Question

Which element in the following pairs is likely to lose an electron more easily? (a) \(\mathrm{Be}\) or \(\mathrm{B}\) (b) \(\mathrm{Ca}\) or \(\mathrm{Co}\) (c) \(\mathrm{Sc}\) or Se

Short answer

(a) Be, (b) Ca, (c) Sc

Step-by-step solution

Compare Be and B

To determine which element between beryllium (Be) and boron (B) is more likely to lose an electron, consider their positions in the periodic table. Be is in group 2 and B is in group 13. Elements on the left side, like Be, tend to lose electrons more easily because they have lower ionization energies compared to elements further right, like B, which form covalent bonds by sharing electrons more often. Therefore, Be is likely to lose an electron more easily than B.

Compare Ca and Co

Calcium (Ca) and cobalt (Co) need to be compared in terms of ease of losing an electron. Ca is an alkaline earth metal in group 2 and Co is a transition metal in group 9. Generally, the alkali and alkaline earth metals (like Ca) lose electrons more readily because they achieve a stable noble gas configuration upon losing a relatively small number of electrons. Therefore, Ca is more likely to lose an electron than Co.

Compare Sc and Se

Scandium (Sc) is a transition metal, whereas selenium (Se) is a nonmetal located in group 16. Metals, like Sc, generally have lower ionization energies compared to nonmetals and thus lose electrons more easily. Since Sc is a transition metal and Sc tends to lose electrons to achieve a more stable configuration, Sc is likely to lose an electron more easily than Se.

Key concepts

Periodic Table

The periodic table is like a map of the elements, arranged in a way that showcases their properties and reactions. Each element has its own place, determined by its atomic number, which is the number of protons in its nucleus. This structure helps to predict how elements will behave in chemical reactions.
Moving from left to right across a period of the table, the elements become less likely to lose electrons as their ionization energy generally increases. Ionization energy is the energy required to remove an electron from an atom. Elements on the left, such as those in groups 1 and 2, have a lower ionization energy, making them more likely to lose electrons easily.
The groups, or columns, of the periodic table, show elements with similar chemical properties. For example, the elements in group 2, the alkaline earth metals, are known for their tendency to lose electrons.

Electron Configuration

Electron configuration describes how electrons are arranged around the nucleus of an atom. These electrons occupy regions called orbitals, which are grouped as s, p, d, and f based on their shapes and energy levels.
Understanding an element's electron configuration can help predict its reactivity and the types of bonds it can form. Elements with a nearly full or empty outer shell tend to react more readily. For instance, elements like beryllium (Be) and calcium (Ca) have only a few electrons in their outer shell. They tend to lose these electrons to achieve a stable state similar to the noble gases, which have full outer shells.
Having knowledge of electron configurations clarifies why elements in the same group behave similarly during chemical reactions, as they typically have the same valence electron configuration.

Alkaline Earth Metals

Alkaline earth metals, found in group 2 of the periodic table, include elements like beryllium (Be) and calcium (Ca). These metals have two electrons in their outermost shell, which they readily lose to form positive ions or cations. This process allows them to reach the stable electron configuration of a noble gas.
The overall reactivity of alkaline earth metals is less than that of alkali metals from group 1, but they are still quite reactive. These metals often react with water to form hydroxides and hydrogen gas, though not as vigorously as alkali metals. The reactivity increases as you move down the group from beryllium to barium.
These elements play vital roles in various biological and industrial applications and are essential for life processes in organisms.

Transition Metals

Transition metals are located in the central block of the periodic table, specifically groups 3 to 12. They are characterized by the presence of d orbitals in their electron configurations, which can house a varying number of electrons in their subshells.
The transition metals include elements such as scandium (Sc) and cobalt (Co). These metals are known for their ability to form colorful compounds, exhibit various oxidation states, and act as catalysts in many chemical reactions.
Compared to alkali or alkaline earth metals, transition metals generally have higher ionization energies and are less likely to lose electrons. However, their unique electron configurations allow them to form complex ions and participate in a range of bonding scenarios, making them versatile in chemical reactions.

Nonmetals

Nonmetals primarily occupy the right-hand side of the periodic table. They include elements like boron (B) and selenium (Se). Nonmetals have high ionization energies, which means they tend to hold onto their electrons tightly and frequently gain electrons to form anions or share electrons in covalent bonds.
These elements are critical in organic chemistry and biological systems. Nonmetals can exist in different states: gases (e.g., oxygen), liquids (e.g., bromine), and solids (e.g., carbon).
While they don't often lose electrons easily like metals, nonmetals play a fundamental role in forming complex molecules and compounds essential for life and various chemical processes.