Atomic Models

Flashcards covering atomic models from Dalton through the Quantum Mechanical Model, including related concepts like emission spectra, wave-particle duality, and quantum numbers.

Dalton's Model of the Atom

Elements are made up of tiny, indestructible particles called atoms, depicted as a spherical singular entity.

Plum Pudding Model

Proposed that atoms contain negatively charged particles (electrons) existing in a positively charged space with no organization, disproving Dalton's model.

Nuclear Model of the Atom (Rutherford)

Proposed that most of the atom's mass and all its positive charge are contained in a small core called the nucleus, with electrons dispersed in mostly empty space, making the atom electrically neutral. Later incorporated neutral particles (neutrons) within the nucleus.

Nucleus

A small core within an atom containing most of its mass and all of its positive charge (protons), with neutrons also present.

Bohr Model of the Atom

States that electrons travel in fixed orbits at discrete/quantized energy levels around the nucleus, explaining emission spectra observations.

Emission Spectra

The pattern of light released when excited electrons transition from a higher energy orbit to a lower energy orbit, unique for each element.

Excited State (electron)

The state an electron enters after absorbing energy, causing it to move to a higher energy level.

Ground State (electron)

The lowest energy level an electron normally occupies.

Quantized Energy Levels

Discrete, specific energy levels that electrons can occupy within an atom, like steps on a staircase, rather than a continuous ramp.

Quantum Mechanical Model of the Atom

Describes electrons as existing in probability domains (orbitals) around the nucleus, predicting their position about 95% of the time, acknowledging wave-particle duality.

Wave-Particle Duality

The concept that matter, such as electrons, exhibits characteristics of both waves and particles.

Complementary Properties (electrons)

When observing the wave nature of an electron (e.g., interference pattern), its particle nature (e.g., position) cannot be simultaneously observed, and vice versa.

Schrödinger Equation

An equation that allows for the calculation of the probability of finding an electron with a particular amount of energy at a specific location within an atom.

Quantum Numbers

A set of four coordinates (n, l, ml, ms) derived from the Schrödinger equation that describe the probable location and state of an electron within an atom, including its energy level, orbital type, orbital orientation, and spin.

Principal Quantum Number (n)

Denotes the electron's principal energy level and its approximate distance from the nucleus.

Angular Momentum Quantum Number (l)

Denotes the type or shape of the orbital an electron occupies (e.g., s, p, d, f).

Magnetic Quantum Number (m_l)

Denotes the specific orbital within a subshell, indicating its orientation in space.

Magnetic Spin Quantum Number (m_s)

Denotes the intrinsic spin of an electron, which can be either +1/2 or -1/2.