Textbook Question
Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Se, Te, Br, I; (b) Be, Mg, C, Si (c) Al, Si, P, S (d) Zn, Ge, Ga, As.
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Ch.8 - Basic Concepts of Chemical Bonding
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 8, Problem 39
Which of the following statements about electronegativity is or are true? i. The alkali metals are the family with the largest electronegativity values. ii. The numerical values for electronegativity have no units. iii. Electronegativity is the ability of an atom in a molecule to attract electron density toward itself.
Verified step by step guidance1
Step 1: Understand the concept of electronegativity. Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. It is a dimensionless quantity.
Step 2: Evaluate statement i. The alkali metals are located in Group 1 of the periodic table and are known for having low electronegativity values. Compare this with other groups, such as the halogens, which have higher electronegativity values.
Step 3: Evaluate statement ii. Electronegativity values are indeed dimensionless and have no units. They are typically expressed on the Pauling scale, which is a relative scale.
Step 4: Evaluate statement iii. This statement describes the concept of electronegativity accurately. It refers to the ability of an atom within a molecule to attract electron density towards itself.
Step 5: Determine which statements are true based on the evaluations: Statement ii and iii are true, while statement i is false.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons within a chemical bond. It is a relative scale, often quantified using the Pauling scale, where higher values indicate a stronger attraction for electrons. This property influences molecular polarity and reactivity, making it essential for understanding chemical bonding.
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Electronegativity Trends
Trends in Electronegativity
Electronegativity values vary across the periodic table, generally increasing from left to right across a period and decreasing from top to bottom within a group. Alkali metals, located in Group 1, have the lowest electronegativity values, while halogens, found in Group 17, exhibit the highest. Understanding these trends helps predict how different elements will interact in chemical reactions.
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Units of Electronegativity
Electronegativity is a dimensionless quantity, meaning it does not have units. This characteristic allows for the comparison of electronegativity values across different elements without the need for conversion factors. The absence of units simplifies the understanding of how different atoms will behave in terms of electron attraction in various chemical contexts.
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Related Practice
Textbook Question
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms, showing valence-shell electrons. e. How many bonding pairs of electrons are in the SiCl4 molecule?
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Textbook Question
Place the following pairs of elements in order from smallest to largest difference in electronegativity: K and F, S and O, Br and I, Ca and Se, Li and Cl.
Textbook Question
(b) How many bonding electrons are in the structure?
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Textbook Question
Using Lewis symbols and Lewis structures, diagram the formation of PF3 from P and F atoms, showing valence-shell electrons. (a) How many valence electrons does P have initially? (c) How many valence electrons surround the P in the PF3 molecule? (d) How many valence electrons surround each P in the PF3 molecule?
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Textbook Question
By referring only to the periodic table, select (d) the element in the group K, C, Zn, F that is most likely to form an ionic compound with Ba.
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