The electron affinities of the noble gases have not been conclusively measured, so they may or may not have slightly negative values. Chlorine most strongly attracts extra electrons. Nonmetals like to gain electrons to form anions to have a fully stable electron shell. Nonmetals: Generally, nonmetals have more positive electron affinity than metals.Mercury most weakly attracts an extra electron. The electron affinity of metals is lower than that of nonmetals. Metals: Metals like to lose valence electrons to form cations to have a fully stable shell.Chlorine most strongly attracts extra electrons, while neon most weakly attracts an extra electron.Īffinities of Non metals vs. Atoms whose anions are more stable than neutral atoms have a greater affinity. Moreover, nonmetals have more positive affinity than metals. However, nitrogen, oxygen, and fluorine do not follow this trend. The electron affinities will become less negative as you go from the top to the bottom of the periodic table. Generally, the elements on the right side of the periodic table will have large negative electron affinity.
Although affinity varies greatly across the periodic table, some patterns emerge. The greater the negative value, the more stable the anion is. This affinity is known as the second electron affinity and these energies are positive.Įlectron affinity can be either positive or negative value. Characteristics: Chlorine is a greenish-yellow, diatomic, dense gas with a sharp smell (the smell of bleach). However, more energy is required to add an electron to a negative ion which overwhelms any the release of energy from the electron attachment process. Harmful effects: Chlorine is a toxic gas that irritates the skin, the eyes and the respiratory system. By convention, the negative sign shows a release of energy. In 1811, Sir Humphry Davy concluded the new gas was in fact a new element. By 1810, the scientific consensus was that chlorine was actually a compound that contained oxygen. This affinity is known as the first electron affinity and these energies are negative. Elemental chlorine was first prepared and studied in 1774 by Swedish chemist Carl Wilhelm Scheele.
When an electron is added to a neutral atom, energy is released. To use electron affinities properly, it is essential to keep track of sign. Electron affinities are more difficult to measure than ionization energies.Īn atom of Chlorine in the gas phase, for example, gives off energy when it gains an electron to form an ion of Chlorine.Ĭl + e – → Cl – – ∆H = Affinity = 349 kJ/mol Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. The change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion. In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as: Electron affinity of Chlorine is 349 kJ/mol.