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The Periodic Table
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Dimitri Mendeleev
• Russian scientist developed the first published table in 1869.
• Arranged elements in order of atomic mass
• Elements with similar properties were placed in columns
• left spaces for undiscovered elements
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Periodic Law the pattern of the table
• Mendeleev’s table was called a periodic table because……..
• If the elements were arranged in order of increasing atomic mass then elements with similar properties would show up PERIODICALLY.
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Henri Moseley (1914)
• Used X-rays to reveal atomic numbers of several elements.
• Suggested that the elements should be arranged in order of atomic number instead of atomic mass. – Today that is how it is arranged
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Reading the Periodic Table
• Families or Groups– Up and down
• Numbered 1 to 18• Elements in groups (families) have
similar characteristics
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• Periods–Across the table 1-7
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Classifications of Elements
MetalsNon-metals Metalloids (semi-metals)
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Metals
• Elements to the left of the steps• except H, Ge & Sb
MetalsGe
Sb
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Metal characteristics
• Solids at STP (except mercury)
• good conductors of electricity and heat– Mobile electrons
• shiny luster• ductile - drawn (made) into wire
• malleable - hammered into sheets
• when combined in compound have a positive oxidation state (+, cation)
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• Metallic character increases R to L–Most reactive metals found in
Group 1
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Non-metals
H
18
B
Si
As
Te
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Non-metal characteristics
• Solid, liquid or gas at STP• used as insulators• solids are dull• brittle• when combined in a compound
have negative oxidation state (-, anion)
• Metallic character decreases L to R
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Metalloids
• a.k.a. Semimetals
• both metal and non-metal properties
• “sit on the steps”
• 2 hide underneath
BSi
AsTeSb
Ge
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Elements are (s), (l) & (g)
• Solid – particles have vibratory motion and are
tightly packed– Almost ALL of the elements
• Liquid – particles can move throughout substance – particles are farther apart than in solids– conforms to shape of container
– ONLY Hg and Br
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• Gas– molecules in constant, random,
straight line motion– molecules fill container– large space between “volumeless”
molecules– conforms to the shape of the
container– H, N, O, F, Cl and Group 18
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Allotropes
• Different forms of an element found naturally in the same state– Different molecular structures
Carbondiamond, coal, graphite
OxygenO2 & O3
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N O F
Cl
Br
I
Diatomic elements
• Elements found bonded to itself “uncombined”
• N2 O2 F2 Cl2 Br2 I2 and H2
H
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Monoatomic elements
18
Ne
Ar
Kr
Xe
Rn
HeValence shellfilled with 2e-
Valence shellfilled with8 e-
• Inert• Don’t react
or form compounds
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Valence electrons
• The number of valence electrons correspond to group number
• 1, 2 , 13 - 18
Last digit• The Energy Level (shell) they are in
is the same as the period #
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Group / Family Characteristics
Each group has characteristic properties that are directly related to electron configuration & especially the number of valence electrons
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Group 1
• Alkali Metals• all elements except hydrogen• most reactive metal group• SO reactive they are never found
alone in nature– always bonded to another element
• form +1 ions
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Group 2
• Alkaline Earth Metals• second most reactive metals group• SO reactive they don’t occur alone
in nature– always bonded to another element
• form +2 ions
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d- block elements
• Transition Metals
COLORful
ions and solutions
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• Transition metals not as reactive as other metals
• some found in free state– Au, Ag, Pt
• multiple positive oxidation states– Iron (IV) oxide FeO2
– Iron (II) oxide FeO
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Group 17
• Halogens• Most reactive nonmetal group• SO reactive that they don’t occur
by themselves in nature– at least bonded to themselves
(diatomic)• form -1 ions
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Group 18
• Noble gases• “Inert” gases• don’t like to combine with other
elements– Valence shells filled
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Ionization Energy
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Ionization Energy (first)
• Definition: – energy needed to remove the most
loosely held e-
Valence electronhigh E electronOutermost electron
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What’s holding the e- in place?
• Nuclear charge– There is a force of attraction between
protons (+) in the nucleus and electrons (-) in the orbitals
– “Opposites attract”
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Ionization energy
• Hint: energy needed to make an ion by losing electrons
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MOST elements want 8 e- (octet rule)
• Elements with only a few valence electrons will tend to have lower ionization E
• In other words…– It doesn’t take a lot of E to remove
their e-
Metals
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MOST elements want 8 e- (octet rule)
• Elements with almost 8 valence electrons won’t give them up so easy– It takes a lot of E to remove their e-
• Non-metals have high Ionization E
Who has the highest IEs?
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Graph Ionization Energies
• Label X axis with Atomic #1-20• Label y axis with 1st IE (KJ/mol
atoms)
• AFTER you plot the points– Label data points with element
symbols – Connect data points of same period
only– Separate your graph into Periods
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Period 2 Period 3Period 1 Period 4
Fir
st I
oniz
atio
n E
nerg
y (K
J / m
ol)
H
He
Li
Ne
Na
Ar
Ca
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What is the periodic trend for ionization energy?
INCREASES
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Ionization E trend?
• As move across a period…IE increases. WHY?
3 p+ 9 p+
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• As you go across a period–a large proton and a tiny electron
are being added. – more p+ hold the e- tighter
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• As move UP a group … IE increases. WHY?Period 1Period 2Period 3Period 4
Let’s figure it out . . .
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Potassium
19 p+
+
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Sodium11 p+
+
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Lithium
3 p+
+
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• As you go up a group – the valence shell gets closer to
the nucleus and can hold on to the e- tighter.
because . . .INCREASES
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SHIELDING
• Reason why IE decreases as you go down a group
• the distance increases between the p+ and valence e-–AND
• e- in outer shells repel each other
–WHICH IS WHY low IE are so reactive!
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Electronegativity
• Ability of an atom to attract electrons of other atoms.
• In other words. . . – Atoms with high e-neg are bullies that
steal electrons
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Fluorine
Electronegativity Graph
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Electronegativity
• Determine the periodic trend
INCREASES
EXCEPT for Noble gases. WHY?
F
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Atoms with high electronegativities also havehigh ionization E
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Atomic Radius
• Radius – distance from the center of a circle
(Nucleus) to the outermost edge (valence shell)
R
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Atomic Radius Periodicity
DECREASES
DECREASES
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Why?????
• Why does atomic radius DECREASE as you move up a group?
• Why does atomic radius DECREASE as you move across a period?
• Losing layers of e-
• Increasing the # of p+ holds the e- in tighter
• Increasing NUCLEAR CHARGE
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• What happens to atomic radius as you create a + ion?
• radius decreases
• What happens to atomic radius as you create a - ion?
• radius increases
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• Compare the ionic radus of Mg2+ and the atomic radius of Ne.
The radius of the Mg2+ ion is smaller than the atom of Ne, because the Mg2+ ion has more p+ (12) than the Ne atom (10).
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Compare . . .
• Fluoride ion & Fluorine atom
• Sodium ion & Sodium atom
• Fluoride ion & Neon atom
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General Formulas of compounds
• You can look at the groups on the periodic table and determine how they will combine with elements of different groups.
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Write these formulas
• lithium fluoride• sodium fluoride• potassium fluoride• lithium chloride• sodium chloride• potassium chloride
• What do you notice?
• Write the general formula for Group 1 and Group 17 elementsAB
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Write these formulas
• beryllium fluoride• magnesium fluoride• calcium fluoride• beryllium chloride• magnesium chloride• calcium chloride
• What do you notice?
• Write the general formula for Group 2 and Group 17 elements
AB2
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Write these formulas
• lithium oxide• sodium oxide• potassium oxide• lithium sulfide• sodium sulfide• potassium sulfide
• What do you notice?
• Write the general formula for Group 1 and Group 16 elements
A2B
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Write these formulas
• beryllium oxide• magnesium oxide• calcium oxide• beryllium sulfide• magnesium sulfide• calcium sulfide
• What do you notice?
• Write the general formula for Group 2 and Group 16 elements
AB
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Formula Writing & Naming Review
• Lead IV oxide• Phosphorus pentoxide• SO3
• Oxygen• Argon• Aluminum oxide• NiO
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Different Forms of the Periodic Table
• Changes were made to Mendeleev’s table to look like the modern Periodic table we use today.
• This is not the only form of the periodic table that exists, however it is the most widely accepted.
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Stowe’s Physicists p.t.
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Benfey p.t.
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Zmaczynski p.t.
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Alexander Arrangement p.t.
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立体周期表の組み立て方 p.t.
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THE END