1. Periodic Tables Review

2. Who invented the current periodic table and how is it arranged?
Mendleev, atomic mass
Mendleev, atomic number
Mosley, atomic mass
Mosley, atomic number

3. Which statement regarding the properties of elements arranged in the Periodic Table is correct?
Atomic sizes decrease going down a Group or Family.
Atomic sizes increase going from Fr in Group I to F in Group VII.
Atomic sizes decrease going from left to right in a Period.
All atoms in the same Group have the same size.

4. Which is the most electronegative atom?P Al Cl S

5. Match each letter to the correct description:
Metalloid(s)
Alkali metal(s)
Ending electron configuration of np2
Has 3 valence electrons
Not a representative element(s)
Most reactive nonmetal
Forms anion(s) E
Match each letter to the correct description: A E F A G E F C B I H
C, D D G
F, G

6. Which atom has the lowest second ionization energy?Mg Na K Ar

7. Which set contains three isoelectronic (same # of electrons) species?
Cu, Ag, Au
Cl+, Ar, K-
P3-, Se2-, I-
H-, Li+, Be2+

8. For the representative elements, going from left to right across a period in the periodic table of the elements:
atomic size increases.
electronegativity decreases.
ionization energy becomes greater.
the outer electrons are held more weakly.

9. The following ionization energies represent elements Al, Mg, B and C
The following ionization energies represent elements Al, Mg, B and C. Identify which element is which.
Element
IE1
IE2
IE3
IE4
IE5 A
1086
2353
4621
6223
37,830 B
578
1817
2745
11,578
14,831 C
738
1451
7733
10,540
13,628 D
801
2427
3660
25,026
32,827 C Al Mg B

10. The ability of an atom to attract electrons when bonds are form:
ionization energy
electronegativity
electron affinity
magnetism

11. Which of the following atoms has the largest atomic radius?K Sc Fe Kr

12. In moving from left to right across a period in the periodic table of the elements….
ionization energy decreases
atomic radius decreases
electronegativity decreases
electron affinity decreases

13. Which element should have the smallest first ionization energy?Ca Rb Al Cl

14. Which sequence is arranged in order of increasing ionization energies?
N, O, C, Be
Be, C, O, N
Be, C, N, O

15. The first three ionization energies of an element X are 590, 1145, and 4912 kJ/mol. The most likely formula for a stable ion of X is: X+
X2+
X3+ X-

16. What charge do elements in group 16 have?+2 -2 +6 -6
No charge

17. Which element is the most reactive metal?Li K Cs Ra

18. Which family reacts the most violently with water?
Noble Gases
Halogens
Alkaline Earth
Alkali
Transition

19. Arrange the following elements in order of increasing atomic radii
Arrange the following elements in order of increasing atomic radii. K, Na, Mg, Cs, Cl
Na < Mg < Cl < K < Cs
Cl < Mg < Na < K < Cs
Cs < K < Cl < Mg < Na
Cl < Mg < Cs < K < Na
Cl < Mg < Na < Cs < K

20. Arrange the following set of ions in order of increasing ionic radii
Arrange the following set of ions in order of increasing ionic radii Ca2+, Cl–, K+, P3–, S2–
Ca2+ < K+ < P3– < S2– < Cl–
Ca2+ < K+ < Cl– < S2– < P3–
K+ < Cl– < Ca2+ < S2– < P3–
Cl– < S2– < P3– < Ca2+ < K+
P3– < S2– < Cl– < K+ < Ca2+

21. ______ is a representative element.Zr Mo Ag Ca U

22. _________ is a noble gas.Na Cl Ar W F

23. Which element has the largest atomic radius?
[Ne]3s23p1
[Ne]3s23p2
[Ne]3s23p3
[Ne]3s23p4
[Ne]3s23p5

24. The element most chemically similar to carbon is:
Silicon
Nitrogen
Boron
Oxygen

25. The radius of the bromine atom is smaller than the radius of the bromide ion, Br -. Explain.
Bromine and bromide both have the same number of protons, but bromide has gained one electron. Since the pull of the nucleus, or Zeff, is distributed to more electrons, the pull on each is weaker and the radius of bromide is larger.

26. The first ionization energy of aluminum is lower than the first ionization energy of magnesium. Explain.
Aluminum has two electrons in the 3s and one in the 3p while magnesium has two electrons in the 3s only. Since aluminum has one lone electron, it is easier to remove than the paired electrons of magnesium. Also, the lone electron of aluminum is shielded by the 3s orbital, leading to a lower IE.

27. The second ionization energy of sodium is about three times greater than the second ionization energy of magnesium. Explain.
Magnesium has two valence electrons in the 3s orbital. Both electrons are relatively easy to remove. Sodium has one electron in its valence shell, so the removal of it is easy, but the removal of the second electron from sodium comes from a core energy level, the 2p, and is thus harder to remove.