Choose the element with the higher first ionization energy from each pair. a. Ge or Br b. P or In c. S or Te d. As or Br

Verified step by step guidance

1. Understand that the first ionization energy is the energy required to remove the outermost electron from a neutral atom in the gaseous state.
2. Recall that ionization energy generally increases across a period (from left to right) on the periodic table due to increasing nuclear charge and decreases down a group (from top to bottom) due to increasing atomic size and electron shielding.
3. For each pair, identify their positions on the periodic table: a. Ge (Germanium) and Br (Bromine) are in the same period, with Br to the right of Ge. b. P (Phosphorus) is above In (Indium) in the same group. c. S (Sulfur) is above Te (Tellurium) in the same group. d. As (Arsenic) and Br (Bromine) are in the same period, with Br to the right of As.
4. Apply the periodic trend: a. Since Br is to the right of Ge in the same period, Br has a higher first ionization energy. b. Since P is above In in the same group, P has a higher first ionization energy. c. Since S is above Te in the same group, S has a higher first ionization energy. d. Since Br is to the right of As in the same period, Br has a higher first ionization energy.
5. Conclude that the elements with higher first ionization energies are: a. Br, b. P, c. S, d. Br.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key indicator of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period in the periodic table due to increasing nuclear charge and decreases down a group due to increased distance from the nucleus and electron shielding.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For ionization energy, elements on the right side of the table (like halogens) typically have higher ionization energies than those on the left (like alkali metals). Understanding these trends helps in predicting which element in a pair will have a higher ionization energy.

Comparison of Elements

When comparing elements for their ionization energies, it is essential to consider their positions in the periodic table. Elements in the same group have similar properties, but the one higher up usually has a higher ionization energy due to less electron shielding. In contrast, elements in the same period will show increasing ionization energy from left to right, allowing for effective comparisons between pairs.