Textbook Question
Consider the following Lewis symbols for elements X and Y:
d. What would be the formula of a compound of X and Y?
Ch.6 Ionic and Molecular Compounds
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 6, Problem 97c
Consider the following Lewis symbols for elements X and Y:
c. What ions would be formed by X and Y?
Verified step by step guidance1
Step 1: Analyze the Lewis symbols provided in the image. The element 'M' has six valence electrons, represented by six dots around the symbol. The element 'N' has one valence electron, represented by a single dot around the symbol.
Step 2: Determine the electron configuration and stability of each element. Element 'M' needs two more electrons to complete its octet (8 valence electrons), while element 'N' needs to lose one electron to achieve a stable electron configuration.
Step 3: Predict the type of ions formed based on the electron transfer. Element 'M' will likely gain two electrons to form an anion with a charge of -2 (M²⁻), while element 'N' will lose one electron to form a cation with a charge of +1 (N⁺).
Step 4: Write the chemical symbols for the ions formed. The anion formed by 'M' is represented as M²⁻, and the cation formed by 'N' is represented as N⁺.
Step 5: Confirm the charges and stability of the ions. The transfer of electrons between 'M' and 'N' ensures that both achieve stable electron configurations, satisfying the octet rule for 'M' and the empty valence shell for 'N'.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Lewis Dot Structures
Lewis dot structures are diagrams that represent the valence electrons of an atom. Each dot corresponds to a valence electron, and the arrangement of these dots helps visualize how atoms bond and form ions. Understanding these structures is crucial for predicting the behavior of elements in chemical reactions, particularly in ion formation.
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Ion Formation
Ions are charged particles that form when atoms gain or lose electrons. Metals typically lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions. The ability to predict the ions formed by elements X and Y relies on their position in the periodic table and their respective valence electron configurations.
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Valence Electrons
Valence electrons are the outermost electrons of an atom and play a key role in chemical bonding and reactivity. The number of valence electrons determines how an element interacts with others, including its tendency to gain, lose, or share electrons. Analyzing the valence electrons of elements X and Y will help in predicting the types of ions they will form.
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Related Practice
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Consider the following Lewis symbols for elements X and Y:
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Textbook Question
Using each of the following electron arrangements, give the formulas for the cation and anion that form, the formula for the compound they form, and its name.