1. TEKS 5 – The student understands the historical development of the Periodic Table and can apply its predictive power. (5 A-C) STAAR Chemistry Review Topic: Periodic Table

2. Student Expectation (SE) – 5A Explain the use of chemical and physical properties in the historical development of the Periodic Table.

3. INDEX CARD TIME! Title: History of Periodic Table Front: 1. Mendeleev 2. Moseley Back: Write a statement that explains how each man organized the Periodic Table

4. Mini - Review In 1869, Mendeleev published a table of the elements organized by increasing atomic mass. Through his work with X-rays, Moseley determined the actual nuclear charge (atomic number) of the elements. He rearranged the elements in order of increasing atomic number. Periodic Law states: When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties.

5. Student Expectation (SE) – 5B Use the Periodic Table to identify and explain the properties of chemical families, including alkali metals, alkaline earth metals, halogens, noble gases, and transition metals.

6. INDEX CARD TIME! Title: Periodic Table Front: Definitions » 1. Periodic Table » 2. Valence electrons Back: Define each term

7. Mini - Review Periodic Table – Chart of elements ordered by atomic number and grouped by valence electrons Atomic number is the key to the organization of the periodic table. Elements are listed by atomic number! Valence Electrons – Electrons in an atom’s outermost shell; can be gained, lost or shared A full outermost shell is 8 electrons (except for He which has 2) – known as octet rule for elements with an atomic number of less than 20

8. INDEX CARD TIME! Title: Periodic Table Front: Definitions » 1. Row or Period » 2. Column or Group (family) Back: Define each term

9. Mini - Review Row or Period - The horizontal rows of the periodic table; elements are in order of increasing atomic number atomic number = # of protons = # electrons (in a neutral atom) Column or Group (Family) – The vertical rows of the periodic table; elements in a group have the same number of valence electrons and have similar physical and chemical properties

10. INDEX CARD TIME! Title: Periodic Table Front: Definitions » 1. Oxidation number » 2. Anion » 3. Cation Back: Define each term

11. Mini - Review Oxidation number- number assigned to an atom or ion that represents the number of electrons gained or lost Anion – gains electrons; oxidation number is negative Ex. F gains one electron → F - → oxidation # is -1 Cation – loses electrons; oxidation number is positive Ex. Ca loses 2 electrons → Ca +2 → oxidation # is +2

12. INDEX CARD TIME! Title: Physical Properties of Elements Front: 1. Metals 2. Nonmetals 3. Metalloids Back: Draw and label the periodic table showing where each of these is located

13. Mini - Review

14. INDEX CARD TIME! Title : Properties of Chemical Families Front: Alkali Metals Back: Draw a diagram showing the location of the Alkali Metals and list their properties

15. Mini - Review The Alkali Metals – Group 1 – the first column of the periodic table on the left – have only one electron in their outer shell – very reactive metals; wants to lose one electron – do not occur freely in nature – silvery-colored metals – soft, and can be cut easily with a knife – Malleable – good conductors of heat and electricity – have low densities – can explode if they are exposed to water

16. INDEX CARD TIME! Title : Properties of Chemical Families Front: Alkaline Earth Metals Back: Draw a diagram showing the location of the Alkaline Earth Metals and list their properties

17. Alkaline Earth Metals – Group 2 – found in the second group of the periodic table – 2 electrons in their outer energy shell – very reactive - although not as reactive as the alkali metals; wants to lose 2 electrons – not found freely in nature – are shiny, silvery white metals – each of the metals will give a different colored flame Mini - Review

18. INDEX CARD TIME! Title : Properties of Chemical Families Front: Halogens Back: Draw a diagram showing the location of the Halogens and list their properties

19. Halogens – have 7 electrons in their outer-most energy level – very reactive – found in nature as diatomic molecules – physical appearances of the halogens is very different between elements Mini - Review

20. INDEX CARD TIME! Title : Properties of Chemical Families Front: Noble Gases Back: Draw a diagram showing the location of the Noble Gases and list their properties

21. Noble Gases – have full outer electron shell (8 valence electrons except for He which has 2) – inert; will not readily react with other elements – found at room temperature as gasses, and they have very low boiling points Mini - Review

22. INDEX CARD TIME! Title : Properties of Chemical Families Front: Transition Metals Back: Draw a diagram showing the location of the Transition Metals and list their properties

23. Transition Metals – 38 elements in groups 3 through 12 – Metals in table’s center – Has partially filled shell – have different numbers of valance electrons in their outer energy level (variable oxidation numbers) ex. Cu 1+ or Cu 2+ – mallable – conduct electricity and heat – iron, cobalt, and nickel are the only elements known to produce a magnetic field Mini - Review

24. Use the Periodic table to identify and explain periodic trends, including atomic and ionic radii, electronegativity, and ionization energy Student Expectation (SE) – 5C

25. INDEX CARD TIME! Title: Periodic Trends Front: Atomic Radius Back: 1.Draw a periodic table and label with arrows the trend for atomic radius. 2. In a short sentence describe what is happening.

26. Mini - Review More electrons = fatter = larger radius (attraction from nucleus felt less) Size of the Atom – Measured as half the distance between the nuclei of two atoms of the element Decreases Left to Right – Within the energy level adding more electrons and protons increases the attraction between the nucleus and the electrons causing the electrons to be pulled in tighter Increases Top to Bottom – Adding more levels further out from the nucleus makes the atom bigger

28. Here is a graph of atomic radius

29. INDEX CARD TIME! Title: Periodic Trends Front: Ionic Radii Back: 1.Draw a periodic table and label with arrows the trend for ionic radii. 2. In a short sentence describe what is happening.

30. Mini - Review Size of the ion (atoms that have lost or gained an electron) Decreases Left to Right – Positive Ions decrease & Negative Ions decrease – There is a “jump” crossing from Positive to Negative Ions Increases Top to Bottom – Adding more levels further out from the nucleus makes the Ions bigger

31. Ionic Radius Decreases * IncreasesIncreases * Jumps between + ions and – ions then gets smaller again

32. INDEX CARD TIME! Title: Periodic Trends Front: Ionization Energy Back: 1.Draw a periodic table and label with arrows the trend for ionization energy 2. In a short sentence describe what is happening.

33. Mini - Review Energy needed to take an electron away Increases Left to Right – These atoms are smaller and have a greater pull from the nucleus and will require more energy to take an electron away (they usually want more electrons) Decreases Top to Bottom – Electrons are further away from the nucleus and will require less energy to take an electron away Low ionization energy means that the electron removed is not held tightly

34. Ionization Energy Increases DecreasesDecreases

35. INDEX CARD TIME! Title: Periodic Trends Front: Electronegativity Back: 1.Draw a periodic table and label with arrows the trend for electronegativity 2. In a short sentence describe what is happening.

36. Mini - Review How much it “loves” it electrons Ability of an atom to attract electrons Increases Left to Right – These atoms are smaller and have a greater pull from the nucleus and will have a higher attraction for more electrons Decreases Top to Bottom – Electrons are further away from the nucleus and will have less attraction for more electrons

37. Electronegativity Increases DecreasesDecreases

38. Here is a graph of electronegativity