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Which element would you expect to be less metallic?(a) Sb or As(b) Si or P(c) Be or Na
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- choose three . What are the characteristerses of a metal like element? (a) they try to get additional electrons (b) they are melleable. (c) they are lightly to give away or share electrons. (d) they are good conductors of electricity(a) Would you expect scandium oxide to be a solid, liquid, or gas at room temperature?2.(a) Write the full electron configuration for each of Ge and Ge3-2.(b) Write the noble gas configuration, and valence configuration of Ge 2.(c) Write the orbital diagram for the Ge3-2.(d) For the unpaired electron in the orbital diagram for the Ge3-ion, give its four quantum numbersn,l,ml,ms 2.(e) Is Ge3+ diamagnetic or paramagnetic?
- 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 Sr34. According to general trends in the periodic table, predict which element in each of the following pairs has the greater metallic character. (b) Na or K (d) H or Fe (a) B or Al (c) Mg or Ba 1ist1. An element has the following electronic configuration: [Kr]4d105s25p4(a) What period does it belong to?(b) What is its group number? (Use group numbers from 1 to 18)(c) What kind of element is it? (Main group metal, transition metal, metalloid, nonmetal?)(d) How many unpaired electrons are there in an atom of this element? 3. (a) Which of the following atoms or ions is diamagnetic?Li+ Ni2+ Al Fe2+ Mn3+(b) Which of the following atoms or ions is paramagnetic?C4- S4+ V4+ Se2- Ge4+
- Which of the following elements is expected to have the highest SECOND IONIZATION ENERGY: (A) Be (B) Ca (C) Mg (D) NaArrange in order of increasing ionization energy (a) the Group 1A elements Na, Cs, and K(b) the Period 4 elements As, Ca, and BrBoron, 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) Drawthe orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons inboron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation forthe reaction of solid boron with fluorine gas. (e) ΔHf° for BF31g2 is -1135.6 kJ>mol. Calculate the standard enthalpy change in thereaction 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?
