0
The amount of energy required to remove an electron increases from left to right. This means that the atoms are able to hold on to their valence electrons more and more tightly. Thus, it gets harder to remove an electron as the atomic number increases.
Going down a group, the element doesn't change much. However, the size of the atom increases greatly, and because of this, so does the distance between the nucleus and the valence electrons. That decreases the magnitude of the force of attraction between the nucleus and the outermost electrons. Thus, IE decreases going down a group from top to bottom.
http://forums.studentdoctor.net/showpost.php?p=2720248&postcount=3
Wiki User
∙ 15y ago
Wiki User
∙ 11y agoNoble gases have completely filled orbitals / energy levels. They generally have 8 valence electrons (helium has only 2) and have stable electronic configuration. The electrons are not lost easily and hence a large amount of energy is required (high ionization energy) to remove an electron.
Wiki User
∙ 13y agoThe farther out from the nucleus the easier it is to pull outer electrons. Shielding has something to do with it, but that is college chemistry. Ask your teacher about electron shielding.
Wiki User
∙ 10y agoThat's ionization energy. The trend is: left to right across a period, it increases; and top to bottom down a group, it decreases.
Add your answer:
Earn +20 pts
Define ionization energy of an element?
The energy required to remove an electron~ Apex! :D
The energy required to remove an electron from a neutral atom is the atom's?
Ionization Energy or electron energy
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.
What is the energy required to overcome the attraction of protons in the nucleus and remove an electron from a gaseous atom?
The electron
What is the energy required to remove an electron from an atom in gaseous state called?
ionization energy
Define ionization energy of an element?
The energy required to remove an electron~ Apex! :D
The energy required to remove an electron from a neutral atom is the atom's?
Ionization Energy or electron energy
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.
What is first ionization enegy?
Ionization energy is more commonly used to remove the topmost electron in the atom very important information if you are getting ready for a test.
What does the first ionization energy represent?
The energy required to remove an electron from an atom
What do you call the energy involved when an atom loses an electron?
The amount of energy required to remove an electron form an at is the ionization energy.
What is the energy required to overcome the attraction of protons in the nucleus and remove an electron from a gaseous atom?
The electron
What best describes what the ionization of an element is?
The energy required to remove an electron
What is the energy required to remove an electron from an atom in gaseous state called?
ionization energy
What is the energy required to remove an electron from an atom in the gaseous?
The ionization energy, expressed in kJ/mol.
What do we mean by the first second third ionization energies for a particular atom?
First ionization energy is the energy required to remove the first outermost electron from an atom. The second ionization energy is the energy required to remove the next available electron, and is greater than the first IE. The third IE is that energy needed to remove the third electron, and is greater the the second IE.
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.
