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Unit 3 Marker Board Review Make sure you have the following ready •Marker board and marker •Periodic table 1. ________________ Dmitri Mendeleev created the first periodic table which was arranged according to atomic _____. mass 2. In the modern periodic table, elements are ordered by atomic ________. number ______________ Henry Moseley was the first scientist to order them this way. 3. __________ law says that when the elements Periodic are placed in order by atomic number there is a periodic repetition of their chemical and physical properties. 4. Number ____________________ of protons determine the identity of an element and the atomic number. 5. 2, 13-18 Groups1,___________________ are known as the representative elements because… They act….. 6. The valence electrons of representative p orbitals. elements are in the __ s and __ Metals 7. Group 1: called the _______ They have Alkali metals. 1 s electron configurations ending in __. Properties of these elements include: Extremely reactive, soft in nature a. Stored in ___ oil due to extreme reactivity with oxygen (contains the most reactive metal) butter b. Consistency is ________. electricity heat and ___________. c. Good conductors of ____ 8. Group 2: called the _____________ Alkaline-Earth metals. Their electron configurations end in __. s2 Properties of these elements include: Here are some props soft solids. a. generally ____ b. _______ Harder and denser than alkali metals reactive than alkali metals. c. Less _______ 9. Thetransition ___________ 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 d b. General properties (similar to other metals) are… Properties… c.Most transition metals are hard _____ solids with high _____ melting points. d.Transition metal unpaired d-electrons have the ability to move into the s __ level. Because of this, many transition metals can form several different charged ions. e. Transition metals contain the __________ preciousmetals (like gold & silver) 10. The inner ______________ transition metals are also known as the f-block. The elements in this radioactive block are very ____________. Nonmetals 11. Group 17 is thehalogen _________ family. Their electron configurations 2p5 Properties of these elements include: end in s_____. properties a. Veryreactive _________ nonmetals – they are always in compounds, never alone. b. Halogens tend to gain or share 1 electron because they have7__ valence electrons. d. The most reactive nonmetal, fluorine _________, is in this family. e. Exist in all 3 _______ states of matter (s, l, g) metals especially alkali, to produce salts. f. React readily with ________, (halogen = salt former) 12. Group 18 elements are the _______ noble gases. Their electron configurations end in _____. s2p6 Properties of these elements include: Nonreactive, gases, a. Called inert or ______ noble gases because…. Their outermost energy level is full meaning they don’t need more electrons from other elements. 14. The reason any group has similar properties is because Valence electrons they have the same number of _________________ Hydrogen only element considered to be a chemical family all by itself. 15. Hydrogen is placed in group 1 because it has __ 1 valence electron. 16. Hydrogen has properties of group 1 and group 17 ________. Match the family name to the location: C lanthanides and actinides (inner transition metals) 20. ___ A alkali and alkaline earth metals 21. ___ 22. ___ D halogens 23. ___ E noble gases 24. ___ B transition metals p 25. Label the s, p, d and f blocks on the periodic table. s d f 26. An element has the electron configuration [Ne]3s23p5. What family is this element in? halogen _________ What group? 17 ____________ What period? __ 3 What is this element? Chlorine __________________ Match the element with the family to which it belongs: 27. neon ______ E 28. magnesium ______ B a = alkali metals 29. fluorine ______ D b = alkaline earth metals 30. silver ______ C c = transition metals 31. potassium ______ A d = halogens 32. iron ______ C e = noble gases Use the following words to fill in the blanks. A = alkali metals B = alkaline-earth metals C = transition metals D = halogens E = noble gases B 33. The ____ have electron configurations that end in s2. A 34. The ____ are soft enough to cut with a knife. C 35. The ____ contain the precious metals. D 36. The ____ are the most reactive nonmetals. E 37. The ____ are stable and unreactive due to their full s and p orbitals. D 38. The ____ have a name that means salt-former. Periodic Trends 39. As you move down a group on the periodic table, atomic radii generally _______________ gets larger and across a period it generally __________________. gets smaller Periodic Trends 40. Define ionization energy. Energy needed to remove an electron from an atom 41. Ionization energy generally _____________ gets larger across a period and ______________ gets smaller down a group. 42. Which family of elements has the highest ionization energy? ______________ Noble gases 43. The tendency for an atom to attract electrons of another atom is increases as you electronegativity It generally ___________ called __________________. move left to right across a period and __________ decreases down a group. Circle the atom with the LARGER atomic radius 44. cesium potassium 45. sodium aluminum 46. cesium helium Circle the atom with the LARGER ionization energy 47. boron 48. nitrogen 49. chlorine oxygen. phosphorous selenium Circle the atom with the LARGER electronegativity 50. calcium potassium 51. fluorine bromine 52. phosphorus oxygen 53. Be prepared to describe how the trends change across or down the periodic table.