1. Periodic Table and Groups Periodic Table and Groups

2. Transitional Groups: Representative Groups:

3. Periodic Table: Groups Identify the group number(s) for each group name below. Give an example of an element from each group below. a. Noble Gases b. Alkali Metals c. Alkaline Earth Metals d. Transitional Metals e. Rare Earth Metals f. Halogens

4. Periodic Table: Bell Ringer Periodic Table: Bell Ringer 1. What element is on period 3 group 2 ? 2. Identify the elements below that are not representative elements: Fe, S, Ca, Kr, Ag, U 3. Identify an element on the periodic table that has similar properties with oxygen. 4. a. What is the name of the group that Chlorine is in? b. What is the short-hand electron configuration of Cl? c. How many valence electrons does Cl have?

5. 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?

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

7. Periodic Table: Valence Electrons Periodic Table: Valence Electrons

8. Common Periodic Table Groups Common Periodic Table Groups Periodic GroupsGroup #Valence Electrons Chemical Reactivity (Yes or No) Alkali Metals Alkaline-Earth Metals Transitional Metals Halogens Noble Gases (Inert Gases)

9. Common Periodic Table Groups Common Periodic Table Groups Periodic GroupsGroup #Valence Electrons Chemical Reactivity (Yes or No) Alkali Metals 1 1ve-Yes, chemically reactive because they only has 1 ve-. Most reactive metallic group. Alkaline-Earth Metals 2 2ve- Yes, chemically reactive because they only have 2 ve-. Transitional Metals 3-12 2 ve- Yes, chemically reactive because they only have 2 ve-. Halogens 17 7ve-Yes, chemically reactive because they only have 7ve-. Most reactive non-metallic group. Noble Gases (Inert Gases) 18 8ve-No, not chemically reactive because they have the maximum number of ve-. Most noble elements = 8 ve. Exception: He = 2ve. Most stable elements.

10. Chemical Stability Chemical Stability Octet Rule: Atoms will gain or lose valence electrons to reach maximum stability. Formation of ions. What is maximum stability for most atoms? 8 valence electrons (ve-) Exceptions: H and He max. stability = 2 ve- How do atoms achieve stability ? Atoms chemically bonding with other atoms. Formation of diverse compounds in nature.

11. Metallic vs. Non-metallic Properties Metallic vs. Non-metallic Properties

12. Bell Ringer: Chemical Stability Bell Ringer: Chemical Stability 1. 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 3+ b. Br or Br 1-

13. Chemical Stability Pattern Chemical Stability Pattern Will metals tend to gain or lose valence electrons to reach maximum stability? Will non-metals tend to gain or lose valence electrons to reach maximum stability?

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

15. Chemical Stability Pattern Chemical Stability Pattern Predict what type of ion, if any, each neutral element below would form to reach maximum stability. # of neutral/ion ve- max. stability a. Sodium b. Oxygen c. Argon d. Phosphorus e. Chromium

16. Chemical Stability Chemical Stability Determine what type of ion each element below would form to reach maximum stability. a. Sodium Na 1+ b. Oxygen O 2- c. Argon Ar d. Phosphorus P 3- e. Chromium Cr 2+

17. Valence Electrons Worksheet Key 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-

18. History of the Periodic Table Dmitri Mendeleev: Russian chemist and teacher When organized elements into groups by similar chemical properties, he observed the periods increasing in atomic mass. (1869) His organization system was successful at predicting undiscovered elements. Do you observe any inconsistencies with his organization system?

19. 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. (1913) Currently accepted organization system for elements.

20. Bell Ringer: Atomic Stability Bell Ringer: Atomic Stability 1. What is stability for an atom? 2. Why do many atoms prefer to be ions? 3. Identify each of the following atoms as a neutral, anion, or cation. a. strontium has 36 electrons b. bromine has 36 electrons 4. Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

21. Bell Ringer: Atomic Stability Bell Ringer: Atomic Stability 1. What is stability for an atom? 2. Why do many atoms prefer to be ions? 3. Identify each of the following atoms as a neutral, anion, or cation. a. strontium has 36 electrons b. bromine has 36 electrons 4. Predict, if any, what type of ion each atom below would become to reach stability. a. Fe b. Rn c. I

22. Periodic Table Trends Periodic Table Trends 1. Define each term below related to an atom. 2. Graph data to determine the trend for each term below for an atom. Atomic Radius Ionization Energy Electronegativity

23. Periodic Trend Graph Analysis Periodic Trend Graph Analysis Analysis Procedures: 1. Locate elements in the same period. Does the line graph increase or decrease with these elements in the same period. 2. Repeat step one, but with elements in a different period. 3. Locate elements in the same group. Does the line graph increase or decrease with these elements in the same group? 4. Repeat step three, but with elements in a different group. 5. Share your results with your partners.

24. Periodic Properties and Trends 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. Electronegativity: - The attraction one atom has toward another atom’s valence electron. - Determines the type of chemical bond between atoms.

25. Periodic Table Trends Periodic Table Trends 1. Define each term below related to an atom. 2. Graph data to determine the trend for each term below for an atom. Atomic Radius Ionization Energy Electronegativity

27. Periodic Trends: Atomic Radius

28. Across a Period Down a Group

29. Periodic Table : Atomic Radius

30. Periodic Trends: Ionization Energy Periodic Trends: Ionization Energy

31. Across a Period: Down a Group:

32. Periodic Trend: Electronegativity mmsphyschem.com

33. Periodic Trend: Electronegativity mmsphyschem.com Across a Period: Down a Group:

34. Electronegativity and Chemical Bonding In general what kind of elements have a greater electronegativity value? Using the table, which compounds would have a greater electronegativity difference: NaCl or CO?

35. Electronegativity and Chemical Bonding What do you predict will happen when Na chemically bonds with Cl?

36. Chemical Bonding Chemical Bonding Ionic Bonding: Covalent Bonding:

37. Octet Rule Revised: Octet Rule Revised: Atoms will gain, lose, or share valence electrons to reach stability. The need for stability produces compounds (ionic and covalent)

38. Bell Ringer: Periodic Trends Bell Ringer: Periodic Trends 1Use your graph on atomic radius and ionization energy to answer the following questions: a.Rank the following elements from largest to smallest in size. Explain your results. Ar, Mg, S Al b.Rank the following elements from smallest to largest in ionization energy. Explain your results. Ne, Ar, He

39. Lewis Dot Structures Lewis Dot Structures Illustrate valence electrons for an atom before bonding. Element# of valence electronsLewis Dot Structure Na Mg Si S

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

41. Size of an Ion Size of an Ion Use the diagram below to determine what happens to the size of a neutral atom(parent atom) when it becomes an ion.

42. Size of a Cation Size of a Cation Why is the cation smaller than its parent atom (neutral)?

43. Size of a Cation 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.

44. Size of an Anion Size of an Anion Why is an anion larger than its parent atom?

45. Size of an Anion 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.

46. Size of an Anion Size of an Anion

47. Size of Ions Size of Ions 1. Circle the atom that is larger in size. a. Ca or Ca 2+ b. S or S 2- 2. Circle the atom that is smaller in size. a. Al or Al 3+ b. N or N 3-

48. Ionic Bonding (Lewis Dot Transfer) Ionic Bonding (Lewis Dot Transfer) Metal (Lewis Dot) Non-metal (Lewis Dot) Ionic Bonding (Lewis Dot Transfer) Chemical Formula Na Cl Al N Ca Cl

49. Chemical Bonding Chemical Bonding Lewis Dot Structures: Illustrates the number of valence electrons a neutral atom has prior to chemical bonding.

50. Bell Ringer: Chemical Stability Bell Ringer: Chemical Stability 1. 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 3+ b. Br or Br 1-

51. Hydrogen Lab