Question

Which elements in a given period (horizontal row) of the periodic table lose electrons most easily? Why?

Short answer

In a given period of the periodic table, elements on the left side, such as alkali metals and alkaline earth metals, lose electrons most easily. This occurs due to their low ionization energy, which can be attributed to the low effective nuclear charge and greater atomic radius of these elements.

Step-by-step solution

1. Ionization Energy Definition

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous state. In other words, it is the amount of energy needed to overcome the attractive force between the positively charged nucleus and the negatively charged electrons.

2. Ionization Energy Trend in a Period

As we move across a period from left to right in the periodic table, the ionization energy generally increases. This is because as we move to the right, the number of protons in the nucleus increases, leading to a stronger force of attraction between the electrons and the nucleus. Furthermore, the addition of electrons to the same energy level does not cause a significant increase in electron shielding, so the effective nuclear charge experienced by the outer electrons increases as well. As a result, it becomes more difficult to remove an electron (higher ionization energy required) as we move to the right across a period.

3. Identifying the Elements with the Lowest Ionization Energy

Based on the trend discussed in step 2, the elements that lose electrons most easily (i.e., have the lowest ionization energy) are those found on the left side of the periodic table in a given period. These elements are the alkali metals and alkaline earth metals.

4. Reason for Lowest Ionization Energies

The main reason why the alkali metals and alkaline earth metals (elements on the left side of the periodic table) lose electrons most easily is because of their relatively low effective nuclear charge and greater atomic radius. The low effective nuclear charge means that the attraction between the electrons and the nucleus is weaker, and the greater atomic radius implies that the outer electrons are further from the nucleus, experiencing a weaker force of attraction. As a result, the ionization energy required to remove an electron is lower, making it easier for these elements to lose electrons. In conclusion, elements on the left side of the periodic table in a given period, such as alkali metals and alkaline earth metals, lose electrons most easily due to their low ionization energy. This low ionization energy can be explained by the low effective nuclear charge and greater atomic radius of these elements.