ionic compounds ionic compounds (salts) formed by transferring electrons (giving/taking) occurs...
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Intramolecular forces
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Ionic Compounds Ionic Compounds (SALTS)
formed by transferring electrons (giving/taking) occurs between a metal and a non-metal have an electro negativity difference greater than 1.7 unit is called "formula unit“
Since electrons are transferred, not shared, the atoms aren’t attached to each other like in a molecule
exist as solids, usually crystalline have high melting points
This is because of the strength of their bond. A stronger bond requires more energy to break
soluble in water conducts electricity in water fixed + and – parts (anions & cations )
EXAMPLES: KCl, NaF, KNO3
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Crystalline Structure of Ionic Compounds
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Metallic Bonds A metallic bond is a bond formed by the attraction between neighboring
metal nuclei and the electrons around them. metal atoms create a crystal lattice of positive metallic nuclei in a 'sea of
electrons'.
Electricity is the movement of electrons Metals are good at conducting electricity because their bonds allow the
electrons to flow freely because they are delocalized This means that they do not belong to any one atom but move freely about
the metal’s network of empty atomic orbitals.
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Metallic Bond PropertiesElectrical & thermal conductivity as a solid or liquid
This is because of how freely the electrons can moveHigh melting and boiling points
This is because of the strength of their bond. A stronger bond requires more energy to break
Malleable (sheets) and ductile (wires)The delocalized electrons in the 'sea' of electrons in
the metallic bond, enable the metal atoms to roll over each other when a stress is applied.
Shiny appearance Photons of light do not penetrate very far into the
surface of a metal and reflect off the metallic surface.
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Covalent Compounds formed by sharing electrons occurs between non-metals unit is called "molecule“ exists as liquids, gases, or non-crystal solids have low melting points
This is because a covalent bond isn’t as strong as the other two types of bonds
insoluble in water This is because covalent compounds to not have much of a difference in
charge conducts electricity in water may have slightly + and - parts or totally neutral
When they have a slight difference in charge, they are considered polar When there is no difference in charge, they are considered non-polar
EXAMPLES: NH3, CO2, CH4
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Polar vs. Non-Polar Covalent CompoundPolar BondsBonds in which atoms share electrons
unequally are called polar covalent bonds. The electronegativity difference between the two
atoms is between 0.5 and 1.7
Non-Polar BondsBonds in which atoms share electrons equally
are called non-polar covalent bondsThe electronegativity difference between the two
atoms is below 0.5
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Ionic, Metallic, Polar Covalent or non-polar covalent? Step 1: Figure out what type of element each atom is in
the compound (metal or non-metal)Metal + Metal = MetallicMetal + Non-metal = IonicNon-metal + Non-metal = Covalent (polar or non- polar)
Step 2: If it’s a covalent compound, you must find the difference in negativity to determine if it is polar or non-polar by looking that the chartNon-polar molecules have an electronegativity difference
of less than 0.5Polar molecules have an electronegativity difference of
greater than 0.5 but smaller than 1.7
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Single, Double and Triple Covalent BondsSingle bonds
Only 1 electron pair is shared (total of 2 electrons)Requires the least amount of energy to breakHas the largest distance between nuclei of the 3 bonds
Double bonds2 electron pairs are shared (total of 4 electrons)Requires a moderate amount of energy to breakHas a medium distance between nuclei of the 3 bonds
Triple bonds3 electron pairs are sharedRequires the most amount of energy to breakHas the shortest distance between nuclei of the 3 bonds
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Single, Double and Triple Covalent Bonds
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How do I figure out if it’s a single double or triple bond?ANS: Create a Lewis dot structure!
Organic Chemistry Example: compare the carbon-carbon bond of the following compounds:
1. Ethane (C2H6)
2. Ethene (C2H4)
3. Ethyne (C2H2)
Which one has a single bond? Double bond? Triple Bond?