Chapter 6 Periodic Table

Name: Chapter 6 Questions - Periodic Table Trends Not covered.. All material and questions can be found in the textbook. Organized by section. 6.1 Organizing the Elements Why did Mendeleev leave spaces in his periodic table? He predicted that there were yet undiscovered spaces clements ints that would occupy What effect did the discover of gallium have on the acceptance of Mendeleev's table? The accuracy of Mendelee u's predictions gave his PTE great credibility. What pattern is revealed when the elements are arranged in a periodic table in order of increasing atomic number? An incresse in atomic MASS repitition of many physical & chemical properties. Based on their locations in the periodic table, would you expect carbon and silicon to have similar properties? Explain your answer. Jes. Same number of valence elections hohaviors. says that they should have similar In general, how are metalloids different from metals and nonmetals? Metalloids Can electrons. Metals either gain give away give away . Nomactals gaine Metalloids con do both. 6.2 Classifying the Elements Where are the alkali metals, the alkaline earth metals, the halogens, and the noble gases located in the periodic table? 1A,2A, 7A & 8A respectively Which of the following are symbols for representative elements: Na, Mg, Fe, Ni, CI? ropresentative elements. Gre ones from the SEP blocks. Which noble gas does not have eight electrons in its highest occupied energy level? He: 152 Which of these metals isn't a transition metal? A. aluminum B. silver C. iron D. zirconium Write the electron configuration of these elements. a. the noble gas in period 3 152222 352306 b. the metalloid in period 3 1,2 2,220352 302 6 c. the alkali earth metal in period 3 15² 2s²235 2 6.3 Periodic Trends Which element in each pair has atoms with a larger atomic radius? (Circle best choice for each) A. sodium, lithium B. strontium, magnesium C. carbon, germanium D. selenium, oxygen Explain the difference between the first and second ionization energy of an element. Inst IE Energy to Second IE remove 1 e from a neutral stum. after the 1st has been removed. Which element in each pair has a greater first ionization energy? (Circle best choice for each) A. lithium, boron B. magnesium, strontium C. cesium, aluminum Arrange the following groups of elements in order of increasing ionization energy. a. Be, Mg, Sr Sr, Be, Mg b. Bi, Cs, Ba Cs, B, Bi c. Na, Al, S Na, Al, S Which particle has the larger radius in each atom/ion pair? A. Na, Na B. S. S C. I DAI, AP Which element in each pair has a higher electronegativity value? Options on next page A. CI, F B. CN C. Mg, Ne D. As, Ca alectrong ativity Why are noble gases not included in Table 6.27 They have no desire to attract e. When the elements in each pair are chemically combined, which element in each pair has a greater attraction for electrons? A. Ca or O B. O or F C. Hor O D. Kor S For which of these properties does lithium have a larger value than potassium? A. first ionization energy B. atomic radius C. electronegativity D. ionic radius Understanding Concepts The bar graph shows how many elements were discovered before 1750 and in each 50-year period between 1750 and 2000, a. b. In which 50-year period were the most elements discovered? 1801-1850 How did Mendeleev's work contribute to the discovery of elements? Predicteel Amperties. c. What percent of the elements were discovered by 1900? Discovery of Elements 75% 30 25 20 15 10 15 16 28 26 15 13 Number of elements 0 <1750 1751-1801-1861-1901-1961- 1800 1850 1900 1950 2000 Period of discovery Write the symbol of the element or elements that fit each description. a. a nonmetal in Group 4A C b. the inner transition metal with the lowest atomic number L c. all of the nonmetals for which the atomic number is a multiple of five d. a metal in Group 5A bi 10,15,35 In which pair of elements are the chemical properties of the elements most similar? Explain your reasoning. a. sodium and chlorine b. nitrogen and phosphorus c. boron and oxygen Same group (5A).