Graphing Periodic Trends

Introduction:
The periodic is a table of the elements, organized in order of increasing atomic number. Elements that have similar chemical properties and electronic structures appear in vertical columns, or also called groups. The Periodic Law states that when elements are placed in order of increasing atomic number, their physical and chemical properties display a periodic pattern. The purpose of the lab was to discover how two periodic properties, atomic radius, and first ionization energy, vary with the atomic number for the first 20 elements.
Materials:
Please refer back to the materials listed on pg.45 in the Nelson Chemistry 11.
Procedure:
Please refer back to the materials listed on pg.45 in the Nelson Chemistry 11.
Observations:
Atomic Radius vs. Atomic Number/Name Element | Atomic Radius | H | 53 | He | 31 | Li | 167 | Be | 112 | B | 87 | C | 67 | N | 56 | | O | 48 | F | 42 | Ne | 38 | Na | 190 | Mg | 145 | Al | 118 | Si | 111 | P | 98 | S | 88 | Cl | 79 | Ar | 71 | K | 243 | Ca | 194 | | Analysis: A) Describe any trends for the atomic radius versus atomic number within a period and within a group?
Going from left to right, the radius decreases as the increasing number of protons pulls electrons closer to the nucleus. Comparably, going from top to bottom, the radius increases as the atoms begin filling more and more valence shells. B) In which group of elements do the atoms have the largest radii as you move across the period?
Group 1 have the largest radii as you move across the period. This is because Group 1 is on the start of the periodic table and as you move across the period table, the radii decreases. C) In which group of elements do the atoms have the smallest radii as you move across the period?
Group 8 has the smallest radii as you move across the period. This is because Group 8 is on the end of the periodic table and as you move across the period table, the radii decreases. D) Describe any trends for first ionization energy versus atomic number within a period within a group?
Ionization energies increase moving from left to right across a period, Comparably, Ionization energy decreases moving down a group. E) In which group of elements to the atoms have the greatest first ionization energy as you move across a period?
Group 8 has the greatest first ionization energy. As an example, Argon, Ar, has the first ionization energy of 1521; compared to an element in Group 1, Sodium, Na, has only 496. F) In which group of elements do the atoms have the smallest first ionization energy as you move across a period?
Group 1 has the smallest first ionization energy as ionization energies increase moving from left to right across a period. G) Compare the trend for atomic radius and the trend of ionization energy. How do these properties relate to one another?
They both work like opposites! Ionization energies increase moving from left to right across a period, compatibly, the atomic radii decreases going left to right. Ionization energy decreases moving down a group, atomic radii increases while going down a group. H) Using your graphed data, predict the atomic radius and the ionization energy for scandium, Sc, and titanium, Ti. Research the accepted values. Compare your predictions to the actual values. How close were your predictions?
I believe that the atomic radius of Scandium would decrease because you are moving across the period. My best guess would be based on the fact that Calcium has an atomic radius of 194. As for Titanium, I believe it would continue to go down as you continue to move across the period. As for ionization energy, For Scandium and Titanium, I would believe that is increasing because ionization energy increases as you move across the period. Element | Best Guess for Atomic Radius vs. Actual Values | Best Guess for Ionization Energy vs. Actual Values | Scandium | 180 (guess)- 184(actual) | 600 (guess)- 630(actual) | Titanium | 174(guess)- 176(actual) | 640(guess)-657(actual) |

I) Predict the relationships between electron affinity and atomic number. Sketch a graph of these two variables. Labe the axes properly.
There is a general increase in electron affinity as you move from left to right on the periodic table. This is because of the production of more stable anions as you move right.