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Chemical Bond Webquest

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Elizabeth Poppe

on 1 November 2012

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Transcript of Chemical Bond Webquest

By Elizabeth Poppe, Spencer Morris,
and Suhana Posani Chemical Bonding Types of Bonds Forces Holding Bonds Together How do these all compare? Bonds and
valence configurations Strength of IMFs and physical changes Intermolecular Forces and Their Strengths The forces that hold covalent bonds together are the sharing of electrons between atoms, which hold the atoms in the bond together.
The forces which hold ionic bonds together are the transferring of electrons between a metal and nonmetal where the electrons from the metal are transferred to the nonmetal creating two opposite ions which attract each other Ionic Valence configurations & octets
atoms which have less than a full valence shell of 8 electrons will form bonds with other atoms to form a full octet (8 electrons) in their valence shell
having a full octet gives atoms more stability The physical changes that affect a molecule are dependent on the strength of the IMF that molecule possesses. The molecules with the strongest IMFs take the most energy to change their physical characteristics. Ionic forces are the strongest so they have the highest boiling, melting, condensation point etc. because the forces in the molecules are the strongest (compared to hydrogen bonding, dipole-dipole, and Van Der Waals) and therefore hardest to break.
It is important to note that when phase changes occur, they only affect the IMFs, not he bonds between the atoms themselves. The intermolecular forces will be ranked from strongest to weakest:

1. Ionic
2. Hydrogen Bonding
3. Dipole-Dipole
4. Van der Waals Ionic Bonds between metal and a non-metal
electrons are transfered
electronegativity > 1.7
high melting points
crystal lattice structure
have a permanent charge NaCl Covalent Bonds electrons are shared
structure= true molecules
liquids or solids
low melting points
are not usually soluble
not conductive
tend to have odors
are polar or non-polar
have partial charges
electronegativity of 0-1.7 Metallic Bonding between two metals
extremely high melting point
electrons are delocalized/part of an electron sea
not soluble
conductive in any state
lustrous Covalent Metallic have a permanent charge associated with every bond
have the strongest IMF
the metal loses electrons and the non-metal gains the electron
has melting points between Covalent and Metallic Bonds
electronegativity <1.7 The End Works Cited Bond Types: Examples and Classification Ionic compounds: An example of an ionic compound is a NaCl (referred to commonly as salt).
Covalent compounds: An example of a covalent compound is CO2 (Carbon dioxide)
Metallic compounds: An example of a metallic compound is steel

To differentiate between Ionic compounds, covalent compounds, and metallic compounds, one must look at how the compounds are formed. Ionic compounds are formed between a non-metal and a metal. Covalent compounds are formed between two non-metals or more. Metallic compounds are formed between two metallic compounds or more. Another way consists of looking at their structure. Ionic compounds form crystal lattices, covalent compounds form true molecules, and metallic compounds consist of electron seas. Cscl. N.d. Photograph. Chemistry. Web. 30 Oct. 2012.
Aspirin. N.d. Photograph. Chemistry. Web. 30 Oct. 2012.
Electron-sea-model. N.d. Photograph. Tutorvista. Tutorvista. Web. 30 Oct. 2012.
Figure 4. Digital image. Wustl Chemisty. N.p., n.d. Web. 31 Oct. 2012.
Covalent Bonding. Digital image. WebChem. N.p., n.d. Web. 31 Oct. 2012. have partial charges
have the weakest IMFs
share electrons between 2 non-metals to form a bond
have the lowest melting points
can be polar or non-polar depending on electronegativity
polar bonds have a electonegativity of >0.7 and <1.7
non-polar bonds have an electronegativity of <0.7 have the highest melting points
these bonds are formed between 2 metals
strongest IMFs because of their high melting points Intermolecular Forces Ionic strongest bond
metals to non-metals
highest melting points
crystal lattice structure
formed by the attraction between ions
cation (positive)to anion (negative) Hydrogen Bonding forms when a hydrogen is bonded to an Fluorine, Oxygen or Nitrogen (FON)
the hydrogen must e directly bonded to one of these other molecules to form a hydrogen bond
like a Dipole-Dipole force but stronger
have a higher boiling point than Dipole-Dipole forces Dipole-Dipole Forces must be between polar molecules (not symmetrical) because they have a permanent partial charge
these forces are stronger when the molecules are closer together
the force is formed because of the attraction between the positive and negative charges Van der Waals random shifts is electron location, creating partial charges, create this force
weakest force
present between all molecules
only force present when a molecule is non-polar
the bigger the molecule (the more electrons) the stronger the VDW force
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