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Diff Chemistry
Name______________
Answer questions 1-25 from studying the graphs.
Atomic Radius vs Atomic
Number
Atomic Radius
250
200
150
Series1
100
50
0
1
5
9
13
17
21
25
29
33
Atomic Number
The above graph is a plot of the relative atomic radius and relative ionization energy as a
function of the atomic number. Relative means that adjustments were made so that both
plots fit on the same graph and are both clearly visible.
1.
How does the relative A.R. and I.E. for Li (within the Li to Ne period)
compare with one another?
2.
How does the relative A.R. and I.E. for Ne (within the Li to Ne period)
compare with one another?
3.
What happens to the I.E. for the second half of the transition metals? What
might be an explanation for this observation?
4.
Label Be, Mg, and Ca. Why do these elements have a higher I.E. than the
elements B, Al, and Ga?
5.
How does the size of the atom and I.E. change moving down a column?
Explain why?
6.
How does the size of the atom and I.E. change moving left to right across a
period? Explain why?
7.
How does the size of that atom and subsequent I.E. affect the chemical
properties of atoms?
Ionization Energy vs Atomic Number
Ionization Energy
2500
2000
1500
Se rie s1
1000
500
0
1
4
7
10 13 16 19 22 25 28 31 34
Atomic Number
Label the elements He, Ne, Ar, and Kr. These elements belong to the same group,
namely, the noble gases.
8.
What is the trend concerning ionization energy (IE) going down a column or
group of the periodic table?
9.
Label elements Li, Na, and K on the chart.
10.
What is the trend moving from Li to Ne, Na to Ar, and K to Kr moving from
left to right on the periodic table.
11.
Circle the transition elements 20-30. If these elements were cut out would the
pattern from K to Ar be more like the pattern from Li to Ne and Na to Ar.
Explain why.
12.
Label Zn on the graph. The elements in the column headed by zinc are
sometimes called the pseudonoble gases. Why do you think this name is an
apt description?
13.
What might produce a spike in IE for Zn?
14.
Generally the atoms of metals are (larger or smaller) in size and have (lower
or higher) first ionization energies. What do you think? Metals are more
likely to (lose or gain) electrons to form (cations or anions).
15.
Where on the periodic table are the largest atoms?
16.
Where on the periodic table are the atoms with the lowest ionization energy?
17.
Where on the periodic table are the atoms most likely to lose electrons to other
atoms?
18.
In general what is the relationship between atomic radius (size of the atom)
and first ionization energy?
Comparison Chart of I.E. and
A.R.
Relative I.E. and A.R.
1.6000
1.4000
1.2000
1.0000
Series1
0.8000
Series2
0.6000
0.4000
0.2000
0.0000
1
5
9
13 17 21 25 29 33
Atomic Number
The above graph is a plot of the relative atomic radius and relative ionization energy as a
function of the atomic number. Relative means that adjustments were made so that both
plots fit on the same graph and are both clearly visible.
19.
How does the relative atomic radius and ionization energy for Li (within the
Li to Ne period) compare with one another?
20.
How does the relative atomic radius and ionization energy for Ne (within the
Li to Ne period) compare with one another?
21.
What happens to the I.E. for the second half of the transition metals compared
to the first half? What might be an explanation for this observation?
22.
Label Be, Mg, and Ca. Why do these elements have a higher I.E. than the
elements B, Al, and Ga?
23.
How does the size of the atom and I.E. change moving down a column?
Explain why?
24.
How does the size of the atom and I.E. change moving left to right across a
period? Explain why?
25.
How does the size of that atom and subsequent I.E. affect the chemical
properties of atoms?