It will lose 2 to form Sr2+
5s orbital
It should lose two electrons
Strontium, element with atomic number 38, will lose 2 electrons to form a stable ion as it tends to lose electrons to attain a noble gas configuration.
There are no unpaired electrons in strontium.
It will lose 2 to form Sr2+
5s orbital
It should lose two electrons
Strontium, element with atomic number 38, will lose 2 electrons to form a stable ion as it tends to lose electrons to attain a noble gas configuration.
There are no unpaired electrons in strontium.
Strontium, a group 2 element, will lose 2 electrons to attain a noble gas configuration because it will achieve a stable electron configuration similar to the nearest noble gas, which is krypton. Strontium has 38 electrons in its neutral state, while krypton has 36 electrons. By losing 2 electrons, Strontium becomes Sr2+, and its electron configuration is similar to krypton.
Strontium is a metal element. There are 87 electrons in a single atom.
Strontium typically loses 2 electrons to satisfy the octet rule. Since strontium is in group 2 of the periodic table, it has 2 valence electrons. By losing these two electrons, it attains a stable electron configuration similar to a noble gas.
There are 2 electrons in the outermost shell of strontium. Strontium has an electron configuration of [Kr] 5s^2, indicating that it has two electrons in its outermost shell.
Strontium has 38 electrons.
Strontium has 2 valence electrons. It is in group 2 of the periodic table, which means it has 2 electrons in its outermost energy level.
Strontium has 38 electrons. (Protons and electrons are the same)