Flame Test - Electron Config - Quantum Theory

Bohr's Planetary Model

Model stating that electrons travel around the nucleus in specific energy levels/orbits, similar to planets around the Sun.

Evidence for Bohr's Model

Heated matter produces only specific wavelengths/colors of light, theorized to come from electrons transitioning between energy levels.

Energy Level

A specific allowed energy an electron can have in an atom.

Ground State

The normal, lowest-energy state of an electron.

Excited State

A higher-energy state reached when an electron absorbs energy and jumps to a higher energy level.

Photon

A particle of light energy.

Absorption of a Photon

An electron absorbs energy and jumps UP to a higher energy level.

Emission of a Photon

An electron falls DOWN to a lower energy level and releases a photon.

Energy Gap

Difference in energy between two electron energy levels; larger gap produces higher-energy photon.

Atomic Emission Spectrum

Lines of specific colors separated by dark areas produced when excited electrons fall to lower energy levels and emit photons.

Heisenberg Uncertainty Principle

It is impossible to know both the exact position and velocity of an electron at the same time.

Schrödinger's Quantum Mechanical Model

Model that uses wave equations to describe regions with a high probability of finding electrons.

Orbital

A 3-D region of high probability for locating an electron.

Sublevel

A division within an energy level labeled s, p, d, or f.

s Sublevel

Has 1 orbital and can hold a maximum of 2 electrons.

p Sublevel

Has 3 orbitals and can hold a maximum of 6 electrons.

d Sublevel

Has 5 orbitals and can hold a maximum of 10 electrons.

f Sublevel

Has 7 orbitals and can hold a maximum of 14 electrons.

Shape of an s Orbital

Spherical.

Shape of a p Orbital

Dumbbell shaped.

Shape of a d Orbital

Mostly four-leaf clover shaped; one resembles a dumbbell with a donut.

Number of Orbitals in s, p, d, f

s = 1, p = 3, d = 5, f = 7.

Maximum Electrons in s, p, d, f

s = 2, p = 6, d = 10, f = 14.

Aufbau Principle

Electrons occupy the lowest available energy levels first.

Pauli Exclusion Principle

There cannot be more than 2 electrons in each orbital , and the 2 must spin in opposite directions

Hund's Rule

Within a sublevel, each orbital gets one electron before any orbital gets a second electron.

Camp Electron: Camper

Represents an electron.

Camp Electron: Cabin

Represents a sublevel such as 1s, 2s, or 2p.

Camp Electron: Bunk

Represents an orbital.

Camp Electron Rule: Lowest Cabin First

Represents the Aufbau Principle.

Camp Electron Rule: Maximum Two Campers per Bunk

Represents the Pauli Exclusion Principle.

Camp Electron Rule: One Camper in Each Bunk Before Pairing

Represents Hund's Rule.

1s²

1 = first energy level, s = s sublevel, and ² = 2 electrons in that sublevel.

2p⁶

2 = second energy level, p = p sublevel, and ⁶ = 6 electrons in that sublevel.

Electron Filling Order Around the f Sublevel

5p → 6s → 4f → 5d → 6p.

Why does 4f fill after 6s?

Sublevels fill according to energy, not simply according to the number in front of the letter.