RTH 305 Chemistry Principles

Flashcards covering fundamental chemistry principles, gas laws, solutions, acid-base balance, and respiratory care applications from the RTH 305 study guide.

Matter

Anything that occupies space and has mass; it is classified as either an element or a compound.

Element

A pure substance containing only one type of atom that cannot be broken down into two or more substances.

Compound

A substance composed of two or more elements combined in a fixed ratio, such as $\text{NaCl}$ ($1:1$) or $\text{CaCl}_2$ ($1:2$).

Proton

A subatomic particle located in the nucleus with a $+1$ electrical charge.

Neutron

A subatomic particle located in the nucleus that carries no electrical charge.

Electron

A subatomic particle with a $-1$ charge, located in orbital shells surrounding the nucleus.

Isotope

Atoms of the same element that have the same number of protons but different numbers of neutrons (different mass numbers).

Technetium-99

A radioactive isotope used clinically as a tracer in medical diagnostics, such as in V/Q scans.

Electron Shell Capacity ($2n^2$)

The formula used to determine the maximum number of electrons in shell $n$, yielding $2$ in shell 1, $8$ in shell 2, $18$ in shell 3, and $32$ in shell 4.

Valence Electrons

Electrons located in the outermost shell that play a major role in elemental bond formation and molecular composition.

Cation

A positively charged ion formed when an atom has more protons than electrons.

Anion

A negatively charged ion formed when an atom has more electrons than protons.

Ionic Bond

A type of chemical bond that involves the transfer of electrons between atoms.

Covalent Bond

A type of chemical bond that involves the sharing of electrons between atoms.

Polar Covalent Bond

A covalent bond where electrons are shared unequally, producing a separation of charge or dipole.

Hydrogen Bond

A weak bond produced by the dipolar nature of molecules, such as the attractions between water molecules.

Chemical Equilibrium

The point in a reversible reaction where the forward reaction rate equals the reverse reaction rate and reactant/product concentrations no longer change.

Solid

A state of matter where molecules vibrate in fixed positions, possess strong attractive forces, and hold most of their energy as potential energy.

Liquid

A state of matter where molecules move freely, flow, take the shape of their container, and are relatively dense and not easily compressed.

Gas

A state of matter where molecules move rapidly and randomly, possess weak attractive forces, and are easily compressed or expanded.

Adhesion

The attractive force between unlike molecules.

Cohesion

The attractive force between like molecules.

Temperature

A measure of the average kinetic energy of an object, rather than its total energy.

Endothermic Change

A change of state or reaction that requires the addition of energy.

Exothermic Change

A change of state or reaction that gives off or releases energy.

Boyle’s Law

A gas law stating that pressure and volume are inversely related (P1xV1 = P2xV2) when temperature and mass remain constant.

Charles’s Law

A gas law stating that volume and absolute temperature are directly related (V1/T1 = V2/T2) at constant pressure.

Gay-Lussac’s Law

A gas law stating that pressure and absolute temperature are directly related (P1/T1 = P2/T2) at constant volume.

STPD

Standard conditions representing Standard Temperature ($0^\circ\text{C}$), Standard Pressure ($760\,\text{mmHg}$), and Dry gas (zero water vapor).

ATPD

Conditions characterized by Ambient Temperature, atmospheric Pressure, and Dry gas (zero water vapor).

ATPS

Conditions characterized by Ambient Temperature, atmospheric Pressure, and Saturated water vapor.

BTPS

Body conditions characterized by Body Temperature ($37^\circ\text{C}$), atmospheric Pressure, and Saturated water vapor ($47\,\text{mmHg}$ water-vapor pressure).

Dalton’s Law of Partial Pressure

A law stating that each gas in a mixture exerts pressure as if it were alone, making total pressure equal to the sum of the individual partial pressures.

Henry’s Law

A law stating that at constant temperature, the amount of gas dissolving in a liquid is directly proportional to the partial pressure of that gas contacting the liquid.

Graham’s Law

A law stating that lighter gas molecules diffuse faster through gases, while diffusion through liquids depends on both molecular weight and solubility coefficient.

Diffusion

The passive movement or intermingling of molecules from an area of higher concentration or pressure to an area of lower concentration or pressure.

Solution

A homogeneous mixture of two or more substances containing fully dissolved particles.

Solute

The component of a solution that is being dissolved.

Solvent

The dissolving agent in a solution, typically present in the greater amount.

Colloid

A mixture in water characterized by intermediate-sized dispersed particles.

Suspension

A mixture in water containing large particles that can settle out over time.

Saturated Solution

A solution that contains the maximum amount of solute that can dissolve under given conditions, unable to accept additional solute.

Colligative Property

A property of a solution that depends solely on the number of dissolved solute particles present rather than their chemical identity.

Osmosis

The movement or transfer of water molecules across a semipermeable membrane toward the side with the higher effective solute concentration.

Isotonic

Having an osmotic pressure equal to the osmotic pressure inside the cell.

Hypotonic

Having an osmotic pressure lower than the osmotic pressure inside the cell.

Hypertonic

Having an osmotic pressure greater than the osmotic pressure inside the cell.

Acid

A substance that donates or yields hydrogen ions ($\text{H}$) in an aqueous solution, increasing the concentration of $[\text{H}]$.

Base

A substance that yields hydroxide ions ($\text{OH}$) in an aqueous solution, causing a net decrease in $[\text{H}]$.

pK

The pH at which a weak acid is $50\%$ dissociated and $50\%$ undissociated (the point of half-neutralization).

Buffer

A solution that resists changes in pH when acids or bases are added.

Carbonic Anhydrase

The enzyme that catalyzes the equilibrium reaction $\text{CO}_2 + \text{H}_2\text{O} \rightleftharpoons \text{H}_2\text{CO}_3$, predominantly within red blood cells.

Henderson-Hasselbalch Equation

The physiological buffer equation defined as $\text{pH} = 6.10 + \log\left(\frac{[\text{HCO}_3]}{\text{PaCO}_2 \times 0.03}\right)$.

Density

The ratio of mass to volume ($\text{mass}/\text{volume}$ or $\text{g/mL}$), clinically applied in Heliox therapy and calculated for gases as gram molecular weight divided by $22.4\,\text{L}$.

A shift to the right and increased CO2 production indicates what?

Respiratory Alkalosis

A shift to the left and decreased CO2 productions indicates what?

Respiratory Acidosis

A shift to the right and an increased HCO3 (bicarb) production indicates what?

Metabolic Alkalosis

a shift to the left and a decreased production of HCO3 (bicarb) indicates what?

Metabolic Acidosis

the complete equilibrium reaction between CO2 and H2O

CO₂ + H₂O ⇌ H₂CO₃ ⇌ H⁺ + HCO₃⁻.