Chapter 3, Problem 3.40E

What are the representative elements? In what region(s) of the periodic table are these elements found? In what general area of the periodic table are the metallic elements found? In what general area of the table are the nonmetals found? When in the table are the metalloids located?

The molecules NH3andBF3have the same general formula (AB3)but different shapes. Find the shape of each of the above molecules. Provide more examples of real molecules that have the same general formulas but different shapes.

1. Which would most likely form a metallic bond with gold? a. chlorineb. manganesec. oxygend. argon 2. Why are metals described as having sea of electrons”? a. Electrons move in waves.b. Electrons are fixed to metal atoms.c. Electrons are wet.d. Electrons move freely between atoms.

94. Which of the following statements is/are true? I. Solids are compact but if melted it moves randomly. II. Diamond and graphite are examples of amorphous solids. III. Color is an intensive property. IV. Isobars are the atoms with the same A. A. I, II, III, IV B. I, III C.I, III, IV D. III, IV E. II, III, IV 95. Chalcogens:   a. V A B. IV A C. III A D.VI A E. VII A

Compare the energetic favorability of Fe2+, Cu2+, and Zn2+ to their metallic states by H2.

Using only its location on the periodic table, write the full electron configuration for Molybdenum (Mo). (Do not superscript. Type a space between orbitals: eg. 1s2 2s2 2p6 etc. Use the correct filing order)

What is the trend observed what is the trend observed for ions energy going down a group? Explain why this trend occurs

Compared to their neutral atom counterparts, ions will have smaller or larger atomic radii due to their losing or gaining electrons. According to Jensen (2010), Linus Pauling assigned the radius of the oxygen anion (O“) at 140 pm (larger than the neutral atom, 66 pm). On the other hand, the magnesium atom loses 95 ppm from its 160 ppm radius when it loses two valence electrons, forming the magnesium ion.  Determine the value of constant B wen constant n is approcimately 8. Unit is in N-m9

Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca2+ ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is 3460 kJ/mol; the lattice energy of K2O is 2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.