it lose 2 electron
This is a metal so it will lose its valence electrons.
In ionic bonding, metals tend to lose electrons to form positively charged ions, known as cations. This happens because metals have a relatively low electronegativity compared to nonmetals. The cations formed by metals then bond with negatively charged ions, known as anions, through electrostatic attraction.
Tantalum needs to lose 2 electrons to become stable. Tantalum has 73 protons, so losing 2 electrons will give it a full outer shell of 71 electrons, which is the most stable configuration for the element.
It'll have to lose two to have a stable octet.
Atoms that are less electronegative tend to lose electrons when bonding with atoms that are more electronegative. This is because less electronegative atoms have a lower attraction for electrons, making it easier for them to donate electrons to form a stable bond.
This is a metal so it will lose its valence electrons.
Metals will LOSE electrons to become stable.
In chemistry, metals are the elements that tend to lose electrons when they react to form compounds; Non-metals tend to gain electrons when they form compounds. When metals and non-metals react and exchange electrons with one another they form an ionic bond.
lose 2
Two electrons.
In ionic bonding, metals tend to lose electrons to form positively charged ions, known as cations. This happens because metals have a relatively low electronegativity compared to nonmetals. The cations formed by metals then bond with negatively charged ions, known as anions, through electrostatic attraction.
cations
to become stable
Tantalum needs to lose 2 electrons to become stable. Tantalum has 73 protons, so losing 2 electrons will give it a full outer shell of 71 electrons, which is the most stable configuration for the element.
It'll have to lose two to have a stable octet.
Atoms that are less electronegative tend to lose electrons when bonding with atoms that are more electronegative. This is because less electronegative atoms have a lower attraction for electrons, making it easier for them to donate electrons to form a stable bond.
2