Arrange the following chemical species in order of increasing atomic radius. Explain your arrangement in each case. (a) K, Mg, Ca, Aℓ (b) F–, S2–, Cℓ–.
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6. Arrange the following chemical species in order of increasing atomic radius. Explain
your arrangement in each case.
(a) K, Mg, Ca, Aℓ
(b) F–, S2–, Cℓ–.
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- 7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°5.) Electron Configurations for Ions: Supply the ground state electron configurations for the following ions. You many use the short-hand notation (e.g. Na*: [He]2s 2p°). (a) N (b) Mg*. (c) O (d) Sc* (e) Sn2+ (f) Ar 6.) Formulas of Ions: Predict the formulas of the most stable ions of the following elements (a) Na (b) Mg (c) S (d) Al (e) Br (f) PArrange the following chemical species in order of increasing atomic radius. Explain your arrangement in each case. (a) K, Mg, Ca, Al (b) F–, S2–, Cl–.
- 11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).Consider the Mg2+, Cl-, K+, and Se2- ions. The four spheresbelow represent these four ions, scaled according to ionic size.(a) Without referring to Figure 7.8, match each ion to its appropriatesphere. (b) In terms of size, between which of the sphereswould you find the (i) Ca2+ and (ii) S2- ions?Based on their positions in the periodic table, predict whichatom of the following pairs will have the smaller first ionizationenergy: (a) Cl, Ar; (b) Be, Ca; (c) K, Co; (d) S, Ge; (e) Sn, Te.
- The As¬As bond length in elemental arsenic is 2.48 Å. TheCl¬Cl bond length in Cl2 is 1.99 Å. (a) Based on these data,what is the predicted As¬Cl bond length in arsenic trichloride,AsCl3, in which each of the three Cl atoms is bondedto the As atom? (b) What bond length is predicted for AsCl3,using the atomic radii in Figure 7.7?Using only the periodic table, arrange each set of atoms inorder of increasing radius: (a) Ba, Ca, Na; (b) In, Sn, As; (c) Al,Be, Si.(b) List some properties of Group 1 elements which indicate they are all metals. (c) What valence do all Group 1 elements exhibit in their compounds? (a) Write the names and symbols of the elements of Group 2.
- (D) Zr (Z=40) and Hf (Z = 72) 7. Which halogen has the greatest first ionization energy? (A) F (B) Cl (C) Br (D) I 3. The isotope "Zn undergoes what mode of radioactive decay? (A) Alpha emission (C) Gamma emission (B) Beta emission (D) Positron emission 9. What is the bond order of carbon monoxide, CO? (A) 1.5 (B) 2.0 (C) 2.5 (D) 3.0 50. Which statements about the Lewis structure of theWrite the electron configuration for each of the followingions, and determine which ones possess noble-gasconfigurations: (a) Sr2+, (b) Ti2+, (c) Se2-, (d) Ni2+, (e) Br-,(f) Mn3 + .The ionization energy of lithium is 520.2 kJ/mole, and the electron affinity of hydrogen is 72.8 kJ/mole.(a) Find the separation distance in LiH at which the Coulomb potential energy equals the energy cost of removing an electron from Li and adding it to H.(b) The measured electric dipole moment of the molecule LiH is 2.00 × 10^−29 C · m. What is the fractional ionic character of LiH?(c) Instead of removing an electron from Li and attaching it to H, we could regard the formation of LiH as occurring by removing an electron from H and attaching it to Li (electron affinity = 59.6 kJ/mole). Why don’t we consider this as the formation process?