Which statements completed with a to e will be true and which will be false? An atom of N compared to an atom of Li has a larger (greater) b. ionization energy

Verified step by step guidance

1. Identify the elements involved: Nitrogen (N) and Lithium (Li).
2. Understand ionization energy: It is the energy required to remove an electron from an atom in the gaseous state.
3. Recall periodic trends: Ionization energy generally increases across a period from left to right on the periodic table.
4. Locate N and Li on the periodic table: N is to the right of Li in the same period.
5. Conclude based on periodic trends: Since N is to the right of Li, N has a greater ionization energy than Li.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It is a key factor in determining an element's reactivity and is influenced by the atomic structure, including the number of protons and the distance of electrons from the nucleus. Generally, ionization energy increases across a period and decreases down a group in the periodic table.

Atomic Structure

Atomic structure refers to the arrangement of protons, neutrons, and electrons within an atom. The number of protons defines the element, while the arrangement of electrons in various energy levels affects chemical properties, including ionization energy. Understanding atomic structure is essential for comparing elements like nitrogen (N) and lithium (Li) in terms of their ionization energies.

Periodic Trends

Periodic trends are patterns observed in the periodic table that illustrate how certain properties of elements change across periods and down groups. For instance, ionization energy typically increases from left to right across a period due to increased nuclear charge and decreases down a group due to increased electron shielding. Recognizing these trends is crucial for predicting the behavior of elements like N and Li.