Chemistry Ch. 4 Review

History

100

created first model to include atoms of each element having different masses

Dalton

200

proposed principal energy levels for orbitting electrons to help explain line spectra

Bohr

300

first to refer to smallest particles as atoms

Democritus

400

subatomic particles discovered with cathode rays

electrons

500

James Chadwick discovered (subatomic particles)

neutrons

Numbers

100

azimuthal quantum numbers

sublevels (s, p, d, f)

200

1st quantum number tells

principal energy level

300

protons + neutrons =

mass number

400

weighted average

atomic mass

500

energy emissions come in certain QUANTITIES because levels are

quantized

Electron location

100

number of sublevels in energy level 3

3 (s, p, d)

200

number of electrons possible in energy level 4

32

300

orbital notation for O 

<>  <>  <>  <  < 

400

electron configuration for C

1s^2

2s^2

2p^2

500

found in all principal energy levels

s

Principles/Rules

100

impossible to know both energy and exact position of electron

Heisenberg uncertainty 

200

Pauli exclusion:

no two electrons can have same 

4 quantum numbers

300

Hund's rule:

how electrons fill

sublevel

400

Aufbau principle: 

how electrons fill...

orbitals

500

any sample of same compound always contains same % of each element

law of definite composition

Practice

100

Isotopic notation: 23 protons, 52 neutrons

⁵² ₂₃ X

200

Protons, neutrons, electrons in

¹⁰⁴ ₆₃ X

63 p & e

41 n

300

dot notation: Neon

      --

--   Ne --

      --

400

potassium noble gas (abbreviation) notation

[Ar] 4s¹

500

atomic mass:

35.67%  at 42.3362

64.33% at 40.9768

(15.1013) + (26.1673)

41.2686