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Chapter 7: Problem 90

Rank the following elements in order of increasing ionization energy: Mg, P, O.

Short Answer

Expert verified
The elements ranked in order of increasing ionization energy are: Mg, O, P.

Step by step solution

01

Identify The Location Of The Elements In The Periodic Table

Looking at the positions on the periodic table, Magnesium (Mg) is on the left, then comes Oxygen (O), and on the right, we find Phosphorus (P). The locations on the periodic table significantly determine the ionization energies of these elements.
02

Apply The Trend For Ionization Energy

The trend indicates that ionization energy increases across a period from left to right. Therefore, the element Magnesium (Mg) that is on the far left should have the lowest ionization energy, while Phosphorus (P) on the far right, should have the highest. Oxygen (O) falls in between and its ionization energy should therefore be higher than Magnesium (Mg) but lower than Phosphorus (P).
03

Rank The Elements According To Ionization Energy

Based on the identified positions and the trend of ionization energy, the elements can be ranked in the following order of increasing ionization energy: Magnesium (Mg) - lowest, Oxygen (O) - middle, Phosphorus (P) - highest.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Periodic Table
The periodic table is like a map for chemists. It beautifully organizes all the known elements in a way that reveals a lot about their properties. Each element is placed in a specific spot based on its atomic number, which is the number of protons in its nucleus.
For instance, elements are arranged in rows called periods and columns called groups.
The placement of an element on this table can tell you how it might behave or interact with other elements.
  • Elements in the same column (group) often have similar properties.
  • As you move from left to right across a period, properties of elements gradually change.
This organized arrangement helps us predict how elements like Magnesium (Mg), Phosphorus (P), and Oxygen (O) will compare in terms of various properties, including ionization energy.
Element Properties
Each element on the periodic table has its own set of properties that make it unique. Two of the most significant properties are atomic size and ionization energy.
  • Atomic size generally decreases from left to right across a period. This happens because additional protons in the nucleus pull electrons closer.
  • Ionization energy, the energy needed to remove an electron, often follows the opposite trend where it increases from left to right.
Understanding these properties is crucial when ranking elements like Mg, O, and P based on their ionization energy. Smaller atoms have electrons closer to the nucleus, making them harder to remove and leading to higher ionization energy.
Chemical Trends
Chemical trends help us make educated guesses about the behavior of elements. Ionization energy is a key trend seen across the periodic table.
  • It typically increases as you move across a period from left to right because atoms hold their electrons more tightly.
  • Within the same period, an element located further to the right generally has more protons, exerting a stronger pull on its electrons.
By applying this understanding to Mg, O, and P, we can rank them in increasing order of ionization energy: Magnesium, with its looser hold on electrons, is lowest, followed by Oxygen, and then Phosphorus having the highest ionization energy within these elements.

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Most popular questions from this chapter

Write the electron configuration for each of the following elements. (a) silicon (b) lithium (c) magnesium

Consider the electron configurations of the noble gases. Which valence sublevels are completely filled for each noble gas?

Explain, in terms of ionization energies, why the following ions do not form under normal conditions. (a) \(\mathrm{Ba}^{3+}\) (b) \(\mathrm{O}^{2+}\) (c) \(\mathrm{Cl}^{+}\)

For each pair, identify the larger atom or ion. (a) \(\mathrm{Mg}\) or \(\mathrm{Mg}^{2+}\) (b) \(\mathrm{P}\) or \(\mathrm{P}^{3-}\)

In the Bohr model, how does the electron move to a higher-energy orbit or to a lower-energy orbit?
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