Textbook Question
The following pictures represent structures of the hydrides of four second-row elements:
(1)
(2)
(3)
(4)
(a) Which compound has the highest melting point?
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Ch.22 - The Main Group Elements
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 22, Problem 22.39a
Which element in each of the following pairs has more nonmetallic character?
(a) Se or Te
Verified step by step guidance1
Identify the position of Se (Selenium) and Te (Tellurium) on the periodic table.
Recall that nonmetallic character increases as you move from left to right across a period and decreases as you move down a group.
Note that both Se and Te are in the same group (Group 16) of the periodic table.
Since Se is above Te in the same group, it is higher up on the periodic table.
Conclude that Se has more nonmetallic character than Te because nonmetallic character decreases down a group.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Nonmetallic Character
Nonmetallic character refers to the tendency of an element to exhibit properties typical of nonmetals, such as high electronegativity, poor conductivity, and the ability to gain electrons. Nonmetals are generally found on the right side of the periodic table and are characterized by their ability to form covalent bonds and anions.
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Metallic Character Example
Periodic Trends
Periodic trends are patterns observed in the properties of elements across the periodic table. Nonmetallic character increases as you move from left to right across a period and decreases as you move down a group. Understanding these trends helps predict the behavior of elements based on their position in the periodic table.
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Group and Period Positioning
Elements are organized in groups (columns) and periods (rows) in the periodic table. Selenium (Se) and tellurium (Te) are both in Group 16, but Se is higher in the group than Te. The position of an element in the periodic table influences its properties, including its nonmetallic character, which typically decreases down a group.
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Related Practice
Textbook Question
Write a balanced net ionic equation for the reaction of the amphoteric oxide Ga2O3 with:
a. Aqueous sulfuric acid
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Textbook Question
An important physiological reaction of nitric oxide (NO) is its interaction with the superoxide ion (O2–) to form the peroxynitrite ion (ONOO–).
a. Write electron-dot structures for NO, O2–, and ONOO–, and predict the O–N–O bond angle in ONOO–.
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Textbook Question
In the following pictures of binary hydrides, ivory spheres
represent H atoms or ions, and burgundy spheres represent
atoms or ions of the other element.
(1)
(2)
(3)
(4)
(a) Identify each binary hydride as ionic, covalent, or interstitial.
(b) What is the oxidation state of hydrogen in compounds (1), (2), and (3)? What is the oxidation state of the other
element?
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Textbook Question
The following pictures represent various silicate anions. Write the formula and charge of each anion.
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Textbook Question
Consider the six second- and third-row elements in groups 4A–6A of the periodic table:
Possible structures for the binary fluorides of each of these elements in its highest oxidation state are shown below.
(b) Explain why the fluorides of nitrogen and phosphorus have different molecular structures but the fluorides of carbon and silicon have the same molecular structure.
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