Download Ch10-Atomic Theory

Ch. 10- Modern Atomic Theory
Rutherford’s Atom- but where are
the electrons really?
The positively
charged nucleus
deflects some of
the alpha particles!
What is the nucleus
made up of ?
Key Vocab 10.2
Electromagnetic radiation- energy (_____)
transferred in the form of ___________
waves
Wavelength (__) –
distance b/w ___
__________ wave
peaks
Frequency (___) – the # of wave peaks that
pass a __________ per given ____________
photons- a _________ of electromagnetic energy,
its energy is proportional to its __________ (___)
The equations that deal with
energy of ER radiation
E=
λ=
What is the frequency of red light, with a
wavelength of 7.000 x 10¯5 cm?
What is the frequency of blue light, with a
wavelength of 475 nm?
Problems
What is the frequency of red light, with a
wavelength of 7.000 x 10¯5 cm?
What is the frequency of blue light, with a
wavelength of 475 nm?
Determine the E of each. Which will be
higher in E?
Real-life Chemistry- Global Warming
10.3 Emission of Energy by Atoms
Energy from flame is absorbed by the ions in solution
1. atoms/ions get excited
2. excess energy released in form of
_____ as atom moves to a lower energy of
state and
3. emits _______ of light
Applications:
Notes about burning rainbows
Metal ion (from cmpd?)
Color of Flame
The Bohr Model and Quantized Energy Levels
Niels Bohr’s model of the H atom:
1885-1962
-quantized energy levels
-circular orbits (we know this is not true
now!)
Quantized Energy Levels
Excited atom- an atom with excess energy
(it’s the ______ that are being excited)
Ground state- lowest possible energy state
The energy in the released photon =
Poor Bohr…not quite correct!
Orbitals are nothing like orbits!!
1921- Louis de Brogllie introduces
wave/particle duality of matter
Schrödinger- develops Schrodinger eq’n
to better approx. behavior of
atoms more complicated
than hydrogen (1926)
The quantum (wave)
mechanical model
Orbital – potential area of space where the
electron may be
Principal energy levels are quantized
The shapes
Quiz: Section 10.9
What are valence electrons, what are core
electrons, and which ones are the important
ones for bonding?
Electron Spin
Pauli Exclusion Principle- an atomic orbital
can hold a maximum of two electrons, and
those two electrons must have opposite
spins
1st things 1st: Vocabulary time
Electron configuration: the pattern of how
the e’s of an element fill into available
orbitals
Ex: Li: 1s22s1
Orbital diagram: a representation of electron
configuration using arrows for the electrons
Two more vocab terms before act-out 
Valence electrons – the electrons in the
highest principal energy level, the most
important for bonding!
Core electrons – the inner, non-bonding
electrons
Bitty Bit of Review, then Some New
Write out the full electron configurations of
the following:
N:
Si:
V:
Some rules for e. configs.
• The s orbitals of the n+1 level will fill
before the ___________ of the ____ level
• The lanthanide series are the elements
that fill in the ____ orbitals
• The actinide series are the elements that
fill in the ____ orbitals
Determine the abbreviated electron configurations
for the following and give the number of valence
electrons
Sr:
Mo:
As:
Main-group elements
Elements in groups 1,2, 13-18
Every member of a group has the same
____________ but these electrons are in
different ____________
Atomic Properties
Metals-have luster
-ductile (pulled into
-conductors of
pounded to
+
Atomic Properties
Non-metals
-opposite of metals
Metalloids
-elements that show both _______ and
___________ properties
Atomic Properties
Ionization Energy Trends
Atomic Properties
Atomic Size