Atomic Element First Atomic # symbol ionization radius energy (pm) (kJ/mol) H 1312 32 N He 2372 31 3 Li 520 123 4 Be 899 90 5 B 801 82 6 C 1086 77 7
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Question

Graphing Trends in the Periodic Table


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  1. Draw a line in the middle of a piece of graph paper, separating the page into top and bottom. On the top, plot a graph of ionization energy (y-axis) vs. atomic number (x-axis). On the bottom plot a separate graph of atomic radius vs. atomic number. For each graph connect successive dots with straight lines. Also, ensure that identical atomic numbers are plotted on the same vertical position on the sheet (i.e. atomic number 1 in the top graph should be on the same line as atomic number 1 in the bottom graph). 
  2. Examine your graph of ionization energy vs. atomic number. 
  3. Which elements are found at the main peaks on your graph (there should be 3)? What do these elements have in common? 
  4. Which elements are found at the main valleys on your graph? (there should be 3)
  5. What do these elements have in common? 
  6. Examine your graph of atomic radius versus atomic number. 
  7. Which elements are found at the peaks on your graph? What do these elements have in common? 
  8. Which elements are found at the valleys on your graph? What do these elements have in common? 
  9. How are atomic radii and ionization energy related (i.e. as atomic radius increases, what happens to the ionization energy)? 

Atomic radii and ionization energy related in this way: when we move from left to right across the periodic table, the atomic radii of elements becomes smaller. Having a smaller radius, the electrons are placed very tightly to the nucleus than larger atoms. So, the ionization energy that is required to withdraw an electron would be greater in regard to the smaller atoms.

  1. Generally, as you go from left to right across a period on the periodic table, what happens to atomic radius? What about IE? 

As you go from left to right across a period on the periodic table the atomic the radius tend to decrease.Keep in mind that  atomic radius always decreases from left to right within a period. It happens because the number of protons and electrons across a period are increased.

  1. Generally, as you go down a group in the periodic table, what happens to atomic radius and IE? 

Generally, as you go down a group in the periodic table, the atomic radius increases. Remember that when you move down a group in the periodic table, the number of filled electrons increases. 

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Atomic
Element
First
Atomic
#
symbol
ionization
radius
energy
(pm)
(kJ/mol)
H
1312
32
N
He
2372
31
3
Li
520
123
4
Be
899
90
5
B
801
82
6
C
1086
77
7
N
1402
75
8
O
1314
73
9
F
1681
72
10
Ne
2081
71
11
Na
496
154
12
Mg
738
136
13
Al
578
118
14
Si
786
111
15
P
1012
106
16
S
1000
102
17
CI
1251
99
18
Ar
1521
98
19
K
419
203
20
Ca
590
174

Top Answer

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atomic radius and ionization energy.jpg

Number atonirst ionization energy (KJ/mol)
1
1312
Graphing Trends in the Periodic Table
2372
2500
520
899
20 00
801
1086
15 00
1402
1314
10 00
1681
500
2081
496
738
810 11 12 13 14 15 16 17 18 19...

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