Periodic Table: Bell Ringer

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- 11. 1ve- 2. 5ve- 12. 2ve- 3. 2ve- 13. 4ve- 4. 5ve- 14. 7ve- 5. 2ve- 15. 6ve- 6. 8ve- 16. 2ve- 7. 1ve- 17. 3ve- 8. 2ve- 18. 1ve- 9. 2ve- 19. 8ve- 10. 6ve- 20. 2ve-

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

14. Periodic Table Lab: Valence Electrons What can be concluded from the data table?

15. Periodic Table: Valence Electrons What can be concluded from the data table?

16. Common Periodic Table Groups

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 Al3+ 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 • Representative Elements: tall groups . • Transitional Elements: short groups.

38. Hydrogen Lab