Physical Chemistry: Giant Structures, Ionic Bonding, Heat, Temperature, and Density

Comprehensive vocabulary flashcards covering giant lattices, ionic and covalent bonding, properties of diamond and graphite, heat versus temperature, and density concepts.

Giant Ionic Lattice

A regular, repeating three-dimensional cubic arrangement of millions of oppositely charged ions held together by strong ionic bonds.

Electrostatic Forces

Strong forces of attraction between oppositely charged ions (such as $Na^+$ and $Cl^-$) that hold the ions tightly together within an ionic lattice.

Diamond

A giant covalent allotrope of carbon in which each carbon atom is covalently bonded to $4$ other carbon atoms in a rigid, three-dimensional lattice, making it extremely hard with high melting and boiling points and non-conductive of electricity.

Graphite

A giant covalent allotrope of carbon in which each carbon atom is covalently bonded to $3$ other carbon atoms in planar hexagonal layers held together by weak intermolecular forces, leaving $1$ free electron per carbon atom.

Delocalized Electron

A free electron not tied to a single chemical bond, such as the single unbonded valence electron on each carbon atom in graphite, allowing the material to conduct electricity.

Ionic Compound

A compound formed between a metal and a non-metal via electron transfer that forms formula units arranged in a hard crystal lattice, featuring high melting points and the ability to conduct electricity when molten or dissolved.

Covalent Compound

A substance formed when two or more non-metal atoms share electrons to form discrete molecules, characterized by lower melting points, softer physical properties, and poor electrical conductivity.

Ion

An electrically charged atom or group of atoms formed when an unstable neutral atom either loses or gains valence electrons to attain a full outer electron shell.

Positive Ion (Cation)

A positively charged ion formed when a neutral atom (typically a metal) loses electrons, resulting in more protons than electrons.

Negative Ion (Anion)

A negatively charged ion formed when a neutral atom (typically a non-metal) gains electrons, resulting in more electrons than protons.

Ionic Bonding

The electrostatic attraction that binds oppositely charged ions together after metallic atoms transfer electrons to non-metallic atoms.

Brittleness (in Ionic Compounds)

The tendency of an ionic lattice to shatter under mechanical impact because shifting ion layers bring like charges alongside each other, causing strong electrostatic repulsion.

Thermal Energy

The total energy possessed by vibrating particles in matter, which can be stored, transformed, dissipated, and quantified in joules ($J$).

Heat

The form of energy describing the transfer of total thermal energy between particles within a system from a hotter temperature to a cooler temperature, measured in joules ($J$) or calories.

Temperature

A measure of the average kinetic energy of all the vibrating particles in an object or system, indicating how hot or cold it is.

Absolute Zero

The theoretical minimum temperature of $-273^\circ\text{C}$, corresponding to the point where particle motion would completely cease.

Calorimeter

A device designed to measure quantities of heat energy transferred during physical or chemical processes.

Thermometer

An instrument used to measure the temperature of an object or substance on scales such as Celsius ($^\circ\text{C}$), Kelvin ($K$), or Fahrenheit ($^\circ\text{F}$).

Density

A physical measurement of how tightly matter is packed within a given volume, defined mathematically as $\text{density} = \frac{\text{mass}}{\text{volume}}$ and measured in units such as $g/cm^3$ or $kg/m^3$.

Displacement Method

A laboratory procedure used to determine the volume of an irregularly shaped solid by immersing it in a known volume of water in a graduated measuring cylinder and calculating the difference in liquid level.

Liquid Layers

The visible stratification formed when immiscible liquids of differing densities are poured together, where the densest liquid settles at the bottom and the least dense liquid rests on the top.

Flotation Rule

The buoyancy principle dictating that a substance will float in water if its density is lower than the density of water, and sink if its density is greater than water.