---
title: "The table below shows the first five ionization energies in \\(\\text{kJ/mol}\\) for three unknown representative elements, \\(\\text{X}\\), \\(\\text{Y}\\), and \\(\\text{Z}\\), all located in Period 3 of the periodic table.  | Element | \\(IE_1\\) (\\(\\text{kJ/mol}\\)) | \\(IE_2\\) (\\(\\text{kJ/mol}\\)) | \\(IE_3\\) (\\(\\text{kJ/mol}\\)) | \\(IE_4\\) (\\(\\text{kJ/mol}\\)) | \\(IE_5\\) (\\(\\text{kJ/mol}\\)) | | :— | :— | :— | :— | :— | :— | | \\(\\text{X}\\) | \\(496\\) | \\(4562\\) | \\(6910\\) | \\(9543\\) | \\(13354\\) | | \\(\\text{Y}\\) | \\(738\\) | \\(1451\\) | \\(7733\\) | \\(10543\\) | \\(13630\\) | | \\(\\text{Z}\\) | \\(578\\) | \\(1817\\) | \\(2745\\) | \\(11577\\) | \\(14842\\) |  Based on the data in the table, which of the following is the most likely formula and justification for the stable binary ionic compound formed between element \\(\\text{Y}\\) and nitrogen, \\(\\text{N}\\)?"
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url: "https://nerd-notes.com/ubq/119592/"
date_modified: "2026-08-21T06:54:07+00:00"
---

# The table below shows the first five ionization energies in \(\text{kJ/mol}\) for three unknown representative elements, \(\text{X}\), \(\text{Y}\), and \(\text{Z}\), all located in Period 3 of the periodic table.

| Element | \(IE_1\) (\(\text{kJ/mol}\)) | \(IE_2\) (\(\text{kJ/mol}\)) | \(IE_3\) (\(\text{kJ/mol}\)) | \(IE_4\) (\(\text{kJ/mol}\)) | \(IE_5\) (\(\text{kJ/mol}\)) |
| :— | :— | :— | :— | :— | :— |
| \(\text{X}\) | \(496\) | \(4562\) | \(6910\) | \(9543\) | \(13354\) |
| \(\text{Y}\) | \(738\) | \(1451\) | \(7733\) | \(10543\) | \(13630\) |
| \(\text{Z}\) | \(578\) | \(1817\) | \(2745\) | \(11577\) | \(14842\) |

Based on the data in the table, which of the following is the most likely formula and justification for the stable binary ionic compound formed between element \(\text{Y}\) and nitrogen, \(\text{N}\)?

The table below shows the first five ionization energies in \(\text{kJ/mol}\) for three unknown representative elements, \(\text{X}\), \(\text{Y}\), and \(\text{Z}\), all located in Period 3 of the periodic table.

| Element | \(IE_1\) (\(\text{kJ/mol}\)) | \(IE_2\) (\(\text{kJ/mol}\)) | \(IE_3\) (\(\text{kJ/mol}\)) | \(IE_4\) (\(\text{kJ/mol}\)) | \(IE_5\) (\(\text{kJ/mol}\)) |
| :--- | :--- | :--- | :--- | :--- | :--- |
| \(\text{X}\) | \(496\) | \(4562\) | \(6910\) | \(9543\) | \(13354\) |
| \(\text{Y}\) | \(738\) | \(1451\) | \(7733\) | \(10543\) | \(13630\) |
| \(\text{Z}\) | \(578\) | \(1817\) | \(2745\) | \(11577\) | \(14842\) |

Based on the data in the table, which of the following is the most likely formula and justification for the stable binary ionic compound formed between element \(\text{Y}\) and nitrogen, \(\text{N}\)?

- **A.** \(\text{YN}\), because \(\text{Y}\) loses two valence electrons to form a \(\text{Y}^{2+}\) ion and combines in a \(1:1\) ratio with a nitrogen atom that gains two electrons.
- **B.** \(\text{Y}_2\text{N}_3\), because the large increase between \(IE_2\) and \(IE_3\) indicates that \(\text{Y}\) forms a \(\text{Y}^{3+}\) ion, which combines with \(\text{N}^{2-}\) ions to form an electrically neutral compound.
- **C.** \(\text{Y}_3\text{N}_2\), because the large increase between \(IE_2\) and \(IE_3\) indicates that \(\text{Y}\) has two valence electrons and forms a \(\text{Y}^{2+}\) ion, which combines with \(\text{N}^{3-}\) ions to form an electrically neutral compound.
- **D.** \(\text{Y}_3\text{N}\), because the large increase between \(IE_1\) and \(IE_2\) indicates that \(\text{Y}\) has one valence electron and forms a \(\text{Y}^+\) ion, which combines with \(\text{N}^{3-}\) ions to form an electrically neutral compound.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119592/*