the history of the modern periodic table
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The History of the Modern Periodic Table. See separate slide show for Periodic Table History. Periodic Law. When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals. Chemical Reactivity. - PowerPoint PPT PresentationTRANSCRIPT
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The History of the Modern
Periodic TableSee separate slide show for Periodic Table History
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Periodic Law• When elements are arranged in order of
increasing atomic #, elements with similar properties appear at regular intervals.
0
50
100
150
200
250
0 5 10 15 20
Ato
mic
Ra
diu
s (
pm
)
Atomic Number
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Chemical ReactivityFamilies Similar valence e- within a group
result in similar chemical properties
•Alkali Metals•Alkaline Earth Metals•Transition Metals•Halogens•Noble Gases
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Periodic Table Reveals Periodic Trends
• Effective Nuclear charge
• atomic size or radius
• ionization energy
• electron affinity
• electronegativity
• metallic character
• Reactivity
• bonding characteristics
• crystal configurations
• acidic properties
• densities
• Melting/Boiling points
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Electron screening or shielding
• Electrons are attracted to the nucleus• Electrons are repulsed by other electrons• Electrons would be bound more tightly if
other electrons weren’t present.• The net nuclear charge felt by an electron is
called the effective nuclear charge ( Zeff ).
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Quantum Mechanical Model
Zeff is lower than actual nuclear charge.
Zeff increases toward nucleus ns > np > nd > nf
This explains certain periodic changes observed.
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Effective Nuclear Charge ( Zeff)
• The effective nuclear charge acting on an electron equals the number of protons in the nucleus, Z, minus the average number of electrons, S that are between the nucleus and the electron in question.
Zeff = # protons # shielding electrons
Zeff = attractive forces repulsive forces Zeff = Z S
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For Example, Lithium vs. Carbon
Li Zeff = 3 2 = 1
C Zeff = 6 2 = 4
So, carbon has a much smaller atomic radius compared to lithium: Rcarbon =77
pm Rlithium = 152 pm
When moving across a row:The greater the Zeff value, the smaller the atom’s radius.
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Trend #1 Atomic Radii
1
2
3
4 5
6
7
Increases to Left and Down
•Why larger going down?
•Why smaller to the right?
•Higher energy levels have larger orbitals
•Shielding - core e- block the attraction between the nucleus and the valence e-
• Increased nuclear charge without additional shielding pulls e- in tighter
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Atomic radii
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The Periodic Table & Radii
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Periodic Trend is Due to Effective Nuclear Charge
Atomic Radii vs. Zeff:
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Trends in Ionic Radii
• Using your knowledge of Zeff, how would the size of a cation compare to neutral atom? Anion?
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Trends in Ionic Radii
• The cation of an atom decreases in size.
• The more positive an ion is, the smaller it is because Zeff increases
• The anion of an atom increases in size.
• The more negative an ion, the larger it is because Zeff decreases.
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Cations lose electrons, become smaller
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Anions gain electrons, become bigger
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Ion Radii
1
2
3
4 5
6
7
+3 +4 -3 -2 -1
Increases downIncreases moving across, but depends if cation OR anion
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Ions and Ionic Radii
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Trend in Ionization Energy
• Ionization NRG is the NRG required to remove an electron from an atom
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Successive Ionization NRG
• Ionization energy increases for successive electrons from the same atom.
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*Notice the large jump in ionization energy when a core e is removed.
Why do you think there is such a big jump for Mg3+?
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• The smaller the atom, the higher the ionization energy due to Zeff
• Bigger atoms have lower ionization NRG due to the fact that the electrons are further away from the nucleus and therefore easier to remove.
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Increases
Dec
reas
es
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Electron Affinity
• The energy change associated with the addition of an electron
• Tends to increase across a period• Tends to decrease as you go down a group• Abbreviation is Eea, it has units of kJ/mol. Values are
generally negative because energy is released.• Value of Eea results from interplay of nucleus
electron attraction, and electron–electron repulsion.
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Electron Affinity
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Trends in Electronegativity
• tendency for an atom to attract electrons when it is chemically combined with another atom.
• decreases as you move down a group• increases as you go across a period from
left to right.
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Trend #5 Metallic Character• The metallic character of atoms can be related
to the desire to lose electrons.
• The lower an atom’s ionizatoin energy, the
greater its metallic character will be.
• On the periodic table, the metallic character of
the atoms increase down a family and
decreases from left to right across a period.
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Metallic Character
1
2
3
4
5
6
7
Increases moving down and across to the left
Fr
Cs Ba
Ra
Lower left corner -- elements mostlikely to lose their valence electrons
Rb
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# 6 Melting/Boiling Points
• Highest in the middle of a period (generally).
1
2
3
4 5
6
7
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Some Important Properties of Alkali Metals
• Easily lose valence electrons (Reducing Agents)– React with halogens to form salts– React violently with water
• Large Hydration NRG– Positive ionic charge makes ions attractive to
polar water molecules• Radius and Ionization NRG follow expected
trends.