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. However, _________ determine the chemical behavior. Periodic Number of protons electrons

4. 5. Groups ___________________ are known as the representative elements. 6. The valence electrons of representative elements are in the __ and __ orbitals. 1, 2, 13-18 (or 1A-8A) 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. Form ____ (charge) ions. c. Good conductors of ____ and ___________. Alkali s1s1 oil +1 heat electricity Extremely reactive, soft in nature Metals are positive losers

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. d. Form ___ (charge) ions. Alkaline-Earth s2s2 soft Harder reactive +2 Yet more reactive than the transition metals

7. 9. The ___________ metals are a large group of elements in the middle of the periodic table. Properties of these elements include: 10. Transition metals are also known as the __-block elements 11. General properties (similar to other metals) are… a.Most transition metals are _____ solids with _____ melting points. b.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. c. Transition metals contain the __________ metals (like gold & silver) transition d hard high s precious

8. 12. The ______________ metals are also known as the f-block. The top row is called the ___________ and the bottom row the ________. This group contains synthetic and radioactive metals. inner transition Lanthanides Actinides

9. Nonmetals 13. 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. c. Form ___ (charge) ions. 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 reactive 7 fluorine states metals Nonmetals are negative gainers

10. 14. Group 18 elements are the _______ gases. Their electron configurations end in _____. Properties of these elements include: a. Called inert or ______ gases because…. b. Do not form _____ or ______. 15. The reason any group has similar properties is because they have the same number of _________________ noble s2p6s2p6 Their outermost energy level is full meaning they don’t need more electrons from other elements. ionsbonds Valence electrons

11. Hydrogen only element considered to be a chemical family all by itself. 16. Hydrogen is placed in group 1 because it has __ valence electron. 17. Hydrogen has properties of group 1 and group ________. 18. The universe is __________% hydrogen by mass. 1 1 & 17 90

12. Match the family name to the location: 19. ___ lanthanides and actinides (inner transition metals) 20. ___ alkali and alkaline earth metals 21. ___ halogens 22. ___ noble gases 23. ___ transition metals 24. Label the s, p, d and f blocks on the periodic table. C A D E B s p d f

13. 25. 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 or (7A) 3 halogen Chlorine

14. Match the element with the family to which it belongs: 26. neon______ 27. magnesium______a = alkali metals 28. fluorine______b = alkaline earth metals 29. silver______c = transition metals 30. potassium______d = halogens 31. 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 32. The ____ have electron configurations that end in s 2. 33. The ____ are soft enough to cut with a knife. 34. The ____ contain the precious metals. 35. The ____ are the most reactive nonmetals. 36. The ____ are stable and unreactive due to their full s and p orbitals. 37. The ____ have a name that means salt-former. B A C D E D

16. Periodic Trends 38. As you move down a group on the periodic table, atomic radii generally _______________ and across a period it generally __________________. gets larger gets smaller Gets larger because as you move down a group, an energy level is added, which blocks the power of the nucleus to pull in. gets smaller because the more protons an atom has the stronger the pull of the nucleus and the smaller the atom becomes.

17. Periodic Trends 39. Define ionization energy. 40. Ionization energy generally _____________ across a period and ______________ down a group. 41. Which family of elements has the highest ionization energy? ______________ Energy needed to remove an electron from an atom gets larger gets smaller Noble gases gets larger because the atomic radius is getting smaller, which makes it more difficult to take an electron gets smaller because the atomic radius is getting larger, which makes it easier to remove an electron

18. 42. 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. This group of elements doesn’t have an electronegativity _______________________ electronegativity increases decreases Noble gases, because they don’t form compounds Increases because as the ionization energy goes up and the atomic radius goes down, the atom will hold onto electrons shared in a bond more. If an atom will hold onto its own electrons tightly, it will hold onto shared electrons tightly. Decreases because as the ionization energy goes down and the atomic radius goes up, the atom won’t hold onto electrons shared in a bond as tightly. If an atom won’t hold onto its own electrons tightly, it won’t hold onto shared electrons tightly.

19. Circle the atom with the LARGER atomic radius 43. cesiumpotassium 44.sodiumaluminum 45. cesium helium Circle the atom with the LARGER ionization energy 46. boronoxygen. 47. nitrogenphosphorous 48. chlorineselenium Be prepared to justify your answers.

20. Circle the atom with the LARGER electronegativity 49. calcium potassium 50. fluorinebromine 51. phosphorusoxygen Be prepared to justify your answers.