Textbook Question
Determine whether or not each element is a main-group element. a. tellurium b. potassium c. vanadium d. manganese
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Ch.2 - Atoms & Elements
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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Table of contents
- Ch.1 - Matter, Measurement & Problem Solving93
- Ch.2 - Atoms & Elements94
- Ch.3 - Molecules and Compounds103
- Ch.4 - Chemical Reactions and Chemical Quantities44
- Ch.5 - Introduction to Solutions and Aqueous Solutions69
- Ch.6 - Gases97
- Ch.7 - Thermochemistry85
- Ch.8 - The Quantum-Mechanical Model of the Atom48
- Ch.9 - Periodic Properties of the Elements73
- Ch.10 - Chemical Bonding I: The Lewis Model76
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory70
- Ch.12 - Liquids, Solids & Intermolecular Forces41
- Ch.13 - Solids & Modern Materials40
- Ch.14 - Solutions76
- Ch.15 - Chemical Kinetics90
- Ch.16 - Chemical Equilibrium56
- Ch.17 - Acids and Bases121
- Ch.18 - Aqueous Ionic Equilibrium127
- Ch.19 - Free Energy & Thermodynamics78
- Ch.20 - Electrochemistry87
- Ch.21 - Radioactivity & Nuclear Chemistry60
- Ch.22 - Organic Chemistry115
Chapter 2, Problem 70
Which pair of elements do you expect to be most similar? Why? a. nitrogen and oxygen b. titanium and gallium c. lithium and sodium d. germanium and arsenic e. argon and bromine
Verified step by step guidance1
1. The similarity between elements is determined by their position in the periodic table. Elements in the same group (vertical column) of the periodic table have similar properties because they have the same number of valence electrons. These are the electrons in the outermost shell of an atom that are involved in chemical reactions.
2. Nitrogen and oxygen are in the same period (horizontal row) but not in the same group. They have different numbers of valence electrons, so they have different chemical properties.
3. Titanium and gallium are in different periods and different groups. They have different numbers of valence electrons and different chemical properties.
4. Lithium and sodium are in the same group (Group 1: Alkali metals). They have the same number of valence electrons (1 electron in the outermost shell), so they have similar chemical properties.
5. Germanium and arsenic are in the same period but not in the same group. They have different numbers of valence electrons and different chemical properties.
6. Argon and bromine are in the same period but not in the same group. They have different numbers of valence electrons and different chemical properties.
7. Therefore, based on the periodic table and the concept of valence electrons, the pair of elements that are most similar are lithium and sodium because they are in the same group and have the same number of valence electrons.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Periodic Trends
Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. These trends include atomic radius, electronegativity, ionization energy, and reactivity. Understanding these trends helps in predicting the behavior and similarities between elements based on their positions in the periodic table.
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00:38
Periodic Trends
Group vs. Period Similarities
Elements in the same group (column) of the periodic table share similar chemical properties due to having the same number of valence electrons. This similarity often leads to comparable reactivity and bonding characteristics. In contrast, elements in the same period (row) may have different properties as they have different valence electron configurations.
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05:33Periodic Table: Group Names
Metallic vs. Nonmetallic Character
The metallic and nonmetallic character of elements influences their properties and reactivity. Metals, typically found on the left side of the periodic table, are good conductors of heat and electricity, while nonmetals, located on the right, are generally poor conductors and have higher electronegativities. Understanding this distinction is crucial for predicting how elements will interact with one another.
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Related Practice
Textbook Question
The atomic mass of fluorine is 18.998 amu, and its mass spectrum shows a large peak at this mass. The atomic mass of chlorine is 35.45 amu, yet the mass spectrum of chlorine does not show a peak at this mass. Explain the difference.
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Textbook Question
Write the symbol for each element and classify it as a metal, nonmetal, or metalloid. a. gold b. fluorine c. sodium d. tin e. argon
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Textbook Question
Fill in the blanks to complete the table.
Symbol Ion Formed Number of Electrons in Ion Number of Protons in Ion
Cl ______ ______ 17
Te ______ 54 ______
Br Br– ______ ______
______ Sr2+ ______ 38
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