The successive ionization energies for a second-period element are given. What is the identity of the element? (LO 6.8)Ea1 = 1402 kJ/mol Ea2 = 2856 kJ/mol Ea3 = 4578 kJ/mol Ea4 = 7475 kJ/mol Ea5 = 9445 kJ/mol Ea6 = 53,266 kJ/mol Ea7 = 64,630 kJ/mol(a) Be(b) C(c) N (d) F

Verified step by step guidance

1. Identify the pattern in the ionization energies: Notice that the ionization energies increase as more electrons are removed. The large jump between Ea5 and Ea6 suggests that removing the sixth electron requires significantly more energy, indicating that the first five electrons are in the outer shell and the sixth electron is closer to the nucleus.
2. Compare the given ionization energies with known values: Look up the typical ionization energies for second-period elements (Li, Be, B, C, N, O, F, Ne) and compare them with the given values to find a close match.
3. Consider the electron configuration: Elements in the second period have electron configurations starting from 1s2 up to 2p6. The large jump after the fifth ionization energy suggests that the element likely has five electrons in its valence shell.
4. Analyze the options: Check the electron configurations of the given options (Be, C, N, F) and determine which one fits the pattern of having five valence electrons and a significant increase in ionization energy after the fifth electron is removed.
5. Conclude the identity: Based on the analysis, conclude which element among Be, C, N, or F has the ionization energy pattern that matches the given data.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. 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 due to increased nuclear charge and decreases down a group due to increased electron shielding.

Trends in Ionization Energies

The trends in ionization energies can provide insights into the identity of an element. As you move across a period from left to right, ionization energies typically increase due to greater effective nuclear charge. A significant jump in ionization energy, such as the one observed in the provided data, indicates the removal of an electron from a much more stable electron configuration, often suggesting the completion of an electron shell.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. Understanding the electron configuration of an element helps predict its chemical behavior and reactivity. For the second-period elements, the configurations can be used to identify stability and the likelihood of losing electrons, which is crucial when analyzing the provided ionization energies and determining the element in question.