DP1 Chemistry Comprehensive Exam Review

Vocabulary based flashcards covering the DP1 Chemistry syllabus including particulate matter models, bonding, structure, periodic classification, organic chemistry, and chemical kinetics.

Elements

The primary constituents of matter which cannot be chemically broken down into simpler substances.

Compounds

Chemical substances consisting of atoms of different elements chemically bonded together in a fixed ratio.

Mixtures

Substances containing more than one element or compound in no fixed ratio that are not chemically bonded and can be separated by physical methods.

Kinetic molecular theory

A model used to explain the physical properties of matter (solids, liquids, and gases) and changes of state.

States of matter symbols

Notation used to identify physical forms: $(s)$ stands for solid, $(l)$ for liquid, $(g)$ for gas, and $(aq)$ for aqueous.

Temperature $T$

A measure of the average kinetic energy ($E_k$) of particles, given in units of Kelvin ($K$).

Nucleus

The positively charged, dense center of an atom composed of protons and neutrons (nucleons).

Isotopes

Atoms of the same element that contain different numbers of neutrons.

Emission spectra

Produced by atoms emitting photons when electrons in excited states return to lower energy levels.

Main energy level $n$

Given by an integer number and can hold a maximum of $2n^2$ electrons.

Sublevels

The division of the main energy level into labels $s$, $p$, $d$, and $f$ of successively higher energies.

Orbitals

Regions of space where there is a high probability of finding an electron, each capable of holding two electrons of opposite spin.

Mole (mol)

The SI unit of amount of substance, containing exactly the number of elementary entities given by the Avogadro constant.

Relative atomic mass ($A_r$)

The mass of atoms compared on a scale relative to $^{12}C$.

Molar mass ($M$)

The mass of one mole of a substance expressed in units of $g\,mol^{-1}$.

Empirical formula

The simplest ratio of atoms of each element present in a compound.

Molecular formula

The actual number of atoms of each element present in a molecule.

Avogadro’s law

States that equal volumes of all gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.

Ideal gas

A conceptual model of a gas consisting of moving particles with negligible volume, no intermolecular forces, and fully elastic collisions.

Cations

Positive ions formed when metal atoms lose electrons.

Anions

Negative ions formed when non-metal atoms gain electrons.

Ionic bond

An electrostatic attraction between oppositely charged ions.

Covalent bond

An electrostatic attraction between a shared pair of electrons and the positively charged nuclei.

Octet rule

The tendency of atoms to gain a valence shell with a total of 8 electrons.

Coordination bond

A covalent bond in which both electrons of the shared pair originate from the same atom.

VSEPR model

The Valence Shell Electron Pair Repulsion model, used to predict molecular shapes based on the repulsion of electron domains around a central atom.

Allotrope

Different forms of the same element, such as diamond, graphite, fullerenes, and graphene for carbon.

Intermolecular forces

Forces existing between molecules, including London dispersion, dipole-induced dipole, dipole-dipole, and hydrogen bonding.

Chromatography

A technique used to separate mixture components based on their relative attractions involving intermolecular forces to mobile and stationary phases.

Metallic bond

The electrostatic attraction between a lattice of cations and delocalized electrons.

Bonding triangle

A representation showing bonding as a continuum between the ionic, covalent, and metallic models based on electronegativity data.

Alloys

Mixtures of a metal and other metals or non-metals that possess enhanced properties.

Polymers

Large molecules or macromolecules made from repeating subunits called monomers.

Periodicity

Trends in the properties of elements across a period and down a group in the periodic table.

Oxidation state

A number assigned to an atom showing the number of electrons transferred in forming a bond; it represents the charge an atom would have if the compound were ionic.

Homologous series

A family of compounds in which successive members differ by a common structural unit, typically $CH_2$, and share a general formula.

IUPAC nomenclature

A set of rules used by the International Union of Pure and Applied Chemistry to apply systematic names to organic and inorganic compounds.

Structural isomers

Molecules that have the same molecular formula but different connectivities.

Limiting reactant

The substance in a chemical reaction that determines the theoretical yield of products.

Atom economy

A measure of efficiency in green chemistry calculated from the stoichiometry of a reaction.

Rate of reaction

Expressed as the change in concentration of a particular reactant or product per unit time.

Activation energy ($E_a$)

The minimum energy that colliding particles need for a successful collision leading to a reaction.

Catalysts

Substances that increase the rate of reaction by providing an alternative reaction pathway with a lower activation energy ($E_a$).