gain 3
Selenium needs to gain two electrons to achieve a stable electron configuration. By gaining two electrons, selenium will have a complete outer energy level (valence shell), which is the most stable configuration for an atom.
Selenium typically gains two electrons to achieve a stable electron configuration, forming the Se2- ion. Arsenic typically loses three electrons to achieve a Noble Gas electron configuration and forms the As3+ ion.
Selenium typically gains two electrons to form an ion with a charge of -2.
An atom of selenium will gain two electrons to achieve an octet because it has six valence electrons in its outer shell. By gaining these two electrons, selenium will have a total of eight electrons in its outer shell, fulfilling the octet rule.
Nonmetals tend to gain electrons when they react, rather than lose them. This is because they have fewer electrons in their outer shell and they have a higher tendency to gain electrons to achieve a stable electron configuration.
Sulfur typically gains electrons to form a stable electron configuration. It can gain up to two electrons to achieve a full valence shell of eight electrons.
Selenium may lose 2, 4 or 6 electrons and may gain 2 electrons.
Selenium typically gains two electrons to achieve a stable electron configuration, forming the Se2- ion. Arsenic typically loses three electrons to achieve a Noble Gas electron configuration and forms the As3+ ion.
Selenium typically gains two electrons to form an ion with a charge of -2.
An atom of selenium will gain two electrons to achieve an octet because it has six valence electrons in its outer shell. By gaining these two electrons, selenium will have a total of eight electrons in its outer shell, fulfilling the octet rule.
The oxidation states of selenium are: 1 to 6 and -1, -2.
Metals will LOSE electrons to become stable.
lose 2
Compounds will gain or lose electrons in order to reach a more stable state, ideally a full valence shell.
Sulfur gains 2 electrons to become stable, forming the sulfide ion (S2-). This allows sulfur to achieve a full outer electron shell, following the octet rule.
to become stable
A stable electron configuration.
Stable I think.