1 the periodic table chemistry 2 origin of periodic table triads - groups of 3 elements with similar...
TRANSCRIPT
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Origin of Periodic TableTriads - groups of 3 elements with
similar properties
(Dobereiner – 1817)
Law of Octaves – properties of elements repeat every 8 elements
(Newlands – 1863)
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Origin of Periodic TableDimitri Mendeleev – 1869
–Properties of elements are periodic functions of their atomic masses.
–Developed 8 column table–Left spaces for undiscovered
elements–Columns contained elements with
similar properties–Problems with Ni, I, K (Why?)
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Origin of Periodic TableX-ray experiments by Mosley
(1913) led to discovery of atomic numbers.
Modern Periodic Law – properties of elements are periodic functions of their atomic numbers.
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Organization of Periodic TableRows are called periods.Columns are called families or
groups.All elements in a family have similar
properties.Octet Rule – elements with 8 valence
electrons are unreactive
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Easily lose valence electron (Reducing agents)
React violently with water Large hydration energy React with halogens to form
salts
The Properties of a Group: the Alkali Metals
H- Hydrogen Rb- Rubidium
Li-Lithium Cs- Cesium
Na-Sodium Fr-Francium
K-Potassium
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Properties of MetalsProperties of Metals Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster
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Examples of MetalsExamples 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 alkaline metals Be, Mg, Ca, Sr, Ba, Ra The alkaline earth metals, or alkaline
earths, are beryllium, magnesium, calcium, strontium, barium, and radium.
Possess many properties of metals Low electro negativities Low electron affinities They have smaller atomic radii than the
alkali metals
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Transition Metals all have similar properties Middle – purple and can give up different amounts of electrons at different times
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Properties of MetalloidsProperties 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 Some metalloids possess metallic luster
B- Boron As- Arsenic At- Astatine
Ge- Germanium Te-Tellurium
Sb- Antimony Si- Silicon
Al-Aluminum Po- Polonium
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Silicon, Si – A MetalloidSilicon, 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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PropertiesProperties of of NonmetalsNonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element. Nonmetals are poor conductors of heat and electricity Nonmetals tend to be brittle Many nonmetals are gases at room temperature
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Examples of NonmetalsExamples 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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Non-Metals Right of the stair-step line
C-Carbon, N- Nitrogen, O-Oxygen, P-Phosphorus, Cl-Chlorine, Se-Selenium
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Properties of Halogens a particular class of nonmetals. Very high electronegativities Seven valence electrons (one short of a
stable octet) Highly reactive, especially with alkali
metals and alkaline earths Halogens range from solid (I2) to liquid
(Br2) to gaseous (F2 and Cl2) at room temperature.
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Properties of Noble gases
Unreactive gases Odorless Colorless All produce light when an electric
current is applied
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Half of the distance between nucli 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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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 groupOuter electrons are farther from thenucleus
Ionization Energy - the energy required to remove an electron from an atom
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Affinity tends to increase across a period
Affinity tends to decrease as you go down in a period
Electrons farther from the nucleusexperience less nuclear attraction
Some irregularities due to repulsive forces in the relatively small p orbitals
Electron Affinity - the energy change associated with the addition of an electron
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Ionic RadiiIonic RadiiCations
Positively charged ions Smaller than the
corresponding atomAnions
Negatively charged ions Larger than the corresponding atom
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ElectronegativityElectronegativity
A measure of the ability of an atom in a chemicalcompound to attract electrons
Electronegativities tend to increase across a period
Electronegativities tend to decrease down a group or remain the same