1. Section 6.3 Periodic Trends
Compare period and group trends of several properties.
principal energy level: the major energy level of an atom
Relate period and group trends in atomic radii to electron configuration.
ion
ionization energy
octet rule
electronegativity
Trends among elements in the periodic table include their size and their ability to lose or attract electrons
Section 6-3

2. 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

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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4. Atomic Radius (cont.)
Section 6-3

5. Atomic Radius
Increases to the LEFT and DOWN
Atomic Radius

6. Why smaller to the right?
Atomic Radius (cont.)
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

7. Atomic Radius (cont.)
Section 6-3

8. 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:
The loss of a valence electron can leave an empty outer orbital resulting in a small radius.
Electrostatic repulsion decreases allowing the electrons to be pulled closer to the radius.
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9. Ionic Radius (cont.)
When atoms gain electrons, they can become larger, because the addition of an electron increases electrostatic repulsion.
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10. 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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11. Both positive and negative ions increase in size moving down a group.
Ionic Radius (cont.)
Both positive and negative ions increase in size moving down a group.
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12. 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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13. Ionization Energy (cont.)
Section 6-3

14. Why opposite of atomic radius?
Ionization Energy (cont.)
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

15. 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.
Section 6-3

16. 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.
Section 6-3

17. Successive Ionization Energies
Ionization Energy (cont.)
Successive Ionization Energies
Large jump in I.E. occurs when a CORE e- is removed.
Al 1st I.E kJ
2nd I.E. 1,815 kJ
3rd I.E. 2,740 kJ
Core e- 4th I.E. 11,600 kJ
Ionization Energy

18. Ionization Energy (cont.)
Section 6-3

19. 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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20. 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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21. Electronegativity
Section 6-3

22. A B C D Section 6.3 Assessment
The lowest ionization energy is the ____.
A. first
B. second
C. third
D. fourth A B C D
Section 6-3

23. A B C D 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 A B C D
Section 6-3