CSEC Chemistry: Atomic Structure, Bonding, and Reactions Review

Comprehensive vocabulary flashcards covering basic chemical principles, bonding, periodic trends, state changes, energetics, and introductory organic chemistry.

Giant ionic crystalline structures

Structures with high melting points comprised of many identical repeating units of ions held together by strong electrostatic forces.

Covalent bond

A chemical bond formed by the sharing of electrons between atoms, typically occurring between non-metals.

Van-der-Waals forces

Weak intermolecular forces that hold molecules together, resulting in low melting and boiling points.

Isotopes

Different forms of the same element with the same proton number but different neutron number (and hence different mass number).

Mass number

The sum of the number of protons and the number of neutrons in the nucleus of an atom.

Ionic solid

A solid consisting of a lattice of positive and negative ions characterized by high melting points and electrical conductivity when molten or in aqueous solution.

Molecular solid

A solid composed of molecules held together by weak intermolecular forces, typically having a low melting point and no electrical conductivity.

Ease of ionization

The relative facility with which an atom loses valence electrons to form a cation; it increases down a metallic group as the atomic radius increases.

Oxidising power

The ability of an atom to gain electrons to form anions; in non-metals, it increases up a group as the atomic radius decreases and the nucleus pull increases.

Groups

The vertical columns in the periodic table containing elements with the same number of valence electrons.

Periods

The horizontal rows in the periodic table containing elements with the same number of occupied atomic orbitals (shells).

Volatility

The tendency of a substance to easily change its state from a solid or liquid to a gas at room temperature, typical of simple molecular substances.

Melting point

The constant temperature at which a solid changes into a liquid.

Sublimation

The process by which a substance changes directly from a solid state to a gaseous state upon heating, as seen with iodine.

Radioisotopes

Isotopes with unstable nuclei that are radioactive and decay spontaneously by emitting particles and radiation.

Allotropes

Different structural forms of a single element in the same physical state, such as diamond and graphite for carbon.

Metallic bonding

The force of attraction between a lattice of positive metal cations and a sea of delocalized valence electrons.

Fermentation

The chemical reaction where carbohydrates are converted into ethanol and carbon dioxide by yeast under anaerobic conditions.

Fractional distillation

A separation process based on differences in boiling points used to separate mixtures of miscible liquids, such as ethanol and water.

Solution

A homogenous mixture consisting of two or more components.

Suspension

A heterogenous mixture consisting of two or more components where particles may settle over time.

Centrifugation

An industrial process used to separate sugar crystals from molasses during sugar production.

Bagasse

A byproduct of sugar cane processing used as fuel for boiler furnaces to supply heat.

Bauxite

The ore of aluminium, composed of impure, hydrated aluminium oxide ($Al_2O_3 \cdot xH_2O$).

Alloy

A mixture of metals (sometimes involving non-metals) produced to modify or improve the properties of pure metals, such as hardness or corrosion resistance.

Chlorosis

A condition in plants where leaves turn yellow due to a deficiency in magnesium or iron, leading to reduced chlorophyll.

Corrosion

The process where metal surfaces are gradually worn away by reacting with oxygen and water vapor in the environment.

Mole

The amount of a substance that contains exactly $6.0 \times 10^{23}$ particles of that substance.

Molar mass ($M$)

The mass in grams of one mole of a chemical substance ($g\,mol^{-1}$).

Rate of reaction

The measured change in the concentration of a reactant or product with time at a given temperature.

Activation energy

The minimum energy that colliding particles must achieve for a chemical reaction to occur.

Catalyst

A substance that alters the rate of a chemical reaction by providing an alternative pathway with a lower activation energy without being consumed.

Exothermic reaction

A chemical reaction that releases energy to the environment, resulting in a temperature increase.

Endothermic reaction

A chemical reaction that absorbs energy from the environment, resulting in a temperature decrease.

Electrolysis

The chemical decomposition that occurs when an electric current is passed through an electrolyte.

Electrolyte

A compound that forms ions when molten or in aqueous solution and is capable of conducting electricity.

Cathode

The negative electrode connected to the negative terminal of a power supply where reduction occurs.

Anode

The positive electrode connected to the positive terminal of a power supply where oxidation occurs.

Oxidising agent

A substance that causes another reactant to lose electrons (be oxidized) while it itself gains electrons (is reduced).

Reducing agent

A substance that causes another reactant to gain electrons (be reduced) while it itself loses electrons (is oxidized).

Salt

A compound formed when some or all of the hydrogen ions in an acid are replaced by metal or ammonium ions.

Functional group

A particular atom, group of atoms, or bond within a molecule that determines its specific chemical properties.

Structural isomerism

The existence of compounds with the same molecular formula but different connectivity or arrangement of atoms in space.

Homologous series

A family of organic compounds sharing the same functional group, same general formula, and similar chemical properties.

Unsaturated

Refers to organic compounds containing at least one carbon-carbon double or triple bond, such as alkenes.

Saponification

The alkaline hydrolysis of large esters (fats or oils) traditionally using sodium hydroxide to produce soap and glycerol.

Hard water

Water that does not lather easily with soap due to the presence of dissolved calcium ($Ca^{2+}$) or magnesium ($Mg^{2+}$) ions.

Eutrophication

The rapid growth of algae and green plants in waterways due to excess phosphates, leading to oxygen depletion and the death of aquatic life.

Polymer

A macromolecule formed from multiple smaller units, known as monomers, linked together.

Green chemistry

Sustainable chemistry focusing on the design and manufacture of products that reduce or eliminate the use and generation of hazardous substances.