electronegativity represents the size of an atom
B. Elements on the top right, excluding column 18.
The bottom number of the original, unsimplified fraction represents the number of equal parts in one whole, where each part is of the same magnitude as the top number. Once the fraction has been simplified, these links no longer apply directly, but only through equivalence.
Any fraction whose numerator (top number) is larger than the denominator (bottom number), for example 2/3, 11/20, or 59/93.
It is a rational number. The reason that it is rational is that you can represent it as a fraction, where the denominator (the number at the bottom of the fraction) is not equal to 0.So, for example, as we could write the number 15.125 as 15125/1000 then it is rational.
To explain simply, think of a fraction. There is a number (in simple cases) on top and a number on the bottom. The numerator is the top number, the denominator is the bottom one. An easy trick I used to remember is that d is for down- denominator goes down. Though probably not as useful, numerator has a u in it, to represent up. Hope this helps!
On the Periodic Table of elements, electronegativity increases as you move left to right across a period.
Decreases
Electronegativity, for an important trend.
Atoms with the lowest electronegativity values located on the leftmost part of the periodic table. The atom with the lowest electronegativity belongs to Francium.
Atoms to the left on the periodic table Atoms with a large atomic radius
Their metallic properties increase and their atomic radii increase.This can be checked with the Reference Table S with the atomic radii and metallic properties. Easy, right?
Electronegativity increases as you move up and to the right. (apex) <3 kw
Electro negativity is lowest in the bottom of the first group. Cs and Fr have least electro negativity.
Atomic size increases to the bottom left, and the following increase up and to the right with exceptions: Electronegativity Electron Affinity (Z-effective) Ionization Energy Elements to right have fuller valence shells, etc
The atomic size increase from top to bottom of Periodic Table. As the number of shells increases from top to bottom, the atomic size increases.
The atomic size increase from top to bottom of periodic table. As the number of shells increases from top to bottom, the atomic size increases.
Examples for the groups I an II of the periodic table:- the atomic radius grows from top to bottom- the electronegativity descends from top to bottom