I don’t have Microsoft Excel on my computer, nor can I download it without causing a virus on my computer. I’ll be submitting this instead, but I will try to make it as close as possible

Gabi Brooks
Chemistry
27 May 2015
Researching Elements in the Periodic Table

Name
Symbol
Atomic number
Atomic mass
Melting point
Boiling point
Electronegativity value
Atomic radius (pm)
Ionic radius (pm)
First ionization energy (kJ/mol)
Lithium
Li
3
6.941 ± 0.002 u
180.54°C
1342°C
0.98
152
68 (+1e)
519.9
Beryllium
Be
4
9.012182 ± 0.000003 u
1287 °C
2471 °C
1.57
112
35 (+2e)
898.8
Scandium
Sc
21
44.955912 ± 0.000006 u
1814 K
3104 K
1.36
162
72.3 (+3e)
630.8
Lathanum
La
57
138.90547 ± 0.00007 u
1193.2 K
3693 K
1.1
187
117.2 (+3e)
538.1
Actinium
Ac
89
227 u
1320 K
3470 K
1.1
188
118 (+3e)
665.5
Aluminum
Al
13
26.981539 ± 0.0000008 u
660.32 °C
2519 °C
1.61
1.43
51 (+3e)
577.539
Boron
B
5
10.811 ± 0.007 u
4000 °C
2075 °C
2.04
98
23 (+3e)
800.2
Carbon
C
6
12.0107 ± 0.0008 u
3820 K
5100 K
2.55
67
16 (+4e)
1085.7
Flourine
F
9
18.998403 ± 0.0000005 u
-219.62 °C
-188.14 °C
3.98

133 (-1e)
1680
Neon
Ne
10
20.1797 ± 0.0006 u
-248.67 °C
-248.048 °C
0
38
0
2079.4

As you go down groups, the atomic number increases. You get extra shells that increase the size of the higher atoms. Going across periods, the ionic radius tends to decrease, due to the higher nuclear charge in the atoms. This increased charge can pull the electrons more closely to the nucleus. The general trends for ionic radii on the periodic table is that going across the rows, the radii get small and smaller since the electrons are all in the same orbital while adding more protons to the nucleus so it "sucks" the electrons in more, while going down shows larger and larger radii due to more orbitals being present. While you go