Podcast
Questions and Answers
What are nonpolar bonds?
What are nonpolar bonds?
Have electrons that are equally shared and do not have charges on ends.
Metallic bonding is ___________.
Metallic bonding is ___________.
metals only
Covalent bonding is ___________.
Covalent bonding is ___________.
a metal and a nonmetal
The loose electrons are said to be ___________.
The loose electrons are said to be ___________.
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Describe the electric conductivity of metals.
Describe the electric conductivity of metals.
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Describe the heat conductivity of metals.
Describe the heat conductivity of metals.
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How are metals ductile and malleable?
How are metals ductile and malleable?
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What causes metals to have luster?
What causes metals to have luster?
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Why do metals have high melting and boiling points?
Why do metals have high melting and boiling points?
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Describe the metallic bond 'sea of electrons' model.
Describe the metallic bond 'sea of electrons' model.
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What are polar bonds?
What are polar bonds?
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Ionic bonding is generally ___________.
Ionic bonding is generally ___________.
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Study Notes
Nonpolar Bonds
- Electrons in nonpolar bonds are shared equally between atoms.
- These bonds do not exhibit charges at their ends.
Metallic Bonding
- Involves only metals, characterized by the presence of delocalized electrons.
Covalent Bonding
- Occurs between a metal and a nonmetal, leading to the formation of molecules.
Delocalized Electrons
- Refers to electrons that are not tightly bound and can move freely, contributing to metal properties.
Properties of Metals
- Electric Conductivity: Metals conduct electricity due to delocalized electrons allowing movement of charge. Unlike wood and rubber, metals facilitate charge flow.
- Heat Conductivity: Metals transfer heat as delocalized electrons gain energy and move faster, distributing warmth throughout the material.
- Ductility and Malleability: Metals can be stretched or shaped because delocalized electrons allow movement with positive metal ions, maintaining structural stability.
- Luster: The shiny appearance of metals results from delocalized electrons interacting with light, absorbing and reflecting it at similar frequencies.
- High Melting and Boiling Points: Metals have elevated melting and boiling points due to the strong attraction between positive ions and delocalized electrons.
Sea of Electrons Model
- Describes a framework where delocalized electrons move among positively charged metal ions, not being tightly held in place.
- Visual representation includes positive ions surrounded by a "sea" of free-moving electrons, emphasizing their mobility.
Polar Bonds
- Polar bonds do not bear an overall positive charge, indicating a difference in electronegativity between the bonded atoms.
Ionic Bonding
- Typically occurs between a metal and nonmetal, resulting in the transfer of electrons and formation of ions.
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Description
Prepare for your Chemistry Module 5 test with these flashcards covering key concepts such as nonpolar bonds, metallic and covalent bonding. Each card provides definitions and important terms essential for understanding chemical bonding. This review is perfect for reinforcing your knowledge before the exam.
