an ion.
Both. Atoms on the left hand side of the Periodic Table tend to lose electrons so their outer electron shell is empty and thus the one below it is full and thus stable. These form cations. The reverse is true for atoms on the right hand side of the periodic table. They gain electrons to get a full outer energy level and become stable. These are called anions.
Well, every atom wants to become stable, and the only way for this to be accomplished is by either gaining or losing electrons. And yes i do mean losing electrons. The atoms want 8 valence electrons to be stable, and they with either gain electrons or lose them to resemble a noble gas. For example, Oxygen, which is a group 16 element, is closest to the noble gas Ne (neon) and will therefore gain two valence electrons to RESEMBLE neon. Since each electron has a charge of -1, the stable form of Oxygen is O-2. However, Oxygen is a diatomic element and is therefore O sub 2. Carbon and any group 14 element can either gain or lose four electrons. These are stable Ions, however, in some conditions there can be more than one different ion, and a percentage of it which can be found naturally. You can then use this to average them both and find the average ion for an element.
Yes - a positively charge ion.
In a metallic bond, the electrons which make up the 'sea' of delocalised electrons are all of those from the outermost shell from the atoms. The other shells stay unaltered.
Oxygen has 6 valence electrons. A person can determine the number of valence electrons by looking at the periodic table. since oxygen is in the 6th column form the left, it has 6 valence electrons.
valence electrons, they are the ones responsible for bonding with other atoms.
An electric current involves the flow of electrically charged particles - usually electrons, but it may also be other particles, with a positive or negative charge. Now, to say that an electric current "is" a flow of charged particles is an oversimplification - the situation is a bit more complicated.
It is very stable #APEX :P
Valence electrons form the bonds between atoms in a molecule.
Since the valence electrons are the outermost electrons of atoms, they have the highest opportunity to overlap with other orbitals in the valence shells of other atoms. Therefore, they influence the most in forming bonds.
Since the valence electrons are the outermost electrons of atoms, they have the highest opportunity to overlap with other orbitals in the valence shells of other atoms. Therefore, they influence the most in forming bonds.
They are shared by the valence shells of the atoms involved in the bond.
An atom stripped of its valence electrons, so that its remaining electrons are all in closed shells.
They have filled valence shells. Atoms undergo chemical bonding in order to have filled valence shells by sharing electrons or transferring electrons. Because the noble gases already have filled valence shells, they have no need to react with other elements.
Around the nucleus of atoms circulate electrons. They are in shells. The electrons in empty shells are called valence shells. Now, if a shell isn't full, only partly, an atom will want to fill it. Hence, it will connect with an atom with too many electrons. Nature in general abhors energy and will always try to minimize it. It is energetically favorable for atoms with too many electrons to bond with atoms with too few in the valence orbit/shell. Sometimes it is more energetically favorable to share electrons. This type of bond is a covalent bond.
valence electrons
Positively charged cations are formed when atoms lose the valence electrons.
Yes. Only the valence shell will interact with other atoms. This is how different elements are different from eachother. The electrons under the valence shell are never touched. Yes. Only the valence shell will interact with other atoms. This is how different elements are different from eachother. The electrons under the valence shell are never touched.
It is a matter of how full an atom's outer or valence shell of electrons is. For most atoms, the most stable setup is one with a full shell of 8 valence electrons, and an atom will gain or lose electrons to achieve this. For atoms with close to 8 valence electrons, such a chlorine (7 valence electrons, it is generally easier to gain electrons and thus become negatively charged. For atoms with few valence electrons, such as sodium (1 valence electron), it is easier to lose electrons and go down to the next lowest shell, which is already full.
The atoms of the molecule effectively achieve a noble gas configuration by sharing valence electrons.