Chemistry – Chapter 5 Study Guide

Vocabulary

* Amplitude – Amount of a signal, height of a wave crest
* Atomic emission spectrum – set of frequencies of the electromagnetic waves given off by elements
* atomic orbital – shape of the path in which electrons travel
* electromagnetic radiation – Form of energy that exhibits wavelike behaviors as it travels through space
* electron-dot structure – Method of showing elements, and their electrons/valence electrons
* energy sub-levels – S,P,D, and F Orbitals
* frequency – number of waves that pass a given point per second (Hertz)
* ground state – Lowest allowable energy state of an element
* photoelectric effect – electrons come off of metal and are absorbed by non-metals
* photon – Particle of an electromagnetic radiation without any mass
* principal energy levels – Major energy level in the Bohr’s model
* principal quantum number – Indicate relative size
* Quantum – Minimum amount of energy needed for a chemical change (element losing/gaining an electron)
*Valence Electrons – Electrons in the outer shell that can easily jump to it, or jump away from it, to become stable
* Wavelength – Distance from crest to crest

Concepts & Equations

Aufbau Principle – The first energy level fills up before the next orbitals fillup. The last electron is the valence electron; ordered from lowest -> greatest energy

Bohr’s Atomic Model – Model of an element were the nucleus is in the middle and electrons travel in orbitals around the well defined nucleus

deBroglie’s equation – idk & studied wave nature of electrons

Heisenberg Uncertainty Principle – States that you can’t accurately measure where the electron is because if you can see it, your effecting it, thus it isnt innocent anymore and can’t be used to pinpoint elements exactly

Hund’s Rule – Each Degenerate orbital gets 1 electron before they can pair

Pauli Exclusion Principle – no two electrons can raise the same four quantum numbers, no more than 3