Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.
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Transcript of Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.
![Page 1: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/1.jpg)
Chemical Periodicity
Ch. 14
![Page 2: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/2.jpg)
Periodic Table Revisited
14-1
![Page 3: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/3.jpg)
Periodic Table Revisited
• In 1871 Russian chemist, Dmitri Mendeleev, created the periodic table organized by atomic mass
• Now it is organized by increasing atomic #
• Physical and chemical properties within a group are similar
![Page 4: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/4.jpg)
Mendeleev’s Table
![Page 5: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/5.jpg)
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Periodic Trends
14-2
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#1 Patterns in Atomic Size
•Atomic size of an element decreases across a period (from left to right)
–As the # of electrons in an energy level increases, they are held more tightly to the nucleus (attracted to the protons inside)
•Atomic size increases down a group (from top to bottom)
–As the # of energy levels increases the size of the atom increases
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Draw on white blank periodic table
![Page 9: Chemical Periodicity Ch. 14. Periodic Table Revisited 14-1.](https://reader030.fdocuments.us/reader030/viewer/2022032313/56649e705503460f94b6d6e5/html5/thumbnails/9.jpg)
Size increases down a group!
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Size decreases across a period
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#2 Patterns in Ionic Size• Ions are charged atoms.
– Cation: positive ion, loses electrons; smaller than atom because lost electrons
• B+3 is smaller than B
• Lose an energy level + more protons than electrons so held tighter = smaller
– Anion: negative ion, gains electrons; larger than atom because gained electrons
• N-3 is larger than N
• More electrons than protons, not as attracted to nucleus = larger
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• Ionic size decreases across a period
– (Larger) Li+ Be+2 B+3 (Smaller)
– (Larger) N-3 O-2 F- (Smaller)
• Ionic size increases down a group.
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Ionic Size Decreases
across
Ionic Size Increases
Down
Draw on Blank
PeriodicTable
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#3 Ionization Energy• Ionization energy: The energy required to
remove an electron from an atom– Measures the resistance to the loss of electrons
• Ionization energy increases as you move across a period (left to right)– Easy to remove electron from cations (L) not
anions (R)
• Ionization energy decreases as you move down a group (top to bottom)– Farther away from the nucleus, the easier it is to
remove an electron
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Draw on white blank periodic table
CATIONS ANIONS
+1
+2 +3
-1
-3 -20
0Ionization Energy
decreases
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#4 Electronegativity
• Electronegativity measures the ability of an atom to attract, or gain, electrons– Ex: Cation does not want to gain electrons while
anions do; anions have a higher electronegativity• Electronegativity increases across a period
– Anions (R) have greater ability to gain electrons than cations (L)
• Electronegativity decreases down a group– Less ability to attract electrons when the size is
larger (farther from the nucleus with positive protons)
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Draw on white blank periodic tableD
ecreasing EN
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Summary of Periodic Trends
Trend Across Period
(Left to Right)
Down Group
(top to bottom)
Atomic Size
Ionic Size
Ionization Energy
Electronegativity
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Summary of Periodic Trends
Trend Across
(Left to Right)
Down
(top to bottom)
Atomic Size Decrease Increase
Ionic Size Decrease Increase
Ionization E Increase Decrease
Electronegativity Increase Decrease