tour of the periodic tablevanguardchemistry.weebly.com/uploads/9/2/4/7/... · main-group elements...
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![Page 1: Tour of the Periodic Tablevanguardchemistry.weebly.com/uploads/9/2/4/7/... · Main-Group Elements •Elements in groups 1, 2, 13 – 18 •Alkali Metals (Group 1) •Alkaline Earth](https://reader036.vdocument.in/reader036/viewer/2022071102/5fdba1d1c02eae578212750f/html5/thumbnails/1.jpg)
Tour of the Periodic Table Honors chemistry
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Main-Group Elements
• Elements in groups 1, 2, 13 – 18 • Alkali Metals (Group 1) • Alkaline Earth Metals (Group 2) • Halogens (Group 17) • Noble Gases (Group 18)
• Representative elements
• electron configurations are regular and consistent
• Valence electrons easy to write
• n = period • Group 1 and 2 → ns1 or ns2 • Group 13 – 18 (3A – 8A) → ns2 np(1-6)
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Electron Configurations
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Valence Electrons and Reactivity • Number of valence electrons (VE) determines reactivity of element
• Elements most “happy” when outermost shell has 8 electrons
• Elements gain or lose electrons in chemical reactions to get to 8.
• The fewer electrons gained or lost to get to 8, the more reactive it is.
• K has 1 VE, loses it to get to 8 in the next lower shell – very reactive!
• Cl has 7 VE, needs to gain 1 to get full 8 in outer shell – very reactive!
• O has 6 VE, needs to gain 2. Reactive, but not as much as Cl.
• Argon has 8 VE, full shell, not reactive at all!
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Group 1: Alkali Metals (Li – Fr)
• Lithium (Li)
• Sodium (Na)
• Potassium (K)
• Rubidium (Rb)
• Cesium (Cs)
• Francium (Fr)
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Group 1: Alkali Metals (Li – Fr) = metals that react with water to make akaline solutions
e.g. 2K + 2H2O H2 + 2KOH
• 1 valence electron very reactive
• Physical properties:
• Soft
• Shiny, but dulls quickly
• Good conductors of electricity
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Group 2: Alkaline Earth Metals
• Beryllium (Be)
• Magnesium (Mg)
• Calcium (Ca)
• Strontium (Sr)
• Barium (Ba)
• Radium (Ra)
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Group 2: Alkaline Earth Metals
• 2 valence electrons reactive, but less than alkali metals
• Properties:
• Harder than alkali metals
• Higher melting point than alkali metals
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Transition Metals (Groups 3-12)
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Transition Metals (Groups 3-12)
• D-block elements
• Variable outer electron configurations dependent on element they react with
• Less reactive than alkali and alkaline earth metals
• Physical properties:
• Ductile and malleable
• Good conductors of heat and electricity
Copper (Cu), silver (Ag), gold (Au) are in this group
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Groups 13, 14, 15
• Boron (B) 3 valence electrons
• Carbon (C) 4 valence electrons
• Nitrogen (N) 5 valence electrons
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Group 16: Chalcogens • Oxygen (O)
• Sulfur (S)
• Selenium (Se)
• Tellurium (Te)
• Polonium (Po)
• 6 valence electrons
• Biological function (nutrient or toxin)
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Group 17: Halogens
A
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Group 17: Halogens
• 7 valence electrons (ns2np5) most reactive group
• Like to react with alkali metals
• Physical properties:
• Wide range
• Liquid, solid and gas states
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Group 18: Noble Gases
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Group 18: Noble gases
• 8 valence electrons (ns2np6) unreactive
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Hydrogen
• Most common element in universe 3 out of 4 atoms are H
• Consists of 1 proton and 1 electron
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Lanthanides/Actinides
• 4f and 5f orbitals f-block of periodic table
• Actinides radioactive
• Shiny metals (like alkaline earth metals)
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General Properties of Metals
• Most of the periodic table
• Properties:
• Excellent conductors
• Most are
• Ductile (= can be squeezed out into wire)
• Malleable (= can be hammered or rolled into sheets)
• A few are brittle (Mn, Bi)
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Review Questions
• Which group of elements is most unreactive? Why?
• Noble gases; full valence level of electrons
• What properties do halogens have in common?
• 7 valence electrons, highly reactive, like to react with alkali metals to form salts
• Why is hydrogen a group by itself?
• 1 proton, 1 electron behaves differently
• Why are alkaline earth metals less reactive than alkali metals?
• Must lose 2 electrons; takes more energy