THE PERIODIC TABLE
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Transcript of THE PERIODIC TABLE
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THE PERIODIC TABLE
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The Big Questions
• Who developed the first modern periodic table?– How did he organize it, and how does
this differ from the organization of the P. T. today?
• What are some ways in which we group elements on the P. T.?–What does this tell us about the atom’s
structure?
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PATTERNS
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Henning Brand
• First to discover new element: phosphorus
• Was looking for the Philosopher's Stone• Robert Boyle later
rediscovered it
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Robert Boyle
• Defined element as we know it today• Element: a substance that cannot
be broken down into aSimpler substance by aChemical reaction
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Antoine-Laurent de Lavoisier
• Wrote Elementary Treatise of Chemistry (1789)
• First chemical textbook that listed known elements
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John Newlands
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Similar chemical and physical properties
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Divided groups into 11 groups
Noticed that pairs of similar elements differ by 8 in mass number
Called this his law of octaves
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Dmitri Mendeleev
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Atomic Mass
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The First Modern Periodic Table
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The First Modern P. T.
• DM noticed there were “holes” where no known element would fit.– Guessed that these holes represented
undiscovered elements.–Made predictions about their properties.
• When discovered, these elements matched their predicted properties.
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Atomic Number
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PERIODIC LAW
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• When elements are arranged to atomic numbers, elements with similar properties appear at regular intervals.
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STRUCTURE OF PERIODIC TABLE
GR
OU
P
PERIOD
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Metallicity
More Metallic Less Metallic
More
Meta
llic L
ess M
eta
llic
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Metals, Metalloids, and Nonmetals
Metals
Metalloids
Nonmetals
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Ions
• Atoms can lose or gain electrons.– Ion – an atom that has become charged
by gaining or losing electrons.• Cation – positive ion (lost e-)• Anion – negative ion (gained e-)
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Ions
Gain 1 e-
C-
6 p+
7 e-
C
6 p+
6 e-
Lose 1 e-
C+
6 p+
5 e-
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The Octet Rule
• Atoms tend to gain or lose electrons so they can have 8* valence electrons (same e- configuration as a noble gas).–Why?• 8 valence electrons = full s and p sublevel.• Extremely stable configuration.
• *There are a few exceptions to this rule that we will discuss later.
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Families of Elements
• Families – columns or groups.– Elements in a family have similar chem.
properties.– Also have same no. of valence e-.– Coincidence? (No.)
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Blocks
s-block
p-blockd-block
f-block
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Electron Configs. on the P. T.
1s
2s
3s
4s
5s
6s
7s
3d
4d
5d
6d
4p
5p
6p
7p
3p
2p
1s
4f
5f
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Families of the Periodic Table• Group 1 (1A)
– Alkali Metals • Soft, silvery
• Very reactive (never found alone in nature) • ns1 (ex. 1s2 2s1) • 1 val. e-
• Form +1 ions
• Group 2 (2B)– Alkaline earth metals• Harder, denser, stronger than alkali metals
• Reactive (never found alone in nature) • ns2 (ex. 1s2 2s2) • 2 val. e-
•Form +2 ions.
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Families of the Periodic Table
• Groups 3 –12(3 – 12)– Transition metals
• Typical metallic properties• Less reactive than group 1,2• ns2 (n-1)d1-10 (ex. 1s22s22p63s23p64s23d8)• Have variable val. e-
• Can form multiple cations
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Families of the Periodic TableThe p-block elements:Groups 13 (3A) –18 (8A): (Representative elements)
Main-group elements:Includes:
Metalloids, nonmetals, metals ns2 np1-6 (ex. 1s22s22p63s23p4)
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Families of the Periodic Table
• Group 17 (7A)– Halogens
• react with most metals to form salt compounds
• 7 val. e-
• Form –1 ions
• Group 18 (8A)– Noble gases •inert gases (not reactive) •both s and p sublevels = full (8 electrons)
(exc. He) ns2 np6 • Do not form ions