1. THE PERIODIC TABLE The Periodic Table was first put together by Demitri Mendeleev.

3. MENDELEEV’S TABLE (~1872)  Arranged according to increasing atomic mass  Elements with similar properties placed in the same vertical column  Missing elements were yet to be discovered and were left blank on the table

4. HENRY MOSELEY – (1887-1915)  British Physicist determined the atomic numbers of the elements  He arranged the periodic table in order of atomic number  His periodic table is the one used today

5. PERIODS –  horizontal rows of the Periodic Table  There are 7 Periods

6. PERIODIC LAW –  When the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

7. GROUPS –  vertical columns of elements on the Periodic Table  Groups are also known as families because they have similar properties.

8. REPRESENTATIVE ELEMENTS  Group A elements

9.  Alkali Metals – Group 1-A elements  Alkaline Earth Metals – Group 2-A elements  Halogens – Group 7-A elements  Noble Gases – Group 0 elements

10. GROUP B ELEMENTS  Transition Metals – In the middle of the Periodic Table  Inner Transition Metals (rare earth metals) – bottom of the Periodic Table

11. Please label your periodic table with the following:  Color the families as follows:  Alkali metals – red  Alkaline earth metals – yellow  Halogens – green  Noble gases – blue  Please outline the representative elements in purple and the transition metals in orange.  Make a key to your colors on the top of the page along with definitions of each family in your own words.

12. CLASSIFICATION OF ELEMENTS  Metals – found on the left-side of the Periodic Table  Nonmetals – found on the right-hand side of the Periodic Table  Metalloids (or semi-metals) – along the stair-step line  Properties are intermediate between metals and nonmetals

13.  Metals are…  Malleable – can be hammered into sheets  Ductile – can be drawn into wires  Shiny or Lustrous  Good conductors/poor insulators of heat and electricity  All solids at room temperature except Hg  Non-metals are…  Brittle but often form crystals  Dull  Good insulators/poor or non- conductors of heat and electricity  Solids, liquids and gases at room temperature  Metalloids  Have properties that are intermediate between metals and nonmetals. CLASSIFICATION OF ELEMENTS

14. Please label your periodic table with the metals, nonmetals and metalloids. Add definitions of these groups on the top of the page.

15. WEDNESDAY BELLWORK  What group or family do the following elements belong to?  F Ag  Ar Xe  H Sr

16. HOMEWORK  Which scientist first proposed the atom was mostly empty space?  The modern periodic table is arranged in order of increasing atomic _________. a. massb. chargec. numberd. radius  Along the periodic chart, groups and families are located vertically/horizontally, and periods are located vertically/horizontally. (Circle the best choice)  The Halogens are group ______________. a.1A b. 2A c. 6Ad. 7A

19. 14.1 – CLASSIFICATION OF THE ELEMENTS  History of the Periodic Table (A Review)  Mendeleev- arranged elements in order of increasing atomic mass  Moseley- arranged elements in order of increasing atomic number  Periodic Law- When the elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.

20. Periodic Trends  The arrangement of the Periodic Table also provides scientists with a general idea of periodic trends. We will now examine those trends. You are responsible for the trends in boldface and underlined print ONLY.

21. Effective Nuclear Charge (Z eff )  The pull the nucleus exerts on the electrons.  The larger the Z eff, the tighter the electrons are pulled and the smaller the atom.  Trend: Z eff is highest near the top right of the periodic table  Write this trend on the appropriate periodic table in your flip book.

22. Question  Which elements in the following pairs would have the highest Z eff ?  Mg or Cl  Rb or Sr  Al or At

23. 14.2 – PERIODIC TRENDS Atomic radius – one-half the distance between the nuclei of two like atoms in a diatomic molecule (ex: Cl 2 ) The more energy levels present, the larger the atom. When comparing atoms that all have similar energy levels, the atoms with the largest nuclei (and thus greatest number of protons) will have the smallest radii. Trend: atomic radius increases from right to left and from top to bottom. Write the trend in your flipbook

24. Atomic Radius Increasing Atomic Radius BIGGEST SMALLEST

25. Question  Place the following elements in order of increasing atomic radius. Ca, C, Ra, Br

26. Ionization energy - energy required to overcome the attraction of the nuclear charge and remove on electron from a gaseous atom to form an ion. 1st ionization energy: the energy required to remove the first electron 2nd ionization energy: the energy required to remove the second electron 3rd ionization energy: the energy required removing the second electron Trend: ionization energy increases from left to right and bottom to top. Please write this trend onto your flipbook. Periodic Trends: Ionization Energy

27. Question  What electron do you think would be easiest to remove, the first, second, or third? Why?

28. Ionization Energy Increasing Ionization Energy

29. Ion Size Anions, or atoms that have gained electrons, are larger than the atoms from which they were formed. The negative charge means more electrons are present causing the size of the ion to be larger. Cations, which are atoms that have lost electrons, are smaller than the atoms from which they were formed. The positive charge means fewer electrons are surrounding the nucleus, thus pulling the existing electrons closer and causing the ion to be smaller. Trend: ionic radius increases from right to left and from top to bottom. Please add this trend to your flipbook. Periodic Trends: Ion Size

30. Ionic Radius Increasing Ionic Radius

31. Question  What is larger; an atom of nitrogen or its anion? Why?

32. Electronegativity – the tendency for the atoms of the element to attract electrons when they are chemically combined with atoms of another element Note: Nobel gases don’t have any electronegativity because their orbitals are filled so they don‘t bond with other elements. Trend: electronegativity increases from left to right and bottom to top. Please add this trend to your flipbook. Periodic Trends: Electronegativity

33. Electronegativity Increasing Electronegativity HIGHEST

34. Question  If hydrogen and fluorine made a bond, which atom would have more bonded electrons near its nucleus?

35. THURSDAY BELLWORK: Place the following elements in order of increasing atomic radius. Ca, C, Ra, Br Place the following elements in order of decreasing ion size. Fr, Ag, Cl, He

36. WEDNESDAY HOMEWORK:  Which group of the periodic table has the highest ionization energies? 1Ab. 2Ac. 3Ad. 7A  Which of the following elements is in the same period as chlorine? a. carbonb. magnesium c. nitrogen d. oxygen  How does atomic radius change from left to right across a period in a periodic table?

37. THURSDAY BELLWORK: 1. Which elements in the following pairs would have the highest Z eff ? Mg or Cl Rb or SrAl or At 2. Which has the largest electronegativity? a. chlorineb. sodiumc. carbon d. fluorine

38. THURSDAY HOMEWORK: What is true of the electron configurations of the noble gases? a. The outermost s and p sublevels are filled. b. The outermost s and p sublevels are partially filled. c. The outermost s and d sublevels are very close in energy and have electrons in them. d. The outermost s and f sublevels are very close in energy and have electrons in them. Which of the following elements has the smallest atomic radius? a. Neb. Ar c. Kr d. Xe