1-Describe the periodic trend in atomic radius and relate it to atomic structure 2- Describe the periodic trend in electronegativity and relate it to atomic structure Did you know?
There are atoms with no electronegativity because electro negativity refers to the attraction of atoms of electrons in a compound; elements that do not form are assigned no electronegativity values. Atomic Radius ≠ Ionization Energy
As you move from left to right on the periodic table, the number of valance electron increase. As the number of E increases P increases. As positive force increases, the electron get tighter and the radius gets smaller. Ionization energy is the energy required to remove an electron. As you move up and down the periodic table, the number of electron shells changes. As the number of shells increases, there is more shielding between the nucleuses the outermost electron increases. Atomic Radius: is half the distances between 2 identical atoms that are bonded. It is the distance between the nucleus and the outer shell.
When atoms are bonded together, unless they are 2 identical atoms, one of those atoms is always going to be better at attracting electrons to it. Electronegativity: is the ability of an atom to attract electrons to itself. Electronegativity: will increase when it goes from left to right and down to up and will decrease when decreases goes from right to left electronegativity and up to down. Atomic radius: decreases from left to right and down to up, and increases from right to left and up to down. Ionization Energy: will increase when it goes from left to right and down to up and will decrease when decreases goes from right to left electronegativity and up to down. As we move fro, left to right on the periodic table the atomic radius decreases, and as it decreases, the nucleus is better able to attract electrons to it. So, electronegativity increases going from left to right. As you move from top to bottom,...