section 6-3 section 6.3 periodic trends compare period and group trends of several properties....
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Section 6-3
Section 6.3 Periodic Trends
• Compare period and group trends of several properties.
principal energy level: the major energy level of an atom
ion
ionization energy
octet rule
electronegativity
• Relate period and group trends in atomic radii to electron configuration.
Trends among elements in the periodic table include their size and their ability to lose or attract electrons
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Factors that influence Periodic Trends• Shielding - core electrons block the
attraction between the nucleus and the valence electrons.
• Nuclear Charge – The number of protons in the nucleus will impact the attraction of valence electrons
•Across a given period (row) nuclear charge will have a greater influence than shielding
•Down a given group (column) Shielding will have a greater influence than nuclear charge
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Section 6-3
Atomic Radius• Atomic size is a periodic trend influenced
by electron configuration and nuclear charge.
• For Metals, atomic radius is half the distance between adjacent nuclei in a crystal of the element.
• For elements that occur as molecules, the atomic radius is half the distance between nuclei of identical atoms.
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Section 6-3
Atomic Radius (cont.)
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4 5
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• Atomic Radius– Increases to the LEFT and DOWN
Atomic Radius
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• Why larger going down?
– Higher energy levels have larger orbitals
– Shielding - core e- block the attraction between the nucleus and the valence e-
• Why smaller to the right?
– Increased nuclear charge without additional shielding pulls e- in tighter
Atomic Radius
Atomic Radius (cont.)
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Section 6-3
Atomic Radius (cont.)
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Section 6-3
Ionic Radius
• An ion is an atom or bonded group of atoms with a positive or negative charge.
• When atoms lose electrons and form positively charged ions, they always become smaller for two reasons:
1. The loss of a valence electron can leave an empty outer orbital resulting in a small radius.
2. Electrostatic repulsion decreases allowing the electrons to be pulled closer to the radius.
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Section 6-3
Ionic Radius (cont.)
• When atoms gain electrons, they can become larger, because the addition of an electron increases electrostatic repulsion.
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Section 6-3
Ionic Radius (cont.)
• The ionic radii of positive ions generally decrease from left to right.
• The ionic radii of negative ions generally decrease from left to right, beginning with group 15 or 16.
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Section 6-3
Ionic Radius (cont.)
• Both positive and negative ions increase in size moving down a group.
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Section 6-3
Ionization Energy• Ionization energy is defined as the energy
required to remove an electron from a gaseous atom.
• The energy required to remove the first electron is called the first ionization energy.
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Section 6-3
Ionization Energy (cont.)
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• Why opposite of atomic radius?
– In small atoms, e- are close to the nucleus where the attraction is stronger
Why small jumps within each group?
– Stable e- configurations don’t want to lose electrons (p1 and p4) lose p1 leaves s2; lose p4 leaves p3
– S sublevel slightly shields the P sublevel
– The 4th electron in enter into a P sublevel will have to pair up with an electron, thus it experiences more repulsion
Ionization Energy
Ionization Energy (cont.)
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Section 6-3
Ionization Energy (cont.)
• Removing the second electron requires more energy, and is called the second ionization energy.
• Each successive ionization requires more energy, but it is not a steady increase.
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Section 6-3
Ionization Energy (cont.)
• The ionization at which the large increase in energy occurs is related to the number of valence electrons.
• First ionization energy increases from left to right across a period.
• First ionization energy decreases down a group because atomic size increases and less energy is required to remove an electron farther from the nucleus.
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– Al 1st I.E. 577 kJ
2nd I.E. 1,815 kJ
3rd I.E. 2,740 kJ
Core e- 4th I.E. 11,600 kJ
• Successive Ionization Energies
– Large jump in I.E. occurs when a CORE e- is removed.
Ionization Energy
Ionization Energy (cont.)
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Section 6-3
Ionization Energy (cont.)
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Section 6-3
Ionization Energy (cont.)
• The octet rule states that atoms tend to gain, lose or share electrons in order to acquire a full set of eight valence electrons.
• The octet rule is useful for predicting what types of ions an element is likely to form.
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Section 6-3
Ionization Energy (cont.)
• The electronegativity of an element indicates its relative ability to attract electrons in a chemical bond.
• Electronegativity decreases down a group and increases left to right across a period.
•Melting points of elements tend to increase in the middle of a period (row) and will decrease at each end of a given row.•Melting points tend to increase as you go down a given group
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Section 6-3
Electronegativity
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A. A
B. B
C. C
D. D
Section 6-3
A B C D
0% 0%0%0%
Section 6.3 Assessment
The lowest ionization energy is the ____.
A. first
B. second
C. third
D. fourth
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A. A
B. B
C. C
D. D
Section 6-3
Section 6.3 Assessment
A B C D
0% 0%0%0%
The ionic radius of a negative ion becomes larger when:
A. moving up a group
B. moving right to left across period
C. moving down a group
D. the ion loses electrons