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Periodic table notes
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Periodic Table
Fusion: Unit 5, Lesson 2
Holt: Chapter 12
1st Quiz: Thursday, 12/4/14
Periodic Table
• Dmitri Mendeleev-recognized that elements had repeating patterns (periodic) and organized elements into a table by increasing atomic mass
• Predicted and left space for unidentified elements
• Henry Moseley - determined that the number of protons - atomic number (which is unique to each element) would allow the elements to fit into very specific pattern
• All identified elements follow the periodic law – chemical and physical properties change periodically with atomic number
Metals• Most elements are
metals• Found to the left of
the zigzag line• Solid at room temp
(exception: mercury and hydrogen – nonmetal)
• Properties:– Shiny– Ductile– Malleable– Good conductors
Metalloids• Also called semiconductors
• Border the zigzag line (exception Al)
• Have properties of both metals and nonmetals depending on the conditions
• properties: depending on conditions– Brittle
– Good conductors– Some shiny (others
dull)
Nonmetals
• More than half are gases at room temp
• To the right of the zigzag line
• Properties:– Not malleable or
ductile– Not shiny or dull– Poor conductors
• Each square includes:• elements name• chemical symbol
(color coded to identify if element is a solid, liquid or gas at room temp)
• Atomic number (protons)
• Atomic mass (weighted avg)
• Background color (identifies metals, nonmetals and metalloids on table)
REVIEW
• Atomic number = Number of Protons
• Electrons equal to the number of protons
• Neutrons equal atomic mass (rounded) minus the protons
• Protons do not change in a atom, neutrons can change, electrons can be shared or transferred (when bonds are made)
• First letter of chemical symbol is always upper case and any additional letters are lower case
• Newest elements have temporary 3 letter symbols
• *****Rows (left to right) are called periods- determines the number of energy levels
• Properties gradually change moving left to right across each row from reactive (group 1) to non-reactive (group 18)
• Columns are called groups or family• Elements in the same group or family have
similar properties moving up and down each column
• Each element in a family has the same number of valence electrons in the outer shell
• ******Group number determine the valence electrons (ex: group one – all elements in group 1 have 1 valence electron, all of the elements in group 2 have 2 valence and so on)
Group 1: Alkali metals
• Metals• 1 valence electron in
outer level (easily shared and form compounds easily)
• Very reactive with H2O, O2 and other elements
• Don’t appear in nature by themselves, only as compounds
Group 2 – Alkaline-Earth Metals
• Metals
• 2 valence electrons in outer level (slightly less reactive)
Group 3 – 12: Transition
• Metals
• 1 or 2 valence electrons in outer level (depending on element) and are less reactive
Lanthanides and Actinides• In periods 6 and 7
and appear at the bottom of the periodic table to keep table from being too wide
• Lanthanides are shiny reactive metals
• Actinides are unstable; radioactive
• All elements after Pu-94 (plutonium) are man-made in labs and don’t occur in nature
Group 13: Boron Group
• Has 1 metalloid and 4 metals
• 3 valence electrons in outer level and are semi reactive
Group 14 - Carbon group
• 1 nonmetal, 2 metalloids and 2 metal
• 4 valence electrons in outer level and most non-reactive depending on element
• Forms organic compounds (all living things contain carbon)
Group 15 - Nitrogen Group
• 2 nonmetals, 2 metalloids, 1 metal
• 5 valence electrons in outer level and reactivity depends on conditions and element
• P is extremely reactive and only appears in compounds
Group 16 - Oxygen Group
• 3 nonmetals, 1 metalloid, and 1 metal
• 6 valence electrons in outer level and reactivity depends on element– Po-84 is radioactive
Group 17 - Halogens
• Nonmetals• 7 valence electrons in
outer level and has violent reactions with alkali-metals to form salt compounds– Highly reactive with
other elements
– Do not appear in nature alone only in compounds
Group 18 - Noble Gases• Nonmetals• 8 valence electrons in
outer level (full level) (except helium which has 2 valence electrons, which makes helium full) and very un-reactive – inert
• Do not form compounds under normal conditions
Hydrogen
• Nonmetal
• 1 electron in outer level so it is set above the alkali metals and is reactive
• Properties: even though above metal category, has properties of nonmetals
• Most abundant element in universe, makes up stars
Energy Levels
• 1st energy level – 2 valence electrons (max)
• 2nd energy level – 8 valence electrons (max)
• 3rd energy level – 8 valence electrons (max)
• And so on….
• Each energy level can have less valence electrons but they can not have more than the maximum valence electrons.
Bonds
• To form bonds, elements must reach a full state of 8 valence electrons in the outermost energy level (octet rule) (Exception: would be first energy level which is full at 2-helium)