Chemistry: Kinetic Theory, Bonding, and Periodic Table Review

Vocabulary practice flashcards covering states of matter, chemical bonding, allotropes, gas laws, and periodic table trends.

Solids (Particle Arrangement and Movement)

Strong forces of attraction between particles keeps them in fixed positions.

Liquids (Forces)

Forces of attraction between particles that are weaker than those in solids.

Gases (Movement)

Move randomly because there are no intermolecular forces.

Boyle's Law Relationship

As pressure increases, the volume of a gas decreases; as pressure decreases, the volume increases.

Evaporation (Kinetic Theory)

Particles near the surface gain sufficient energy from the surroundings to overcome intermolecular forces and escape.

Diffusion Rate (Molecular Mass)

Smaller relative molecular mass results in 'lighter' particles with higher average speeds, increasing the rate of diffusion.

Temperature and Gas Volume

Increasing temperature increases kinetic energy, causing particles to move and collide with the container more quickly and spread further apart, increasing volume.

Ionic Bonding (Lattice)

A giant regular structure extending in all directions, held together by electrostatic attraction between positive and negative ions.

Ionic Compound Properties

High melting/boiling points, non-conductive when solid (ions fixed), but conductive when molten or dissolved (ions free to move).

Magnesium Oxide formation ($MgO$)

The metal Mg ($Group II$) transfers two outer shell electrons to O ($Group VI$), resulting in $Mg^{2+}$ and $O^{2-}$ ions.

Simple Molecular Covalent Substances

Small molecules with weak intermolecular forces, resulting in low melting and boiling points and no electrical conductivity.

Allotropes

Different structural forms of the same element in the same physical state with distinct physical and chemical properties due to variations in atomic bonding.

Diamond

Carbon allotrope with four strong covalent bonds per atom in a rigid tetrahedral arrangement; it is very hard, has a high melting point, and does not conduct electricity.

Graphite

Carbon allotrope with three covalent bonds per atom in hexagonal layers; soft/lubricant due to weak intermolecular forces between layers and conductive due to delocalised electrons.

Fullerenes

Hollow shaped molecules based on hexagonal rings (sometimes 5 or 7 carbon rings), such as spherical $C_{60}$ (Buckminsterfullerene) or cylindrical nanotubes.

Graphene

A single layer of graphite.

Metallic Bonding

Forces of attraction between delocalised electrons and the nuclei of metal ions.

Alloys

Mixtures of metals with other elements where different atomic sizes distort layers, preventing them from sliding and making the material harder than pure metals.

Periodic Table Arrangement

Elements arranged by increasing atomic number into vertical groups (same outer shell electrons) and horizontal periods (same number of electron shells).

Metallic Character Trend

Decreases across a period.

Group I Trends (Lithium, Sodium, Potassium)

Soft metals that show a decrease in melting point, increase in density, and increase in reactivity with water down the group.

Group I Reactivity

Increases down the group because atomic radius and shielding increase, weakening attraction to the outer electron and requiring less energy to remove it.

Group I Reaction with Water

Vigorous reaction producing hydrogen gas (bubbles) and an alkaline solution.

Halogens ($Group VII$)

Diatomic non-metals including Chlorine, Bromine, and Iodine.

Chlorine (Room Temp State)

Pale green gas.

Bromine (Room Temp State)

Red-brown liquid.

Iodine (Room Temp State)

Grey-black solid.

Fluorine and Astatine Predictions

Fluorine is a gas (lower boiling point than chlorine); Astatine is a solid (higher melting point than iodine).

Halogen Displacement Reaction

Occurs when a more reactive halogen displaces a less reactive halogen from an aqueous solution of its halide ions.

Group VII Reactivity

Decreases down the group because increased atomic radius and shielding make it harder for the nucleus to attract and gain an electron.

Transition Metals

Metals with high densities and melting points that form coloured compounds, have variable oxidation states (e.g., $Fe^{2+}$ and $Fe^{3+}$), and act as catalysts.

Noble Gases

Chemically inert elements with stable, full outer electron shells.

Silicon (IV) Oxide ($SiO_2$)

A giant covalent structure where each silicon atom is bonded to 4 oxygen atoms and each oxygen atom is bonded to 2 silicon atoms in a tetrahedral arrangement.