Type:

E-book

Description:

This folder contains resources about chemical bonds.

This unit is part of the Chemistry collection, an open source California digital textbook plus supplementary resources.

Subjects:

  • Science > General
  • Science > Chemistry

Education Levels:

  • Grade 9
  • Grade 10
  • Grade 11
  • Grade 12

Keywords:

Language:

English

Access Privileges:

Public - Available to anyone

License Deed:

Creative Commons Attribution 3.0
Update Standards?

SCI.9-12.CH.2.a: Science

Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.

SCI.9-12.CH.2.b: Science

Students know chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent.

SCI.9-12.CH.2.c: Science

Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction.

SCI.9-12.CH.2.d: Science

Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form.

SCI.9-12.CH.2.e: Science

Students know how to draw Lewis dot structures.

SCI.9-12.CH.2.f: Science

Students know how to predict the shape of simple molecules and their polarity from Lewis dot structures.

SCI.9-12.CH.2.g: Science

Students know how electronegativity and ionization energy relate to bond formation.

SCI.9-12.CH.2.h: Science

Students know how to identify solids and liquids held together by Van der Waals forces or hydrogen bonding and relate these forces to volatility and boiling/melting point temperatures.

SCI.10-12.7.B: Science

write the chemical formulas of common polyatomic ions, ionic compounds containing main group or transition metals, covalent compounds, acids, and bases;

SCI.10-12.7.C: Science

construct electron dot formulas to illustrate ionic and covalent bonds;

SCI.10-12.7.D: Science

describe the nature of metallic bonding and apply the theory to explain metallic properties such as thermal and electrical conductivity, malleability, and ductility; and
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