chemistry

Predictions:

Atomic Radius Vs. Atomic number of Representative Elements

As you go down a group, the atomic radius increases, because we are adding an additional energy level to the outer shell, therefore causes the atomic radius to increase.
As you move across the period table, the atomic radius should decrease, because adding another proton as you go across the period would have a greater attraction to the nucleus pulling it closer together, which decreases the size of the atomic radius.

Ionization Energy Vs. Atomic number of Representative Elements

As you go down a group, the ionization energy should stay constant, because it either has the same cation energy of anion energy, keeping it consistently staying the same.
As you go across the periodic table, the ionization energy will increase, because Ionization is the energy needed to remove an electron from an atom.



Electronegativity Vs. Atomic number of Representative Elements

As you move across the period table, the electro negativity should increase, because the atomic number increases and electro negativity is the ability for an atom to pull electrons towards itself. So I believe it’s the opposite of ionization, and metals tend to loose electrons in bonds while non metals tend to gain the electron.
As you go down a group, the ionization energy should stay constant also, because it either has the same cation energy of anion energy, keeping it consistently staying
the same.







Atomic Radius Vs. Atomic number of Representative Elements

My predictions were correct. When moving down a group in the periodic table, the
atomic radius will increase, because the valence electron occupy’s an extra energy level (shell) that is farthest from the nucleus, causing less of an attraction to the nucleus. That is why the atomic radius decreases while going down a group on the period table. While going across the period table, the size of an atom decreases because the positive charge on the nucleus also increases across a period. For ex. Lithium has 3 protons, 3 electrons vs. Beryllium, 4 protons, and 4 electrons. By having that extra proton causes a greater attractions with the electrons on the outer energy level, thus resulting in the radius decreases as we move left to right on the periodic table because the nucleus is pulling the outer energy level closer to it.

Ionization Energy Vs. Atomic number of Representative Elements

My predictions were partially true. While going down a group on the period table, the ionization decreases. It decreases because as you move down, the atomic number increases which has more energy levels, which has a weaker attraction to the nucleus and is easier to remove that electron to occupy a full outer shell. For example, Cesium has 55 electrons. It has many energy levels, which has 1 valence electron on the outer shell, causing a weak attraction to the nucleus and is easier to loose it’s electron, vs. Lithium which has 3 electrons, 2 energy levels, 1 valence electron, BUT is closer to the nucleus which is harder to remove than cesium. While going across the periodic table, the ionization does increase, because it gets harder to remove an electron. On the left side, they’re all cation, which need to loose their electron to balance a full outer shell, and on the right side they’re all anions. For example, Potassium has 19 electrons, and needs to occupy 18 to have a full outer shell. So it is most likely for potassium to loose that 1 electron vs. Argon, which has 18 electrons, and is satisfied having a full outer shell.

Analyzing Atomic Radius, Ionic Radius, Ionization Energy and Electronegativity.

Predictions:
Atomic Radius vs. Number of Representative Elements
Going across the periodic table, I would predict that the pattern of the atomic radius will decrease, while going down the period table the atomic radius will increase.
Ionization vs. Number of Representative Elements
Trend-wise, ionization potentials tend to increase while one progresses across a period because the greater number of protons (higher nuclear charge) attract the orbiting electrons more strongly, thereby increasing the energy required to remove one of the electrons.



Question: How do these four properties of the main-group atoms compare within a group and across a period.
As you go down the period table the atomic raius