warm-up – you’ll need a periodic table and page 8 of the formative assessment
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Warm-up – You’ll need a periodic table and page 8 of the formative assessment. What type of light has a wavelength of 1 x 10 -11 m? What type of light is released when an electron jumps from = 4 to n = 1 in a Hydrogen atom? What type of light has a wavelength of 6.3 x 10 -7 m? - PowerPoint PPT PresentationTRANSCRIPT
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Warm-up – You’ll need a periodic table and page 8 of the formative assessment
What type of light has a wavelength of 1 x 10-11 m? What type of light is released when an electron
jumps from = 4 to n = 1 in a Hydrogen atom?What type of light has a wavelength of 6.3 x 10 -7m?Is light energy released or absorbed in the following
jumps of an electron in a Hydrogen atom?n=1 to n = 3 n = 2 to n = 5 n = 6 to n = 3n = 2 to n = 3
Rank the following types of light in increasing energy:
X – ray, green light, microwaves, violet light.
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Unit Three, Day ThreeKimrey
19 September 2010
Chemistry
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Atomic TheoryOrbital: 3-D regions around the
nucleus where electrons are foundElectrons are all in constant, random motion
The current atomic theory is based on probability
Electron configuration describes the most likely location of the electron in an atom.
It breaks the electron cloud into energy levels, sublevels, and spin direction
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Quantum Numbers
Numbers used to describe where the electron is in the atom
There are four different quantum numbers
Today, we’re going to focus on the first two
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Principle Quantum Number (n)
Tells the energy level of the electronNumbers 1 through 7
1 – smallest orbital, closest to nucleus, lowest energy
7 – largest orbital, farthest from nucleus,
highest energy
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Orbital Quantum Number (l)Tells the shape of the orbitalAlso called a sublevel
s – sphere shapedExists on every energy level (1-7)
p – peanut shapedOnly exists on energy levels 2-7
d – daisy shapedOnly exists on energy levels 3-7
f – “funky”Only exists on energy levels 4-7
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Energy levels based on location
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How many electrons can fit in each sublevel?
The s sublevel can hold up to 2 electrons
The p sublevel can hold up to 6 electrons
The d sublevel can hold up to 10 electrons
The f sublevel can hold up to 14 electrons
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Electrons will completely fill up the first sublevel they get to before moving on to the next oneElectrons like to be close to the nucleus
Remember the hotel… the boys don’t want to have to climb the stairs
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Electron ConfigurationAll of this will help us to write the
electron configuration for elementsEACH ELECTRON MUST BE
ACCOUNTED FOR!!So, it is extremely important that
you know how to determine how many electrons are present in a specific isotope. If you’re still struggling with this, you’ll be getting lots of practice in the next few days, don’t worry.
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The diagonal rule
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PracticeLet’s start with Hydrogen.
Has only 1 electron (in its neutral state) The electron must be in the orbital closest to
the nucleus. That orbital is number 1The only sublevel in the first orbital is s
H 1s1
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Helium isn’t much more difficult
Has 2 electronsThe electrons must be in the orbital closest
to the nucleus. That orbital is number 1The only sublevel in the first orbital is s
He 1s2
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A little tougher…Lithium
Has 3 electronsOnly 2 can fit in an s sublevel, so the first
orbital is filled with the first two electronsThe one that’s left has to move to the second
orbital (since only two electrons are allowed in the first)
It goes in the first sublevel there
Li 1s22s1
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Let’s do a harder oneOxygen
First, how many electrons?How many can go in the first orbital, and
what sublevel are they in?Now, how many can fit in the second orbital?How many of those go in the first (s)
sublevel?How many are left and which sublevel are
they in?
O 1s22s22p4
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Lots of practice!!!
NitrogenCalciumFluorineSulfurSodium
1s22s22p3
1s22s22p63s23p64s2
1s22s22p5
1s22s22p63s23p4
1s22s22p63s1
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Now, look at ManganeseHow many electrons???
Mn 1s22s22p63s23p64s23d5
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More PracticeYSeRbGeAr
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Noble GasesElements in group 18 of the periodic
tableThese elements are the most stable
of the elements because their outer energy level is full
Helium, Neon, Argon, Krypton, Xenon, and Radon
We can use the noble gases as a short-cut with electron configuration
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Noble Gas Configuration - short-hand method Count the number of electrons in the
atomFind the Noble Gas with the closest
(BUT NOT GREATER THAN) number of electrons to the atom you are working on.
Use brackets [ ] and the noble gas symbol to represent the number of electrons equal to the noble gas
Write the remainder of the electron configuration normally
Ex: Fe – 26 electrons : [Ar] 4s2 3d6
[Ar] represents the first 18 electrons; 4s2 3d6 represents the remaining 8
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Try these again now.YSeRbGeAr
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You still have to know how to do the long-hand, electron configuration!
NaArFeBa