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Name: _____ KEY _________ Date: __________ Pd.: ______ AKS Review: The Periodic Table 11) use the organization of the periodic table of elements to predict the properties of elements (GPS, HSGT) (SCCH_B2005-11) 11a) use the periodic table to predict periodic trends including atomic radii, ionic radii, ionization energy, electronegativity, reactivity, and oxidation number of various elements (GPS) 11b) compare and contrast trends in the chemical and physical properties of elements based on their position on the periodic table (GPS) 11b1) identify metals, nonmetals, and metalloids 11b2) determine phases at room temperature __________________________________________________________________________ 1. Define the following terms: Period- horizontal row on periodic table, repeating pattern of properties Groups(families)- vertical column on periodic table. Elements in the same family have similar properties because they have the same valence electron configuration Periodic law- “Properties of elements are a Periodic Function of the atomic number.” When elements are arranged by increasing atomic number there is a periodic repetition of chemical and physical properties. Periodic trend- The properties, atomic radius, ionization energy and electronegativity exhibit a pattern (trend) horizontally across periods and vertically up or down groups. Synthetic- Man Made, usually referring to elements that do not occur naturally Ion- an atom or group of atoms having a charge due to excess or lack of electrons a. Cation- particle having a positive charge (atoms lose electrons to become cations) b. Anion- a particle having a negative charge (atoms gain electrons to become anions) Electronegativity- tendency of an atom to hold electrons of other atoms in a bond; an arbitrary scale indicating how tightly atoms hold electrons. Ionization energy- Energy required to remove the most loosely held (outer) electron (first ionization energy) 2. What were the contributions to the development of the Periodic Table of Mendeleev and Moseley? Mendeleev arranged the periodic table by increasing atomic mass. He predicted that elements like Ge would be discovered and what their properties would be. Using X-ray crystallography, Moseley figured out that the periodic table should be arranged by increasing atomic number instead of atomic mass. 3. Represent the valence electrons by drawing Lewis diagrams for each element across the second period. 4. Label the periodic table below as follows: a. Draw the location of the staircase line b. Shade the metal section, place lines in the nonmetal section and leave the metalloid section blank c. Number Groups 1A-8A d. Label the alkali metals, the alkaline earth metals, the transition metals, the halogens, the noble gasses, the lanthanide and actinide series. IA = alkali metals IIA = alkaline earth elements All the B columns = transition metals IIIA = boron family IVA = carbon family VA = nitrogen family VI A = oxygen family VII A = halogen family VIII a = noble gases 5. What state are most elements in at room temperature? __ 6. What two elements are liquid at room temperature? __ solid __ Hg, Br __ 7. List several physical and chemical characteristics of: Metals Nonmetals Metalloids Physical Malleable, ductile, luster Conduct heat and electricity Solids are brittle crystals Poor conductors of heat and electricity Properties of both metals and nonmetals. semiconductors Chemical Corrode (with notable exceptions) Wide variety of properties Properties of metals and nonmetals Lose electrons to form positive ions (cations) Phase (state of matter) All but Hg solid at room temp. Gain electrons to form negative ions (anions) Various states at room temp. All phases; solid, liquid, gas, are represented 8. Fill in the trend and briefly explain why it occurs. Trend Atomic Radius Ionization Energy Electronegativity Solids at room temp Ionic radius Group Period Increases down because of added energy levels Increases to left because of increased nuclear charge to right Increases up family because valence electrons of smaller atoms are closer to nucleus (held more tightly). Same as EI Smaller atoms hold electrons more tightly than larger atoms Increases to right because larger atoms lose electrons more easily than smaller (atomic radius) Same as ionization energy Smaller atoms hold electrons more tightly than larger atoms - Metal ions are smaller than metal atoms (lose valence electrons) - Nonmetal ions are larger than nonmetal atoms (gain valence electrons) Compare metal and non metal 9. Describe the trend for reactivity in metals. Describe the trend for chemical activity (reactivity) in nonmetals. Since metals lose electrons to react, larger metal atoms are more reactive than smaller ones. Metal reactivity increases to left across a period (from staircase) and down a family. Francium is the most active metal. Since nonmetals gain electrons to react, smaller nonmetal atoms are more reactive than larger ones. Nonmetal reactivity increases to right across a period and up a family. Fluorine is the most active nonmetal. 10. Which metal is most reactive? ___ Francium __ 11. Which nonmetal is most reactive? _ Fluorine __ 12. From the following series choose the element with the larger atomic radius between the two that are given for each problem: a. Na or Cs b. K or Br c. B or F d. O or Se 13. From the following series choose the element with the smaller radius between the two that are given for each problem: a. Mg or Cl b. K or K+ c. Cl or Cld. Ca+ or Br14. From the following series choose the element that is more electronegative and have a higher ionization between the two that are given for each problem: a. Fr or F b. Li or Rb c. Al or S d. N or P Use the list below to answer questions below a. K b. Ag c. O d. F e. S f. Kr 15. Which two elements have similar properties and why? _ P and S because they are in the same family and have similar electron configurations _ 16. Which element(s) is/are halogen(s)? _ F in column VIIA __ 17. Which element(s) is/are transition metal(s)? _ Ag _ 18. Which element(s) would form an anion? _ F, O, and S __ 19. Which element(s) has/have a complete octet and is therefore unreactive? _ Kr _ 20. Which element(s) has/have an oxidation number of -2? _ O and S _ 21. Which Group(s) end(s) with ”s” sublevels? _ alkali metals & Alkaline earth metals _ 22. Why is the d-block ten elements in width? There are 5 orbitals in the d-block. Each orbital holds a maximum of two electrons. 23. What is the purpose of the staircase line? The line separates the metals and nonmetals, and shows the location of metalloids. 24. How do metals become cations? How do nonmetals become anions? Metals lose electrons (negative particles) and become positively charged. Nonmetals gain electrons and become negatively charged. 25. Use the graph below to answer the questions that follow. TREND-ATOMIC RADIUS ATOMIC RADIUS 2.5 2 1.5 1 0.5 0 3 4 5 C6 N7 O8 F9 Ne 10 Na 11Mg 12 Al 13 Si 14 15 16 17 18 19 20 P S Cl Ar K Ca Li Be B C N O Fl Ne Na Mg Al Si P S Cl Ar K Ca ATOMIC NUMBER-ELEMENTS Atomic number Li Be B a. Which general trend exists for atomic size across a period? __ increases to left _ b. What general trend exists for atomic size down a family? ____ increases down the family _ c. Which group has the largest size? __ alkali metals (1) __ The smallest? _ halogens (15) _ d. Why does atomic size decrease as you move left to right across a period? Nuclear charge increases to the right across a period. Thus the electrons are pulled closer to the nucleus making the atom smaller. 26. Why does atomic size increase as you move down a family/group? Moving down a family/group adds energy levels full of electrons thus increasing the size of the atom. 27. Write the full electron configuration and short hand configuration for: a. N b. Sr c. Cu a. N [He] 2s2 2p3 b. Sr [Kr] 5s2 c. Sr [Ar] 4s2 3d9 1s2 2s2 2p3 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 1s2 2s2 2p6 3s2 3p6 4s2 3d9 28. Draw orbital diagrams for: Ni and Na