3. Which of the following species is smaller: I or I-? why?
4. What simple ion is formed from the element with Z=89?
6. What is(are) the noble gas(es) that has (have) the same electron configuration as each of the ions in the compound formed from Z=31 and Z=16
8. Draw the Lewis structure for the compound formed from elements Z=6 and Z=16.
9. Draw the Lewis structure for the following compound: GeBr4.
10. Draw the Lewis structure for the PO4-3 ion, indicating any resonance forms.
11. Draw the Lewis structure for the hydrogen sulfate ion, indicating any resonance forms.
12. Using VSEPR theory, predict the molecular structure of PbCl4 and H2Te.© BrainMass Inc. brainmass.com October 24, 2018, 6:26 pm ad1c9bdddf
The solution provides detailed explanations for various atomic theory and bonding related questions. Diagrams and formulas are also included.
Atomic theory and bonding - Lewis structures and ionization energy
1. Predict how valence electrons would pair up in the AsO4-3 ion.
2. Predict the bond angles in SbCl3 and BH3.
3. Predict the geometric structure of the carbonate ion. What bond angles would you predict. Why?
4. Predict the less polar bond in the following pair: Br-Cl or Br-I
5. Using electronegativity, predict in the order of decreasing polarity the following bonds: N-P, N-O, N-C, N-S, N-F. why?
6. Write the Lewis structures for the following NI3, and PF3.
7. Predict the Lewis structure(s) for the following: N2O
8. Why is the molecular structure of water nonlinear while that for beryllium fluoride is linear?
9. Predict the bond angle between the chlorine atoms in Cl2O. Why?
10. Predict and explain which atom would have the higher second ionization energy: lithium or beryllium.
11. Using the symbol for the previous noble gas to indicate core electrons, write the electron configuration for Z=107.
12. Based on its position in the periodic table, how many 4d electrons are found in Z=44?
13. For Z=84 which orbital is filled last? Why?
14. Arrange the following in order of decreasing atomic size: At, Ba, Cs, Pb.
15. Why do the metallic elements of a given horizontal row typically have much lower ionization energy than do the nonmetallic elements in the same row?View Full Posting Details