ch 6.3 periodic trends section 6-3 section 6.3 periodic trends compare period and group trends of...
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CH 6.3 Periodic Trends
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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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Section 6-3
Atomic Radius
• Atomic size is a periodic trend influenced by electron configuration.
• For metals, atomic radius is half the distance between adjacent nuclei in a crystal of the element.
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Section 6-3
Atomic Radius (cont.)
• 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.)
• There is a general decrease in atomic radius from left to right, caused by increasing positive charge in the nucleus.
• Valence electrons are not shielded from the increasing nuclear charge because no additional electrons come between the nucleus and the valence electrons.
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Section 6-3
Atomic Radius (cont.)
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Section 6-3
Atomic Radius (cont.)
• Atomic radius generally increases as you move down a group.
• The outermost orbital size increases down a group, making the atom larger.
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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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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.)
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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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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.
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Section 6-3
Ionization Energy (cont.)
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• Electron affinity- the attraction of an atom for an electron• Metals have low electron affinities• Nonmetals have high electron affinities• General trend of electron affinities as we go down the group is a decreasing tendency
to gain electrons• As we go across the periodic table from left to
right the attraction for electrons increases
Electron Affinity
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A. A
B. B
C. C
D. D
Section 6-3
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
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
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CH 6.3 Assign. Q.20-23, 49, 58-67, 69, 85
THE END