Since the electrons in a smaller atom are closer to the protons in the nucleus, the pull is stronger, so it tends to hold on the the electrons rather than release them during a reaction. Think of a magnet trying to lift a paper clip from far away instead of close up; that's why larger atoms tend to only loosely hold their electrons.
Yes. Ionization energy (IE) is the energy required to remove one electron from the valence shell of a gaseous atom, forming a positively charged ion (cation). Metals have low IE, and give up their valence electrons to nonmetals, which have high IE. IE increases from left to right across a period, and decreases from top to bottom down a group.
No; the phrase given characterizes high rather than low ionization.
it depends how far it is from the nucleus. the lower in the Periodic Table, the further it is from the nucleus.
false
It is ionization energy, and the bond itself is called a covalent bond.
Nonmetal atoms are the atoms that borrow electrons. The number of atoms that can be borrowed or lent are what's known as valence.
The number of electrons of both atoms and its valence number.
The valence electrons in the otermost shell of an atom are from an energy point of view the easiest to rmove or share with other atoms. The inner sheel alectrons are much more tightly bound. The important measure of this energy is the ionization energy.
In the short form: elements are striving to completely fill valence shells of electrons to reach a quantumly stable energy state. They react to take electrons away from elements willing to give up electrons or share outer shell electrons with elements they aren't strong enough to steal from.
It is ionization energy, and the bond itself is called a covalent bond.
Nonmetal atoms are the atoms that borrow electrons. The number of atoms that can be borrowed or lent are what's known as valence.
The valence electrons in the otermost shell of an atom are from an energy point of view the easiest to rmove or share with other atoms. The inner sheel alectrons are much more tightly bound. The important measure of this energy is the ionization energy.
The ionization energy increases because the energy required to remove a valence electron will increase. The atoms want to keep their valence electrons because as you move more towards the right of the Periodic Table towards the noble gases. To write an abbreviation for electron configuration, it requires a noble gas and the valence electron configuration.
valence electrons
magnesium has a 2 valence electrons. because the third electron is not a valence electron, or in the outer shell, much more energy would be needed to remove it
Valence electrons form the bonds between atoms in a molecule.
The ionization energy increases because the energy required to remove a valence electron will increase. The atoms want to keep their valence electrons because as you move more towards the right of the Periodic Table towards the noble gases. To write an abbreviation for electron configuration, it requires a noble gas and the valence electron configuration.
The number of electrons of both atoms and its valence number.
Ionization energy is the energy needed to remove 1 mole of loosely bonded electrons from one mole of atoms or ions.
The ionization energy of an element.
They share their valence electrons