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Vocabulary:
AMU
Atom
Atomic emission spectrum
Atomic mass
Atomic number
Chemical reaction
Compound
Distillation
Electron
Element
Frequency
Heterogeneous mixture
Homogeneous mixture
Isotope
Mass
Mass number
Mixture
Neutron
Nucleus
Phase
Photon
Product
Proton
Quantum
Reactant
Spectrum
Vapor
Wavelength
I. The History of Atomic Structure:
A.
B.
C.
D.
E.
F.
G.
H.
I.
J.
K.
Democritus
Aristotle
John Dalton
1.
Dalton’s Atomic Theory
a)
All matter is composed of atoms
(1)
Dalton’s atom – an indestructible, indivisible particle
(2)
All atoms of the same element are identical
(3)
Atoms of different elements are different
(4)
Atoms unite in whole number, fixed ratios to form compounds
b) Dalton’s Atomic Model JJ Thompson
1.
Thompson’s Experiment – Cathode Ray Tube Experiment
2.
Thompson’s Discovery – The electron
3.
Thompson’s Atomic Model –
Plum Pudding Model – An atom is mostly positive charge, with some negatively charged
electrons stuck in it.
Ernest Rutherford
1.
Rutherford’s Experiment – Gold Foil Experiment
2.
Rutherford’s Discovery – Disproved Thompson’s Plum Pudding Model
3.
Rutherford’s Atomic Model –
Nuclear Atom Model – An atom is mostly empty space with a dense, positively charged nucleus
in the center and electrons moving around it.
Neils Bohr –
1.
Bohr’s Experiment – Used atomic spectra to describe how atoms absorb and emit light
2.
Bohr’s Discovery - Electrons are only found in specific circular paths around the nucleus
3.
Bohr’s Atomic Model Planetary System Model – Electrons move around the nucleus of an atom, like the planets
around the sun.
James Maxwell – Proposed that visible light consists of electromagnetic waves.
Maxwell Planck – Suggested that atoms and molecules emit energy in discrete quantities, called quantum
Albert Einstein Einstein’s Discovery – Photoelectric Effect
Einstein’s Theory - Beam of light behaves like a stream of particles
Louis DeBroglie - Determined that light as properties of both waves and particles.
Erwin Schrodinger - Describes motion of electrons using complicated mathematical equations
Schrodinger’s Atomic Model Although not Schrodinger’s, his work gave way to the modern atomic theory, and the electron
cloud model.
II.
The Parts of the Atom
Proton
Neutron
Electron
III.
Atomic Symbols
Atomic Mass
A
# Protons + # Neutrons
Z
Atomic Number
# Protons
Element Symbol
Isotopes – Atoms of elements with the same # of protons, but different #s of neutrons.
Atomic Mass Unit – 1/12th the mass of a carbon atom containing 6 p+ and 6 n0.
X
Example Problem:
Atomic
Element Number Protons Neutrons Electrons
130
Te
52
50
37
27
Al
Europium
89
Element
Example Problems:
1) Determine Average atomic Mass:
Calculate the average atomic mass of bromine. The two isotopes of bromine have atomic masses and relative
abundances of 78.92amu (50.69%) and 80.92amu (49.31%).
2) Determine Percent Abundance given the average atomic mass.
The average atomic mass of element X is 10.810amu. Element X has two isotopes, 10X and 11X. If isotope 10X
has a mass of 10.012 amu and isotope 11X has a mass of 11.009, what is the percent abundance of each?
IV.
Waves – a vibrating disturbance by which energy is transferred.
A.
Wave Types
1.
Longitudinal Wave – Particle displacement is parallel to wave propagation
2.
Transverse Wave – Particle displacement is perpendicular to wave propagation.
B.
Parts of a Wave
4.
Amplitude
1.
Crest
5.
Frequency
2.
Trough
6.
Midline
3.
Wavelength
C.
Important Info from the Electromagnetic Spectrum
1.
Name different regions of electromagnetic radiation
Radio, Radar, Microwaves, Infrared, Visible light, Ultraviolet, X-Rays, Gamma Rays
2.
3.
4.
V.
As wavelength decreases, frequency increases. (Inversely proportional)
As frequency increases, energy increases. (Directly proportional)
The region of visible light (ROYGBIV) on the EMS is 700 nm (Red) to 380 nm (Violet)
Equations, Variables, and Constants.
c = speed of light
λ = wavelength
υ = frequency
E = Energy
h
= Planck’s constant
☺
m = mass
u☺ = wave velocity
c = λυ
E = hυ
λ = h / mu
=
3.00x108 m/s
measured in m or nm
measured in Hz = 1/s
measured in J = kg*m2 / s2
=
6.626x10-34 J*s
measured in g or kg
NOT SPEED OF LIGHT!
(1 m = 1x109 nm)
(1MHz = 1x106 Hz)
(1kJ = 1x103 J)
(1kg = 1x103 g)
(1 m/s = 2.24 mi/hr)
Please reference your homework worksheets or www.vvhomework.org for example problems and answers.