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PERIODIC TRENDS PRACTICE QUESTIONS:
Name ______________________
Per. ________
For each set of elements indicate which one of the four is the answer.
1) B
Al
Ga
In
a) Most metallic (easiest to lose an electron)? _____
b) Least metallic (hardest to lose an electron)? _____
c) Lowest electronegativity? _____
d) Highest ionization energy? _____
e) Largest atomic radius? _____
f) Which are non-metals? _____
g) Which are conductors? _____
h) Highest shielding effect? _____
i) List them in order from small to large. _____, _____, _____, _____
j) Would they gain or lose electrons to form ions? _____
What charge would the ion
have? _____
k) Would these be considered cations or anions? _____
l) Would the ion be larger or smaller than the atom? _____
2) Sb
Sn
Te
I
a) Highest metallic character? _____
b) Highest electron affinity? _____
c) Lowest I.E.? _____
d) Smallest? _____
e) Which are metalloids? _____
f) List in order of increasing size (from small to large) _____, _____, _____, _____
g) Which is least dense? _____
h) When Iodine becomes an ion, is the ion larger or smaller than the atom? _____
i) When Tin (Sn) becomes an ion, is the ion larger or smaller than the atom? _____
j) Highest shielding effect? _____
k) Which one is a halogen? _____
3) In each set, circle the larger atom or ion AND explain why.
a) Ca v. K ___________________________________________________
b) As v. Se __________________________________________________
c) S
v. O ___________________________________________________
d) Rb v. Li __________________________________________________
e) O v. O-2 ___________________________________________________
f) Ca v. Ca+2 _________________________________________________
g) O-2 v. F-1 __________________________________________________
h) S-2 v. Se-2 __________________________________________________
4) Define atomic radius:
____________________________________________________________
Arrange the following elements in order of decreasing atomic size:
a) sulfur, chlorine, aluminum, and sodium.
b) carbon, germanium, lead, silicon
c) cesium, lead, bismuth, barium
5) Define ionization energy:
________________________________________________________________
Arrange the following elements in order of increasing ionization energy:
a) Be, Mg, Sr
b) Bi, Cs, Ba
c) Na, Al, S
6)
a)
b)
c)
d)
In each of the following pairs, circle the most electronegative element
chlorine, fluorine
carbon, nitrogen
magnesium, neon
arsenic, calcium
7) Give the name and symbol for the element found at each of the following
locations on the periodic table:
a) Group 1, period 4.
b) Group 13, period 3.
c) Group 16, period 3
d) Group 2, period 6
8) What is the general term applied to the elements:
a) in Groups 3 - 12?
b) The "4f" row?
c) The "5f" row?
d) in the "d block"?
e) in Group 18?
f) along the zig-zag line?
g) to the right of the zig-zag line?
9) What are some characteristics of metals? Which metals are the most reactive?
Which non-metals?
________________________________________________________________
________________________________________________________________
10) In general do metals or non-metals have:
a) higher ionization energies? ______________________
b) higher electronegativities? ______________________
c) higher malleability? ______________________
d) higher conductivity? ______________________
e) larger ion size compared to the size of the neutral atom? ______________________
11) Be able to Explain the following trends:
a) atomic radius decreases as you go across a period ___________________________
______________________________________________________________________
b) ionization energy increases as you go across a period __________________________
________________________________________________________________________
c) ionization energy decreases as you go down a group ___________________________
________________________________________________________________________
d) negative ions are larger than their neutral atoms___________________________
12) The values of the first three ionization energies (I1, I2, I3) for magnesium and argon
[in kJ/mole] are as follows:
I1
I2
I3
Mg 735 1443 7730
Ar 1525 2665 3945
(a) Give the Noble Gas electronic configuration of Mg and Ar.
(b) In terms of these configurations, explain why the values of the first and second
ionization energies of Mg are significantly lower than the values for Ar, whereas
the third ionization energy of Mg is much larger than the third ionization energy
Ar.
(c) Element Q has the following first three ionization energies [in kJ/mole]:
I1
Q
I2
I3
496 4568 6920
What is the formula for the most likely compound of element Q with chlorine?
Explain the choice of formula on the basis of the ionization energies.
13) Explain each of the following observations using principles of atomic structure
and/or bonding.
a) Potassium has a lower first-ionization energy than lithium.
b) The ionic radius of N3¯ is larger than that of O2¯.
c) A calcium atom is larger than a zinc atom.
d) Boron has a lower first-ionization energy than beryllium.