The Periodic Table and the Elements

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The Periodic Table and the Elements

• Pioneer High School
• Chemistry

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Chemistry Standards
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Across the Periodic Table

• Periods Are arranged horizontally across the
  periodic table (rows 1-7)

2nd Period
6th Period
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Down the Periodic Table

• Family Are arranged vertically down the periodic
  table

Family IA
Family VIIA
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• Chemical Families Names
• Alkali metals - react with water to form an
  alkaline solution
• Alkaline earth metals - are reactive, but not as
  reactive as Group IA.
• They are also soft metals like Earth.
• Halogens - need only one electron to fill their
  outer shell
• They are very reactive.
• Noble gases - have completely filled outer shells
• They are almost non reactive.

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• Chemical Families Names
• The two groups located at the bottom of the
  periodic table are also given their own names.
• Lanthanide
• Actinide
• If the groups were in their normal place the
  table would be extremely long.

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Elemental Categories

• There are three categories that the elements can
  be placed into
• Metals
• Non-Metals
• Metalloids
• Each one of the categories have there own
  physical and chemical characteristics

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Category Characteristics
Metal Elements that are usually solids at room
temperature. Shiny, bendable, stretchable and
are great conductors of electricity and heat.
Non-Metal Elements in the upper right corner of
the periodic table. Are either brittle solids
(can be broken easily), liquids, or gasses.
Metalloid Elements that lie on a diagonal line
between the metals and non-metals (except for
Al). They share properties of both metals and
non-metals.
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Reading the Periodic Table Classification

• Nonmetals, Metals, Metalloids, Noble gases

Nonmetals
Metals
Metalloids
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• Periodic Table
• Trends

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1. Trend in Atomic Radius

• Atomic Radius
• The size of an atom is determined by the total
  number of electrons.
• The bigger the of e- the larger the atom

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1. Trend in Atomic Radius

• Atomic Radius
• As the nucleus becomes more positive, from left
  to right, the radius of the atoms becomes smaller
  as the electrons are attracted to the stronger
  nucleus.

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1. Trend in Atomic Radius

• Atomic Radius
• As each new period begins, so does a new energy
  level and so there is a large jump in the radius
  at the start of each new level.

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Atomic Radius vs. Atomic
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1. Trend in Atomic Radius
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2. Trend in Ionization Energy
Ionization Energy The energy required to remove
the valence electron from an atom.
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Atomic Radius vs. Ionization Energy

• Large atoms have low ionization energies.
• The reasons
• Large radius
• The e- are so far away from the nucleus that the
  atoms hold on them is weak
• Therefore the energy needed to steal them is
  small

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Atomic Radius vs. Ionization Energy

• Large atoms have low ionization energies.
• The reasons
• Sheilding Effect
• The e- in the inner levels push away the e- in
  the outer shell
• Therefore the energy needed to steal them is
  small

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Nuclei vs. Ionization Energy

• In the same period, elements with larger nuclei
  have higher ionization energies
• Larger nucleus
• A stronger pull on the electrons

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Nuclei vs. Ionization Energy

• In the same period, elements with larger nuclei
  have higher ionization energies
• Larger nucleus
• A stronger pull on the electrons

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Nuclei vs. Ionization Energy

• In the same period, elements with larger nuclei
  have higher ionization energies
• Larger nucleus
• A stronger pull on the electrons

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Atomic Stability

• The Noble gasses are stable elements because they
  have 8 valence e-.
• All other atoms react to either gain or lose e-
  to become stable like the Noble gasses.
• This strive to be stable is called the Octet rule
• When an atom accomplishes this it is unreactive.

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Atomic Stability

• There are times when atoms cannot get all 8 e-
• Some atoms will be happy to get as close as
  possible
• Having filled sublevels s2, p6, d10, f14
• Having half-filled sublevels s1, p3, d5, f7
• This is why Au, Ag, Cr, and others steal
  electrons

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Stablility vs. Ionization Energy

• Stable elements have higher ionization energies.
• If the elements end in
• If they complete their outer shell, s2 p6
• s2, d10, or f14 they have a full sublevel
• s1, p3, d5, or f7 they have a ½ full sublevel

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Ionization Energy vs. Atomic
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Ionization Energy Summary
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2. Trend in Electronegativity

• Electronegativity the relative ability for an
  atom to attract e- in a chemical bond

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4. Trend in Electron Affinity
Electron Affinity The energy release when an
electron is added to an atom.
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Electronegativity and electron Affinity Trends

• Both electronegativity and electron affinity have
  the same patterns as IE.

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• Dot Diagram Assignment

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Lewis Dot Diagrams

• Lets look at the trends you found out for homework

He
H
C
N
O
F
Ne
Be
B
Li
Si
P
S
Cl
Ar
Na
Al
Mg
K
Ca
Zn
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Ag
Nb
Mo
Ru
Rh
Cd
Zr
Y
Tc
Pd
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Periodic Table
We see even more trends when we look at the
ending of the e- configurations
H 1s1
He 1s2
F 2p5
Be 2s2
B 2p1
C 2p2
N 2p3
Ne 2p6
Li 2s1
O 2p4
Na 3s1
Mg 3s2
Cl 3p5
Al 3p1
Si 3p2
P 3p3
S 3p4
Ar 3p6
K 4s1
Ca 4s2
Zn 3d10
As 4p3
Be 4p5
Sc 3d1
Ti 3d2
V 3d3
Cr 4s3d5
Mn 3d5
Fe 3d6
Co 3d7
Ga 4p1
Ge 4p2
Se 4p4
Kr 4p6
Ni 3d8
Cu 4s13d10
Sr 5s2
Rb 5s1
Nb 4d3
Mo 5s14d5
Ru 4d6
Rh 4d7
Sn 5p2
I 5p5
Xe 5p6
Cd 4d10
Zr 4d2
Tc 4d5
In 5p1
Sb 5p3
Te 5p4
Y 4d1
Ni 4d8
Ag 5s14d10
Cs 6s1
Hf 5d2
Ta 5d3
W 6s15d5
Re 5d5
Os 5d6
Ir 5d7
At 6p5
Rn 6p6
La 5d1
Ni 5d8
Ba 6s2
Tl 6p1
Pb 6p2
Bi 6p3
Po 6p4
Hg 5d10
Au 6s15d10
Mt 6d7
Fr 7s1
Bh 6d5
Hs 6d6
Ra 7s2
Rf 6d2
Db 6d3
Sg 7s16d5
Ac 6d1
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Electron Configuration Trends

• Using the patterns set in this fashion, we can
  write e- configs.

s
p
S
d n-1
f n-2
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Write the e- configurations for

• Calcium Iodine
• Zinc Phosphorous