Chem - Unit 4 Electrons

Sublevel F (flower)

7 orbitals, 14 total electrons

Sublevel D (Clover)

5 orbitals, 10 total electrons

Sublevel S (sphere)

1 orbital, 2 total electrons

Sublevel P (dumbell)

3 orbitals, 6 total electrons

In 5s², 5=

principal energy level

In 5s², s=

sublevel type

In 5s², 2=

number of electrons in the sublevel

Aufbau Principle

A rule that states electrons occupy the lowest energy orbitals first before filling higher energy levels.

Hund’s Rule

Electrons will fill all orbitals on a sublevel first before filling rest of orbital (empty bus seat)

Pauli Exclusion Principle

Each orbital can only hold two electrons of opposite spin

Wavelength

In equation c=λv, what does λ stand for

Speed of light

In equation c=λv, what does c stand for

Frequency

In equation c=λv, what does v stand for

Planck’s constant

In E=hv, what does h stand for?

energy

In E=hv, what does E stand for?

frequency

In E=hv, what does v stand for?

Inverse

Relationship between wavelength and frequency

Violet

Which color of light has the highest energy?

Excited electron

Gives off energy in form of light

Column number of periodic table

number of valence electrons

Dalton’s Model (1803)

Atoms are indivisible, indestructible particles

Thomson’s Plum Pudding Model (1897)

Atoms are positively charged spheres with negatively charged electrons scattered throughout (cathode ray tube)

Rutherford’s Nuclear Model (1911)

Atoms have small, dense nucleus containing positively charged protons, with electrons orbiting around the nucleus (gold foil experiment)

Bohr’s Planetary Model (1913-1923)

Special orbits and energy levels, quantized energy levels, limitations (hydrogen only)

Quantum Mechanical model (1926)

Atoms consist of nucleus with protons and neutrons, surrounded by electron clouds representing areas of electron probability

Wave-particle duality

Louis de Brogelie’s idea that electrons exhibit both wave and particle properties

Heisenberg’s Uncertainty Principle

It’s impossible to known both the exact position and momentum of a particle simultaneously

Schrodinger’s contributions

developed mathematical equations describing electron behavior, leading to concept of orbitals