Video Notes: Biochemistry & General Chemistry Concepts (Vocabulary Flashcards)

A comprehensive set of vocabulary flashcards covering matter, atoms, chemical bonds, energy, organic/inorganic compounds, acids/bases, pH, buffers, biomolecules, and nucleic acids as presented in the video notes.

Matter

Anything that has mass and occupies space.

States of matter

The three forms: solid, liquid, and gas.

Solid

A state of matter with definite shape and volume.

Liquid

A state of matter with definite volume but no fixed shape.

Gas

A state of matter with no definite shape or volume; fills the space available.

Chemistry

The science that studies matter and its interactions.

Element

A pure substance composed of one type of atom; cannot be broken down by ordinary chemical methods.

Atom

The basic unit of matter; the smallest unit of an element that retains its properties, made of protons, neutrons, and electrons.

Proton

Positively charged subatomic particle in the nucleus.

Neutron

Electrically neutral subatomic particle in the nucleus.

Electron

Negatively charged subatomic particle orbiting the nucleus.

Hydrogen (H)

Element with 1 proton and 1 electron (common isotope has 0 neutrons).

Helium (He)

Element with 2 protons, 2 neutrons, and 2 electrons.

Lithium (Li)

Element with 3 protons, 4 neutrons, and 3 electrons.

CH4

Methane; molecule consisting of one carbon atom bonded to four hydrogen atoms.

Molecule

Two or more atoms bonded together; in this context often formed from atoms of the same element.

Compound

Substance formed when two or more atoms from different elements bond.

Chemical bonds

Energy-based attractions holding atoms together.

Ionic bond

Bond formed when electrons are transferred from one atom to another.

Covalent bond

Bond formed when electrons are shared between atoms.

Nonpolar covalent bond

Covalent bond in which electrons are shared equally, producing no significant charge separation.

Polar covalent bond

Covalent bond with unequal sharing of electrons, creating partial charges.

Hydrogen bond

Weak attraction between a partially positive hydrogen and a partially negative atom.

Ion

Atom with a net electric charge due to gain or loss of electrons.

Cation

Positively charged ion; formed when a metal loses electrons.

Anion

Negatively charged ion; formed when a nonmetal gains electrons.

Salt

Ionic compound formed by the attraction between cations and anions.

Valence electron

Electron in the outermost electron shell involved in bonding.

Sodium (Na)

Element with atomic number 11; typically donates its lone valence electron in bonding.

Chlorine (Cl)

Element with atomic number 17; commonly gains an electron to form Cl−.

Sodium cation (Na+)

Na+ formed after donating one electron.

Chloride anion (Cl-)

Cl− formed after gaining one electron.

Sodium chloride (NaCl)

Ionic compound formed by Na+ and Cl− (table salt).

Reactants

Starting substances on the left side of a chemical equation.

Products

Substances produced on the right side of a chemical equation.

Chemical reaction

Process involving the formation, breaking, or rearrangement of bonds or transfer of electrons.

Chemical notation

System of symbols and abbreviations used to describe a chemical reaction.

Carbonic acid (H2CO3)

Product formed when CO2 reacts with water.

Potential energy

Stored energy due to position; can be released to do work later.

Kinetic energy

Energy of motion; energy possessed by moving objects.

Energy

Capacity to do work or cause change; includes potential and kinetic forms.

Chemical energy

Energy stored in chemical bonds.

Synthesis

Chemical reaction where smaller substances combine to form a larger, more complex substance.

Decomposition

Chemical reaction where a compound breaks down into simpler substances.

Exchange

Chemical reaction where parts of two molecules swap places.

Redox

Oxidation-reduction reaction; transfer of electrons between species.

Inorganic compound

Compound that does not contain carbon (generally, with some exceptions).

Organic compound

Compound that contains carbon.

Acid

Substance that releases hydrogen ions (H+); a proton donor.

Base

Substance that accepts hydrogen ions; a proton acceptor.

pH

Measurement of the hydrogen ion concentration, ranging from 0 to 14.

Hydrogen ion (H+)

Proton; the positively charged part of an acid.

Neutral solution

pH 7; [H+] = [OH−].

Acidic solution

pH < 7; higher [H+] than [OH−].

Basic/alkaline solution

pH > 7; higher [OH−] than [H+].

Coffee (pH 5.0)

Example of an acidic solution.

Lemon juice (pH ~2)

Very acidic solution.

Urine (pH 5–8)

Range from slightly acidic to slightly basic.

Distilled water (pH 7)

Neutral solution.

Seawater (pH ~8.4)

Slightly basic solution.

Blood (pH ~7.4)

Slightly basic; normally tightly regulated.

Household ammonia (pH ~11.5–11.9)

Strongly basic solution.

Oven cleaner (pH ~13.5)

Very strongly basic solution.

Buffer

Substance that resists changes in pH by releasing or absorbing H+.

Bicarbonate buffer system

Buffer system in blood helping maintain stable pH.

Biochemistry

Study of chemical processes within and related to living organisms.

Inorganic compound

Compound that does not contain carbon.

Organic compound

Compound that contains carbon.

Carbohydrates

Sugars and starches; C:H:O in about a 1:2:1 ratio; e.g., glucose (C6H12O6).

Lipids

Hydrophobic molecules including neutral fats, phospholipids, and steroids.

Proteins

Macromolecules that function as enzymes, structural components, in movement, defense, and as fuel.

Nucleic acids

Biomolecules (DNA and RNA) that store and transfer genetic information.

Monosaccharide

Simple sugar (e.g., glucose, fructose, galactose).

Disaccharide

Two monosaccharides linked; e.g., sucrose, maltose, lactose.

Polysaccharide

Many monosaccharides linked together (e.g., starch).

Dehydration synthesis

Process that joins monomers with removal of water.

Hydrolysis

Chemical breakdown of a compound by reaction with water.

Glucose

Monosaccharide with formula C6H12O6; main energy source for cells.

Fructose

Monosaccharide found in fruits; isomer of glucose.

Galactose

Monosaccharide; part of lactose in milk.

Sucrose

Disaccharide composed of glucose and fructose.

Maltose

Disaccharide composed of two glucose units.

Lactose

Disaccharide composed of glucose and galactose.

Lipids (overview)

Hydrophobic biomolecules including triglycerides, phospholipids, and steroids.

Amino acids

Building blocks of proteins; linked by peptide bonds.

Peptide bond

Bond linking amino acids in a protein.

Denaturation

Alteration of a protein’s shape and function due to environmental changes.

Nucleic acids

Biomolecules (DNA and RNA) made of nucleotides.

Nucleotides

Nucleic acid subunits containing a nitrogenous base, sugar, and phosphate.

Purines

Double-ring bases: adenine (A) and guanine (G).

Pyrimidines

Single-ring bases: cytosine (C), uracil (RNA), thymine (DNA).

DNA (deoxyribonucleic acid)

Double-stranded molecule that stores genetic information.

RNA (ribonucleic acid)

Single-stranded molecule involved in protein synthesis; uses uracil instead of thymine.

Adenine

Purine base; pairs with thymine in DNA and with uracil in RNA.

Guanine

Purine base; pairs with cytosine.

Cytosine

Pyrimidine base; pairs with guanine.

Thymine

Pyrimidine base in DNA; pairs with adenine.

Uracil

Pyrimidine base in RNA; pairs with adenine.

Sugar-phosphate backbone

The alternating sugar and phosphate groups forming the structural framework of DNA and RNA.

Double helix

Two long DNA strands twisted around each other.