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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. However, _________ electrons determine the chemical behavior. 5. 1, 2, 13-18 (or 1A-8A) are Groups ___________________ known as the representative elements. 6. The valence electrons of representative p orbitals. elements are in the __ s and __ Metals 7. Group 1: called the _______ Alkali metals. They have 1 Properties of these electron configurations ending in s__. elements include: Extremely reactive, soft in nature a. Stored in ___ oil due to extreme reactivity with oxygen (contains the most reactive metal) b. Form ____ +1 (charge) ions. Metals are positive losers c. Good conductors of ____ electricity heat and ___________. 8. Group 2: called the _____________ Alkaline-Earth metals. Their electron configurations end in __. s2 Properties of these elements include: soft solids. a. generally ____ b. _______ Harder and denser than alkali metals c. Less reactive _______ than alkali metals. Yet more reactive than +2 (charge) ions. d. Form ___ the transition metals transitionmetals are a large group of elements in the 9. The ___________ middle of the periodic table. Properties of these elements include: 10. Transition metals are also known as the __-block elements d 11. General properties (similar to other metals) are… a.Most transition metals are _____ _____ melting points. hardsolids with high b.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. c. Transition metals contain the __________ precious metals (like gold & silver) 12. The ______________ inner transition metals are also known as the f-block. The top row is called the Lanthanides ___________ and the bottom row the Actinides This group contains synthetic ________. and radioactive metals. Nonmetals 13. Group 17 is thehalogen _________ family. Their electron configurations 2p5 Properties of these elements include: end in s_____. a. Very _________ reactivenonmetals – they are always in compounds, never alone. b. Halogens tend to gain or share 1 electron because they have __ 7 valence electrons. c. Form ___ -1 (charge) ions. Nonmetals are negative gainers d. The most reactive nonmetal, _________, fluorine is in this family. e. Exist in all 3 _______ states of matter (s, l, g) f. React readily with ________, metals especially alkali, to produce salts. (halogen = salt former) 14. Group 18 elements are the _______ noble gases. Their electron configurations end in _____. s2p6 Properties of these elements include: a. Called inert or ______ noble gases because…. Their outermost energy level is full meaning they don’t need more electrons from other elements. b. Do not form _____ ions or ______. bonds 15. The reason any group has similar properties is because they have the same number of _________________ Valence electrons Hydrogen only element considered to be a chemical family all by itself. 16. Hydrogen is placed in group 1 because it has __ 1 valence electron. 17. Hydrogen has properties of group 1 and group ________. 1 & 17 18. The universe is __________% hydrogen by mass. 90 Match the family name to the location: C lanthanides and actinides (inner transition metals) 19. ___ A alkali and alkaline earth metals 20. ___ 21. ___ D halogens 22. ___ E noble gases 23. ___ B transition metals p 24. Label the s, p, d and f blocks on the periodic table. s d f 25. An element has the electron configuration [Ne]3s23p5. What family is this element in? halogen _________ What group? 17 ____________ or (7A) What period? __ 3 What is this element? Chlorine __________________ Match the element with the family to which it belongs: 26. neon ______ E 27. magnesium ______ B a = alkali metals 28. fluorine ______ D b = alkaline earth metals 29. silver ______ C c = transition metals 30. potassium ______ A d = halogens 31. 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 32. The ____ have electron configurations that end in s2. A 33. The ____ are soft enough to cut with a knife. C 34. The ____ contain the precious metals. D 35. The ____ are the most reactive nonmetals. E 36. The ____ are stable and unreactive due to their full s and p orbitals. D 37. The ____ have a name that means salt-former. Periodic Trends 38. As you move down a group on the periodic table, atomic radii generally _______________ gets larger and across a period it generally __________________. 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. Periodic Trends 39. Define ionization energy. Energy needed to remove an electron from an atom 40. Ionization energy generally _____________ gets larger across a period and ______________ gets smaller down a group. • gets larger because the atomic radius is getting • gets smaller because the atomic smaller, which makes it radius is getting larger, which more difficult to take an makes it easier to remove an electron electron 41. Which family of elements has the highest ionization energy? ______________ Noble gases 42. The tendency for an atom to attract electrons of electronegativity another atom is called __________________. It increases generally ___________ as you move left to right decreases across a period and __________ down a group. • 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. This group of elements doesn’t have an electronegativity _______________________ Noble gases, because they don’t form compounds Be prepared to justify your answers. Circle the atom with the LARGER atomic radius 43. cesium potassium 44. sodium aluminum 45. cesium helium Circle the atom with the LARGER ionization energy 46. boron 47. nitrogen 48. chlorine oxygen. phosphorous selenium Circle the atom with the LARGER electronegativity 49. calcium potassium 50. fluorine bromine 51. phosphorus oxygen Be prepared to justify your answers.