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So What is The Atom?
Mr. BarnerChemistry
Atoms in Space!
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Three Major Particles
• J.J. Thompson Discovered Electron
• Used Cathode Ray Tube• Found in TV sets, computer monitors
• 1/2000 the mass of Hydrogen
• Negatively Charged – e-1
• First Sub-Atomic Particle• Each Element has a fixed number of
electrons
-1
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Henry Mosely
• Positive Sub-Atomic Particles called Protons
• Every Atom of an Element has same Number of Protons
• Assigned Atomic Number
• Equal to # of Protons
• Identifies Element
•Modern Periodic Table
+1
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James Chadwick
• Discovered a Neutral Particle - Neutron
• Was not affected by electric or magnetic forces.
• Atoms can have different amounts of Neutrons - Isotopes
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Atom has Three Basic Particles
Atomic Number
Protons
+1 Charge
1 mass unit
Electrons
-1 Charge
1/2000 mass units
Mass Number =
Protons +Neutrons
Neutrons0 charge1 mass unit
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Element Symbols as Models
1021Ne
ElementSymbol
Atomic Number10 Protons
10 Electrons
Mass Number10 Protons + 11 Neutrons
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Three Isotopes of HydrogenSame Element – Different Mass
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Isotopes of Carbon have the same number of protons but different numbers of
neutrons.
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The Atomic Weight Reflects the Abundance and Mass of Each Isotope.
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Atomic Number is the Number of Protons or Electrons
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Mass Number Tells How Protons and Neutrons
H - 1
C - 12
U - 238
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Parts of an Atom
Complete the TableIsotope Atomic
Number Mass
Number Protons Neutrons
8135Br
81 123
12 25 92 41 31 15
7835Br
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IonsCations – have a shortage of electrons
+1 charge means one less e-+3 charge means 3 less e-
Anions – have an excess of electrons-1 charge means one extra e--2 charge means 2 extra electrons
The charge is shown in superscript
22512
MgCharge +2
10 Electrons
12 Protons
12 Protons + 13 Neutrons
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Parts of an IonComplete the Table
Isotope Atomic Number
Mass Number
Protons Neutrons Electrons
3517Cl
1-
15 31 18
15 33 18 20 41 18 47 60 46
3116S
2-
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CationsCations:
1. _______________ charged particles
2. _______________ of electrons = positive charge
3. _______________ are +1 and
_______________ are + 2;
Aluminum is +3, Zinc is +2, and Silver is +1
4. _______________ Numerals in ( ) are added to all other Cation names.
POSITIVELY
SHORTAGE
GROUP 1
GROUP 2
ROMAN
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22512Mg
26630 Zn
Name Symbol Protons Electrons Neutrons Mass Number
Magnesium 12 10 13 25
19 18 39
Nickel (II) 29
13 10 27
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ANIONS1. _________________ charged
particles2. _________________ of electrons =
negative charge3. _________________ is -1,
_________________ is -2, and _________________ is -3
4. _________________ goes at the end of Anion names
NEGATIVELY
EXCESS
GROUP 17
GROUP 16GROUP 15
-ide
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1199F
23216S
Name Symbol Protons Electrons Neutrons Mass Number
Fluoride 9 10 10 19
17 18 36
Phosphide 16
6 10 7
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Quantum Model of the Atom
Central NucleusExtremely small~all the massAll the positive chargeProtons & Neutrons
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The Nucleus Would be like a Baseball in the Center of the Houston Astrodome.
MOST of the atom is EMPTY space Most of the MASS is in the NUCLEUS The motion of the ELECTRONS provide the SIZE and
HARDNESS of the atom.
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First Property
All electrons SPINThey can spin clockwise
Called an up spin - ↑They can spin
counterclockwiseCalled a down spin - ↓
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North
North
Clockwise SpinCounter-clockwise Spin
Electron Spin
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Orbitals Electrons form a CLOUD They move RANDOMLY Cannot predict exact LOCATION and
EXACT MOTION The clouds has specific shapes – ORBITALS The ORBITAL cloud is made from ONE or
TWO electrons ORBITAL DIAGRAMS 2 Electron cloud ( ↑↓)
1 electron clouds (↑ ) OR ( ↓)
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Orbitals can come in different shapes
“s” shape “Simple” shape Spherical Can hold up 2 electrons Lowest energy
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The next shape – “p” Three similar orbitals Each orbital is along a 3-D axis Each orbital have up to 2 electrons Slightly higher energy than “s” orbital
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2py
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2pz
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2px
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The third shape – “d” 5 different orbital shapes 4 of the orbitals look like 4-leaf clovers 5th orbital looks like a fan blade with a
ring Each orbital can have up to 2 electrons Total of 10 electrons
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“d” orbitals
z-axis
x-axis
y-axis
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“d” orbitals
z-axis
x-axis
y-axis
z-axis
x-axis
y-axis
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dz2
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dxy
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dxz
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dyz
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dx2 - y2
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The forth shape – “f”• Very complex shapes
• There are 7 shapes that are called “f” orbitals
• They all have the same energy at the same size
• Each “f” orbital can have up to 2 electrons
• Total of 14 electrons
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Seven “f” shapes
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Seven “f” shapes
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Seven “f” shapes
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Seven “f” shapes
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Seven “f” shapes
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Seven “f” shapes
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Seven “f” shapes
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Putting Electrons in Orbitals
• Only at most two electrons in an orbital - ↑ and ↓• Orbitals of same shape are made
with one electron before pairing.( ) ( ) ( ) is OK
Three orbitals with electrons of same spin
() ( ) ( ) Must make third orbital before pairing
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Orbitals together make aSublevel
• The “s” sublevel• Only one orbital –
spherical• Maximum of 2
electrons• The “p” sublevel• Made of the three
orbitals• Maximum of 6
electrons
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More sublevels
• The “d” sublevel• Made of the five
“d” orbitals• Maximum of 10
electrons• Very high energy
as very restrictive
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More Sublevels
• The “f” sublevel•Made of the seven “f” orbitals
•Maximum of 14 electrons
•Highest energy as MOST restrictive
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Finally we make a complete ENERGY LEVEL
• Each level surrounds the nucleus• The levels are numbered
1, 2, 3, 4, 5 … n• The levels get larger so can
hold “n” sublevels
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Energy Levels
• Level n = 1•Only 1 sublevel
•Titled 1s•1st Level, “s” sublevel
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Energy Levels
• Level n = 2•Contains 2
sublevels• 2s = 2nd Level,
“s” orbital• 2p = 2nd Level,
“p” orbitals
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Energy Levels
• Level n = 3
•Contains 3 sublevels• 3s = 3rd level, “s” orbital
• 3p = 3rd level, “p” orbitals
• 3d = 3rd level, “d” orbitals
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Energy Levels
• Level n = 4
•Contains 4 sublevels• 4s = 4th level, “s” orbital
• 4p = 4th level, “p” orbitals • 4d = 4th level, “d” orbitals • 4f = 4th level, “f” orbitals
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Levels, Sublevels & OrbitalsLevels Sublevels Orbitals Electrons
1st s only 1s2 2
2nd s & p 2s2 2p6 8
3rd s, p & d 3s2 3p6 3d10 18
4th s, p, d & f 4s2 4p6 4d10 4f1432
Complete the chart up to n = 7!
After f comes g, h, and i
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Placing Electrons into the Atom
Tempe AZ Town Hall is Like an Atom Fill the Levels Top to Bottom
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Filling an Orbital Diagram• ( ) represents an orbital, electron cloud
• ↑↓ represent the electron placed in an orbital
• Fill Orbitals from lowest energy to highest energy
• Orbitals of same energy are given one electron at a time BEFORE pairing
• Simple orbitals of larger clouds are less energy than complex orbitals
• 4s < 3d
• 6s < 4f
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Electron Configuration
• Shows the levels and sublevels formed by the electrons - 1s 2s 2p• Considers that 4s < 3d and 5s < 4d• Use superscripts to show the number
of electrons in each sublevel• Total of superscripts is the Atomic
Number• 1s2 2s2 2p6 3s2 --> = 12, Mg
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Diagonal Rule1s2
2s2
3s2
4s2
5s2
6s2
7s2
2p6
3p6
4p6
5p6
6p6
7p6
3d10
4d10
5d10
6d10
7d10
4f14
5f14
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More Configurations
9F 1s2 2s2 2p5
11Na 1s2 2s2 2p6 3s1
14Si 1s2 2s2 2p6 3s2 3p2
18Ar 1s2 2s2 2p6 3s2 3p6
19K 1s2 2s2 2p6 3s2 3p6 4s1
22Ti 1s2 2s2 2p6 3s2 3p6 4s2 3d2
29Cu 1s2 2s2 2p6 3s2 3p6 4s2 3d9
33As 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3
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Terminar
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All the Energy LevelsDiagonal Rule
1s2
2s2
3s2
4s2
5s2
6s2
7s2
2p6
3p6
4p6
5p6
6p6
7p6
3d10
4d10
5d10
6d10
7d10
4f14
5f14
6f14
7f14
LevelSublevel Maximum
Electrons
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Filling LevelsDetermine how many levels
Equals the Period NumberDetermine how many electrons
in outer orbit1 or 2; 3-8 for Groups 13-18
Fill orbits from lowest upward to capacityCapacity = 2(n2)
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Orbit Diagrams
OxygenNeonMagnesiumPhosphorousSiliconCalcium
IronZincChlorineAluminumBoronArgon
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SublevelsDetailed analysis of the colors show subdivisionsThese sublevels tell us what region around the atom the electron is
usually located.Each level has a number of sublevels = # of level
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“s” sublevel“Simple” shapeSphericalCan hold up 2
electrons3s2 is 3rd level,
“s” sublevel with 2 electrons
5s1 ?
2s2 ?
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“s” shape for each Primary Level
n = 1 1s sublevel
n = 2 2s sublevel
n = 3 3s sublevel
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“p” sublevelMade of three shapesEach shape is along a 3-D
x, y, or z axisCan have up to 6 total
electronsSlightly higher energy than
“s” sublevel3p4 means 3rd level, “p”
sublevel with 4 electrons
5p3 ?
3p2 ?
1p2 ?
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Higher “p” sublevels
n = 1 has NO “p” sublevelsn = 2 2p
sublevel
n = 33p
sublevel
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“d” sublevel Made of 5 shapes 4 of the shapes look like 4-leaf
clovers 5th shape looks like fan blade with a
ring Can have up to 10 electrons Because it is so complex it requires
more energy than next level with “s” sublevel3d > 4s, 5d > 6s
dz2
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“d” shapes
z-axis
x-axis
y-axis
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z-axis
x-axis
y-axis
z-axis
x-axis
y-axis
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“f” sublevel Very complex shapes There are 7 shapes that make up “f”
sublevel “f” sublevel may have up to 14 electrons “f” sublevel requires more energy than
next higher “s” sublevel and second higher “p” sublevel4f > 6s & 5p5f > 7s & 6p
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Orbitals Magnetic fields showed that sublevels were
made of individual clouds - orbitals Each Orbital has up to two electrons The orbital shows the orientation of the
cloud along or between the x,y,z axis Each orbital in a level has the same energy
“p” sublevel orbitals
px pz py
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Levels, Sublevels & OrbitalsLevels Sublevels Orbitals Electrons
1st s only 1s2 2
2nd s & p 2s2 2p6 8
3rd s, p & d 3s2 3p6 3d10 18
4th s, p, d & f 4s2 4p6 4d10 4f1432
Complete the chart up to n = 7!
After f comes g, h, and i
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LevelsElectron Levels
Clouds or ShellsIncreasing size and energyNumbered 1,2,3,4,5, ...Each Level holds 2(n2) electrons
Level 1 holds 2(12) = 2 e-Level 2 holds 2(22) = 8 e-Level 3 holds 2(32) = ___Level 5 holds _______ e-
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Configurations and the Periodic Table
Li has 3 electrons1s2 2s1
Sodium has 11 electrons1s22s22p63s1
Potassium has 19 electrons1s22s22p63s23p63d1 BUTPotassium as 4 levels ending with 1 valance electron SO1s22s22p63s23p64s1
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Arrange the levels by energy
4s is simpler and less energy than 3d so it comes first
After 3d then continue to 4p5s is less than 4d6s is less than 4f and 5d7s is less than 5f and 6d
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Correct Order of Energy
Sublevels
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Periodic Table w/ Sublevels
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Configuration of Sulfur
1s2
2s2 2p6
3s2 3p4
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Configuration for Iron1s2
2s2 2p6
3s2 3p6
4s2 3d6
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Configuration for Gd
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Use the Table to find the configuration of electrons
ClMgCuGeTeAu
1s22s23s23p5
1s22s22p63s2
1s22s23s24s23d9
1s22s23s24s23d104p2
1s22s23s24s23d104p65s24d105p4
1s22s23s24s23d104p65s24d105p6 6s2 4f14 5d9
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Compounds
There is special stability if an atom has 8 valance electrons
Octet RuleMetals tend to lose electronsNonmetals tend to gain electrons
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Atomic Size
In a group size increases as there are more levels
In a period size decreases as the greater positive nucleus draws in the valance electrons
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Orbital = Electron cloud made by one or two electrons
Both electrons must have opposite spins!() is OK – opposite spins() is NOT OK – same spin