Download periodicity review sheet key

PERIODICITY REVIEW SHEET KEY
1. Valence electrons are always the electrons in the _s__ and _p_ orbitals of the highest
level.
2. Fill in the table below.
Element
Complete Electron Configuration
Noble Gas
Configuration
Number of
Valence Electrons
1s22s22p63s23p64s1
[Ar]4s1
1
1s22s22p63s23p64s23d104p2
[Ar] 4s23d104p2
4
1s22s22p63s23p5
[Ne] 3s23p5
7
1s22s22p63s23p64s23d104p65s24d8
[Kr]5s24d8
2
1s22s22p3
[He]2s22p3
5
1s22s22p63s23p64s23d2
[Ar] 4s23d2
2
1s22s22p1
[He]2s22p1
3
1s22s22p63s23p64s23d104p65s24d105
p66s2
[Xe]6s2
2
K
Ge
Cl
Pd
N
Ti
B
Ba
3. Why do atoms form ions? Full valence electrons – complete the octet rule_.
4. Name an element that has its last electron placed in a “p” orbital of level 3?
Al, Si, P, S, Cl, Ar
5. What is an anion? negative ion – an atom that has gained one or more electrons
6. Will metals or non-metals form cations? Metals
7. What is the electron configuration of the most common ion formed by Sulfur?
1s22s22p63s23p6
8. What is the electron configuration of a sulfur atom? 1s22s22p63s23p4
9. What is the electron configuration of the most common ion formed by boron (B) 1s2
10. What is the electron configuration of a boron atom? 1s22s22p1
11. What noble gas has the same configuration as a Mg2+ ion? Neon
12. What noble gas has the same configuration as an O2- ion? Neon
13. What is the Shielding Effect? Attraction between the nucleus of an atom and the
valence electrons is shielded by levels of electrons in between
Using the graphs from your notes, period table or text book, answer the
following with:
increases(I), decreases (D), or remains the same (R).
__R___ 14. As the number of neutrons in an atom of a given element increases, its
atomic number generally ________________ .
__I___ 15. Going down a group of elements, the atomic radius (size)?
__D___ 16. Going down a group of elements, the ionization energy?
__D___ 17. Going left to right across a period, the atomic radius?
__R___ 18. Going down a group 2, then number of valence electrons?
__D___ 19. As a metallic atom becomes a cation, its radius?
__D___ 20. As the atomic radius of the noble gases increases, the ionization energy
__I___ 21. As a nonmetallic atom becomes an anion, its radius?
__I___ 22. Going from left to right across a period, the ionization energy?
__I___ 23. Going from left to right across a period, the number of valence electrons?
__I___ 24. Gong down group 1, the tendency to lose electrons?
__I___ 25. Going from left to right across a period, the tendency to gain electrons?
26. The primary factor in determining the variation in size going down a group is?
a) increase in nuclear charge
c) decrease in size
b) increase in the number of neutrons
d) addition of energy levels (shielding)
27. The primary factor in determining the variation in size going from left to right in the
periodic table is ? .
a) increase in nuclear charge
c) decrease in size
b) increase in the number of neutrons
d) addition of energy levels
28. The primary factor in determining the variation in ionization energy going down a
group is?
a) increase in shielding
c) increase in nuclear charge
b) decrease in shielding
d) decrease in nuclear charge
29. The electron dot notation for S-2 ion is?
S
-2
30. The electron dot notation for Si+4 ion is?
Si+4
31. The electron dot notation for an atom of Nitrogen (N) is?
N
Fill in the table below
Element or Ion of
element
Ni2+
Noble Gas Configuration
Dot diagram
[Ar]3d8
Ni2+
Si
[Ne]3s23p2
Br[Ar]4s23d104p6
Cr
[Ar]4s23d4
Cr
W
[Xe]6s24f145d4
Y2+
33.
Be
34.
35.
a.
b.
c.
d.
e.
W
Y2+
[Kr]4d1
Which of the following elements is most metallic?
Ca
Ba
Which group holds electrons more tightly?
Metal or Non-metals?
Name that element:
Halogen with the lowest ionization energy Astatine
Alkali metal with the highest electronegativity. Lithium (Hydrogen???)
Period 3 element with the smallest atomic radius. Argon
Group 14 element with the greatest shielding. Lead
Period 4 element with the greatest nuclear charge. Lead
1s22s22p63s23p64s23d104p3
36. How many electrons does the above element contain? ___33___
37. How many valence electrons does the above element contain? ___5______
38. How many electrons are in the highest energy level of the above element? ___5
39. What element is it?
Arsenic
40. Sodium (Na) and potassium (K) are in the same group on the periodic table.
Based on their locations, which statement about sodium and potassium is true?
a. Sodium is less electronegative than potassium.
b. Sodium has fewer orbital shells than potassium.
c. Sodium has a larger ionic radius than potassium.
d. Sodium has lower ionization energy than potassium.
41. The chart shows the electronegativity values as the elements are arranged on the
periodic table.Which statement best describes the electronegativity values of the
elements shown?
a. Electronegativity decreases with increasing atomic number within a period.
b. Electronegativity decreases with increasing atomic number within a group.
c. Electronegativity tends to be higher in the metals than in the nonmetals.
d. Electronegativity tends to be lower in the gases than in the solids.
42. The Periodic Table of the Elements is useful for revealing patterns and trends in
the elements. Which statement accurately describes a pattern in the size of atomic
radii in the Periodic Table of the Elements?
a. Atomic radii decrease from left to right across a period and decrease from top
to bottom in a group.
b. Atomic radii increase from left to right across a period and increase from top
to bottom in a group.
c. Atomic radii decrease from left to right across a period and increase from top
to bottom in a group.
d. Atomic radii increase from left to right across a period and decrease from top
to bottom in a group.
.
43. The diameter of neutral atoms generally decreases going left to right across one
period on the periodic table. What change causes this decrease in diameter of
atoms?
a. The number of outermost electrons decreases.
b. The number of outermost electrons increases.
c. The attractive force between the protons and neutrons increases.
d. The attractive force between the protons and electrons increases.
44. The atomic radius of magnesium is 150 pm. The atomic radius of strontium is 200
pm. What is the atomic radius of calcium?
a. Smaller than 150 pm
b. Greater than 200 pm
c. between 150 and 200 pm
d. not enough information
45. Which element has the largest atomic radius?
a. A
b. B
c. C
d. D
46. Which of these elements is the most electronegative?
a. Argon
b. Chlorine
c. Phosphorus
d. Sulfur
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