Chemistry: Acids, Bases, Electrochemistry, and Organic Chemistry Flashcards

Comprehensive vocabulary flashcards covering Acid-Base theories, Electrochemistry definitions, Organic molecule structures and isomers, and Chemical Equilibrium principles based on the lecture notes.

Arrhenius theory

Acids produce hydrogen ions ($H^+/H_3O^+/\text{hydronium ions}$) in aqueous solution. Bases produce hydroxide ions ($OH^-$) in aqueous solution.

Lowry-Brønsted theory

An acid is a proton ($H^+$ ion) donor. A base is a proton ($H^+$ ion) acceptor.

Strong acid

Ionises completely in water to form a high concentration of $H_3O^+$ ions.

Weak acid

Ionises incompletely in water to form a low concentration of $H_3O^+$ ions.

Strong base

Dissociates completely in water to form a high concentration of $OH^-$ ions.

Weak base

Dissociate/ionise incompletely in water to form a low concentration of $OH^-$ ions.

Concentrated acids/bases

Contain a large amount (number of moles) of acid/base in proportion to the volume of water.

Dilute acids/bases

Contain a small amount (number of moles) of acid/base in proportion to the volume of water.

Ampholyte

A substance that can act as either acid or base.

Hydrolysis

The reaction of a salt with water.

Equivalence point of a titration

The point at which the acid/base has completely reacted with the base/acid.

Endpoint of a titration

The point where the indicator changes colour.

Galvanic cell

A cell in which chemical energy is converted to electrical energy.

Oxidation (in terms of electron transfer)

A loss of electrons.

Reduction (in terms of electron transfer)

A gain of electrons.

Oxidation (in terms of oxidation numbers)

An increase in oxidation number.

Reduction (in terms of oxidation numbers)

A decrease in oxidation number.

Oxidising agent

A substance that is reduced/gains electrons.

Reducing agent

A substance that is oxidised/loses electrons.

Anode

The electrode where oxidation takes place.

Cathode

The electrode where reduction takes place.

Electrolyte

A substance of which the aqueous solution contains ions OR a substance that dissolves in water to give a solution that conducts electricity.

Electrolytic cell

A cell in which electrical energy is converted into chemical energy.

Electrolysis

The chemical process in which electrical energy is converted to chemical energy OR the use of electrical energy to produce a chemical change.

Boiling point

The temperature at which the vapour pressure of a substance equals atmospheric pressure.

Melting point

The temperature at which the solid and liquid phases of a substance are at equilibrium.

Vapour pressure

The pressure exerted by a vapour at equilibrium with its liquid in a closed system.

Organic molecules

Molecules containing carbon atoms.

Molecular formula

A chemical formula that indicates the element and numbers of each of the atoms in a molecule.

Structural formula

A structural formula of a compound shows which atoms are attached to which within the molecule.

Condensed structural formula

This notation shows the way in which atoms are bonded together in the molecule but DOES NOT SHOW ALL bond lines.

Hydrocarbon

Organic compounds that consist of hydrogen and carbon only.

Homologous series

A series of organic compounds that can be described by the same general formula OR in which one member differs from the next with a $CH_2$ group.

Saturated compounds

Compounds in which there are no multiple bonds between C atoms in their hydrocarbon chains.

Unsaturated compounds

Compounds with one or more multiple bonds between C atoms in their hydrocarbon chains.

Functional group

A bond or an atom or a group of atoms that determine(s) the physical and chemical properties of a group of organic compounds.

Structural isomer

Organic molecules with the same molecular formula, but different structural formulae.

Chain isomers

Same molecular formula, but different types of chains.

Positional isomers

Same molecular formula, but different positions of the side chain, substituents, or functional groups on the parent chain.

Functional isomers

Same molecular formula, but different functional groups.

Heat of reaction

The energy absorbed or released in a chemical reaction.

Exothermic reactions

Reactions that release energy.

Endothermic reactions

Reactions that absorb energy.

Activation energy

The minimum energy needed for a reaction to take place.

Activated complex

The unstable transition state from reactants to products.

Reaction rate

The change in concentration of reactants or products per unit time.

Catalyst

A substance that increases the rate of a chemical reaction without itself undergoing a permanent change.

Open system

A system that continuously interacts with its environment.

Closed system

A system that is isolated from its surroundings.

Reversible reaction

A reaction where the products can be converted back to reactants and vice versa.

Chemical equilibrium

A dynamic equilibrium when the rate of the forward reaction equals the rate of the reverse reaction.

Le Chatelier's principle

When the equilibrium in a closed system is disturbed, the system will re-instate a new equilibrium by favouring the reaction that will oppose the disturbance.

Momentum

The product of an object’s mass and its velocity

Newton’s second law of motion in terms of momentum

The net force acting on an object is equal to the rate of change of momentum of the object in the direction of the net force

Impulse

The product of the resultant/net force acting on an object and the time the net force acts on the object