negative Ion

An anion, which has gained one or more electrons, acquiring a negative charge.

Positive Ion

A cation, which has lost one or more electrons, acquiring a positive charge.

Half-life

The time taken for the radioactivity of a specified isotope to fall to half its original value.

Catalyst

A substance that increases the rate of a chemical reaction without undergoing permanent change.

Entropy

A measure of disorder or randomness in a system.

Biochemical Reactions

Chemical reactions that occur within living organisms to maintain life processes.

Thermodynamics

The study of energy transformations that occur in a collection of matter.

vaan der Waal’s Forces

Electrostatic interactions between atoms that have a temporary partial charge.