Warm Up: Mendeleev’s Card Game

# Warm Up: Mendeleev’s Card Game

## Warm Up: Mendeleev’s Card Game

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##### Presentation Transcript

1. Work with a partner. Use the scissors to cut the 20 cards from the sheet on your table. You and your partner are together going to make one set of cards. Arrange the cards according to these rules: Mass must increase from left to right in each row. Mass must increase from top to bottom in each column. Combining ratios (O in oxide, Cl in chloride) must be the same in each column.There will be some gaps if you do it right.When you are certain of your arrangement, use little pieces of tape to tape your table together. Warm Up: Mendeleev’s Card Game

2. Chapter 6“The Periodic Table”

3. Section 6.1Organizing the Elements • OBJECTIVES: • Explain how elements are organized in a periodic table.

4. Section 6.1Organizing the Elements • OBJECTIVES: • Identify three broad classes of elements.

5. Section 6.1Organizing the Elements • Some elements (gold & copper) known for 1000s of years. • Only about 13 had been identified by the year 1700. • As more were discovered, a way was needed to organize the elements.

6. The First “Periodic Table” • Mid-1800s, about 70 elements were known • Dmitri Mendeleev – Russian chemist • Arranged elements in order of increasing atomic mass

7. Mendeleev • Left blanks for undiscovered elements • When they were discovered, he had made good predictions • But, there were problems: • Co and Ni; Ar and K; Te and I

8. A better arrangement • In 1913, Henry Moseley – British physicist, arranged elements according to increasing atomic number • The arrangement used today

9. Another possibility: Spiral Periodic Table

10. The Periodic Law says: • When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. • Horizontal rows = periods • There are 7 periods • Vertical column = group (or family) • Similar physical & chemical prop. • Identified by number & letter

11. Areas of the periodic table •One way to categorize elements is by classifying them as: Metals Non-metals and Metalloids •Color-code and label one of the periodic tables on the blank periodic table sheet to indicate which elements are metals, non-metals, and metalloids.

12. Areas of the periodic table • Three classes of elements are: 1) metals, • 2) nonmetals, and • 3) metalloids • Metals: electrical conductors, have luster, ductile, malleable • Nonmetals: gererally brittle and nonlustrous, poor conductors of heat and electricity

13. Areas of the periodic table • Metalloids: border the line • Properties are intermediate between metals and nonmetals

14. Section 6.2Classifying the Elements • OBJECTIVES: • Describe the information in a periodic table.

15. Section 6.2Classifying the Elements • OBJECTIVES: • Classify elements based on electron configuration.

16. Section 6.2Classifying the Elements • OBJECTIVES: • Distinguish representative elements and transition metals.

17. Electron Configurations in Groups • Elements can be sorted into groups based on electron configurations: • Noble gases • Representative elements • Transition metals • Inner transition metals

18. Electron Configurations in Groups • Noble gases are the elements in Group 8A • “Inert gases” - rarely take part in a reaction • Outer s and p sublevels completely full

19. Electron Configurations in Groups • Representative Elements Groups 1A through 7A • Wide range of properties, = a good “representative” • Metals, nonmetals, or metalloids; • Solids, gases, or liquids • Their outer s and p electron configurations are NOT filled

20. Electron Configurations in Groups • Transition metals The B columns of the periodic table • Outer s sublevel full, and is now filling the d sublevel • A “transition” between metal area and nonmetal area • Examples: gold, copper, silver

21. Electron Configurations in Groups • Inner Transition Metals located below the main body of the table, in two horizontal rows • Outer s sublevel full, now filling the f sublevel • Formerly called “rare-earth” elements. Not true. Some are very abundant

22. Electron Configurations in Groups On the same periodic table you color-coded before, indicate which groups are Representative elements Transition metals Inner transition metals and Noble gases.

23. Electron Configurations in Groups Some Groups (columns) have special names. On the blank periodic table, color and label the groups: • Alkali metals • Alkali earth metals • Noble gases • Halogens • Transition metals • Lanthanides • Actinides

24. Groups of elements • Group IA – alkali metals • Forms a “base” when reacting with water • Group 2A – alkaline earth metals • Also form bases with water; do not dissolve well, hence “earth metals” • Group 7A – halogens • Means “salt-forming”

25. 8A 1A • Elements in the 1A-7A groups are called the representative elements outer s or p filling 2A 3A 4A 5A 6A 7A

26. These are called the inner transition elements, and they belong here The group B are called the transition elements

27. Group 1A are the alkali metals (not Hydrogen) Group 2A are the alkaline earth metals H

28. Group 8A are the noble gases • Group 7A is called the halogens

29. H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Do you notice any similarity in these configurations of the alkali metals? 1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1

30. He Do you notice any similarity in the configurations of the noble gases? 2 1s2 1s22s22p6 1s22s22p63s23p6 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p65s24d105p6 1s22s22p63s23p64s23d104p65s24d10 5p66s24f145d106p6 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86

31. Elements in the s - blocks s1 • Alkali metals all end in s1 • Alkaline earth metals all end in s2 • really should include He, but it fits better in a different spot, since He has the properties of the noble gases, and has a full outer level of electrons. s2 He

32. Transition Metals - d block Note the change in configuration. s1 d5 s1 d10 d1 d2 d3 d5 d6 d7 d8 d10

33. The P-block p1 p2 p6 p3 p4 p5

34. f6 f13 f1 f2 f3 f4 f5 f7 f8 f10 f12 f14 f11 f9 F - block • Called the “inner transition elements”

35. 1 2 3 4 5 6 7 • Each row (or period) is the energy level for s and p orbitals. Period Number

36. The “d” orbitals fill up in levels 1 less than the period number, so the first d is 3d even though it’s in row 4. 1 2 3 4 5 6 7 3d 4d 5d

37. 1 2 3 4 5 6 7 • f orbitals start filling at 4f, and are 2 less than the period number 4f 5f

38. Thank you for rescuing me, Michael C!

39. Section 6.3Periodic Trends • OBJECTIVES: • Describe trends among the elements for atomic size.

40. Section 6.3Periodic Trends • OBJECTIVES: • Explain how ions form.

41. Section 6.3Periodic Trends • OBJECTIVES: • Describe periodic trends for first ionization energy, ionic size, and electronegativity.

42. Trends in Atomic Size • First problem: Where do you start measuring from? • The electron cloud doesn’t have a definite edge. • They get around this by measuring more than 1 atom at a time.

43. Atomic Size } • Measure the Atomic Radius - this is half the distance between the two nuclei of a diatomic molecule. Radius

44. Periodic Table Trends • Influenced by three factors: 1. Energy Level • Higher energy level is further away. 2. Charge on nucleus (# protons) • More charge pulls electrons in closer. • 3. Shielding effect (a blocking effect?)

45. What do they influence? • Energy levels and Shielding have an effect on the GROUP (  ) • Nuclear charge has an effect on a PERIOD (  )