Transcript Periodic Table - Spring Branch ISD

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Who developed the Periodic Table?
• Dimitri Mendeleev – (Russian Chemist)
In 1871 developed the first Periodic Table
with 63 elements that were known at the
time.
• He found that as the atomic mass
increased, a repeating patterns of
properties developed.
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Rearranging Table
Henry Moseley- English scientist
• In 1913 he rearranged the periodic table
by the atomic number and chemical
properties.
• This is the periodic table we use today
Arrangement of the Periodic Table
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Mendeleev arranged these elements into
ROWS called PERIODS…
and COLUMNS called GROUPS or FAMILIES.
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Arrangement of the Periodic Table
You can think about it like this…
You have to use a PERIOD at the end of
a sentence……..that goes left to right.
And a COLUMN holds up the porch on the
house where your GROUP / FAMILY gather.
Periods represent the number of rings.
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These outer ring is called
Valence Shell or energy level
Energy Level 2: Li, Be, B, C, N, O, F & Ne
Locate them on your periodic table
2nd Row = 2 Rings
electron
Period #’s run down the
side of the Periodic Table.
1
2
3
4
5
6
7
This is period
number 3
Which means it has
3 energy levels
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1
IA
2
IIA
The Group Numbers
run on top
Of the Periodic Table
This is group 1
the alkali group.
Families have similar
but not identical
characteristics
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18
VIIIA
13 14 15 16 17
IIIA IVA VA VIA VIIA
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Metalloids
Non-Metals
Metals
Transition Metals
Inner Transition Metals
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Left of the STAIRS
Fr
Properties of Metals
• Good conductors of heat and electricity
• Malleable, Ductile
• Have Luster
• High melting & boiling points
• High density
• Mostly solids – except for Hg (liquid)
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F
Right of the STAIRS
Properties of Nonmetals
• Poor conductors of heat and electricity
• Dull, Brittle
• Low melting and boiling points
• Most are GASES, some SOLIDS, and only
1 Liquid - Bromine
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Touch the STAIRS
Properties of Metalloids
• Conduct…not as well as TRUE metals
• Shiny or dull
• Have other properties of metals and nonmetals
• All Solids
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Characteristics
 Group IA or 1
 Has 1 Valence electron
 Make salts such as NaCl and KCl
 Lithium - Treatment for bi-polar disorder
 Highly reactive
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Characteristics
 Group IIA or 2
 Has 2 Valence electrons
 Gemstones and fireworks
 Magnesium burns brightly.
 Calcium makes bones strong.
 Makes strong and light materials-planes, cars
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Characteristics
 Group VIIA or 17
 Has 7 Valence electrons
 Cl - is the most abundant, used in bleach
 Br - used as dyes in cosmetics
 I- (shiny gray) used to make thyroxin.
 Highly reactive group of Non-Metals
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Characteristics
 Group VIIIA or 18
 Have 2 or 8 Valence electrons
 Uses: Neon lights, laser lights...
 Most Stable Group of Elements
 Normally don’t mix with other compounds
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Characteristics
 Group 1, IA but not an Alkali Metal
 Has 1 Valence Electron
 Used in everything from water to acids and bases.
 Most abundant element
 Acts more like a Metal than a Non-Metal
 Has properties of both Alkali Metals & Halogens
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Characteristics
 Groups 3 through 12 or IIIB to IIB
 Has 1 or 2 valence electrons
 Iron, copper, and silver are examples
 Makes gemstones
 From Left to Right –gain properties of Non-Metals
 Less active than alkali metals and alkaline earth metals
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Inner Transition Elements
• Lanthanide series
• Elements 57-71
• 1 or 2 valence electrons
• Actinide Series
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Elements 89-103
1 or 2 valence electrons
All are radioactive
Most are synthetic (man-made)