The Periodic Table Physical Science Unit 8. PERIODIC TABLE Part 1:
Unit 03 the periodic table
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Transcript of Unit 03 the periodic table
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The Periodic Table of the
Elements
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Basic OrganizationAtomic structure is used to organize
the elements in the periodic table.Organized by atomic numberThe periodic table is useful in
predicting the chemical behavior, trends, and the properties on the elements.
3 basic categories:MetalsNonmetalsMetalloids
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Atomic Structure ReviewAtoms are made of protons,
electrons, and neutrons.
Elements are atoms of only one type.
Elements are identified by the atomic number (# of protons in nucleus).
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Energy Levels ReviewElectrons are arranged in regions
around the nucleus called energy levels.
At least 1 energy level and as many as 7 levels exist in atoms.
Electrons in levels farther away from the nucleus have more energy.
Inner levels will fill first before outer levels.
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Energy Levels & Valence Electrons
Energy levels hold a specific amount of electrons: 1st level = up to 2, 2nd level = up to 8 3rd level = up to18
The electrons in the outermost level are called valence electrons. Determine how elements will react with others Outermost level does not usually fill completely
with electrons.
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Using the Table to Identify Valence Electrons
Elements are grouped because they have similar properties.
Group numbers can help you determine the number of valence electrons:Group 1 has 1 valence electron.Group 2 has 2 valence electrons.Groups 3 – 12 are transition metals and
have 1 or 2 valence electrons.
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Using the Table to Identify Valence Electrons cont.
Groups 13 – 18 have 10 fewer than the group number. For example:group 13 has 3 valence electronsgroup 15 has 5 valence electronsgroup 18 has 8 valence electrons
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Grouping the Elements
The most reactive metals are the elements in Group 1 and 2.
What makes an element reactive?● Number of valence electrons each atom
has● When outer levels are full, atoms are
stable● When they are not full, they react: gain,
lose, or share 1 or 2 electrons
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Groups Groups run vertically in the periodic
table. They are numbered from 1 – 18.Elements in the same groups have
the same number of electrons in the outer energy level.
Grouped elements behave chemically in similar ways.
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Group 1: Alkali MetalsContains: MetalsValence Electrons: 1Reactivity: Very ReactiveProperties:
solidssoftreact violently with watershiny low density
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Group 2: Alkaline-Earth Metals
Contains: MetalsValence Electrons: 2Reactivity: very reactive but less
reactive than alkali metals (Group 1)Properties:
SolidsSilver coloredMore dense than alkali metals
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Groups 3-12 Transition Metals
Contain: MetalsValence electrons: 1 or 2Reactivity: less reactive than alkali
and alkaline-earth metalsProperties:
Higher densityGood conductors of heat and electricity
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Groups 3-12 Transition MetalsBelow Main Table
Contain: The Lanthanide and Actinide SeriesThese two rows are pulled out of
sequence and placed below the main table to keep the table from being too wide.
Lanthanides are #’s 58 – 71.Actinides are #’s 90 – 103.
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Groups 3-12 Rare Earth Elements ~ Lanthanides
Lanthanides follow the transition metal # 57 Lanthanum in Period 6.
Valence electrons: 3Reactivity: Very reactiveProperties:
● High luster but tarnish easily ● High conductivity for electricity● Very small differences between them
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Groups 3-12 Rare Earth Elements ~ Actinides
Actinides follow the transition metal # 89 Actinium in Period 7
Valence electrons: 3 (but up to 6)Reactivity: unstable
All are radioactiveMost made in laboratories
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Metalloids A zig-zag line that separates metals
from metalloidsElements from Groups 13 – 17
contain some metalloids.
These elements have characteristics of metals and nonmetals.
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Group 13: Boron Group
Group 13: Boron GroupContains: 1 metalloid and 4 metalsValence Electrons: 3Reactivity: ReactiveOther shared properties:
Solid at room temperature
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Group 14: Carbon Group
Contains: 1 non-metal, 2 metalloids, and 3 metals
Valence Electrons: 4Reactivity: VariesOther shared properties:
Solid at room temperature
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Group 15: Nitrogen Group
Contains: 2 non-metals, 2 metalloids, and 1 metal
Valence electrons: 5Reactivity: VariesOther shared properties:
All but N are solid at room temperature
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Group 16: Oxygen Group
Contains: 3 non-metals, 1 metalloid, and 2 metals
Valence Electrons: 6Reactivity: ReactiveOther shared properties:
All but O are solid at room temperature.
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Groups 17 : Halogens
Contain: NonmetalsValence Electrons: 7Reactivity: Very reactiveOther shared properties
● Poor conductors of electric current● React violently with alkali metals to form
salts● Never found uncombined in nature
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Group 18 Noble Gases
Contains: NonmetalsValence Electrons: 8 (2 for He)Reactivity: Unreactive (least reactive
group)Other shared properties:
Colorless, odorless gases at room temperature
Outermost energy level fullAll found in atmosphere
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Hydrogen Stands Apart
H set apart because its properties don’t match any single group.
Valence electrons: 1Reactivity: very but loses the 1
electron easilyProperties:
Similar to those of non-metals rather than metals
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PeriodsPeriods run horizontally across the
Periodic TablePeriods are numbered 1 – 7All the elements in a period will have
the same number of energy levels, which contain electrons. Examples:
Period 1 atoms have 1 energy level.
Period 2 atoms have 2 energy levels.
Period 5 atoms have 5 energy levels.
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Periods continuedMoving across from left to right across
a period, each element has one more electron in the outer shell of its atom than the element before it.
This leads to a fairly regular pattern of change in the chemical behavior of the elements across a period.