Chemistry Module 5 Test Review

Questions and Answers

What are nonpolar bonds?

Have electrons that are equally shared and do not have charges on ends.

Metallic bonding is ___________.

metals only

Covalent bonding is ___________.

a metal and a nonmetal

The loose electrons are said to be ___________.

delocalized Signup and view all the answers

Describe the electric conductivity of metals.

Metal conducts electricity when the delocalized electrons allow electrons to move from one side of the metal to another transferring the electric charge. Signup and view all the answers

Describe the heat conductivity of metals.

Metal conducts heat because when the delocalized electrons are heated they move faster and transfer heat throughout the metal object. Signup and view all the answers

How are metals ductile and malleable?

Metal can be ductile and malleable because of the sea of electrons that allows them to move freely. Signup and view all the answers

What causes metals to have luster?

Metal has luster because the sea of electrons absorbs and reflects light at the same frequency. Signup and view all the answers

Why do metals have high melting and boiling points?

Metals have high melting and boiling points because of the strong connections created by the positive and negative charges from the sea of electrons. Signup and view all the answers

Describe the metallic bond 'sea of electrons' model.

The 'sea of electrons' model shows how delocalized electrons can freely move around between positively charged metal ions. Signup and view all the answers

What are polar bonds?

DO NOT have an overall positive charge. Signup and view all the answers

Ionic bonding is generally ___________.

a metal and a nonmetal Signup and view all the answers

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.

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.