Name: _____________________________________ Date: _____________________ Block: _________
Chapter Five, Six, Seven and Eight Review Sheet
Chapter Five
1. The maximum number of valence electrons possible in any outermost shell is
______________________.
2. In any p sublevel, there are how many p orbitals _______________.
3. The maximum number of electrons possible in any p sublevel is _______________________.
4. A 3d orbital has (more, less) ___________ energy than a 3p orbital.
5. Bohr postulated that electrons could only exist in certain paths around the nucleus when he
termed
a. orbits
b. quanta
c. orbitals
d. spectral lines
6. The number of sublevels in the fifth principal energy level is
a. 7
b. 3
c. 5
d. 4
7. The 4f sublevel is filled next after
a. the 6s sublevel
b. the 5p sublevel c. the 5s level
d. the 4d
sublevel
8. The maximum number of electrons in the fourth principal energy level is
a. 8
b. 16
c. 32
d. 64
9. A p orbital is
a. best described as a cube b. sphere shaped
c. too complicated to describe d.
dumbbell shaped
10. The sublevel of lowest energy is
a. 3d
b. 3p
c. 2s
d. 2p
2
11. 1s is the representation of
a. H
b. F
c. Hg
d. He
Base your answers to questions 12-16 on the following electron configuration of a neutral atom:
1s22s22p63s23p4
12. What is the number of valence electrons in this atom?__________
13. The total number of electrons in the second principal energy level of this atom is
______________________.
14. How many orbitals are half filled in an atom of this element in the ground state?______________
15. What is the total number of electron energy levels in this atom?_______________
16. What element is this atom?__________________
Provide the electron configuration for the following:
17. Copper (ground state)____________________________________________________________________
18. Iodine (abbreviated)_____________________________________________________________________
Identify the element
19. 1s22s22p63s23p64s23d104p65s1__________
20. 1s22s22p63s23p2___________
21. [Kr] 5s24d105p3__________
Chapter Six
22. How is ionic size different than atomic size?
Name: _____________________________________ Date: _____________________ Block: _________
23. Sodium chloride (NaCl) is an example of an ionic bond. What is the difference in electronegativity
between sodium and chlorine vs Nitrogen dioxide (NO2), which is an example of a covalent
bond.
24. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium.
25. Why does fluorine have a higher ionization energy than iodine?
26. Why do elements in the same family generally have similar properties?
Chapter Seven
27. Bond the following atoms. Determine if they are ionic or covalent, circle your choice. Show the
valence electrons and how they are either shared between the atoms or how they are transferred
between atoms. Then write the chemical formula in the space provided.
Ionic or covalent
Fe3+
Cl
Ionic or covalent
Mg
Cl
Formula ____________
Formula _____________
28. Ionic bonds form between ______________ and _________________.
29. In naming simple ionic compounds, the ____________ is always first, the
____________ second (e.g., sodium chloride).
30. Ionic compounds dissolve easily in ________________ and other polar solvents.
31. In solution, ionic compounds easily _______________________________.
32. Ionic compounds tend to form ________________ with _______ melting
temperatures.
Chapter Eight
33. Compare and contrast ionic and covalent bonds.
Name: _____________________________________ Date: _____________________ Block: _________
For each of the following covalent compounds,
a) draw the lewis structure
b) identify the electronic geometry
c) identify the molecular geometry
d) identify the bond angle
34. CF4
35. CO2
36. SiH4
37. OF2
38. SO2