So this is an exothermic reaction. The noble gases already have a complete set of electrons and an additional electron must go into the next highest shell which will cost energy to start populating.
In general electron affinity follows the following trends.
Electron affinity trends. The trends for electron affinity are not as smooth as those for atomic radius ionization energy and electronegativity as can be seen on the following graphs. As with ionization energy there are two rules that govern the periodic trends of electron affinities. This clip shows how electron affinity generally increases moving to the right on the periodic table and up a column.
Now Ill tell you about the Electron affinity trend in the periodic table. Electron affinity decreases from top to bottom in a Group. Generally electrons tend to repel one another.
Electron affinity becomes less negative down a group. Electron affinity is the energy change when an electron is added to an atom to form an anion negatively charged ion. For example when a fluorine atom in the gaseous state gains an electron to form Fg the associated energy change is -328 kJmol.
Definition of electron affinity Electron affinity is the affinity of an element to an electron. Therefore electron affinity becomes increasingly negative as we move left to right across the periodic table and decreases as we move down a group. Electron affinity is the energy change that results from adding an electron to a gaseous atom.
What are the general trends of electron affinity. Electron affinity Electronegativity Ionization energy 1. Actually there are many factors which affect the electron affinity but to make it simple and easy to remember Ill explain to you with a simple logic.
Because this value is negative energy is released we say that the electron affinity of fluorine is favorable. The symbol is EA and the unit is kJmol. Electron affinity is one of the trends that can be predicted using the organization of elements in the periodic table.
Electron affinity generally increases moving left to right across an element period periodic table row. Patterns in Electron Affinity Electron affinity increases upward for the groups and from left to right across periods of a periodic table because the electrons added to energy levels become closer to the nucleus thus a stronger attraction between the nucleus and its electrons. But the effect if increase in atomic size dominates the increase in nuclear charge.
Because of this electron affinity measures the attraction an atom has for an. Electron affinity decreases down a group and increases along a period. Electron affinity the energy associated with forming an anion is more favorable exothermic when electrons are placed into lower energy orbitals closer to the nucleus.
This is due to increasing effective nuclear. The electron affinity trend describes the trend across the periodic table and describes how much energy in an atom is released or spent when an electron is added to a neutral atom or the energy change that occurs when an electron is added to a neutral atom. Electron affinity increases moving down an element group periodic table column.
In the Periodic Table electron affinity increases becomes more negative from left to right in a period. But there are some exceptions. This is measured by the energy released when an element in its gaseous state accepts an electron to form an anion.
The energy released when an electron is added to a gaseous atom which is in its ground state to form a gaseous negative ion is defined as the first electron affinity. Trend of Electron Affinity Down A Group In general electron affinity electron affinity becomes becomes less negative on going down a group. The observed periodic trends in electron affinity are that electron affinity will generally become more negative moving from left to right across a period and that there is no real corresponding trend in electron affinity moving down a group in the periodic table.
The change is small and there are many exceptions. As a result when an electron is added to an atom it can cause some atoms to become highly unstable. As the principal quantum number increases the size of the orbital increases and the affinity for the electron is less.
Electron Affinity – Chemistry Tutorial. In general electron affinity increases or becomes more negative from left to right across a period. Halogens Oxygen family Carbon family Nitrogen family Metals of group 1 and 13 Metals of group 2 Electron Affinity of Halogens Ionization potential is the energy required to remove an electron from a gaseous atom.
On moving down a group the nuclear charge as well as the atomic size increase regularly. In simple words electron affinity is the tendency of an atom to accept the electron.