Chapter 1 starts off with a comprehensive summary of basic chemical principles, such as atomic structure, ionic radii, electronegativity and solubility products.
An atom's electronegativity is affected by both its atomic number and the distance between the valence electrons and the nucleus.
Electronegativity is a chemical property that describes the tendency of an atom or a functional group to attract electrons (or electron density) towards itself.
The oxidizing tendency of peroxides is related to the electronegativity of the substituents.
The atomic orbital energy correlates with electronegativity as more electronegative atoms hold their electrons more tightly, lowering their energies.
Elements in the same group tend to show patterns in atomic radius, ionization energy, and electronegativity.
Conversely, bonds to other atoms are very strong because of fluorine's high electronegativity.
The trifluomethyl group has a significant electronegativity that is often described as being intermediate between the electronegativities of fluorine and chlorine.
