The thermite reaction used to weld the iron rails releases about 850 kJ of energy per mole of iron oxide consumed. Electron affinity and ionization energy are two chemical terms used to quantitatively describe the behavior of electrons and atoms. The main difference between electron affinity and ionization energy is that electron affinity indicates the amount of energy released when an atom gains an electron, while ionization energy is the amount of energy needed to remove an electron from an atom. The second ionization energy is the energy needed to remove another electron to form a Na2+ ion in the gas phase. The electron affinity of an element is the energy released when a neutral atom in the gas phase receives an extra electron to form a negatively charged ion. For example, a fluorine atom in the gas phase releases energy when it gains an electron to form a fluoride ion. This can be explained by finding that the outermost or most energetic electron is on a lithium atom in orbital 2s. Since the electron in a 2s orbital already has a higher energy than the electrons in a 1s orbital, it takes less energy to remove that electron from the atom. Electronic affinities are more difficult to measure than ionization energies and are generally known to a smaller number.

The electronic affinities of the main elements of the group are illustrated in the following figure. But there is an important difference in how electrons are distributed in these atoms. Hund`s rules predict that the three electrons in the 2p orbitals of a nitrogen atom all have the same spin, but the electrons are paired in one of the 2p orbitals on an oxygen atom. The process by which the first ionization energy of hydrogen is measured would be represented by the following equation. However, if this data is listed with the electronic configurations of these elements, it makes sense. These data can be explained by noting that electronic affinities are much smaller than ionization energies. As a result, elements such as helium, beryllium, nitrogen, and neon, which have exceptionally stable electronic configurations, have such low affinities for extra electrons that no energy is emitted when a neutral atom of these elements takes on an electron. These configurations are so stable that it takes energy to force one of these elements to take an extra electron to form a negative ion.

The energy required to form a Na3+ ion in the gas phase is the sum of the first, second and third ionization energies of the element. Ionization energy: Ionization energy describes the absorption of energy from outside. Use the Bohr model to calculate the wavelength and energy of the photon that would have to be absorbed to ionize a neutral hydrogen atom in the gas phase. Electronic affinity: Electron affinity is the amount of energy released when a neutral (gas-phase) atom or molecule takes an electron from outside. The electron affinity shows periodic variations in the periodic table. This is because the incident electron is added to the outermost orbital of an atom. The elements of the periodic table are arranged in ascending order of their atomic number. As the atomic number increases, the number of electrons they have in their outermost orbitals increases. Now you know that sodium forms Na+ ions, magnesium Mg2+ ions and Al3+ aluminum ions. But have you ever wondered why sodium doesn`t make Na2+ ions or even Na3+ ions? The answer can be obtained from the data for the second, third and higher ionization energy of the element.

Therefore, it takes more energy to remove an electron from a neutral sodium atom than is emitted when the electron is absorbed by a neutral chlorine atom. We will obviously have to find another explanation for why sodium reacts with chlorine to form NaCl. However, before we can do that, we need to know more about the chemistry of ionic compounds. The energy required to remove one or more electrons from a neutral atom to form a positively charged ion is a physical property that affects the chemical behavior of the atom. By definition, the first ionization energy of an element is the energy required to remove the outermost or most energetic electron from a neutral atom in the gas phase. Electrons are subatomic particles of atoms. There are many chemical concepts to explain the behavior of electrons. Electron affinity and ionization energy are two such concepts in chemistry. Electron affinity is the amount of energy released when a neutral atom or molecule gains an electron. Electron affinity can also be called electron winning thalpy when meaning is taken into account, but these are different terms because electron winning thalpy describes the amount of energy absorbed by the environment when an atom gains an electron. Ionization energy, on the other hand, is the amount of energy needed to remove an electron from an atom.

The main difference between electron affinity and ionization energy is that electron affinity indicates the amount of energy released when an atom gains an electron, while ionization energy is the amount of energy needed to remove an electron from an atom. The second trend comes from the fact that the principal quantum number of the orbital containing the outermost electron increases as we descend into a crack in the periodic table. Although the number of protons in the nucleus also increases, electrons in the small layers and subshells tend to protect the outermost electron from some of the gravitational pull of the nucleus. In addition, the electron that is removed when the first ionization energy is measured spends less time near the atomic nucleus and therefore requires less energy to remove this electron from the atom. Ionization energy is the amount of energy required for a gaseous atom to remove an electron from its outermost orbital. This is called ionization energy because after removing an electron, the atom receives a positive charge and becomes a positively charged ion. Each individual chemical element has a specific ionization energy value because the atoms of one element are different from the atoms of another element. For example, the first and second ionization energies describe the amount of energy an atom needs to remove an electron and another electron, respectively.

The first ionization energy is the amount of energy needed for a neutral gaseous atom to remove its outermost electron. This outermost electron is located in the outermost orbital of an atom. Therefore, this electron has the highest energy among the other electrons in this atom. Therefore, the first ionization energy is the energy needed to discharge the most energetic electron of an atom. This reaction is essentially an endothermic reaction. The electrons that are removed during nitrogen and oxygen ionization also come from 2p orbitals. Ionization energy: Ionization energy is used to describe the removal of electrons. Ionization energy: Ionization energy is the amount of energy needed for a gaseous atom to remove an electron from its outermost orbital. Hund`s rules can be understood by assuming that electrons try to stay as far apart as possible to minimize the repulsive force between these particles. The three electrons of the 2p orbitals on nitrogen therefore enter different orbitals with their spins in the same direction. In oxygen, two electrons must occupy one of the 2p orbitals.

The repulsive force between these electrons is minimized to some extent by electron pairing. However, there is still some residual repulsion between these electrons, making it slightly easier to remove an electron from a neutral oxygen atom than we would expect from the number of protons in the atomic nucleus. Adding an electron to a neutral atom or molecule releases energy. This is called an exothermic reaction. This reaction results in a negative ion. But if another electron is added to this negative ion, energy should be given to continue this reaction. This is because the incident electron is repelled by the other electrons. This phenomenon is called the endothermic reaction.

In general, the electron affinity should increase along the period from left to right, as the number of electrons increases over a period; Therefore, it is difficult to add a new electron. In experimental analysis, electron affinity values show a zigzag pattern rather than a pattern that shows a gradual increase. The following figure shows the first ionization energies for the elements in the second row of the periodic table. Although there is a general trend towards an increase in the first ionization energy when we go from left to right on this series, there are two smaller inversions in this model.