Which atom will have the lowest ionization energy?
Answer (1)
Ionization energy decreases down a group.
Ionization energy increases across a period.
P is below N, so P has lower ionization energy than N.
Si is below C, so Si has lower ionization energy than C.
Si is to the left of P, so Si has lower ionization energy than P.
Therefore, Si has the lowest ionization energy: S i
Explanation
Understanding the Problem We are asked to identify the atom with the lowest ionization energy from the given options: C, P, N, and Si. Ionization energy generally decreases down a group and increases across a period in the periodic table.
Locating Atoms in the Periodic Table Let's locate the positions of C, P, N, and Si in the periodic table.
Comparing N and P Comparing N and P: P is below N in the same group (Group 15). Therefore, P has a lower ionization energy than N.
Comparing C and Si Comparing C and Si: Si is below C in the same group (Group 14). Therefore, Si has a lower ionization energy than C.
Comparing P and Si Comparing P and Si: P and Si are in the same period (Period 3). P is to the right of Si. Ionization energy generally increases from left to right across a period, so Si has a lower ionization energy than P.
Final Answer Conclusion: Among the four atoms (C, P, N, Si), Si has the lowest ionization energy.
Examples
Understanding ionization energy helps in predicting the chemical reactivity of elements. For example, elements with low ionization energies, like alkali metals, readily lose electrons to form positive ions and are highly reactive. This concept is crucial in designing batteries, understanding corrosion, and developing new materials with specific electronic properties. By knowing which elements easily lose electrons, we can better control chemical reactions and create innovative technologies.
