Unit #: 3
Subject(s): Chemistry
Grade(s): 9-12
Designer(s): Meryl Hurley, Jessie Enlow, Brandi Coley,
STAGE 1 – DESIRED RESULTS
Unit Title: Bonds: Chemical Bonds (Taken, Not Shared)
Transfer Goal(s): Students will be able to independently use their learning to…
 Understand that interactions are prevalent and predictable in everyday life.
Enduring Understandings:
Students will understand that…
 Polarities exist in all facets of nature and are caused by imbalance.
Polarities are useful in predicting behavior.
 Microscopic structure is used to predict compound formation and
properties.
 The predictable nature of compounds stems from electron
interactions.
Essential Questions:
Students will know:
 Terms: ionic, covalent, metallic, electronegativity, anion, cation,
valence electrons, delocalized, malleable, ductile, volatile,
conductivity, luster, polar, intermolecular, intramolecular,
macromolecule, network solid, bond angle, diatomic
 Electronegativity differences greater than or equal to 1.7 result in
ionic bond formation.
 Electronegativity differences less than or equal to 0.5 result in
nonpolar covalent bond formation.
 Electronegativity differences greater than 0.5 and less than 1.7 result
in polar covalent bond formation.
 Metallic bonds consist of metal cations attracted to delocalized
electrons (“sea of mobile electrons”)
 Stable bonding can be achieved by forming single, double, or triple
bonds in covalent compounds.
 Bond energy increases and bond length decreases from single, double,
to triple bonds (conceptual, no numbers).
 Molecular shapes can be described as linear, bent, trigonal planar,
trigonal pyramidal, and tetrahedral.
 Electron paired geometry can be described as linear, trigonal planar,
and tetrahedral.
Students will be able to:
 Obtain information (valence electrons, type of bond based on location
on the PTOE and electronegativity trends) from the periodic table for
the purpose of modeling compounds.
 Predict the number of electrons lost, gained or shared by atoms in
order to gain chemical stability during bonding.
 Draw Lewis structures (dot diagram) for atoms, ions, ionic
compounds, simple covalent compounds, and diatomic molecules.
 Relate Lewis dot structure to chemical formula.
 Interpret electron dot structures according to Valence Shell Electron
Pair Repulsion Theory (molecular shape, electron pair geometry)
 Use geometry and symmetry to determine molecular polarity.
 Describe electron dot structures in terms of polarity, physical
properties (melting point, boiling point, solubility, conductivity), and
bond angle distortion.
 Predict the predominant intermolecular force (IMF) based on
molecular polarity.
 Predict macroscopic properties of a substance based on its
intermolecular forces.
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Why does matter exist in different forms?
Why should solubility matter to you?
Adapted from Understanding by Design, Unit Design Planning Template (Wiggins/McTighe 2005)
Last revision 9/9/16
1
Unit #: 3
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Subject(s): Chemistry
Grade(s): 9-12
Designer(s): Meryl Hurley, Jessie Enlow, Brandi Coley,
Lone pairs of electrons create more repulsion than bonding pairs of
electrons which determines the geometry of the molecule.
Ionic compounds generally have high melting/boiling points, are
brittle, have high electrical conductivity when melted (molten) or in
aqueous solution.
Covalent compounds characteristics: low MP, low BP, poor
electrical conductivity, polar nature, etc.
Metallic bonding characteristics: high MP, high BP, high
conductivity, malleability, ductility, and luster.
Intermolecular forces are weaker than ionic, covalent or metallic
bonds.
Intermolecular forces for molecular compounds:
 H-bond as attraction between molecules when H is bonded to O,
N, or F.
 Dipole-dipole attractions between polar molecules.
 London dispersion forces (electrons of one molecule attracted to
another molecule due to temporary unequal distribution of
electrons) – i.e. liquefied inert gases.
 Relative strengths due to bond polarity differences and atomic
size. (H>dipole>London/van der Waals).
Macromolecules (polymers including PVC and nylon, proteins
including hair and DNA) and network solids (ice, graphite/diamond)
have unique properties.
Review as needed from previous grade levels:
 Melting point and boiling point concepts (8.P.1.3)
Adapted from Understanding by Design, Unit Design Planning Template (Wiggins/McTighe 2005)
Last revision 9/9/16
2
Unit #: 3
Subject(s): Chemistry
Grade(s): 9-12
Designer(s): Meryl Hurley, Jessie Enlow, Brandi Coley,
STAGE 1– STANDARDS
Essential Standards
Chm.1.2
Understand the bonding that occurs in simple compounds in
terms of bond type, strength, and properties.
Clarifying Objectives
Compare (qualitatively) the relative strengths of ionic, covalent,
Chm.1.2.1
and metallic bonds.
Infer the type of bond and chemical formula formed between
Chm.1.2.2
atoms.
Chm.1.2.3 Compare inter- and intra- particle forces.
Compare the properties of ionic, covalent, metallic, and network
Chm.1.2.5
compounds.
Adapted from Understanding by Design, Unit Design Planning Template (Wiggins/McTighe 2005)
Last revision 9/9/16
3