1. Section 6.3 Periodic Trends
Do Now: Standard:1g,2g Terms:163 MasteringConcepts:175(54-67) Practice Problems: 165(16-18) Homework: Cornell Notes:6.3 SectionAssessment:169(19-22)

2. Section 6-3 Compare period and group trends of several properties.
Section 6.3 Periodic Trends
Section 6-3
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

3. Atomic size is a periodic trend influenced by electron configuration.
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.

4. Section 6-3
Atomic Radius (cont.)
For elements that occur as molecules, the atomic radius is half the distance between nuclei of identical atoms.

5. 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.

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

7. Atomic radius generally increases as you move down a group.
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.

8. 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:
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.

9. Section 6-3
Ionic Radius (cont.)
When atoms gain electrons, they can become larger, because the addition of an electron increases electrostatic repulsion.

10. 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.

11. Both positive and negative ions increase in size moving down a group.
Section 6-3
Ionic Radius (cont.)
Both positive and negative ions increase in size moving down a group.

12. 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.

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

14. 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.

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

16. First ionization energy increases from left to right across a period.
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.

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

18. 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.

19. 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.

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

22. Practice Problems: 165 (16-18)
Answer the following questions using your knowledge of group and period trends in atomic radii. Do not use the atomic radii values in Figure 6-11 to answer the questions.

23. Section 6-3 smallest largest Si S
Atomic Radius (cont.)
smallest
largest Mg Si S Na
16. Which has the largest radius: magnesium (Mg), silicon (Si), sulfur (S), or sodium (Na)? The smallest?

24. Section 6-3 smallest Ar largest Xe
Atomic Radius (cont.)
smallest He Ar
largest Xe
17. Which has the largest radius: helium (He), xenon (Xe), or argon (Ar)? The smallest?

25. Section 6-3 smallest Ar largest Xe
Atomic Radius (cont.)
smallest He Ar
largest Xe
17. Which has the largest radius: helium (He), xenon (Xe), or argon (Ar)? The smallest?

26. Practice Problems: 165 (16-18)
Can you determine which of two unknown elements has the larger radius if the only known information is that the atomic number of one of the elements is 20 greater than the other?
No. Based on given information given, periodic trend can’t be applied.