Chapter 1-7 Review: Chemistry, Bonds, Reactions, and Body Materials

A set of 100 vocabulary-style flashcards covering atoms, bonds, reactions, electrolytes, organic/inorganic matter, bone anatomy, imaging contrast, and body pH-related concepts drawn from Chapter 1 through Chapter 7 notes.

Atom

The basic unit of matter composed of a nucleus (protons and neutrons) with electrons in orbit.

Proton

Positively charged subatomic particle located in the nucleus.

Neutron

Electrically neutral subatomic particle located in the nucleus.

Electron

Negatively charged subatomic particle that orbits the nucleus in an electron cloud.

Nucleus

Center of the atom containing protons and neutrons.

Electron cloud

Region around the nucleus where electrons are found.

Atomic number

Number of protons in the nucleus; defines the element.

Atomic mass

Sum of protons and neutrons in the nucleus.

Isotopes

Atoms of the same element with different numbers of neutrons.

Carbon-12

The most common carbon isotope (6 protons, 6 neutrons).

Carbon-14

Radioactive carbon isotope used in dating; unstable and radioactive.

Protium

Hydrogen-1 isotope with no neutrons.

Deuterium

Hydrogen-2 isotope with one neutron.

Tritium

Hydrogen-3 isotope with two neutrons.

Hydrogen ion

Proton; the positively charged form of hydrogen (H+).

Oxygen

One of the four major body elements; essential in many molecules.

Carbon

One of the four major body elements; basis of organic molecules.

Nitrogen

One of the four major body elements; key in amino acids and nucleic acids.

Four major body elements

Oxygen, carbon, hydrogen, and nitrogen make up about 95% of the body.

Electron shell

Energy levels around the nucleus where electrons reside.

Ionic bond

Bond formed by transfer of electrons; ions attract (e.g., Na+ and Cl− in NaCl).

Cation

Ion with a positive charge.

Anion

Ion with a negative charge.

Sodium chloride

Table salt; Na+ and Cl− held together by ionic bond.

Oxidation

Loss of an electron.

Reduction

Gain of an electron.

Covalent bond

Bond formed by sharing electrons between atoms.

Double covalent bond

Covalent bond where two electrons pairs are shared (e.g., O=O in O2).

Oxygen gas (O2)

Diatomic molecule with a double covalent bond.

Carbon dioxide (CO2)

Molecule with covalent bonds; example of a stable molecule like CO2.

Hydrogen bond

Weak bond based on polarity between molecules; important in water structure.

Water

Inorganic, universal solvent; ~70% of body weight; supports cohesion and reactions.

Surfactant

Substance that lowers surface tension in the lungs to keep airways open.

Cohesion

Water molecules sticking to each other due to hydrogen bonding.

Surface tension

Tendency of liquid surface to resist external force due to cohesive forces.

Hydrophilic

Water-loving; dissolves in water.

Hydrophobic

Water-fearing; resists dissolving in water.

Gadolinium

Contrast agent used in CT/MRI to improve visibility; can cause allergies.

Contrast agent

Substance used to enhance imaging by improving tissue visibility.

Ground bone

Bone prepared to view inorganic salts; organic components removed.

Decalcified bone

Bone prepared to reveal organic components like collagen and vessels.

Inorganic bone salts

Mineral salts present in bone; shown in ground bone.

Organic bone components

Collagen and living components in bone; shown in decalcified bone.

Osteocytes

Mature bone cells embedded in bone matrix.

Collagen

Organic protein matrix in bone; provides structure.

Blood vessels (in bone)

Vascular supply within bone tissue.

Nerves (in bone)

Nerve fibers present in bone tissue.

Inorganic salts

Mineral components that do not contain carbon-hydrogen bonds.

Electrolyte

Ions in body fluids that conduct electricity; essential for function.

Na+

Sodium ion with a positive charge.

K+

Potassium ion with a positive charge.

Cl−

Chloride ion with a negative charge.

Ca2+

Calcium ion with a 2+ charge.

Cation

Positively charged ion.

Anion

Negatively charged ion.

Salt

Ionic compound formed by cation and anion; dissociates in water.

Dissociation

Separation of ions in solution (e.g., salts in water).

Acid

Substance that releases H+ in solution.

Base

Substance that releases OH− or accepts H+ in solution.

Buffer

Weak acid or base that resists pH changes by accepting/ releasing H+.

pH

Measure of acidity or alkalinity of a solution.

Carbonic acid

Weak acid formed from CO2; part of blood buffering system.

Bicarbonate

Conjugate base form in buffering system; helps maintain pH.

Blood pH range

Healthy arterial pH approximately 7.35–7.45.

Urine pH range

Normal urine pH range about 4.5–8.

Stomach pH

Very acidic; typically ~1.5–3.5 to aid digestion.

Acidosis

Condition of excessive acidity (low pH) in body fluids.

Alkalosis

Condition of excessive basicity (high pH) in body fluids.

Glycolysis?

Not in notes; placeholder avoided.

Acid

Substance that donates protons or increases H+ concentration.

Base

Substance that donates OH− or accepts protons; increases pH.

Carbon dioxide sensing

Receptors in brain and aorta monitor CO2 levels to regulate respiration.

Carbonic acid–bicarbonate buffer

Primary buffering system in blood; shifts between carbonic acid and bicarbonate.

Dehydration synthesis

Reaction that builds molecules with release of a water molecule.

Hydrolysis

Reaction that breaks bonds by adding water.

Reactants

Substances input to a chemical reaction.

Products

Substances produced by a chemical reaction.

Enzyme

Biological catalyst that lowers activation energy of a reaction.

Activation energy

Energy required to start a chemical reaction.

Catalyst

Substance that speeds up a reaction without being consumed.

Synthesis

Building larger molecules from smaller ones (anabolism).

Decomposition

Breaking down large molecules into smaller ones (catabolism).

Anabolism

Metabolic pathways that build molecules (synthesis).

Catabolism

Metabolic pathways that break down molecules (decomposition).

Exchange reaction

Reaction that switches parts between molecules.

Exergonic

Reactions that release energy.

Endergonic

Reactions that consume energy.

Organic molecules

Carbon-based molecules (carbon-hydrogen bonds predominate).

Inorganic molecules

Molecules not primarily carbon-hydrogen-based.

Water as lubricant

Water provides lubrication in joints and tissues.

Water as cushion

Water cushions organs and protects tissues.

Heat sink

Water’s ability to distribute heat evenly across the body.

Universal solvent

Water’s ability to dissolve many substances easily.

Ground bone vs decalcified bone distinction

Ground bone shows inorganic salts; decalcified bone shows organic matrix and vessels.

Osteocytes

Mature bone cells present in bone tissue.

Vessels (bone)

Blood vessels that supply bone tissue.

Nerves (bone)

Nerves that run through bone tissue.

Bone salts

Inorganic mineral components that form bone structure.

Osteoblasts

Bone-forming cells (not explicitly named in notes but related to bone formation).

Osteoclasts

Bone-resorbing cells (not explicitly named in notes but related to bone remodeling).