chapter 5 periodic table. mendeleev chemist that looked for patterns among their properties of...
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Mendeleev
• Chemist that looked for patterns among their properties of elements
• Used pieces of paper and wrote the names and properties of the elements
• Arranged items due to increasing atomic mass
• Periodic – have regular, repeating pattern
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• When he arranged the elements according to atomic mass, similar chemical and physical properties were observed every 8th element
• Left spaces for missing elements• Used his table because when missing
elements were found they fit in locations where Mendeleev thought they would
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Changing the Arrangement
• Some locations for elements was incorrect until Henry Moseley figured it out
• He determined the number of protons (atomic number) for each element and put them in order according to atomic number
• Periodic Law
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• Each element is identified by its chemical symbol
• Each square on periodic table has its symbol, atomic number, atomic mass and name
• Each symbol contains one or two letters
• First letter is always capital and if there is a second letter it is lower case
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• Rows = periods (left to right)–Repeating patterns
• Columns = groups (up and down)–Similar physical and chemical
properties–Sometimes called a family
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Metals
• Good conductors of heat• Malleable• Shiny• Ductile• Most elements are metals• Left side of periodic table• Most are solid at room temp (except
mercury)
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Nonmetals• Not shiny• Not malleable• Not ductile• Poor conductors of heat• Found on right side of periodic
table• More than half are gases at room
temp
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Metalloids
• Called semiconductors
• Some properties of metals and nonmetals
• Can be shiny, brittle, hard, soft, etc
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Grouping Elements• Group 1
–Most reactive metals
–Called alkali metals
–Very soft metals
–Shiny
–1 valence electron (electron in outer shell)
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• Group 2–Very reactive
metals (less than alkali)
–2 valence electrons
–Called Alkaline Earth Metals
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• Groups 3-12 –Called transition metals–1 or 2 valence electrons–Less reactive–Shiny–Good conductors of heat–Found between metals and nonmetals
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• Lanthanides
–Follow transition metal lanthanum
–Shiny reactive metals
• Actinides
–Follow transition metal actinium
–Radioactive (unstable)
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• Group 13
–Boron Group
•One metalloid and four metals
•Reactive
•Solid at room temp
•3 valence electrons
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• Group 14–Carbon Group
•One nonmetal, 2 metalloids, and 2 metals
•4 valence electrons•Solid at room temp•Reactivity varies
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• Group 15–Nitrogen Group
• 2 nonmetals, 2 metalloids, and 1 metal
• 5 valence electrons• Reactivity varies• All but nitrogen are solid at room temp
• Nitrogen = 80% of air you breathe
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• Group 16–Oxygen Group
•3 nonmetals, 1 metalloid and 1 metal
•6 valence electrons•Reactive•All but oxygen are solid at room temp
•Oxygen makes up 20% of air
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• Group 17–Halogens
• Nonmetals• 7 valence electrons• Very reactive• Poor conductors of heat• Never alone in nature• React violently with alkali metals
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• Group 18–Noble Gases
• Nonmetals• Nonreactive• 8 valence electrons except for He• Colorless• Odorless• Gases at room temp• Found in Earth’s atmosphere
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• Hydrogen–1 valence electron–Reactive–Colorless–Odorless–Gas at room temp–Low density–Reacts with oxygen–Stands apart from other
elements