When they attempt to stabilize themselves. For atoms to be stable they have to have a full outer shell of electrons and so they gain electrons to fill the current outer shell, or lose electrons in order for next shell in (which is full) to be the outer shell.
Atoms gain electrons when the electrons in the last orbit are 5, 6 or 7.
Atoms which have 4 electrons in their last orbit give or take electrons based on the element or compound they are reacting with
The Lewis Theory used observations from chemists and physicists to form a theory about chemical bonding.
The Octet Rule is a chemical rule that atoms of main-group elements tend to combine in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas.
An atom's electrons tend to be stable so it will gain or lose electrons. To be stable, it will have to have exactly 8 or 18 electrons in its top energy levels. Energy levels increase as you go down row by row of the Periodic Table.
Atoms of one element will always have the same number of protons and will form a neutral charge by the number by balancing protons with electrons.
Atoms gain or lose electrons to attain a stable state on their electron shell. When they do this they form ionic compounds with charges.
In order to achieve a stable, Noble Gas (Group VIII), electronic configuration.
Remember LEO GER
Lose electrons, Oxidized
Gain electrons, Reduced
An Ion is an atom that gains or loses an electron.
It depends. Metals tend to lose electrons and nonmetals tend to gain electrons.
ions
The atoms become electrically neutra
No! Atoms with more than 4 electrons gain electrons during bonding. Atoms with less than 4 electrons tend to lose electrons during bonding. Hope this helps!
A completely filled shell of electrons has 8 electrons.
Alkali metals tend to lose electrons in chemical reactions.
Group 2A elements tend to GAIN electrons!!
In the simplest sense, an atom can either gain or lose an electron to become more stable. Very electronegative atoms like fluorine and oxygen tend to gain electrons, whereas atoms that are less electronegative like the alkali metals tend to lose electrons. In these cases, an electron is sent to a lower energy state, thus making the atom more stable.
Atoms with eight valence electrons usually do not gain or lose electrons. Atoms with one, two, or three valence electrons will lose electrons.
se and sometimes gain electrons. Atoms with eight valence electrons do not easily lose electrons
Choices: a) eject, retain B) lose, gain c) retain,gain d) gain, lose e) lose, retain
No! Atoms with more than 4 electrons gain electrons during bonding. Atoms with less than 4 electrons tend to lose electrons during bonding. Hope this helps!
A completely filled shell of electrons has 8 electrons.
Metals usually lose electrons, this is why many charges are positive.
se and sometimes gain electrons. Atoms with eight valence electrons do not easily lose electrons
Metals lose electrons.
Since platinum is a metal it will tend to lose electrons.
Atoms lose or gain or share electrons and tend to attain noble gas configuration
Atoms that tend to gain electrons are located on the far left side of the periodic table.
The most stable electron configuration for any atom is to have a complete outer shell. For the smallest atoms, that can be no electrons at all (for H+) since no shell is equivalent to a complete shell, or just two electrons in the outer shell, such as for a helium atom, but for most elements that means 8 electrons in the outer shell. We then have atoms which have five or more electrons in their outer shell and therefore need three or less to complete their shell, and they tend to gain electrons because it is easier to gain three than it is to lose five. Similarly, there are atoms with three or fewer electrons in their outer shell, and they tend to lose electrons because it is easier to lose three than it is to gain five. In the middle we have an atom such as carbon, with four electrons it its outer shell; it can gain or lose electrons with equal ease.