Which of the following shows the correct relationship between the first ionization energies of the given elements?

Question

BlackTom AI · Accepted Answer

Question restatement: Which of the following shows the correct relationship between the first ionization energies of the given elements? Option-by-option analysis: Option 1: Ne > F - This statement says the first ionization energy of Neon is greater than that of Fluorine. Across a period, ionization energy generally increases from left to right, and Neon (a noble gas with a complete octet) indeed has a higher first ionization energy than Fluorine. The actual values are roughly Ne ≈ 2080 kJ/mol and F ≈ 1680 kJ/mol, so Ne > F is correct based on periodic trends and empirical data. Option 2: Li > Be - Here we would be claiming Lithium has a higher first ionization energy than Beryllium. In the same period (period 2), Be is to the right of Li, and ionization energy increases across a period. Therefore Be should have a higher IE than Li. The correct relation is Li < Be, so this statement is false. Option 3: Ga > Ge - This compares Gallium (period 4, group 13) and Germanium (period 4, group 14). Within the same period, Ge, being to the right of Ga, generally has a higher ionization energy. In fact, Ga has IE ≈ 578 kJ/mol, while Ge has IE ≈ 762 kJ/mol, making Ga < Ge. The claim Ga > Ge is incorrect. Option 4: Xe > Ne - This option suggests Xenon has a higher first ionization energy than Neon. In fact, Neon has a higher IE because it is a noble gas with a complete valence shell and a relatively high effective nuclear charge compared to Xe, but Xe is larger and more easily ionized than Ne for the first electron due to shielding and energy level considerations. Empirically, Xe’s IE is about 1170 kJ/mol, whereas Ne’s is about 2080 kJ/mol, so Xe < Ne. Therefore this statement is false. Option 5: I am unsure and need to study this concept to prepare for the exam - This is not a statement about the actual ionization energies; it simply expresses uncertainty. While it’s okay to seek study help, it does not reflect a true comparison between the given elements. It’s not a valid evaluation of the relationship. Key takeaway for the correct option: The correct relationship is Ne > F because Neon’s first ionization energy is higher than Fluorine’s, in line with periodic trends and actual data. The other options fail to match known IE patterns across periods and within groups, or rely on incorrect assumptions about trends.

CHEM 1210 AU2025 (15738) CHEM 1210 Practice Exam #4 v2 (Ch 7.1–7.4, 8, 9.1–9.6)- Requires Respondus LockDown Browser

Which of the following shows the correct relationship between the first ionization energies of the given elements?

View Explanation

Log in for full answers

Similar Questions

Given the following elements and three values of possible first ionization energies: Si, Na, Cl and 496, 1251, and 786 kJ·mol–1 Match the atoms with their ionization energies.

Nonmetals rarely lose electrons in chemical reactions because

For the elements Be, B, N and O, the order of increasing ionization energies are:

Which of the following equations represents the second ionization energy of calcium? 04A

Identify the figure showing the successive ionization energies of Mg.

For the elements Be, B, and N, the first ionization energy increases in the order:

Select the response which presents the three elements below in order of increasing first ionisation potential (IE1).

Select the response which presents the three elements below in order of increasing first ionisation potential (IE1).

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler