Atomic Theory and Bonding Problem Set
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1. Draw the lewis structure and indicate the direction of the bond dipole for C-F and Si-S.
2. Draw the lewis structure for NI3 and PF3.
3. Use the symbol for the previous noble gas to indicate core electrons. Write the electron configuration for Z=107.
4. Based on its position on the periodic table, how many 4d electrons are found in Z=44?
5. Which element in group 16 is the most reactive why?
6. What is the Z number of the largest atom in group two? why?
7. Write the electron configuration for the last row of electrons for the element with Z=39.
8. How many core electrons are in Z=51 and Z=88
9. How does the attraction that the nucleus exerts on an electron change with the principle energy of the electron why?
10. Explain why the following electron configuration is not possible 1s2 2s2 2p6 3s2 3p63d2 4s1.
11. What simple ion is formed from the element with Z=89?
12. The first four ionization energies for the elements X and Y are shown in the table below. Identify the elements X any Y. There may be more than one correct answer.
Ionization energy X Y
first 170 200
Second 350 400
Third 1,800 3,500
Fourth 2,500 5,000
13. What is/are the gas/gases that has/have the same electron configuration as each of the ions in the compound formed from Z=31 and Z=16
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Solution Summary
Solution includes structure drawings for (1) and (2) and calculations and answers for (3) through (13). 282 words.
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3) Z = 107
[Rn]5f146d57s2
4) Z = 44
Ru: 1s22s22p63s23p64s23d104p65s14d7
Therefore, a total of 17 d electrons.
5) Oxygen: The electronegativity of oxy genis second only to that of fluorine. Elements in group 16's general reactivity is therefore dominated by their abibility to gain electrons.
6) Radium: size increases down a group as there are more subshells.
7) Z = 39
Y: ...
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