Metallic Bonding Review
Flashcard
•
Chemistry
•
11th Grade
•
Practice Problem
•
Hard
Wayground Content
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15 questions
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1.
FLASHCARD QUESTION
Front
What is metallic bonding?
Back
Metallic bonding is the electrostatic attraction between positively charged metal ions and a sea of delocalized electrons that are free to move throughout the structure.
2.
FLASHCARD QUESTION
Front
What are valence electrons?
Back
Valence electrons are the electrons located in the outermost shell of an atom, which are involved in forming bonds with other atoms.
3.
FLASHCARD QUESTION
Front
What is the electron sea model?
Back
The electron sea model describes metals as a lattice of positively charged ions surrounded by a sea of free-moving electrons, which explains their conductivity and malleability.
4.
FLASHCARD QUESTION
Front
Why do metals have high melting and boiling points?
Back
Metals have high melting and boiling points due to the strong metallic bonds between the metal ions and the delocalized electrons, requiring significant energy to break.
5.
FLASHCARD QUESTION
Front
What is electrical conductivity in metals?
Back
Electrical conductivity in metals is the ability of metals to conduct electric current, primarily due to the presence of free-moving electrons.
6.
FLASHCARD QUESTION
Front
What is the significance of electronegativity in metallic bonding?
Back
Electronegativity measures an atom's ability to attract bonding electrons; in metals, lower electronegativity allows for the delocalization of electrons.
7.
FLASHCARD QUESTION
Front
How does the structure of metals contribute to their properties?
Back
The closely packed arrangement of metal atoms allows for efficient electron delocalization, contributing to properties like conductivity, malleability, and ductility.
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