agenda get to know periodic table and history make your own periodic table do now grab packet and...
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AGENDA•GET TO KNOW PERIODIC TABLE AND HISTORY•MAKE YOUR OWN PERIODIC TABLE
DO NOWGrab packet and periodic table
1. Study these ions with a partner:acetate, bromate, chlorate, chlorite, cyanide,
bicarbonate
REMINDERS•ION QUIZ FRIDAY
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THE PERIODIC LAW
Chemistry Chapter 5
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Mendeleev’s Periodic Table
Dmitri Mendeleev
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Mendeleev – organized periodic table
Tried to organize periodic table according to properties
Vertical columns in atomic mass orderMade some exceptions to place elements in
rows with similar properties (Tellurium and Iodine)
Horizontal rows have similar chemical properties
Gaps for “yet to be discovered” elementsLeft questions: why didn’t some elements fit in
order of increasing mass? Why did some elements exhibit periodic behavior?
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Henry Moseley
Discovered that periodic table was in atomic number order, not atomic mass order
Explained the Te-I anomaly
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Periodic Law
Physical and chemical properties of the elements are periodic functions of their atomic numbers
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Modern Periodic Table
Discovery of noble gases yields new family (Group 18 – aka inert gases)
Lanthanides (#58 - #71)Actinides (#90 – #103)
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Periods and Blocks of the Periodic Table
Periods – horizontal rows Corresponds to highest principal quantum number
Groups/Families – vertical columns; these elements share similar chemical properties (they have the same number of valence electrons)
Blocks – periodic table can be broken into blocks corresponding to s, p, d, f sublevels
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Orbital filling table
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s block
S block includes groups 1 and 2Group1 – “The alkali metals” One s electron in outer shellSoft, silvery metals of low density and low
melting pointsHighly reactive, never found pure in nature
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s block
Group 2 – “Alkaline Earth Metals”2 s electrons in outer shellDenser, harder, stronger, less reactive than
Group 1Too reactive to be found pure in nature
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Periodic Table with Group Names
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Easily lose valence electron (Reducing agents)
React violently with waterReact with halogens to form
salts
The Properties of a Group: the Alkali Metals
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d block
Groups 3 -12Metals with typical metallic propertiesReferred to as transition metalsGroup number = sum of outermost s and d
electrons
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p block
Groups 13-18Properties vary greatly – metals, metalloids,
and nonmetalsGroup 17 – halogens are most reactive of non
metalsGroup 18 – noble gases are NOT reactive
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f block
Lanthanides – shiny metals similar to group 2Actinides – all are radioactive; plutonium –
lawrencium are man-made
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Make your own periodic table!
1. Number the groups (18) 2. Number the periods (7) 3. Draw a heavy lack line between the metals and nonmetals. 4. Write the symbol of each element that exists as a gas at ordinary conditions in
RED. 5. Write the symbol of each element that is a solid at ordinary conditions in
BLACK. 6. Write the symbol of each element that is a liquid at ordinary condition in BLUE. 7. Write the symbol of each element that is a man-made element as an outline. 8. Place the atomic number for each element above the symbol. 9. Color each of these a different color and make a key at the bottom:
Halogen (group 17) Noble gases (group 18) Alkali metals (group 1) Alkaline earth metals (group 2) Transition elements (group 3-12) Lanthanides Actinides Metalloids Post-transition metals Other non-metals
10. Outline the symbol’s box in dark green if it is RADIOACTIVE in its most common form.
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Properties of Metals
Metals:
good conductors of heat and electricity
Malleable
Ductile
Have high tensile strength
luster
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Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Zinc, Zn, is more stable than potassium
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Mercury, Hg, is the only metal that exists as a liquid at room temperature
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Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are: poor conductors of heat and electricity brittleMany are gases at room temperature
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Examples of Nonmetals
Sulfur, S, was once known as “brimstone”
Microspheres of phosphorus, P, a reactive nonmetal
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure
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Properties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.Metalloids are more brittle than metals, less brittle than most nonmetallic solids Metalloids are semiconductors of electricity
Many used in computer parts Some metalloids possess metallic luster
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Silicon, Si – A Metalloid
Silicon has metallic luster Silicon is brittle like a nonmetal Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B Germanium, Ge Arsenic, As Antimony, Sb Tellurium, Te
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Half of the distance between nuclei in covalently bonded diatomic molecule
"covalent atomic radii"
Periodic Trends in Atomic Radius
Radius decreases across a period Increased effective nuclear charge dueto decreased shielding
Radius increases down a group
Addition of principal quantum levels
Determination of Atomic Radius:
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Table of Atomic Radii
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Increases for successive electrons taken from the same atom
Tends to increase across a period
Electrons in the same quantum level do not shield as effectively as electrons in inner levels
Irregularities at half filled and filled sublevels due to extra repulsion of electrons paired in orbitals, making them easier to remove
Tends to decrease down a group
Outer electrons are farther from thenucleus
Ionization Energy - the energy required to remove an
electron from an atom
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Ionization of Magnesium
Mg + 738 kJ Mg+ + e-
Mg+ + 1451 kJ Mg2+ + e-
Mg2+ + 7733 kJ Mg3+ + e-
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Table of 1st Ionization Energies
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Another Way to Look at Ionization Energy
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Ionic Radii
Cations Positively charged ions Smaller than the
corresponding atomAnions Negatively charged
ions Larger than the corresponding atom
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Table of Ion Sizes
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Electronegativity
A measure of the ability of an atom in a chemicalcompound to attract electrons
Electronegativities tend to increase across a period
* more nuclear charge, more power to attract electrons
Electronegativities tend to decrease down a group or remain the same
* additional energy levels result in less attraction to the nucleus
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Periodic Table of Electronegativities