Atomic Structure, Periodic Table, Bonding, and Quantitative Chemistry Flashcards

Flashcards covering key concepts of atomic models, periodic trends, chemical bonding, structures, and quantitative chemistry based on the lecture notes.

John Dalton's Atomic Theory

A theory stating that atoms cannot be created, divided, or destroyed; atoms of the same element are exactly the same; and atoms join with other atoms to make new substances.

J.J. Thomson's Cathode Ray Experiment

An experiment where a cathode ray beam moved towards a positively charged plate, proving that the particles in the beam possessed a negative charge.

Plum Pudding Model

An atomic model proposed by J.J. Thomson featuring negatively charged electrons scattered throughout a positively charged material.

Gold Foil Experiment

An experiment by Ernest Rutherford where positively charged particles were shot at gold foil; most passed straight through, while a few deflected or bounced back, showing that atoms have a tiny, dense, positively charged nucleus.

Rutherford's Atomic Model

An atomic model where mass is concentrated in a central nucleus, the atom consists mostly of empty space, and electrons travel in random paths around the nucleus.

Radius of the Nucleus

$1 \times 10^{-14}\,\text{m}$, which is $\frac{1}{10000}$ of the atomic radius.

Atomic Electrical Neutrality

The condition where an atom has no overall charge because it contains equal numbers of positively charged protons and negatively charged electrons.

Mass Number

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

Atomic Number

The unique number of protons in the nucleus of an atom of a specific element.

Isotope

Atoms of the same element with the same number of protons (same atomic number) but a different number of neutrons (different mass numbers).

Relative Atomic Mass

The weighted average of the masses of all isotopes of an element, calculated using the mass numbers and relative abundances of each isotope.

Mendeleev's Periodic Table

A periodic table arrangement ordered by increasing atomic mass, grouping elements with similar chemical properties, leaving gaps for undiscovered elements, and swapping element positions when necessary.

Group (Periodic Table)

A vertical column in the periodic table containing elements that have the same number of outer shell electrons and similar chemical properties.

Period (Periodic Table)

A horizontal row in the periodic table where all elements share the same total number of electron shells.

Electron Shell Capacities

The maximum number of electrons allowed in the first three shells: 2 in the 1st shell, 8 in the 2nd shell, and 8 in the 3rd shell.

Ionic Bonding

The transfer of electrons where a metal atom loses electrons to form a positively charged cation and a non-metal atom gains electrons to form a negatively charged anion.

Ion

An atom or group of atoms that has acquired a positive or negative charge.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Compound Suffix '-ate'

A chemical naming convention indicating that an ionic compound contains at least three elements, one of which is oxygen.

Ionic Lattice

A regular structure of ions held together by strong electrostatic forces between oppositely charged ions.

Simple Molecule

A chemical structure formed by atoms joined together by strong covalent bonds within the molecule.

Intermolecular Forces

Weak forces of attraction between molecules that require relatively little energy to overcome.

Graphite

An allotrope of carbon where each atom is covalently bonded to three other carbon atoms in hexagonal layers, featuring weak intermolecular forces between layers and one delocalised electron per carbon atom.

Diamond

An allotrope of carbon where every carbon atom is covalently bonded to four other carbon atoms, resulting in a very hard structure with a very high melting point and no electrical conductivity.

Fullerene

A carbon molecule shaped like a closed tube or hollow ball.

$C_{60}$ Fullerene

A spherical fullerene molecule with strong covalent bonds within the molecule, low melting point, and slippery properties due to weak intermolecular forces.

Graphene

A single, one-atom-thick layer of graphite that is extremely strong, has a high melting point, and conducts electricity via delocalised electrons.

Empirical Formula

The smallest whole-number ratio of the atoms of each element in a compound.

Relative Formula Mass ($M_r$)

The total value calculated by adding together all the relative atomic masses of the atoms in a chemical formula.

Law of Conservation of Mass

The principle stating that in a closed system, the total mass remains constant throughout a chemical reaction.

Avogadro Constant

The number of atoms, molecules, or ions in one mole of any given substance, equal to $6.02 \times 10^{23}$.

Limiting Reagent

The chemical reactant that is completely consumed first in a reaction, preventing the formation of further products.