Periodic Table What we already know: Periodic Law: when Atoms arranged by increasing atomic number,...
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![Page 1: Periodic Table What we already know: Periodic Law: when Atoms arranged by increasing atomic number, patterns appear Rows = Periods Columns = Families or.](https://reader036.fdocuments.in/reader036/viewer/2022082821/5697c0271a28abf838cd6058/html5/thumbnails/1.jpg)
Periodic TableWhat we already know:
Periodic Law: when Atoms arranged by increasing atomic number, patterns appear
Rows = Periods
Columns = Families or Groups
Elements within a group or family have similar properties
![Page 2: Periodic Table What we already know: Periodic Law: when Atoms arranged by increasing atomic number, patterns appear Rows = Periods Columns = Families or.](https://reader036.fdocuments.in/reader036/viewer/2022082821/5697c0271a28abf838cd6058/html5/thumbnails/2.jpg)
Why do groups have similar properties?
Valence electrons- electrons in outer energy level
Elements in a group have similar properties because they have valence electrons in similar configurations
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Metals, Nonmetals, Semimentals
Separated by staircase black line on right side of periodic table
Metals on left side Nonmetals on right side Semimetals border the black line
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Properties of Metals Have luster (shiny) Conductors of electricity Malleable- can be hammered into
thin sheets (example: aluminum or tin foil)
Usually solids at room temperature
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Properties of Nonmetals Opposite of metals Not shiny Do not conduct electricity Not malleable. They are brittle Usually a gas at room temp Fantastic seven- these are
diatomic, written N2 instead of N
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Semimetals Also known as metalloids Properties of both metals and
nonmetals
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Alkali Metals 1st column in blue End in s1
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Alkaline Earth Metals 2nd column – green End in s2 , full s sublevel
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Alkali Metals & Alkaline Earth metals
Soft metals- you can cut them with a knife
EXTREMELY reactive (especially alkali metals)
Why so reactive? What sort of charge do they form?
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Transition Metals Middle – purple Electrons being added to the d sublevel
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Inner transition Metals F- block (beige color) Electrons being added to the f sublevel
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Transition metals and Inner transition metals Harder metals Not as reactive as alkali & alkaline
earth Can change their number of valence
electrons (this is why they are called transition metals– no set charge)
Always give up valence electrons (form a positive charge- +1, +2, +3, or +4)
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Non-Metals Right of the stair-step line
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Halogens Group 7A(light orange) Always end in s2p5
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Halogens Most are gases Most are diatomic Used in Halogen lights Very reactive- Why? What kind of charge do they form?
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Noble Gases Group 8A (yellow) s2 p8 (full s and p sublevels)
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Noble Gases Gases at room temp. Extremely UNREACTIVE = inert Why so unreactive?