Atomic Structure and Periodic Properties Flashcards (Unit 1)

Flashcards covering vocabulary and definitions related to atomic structure and periodic properties.

Atomic Structure

The arrangement of protons, neutrons, and electrons in an atom.

Periodic Table

A table that organizes elements by their atomic number and properties.

Subatomic Particles

The smaller particles that make up an atom: protons, neutrons, and electrons.

Proton

A positively charged subatomic particle found in the nucleus of an atom.

Neutron

A neutrally charged subatomic particle found in the nucleus of an atom.

Electron

A negatively charged subatomic particle that orbits the nucleus of an atom.

Atomic Number

The number of protons in the nucleus of an atom, defining the element.

Mass Number

The total number of protons and neutrons in an atom's nucleus.

Isotope

Atoms of the same element with different numbers of neutrons.

Cation

A positively charged ion formed by losing electrons.

Anion

A negatively charged ion formed by gaining electrons.

Monoatomic Ion

An ion consisting of a single atom with a positive or negative charge.

Polyatomic Ion

An ion composed of two or more atoms that are covalently bonded.

Valence Electrons

Electrons in the outermost shell of an atom that determine its chemical properties.

Octet Rule

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons.

Electronegativity

The tendency of an atom to attract electrons in a chemical bond.

Ionization Energy

The energy required to remove an electron from an atom.

Atomic Radius

The distance from the nucleus to the outermost electron shell; influences the size of an atom.

Coulombic Attraction

The force of attraction between positively and negatively charged particles.

Shielding Effect

The phenomenon where inner electrons reduce the effective nuclear charge experienced by outer electrons.

Orbital

Regions in an atom where electrons are likely to be found.

S-orbital

A spherical orbital where a maximum of 2 electrons can exist.

P-orbital

A dumbbell-shaped orbital that can hold a maximum of 6 electrons.

D-orbital

A more complex shaped orbital that can hold a maximum of 10 electrons.

F-orbital

An even more complex shaped orbital that can hold a maximum of 14 electrons.

Electron Configuration

A representation of the arrangement of electrons in an atom.

Aufbau Principle

The rule that electrons occupy the lowest energy orbitals available.

Pauli Exclusion Principle

The principle that no two electrons in an atom can have the same set of quantum numbers.

Hund's Rule

Electrons will fill degenerate orbitals singly before pairing up.

First Ionization Energy

The energy required to remove the first electron from a neutral atom.

Orbital Filling Diagram

A diagram that illustrates how electrons are distributed across the orbitals.

Periodic Trends

Patterns in the properties of elements as you move across periods or down groups.

Metallic Character

The tendency of an element to behave like a metal, including conductive properties and ion formation.

Nonmetal Reactivity

The tendency of nonmetals to gain electrons and form anions.

Electrostatics

The study of electric charges at rest and the forces between them.

Chemical Bond

The force that holds atoms together in molecules or compounds.

Molecule

A group of two or more atoms bonded together.

Compound

A substance formed when two or more elements chemically bond.

Hydrogen Bond

A weak bond between two molecules resulting from an electrostatic attraction.

Atomic Mass Unit (amu)

A unit of mass used to express atomic and molecular weights.

Quantum Mechanics

A branch of physics that deals with the behavior of matter on a very small scale.

Bohr Model

A model of the atom that depicts electrons traveling in fixed orbits around the nucleus.

Wave-Particle Duality

The concept that matter exhibits both particle and wave properties.

Heisenberg Uncertainty Principle

The principle that states it is impossible to simultaneously know the exact position and momentum of a particle.

Schrödinger Equation

The key equation of quantum mechanics that describes how the quantum state of a physical system changes over time.

Electrolyte

A substance that dissolves in water to produce a solution that conducts electricity.

Solvent

A substance that dissolves a solute, resulting in a solution.

Reaction Rate

The speed at which a chemical reaction proceeds.

Catalyst

A substance that increases the rate of a chemical reaction without being consumed.

Activation Energy

The minimum energy required for a chemical reaction to occur.

Enzyme

Biological catalysts that speed up biochemical reactions.