Textbook Question
Use Coulomb's law to calculate the ionization energy in kJ/mol of an atom composed of a proton and an electron separated by 110.00 pm. What wavelength of light has sufficient energy to ionize the atom?
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Ch.9 - Periodic Properties of the Elements
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving90
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities46
- Ch.5 - Introduction to Solutions and Aqueous Solutions65
- Ch.6 - Gases100
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom51
- Ch.9 - Periodic Properties of the Elements79
- Ch.10 - Chemical Bonding I: The Lewis Model70
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory68
- Ch.12 - Liquids, Solids & Intermolecular Forces44
- Ch.13 - Solids & Modern Materials42
- Ch.14 - Solutions77
- Ch.15 - Chemical Kinetics88
- Ch.16 - Chemical Equilibrium57
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium126
- Ch.19 - Free Energy & Thermodynamics80
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry61
- Ch.22 - Organic Chemistry114
Chapter 9, Problem 114c
Consider the elements: Na, Mg, Al, Si, P. c. Which element is least metallic?
Verified step by step guidance1
Identify the elements given: Na, Mg, Al, Si, P.
Recall that metallic character decreases across a period from left to right on the periodic table.
Locate the elements on the periodic table: Na, Mg, Al, Si, and P are all in the same period (Period 3).
Understand that as you move from left to right across a period, elements become less metallic and more non-metallic.
Determine that phosphorus (P) is the furthest to the right in this list, making it the least metallic element among the given options.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Metallic Character
Metallic character refers to the tendency of an element to exhibit properties typical of metals, such as conductivity, malleability, and luster. Elements with high metallic character tend to lose electrons easily, forming positive ions. As you move across a period in the periodic table from left to right, metallic character generally decreases due to increasing nuclear charge, which attracts electrons more strongly.
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Periodic Trends
Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, ionization energy, electronegativity, and metallic character. Understanding these trends helps predict the behavior of elements, such as which will be more or less metallic based on their position in the table.
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Position in the Periodic Table
The position of an element in the periodic table is crucial for determining its properties, including metallic character. Elements are arranged by increasing atomic number, with metals located on the left and nonmetals on the right. For the elements Na, Mg, Al, Si, and P, their positions indicate that Na is the most metallic and P is the least metallic, as P is a nonmetal located further to the right.
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Related Practice
Textbook Question
Consider the elements: Na, Mg, Al, Si, P. d. Which element is diamagnetic?
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Textbook Question
Consider the elements: Na, Mg, Al, Si, P. b. Which element has the smallest atomic radius?
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Textbook Question
Consider the elements: B, C, N, O, F. d. Which element has three unpaired electrons?
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