Electron electronegativity

Matter consists of atoms that are made up of protons (electropositive), electrons (electronegative), and neutrons (electrically neutral). Because the number of electrons and protons is equal, elements, atoms with different numbers of protons, have different numbers of electrons. The chemical properties of an element depend on the number of electrons, but because the electrons have almost no mass, the atomic weight of an element is its number of protons and neutrons. Neutrons are needed to hold the protons together in the nucleus. Isotopes are elements with different numbers of neutrons. Isotopes with too many neutrons are unstable and emit radioactivity. Radioactive and nonradioactive isotopes are used to follow biochemical reactions in health and disease, to date paleontology specimens, usually bones and teeth, and detect traces of life in ancient rocks. 

Whenever two atoms form a bond, the nucleus of each atom attracts the other s electrons. Electronegativity is a measure of the strength of this attraction. 

Electronegativity is defined as the attraction of an atom for its outer shell electrons. Electronegative elements have a strong attraction for electrons and form anions in chemical reactions electropositive elements have relatively weak attractions for electrons and form cations. 

The octet rule states that an atom will give up, accept, or share electrons in order to fill its outer shell or attain an outer shell with eight electrons. Electropositive elements readily lose electrons electronegative elements readily acquire electrons. The electronic configuration of an atom describes the orbitals occupied by the atom s electrons. Electrons in inner shells are called core electrons electrons in the outermost shell are called valence electrons. Lone-pair electrons are valence electrons that are not used in... 

The mutual satisfaction of the need to attain the inert gas electronic configuration by those elements that lose electrons (electropositive elements) and those that gain electrons (electronegative elements) leads to the ionic bond. To illustrate this, consider sodium chloride [NaCl]. Sodium (with low iorrization energy) can easily lose the outermost 3 s electron to achieve the stable inert gas corrfiguration. Chlorine,... 

We should note that the last seven elements are all metals and the first twelve all non-metals. Also that oxygen is particularly greedy f or electrons and nitrogen only a little less so. Carbon and hydrogen are moderately electronegative, but do not differ much in their attractive power for electrons. Electronegativity determines much of the behaviour of elements and their compounds. 

Electron affinity is defined for an isolated atom and measures the energy change for adding an electron. Electronegativity is defined within chemical compounds and it estimates the propensity of an atom to attract electrons to itself. 

Linus Pauling, one of America s most famous chemists, devised a scale of numerical values reflecting the tendency of an atom to attract electrons. Electronegativity is a measure of the abiiity of an atom in a chemicai compound to attract eiectrons from another atom in the compound. The most electronegative element, fluorine, is arbitrarily assigned an electronegativity of four. Other values are then calculated in relation to this value. 

Electron affinity is the attraction a free atom has for electrons. Electronegativity is the attraction a bonded atom has for it shared electrons. A number is assigned to the electronegativity of an element in order to compare one element to another and determine the polarity of a bond. 

---