CRAM: Atomic Structure Models Flashcards
(34 cards)
Dalton’s Atomic Theory
The first formal description of atoms, proposing they are indivisible particles that make up matter.
Indivisibility of Atoms
Dalton’s principle that atoms cannot be split into smaller parts.
Elemental Identity
Atoms of a specific element are identical in mass and properties.
Conservation in Reactions
In chemical reactions, atoms are rearranged but neither created nor destroyed.
Thomson’s Plum Pudding Model
A model suggesting that atoms consist of electrons in a positive matrix.
Subatomic Particles
Particles smaller than atoms, introduced by Thomson’s model.
Rutherford’s Nuclear Model
A model showing that atoms have a dense nucleus around which electrons orbit.
Nucleus Discovery
Rutherford’s finding that atoms contain a small, dense, positively charged nucleus.
Planetary Model
A model depicting electrons orbiting the nucleus like planets around the sun.
Bohr’s Atomic Model
A model introducing fixed paths for electrons around the nucleus.
Fixed Electron Orbits
Electrons in Bohr’s model occupy specific, quantized paths.
Energy Absorption and Emission
Electrons absorb energy to move to a higher level and release energy when falling back.
Quantum Mechanical Model
A model describing electrons as probabilistic clouds around the nucleus.
Wave-Particle Duality
The concept that electrons exhibit both wave-like and particle-like properties.
Atomic Orbitals
Regions in space where electrons are likely to be found, differing in shape and size.
Complex Math of Quantum Mechanics
Mathematical equations used to predict electron positions probabilistically.
Schrödinger’s Wave Model
Model that uses wave functions to describe electron behavior as probability distributions.
Wave Equation
An equation developed by Schrödinger to describe the behavior of electrons.
Electron Probability Distributions
Regions where there is a higher likelihood of finding electrons.
Dual Nature of Electrons
The principle emphasizing that electrons have both wave and particle characteristics.
Limitations of Dalton’s Theory
Ignored subatomic particles and treated atoms as indivisible.
Limitations of Thomson’s Model
Incorrectly predicted how electrons were distributed within the atom.
Limitations of Rutherford’s Model
Did not account for defined energy levels of electrons.
Limitations of Bohr’s Model
Only accurate for hydrogen atoms.
