1. a) The trend I notice from hydrogen to the highest numbered atom is that the atomic size increases as you go left from the element, and it decreases once you go up a group.

b) Across a period, the size of an atom decreases (left to right). The increased positive charge in the nucleus has a greater attractive force for the outer valence electrons in the same energy level

c) Up a group, the size of an atom decreases. The attractive force between the positive charge in the nucleus and the valence electrons decreases because these electrons are farther from the nucleus.

4. a) The elements that are found at the main peaks of my graph are Lithium, Sodium, Potassium, and Rubidium. These elements are all found in the same group. They are all Alkali Metals.

b) The elements that are found at the main valleys of my graph are Neon, Argon, Krypton, and Helium. These elements are all found in the same group. They are all …show more content…
a) Ionization energy increases as the atomic radius decreases.

b) When the atomic radius is smaller, you will need more energy to remove an electron because the pull from the nucleus on the electron is stronger. If the atomic radius is larger, then it will be much easier to remove an electron from the valence shell because there are more layers between the nucleus and valence shell.

11. a) Ionization energy decreases when atomic number increases. As Atomic Number increases, the number of electrons around the nucleus goes up also. As the size of the electron cloud increases, the outer electrons are more shielded from the protons, so it requires less energy to overcome the positive-negative attraction forces.

b) Ionization energy increases across a period. The attractive force between the positive charge in the nucleus and the outer valence electrons is increased.

c) Ionization energy increases up a group. There is a weaker attraction between the positive charge in the nucleus and the outer valence electrons as they occupy higher energy