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- have varied physical properties and are found in many different compounds. Nonmetals Metals MetalloidsClassify each of the following elements as a main-group or transition element. Also,specify whether they are metals, metalloids, or nonmetals: Na, Re, S, I, Kr, Mg, U, Si, B, Al, As, H.Classify each element in the fourth row of the periodic table as a metal, nonmetal, or metalloid.
- When a nonmetal oxide reacts with water, it forms an oxoacid with the same oxidation number as the nonmetal. Give the name and formula of the oxide used to prepare each of these oxoacids: (a) hypochlorous acid; (b) chlorous acid; (c) chloric acid; (d) perchloric acid; (e) sulfuric acid; (f ) sulfurous acid; (g) nitric acid; (h) nitrous acid; (i) carbonic acid; ( j) phosphoric acid.Arrange in order of increasing nonmetallic character. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 4 elements V, Ge, and K (b) the Group 5A elements N, As, and Bi Arrange in order of increasing atomic size. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) the Period 3 elements Mg, Si, and Ar (b) the Group 2A elements Ca, Ba, and SrGive the symbol of the element that has the least metallic character in Group 8A (18). Give the symbol of the element that has the lowest ionization energy in Group 7A (17). Give the symbol of the element that has the highest ionization energy in Group 5A (15). Give the symbol of the element that has the largest atomic size in Period 1.
- In the table below, I1 – I6 represent first 6 ionization energies of a certain element. All units are kJ/mol. I1 I2 I3 I4 I5 I6 738 1450 7730 10500 13600 18000 This element is in the 3rd row of the periodic table, the row starting with Na. Identify the element, and explain your reasoning, based on the data in the above table.Consider two different elements, element 1 and element 2. Element 1 has both a smaller radius and a smaller molar mass than element 2. What accounts for their differences in radius?Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ΔHf° for BF3(g) is -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
- Two sets of ionizations are shown in the tables below. Complete the tables by ordering each set of ionizations by increasing amount of energy required. In other words, for each set choose "1" next to the ionization that would require the least energy, "2" next to the ionization that would require the next least energy, and so on. ionization + Cs Cs + e + Xe → Xe te + Kr→ Kr + e energy required ? ? ? O ionization He → He + e Br→ Br te + Fr → Fr + e energy required ? ? ?2. The elements vary from metals through metalloids to nonmetals. They form halides in oxidation states +5 and +3 and the hydrides are all toxic gases. Identify this group of elements.Explain what characteristics of metalloids are more like metals and which are more like nonmetals, based on Na, Mg, Fe, Cl, and Ar.