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- ALL ABOUT ATOMIC RADIUS
- ALL ABOUT ATOMIC RADIUS!!
- Today we will be learning about Atomic Radius, and the different trends that can be seen throughout the period table!
- Today we will be learning about Atomic Radius, and the different trends that can be seen throughout the periodic table!
- Let's look at the 2nd period on the periodic table. Do you notice something? The atomic radius is decreasing as you move across the period!
- Li - has an atomic radius of 134pmN - has an atomic radius of 75pmNe - has an atomic radius of 69pm
- Let's look at the 2nd Period on the periodic table. Do you notice something? The atomic radius is decreasing as you move across the period!
- Li - has an atomic radius of 134pmK - has an atomic radius of 196pmCs - has an atomic radius of 225pm
- Now, let's look at the trend of Atomic Mass as we move down a group. Please look at the 1st group on the Periodic Table. What do you notice? The Atomic Mass is increasing as you move down the group!! Isn't that interesting?
- COULOMBIC ATTRACTIONCoulombic Attraction refers to the attraction between two oppositely chargedparticles in an atom, which refers to protons and electrons. Coulombic Attraction refers to the attraction force exerted on the valence electron bythe protons, and the amount of force changes based on the Atomic Radius
- Atomic Radius affects Coulombic Attraction because, if the Atomic Radius is smaller, that means that the valence electron of the atom is closer to the proton, which allows the proton to have a stronger attraction force on the valence electron.
- WHY DO WE SEE THIS TREND?We see the Atomic Radius decrease as we move across the period because there are more protons present in the atom but the samenumber of electron shells
- There are more protons present in each atom as you move across the period, but the same number of electron shells. This means that the valence electrons are in the same energy level for all the atoms in the period, but the number of protons increases, and hence the positive charge present in the atom, increases, pulling the valence electrons closer and causing the Atomic Radius to be smaller.
- WHY DO WE SEE THIS TREND?We see the Atomic Radius increase as you move down a group because the valenceelectrons get further away from the nucleus
- As you move down a group, the number of electron shells increases. This meansthat the valence electrons get further from the nucleus as you move down the group, and because of that, the attraction force that is exerted by the protons has a weaker effect on the valence electron and cannot pull it closer to the nucleus.
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