Chapter 10-12 Vocabulary Flashcards: Water, Acids & Bases, Redox

Vocabulary flashcards covering key terms from notes on water properties, acid-base chemistry, redox reactions, pH, and related topics.

Freshwater

Approximately 2.5% of Earth's water is freshwater; only about 0.5% is drinkable and accessible.

Drinking water sources

Rivers and lakes; groundwater; rainwater collected and stored; desalinated seawater.

H2O molecule shape

bent (V shape)

Polar covalent bonds

Electrons are shared unequally between atoms, creating partial positive and negative charges; in water, O–H bonds are polar covalent.

Hydrogen bonds

Strong intermolecular forces between water molecules; each water molecule can form up to four hydrogen bonds with others.

Amphiprotic substance

A substance that can act as both an acid (proton donor) and a base (proton acceptor).

Acid

A substance that donates a proton (Bronsted-Lowry acid).

Base

A substance that accepts a proton (Bronsted-Lowry base).

Strong acid

An acid that fully ionizes in water to donate H+ ions.

Weak acid

An acid that only partially ionizes in water.

Strong base

A base that readily accepts H+ in solution.

Weak base

A base that accepts H+ to a limited extent.

Neutralization reaction

Acid reacts with base to form a salt and water (e.g., H+ + OH− → H2O; overall acid + base → salt + water).

Acid + metal hydroxide

Acid + OH− → salt + water.

Acid + carbonate

Acid + CO3 2− → salt + CO2 + H2O.

Acid + hydrogen carbonate

Acid + HCO3− → salt + CO2 + H2O.

Acid + reactive metal

Acid reacts with a reactive metal to produce salt and hydrogen gas (H2).

Polyprotic acids

Acids that donate more than one proton; monoprotic (1), diprotic (2), triprotic (3).

Displacement (single displacement)

A more reactive metal displaces a less reactive metal from its compound, transferring electrons.

Oxidation

Loss of electrons; oxidation state increases.

Reduction

Gain of electrons; reduction state decreases.

OILRIG

Oxidation Is Loss, Reduction Is Gain; mnemonic for redox reactions.

Reducing agent

Substance that donates electrons and is oxidized in a redox reaction.

Oxidising agent

Substance that accepts electrons and is reduced in a redox reaction.

Galvanic cell

Device that converts chemical energy into electrical energy via a spontaneous redox reaction; involves anode and cathode; spectator ions are not part of the reaction.

Anode

Electrode where oxidation occurs.

Cathode

Electrode where reduction occurs.

pH

A measure of how acidic or basic a solution is; pH 7 is neutral; lower values are more acidic, higher values more basic.

pH formula

pH = −log10[H3O+]

pH = log10 [H+]

OR

[H3O+] = 10^(−pH).

Ocean acidification & calcification

Atmospheric CO2 dissolves in seawater forming carbonic acid and bicarbonate, increasing H+ and lowering pH; calcification is Ca2+ + CO3^2− → CaCO3(s).

Density

Mass per unit volume (Density = mass/volume).

Ice density

Ice is less dense than liquid water due to a hexagonal lattice that keeps molecules farther apart, causing ice to float.

Heat capacity

The amount of heat required to raise the temperature of a substance by 1°C; water has a high heat capacity (≈4.18 J g−1 °C−1) due to hydrogen bonding.

q = m c ΔT

Heat transferred equals mass × specific heat capacity × temperature change.

Latent heat of vaporization

Energy required to convert 1 mole of liquid to gas; for water ≈ 40.7 kJ/mol.

Latent heat of fusion

Energy required to convert solid to liquid; for water ≈ 6.0 kJ/mol.

Group 16 hydrides

Hydrides containing hydrogen bonded to Group 16 elements; water (H2O) is an example.

heat capacity for water

4.18 J g−1 °C−1

finding the pH of strong bases

10^-14 / OH-

when would you use the Ionic Production (KW)= [H₃O⁺] x [OH^-]

to find the conncentration of hydronium or hydroxide ions in any aqueous solution where the temprature is 25 degrees celcius