- Apr 2020
-
chem.libretexts.org chem.libretexts.org
-
Generally, the stronger the bond between the atoms of an element, the more energy required to break that bond.
This makes sense and it would be vice versa for weak bond between the atoms of an element, the less energy required to break that bond.
-
The atomic radius is one-half the distance between the nuclei of two atoms (just like a radius is half the diameter of a circle).
When I read this It brought me back to when I was taught about the radius of a circle and diameter in math class.
-
The first ionization energy is the energy requiredto remove the outermost, or highest, energy electron, the second ionization energy is the energy required to remove any subsequent high-energy electron from a gaseous cation, etc.
Good thing to note that some elements could have several ionization energies.
-
The lower this energy is, the more readily the atom becomes a cation. Therefore, the higher this energy is, the more unlikely it is the atom becomes a cation.
I realized that cation means to become a more positive charged ion.
-
The lanthanides and actinides possess more complicated chemistry that does not generally follow any trends.
No wonder they dont follow any general trends their more complex then Noble gases.
-
Because elements on the left side of the periodic table have less than a half-full valence shell, the energy required to gain electrons is significantly higher compared with the energy required to lose electrons. As a result, the elements on the left side of the periodic table generally lose electrons when forming bonds.
On the periodic table from left to right the electronegativity increases.
-
However, the most common scale for quantifying electronegativity is the Pauling scale (Table A2), named after the chemist Linus Pauling.
This was interesting to realized Pauling scale was named after Linus Pauling. Also, how electronegativity describes an atoms ability to attract and bin with other electrons.
-
Periodic trends are specific patterns that are present in the periodic table that illustrate different aspects of a certain element, including its size and its electronic properties.
The periodic table has different patterns involved such as electronegativity, ionization energy, electron affinity, atomic radius, the types of groups, and more.
-