Quantum Concepts
Name ____________________________________________Date______ Period _____
1. The n=1 energy level contains _________orbital, it has a(n) _____________________ shape.
The 1S orbital can hold ______________ electrons.
2. The second energy level contains __________ subshells (types of orbitals) with a total of _______
orbitals. The lower energy orbital is the _____ orbital, it is spherical in shape. The higher energy
subshell is the 2p subshell. This shell contains __________ p orbitals. Each orbital can hold ______
electrons for a total of ______ electrons in this subshell. The total number of electrons that can be
accommodated in the n=2 energy level is ___.
3. The third energy level contains ________ subshells with a total of _______ orbitals. The lowest energy
subshell is spherical and it is designated the _____ orbital. The next energetic subshell consists of
three _________ orbitals. The most energetic subshell consists of five d _____________________. If
each orbital holds 2 electrons, the 3d subshell can hold a total of _________ electrons. The entire n=3
energy shell can hold ______ electrons. The 3d subshell fills after the _______.
4.
The fourth energy level has __________ subshells with one s, ________ p, _________ d and
_________f orbitals. There is a total of ______ orbitals in the n=4 shell. Thus the n=4 shell can
accommodate _______ electrons: two in 4s, ______ in 4p, ______ in the 4d and ______ in the 4f.
5. The first element to have an electron in a p orbital is _______________.
6. The first element to have an electron in a d orbital is ______________.
7. The first element to have an electron in an f orbital is _____________.
8. What is the electrons configuration (long) of Ar? _________________________
9. What is the electron configuration (noble gas shorthand) of Na? __________________________
10. Draw the orbital diagram for sulfur. _______________________________________________
11. List the orbitals in the order that they fill (stop at the last electron to go into the 5d subshell. page 242
____________________________________________________________________________
12. Why is the s block 2 columns wide? __________________________________________________
13. Why is the p block 6 columns wide? __________________________________________________
14. Why is the d block 10 columns wide? __________________________________________________
15. Why is the f block 14 columns wide? __________________________________________________
16. Define ionization energy.
17. Define electronegativity.
18. Define valence electrons.
19. What are the first 3 elements of the Alkali metal family __________________________________
Color and label the alkali metals on your blank periodic table. Remember hydrogen is not a metal.
20. What is the valence shell electron configuration for elements of the alkali metal family?
21. If an alkali metal atom loses its valence electron, what will be the charge on the resulting ion?
_____________
22. What are the first 3 elements of the Alkaline Earth metal family? __________________________
Color and label the alkaline metals on your blank periodic table.
23. What is the valence shell electron configuration for elements in the alkaline earth metal family?
24. If an alkaline metal atom loses its valence electrons, what will be the charge on the resulting ion?
_______________
25. What are the first 3 elements of the Boron family? _________________________________
Color and label the boron family on your blank periodic table.
26. What is the valence shell electron configuration for elements in the boron family?
27. If a member of the boron family loses its valence electrons, what will be the charge on the resulting
ion? _______________________
28. The pnictogen family is the nitrogen family. Color and label the nitrogen family. How many valence
electrons do members of the nitrogen family have?________
29. If an atom in the pnictogen family gains 3 electrons it will have the same electron configuration as the
nearest noble gas. What will the charge on the ion be if the atom gains 3 electrons?
30. The chalcogens family is another name for the oxygen family. Color and label the chalcogens family.
How many valence electrons do members the chalcogens family have? ________
31. Will members of this family gain or lose electrons to become “isoelectric” with the nearest noble gas?
32. The halogen family is another name for the fluorine family. Color and label the halogen family. How
many valence electrons do members of the halogen family have?________
33. If an atom in the halogen family gains 1 electron it will be isoelectric with the nearest noble gas. What
will the charge on the ion be if the atom gains 1 electron?
34. Not including helium, how may valance electrons do members of the noble gas family have?
35. Why do you think noble gases do not take part in chemical reactions?
36. Define metalloid. Color and label the metalloids on the periodic.
37. Do metals tend to gain or lose electrons? Do nonmetals tend to gain or lose electrons?