Biology Chapter: Properties of Water

A molecule with opposite charges at opposite ends. Water is a polar molecule due to the unequal sharing of electrons between the oxygen and hydrogen atoms.

The biological medium on Earth that is essential for all living organisms. It makes up the majority of cells and surrounds them.

The ability of water molecules to bond with each other, forming a strong network. These bonds give water its unique properties.

Water's ability to moderate temperature fluctuations. It absorbs and releases heat slowly, helping to regulate temperature in organisms and the environment.

Water's capacity to dissolve many substances, making it a versatile solvent. This property allows for transport within organisms and chemical reactions.

Water molecules have a slightly negative charge near the oxygen atom and a slightly positive charge near the hydrogen atoms due to unequal sharing of electrons in covalent bonds.

A weak bond between a slightly positive hydrogen atom of one molecule and a slightly negative atom (like oxygen) of another molecule.

Water's ability to form hydrogen bonds with other water molecules is responsible for a wide range of its properties.

The tendency of an atom to attract electrons towards itself in a chemical bond.

A type of covalent bond where electrons are shared unequally between two atoms, resulting in a slightly positive and slightly negative end on the molecule.

Oxygen is more electronegative than hydrogen, meaning it attracts electrons more strongly in a water molecule.

Due to the uneven distribution of electrons, the oxygen atom in water has a partial negative charge (-) and the hydrogen atoms have partial positive charges (+).

The slightly negative oxygen of one water molecule can form a hydrogen bond with the slightly positive hydrogen of another water molecule.

Attraction between water molecules due to hydrogen bonds. This property helps water stick together, aiding in upward transport against gravity.

Attraction between water molecules and other substances, like plant cell walls, due to hydrogen bonds. This helps move water upwards in plants.

A measure of how difficult it is to break the surface of a liquid. Water has high surface tension due to strong hydrogen bonding.

The total amount of kinetic energy in a substance due to molecular motion.

The intensity of heat, measured by the average kinetic energy of molecules.

The amount of heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius. Water has a high specific heat.

Water's ability to resist changes in temperature. This is due to its strong hydrogen bonds.

Water can moderate air temperature by absorbing heat when it's warmer and releasing heat when it's cooler.

The force of attraction between oppositely charged ions in a solution, like Na+ and Cl- in water.

The weak attraction between a hydrogen atom in one molecule and a highly electronegative atom (like oxygen) in another molecule. This is crucial for water's properties.

Substances that love water and readily dissolve in it. They typically have polar or ionic properties.

Substances that fear water and don't mix with it. They are usually non-polar and lack charges.

The amount of solute dissolved in a given volume of solvent. It's crucial for understanding biochemical reactions.

The number of moles of a solute dissolved in one liter of solution.

The sum of the atomic masses of all atoms in a molecule.

A unit of measurement that represents a specific number of molecules (6.02 x 10^23) of a substance.

The process where water molecules break down into hydronium ions (H3O+) and hydroxide ions (OH-), which creates acidity or basicity.

A molecule with a positive and negative charge at different ends due to unequal sharing of electrons.

Ions that result from the dissociation of water, making a solution acidic.

Ions that result from the dissociation of water, making a solution basic.

The degree of acidity or basicity of a solution determined by the concentration of H3O+ and OH- ions.

A measure of the acidity or basicity of a solution, measured on a scale from 0 to 14.

A substance that increases the hydrogen ion concentration in a solution by releasing H+ ions.

A substance that reduces the hydrogen ion concentration in a solution, either by accepting H+ ions or releasing OH- ions.

A solution with a pH value less than 7, indicating a higher concentration of hydrogen ions (H+).

A solution with a pH value greater than 7, indicating a lower concentration of hydrogen ions (H+).

The neutral point on the pH scale where the concentration of hydrogen ions (H+) and hydroxide ions (OH-) are equal.

A change in the pH of a solution, usually caused by the addition of acids or bases.

The relative concentration of hydrogen ions (H+) in a solution, determining its acidity.

The process of adding acids or bases to a solution to change its pH.

Fluids that are found within living organisms, typically with pH values ranging from 6 to 8.