the periodic table. objective you will be able to discuss the contributions of mendeleev, moseley,...
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The Periodic Table
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Objective
• You will be able to discuss the contributions of Mendeleev, Moseley, and Seaborg in the development of the periodic table.
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The Periodic TableDmitri Mendeleev (1869):published first periodic table.
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• arranged by increasing atomic mass• grouped by similar properties• predicted the existence and properties of unknown elements (Ga, Ge, Hf)
Mendeleev’s Periodic Table
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Mendeleev’sPredictions
Property
Prediction
for
ekasilicon
Actual
for
Ge
Atomic
mass
72
amu
72.59
amu
Density 5.5
g/cm3
5.32
g/cm3
Formula
of oxide
EsO2 GeO2
Formula of
chloride
EsCl4 GeCl4
Predicted in 1871;Ge was discovered in 1886.
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Is the atomic mass of Tellurium (Te) incorrect?
Mendeleev’sQuestion
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Henry Moseley
Henry Moseley (1911): each element has different # of p+.The table should be arranged by atomic number, not atomic mass.
Moseley was killed in Turkey during WWI.
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The Modern TableGlenn Seaborg arranged our modern table (d-block and f-block).
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Objectives
• Know the periodic law.• Explain how atomic radius is measured.• Understand, identify, and discuss the trends on
the periodic table for atomic radius and for electronegativity.
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Periodic Law
periodic law:the propertiesof the elementsrepeat periodically
“periodicity”
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Atomic Radius
It is difficult to measure atomic size (no definite edge).
atomic radius: ½ the distance between the nuclei of two bonded atoms
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Atomic Radius Trendsgroup trend (down a column): radius increasesbecause new energy levels
period trend (across a row): radius decreases because electrons are in the same “shell” but added protons pull inward on the shell.
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Electronegativity
electronegativity: the tendency of an atom to attract electrons when it is bonded to another atom
The nucleus of a small atom pulls strongly on the outer electrons of a large atom
+ + +
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Electronegativity Trends
group trend: electronegativity decreases (atoms get larger)
period trend: electronegativity increases (atoms get smaller)
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Objectives
• You will be able to compare the reactivity of elements.
• You will be able to explain why specific elements are either reactive or unreactive.
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Metals and Non-Metals
Metals tend to lose their outer “valence” electronsbecause they are large (low electronegativity).
Non-metals tend to attract electrons becausethey are small (high electronegativity).
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Reactivity Trendssame group = similar properties (like reactivity) = similare- configurations
metals: largest, with fewest valence e- are most reactive non-metals: smallest, with most valence e- are most reactive (excluding noble gases—outer shell is full)
Which is the most reactive?• Ca, Cu, Rb, Na• S, Cl, Br, C, Ne
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Reaction Clips
• Alkali Metal Reactions• Sodium and Chlorine Reaction• Fluorine Reactions