The Periodic Table

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The Periodic table is a method of classifying elements.

  • Elements are arranged in order of increasing atomic number (each proceeding element has one more proton)
  • Made up of rows called periods and columns called groups; the position of an element helps determine its electronic configuration
  • Period number: number of electron shells
  • Group number: number of valency electrons (outer shell electrons)
  • ^^Elements in the same group have similar chemical properties^^

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Periodic Trends

  1. Table moves from metals on the left to non-metals on the right.
  2. Down a group of metals, elements become more reactive
  3. With non-metals, going down a group, reactivity decreases

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^^Alkali Metals^^

  • Group I metals: Lithium, sodium and potassium
Chemical PropertiesPhysical Properties
Readily react with oxygen and water; stored in oilGood conductors of heat and electricity
React violently with chlorineSoft and easy to cut
Burst into flames when heated with oxygen[red flame for lithium; yellow flame for sodium; lilac flame for potassium]Shiny when freshly cut
Produce soluble white compounds.Low melting and boiling points compared to most metals.
React with water to form alkaline metal and hydrogen gasLow densities for metals
  • Reactivity increases down the group

  • Density Increases

  • Softness increases

  • Melting point decreases

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^^Halogens^^

PropertiesPatterns
States and Colors, at RTP: \n Fluorine- Yellow gas \n Chlorine- Green gas \n Bromine- Red liquid \n Iodine- Black solidDown the group; size, mass and density increase
PoisonousDown the group, color darkens
Diatomic; form halide ions in displacement reactionReactivity decreases down the group, \n because it has to gain an electron, \n so the closer the electron is to the positive nucleus the more easily it will be gained, \n so atoms with fewer shells will react more easily.
Do not conduct electricitymelting point increases down the group
Brittle and crumbly when solid

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^^Transition Metals^^

  • High melting points (except mercury)

  • Malleable and ductile

  • Good conductors of heat & electricity (silver is the best)

  • High density

  • Have no trend in reactivity

  • Used as catalysts

  • Form colored compounds

  • Can form complex ions as they have variable valences

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^^Noble Gases^^

PropertiesUses
Density increases down the groupHelium- filling balloons and aircrafts because it is lighter than air and will not catch fire.
Monoatomic and colorlessArgon – filling (tungsten) light bulbs to stop the filament reacting with oxygen.
M.P. and B.P. increases down the groupNeon – is used in advertising signs because it glows red.
Don’t conduct electricity
Inert due to full outer shell electrons

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