Chapters
5 Name
_________________________________________ Per_________
1. Based
only the periodic table placement, predict the oxidation number of the
following elements:
a) Rb b) In c) Bi d) Cl e) Ba f) Te g) Xe
2. To
what period and group would an element ending with a 3d5 electron
belong?
3. To
what period and group would an element ending with a 6p2 electron
belong?
4. Would
an element with two electrons on the highest (outer) energy level be a metal or
a nonmetal?
5.
Classify the following elements as metal, nonmetal, metal metalloid or
nonmetal metalloid.
a) chlorine b) radium c) arsenic d) cerium
e) tin f) boron g) phosphorus h) osmium
i) iodine j) manganese k) uranium l) argon
6.
Within a period, does the size of an atom increase or decrease with
increasing atomic number? ________________
7.
Within a family, does the size of an atom increase or decrease with
increasing atomic number? ________________
8.
Within a period, does the first ionization energy increase or decrease
with increasing atomic number? ______________
9.
Within a family, does the first ionization energy increase or decrease
with increasing atomic number? ______________
10. Within
a period, does the metallic character increase or decrease with increasing
atomic number? ________________
11.
Within a family, does the metallic character increase or decrease with
increasing atomic number? ________________
12.
Within a period, does the electron affinity increase or decrease with
increasing atomic number? ________________
13.
Within a family, does the electron affinity increase or decrease with
increasing atomic number? ________________
14. In
each of the following pairs and using only
the periodic table, circle the one with the
lowest electronegativity:
a) Fe S b) In B c) F N d)
Br Te e) Sr Zn f) As
Ag
15. In
each of the following pairs and using
only the periodic table, circle the one with the
lowest first ionization energy:
a) Fe S b) In B c) F N d)
Br Te e) Sr Zn f) As
Ag
16. In
each of the following pairs and using
only the periodic table, circle the one with the
highest electron affinity:
a) Fe S b) In B c) F N d)
Br Te e) Sr Zn f) As
Ag
17. In
each of the following pairs and using
only the periodic table, circle the most metallic
one:
a) Fe S b) In B c) F N d)
Br Te e) Sr Zn f) As
Ag
18. In
each of the following pairs and using
only the periodic table, circle the one that is
larger:
a) Fe
S b) Al B c) F N d)
Br Se e) Ne Ar f) As
Ag
19. In
each of the following pairs, circle the one that is
larger:
a) Na
Na+1 b) H H-1 c) S S-2 d)
Ba Ba+2 e)
Al Al+3 f) P P-3
20. Do
metals tend to form positive or negative ions?
Is the ion formed larger or smaller than the neutral it came from?
21. Do
nonmetals tend to form positive or negative ions? Is the ion formed larger or smaller than the neutral it came
from?
22. A
low ionization energy is characteristic of
________________________________________________.
23. An
element having a high electron affinity is classified as a
____________________________________.
24.
Aluminum has _______________ electrons in its outer energy level.
25. The
alkaline earth metals all form ions with a ____________________ charge.
26.
Alkali metals are the Group _______________________ elements on the
periodic table.
27. Transition metals are
those elements whose highest energy electrons are in the ______ sublevel, and
whose last filled
28 electron
is on the _____ sublevel.
29. The
elements in Group VIIIA were once called ____________________ because they
didn't react.
30. The
________________________ are the most reactive nonmetallic family on the
periodic table.
31. The
element ______________________ is the most reactive nonmetal on the periodic
table.
32. The
element ______________________ is the most reactive metal on the periodic
table.
33. Group VIIA is called the "salt formers" or
__________________________ family.
34. The
element ______________________ is the most reactive of all the elements on the
periodic table.
35. The
energy necessary to remove the most loosely held electron from an atom is
called _______________.
36. The
attraction an atom has for its outer electrons is called
_____________________________________.
37. The ability of a bonded atom to attract
electrons to itself is referred to as the atom's ______________________________.
38. Electronegativity generally
_______________________________ as you go from left to right in a period and
generally
39 ________________________________ as you go
from top to bottom in a group.
40. ____________________ elements have high electronegativities.
41. What is
the difference between electronegativity and electron affinity?
42.
Given the following formulas:
GaCl3 , GaAs, and Ga2O3, Ga(NO3)3;
a)
predict the formula for compounds formed if aluminum, instead of gallium,
combines with these same negative ions
b) predict the formula for compounds formed if fluorine, phosphorus, and selenium combine with gallium (in the same oxidation state as in these compounds).