You dont remove an electron from an atom. Its kept there by the bonds of the atom. However, you can split an atom from an atom.
The energy needed to remove an electron from a negative ion to form a neutral atom or molecule is called the electron affinity. It represents the energy change when an electron is added to a neutral atom or molecule to form a negative ion. The higher the electron affinity, the greater the energy needed to remove an electron.
The first ionization energy is the energy required to remove the outermost (most loosely held) electron from a neutral atom in its gaseous state. It is a measure of how strongly an atom holds onto its electrons, with higher ionization energies indicating a stronger hold.
The force that must be overcome to remove an electron from an atom is the electrostatic attraction between the electron and the positively charged nucleus. This force is governed by Coulomb's law and is known as the ionization energy. The amount of energy required to remove an electron depends on the specific atom and its electron configuration.
This is an electron situated on the outermost level.
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
The energy required to remove an electron from a neutral atom is the atom's ionization energy. It represents the amount of energy needed to remove the most loosely bound electron from an atom in its gaseous state.
The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.
remove either a proton or electron OR add a proton or electron...
The amount of energy required to remove an electron form an at is the ionization energy.
The energy needed to remove an electron from a negative ion to form a neutral atom or molecule is called the electron affinity. It represents the energy change when an electron is added to a neutral atom or molecule to form a negative ion. The higher the electron affinity, the greater the energy needed to remove an electron.
Ionization energy is the amount of energy required to remove an electron from a neutral atom, resulting in the formation of a positively charged ion. It is a measure of how tightly an electron is held by an atom. The higher the ionization energy, the more difficult it is to remove an electron from the atom.
Ionization energy is an expression linked to extraction of an electron.
ionization energy
The energy required to remove an electron from a gaseous atom is called the ionization energy. This energy depends on factors such as the atomic structure and the strength of the attraction between the nucleus and the electron. The higher the attraction, the higher the ionization energy needed to remove the electron.
An electron can be removed from an atom if ionization energy is supplied. Ionization energy is the energy required to remove an electron from an atom, resulting in the formation of a positively charged ion.
There is an attraction of the nucleus for electrons. This attractive force must be overcome to remove an electron. The energy to overcome this attraction and remove an electron from the atom is 'ionization energy'.
It is harder to remove an electron from a fluorine atom than a bromine atom because fluorine has a higher effective nuclear charge due to its smaller atomic size. This leads to stronger attraction between the nucleus and the outermost electron, making it more difficult to remove. Additionally, fluorine has a full valence shell with 7 electrons, making it energetically unfavorable to lose an electron.