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The energy required to remove electrons from an atom is called?
Wiki User
∙ 12y ago
Ionization energy
Wiki User
∙ 12y ago
Wiki User
∙ 14y agoionization energy :D
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What energy is required to remove an electron from an atom?
The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.
Is atoms with high ionization energy allow their electrons to be easily taken?
This is false. The ionization energy is the amount of energy that is required to remove the electron. Therefore, if it requires more energy, it is harder to remove the electron.
What is the energy required to remove an electron from an atom in gaseous state called?
ionization energy
Why is it easier to lose electrons from a cesium atom than from a lithium atom?
It all has to due with ionization energy. Ionization energy is the energy required to remove an electron from an atom to make it an ion. Cesium has a lower ionization energy than Lithium, so it is easier to remove electrons, and thus lose electrons, from a Cesium atom than a Lithium atom.
What is the factor that affects how easily an electron can be removed from an atom called?
The factor that affects how easily an electron can be removed from an atom is called ionization energy. It is the energy required to remove an electron from a neutral atom in its gaseous state. A higher ionization energy indicates a stronger hold on its electrons by the atom.
What energy required to remove two valency electrons of a metallic atom?
This is the second ionization energy.
What is the energy needed to remove electrons from an atom called?
ionization potential energy. but remember the atom must be neutral .
The amount of energy required to remove one mole of electrons from one mole of sodium atoms is the?
ionization energy
Endothermic energy is?
Yes, it is the energy input required to remove 1 mol of electrons from 1 mol of an atom
What energy is required to remove an electron from an atom?
The energy needed to remove an electron from an atom (in the gaseous state) is called the IONIZATION ENERGY.
Is atoms with high ionization energy allow their electrons to be easily taken?
This is false. The ionization energy is the amount of energy that is required to remove the electron. Therefore, if it requires more energy, it is harder to remove the electron.
What is the energy required to remove an electron from an atom in gaseous state called?
ionization energy
What is the difference between work function and ionization energy?
The work function is the amount of energy required to remove an electron from an atom in a solid (ie: the Photoelectric effect). The ionization energy is the amount of energy required to remove an electron from a single "free" atom of the same material. As I understand it, atoms in a solid hold onto their electrons more loosely (because of the bonds) and free electrons hold onto their electrons more tightly.
In order for NAD plus to remove electrons from glucose or other organic molecules what must be true?
the free energy liberated when electrons are removed from the organic molecules must be greater than the energy required to give the electrons to NAD+
What is ionization energy?
Ionization energy is the amount of energy required to remove an electron from an atom or molecule, turning it into a positively charged ion. The higher the ionization energy, the more difficult it is to remove an electron. It is a key factor in determining the reactivity and chemical properties of an element.
The energy required to overcome the attraction of the nuclear charge and remove an eectron from a gaseous atom is called?
The energy required to overcome the attraction of the nuclear charge and remove an electron from a gaseous atom is called ionization energy. This energy is measured in electron volts (eV) or kilojoules per mole (kJ/mol). It represents the strength of the bond between the electron and the nucleus.
Define ionization energy of an element?
Ionization energy is the amount of energy required to remove one electron from a neutral atom in the gaseous state. It is a measure of how tightly the electron is held by the nucleus of the atom. Elements with higher ionization energies require more energy to remove an electron and are less likely to form ions.
