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Unit 10: the Periodic Table Unit 10: The Periodic Table (Chapter 6) Name ____________________________________________________ Period ___________________ 1 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155–160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification of elements into metals, nonmetals, and metalloids. Searching For An Organizing Principle (page 155) 1. How many elements had been identified by the year 1700? ________________ 2. What caused the rate of discovery to increase after 1700? _____________________________________ _________________________________________________________________________________________ 3. What did chemists use to sort elements into groups? __________________________________________ _______________________________________________________________________________________ Mendeleev’s Periodic Table (page 156) 4. Who was Dmitri Mendeleev? _______________________________________________________________ 5. What property did Mendeleev use to organize the elements into a periodic table? _________________________________________________________________________________________ 6. True/false? Mendeleev used his PT to predict the properties of undiscovered elements.__________ The Periodic Law (page 157) 7. How are the elements arranged in the modern periodic table? _________________________________ 8. True or false? The periodic law states that when elements are arranged in order of increasing atomic number, there is a periodic repetition of physical and chemical properties. ______________________ Metals, Nonmetals, and Metalloids (pages 158–160) 9. Explain the color coding of the squares in the periodic table in Figure 6.5. _______________________ ________________________________________________________________________________________ 10. Which property below is not a general property of metals. a. ductile b. poor conductor of heat c. malleable d. high luster 11. True/False. The variation in properties among metals is greater than the variation in properties among nonmetals. __________________ 12. Under some conditions, a metalloid may behave like a _____________________ . Under other conditions, a metalloid may behave like a _____________________ . 2 SECTION 6.2 CLASSIFYING THE ELEMENTS (pages 161–167) This section explains why you can infer the properties of an element based on the properties of other elements in the periodic table. It also describes the use of electron configurations to classify elements. 5. Classify each as a (an) alkali metal, alkaline earth metal, halogen, or noble gas. a. sodium ______________________ e. xenon ______________________ b. chlorine ______________________ f. potassium ______________________ c. calcium ______________________ g. magnesium ______________________ d. fluorine ______________________ 6. How many electrons are in the highest occupied energy level? a. Group 3A __________ b. Group 1A __________ c. Group 8A __________ it 8. Circle the letter of the elements found in the p block. a. Groups 1A and 2A and helium b. Groups 3A, 4A, 5A, 6A, 7A, and 8A except for helium c. transition metals d. inner transition metals Match the category of elements with an element from that category. _______________ 9. Noble gases a. gallium _______________ 10. Representative elements b. nobelium _______________ 11. Transition metals c. argon _______________ 12. Inner transition metals d. vanadium 13. Use Figure 6.12 on page 166. Write the electron configurations for the following elements. a. magnesium ______________________________________ b. cobalt ______________________________________ c. sulfur ______________________________________ 3 Historical Figures in Chemistry Dmitri Mendeleev and the Periodic Table The arrangement of elements in the Using the modern periodic table, modern periodic table is clearly connected look at the following pairs of to atomic structure. However, the concept elements: Ar and K, Te and I, and of the periodic table has been known for Co and Ni. In each case, the first more than 100 years, and it was developed element has the greater atomic long before our more recent knowledge weight. Arranging them in order of of electron configurations. The history of increasing atomic weight would the ideas of chemical periodicity is filled place a very reactive metal in the with interesting people, and one of the column with the very inert elements. most important was the Russian chemist The fault lies in Mendeleev’s Dmitri Mendeleev (1834 - 1910). assumption that properties of In the 19th century many chemists tried elements are periodic functions of to find relationships between atomic their weight. weights and the properties of the elements. H.G.J. Moseley, a young scientist These efforts largely failed because atomic A young Dmitri Mendeleev working with Ernest Rutherford, weights were not known for all elements, found that the wavelengths of x-rays emitted by an and many measured values were inaccurate. element are related in a precise way to the atomic However, at a conference in 1860 in Germany, number of the element. He quickly realized that Stanislao Cannizzaro (1826 - 1910) described his other atomic properties may be related to atomic method for determining accurate and unambiguous number and not, as Mendeleev had proposed, to atomic weights, and this began to set things right. atomic weight. Indeed, if the elements are arranged Mendeleev was at the conference and doubtless by atomic number, the defects in Mendeleev’s table head Cannizzaro’s paper. It led him to become the are corrected. It was therefore Moseley who founder of the concept of chemical periodicity. discovered the law of chemical periodicity, which Mendeleev’s ideas on periodicity began in the late states that the properties of elements are periodic 1860’s with his work on a book on inorganic functions of their atomic numbers. chemistry. To help organize the material for his book, After Mendeleev published his work on chemical he had a file of note cards, one for each element. On periodicity, he did little else with the subject. Instead, each card he wrote the atomic weight of the he went on to other interests. In 1876 he visited the element, then known more accurately owing to US to study the fledgling oil industry and was Cannizzaro’s work, and some properties of the impressed by the industry but not the country. element. When he arranged these cards in order of America, he thought, was not interested in science, increasing atomic weight, he saw there was a and even worse, carried on the worst features of repetition of properties every eight or eighteen European civilization. elements. Thus was born Mendeleev’s periodic table. One final note: All pictures of Mendeleev show More than 100 years later, we recognize Mendeleev’s him with long hair. He made it a rule to get his hair work as a milestone, because he had the genius to cut only once a year, in the spring, whether he realize that (a) there were many elements to be needed it or not. discovered and (b) the characteristics of an element could be predicted from its atomic weight and its position on the table. Mendeleev’s table led directly to the discovery of several elements within a few years after he published the table. In spite of Mendeleev’s great achievement, problems arose when new elements were discovered and more accurate atomic weights were determined. Dmitri Mendeleev in 1904 4 5 Properties of the groups on the periodic table Circle the correct answer 1. Mendeleev noticed that properties of elements appeared at regular intervals when the elements were arranged by a. atomic mass. c. reactivity. b. number of protons. d. atomic number. 2. Elements in the same group or column on the periodic table can be expected to have similar a. atomic masses. c. atomic numbers. b. number of neutrons. d. properties. 3. The radioactive elements with atomic numbers from 89-102 on the periodic table are referred to as the a. noble gases. c. lanthanides. b. actinides. d. halogens. 4. Argon, krypton, and xenon are all a. noble gases. c. alkaline earth metals. b. actinides. d. transition elements. 5. Elements on the right side of the periodic table tend to exhibit properties of a. nonmetals. c. metals. b. metalloids. d. gases. 6. Elements in which the d sublevel is being filled exhibit properties of a. nonmetals. c. metals. b. metalloids. d. gases. 7. Since the column one elements are highly reactive, these alkali metals exist as ______ in nature. a. elements. c. compounds. b. solutions. d. gases. 8. Compared to the alkali metals, the alkaline earth metals a. are less reactive. c. are less dense. b. have lower melting points. d. combine more readily with nonmetals. 9. What group of elements reacts vigorously with water? a. halogens c. noble gases b. alkali metals d. transition metals 10. Tungsten and copper are elements that belong to the a. halogens. c. noble gases. b. alkali metals. d. transition metals. 11. The most reactive nonmetals are the 6 a. halogens. c. noble gases. b. oxygen family of elements. d. 1s electron filling elements. Fill in the blank with the correct word or phrase. 12. The Law _________________________________________________________________, also called the Periodic Law, states that “the physical and chemical properties of elements are periodic functions of their atomic numbers.” 13. The work of _________________________________ led to the periodic table based on atomic number. 14. Neutral atoms with an s2p5 configuration are called _____________________________________.
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