Atomic-Man
Storyboard Text
- Hey Guys, my name is Atomic Man and today we will be using your knowledge on protons, electrons, atomic number, and mass in order to learn about Atomic Radius and Ionization Energy.
- Let's first look at Coulombic Attraction. Coulombic Attraction defines the attraction between the positively charged protons and the negatively charged electrons in an atom. This force's power can also be affected by how far away the protons and electrons are from each other.
- Atomic Radius is the distance between the atom’s nucleus and its valence shell. It increases as we go down a group and decreases as we go across a period. For example in group 1 Hydrogen’s atomic radius is 37pm, Lithium’s 152pm,and Sodium’s is 186pm. In Period 3, Sodium’s atomic radius is 186pm, Magnesium’s 160pm, and Silicon’s 117pm.
- Atomic Radius is based on the Coulombic Attraction of an element. The Coulombic attraction causes an element to have attraction force between the protons and the electrons, this in turn can cause an element to have a certain atomic radius based on how strong the connection between their electrons and protons are. We see the uptrend down the group because all the elements have the same valence electron amount there, but have more protons as you go down the group.
- We see the downtrend in the period because there are more electrons in the valence shell and protons in the nucleus as we go across a period. We see the uptrend in the group because, the electron amount in the valence shell stays the same, while the protons increase as we go down.
- Ionization energy is the amount of energy required to remove an electron from an atom. This energy amount increases as we go across a period and decreases as we go down a group. For example Lithium’s ionization energy is 520.2, Boron’s 800.6, and Oxygen’s 1313.9. In group 1, Lithium’s ionization energy is 520.2, Sodium’s 495.8, Potassium’s 418.8. The Shielding effect is basically where the more inner electrons in an atom, the less force there is between the nucleus and outer electron and that’s why the higher the shielding effect the lower the ionization energy.
- This in turn causes the element to have high Ionization energy since it needs more energy to pull an electron out of a high attractive force. We see the downtrend in the group because the atomic radius of elements increase as we go down the group and in turn this means the coulombic attraction decreases. We see the uptrend in the period because the atomic radius of elements decrease as we go across the period, and in turn the coulombic attraction decreases.
- Ionization energy is based on the Coulombic Attraction of an element. The Coulombic Attraction as previously mentioned affects the atomic radius, and this in turn affects the Ionization Energy. For example, when an element has a high Coulombic Attraction it has a low Atomic Radius since the opposites ends of the atom are pulling to each other.
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