Principles of Biology 1 (BIO 001) Chapter 3 Study Guide - Water and Life

Vocabulary flashcards covering core topics from Patel's Study Guide for Chapter 3: Water and Life, including emergent properties of water, molecular conversions, stoichiometry definitions, and acid-base characteristics.

Hydrogen Bond Formation

The process where hydrogen bonds form and release heat (energy) because molecules become more stable, which tends to increase temperature.

Hydrogen Bond Breaking

The process where hydrogen bonds break and absorb heat (energy) because energy is needed to separate molecules, which tends to decrease temperature.

Density of Ice

Ice has a lower density than liquid water because hydrogen bonds create an open structure in ice that takes up more space, causing ice to float on liquid water.

Dissolving Ionic Compounds

The process where water molecules, being polar with a slightly positive end near hydrogen atoms and a slightly negative end near oxygen, attract, surround, and pull apart positive and negative ions, allowing them to spread through the liquid.

Dissolving Large Polar Molecules

The process where water molecules surround large molecules with partial positive or negative charge regions through hydrogen bonding or other intermolecular attraction to keep them dissolved.

Molecular Mass

The mass of one molecule, measured in atomic mass units ($\text{amu}$), calculated by adding the atomic masses of all the atoms in the molecule.

Moles

A counting unit where $1\,\text{mole}$ equals Avogadro's number ($6.022 \times 10^{23}$) of particles.

Avogadro's Number

$6.022 \times 10^{23}\,\text{particles/mol}$, which tells how many particles are contained in $1\,\text{mole}$ of a substance.

Molarity

A measure of concentration that tells how many moles of a substance are dissolved in $1\,\text{liter}$ of solution, calculated using the formula $M = \frac{\text{moles}}{\text{liters of solution}}$.

Molar Mass

The mass of $1\,\text{mole}$ of a substance, measured in $\text{g/mol}$, found by adding the atomic masses of every atom in the chemical formula.

Conversion: Moles to Grams

A conversion performed by multiplying the number of moles by the molar mass of the substance ($\text{grams} = \text{moles} \times \text{molar mass}$).

Conversion: Grams to Moles

A conversion performed by dividing the mass in grams by the molar mass of the substance ($\text{moles} = \frac{\text{grams}}{\text{molar mass}}$).

Conversion: Moles to Molecules

A conversion performed by multiplying the number of moles by Avogadro's number ($\text{molecules} = \text{moles} \times 6.022 \times 10^{23}$).

Conversion: Molecules to Moles

A conversion performed by dividing the number of molecules by Avogadro's number ($\text{moles} = \frac{\text{molecules}}{6.022 \times 10^{23}}$).

Conversion: Molecules to Atoms

A conversion performed by multiplying the number of molecules by the number of that type of atom in the chemical formula.

Acids

Substances that produce $H^+$ (hydrogen ions) in water, usually taste sour, and can be corrosive (e.g., $HCl$, $H_2SO_4$, and acetic acid/vinegar).

Bases

Substances that produce $OH^-$ (hydroxide ions) in water or accept $H^+$, feel slippery, and can be corrosive (e.g., $NaOH$, $KOH$, and ammonia $NH_3$).

Strong Acids

Acids that completely ionize/dissociate in water, including $HCl$, $HBr$, $HI$, $HNO_3$, $H_2SO_4$, and $HClO_4$.

Weak Acids

Acids that only partially ionize in water, such as acetic acid ($CH_3COOH$) and carbonic acid.

Strong Bases

Bases that completely dissociate in water, including $NaOH$, $KOH$, and $Ba(OH)_2$.

Weak Bases

Bases that only partially react with water, such as ammonia ($NH_3$).

pH Scale

A measurement scale of how acidic or basic a solution is based on the concentration of $H^+$, where values from 0 to 6 represent acidic, 7 represents neutral, and 8 to 14 represent basic/alkaline.