Calcium is in group IIA. Predict the number of electrons that calcium gains or loses to form stable ions. Explain your reasoning. Write the symbol of the ion.
Calcium is located in group IIA of the periodic table, which means it has 2 valence electrons. To achieve a stable electron configuration, calcium would prefer to lose these two valence electrons rather than gaining six more to fill its valence shell.
By losing the two valence electrons, calcium achieves a stable electron configuration similar to the noble gas argon. This results in the formation of a calcium ion with a 2+ charge, written as Ca2+.
To determine the number of electrons that calcium (Ca) gains or loses to form stable ions, we need to look at its position on the periodic table. Calcium is in group IIA, which means it belongs to the alkaline earth metals. Group IIA elements typically lose two electrons to achieve a stable electron configuration.
Calcium has an atomic number of 20, which means it has 20 protons and 20 electrons in its neutral state. To form a stable ion, calcium will lose two electrons, as group IIA elements tend to have two valence electrons. Therefore, the symbol of the ion formed by calcium will be Ca2+.
In summary:
- Calcium (Ca) is in group IIA, which suggests it will lose two electrons to form a stable ion.
- The symbol of the ion formed by calcium is Ca2+.
Calcium (Ca) is in Group IIA of the periodic table, also known as Group 2. This means that calcium has 2 valence electrons, which are the electrons in the outermost energy level of an atom.
To become stable, elements in Group IIA typically lose their valence electrons and form positive ions. In the case of calcium, it would lose its 2 valence electrons to form a stable ion.
By losing 2 electrons, calcium will achieve a full octet, which means it will have a stable electron configuration similar to the noble gas, argon (Ar). The symbol for the calcium ion with a 2+ charge, obtained by losing 2 electrons, is Ca2+.