Inorganic Chemistry Chapter 2

Atomic Structure

Name all groups on periodic Table

Alkali Metals, Alkaline Earth Metals, Transition Metals, Coinage Metals, Halogens, Halogens, Noble Gases, Lathnides and Actinides

Energies of visible light emitted by te hydrogen Atoms

E= Rh(1/(2²) - 1/(n²h)

E=

hv= hc/wavelenght

The energy of the light emitted or absorbed can be found, according to the Bohr model of the hydrogen atom, from the equation

E = -Rh(1/nf^2 - 1/ni^2)

Heisenberg’s uncertainty principle

It states that the position and momentum of a particle cannot both be precisely determined at the same time. This principle has implications for the behavior of electrons in atoms.

The Schrödinger Equation

Describes how the quantum state of a physical system changes over time, providing a fundamental framework for understanding quantum mechanics and electron behavior in atoms. H(wave function)= E(Wave function)

Aufbau Principle

to determine the electron configuration of atoms in their ground (lowest energy) state.

Paul Exclusion principle

each electron in an atom have a unique quantum number

HunD’s Rule of maximum multiplicity

requires that electrons be placed in orbitals to give the maximum total spin possible (the maximum number of parallel spins).

degenerate

have the same energy