1. Periodic Table: Bell Ringer
What does a period and a group refer to on the periodic table?
What period and group is Bromine on?
What element is on period 5 and group 10?
For homework, how did you classify the elements on the periodic table?

2. Periodic Table

3. Metallic Properties

4. Non-metallic Properties

5. History of the Periodic Table
Dmitri Mendeleev:
Russian chemists and teacher
When organized elements into groups by similar chemical properties,
he observed the periods increasing in atomic mass.
His organization system was successful at predicting undiscovered elements.
Do you observe any inconsistencies with his organization system?

6. History of Periodic Table
Henry Moseley:
British Physicists
Observed that when elements were placed in groups by chemical properties, the periods consistently increased by atomic number.
Currently accepted organization system for elements.

7. Bell Ringer: Periodic Table
1. How is the current periodic table arranged?
2. Classify the following properties as metallic or non- metallic.
a. ductile b. low density c. high luster d. insulator
3. What element is on period 3; group 16?
4. Circle the elements below that have similar chemical properties:
Carbon (C); Nitrogen (N); Silicon (Si); Boron (B)

8. Organization of Periodic Table
Why do elements in the same group have similar chemical properties?

9. Valence Electrons
Electrons in the highest energy level of an element’s atom.
Calculate using short-hand electron configuration.
Determines the chemical reactivity of an element.

10. Periodic Table : Bell Ringer
1. a. What period and group is Aluminum on?
b. What element is in period 4; group 2 ?
2. Circle the elements below that have similar chemical properties.
Carbon (C), Nitrogen, (N), Silicon (Si), Boron (B)
3. What are valence electrons?
4. Why is it important to know the number of valence electrons an element can have?

11. Short-Hand Electron Configuration
Short -hand configuration targets valence electrons
Ex.
Sulfur (S): [ Ne] 2s22p4 = 6 valence electrons

12. Valence Electrons Worksheet Key
1. 7 ve ve- 2. 5ve ve- 3. 2ve ve- 4. 5ve ve- 5. 2ve ve- 6. 8ve ve- 7. 1ve ve- 8. 2ve ve- 9. 2ve ve ve ve-

13. Organization of Periodic Table
Why do elements in the same group have similar chemical properties?

14. Periodic Table Lab: Valence Electrons
grps
grp 1
ve-
grp 2
grp 3-12
grp 13 ve-
grp 14
grp 15
grp 16
grp17
grp18 A B C D
What can be concluded from the data table?

15. Periodic Table: Valence Electrons
Lab
grps
grp 1
ve-
grp 2
grp 3-12
grp 13 ve-
grp 14
grp 15
grp 16
grp17
grp18 A 1 2 3 4 5 6 7 8 B C D
What can be concluded from the data table?

16. Common Periodic Table Groups
Periodic Groups
Group #
Valence Electrons
Chemical Properties
Alkali Metals 1
1 ve-
Highly Reactive metals
Only needs to lose 1 ve- to reach STABILITY. Depends on lower energy level that is filled.
Alkaline-Earth Metals 2
2ve-
Reactive
Only needs to lose 2 ve- to reach STABILITY.
Depends on lower energy level that is filled.
Transitional
Metals
3-12
Varies in amount of valence electrons lost to reach STABILITY.
Halogens 17
Highly Reactive non-metals.
Only needs to gain 1 ve- to reach STABILITY.
Depends on filling up outer energy level.
Noble Gases 18
Inert non-metal gases.
Not reactive elements.
Very STABLE elements because outermost energy level is filled, 8ve.
Exception: 2 ve for He.

17. Chemical Stability Metals: Will lose ve- to reach stability.
Form cations (+ charged atoms)
Non-metals:
Will gain ve- to reach stability.
Form anions (- charged atoms)

18. Chemical Stability
Determine what type of ion each element below would form to reach maximum stability. a. Sodium Na1+ b. Oxygen O2- c. Argon Ar d. Phosphorus P3- e. Chromium Cr2+

19. Bell Ringer: Chemical Stability
Write down what comes to mind when you think about chemical stability for elements.
2. Label your periodic table with the following groups:
Alkali metals (Group 1)
Alkaline earth metals (Group 2)
Halogens (Group 17)
Noble gases (Group 18)
Transitional metals (Group 3-12)

20. Periodic Table and Groups

21. Ions and Chemical Stability Lab
In pairs, look at 16 different elements and answer the following questions:
Metal or non-metal
Neutral, anion, or cation.
Symbol and specific charge if needed.
*neutral if element is naturally stable (noble gas)
*anion: non-metal not naturally stable
*cation: metals

22. Size of an Ion
Use the diagram below to determine what happens to the size of an atom when it becomes an ion.

23. Size of a Cation A cation is smaller than its parent atom.
Why? Because metals will lose an energy level in the process
of becoming a cation.

24. Size of a Cation

25. Size of an Anion

26. Size of an Anion A anion is larger than its parent isotope.
Why? Repulsion force increases as more electrons are
added to the outer most energy level. Swells the energy level.

27. Size of an Anion

28. Size of Ions Circle the atom that is larger in size. Ca or Ca2+
S or S2-
Circle the atom that is smaller in size.
a. Al or Al3+
b. N or N 3-

29. Bell Ringer: Chemical Stability
a. Most stable group on periodic table? Explain.
b. Most reactive metallic group? Explain.
c. Most reactive non-metallic group? Explain.
2. Predict what type of ion each element below would form to reach maximum stability.
a. Cesium b. Selenium c. Helium
3. Identify which atom is larger in each example below.
a. Al or Al b. Br or Br 1-

30. Periodic Trends

31. Periodic Properties and Trends
Atomic Radius:
-Size of an atom.
Distance from nucleus to highest energy level for that atom. (picometers, pm).
Ionization Energy:
Energy required to remove an electron from an atom.
Energy required to form a cation.

32. Periodic Trends: Atomic Radius

33. Periodic Trends: Atomic Radius
Across a Period
Down a Group

34. Periodic Trends: Ionization Energy

35. Periodic Trends: Ionization Energy
Across a Period:
Down a Group:

36. Exit Slip
Use your graph on atomic radius and ionization energy answer these questions:
Rank the following elements from largest to smallest in size. Explain your results.
Ar, Mg, S Al
Rank the following elements from smallest to largest in ionization energy. Explain your results.
Ne, Ar, He

37. Periodic Table Transitional Elements: short groups.
Representative Elements: tall groups .
Transitional Elements: short groups.

38. Hydrogen Lab