1. The Periodic Table and The Periodic Law

2. Development of the Modern Periodic Table There were multiple people/scientist who contributed to the making of the periodic table as we know it….. 1. Antoine Lavoiser – compiled a list of the 23 elements known in the late 1790s. 2. John Newland – noticed that if the elements were arranged according to the atomic masses, the properties of the elements were repeated. He called it the “Law of Octaves”.

3. Development of the Modern Periodic Table 3. Dimitri Mendeleev – is the person credited with making the 1 st periodic table leaving spaces for the predicted elements in future. (It was based on the atomic masses) 4. Henry Mosley – he then rearranged the periodic table based on atomic numbers and their characteristics, it is used till this date.

4. Modern Periodic Table (Recap) Lavoiser – original 23 elements, 1790’s Newland – Arranged by atomic mass; Law of Octaves – Properties repeated Mendeleev – Left spaces for future elements Moseley – Arranged by atomic numbers and characteristics (current version)

5. Break-up of Periodic Table How is table arranged? What are the rows called? What are the columns called? What are groups? What are families?

6. Break-up of the Periodic Table Periods – Rows of the periodic table are called the periods. (7 periods at present)

7. Periodic Table two rows below the periodic table are the lanthanide and actinide series these rows fit after #57 and #89 they are only at the bottom to keep the width of the chart smaller

8. Break-up of Periodic Table Period

9. Break-up of the Periodic Table Groups/Family – Columns in the periodic table are called the groups. There a total of 18 but further classified: All “A” groups – representative elements All “B” groups – transition element Groups have similar properties

10. Break-up of Periodic Table

11. Break-up of the Periodic Table Within the groups and periods there is further classification: Metals Non-metals Metaloids

12. Break-up of the Periodic Table Within the groups and periods there is further classification: Metals – located on the left, center and bottom of the periodic table.

13. Break-up of Periodic Table

14. Break-up of the Periodic Table Metals Usually, solids at room temperature. Solid at room temperature (all but Hg) malleable- can be rolled or hammered into sheets ductile- can be made into wire high tensile strength- can resist breakage when pulled Lustrous – shiny most have silvery or grayish white luster

15. Break-up of the Periodic Table Within the groups and periods there is further classification: Metals – located on the left, center and bottom of the periodic table. Non-metals – They are located on the right side of the table.

16. Break-up of Periodic Table

17. Break-up of the Periodic Table Non-metals Many are gases If in solid form, they are brittle They are poor conductors of heat and electricity

18. Break-up of the Periodic Table Within the groups and periods there is further classification: Metals – located on the left, center and bottom of the periodic table. Non-metals – located on the right side of the table. Metalloids – located on the “staircase” seen in the periodic table.

19. Break-up of Periodic Table

20. Break-up of the Periodic Table Metaloids Also, known as “semi-conductors” They exhibit properties of both metals and non- metals. B, Si, Ge, As, Sb, Te all are solids at room temperature less malleable than metals but less brittle than nonmetals

21. The s, p, d and f blocks s-block elements – Groups 1 and 2 (1-A and 2-A) Group 1 (1-A) – are called Alkali metals Group 2 (2 – A) – are called Alkaline earth metals p-block elements – Groups 13 – 18 (3-A => 8-A) Group 17 (7-A) – are called Halogens Group 18 (8-A) – are called Noble gases

22. The s, p, d and f blocks d-block elements – are the B group elements (Groups 3 – 12 or 1B – 8B) They are called transition metals f-block elements – are also within the B group placed at the bottom of the periodic table. They are known as the inner-transition metals They are also classified as the Lanthanide and Actinide series

23. Periodic Trends What is an ion? An ion is a charged atom or molecule. It is charged because the number of electrons do not equal the number of protons in the atom or molecule. An atom can be positively charged or a negatively charged depending if the number of electrons in an atom is greater or less then the number of protons in the atom.

24. Ions

25. Periodic Trends

26. What is a trend? It is a characteristic that is repeated. (OR the general course or prevailing tendency) In the periodic table trends occur across a period and down the group. For example: The elements get less metallic across the period The elements become larger in size down a group.

27. Periodic Trends Atomic Radius: It is the distance from the center of the nucleus to the outermost energy level where there are electrons. It increases down the group. Why? The principal energy level increases. It decreases across the period. Why? The energy level is the same but the number of electrons increases and hence the electrostatic attraction increases. Pg. 163

28. Periodic Trends Ionic Radius: It is the distance from the center of the nucleus to the outermost energy level where there are electrons in an ion. Positive ions are small Negative ions are large Pg. 166

29. Periodic Trends Ionization Energy (I.E.): It is the amount of energy needed to remove an electron from an atom. (pg. 167 – 168) The amount of I.E. increases across a period (that is left to right) WHY? The more electrons in the outermost orbital hence more electrostatic attraction The amount of I.E. decreases down a group WHY? The electrons are further away form the nucleus

30. Periodic Trends Electronegativity (E.N.): It is known as the ability of an atom to attract electrons. (pg. 169) E.N. increases across a period E.N. decreases down a group Noble gases are ignored. Fluorine has the largest E.N. Francium the smallest E.N.

31. Practice Problems Which has a higher ionization energy? 1. Fe or Cu 2. Na or Rb 3. Ge or Ga 4. C or Si

32. Practice Problems Which is bigger? 1. K or Li 2. B or Al 3. O or F 4. Fe 2+ or Fe +

33. Practice Problems Which has a greater electronegativity? 1. Ca or Sr 2. Cu or Ag 3. Al or Cl 4. F or N

34. Choose the element with the smaller radius 1. Chromium or tungsten 2. Cadmium or silver 3. Tin or antimony

35. Choose the element with the larger ionization energy 1. Magnesium or aluminum 2. Lithium or potassium 3. Yttrium or scandium 4. Carbon or germanium

36. Choose the element with the smaller electronegativity 1. Lead or Bismuth 2. Bromine or astatine 3. Gallium or phosphorus 4. Mercury or Gold