1. Unit 3 Marker Board Review Make sure you have the following ready Marker board and marker Periodic table

2. 1.________________ created the first periodic table which was arranged according to atomic _____. 2.In the modern periodic table, elements are ordered by atomic ________. ______________ was the first scientist to order them this way. Dmitri Mendeleev mass number Henry Moseley

3. 3. __________ law says that when the elements are placed in order by atomic number there is a periodic repetition of their chemical and physical properties. 4. ____________________ determine the identity of an element and the atomic number. Periodic Number of protons

4. 5. Groups ___________________ are known as the representative elements because… 6. The valence electrons of representative elements are in the __ and __ orbitals. 1, 2, 13-18 They act….. p s

5. Metals 7. Group 1: called the _______ metals. They have electron configurations ending in __. Properties of these elements include: a. Stored in ___ due to extreme reactivity with oxygen (contains the most reactive metal) b. Consistency is ________. c. Good conductors of ____ and ___________. Alkali s1s1 oil butter heat electricity Extremely reactive, soft in nature

6. 8. Group 2: called the _____________ metals. Their electron configurations end in __. Properties of these elements include: a. generally ____ solids. b. _______ and denser than alkali metals c. Less _______ than alkali metals. Alkaline-Earth s2s2 Here are some props soft Harder reactive

7. 9. The ___________ metals are a large group of elements in the middle of the periodic table. Properties of these elements include: a. Transition metals are also known as the __-block elements b. General properties (similar to other metals) are… c.Most transition metals are _____ solids with _____ melting points. d.Transition metal unpaired d-electrons have the ability to move into the __ level. Because of this, many transition metals can form several different charged ions. e. Transition metals contain the __________ metals (like gold & silver) transition d Properties… hardhigh s precious

8. 10. The ______________ metals are also known as the f-block. The elements in this block are very ____________. inner transition radioactive

9. Nonmetals 11. Group 17 is the _________ family. Their electron configurations end in _____. Properties of these elements include: a. Very _________ nonmetals – they are always in compounds, never alone. b. Halogens tend to gain or share 1 electron because they have __ valence electrons. d. The most reactive nonmetal, _________, is in this family. e. Exist in all 3 _______ of matter (s, l, g) f. React readily with ________, especially alkali, to produce salts. (halogen = salt former) halogen s2p5s2p5 properties reactive 7 fluorine states metals

10. 12. Group 18 elements are the _______ gases. Their electron configurations end in _____. Properties of these elements include: a. Called inert or ______ gases because…. 14. The reason any group has similar properties is because they have the same number of _________________ noble s2p6s2p6 Nonreactive, gases, noble Their outermost energy level is full meaning they don’t need more electrons from other elements. Valence electrons

11. Hydrogen only element considered to be a chemical family all by itself. 15. Hydrogen is placed in group 1 because it has __ valence electron. 16. Hydrogen has properties of group 1 and group ________. 1 17

12. Match the family name to the location: 20. ___ lanthanides and actinides (inner transition metals) 21. ___ alkali and alkaline earth metals 22. ___ halogens 23. ___ noble gases 24. ___ transition metals 25. Label the s, p, d and f blocks on the periodic table. C A D E B s p d f

13. 26. An element has the electron configuration [Ne]3s 2 3p 5. What family is this element in? _________ What group? ____________ What period? __ What is this element? __________________ 17 3 halogen Chlorine

14. Match the element with the family to which it belongs: 27. neon______ 28. magnesium______a = alkali metals 29. fluorine______b = alkaline earth metals 30. silver______c = transition metals 31. potassium______d = halogens 32. iron______e = noble gases E B D C A C

15. Use the following words to fill in the blanks. A = alkali metals B = alkaline-earth metals C = transition metals D = halogens E = noble gases 33. The ____ have electron configurations that end in s 2. 34. The ____ are soft enough to cut with a knife. 35. The ____ contain the precious metals. 36. The ____ are the most reactive nonmetals. 37. The ____ are stable and unreactive due to their full s and p orbitals. 38. The ____ have a name that means salt-former. B A C D E D

16. Periodic Trends 39. As you move down a group on the periodic table, atomic radii generally _______________ and across a period it generally __________________. gets larger gets smaller

17. Periodic Trends 40. Define ionization energy. 41. Ionization energy generally _____________ across a period and ______________ down a group. 42. Which family of elements has the highest ionization energy? ______________ 43. The tendency for an atom to attract electrons of another atom is called __________________. It generally ___________ as you move left to right across a period and __________ down a group. Energy needed to remove an electron from an atom gets larger gets smaller Noble gases electronegativity increases decreases

18. Circle the atom with the LARGER atomic radius 44. cesiumpotassium 45.sodiumaluminum 46. cesium helium Circle the atom with the LARGER ionization energy 47. boronoxygen. 48. nitrogenphosphorous 49. chlorineselenium

19. Circle the atom with the LARGER electronegativity 50. calcium potassium 51. fluorinebromine 52. phosphorusoxygen 53. Be prepared to describe how the trends change across or down the periodic table.