1. Chapter 6 The Periodic Table and Periodic Law

2. I. History of the Periodic Table A. Just a list In the late 1790s, there were only 23 known elements The advent of electricity made it possible to break down compounds into their component elements http://www.youtube.com/watch?v=OTEX38bQ-2w

3. The development of the spectrometer made it possible to identify new elements By 1870 there were 70 known elements Scientists needed a tool for organizing the many facts associated with the elements

4. B.John Newlands Noticed that when the elements were arranged by increasing atomic mass, their properties repeated every eighth element A pattern such as this is called periodic

5. C. Mendeleev and Moseley Mendeleev organized the elements into the first periodic table He predicted the existence and properties of undiscovered elements

6. Moseley rearranged the elements by increasing mass number, or number of protons, for a more accurate table The repetition of chemical and physical properties of elements by increasing atomic number is called the periodic law

7. II. The Modern Periodic Table Elements are arranged in order of increasing atomic number into a series of columns, called groups or families, and rows, called periods

8. Each group is number 1 through 8, followed by the letter A or B - the groups designated with an A are often referred to as the main group, or representative elements - the groups designated with a B are referred to as the transition elements

9. A. Classifying the elements 1. Metals Generally shiny when smooth and clean Solid at room temperature Good conductors of heat and electricity Ductile, or easily pounded into thin sheets Malleable, or easily drawn into wires

11. a. Alkali metals Group 1A elements (except for Hydrogen) Extremely reactive

12. b. Alkali earth metals Group 2A elements Less reactive than the alkali metals

13. c.Transition metals d.Inner transition metals i. Lanthanide series Used extensively as phosphors, substances that emit light when struck by electrons ii. Actinide series

14. 2. Nonmetals Generally gases or brittle, dull-looking solids Poor conductors of heat and electricity The only liquid nonmetal is bromine (Br)

15. a.Halogens Group 7A Highly reactive

16. b. Noble gases Group 8A Extremely unreactive

17. 3. Metalloids, or semimetals Elements with physical and chemical properties of both metals and nonmetals

18. III. Organizing the Elements by Electron Configuration A. Valence electrons Electrons in the highest principal energy level Atoms in the same group have similar chemical properties because they have the same number of valence electrons

20. B. Valence electrons and period The energy level of an element’s valence electrons indicates the period on the periodic table in which it is found ex. Lithium’s valence electron is in the second energy level and lithium is found in period 2

21. C.Valence electrons and group number A representative element’s group number indicates the number of valence electrons it has (with the exception of helium)

22. IV. The s-, p-, d-, and f-block Elements The periodic table is divided into four blocks

23. A. s-block elements Consists of groups 1A and 2A as well as helium Valence electrons occupy only s orbitals Group 1A elements have partially filled s orbitals containing one valence electron (s 1 )

24. Group 2A elements have completely filled s orbitals containing two valence electrons (s2) Because s orbitals hold a maximum of two electrons, the s-block portion of the periodic table spans two groups

25. B. p-block elements After the s-block is full, valence electrons next occupy the p sublevel and its three p orbitals The p-block spans six groups on the periodic table because three p orbitals can hold a maximum of six electrons

26. The group 8A elements have s and p sublevels that are completely filled - this results in an unusually stable atomic structure leaving the elements virtually unreactive

27. C. d-block elements Contains the transition metals The five d orbitals can hold a total of ten elements; thus the d-block spans ten groups on the periodic table

28. Have a filled outermost s orbital of energy level n Have filled or partially filled d orbitals of energy level n-1 ex. Titanium = [Ar] 4s23d2 s-orbital=n= 4 d-orbital=n-1= 3

29. D.f-block elements Contains the inner transition metals Because there are seven f orbitals holding up to a maximum of 14 electrons, the f- block spans 14 columns

30. E. Putting it all together As you proceed down through the periods, the principle energy level increases as well as the number of energy sublevels Period 1:s-block elements Periods 3 and 4:s- and p-block elements Periods 4 and 5:s-, p-, and d-block elements Periods 6 and 7:s-, p-, d-, and f-block elements

31. V. Atomic Radius The outer limit of an electron cloud is defined as the spherical surface within which there is a 90% probability of finding an electron

32. Atomic size is defined by how closely an atom lies to a neighboring atom, which varies from element to element

33. A. Trends within periods Atomic size decreases left-to-right across a period Each successive element has one additional electron in the same principal energy level Each element also gains one more proton that pulls the outermost electrons closer to the nucleus

34. B. Trends within groups Atomic size increase as you move down a group A principal energy level is added to elements in each period going down the table Each orbital also increases in size, separating valence electrons further from the nucleus which offsets the pull of the increased nuclear charge

35. Atomic Radius

36. VI. Ionic Radius An ion is an atom that has a positive or negative charge A. When atoms lose electrons and form positively charged ions, they always become smaller

37. The electron lost is always a valence electron 1. may leave an empty outer orbital 2. the repulsion between electrons is less, allowing them to be pulled closer to the nucleus

38. B.When atoms gain electrons and form negatively charged ions, they always become larger The electrostatic repulsion between the atom’s outer electrons forces them to move apart

39. C.Trends within periods 1. Positive ions on the left side of the table become smaller left-to-right 2. Negative ions on the right side of the table become smaller left to right

40. D.Trends within groups As you move down a group, an ion’s outer electrons are in higher principal energy levels, resulting in a gradual increase in ionic size

41. VII. Ionization Energy Ionization energy is the energy required to remove an electron from an atom Energy is needed to overcome the attraction between the positive charge in the nucleus and the negative charge in the electrons -a high ionization energy indicated the atom has a strong hold on its electrons -a low ionization energy indicates an atom loses its outer electrons easily

42. Group 1A elements have low ionization energies Group 8A elements have high ionization energies

43. The energy required to remove the first electron from an atom is called the first ionization energy The energy required to remove the second electron is called the second ionization energy

44. For each element there is an ionization for which the required energy jumps dramatically - related to the atom’s number of valence electrons - atom’s hold onto their core electrons much more strongly than they hold onto their valence electrons

45. A. Trends within periods Generally increases left-to-right B.Trends within groups Generally decreases down a group Valence electrons farther from the nucleus require less energy to remove them

46. C. Octet rule States that atoms tend to gain, lose, or share electrons in order to acquire a full set of eight valence electrons - hydrogen and helium are complete with two valence electrons

47. 1.Elements on the right side of the table tend to gain electrons (become negative ions) to acquire the noble gas configuration 2.Elements on the left side of the table tend to lose electrons (become positive ions)

48. VIII. Electronegativity Indicates the relative ability of its atoms to attract electrons in a chemical bond Expressed in Paulings; numerical values of 4.0 or less Fluorine is the most electronegative element (3.98) Cesium (0.79) and Francium (0.7) are the least electronegative elements

49. A.Trends within periods and groups Generally decreases as you move down a group Increases from left-to-right