Give the electron configuration for tin, Sn. 3) (1 point) Draw an orbital diagram (with arrows representing electrons) for technetium, Tc. 4) (1 point) Explain the trend in ionization energy that is observed in elements within the same column on the periodic table.
The Correct Answer and Explanation is:
1. Electron Configuration for Tin (Sn):
Tin has an atomic number of 50, so it has 50 electrons in its neutral state.
Electron configuration:
[Kr] 5s² 4d¹⁰ 5p²
2. Orbital Diagram for Technetium (Tc):
Technetium has an atomic number of 43, so it has 43 electrons. Its configuration is:
[Kr] 5s¹ 4d⁶
Orbital Diagram:
- 5s: ↑
- 4d: ↑ ↑ ↑ ↑ ↑ ↓
This shows one electron in the 5s orbital and six electrons filling the 4d orbitals following Hund’s rule, with five unpaired electrons and one paired.
3. Trend in Ionization Energy Within a Column (Group) of the Periodic Table:
Ionization energy is the amount of energy required to remove an electron from an atom in the gaseous state. As you move down a column in the periodic table, the ionization energy decreases. This trend occurs for several reasons:
First, atomic size increases down a group. Each successive element has an additional electron shell, so the outermost electrons are farther from the nucleus. The electrostatic attraction between the positively charged nucleus and the negatively charged valence electrons becomes weaker as the distance increases.
Second, with more inner electrons present, there is greater electron shielding. This shielding reduces the effective nuclear charge felt by the outermost electrons. As a result, these electrons are more easily removed.
Therefore, elements at the top of a group, such as fluorine or lithium, hold onto their electrons more tightly than elements lower in the group, like iodine or cesium. This is why fluorine has a higher ionization energy than iodine and lithium has a higher ionization energy than cesium.
This trend is consistent across all groups in the periodic table and plays a crucial role in predicting chemical reactivity and bonding behavior in elements.
