1. 1/5/15 CHEMISTRY MRS.TURGEON “ You create your own reality.” - Jane Roberts OBJECTIVES SWBAT: 1. Identify 4 periodic trends on the periodic table DO NOW: 1. What was your favorite thing about winter break?

2. 1/9/15 CHEMISTRY MRS.TURGEON “ You create your own reality.” - Jane Roberts OBJECTIVES SWBAT: 1. Identify if there is a periodic trend for density DO NOW: 1. What does it mean to interpolate from a graph?

3. 1/9/15 CHEMISTRY MRS.TURGEON REMINDERS : 1.If you want your science fair board, pick it up by today after school 2.Homework: finish lab analysis

4. 1/9/15 CHEMISTRY MRS.TURGEON “ You create your own reality.” - Jane Roberts OBJECTIVES SWBAT: 1. Identify if there is a periodic trend for density DO NOW: 1. What does it mean to interpolate from a graph?

5. Use a periodic table and your knowledge of the element families to identify each element by name. 1. I am a Noble Gas that is found in the 6 th period. 2. I am a member of the Alkaline Earth family and have 88 electrons. 3. I am a transition metal that is a liquid at room temperature. 4. I am a member of the miscellaneous carbon family that is found in the 5 th period. 5. I am a Halogen that is a gas at room temperature and have 3 energy levels.

6. The answers are … Radon Radium Mercury Tin Chlorine 1. I am a Noble Gas that is found in the 6 th period. 2. I am a member of the Alkaline Earth family and have 88 electrons. 3. I am a transition metal that is a liquid at room temperature. 4. I am a member of the Miscellaneous carbon family that is found in the 5 th period. 5. I am a Halogen that is a gas at room temperature and have 3 energy levels.

7. Periodic Trends In your groups: What is the definition of a “trend”?

8. Periodic Trends There are several important atomic characteristics that show predictable trends that you should know: –Atomic Size –Ionization Energy –Electron Affinity –Electronegativity

9. Atomic Size The bonding atomic radius is defined as one- half of the distance between bonded nuclei.

10. + + + + + + + + Decreasing Atomic Size Across a Period The effect is that the more positive nucleus (+) has a greater pull on the electron cloud (-) The increased attraction pulls the cloud in, making atoms smaller as we move from left to right across a period + + + + Li BeB 1s22s11s22s1 1s22s21s22s2 1s22s22p11s22s22p1 Li Be B

11. Increasing Atomic Size Down a Group Electron Shielding: When you add a significant number of electrons (to a higher energy level) the inner electrons start to “shield” the nucleus from the outer electrons

12. Atomic Radii Li Na K Rb Cs Cl S P Si Al Br Se As Ge Ga I Te SbSn In Tl Pb Bi Mg Ca Sr Ba Be F O N C B 1.52 1.11 1.86 1.60 2.31 1.97 2.44 2.15 2.62 2.17 0.88 0.77 0.70 0.66 0.64 1.43 1.17 1.10 1.04 0.99 1.22 1.22 1.21 1.17 1.14 1.62 1.40 1.41 1.37 1.33 1.71 1.75 1.46 1 2 13 14 15 16 17 INCREASES

13. Li Na K Rb Cs La Xe Kr Zn Cl F He H 3d transition series 4d transition series 0.3 0.25 0.2 0.15 0.1 0.05 0 0 10 20 30 40 50 60 atomic number atomic radius

14. Ionization Energy Amount of energy required to remove an electron from the ground state of a gaseous atom or ion. Given enough energy (in the form of a photon) an electron can leave the atom completely. The number of protons and electrons is no longer equal IONS!!!

15. Ionization Energy Make a prediction in your groups: “As you move from left to right across a period, will ionization energy increase or decrease?”

16. Ionization Energy Generally, as one goes across a row, it gets harder to remove an electron. The larger the atom is, the easier its electrons are to remove. Ionization energy and atomic radius are inversely proportional

17. Ionization Energies Period Group 1 18 INCREASES DECREASES

18. Ions Here is a simple way to remember which is the cation and which the anion: This is a cat-ion. This is Ann Ion. Cats are “paw-sitive” She’s unhappy and negative. +

19. Sizes of Ions Cations are smaller than their parent atoms. –The outermost electron is removed and repulsions are reduced.

20. Sizes of Ions Anions are larger than their parent atoms. –Electrons are added and repulsions are increased.

21. 1/6/15 CHEMISTRY MRS.TURGEON “ We see things as we are, not as they are.” - Jane Roberts OBJECTIVES SWBAT: 1. Identify 4 periodic trends on the periodic table DO NOW: 1. What is electron shielding? How does it affect atomic radius?

22. Electron Affinity Electron affinity = “Love” of electrons Energy change accompanying addition of electron to gaseous atom: Cl + e −  Cl −

23. Electronegativity Electronegativity is a measure of an atom’s attraction for another atom’s electrons. Is directly related to Electron Affinity scale that ranges from 0 to 4. –Fluorine is the most electronegative!!!!

24. ` 1 2 3 4 5 6 1 2 3 4 5 6 Electron Affinity & Electronegativity 7 Be 1.5 Al 1.5 Si 1.8 Ti 1.5 V 1.6 Cr 1.6 Mn 1.5 Fe 1.8 Co 1.8 Ni 1.8 Cu 1.9 Zn 1.7 Ga 1.6 Ge 1.8 Nb 1.6 Mo 1.8 Tc 1.9 Ag 1.9 Cd 1.7 In 1.7 Sn 1.8 Sb 1.9 Ta 1.5 W 1.7 Re 1.9 Hg 1.9 Tl 1.8 Pb 1.8 Bi 1.9 1.5 - 1.9 N 3.0 O 3.5 F 4.0 Cl 3.0 3.0 - 4.0 C 2.5 S 2.5 Br 2.8 I 2.5 2.5 - 2.9 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Ba 0.9 Fr 0.7 Ra 0.9 Below 1.0 H 2.1 B 2.0 P 2.1 As 2.0 Se 2.4 Ru 2.2 Rh 2.2 Pd 2.2 Te 2.1 Os 2.2 Ir 2.2 Pt 2.2 Au 2.4 Po 2.0 At 2.2 2.0 - 2.4 Period Actinides: 1.3 - 1.5 Li 1.0 Ca 1.0 Sc 1.3 Sr 1.0 Y 1.2 Zr 1.4 Hf 1.3 Mg 1.2 La 1.1 Ac 1.1 1.0 - 1.4 Lanthanides: 1.1 - 1.3     1A 2A 3B 4B 5B 6B 7B 1B 2B 3A 4A 5A 6A 7A 8A Hill, Petrucci, General Chemistry An Integrated Approach 2 nd Edition, page 373 INCREASES DECREASES Electronegativity

25. Atomic Radii - size Ionization Energy – energy change when losing an e - Electron Affinity - energy change when gaining an e - Electronegativity – ability to attract e - when in a compound Periodic Trends Forms cation! Forms anion!

26. Octet Rule: atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons As a group: carefully read about the octet rule on pg. 193 in your textbook and make your own notes about this VERY important rule! Periodic Trends Forms cation!

27. Summary of Periodic Trends Ionic size (cations) Ionic size (anions)‏ decreases Atomic radius decreases Ionization energy increases Electron affinity increases Electronegativity increases Atomic radius increases Ionization energy decreases Electron Affinity decreases Electronegativity decreases 1A 2A3A4A 5A 6A7A 0

28. What ion will be formed when K loses 1 e - ? K 1 + (cation) What ion will be formed when O gains 2 e - ? O 2- (anion) Which ion above is more electronegative? O 2- (anion)