Lecture 1: Atomic Structure and Chemical Bonds

These flashcards summarize key concepts from the lecture on atomic structure and chemical bonds.

Atom

The basic building block of all matter in the Universe, consisting of electrons, protons, and neutrons.

Electron

A negatively charged particle found in orbitals, with negligible mass compared to protons and neutrons.

Proton

A positively charged particle located in the nucleus of an atom, contributing to the atomic mass.

Neutron

A particle with no charge located in the nucleus; its presence contributes to the atomic mass.

Atomic Number

The number of protons in the nucleus of an atom, determining the element's identity.

Atomic Mass Number

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

Orbital

A defined area of space around the nucleus where electrons are likely to be found.

Ground State

The lowest energy state of an atom, where all electrons occupy the lowest available orbitals.

Covalent Bond

A type of chemical bond that involves the equal sharing of electrons between two atoms.

Ionic Bond

A chemical bond formed by the attraction between oppositely charged ions.

Hydrogen Bond

A weak attraction between a partially positively charged hydrogen atom and an atom with unpaired electrons, typically in different molecules.

Van der Waals Interaction

A weak, non-specific attraction between atoms that arises from temporary fluctuations in electron density.

Hydrophobic Effect

The tendency of nonpolar molecules to aggregate in aqueous environments, minimizing their exposure to water.

Hund's Rule

A principle stating that electrons fill orbitals of equal energy singly before pairing up in orbitals.

Single Bond

A covalent bond formed by the sharing of one pair of electrons between two atoms.

Double Bond

A covalent bond formed by the sharing of two pairs of electrons between two atoms.

Triple Bond

A covalent bond formed by the sharing of three pairs of electrons between two atoms.