Alkaline Earths will most easily lose an electron. This is because the have a smaller alkali radii than alkali metals causing them to not be as tightly bound to the nucleus. This makes the more readily lose their electrons.
Barium would lose an electron more readily, because its outer electrons are farther away from the nucleus than those in magnesium, and thus are not held as tightly. =] Hopefully this helps you out alot.
The oxidation state of an element is determined by the number of electrons the element needs to lose or gain to have a full valence electron shell.
A neutral sodium must lose one electron in order for the resulting sodium ion to have the same electron configuration as an atom of the element neon.
The Alkali Metals, which are the elements in Group 1 of the periodic table, each have one lone electron in their valence shell. And each of these elements wants to get rid of that single electron. These metals, which include lithium, sodium, potassium, rubidium, caesium and francium, are the most likely to lose electrons.
It is an alkali metal (Group 1 element). So, it needs to lose one electron in order to form a full valence shell (the one beneath it). Full valence shells are more stable states.
Na, sodium, should have the lowest first ionization energy of those four elements.
Valence electron describes type of element. It either lose or gain electron.
Na i believe since it has only one in its outer shell
As we go down the group, nuclear charge deceases and atomic radii increases. So the element can easily lose electron and hence react.
They use a force called bonding where they either gain or lose an electron.
Metals are the elements that usually lose electrons in their chemical reactions. This is because they have few electrons in their outermost shells which are easily lost.
The elements in the halogen family are in group 7 and thus have 7 valence electrons. They are very reactive because the want an additional electron to complete the octet. They can get this additional electron by reacting with another element willing to donate that electron. A perfect example is an element from group 1 or 2 (alkali or alkali earth) which wants to donate an electron.
Barium would lose an electron more readily, because its outer electrons are farther away from the nucleus than those in magnesium, and thus are not held as tightly. =] Hopefully this helps you out alot.
The oxidation state of an element is determined by the number of electrons the element needs to lose or gain to have a full valence electron shell.
Francium has the lowest electronegativity and fluorine the highest.
The metal tends to lose the electron because it has a higher electron affinity, and the nonmetal tends to gain the electron because it has a higher electronegativity. This has to do with the placement of the element on the periodic table. The further to the right you go, the more the element wants to gain electrons in an ionic compound.
Hydrogen has 1 electron. It can easily gain or lose electron to form metal or non metal