FAIR USE STATEMENT :
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FAIR USE STATEMENT: Please feel free to edit and use this presentation in your
classroom. Please do not remove the credit line on the title page or republish the file in whole or in part as your own. Please do not distribute the file to individuals or at conferences or workshops. I am more than willing to share the presentation with anyone that contacts me at [email protected]. The images used in the presentation are not original and the presentation is distributed freely but only for classroom instruction.
Rhonda Alexander
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Principle quantum numberDepends on energy leveln=(1,2,3, …)
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Azimuthal quantum number
Shape of orbital-depends on location on periodic chart
If s block then l=0If p block then l=1If d block then l=2If f block then l=3
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Atomic Orbitals1 – s
3 - p
5 – d
7 - f
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Atomic Orbitals
d - orbitals
l ranges from 0 to n-1. If n=1, then l=0 If n=2 then l=0,1 If n=3 then l= 0, 1, 2
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Angular Quantum Number
• ml represents the individual orbitals of a given type.
• ml ranges from –l to +l
• ml tells you which p, d, or f orbital the electron is in
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Magnetic Quantum Number (ms): Spin
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QuantumNumbers
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Quantum Numbers
• n = integer from 1 to 7• l = 0 to n-1
• ml = -l to +l
• ms = 2
1or
2
1
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HOW DO WE DESCRIBE THE LOCATION OF EACH ELECTRON IN AN ATOM?
WITH A SYMBOLIC NOTATION CALLED AN ELECTRON CONFIGURATION.
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An Electron Configuration is a shorthand method of listing the location of the electrons in an atom. The system locates each electron by energy level and sublevel. The number of electrons in each sublevel is indicated with a superscript. For instance, the electronic configuration of Sodium is 1s22s22p63s1.This indicates that there are two electrons located in the 1s orbital, two electrons in the 2s orbital, six electrons in the 2p orbital and a single electron in the 3s orbital.
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Remember:
ENERGY
LEVEL 1 2 3 4 SUBLEVELS s s p s p d s p d f
NUMBER OF
ORBITALS IN
SUBLEVELS
1 1 3 1 3 5 1 3 5 7
MAXIMUM
# OF e IN
SUBLEVELS
2 2 6 2 6 10 2 6 10 14
MAXIMUM
3 OF e IN
ENERGY LEVEL
2 8 18 32
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Filling Orbitals
Follow rules of modern atomic model:Aufbau Principle -electrons fill from lowest energy level first
Hund’s Rule -have maximum number of unpaired electrons
Pauli Exclusion Theory -no electron has same set of quantum numbers because of electron spin
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1. Electrons occupy lowest energy orbitals first.
2. An orbital can hold a maximum of 2 electrons. The Pauli Exclusion Principle must be obeyed.
3. Hund's Rule must be obeyed; when placing electrons into degenerate orbitals, there must be one electron in each orbital before any pairing of electrons can take place. {Degenerate orbitals are orbitals of the same energy level and sublevel.}
RULES FOR PLACING ELECTRONS IN ORBITALSRULES FOR PLACING ELECTRONS IN ORBITALS
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Aufbau Diagram
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The Order Electrons Fill The Order Electrons Fill OrbitalsOrbitals
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__ __ __ __ __ __ __ __ __ __ 5s 4d 5p 6s
__ __ __ __ __ __ __ __ __
1s 2s 2p 3s 3p__ __ __ __ __ __ __ __ __
4s 3d 4p
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Electron Configuration of ZrElectron Configuration of Zr
1s2 2s2 2p63s2 3p6 4s2 3d10 4p6 5s2 4d2
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Practice
• Write the electron configuration of the following on a separate page.– Oxygen– Lithium– Iron– Bromine– Tin
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Core Notation of SnCore Notation of Sn• Locate Sn on the periodic table
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Electron Configuration of SnElectron Configuration of SnSn [Kr]
• The noble gas core is Kr
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Sn [Kr]5s2
• The noble gas core is Kr
• From Kr, go 2 spaces across the s-block in the 5th row 5s2
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Sn [Kr]5s24d105p2
• The noble gas core is Kr
• From Kr, go 2 spaces across the s-block in the 5th row 5s2
• Then go 10 spaces across the d-block on the 5th row 4d10
• Finally go 2 spaces into the p-block on the 5th row 5p2
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Steps
• Locate the element
• Go to the end of the row and up 1 noble gas
• Write the Noble gas core in brackets
• Continue electron configuration with the next period
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• Refer to a periodic table and write the electron configurations of these atoms. Use the noble gas core.
• Zn
• I
Nobel Gas (Core) & Orbital DiagramNobel Gas (Core) & Orbital Diagram
[Ar]4s23d10
[Kr]5s24d105p5
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4s 3d
5s 4d
5p
•Zn [Ar]4s23d10
•I [Kr]5s24d105p5
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Quiz - Quantum Numbers
1. Zn
2. Sb
3. Cs
4. .n = 4.l = 3.ml = -3.ms = -1/2
.n = 3
.l = 2
.ml = +2
.ms = -1/2
.n = 5
.l = 1
.ml = +1
.ms = + 1/2.n = 6.l = 0.ml = 0.ms = +1/2
Tb
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The Periodic Table
•Is a table that arranges the elements according to similarities in their properties.
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Dmitri Mendeleev
Father of the Periodic Table
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Mendeleev’s Periodic Table
(63 known elements)
Developed the Periodic Law that said: - columns arranged by increasing atomic mass (not correct) - rows arranged by chem. & physical properties
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Mendeleev’s Table (cont.)
•Concluded gaps in table were elements yet to be discovered.
•- led to the search for missing elements
•- predicted existence of aluminum, boron, silicon, germanium
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Predicted Properties Observed PropertiesAtomic weight 72 72.61Density 5.5 g/cm3 5.32 g/cm3
Melting point 825 C 938 COxide formula RO2 GeO2
Density of oxide 4.7 g/cm3 4.70 g/cm3
Chloride formula RCl4 GeCl4
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Mendeleev’s Original Table
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Modern Periodic Table- Developed by Henry Moseley
- Solved problems in Mendeleev’s table.- Periodic law is based on increasing
atomic #, NOT atomic mass.
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Structure of the Periodic Table
periods: rows going across, numbered 1-7
groups: columns going down, numbered 1-18; aka families- Elements w/in groups have similar physical and chemical properties.
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The Metals
•located left of zig-zag or stair-step
Properties - good conductors
- lusterous- malleable
- ductile
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The Nonmetals
•located right of zig-zag or stair-step
•Properties:dull; brittle;
poor conductors,
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The Metalloids
• Border zig-zag / stair-stepexcept aluminum and polonium
• Properties:- some metallic- some nonmetallic- semi-conductors
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Transition Metals
Inner Transition Metals
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18IA IIA IIIA IVA VA VIA VIIA
VIIIA
Representative Elements
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Transition Metals
Inner Transition Metals
Elements:
Alkali Metals
Halogens
Lanthanides
Metals Nonmetals Metalloids Transition Metals Inner Transition Groups/Families:
Alkali Earth Metals
Noble GasesActinides
nonmetalsmetals
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Key Terms• Atomic radius – ½ distance btwn
nuclei of two atoms in a molecule.• Ionization energy – amt. of energy
needed to remove an e- from an atom.
• Electronegativity – tendency for an atom to attract e-
• Valence e- - e- on outermost energy level.
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1 valence electron
2 valence electrons
3 valence electrons
4 valence electrons
5 valence electrons
6 valence electrons
7 valence electrons
8 valence electrons
Electrons in the outermost level are called valence electrons.
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Element Families
Group 1) Alkali Metals (I A) - highly reactive, especially with water - 1 valence e-
- loses valence e-
- become 1+ ions
Li, Na, K, Rb, Cs, Fr
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Group 2) Alkaline Earth Metals (II A)
- very reactive but less than group 1- 2 valence e-
- lose valence e-’s- become 2+ ions
Be, Mg, Ca, Sr, Ba, Ra
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Groups 3-12) Transition Metals (B) - most have 2 valence e-, some with 1 or more - all lose valence e-
- several become 2+ ions
Sc Ti V Cr Mn
Fe Co Ni Cu Zn
Y Zr Nb Mo
Tc Ru Rh Pd Ag Cd
Lu Hf Ta W Re Os Ir Pt Au Hg
Lr Rf Db Sg Bh Hs Mt
3 4 5 6 7 8 9 10 11 12
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Group 17) Halogens (VII A) - highly reactive - form cmpds called halides - fluorine most reactive element - 7 valence e-
- Gain 1 e-
- become 1- ions
F, Cl, Br, I, At
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Group 18) Noble Gases (VIII A) - not reactive (inert) - cmpds formed only under special conditions - full outer energy level (8 valence e-) except He, 2 valence e-
He, Ne, Ar, Kr, Xe, Rn
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Other Groups/Families
Group 13: 3 valence e- (IIIA) 14: 4 valence e- (IVA) 15: 5 valence e- (V A)
16: 6 valence e- (VI A)
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Periodic TrendsAtomic Radius
INCREASEINCREASES
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Atomic Radii
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Ionization Energy
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Periodic Trends
Ionization Energy
INCREASES
INCREASES
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Ionization Energy
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Periodic Trends
Electronegativity
O
M
I
T
INCREASES
INCREASES
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Electronegativity
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Ion Radius