General Chemistry

1. Faculty of Allied Medical Sciences General Chemistry (MGGC-101)& (GRGC-101)

2. Periodic Table andPeriodic properties Supervision: Prof.Dr.Shehata El-Sewedy Dr.Fatma Ahmed

3. Outcomes By the end of this lecture, the students will be able to 1-Understand Periodic Table and the Elements 2-learn to classification of Periodic Table and the Elements 3-To differentiate between Periodic properties such as Atomic radius , Ionization energy, Electron affinity and Electron negativity 4-Recognize development of periodic table

4. What is the periodic table ? What information is obtained from the table ? How can elemental properties be predicted base on the PT ? The Periodic Table and the Elements

5. Dmitri Mendeleev (1869) In 1869 Mendeleev and Lothar Meyer (Germany) published nearly identical classification schemes for elements known to date. The periodic table is base on the similarity of properties and reactivities exhibited by certain elements. Later, Henri Moseley ( England,1887-1915) established that each elements has a unique atomic number, which is how the current periodic table is organized. http://www.chem.msu.su/eng/misc/mendeleev/welcome.html

6. A map of the building block of matter. The Periodic Table http://www.chemsoc.org/viselements/pages/periodic_table.html

7. The way the periodic table usually seen is a compress view, placing the Lanthanides and actinides at the bottom of the stable. The Periodic Table can be arrange by subshells. The s-block is Group IA and & IIA, the p-block is Group IIIA - VIIIA. The d-block is the transition metals, and the f-block are the Lanthanides and Actinide metals Periodic Table Expanded View

8. Layout of the Periodic Table: Metals vs. nonmetals Periodic Table: Metallic arrangement Nonmetals Metals

9. Main (Representative), Transition metals, lanthanides and actinides (rare earth) Periodic Table: The three broad ClassesMain, Transition, Rare Earth

10. Nonmetals, Metals, Metalloids, Noble gases Reading the Periodic Table: Classification

11. Periods: Are arranged horizontally across the periodic table (rows 1-7) These elements have the same number of valence shells. Across the Periodic Table 2nd Period 6th Period

12. Alkali Family: 1 e- in the valence shell Halogen Family: 7 e- in the valence shell Family:Are arranged vertically down the periodic table (columns or group, 1- 18 or 1-8 A,B) These elements have the same number electrons in the outer most shells, the valence shell. Down the Periodic Table

13. Halogen Alkali Noble Gas Alkaline (earth) Chalcogens Transition Metals Notable families of the Periodic Table and some important members: Infamous Families of the Periodic Table

14. He H C N O F Li P Si S Cl Na Al Mg K Ca Zn Cu Fe Br Ag I Individual members of selected Elements & their characteristics Important members - the Elements

15. B • 2p1 Periodic Table e- configuration from the periodic periodic table H 1s1 He 1s2 F 2p5 Be 2s2 B 2p1 C 2p2 N 2p3 Ne 2p6 O 2p4 Li 2s1 Na 3s1 Mg 3s2 Cl 3p5 Si 3p2 S 3p4 Ar 3p6 Al 3p1 P 3p3 K 4s1 Ca 4s2 Zn 3d10 As 4p3 Be 4p5 V 3d3 Mn 3d5 Fe 3d6 Co 3d7 Sc 3d1 Ti 3d2 Ga 4p1 Ge 4p2 Se 4p4 Cr 4s13d5 Kr 4p6 Ni 3d8 Cu 4s13d10 Sr 5s2 Rb 5s1 Nb 4d3 Ru 4d6 Rh 4d7 Mo 5s14d5 Cd 4d10 Sn 5p2 I 5p5 Xe 5p6 Zr 4d2 Tc 4d5 Y 4d1 In 5p1 Sb 5p3 Te 5p4 Ni 4d8 Ag 5s14d10 Hf 5d2 Cs 6s1 Ta 5d3 Re 5d5 Os 5d6 Ir 5d7 W 6s15d5 La 5d1 Rn 6p6 At 6p5 Ni 5d8 Ba 6s2 Hg 5d10 Tl 6p1 Pb 6p2 Bi 6p3 Po 6p4 Au 6s15d10 Mt 6d7 Bh 6d5 Hs 6d6 Fr 7s1 Rf 6d2 Ra 7s2 Db 6d3 Sg 7s16d5 Ac 6d1

16. The periodic table can be classified by the behavior of their electrons Periodic Table: electron behavior

17. Periodic properties The periodic law states that when the elements are arranged by atomic number, their physical and chemical properties vary periodically. Among periodic properties, we will discuss 1- Atomic radius 2- Ionization energy 3- Electron affinity 4- Electron negativity.

18. Atomic Radius: Within the groups of the periodic table, the atomic radius increases as you go down the group. Within the periods of the periodic table, the atomic radius decreases as you move to the right. .

19. Ionization potential: ****ionization energy of an atom is the minimal energy needed to remove the outermost electron from the neutral atom. Within a period, as you move from left to right across a period, first ionization energy increases. WHY? As you move across a period, the atomic radius decreases, that is, the atom is smaller.  The outer electrons are closer to the nucleus and more strongly attracted to the center.  Therefore, it becomes more difficult to remove the outermost electron.

20. Within a group, as you move down a group, first ionization energy decreases. WHY? As you move down a group, the atomic radius increases, that is, the atom is bigger. The outer electrons are farther away from the nucleus and weakly attracted to the center.  Therefore, it becomes easier to remove the outermost electron.

21. Electron Affinity: The electron affinity EA of an atom or ion is the energy change (mainly energy released) with gaining an e by the atom in the gaseous state Cl(g) + e- → Cl-(g) EA= -439 kJ/mol

22. Summary Periodic Table: Map of the Building block of matter Type: Metal, metalloid and Nonmetal Groupings: Representative or main, transition and Lanthanide/Actanides Family: Elements in the same column have similar chemical property because of similar valence electrons Alkali, Alkaline, chalcogens, halogens, noble gases Period: Elements in the same row have valence electrons in the same shell.

24. Quiz time

25. Arrange these elements based on their increasing • Electronegativity • a-Se, Ge, Br, As b. Be, Mg, Ca, Ba

26. Student Question

27. Arrange these elements based on their increasing • Electronegativity • a-Se, Ge, Br, As b. Be, Mg, Ca, Ba Arrange these elements based on their increasing and why?????????? 1- Atomic radius 2- Ionization energy 3- Electron affinity 4- Electron negativity. • Cr, K, Br, Sc • Se, Ca, Cu, Kr

30. Recommended textbooks: 1-Raymond Chang. Chemistry. 10th ed. 2009 2-Zumdehl. International edition. 2009