SOL CH.2 Electrons & the Periodic Table Review
NAME THE TERM DESCRIBED BY THE FOLLOWING DEFINITIONS:
1.
A packet of light energy that carries a quantum of energy.
2.
The state when all electrons of an atom are in the lowest possible energy levels.
3.
When an electron jumps up to a higher energy level, the atom is in its ___.
4.
The scientist who applied Einstein’s particle-wave theory to electrons.
5.
The theory that it is impossible to know both the position and speed of an electron
simultaneously.
6.
The theory that no two electrons in an atom can share the same 4 quantum numbers.
7.
The theory that electrons fill the lowest energy orbitals first.
8.
The theory that, within a sublevel, electrons prefer to occupy their own orbital.
9.
A term describing the outermost electrons in an atom.
10. A positively charged ion is called a(n) ___. A negatively charged ion is called a(n) ___.
11. The most stable type of electron configuration.
12. The lower, left-hand section of the periodic table that includes most of the elements.
13. The upper right-hand section of the periodic table.
14. The section of the periodic table that includes only the elements in the d-block.
15. The section of the periodic table that includes both the s-block and the p-block.
16. A three-dimensional region in space where an electron is likely to exist.
Electrons & the Periodic Table Review
C. Johannesson
SOL CH.2 Electrons & the Periodic Table Review
17. The process by which the core electrons partially block the attraction between the
nucleus and the valence electrons.
DRAW ORBITAL DIAGRAMS FOR THE FOLLOWING ELEMENTS:
18. Mg
19. Si
20. Ti
WRITE LONGHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
21. N
22. K
23. Cr
WRITE SHORTHAND ELECTRON CONFIGURATIONS FOR THE FOLLOWING ELEMENTS:
24. Sb
25. Bi
26. Tc
27. Ge
Electrons & the Periodic Table Review
C. Johannesson
SOL CH.2 Electrons & the Periodic Table Review
WRITE THE ION SYMBOL AND ITS SHORTHAND ELECTRON CONFIGURATION:
28. Te
29. B
30. Ba
31. Br
32. K
WHICH ATOM HAS THE LARGER ATOMIC RADIUS?
33. C vs. Sn
34. Sr vs. In
RANK THESE ATOMS FROM SMALLEST TO LARGEST ATOMIC RADIUS.
35. Li, K, Cs, O
36. Fe, P, Ra, Ti
WHICH ATOM HAS THE LARGER 1ST IONIZATION ENERGY?
37. Fr vs. Ne
38. Na vs. Si
RANK THESE ATOMS FROM SMALLEST TO LARGEST 1ST IONIZATION ENERGY.
39. Ar, Xe, Ba, Sn
40. Mg, C, F, Sr
WHICH ATOM HAS THE HIGHER MELTING/BOILING POINT?
41. Cs vs. W
42. Fe vs. As
43. Na vs. Si
WHICH PARTICLE HAS THE LARGER RADIUS?
44. Mg vs. Mg2+
45. I vs. I
Electrons & the Periodic Table Review
C. Johannesson
SOL CH.2 Electrons & the Periodic Table Review
Electrons & the Periodic Table Review – Ch. 4 & 5
ANSWER SHEET
**ALL NUMERICAL ANSWERS MUST INCLUDE THE PROPER UNITS **
Electrons & the Periodic Table Review
C. Johannesson
SOL CH.2 Electrons & the Periodic Table Review
1.
1.3  10-21 J
2.
7.0  10-7 m
3.
3.3  1016 Hz
4.
9.9  10-14 J
5.
5.1  108 Hz
6.
7.
8.
9.
photon
ground state
excited state
Louis de Broglie
10. Heisenberg Uncertainty Principle
11. Pauli Exclusion Principle
12.
13.
14.
15.
16.
17.
18.
19.
Aufbau Principle
Hund’s Rule
valence electrons
cation, anion
full energy level (or full shell)
metals
nonmetals
transition metals (or transition elements)
20. main group elements
21. orbital
22. shielding
23.      
1s 2s
2p
3s
24.         __
1s 2s
2p
3s
3p
25.         
1s 2s
2p
3s
3p
   __ __ __
4s
3d
Electrons & the Periodic Table Review
C. Johannesson
SOL CH.2 Electrons & the Periodic Table Review
26. 1s22s22p3
27. 1s22s22p63s23p64s1
28. 1s22s22p63s23p64s13d5
(Remember: Cr makes an exception to gain stability.)
29. [Kr] 5s24d105p3
30. [Xe] 6s24f145d106p3
31. [Kr] 5s24d5
32. [Ar] 4s23d104p2
33. Te2
[Kr] 5s24d105p6
34. B3+
35. Ba2+
1s2
[Kr] 5s24d105p6
36. Br 
[Ar] 4s23d104p6
37.
38.
39.
40.
41.
42.
43.
44.
45.
46.
47.
48.
49.
K+
[Ne] 3s23p6
Sn
Sr
O < Li < K < Cs
P < Fe < Ti < Ra
Ne
Si
Ba < Sn < Xe < Ar
Sr < Mg < C < F
W
Fe
Si
Mg
50. I
Electrons & the Periodic Table Review
C. Johannesson