Textbook Question
Give the charge most likely to result from ionization of the following nonmetals.
(b) Sulfur
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Ch. 2 - General Chemistry Translated: Finding the Electrons
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471
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Table of contents
- Ch. 2 - General Chemistry Translated: Finding the Electrons114
- Ch. 3 - Alkanes and Cycloalkanes: Properties and Conformational Analysis109
- Ch. 4 - Acids and Bases: Electron Flow144
- Ch. 5 - Chemical Reaction Analysis: Thermodynamics and Kinetics118
- Ch. 6 - Stereoisomerism: Arrangement of Atoms in Space112
- Ch. 7 - Principles of Green (Organic) Chemistry3
- Ch. 8 - Alkenes I: Properties and Electrophilic Additions158
- Ch. 9 - Alkenes II: Oxidation and Reduction150
- Ch. 10 - Alkynes: Electrophilic Addition and Redox Reactions101
- Ch. 11 - Properties and Synthesis of Alkyl Halides: Radical Reactions108
- Ch. 12 - Substitution and Elimination: Reactions of Haloalkanes172
- Ch. 13 - Alcohols, Ethers and Related Compounds: Substitution and Elimination239
- Ch. 14 - Structural Identification I: Infrared Spectroscopy and Mass Spectrometry54
- Ch. 15 - Structural Identification II: Nuclear Magnetic Resonance Spectroscopy93
- Ch. 16 - Metals in Organic Chemistry48
- Ch. 17 - Carbonyl Addition Reactions: Aldehydes and Ketones45
- Ch. 18 - Nucleophilic Acyl Substitution I: Carboxylic Acids18
- Ch. 19 - Nucleophilic Acyl Substitution II: Carboxylic Acid Derivatives39
- Ch. 20 - Enolates: Carbonyl Addition and Substitution13
- Ch. 21 - Conjugated Systems I: Stability and Addition Reactions56
- Ch. 22 - Conjugated Systems II: Pericyclic Reactions54
- Ch. 23 - Benzene I: Aromatic Stability and Substitution Reactions64
- Ch. 24 - Benzene II: Reactions Influenced by the Aromatic Ring62
- Ch. 25 - Amines: Structure, Reactions, and Synthesis27
- Ch. 26 - Amino Acids, Proteins, and Peptide Synthesis9
- Ch. 27 - Carbohydrates, Nucleic Acids, and Lipids54
Mullins1st EditionOrganic Chemistry: A Learner Centered ApproachISBN: 9780137566471Not the one you use?Change textbook
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Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 18b
Mullins 1st EditionCh. 2 - General Chemistry Translated: Finding the ElectronsProblem 18bChapter 1, Problem 18b
Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.
(b) Mg and Br
Verified step by step guidance1
Step 1: Identify the charges of the metal and nonmetal based on their positions in the periodic table. Magnesium (Mg) is an alkaline earth metal in Group 2, so it typically forms a +2 charge (Mg²⁺). Bromine (Br) is a halogen in Group 17, so it typically forms a -1 charge (Br⁻).
Step 2: Determine the ratio of ions needed to balance the charges. Since Mg²⁺ has a +2 charge and Br⁻ has a -1 charge, two bromide ions are required to balance the charge of one magnesium ion.
Step 3: Write the formula of the ionic compound by combining the ions in the correct ratio. The formula will be MgBr₂, indicating one magnesium ion and two bromide ions.
Step 4: Label the charges on each species in the compound. Magnesium will have a +2 charge (Mg²⁺), and each bromide ion will have a -1 charge (Br⁻).
Step 5: Confirm the neutrality of the compound. The total positive charge from Mg²⁺ is +2, and the total negative charge from two Br⁻ ions is -2, resulting in a neutral compound overall.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ionic Bonding
Ionic bonding occurs when electrons are transferred from one atom to another, resulting in the formation of charged ions. Typically, this happens between metals, which lose electrons and become positively charged cations, and nonmetals, which gain electrons to become negatively charged anions. The electrostatic attraction between these oppositely charged ions leads to the formation of an ionic compound.
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Differences between ionic, polar and covalent bonds
Charge of Ions
The charge of ions is determined by the number of electrons lost or gained during the formation of the ionic bond. For example, magnesium (Mg) typically loses two electrons to form a Mg²⁺ ion, while bromine (Br) gains one electron to form a Br⁻ ion. Understanding the charges of the ions is crucial for predicting the formula of the resulting ionic compound.
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Empirical Formula
The empirical formula of an ionic compound represents the simplest whole-number ratio of the ions present in the compound. In the case of magnesium and bromine, the charges of Mg²⁺ and Br⁻ indicate that two bromide ions are needed to balance the charge of one magnesium ion, resulting in the empirical formula MgBr₂. This formula reflects the stoichiometry of the ionic compound formed.
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Related Practice
Textbook Question
Fill in the blank. Oxygen ionizes to become ― 2 instead of ― 1 because O2- is more ___________ .
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Textbook Question
(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(b) N vs. O
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Textbook Question
Show the ionic compound that you would expect to form between the given metal and nonmetal. Label the charges on each species.
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Textbook Question
Give the charge most likely to result from ionization of the following metals.
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Textbook Question
(i) Using the periodic trend, choose the more electronegative atom in each pair. For one pair, you'll need to look at the actual Pauling values. (ii) For which one? (iii) Why?
(d) B vs. Si
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