3. The Periodic Table Dmitri Mendeleev (1834 - 1907)

4. Elements are arranged: Vertically into Groups Horizontally Into Periods

5. Why?

6. If you looked at one atom of every element in a group you would see…

7. Each atom has the same number of electrons in its outermost shell. An example…

8. The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

9. The number of outer or “valence” electrons in an atom affects the way an atom bonds. The way an atom bonds determines many properties of the element. This is why elements within a group usually have similar properties.

10. If you looked at an atom from each element in a period you would see…

11. Each atom has the same number of electron shells. An example…

12. The period 4 atoms each have 4 electron containing shells K (Potassium) Atom Fe (Iron) Atom Kr (Krypton) Atom 4 th Shell

13. Each group has distinct properties The periodic Table is divided into several groups based on the properties of different atoms.

14. Alkali Metals Soft, silvery coloured metals Very reactive!!! http://www.lyon. edu/webdata/U sers/DMcDowel l/GenChem/alka lishow.html

15. Group 1A: Alkali Metals Cutting sodium metal Reaction of potassium + H 2 O

16. Alkali Metals reacting with water: Li (Lithium) – least reactiveLi (Lithium) Na (Sodium) K (Potassium) Rb (Rubidium) Cs (Cesium) – more reactiveCs (Cesium)– What would you expect from Francium?!?!

17. Magnesium Magnesium oxide Group 2A: Alkaline Earth Metals

18. Alkaline Earth Metals Silvery-White Metals Fairly reactive Many are found in rocks in the earth’s crust

19. Transition Metals Malleable (easily bent/hammered into wires or sheets) Most are good conductors of electricity

20. How many things can you think of that have Transition Metals in them?

22. Metalloids lie on either side of the “staircase” They share properties with both metals and non-metals Si (Silicon) and Ge (Germanium) are very important “semi-conductors”

23. What are semiconductors used in?

24. Nonmetals Brittle Do not conduct electricity

25. Most are poisonous Fairly reactive – react with alkali metals (eg) Na + and Cl - Halogens

26. Chlorine Gas was used as a chemical weapon during World War I. It was used by the Germans in World War II.

27. Chlorine Gas The Germans were the first to use Chlorine gas at Ypres in 1915 Chlorine gas is a lung irritant The symptoms of gas poisoning are bright red lips, and a blue face People affected die a slow death by suffocation Decades later men who thought they had survived the war died from lung diseases such as Emphysema

28. CHLORINE

29. Unreactive Gases at room temperature Noble Gases

30. Jellyfish lamps made with noble gases artist- Eric EhlenbergerEric Ehlenberger

31. Colors Noble Gases produce in lamp tubes: Ne (Neon): orange-red Hg (Mercury): light blue Ar (Argon): pale lavender He (Helium): pale peach Kr (Krypton): pale silver Xe (Xenon): pale, deep blue

32. Lanthanide Series Actinide Series

33. (A) Periods of the periodic table, and (B) groups of the periodic table.

34. Chemical “Groups” –IA are called alkali metals because they react with water to form an alkaline solution (basic) They are very reactive –Group IIA are called the alkaline earth metals because they are reactive, but not as reactive as Group IA. They are also soft metals –Group VIIA are the halogens These need only one electron to fill their outer shell They are very reactive –Group VIIIA are the noble gases as they have completely filled outer shells They are almost non-reactive.

35. Four chemical families of the periodic table: the alkali metals (IA), the alkaline earth metals (IIA), halogens (VII), and the noble gases (VIIIA).

36. Metal: Elements that are usually solids at room temperature. Most elements are metals. Non-Metal: Elements in the upper right corner of the periodic Table. Their chemical and physical properties are different from metals. Metalloid: Elements that lie on a diagonal line between the metals and non-metals. Their chemical and physical properties are intermediate between the two.

37. An atom consists of a nucleusnucleus –(of protons and neutrons) electrons in space about the nucleus.electrons in space about the nucleus. The Atom Nucleus Electron cloud

38. ATOM COMPOSITION protons and neutrons in the nucleus.protons and neutrons in the nucleus. the number of electrons is equal to the number of protons.the number of electrons is equal to the number of protons. electrons in space around the nucleus.electrons in space around the nucleus. extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water.extremely small. One teaspoon of water has 3 times as many atoms as the Atlantic Ocean has teaspoons of water. The atom is mostly empty space

39. Compounds –composed of 2 or more elements in a fixed ratio –properties differ from those of individual elements –EX: table salt (NaCl)

40. A MOLECULE is 2 more atoms bonded together – they may be the same element (ie diatomic molecule) or they may be different elements (ie caffeine) Composition of molecules is given by a MOLECULAR FORMULA H2OH2OH2OH2O C 8 H 10 N 4 O 2 - caffeine

41. ELEMENTS THAT EXIST AS DIATOMIC MOLECULES Remember: The “GENS” These elements exist as PAIRS when ALONE. Hydrogen (H 2 ) Nitrogen (N 2 ) Oxygen (O 2 ) Halogens (F 2, Cl 2, Br 2, I 2 ) (P 4 and S 8 )

42. Isotopes Atoms of the same element (same Z) but different mass number (A). Boron-10 ( 10 B) has 5 p and 5 n Boron-11 ( 11 B) has 5 p and 6 n 10 B 11 B

43. Isotopes & Their Uses Bone scans with radioactive technetium-99.

44. CARBON-14 – RADIOACTIVE ISOTOPE Occurs in trace amounts in the atmosphere Absorbed into living organisms The half-life of carbon-14 is approx 5700 years (when half the C-14 is converted to N-14)

45. Atomic Symbols Show the name of the element, a hyphen, and the mass number in hyphen notation sodium-23 Show the mass number and atomic number in nuclear symbol form mass number 23 Na atomic number 11

46. Isotopes? Which of the following represent isotopes of the same element? Which element is it? 234 X 234 X 235 X 238 X 92 93 9292 1 2 3 4

47. IONS IONS are atoms or groups of atoms with a positive or negative charge. Donating an electron from an atom gives a CATION with a positive charge Accepting an electron to an atom gives an ANION with a negative charge To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na + Ca +2 I - O -2 Na Ca I O

48. Forming Cations & Anions A CATION forms when an atom loses one or more electrons. An ANION forms when an atom gains one or more electrons Mg --> Mg 2+ + 2 e- F + e- --> F -

49. PREDICTING ION CHARGES In general metals (Mg) lose electrons ---> cations (Mg 2+ ) ons (F - )nonmetals (F) gain electrons ---> anions (F - )

50. –When an atom or molecule gain or loses an electron it becomes an ion. A cation has lost an electron and therefore has a positive charge An anion has gained an electron and therefore has a negative charge.

51. Charges on Common Ions -2-3 +1 +2 By losing or gaining e-, atom has same number of e-’s as nearest Group 8A atom.

52. Learning Check – Counting State the number of protons, neutrons, and electrons in each of these ions. 39 K + 16 O -241 Ca +2 198 20 #p + ___________________ #n o ___________________ #e - ___________________

53. –Elements with 1, 2, or 3 electrons in their outer shell tend to lose electrons to fill their outer shell and become cations. These are the metals which always tend to lose electrons. –Elements with 5 to 7 electrons in their outer shell tend to gain electrons to fill their outer shell and become anions. These are the nonmetals which always tend to gain electrons. –Semiconductors (metalloids) occur at the dividing line between metals and nonmetals.

54. What would the charge be on a sodium ion? EXAMPLE Since sodium in in Group IA it is a metal and so would LOSE an electron You can tell how many would be lost by the group number Group 1A elements lose 1 electron So the charge would be +1 Remember an electron is negatively charged. When you lose them atom becomes positively charged… when you gain them it becomes negatively charged

55. How would you right the symbol for the sodium CATION? EXAMPLE Na +1 How many outer electrons does sodium have before it loses one? It has 1…remember the group number!