sch3u chemical bonding ionic vs. covalent compounds ms. yusuf
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SCH3U Chemical Bonding
Ionic vs. Covalent Compounds
Ms. Yusuf
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Formation of BondsChemical Bonds are formed between two atoms using shared valence electrons; this is the force that holds atoms together in compounds.
Valence Electrons are the electrons that occupies the outermost energy level of an atom
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Type of Bonds
Ionic vs. Covalent Ionic bonding occurs between metals and non-metals Covalent bonding occurs between non-metalsNote: Bonding between metals is called Metallic bonding
Video Clip: Chemical Bonding
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Octet RuleMost Noble gasses have 8 electrons in their outer shell. This is a stable conformation. Thus, the noble gasses do not react with other elements. In other words, noble gasses are very stable.
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Octet Rule (Continued)
When atoms form ions or combine in compounds they obtain electron configurations of the nearest noble gas (eight electrons in their valence shells)
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Ionic BondingIonic Bonds are formed from the electrostatic attraction of positive and negative ions
An atom that can lose an electron to become a positively charged ion, called a cation
An atom can gain electrons to become a negatively charged ion, called an anion
•In each case, the atom attains a noble gas configuration with its valence electrons. •A noble gas configuration is defined as a completely filled outer shell, like the noble gases.
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Ionic Bond: Example (Na and Cl)
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Ionic Bond: Example (Al and O)
Al
Al
O
O
O
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Examples of Ionic Bonding using Lewis Structures
Magnesium and Fluorine Calcium and Oxygen Potassium and Sulfur
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Covalent Bonding
Covalent bonding occurs between two non-metals. Covalent bonding is different from ionic bonding because electrons are shared instead of transferred.
Each atom has eight shared electrons
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Covalent Bonding: Example (H and F)
H F HF
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Covalent Bonding Using Lewis Structures
Silicon Oxygen Hydrogen and chlorine Bromine and Bromine
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Elements will not share the electrons in a bond equally
•The electronegativity (EN) of an element determines its ability to attract electrons in a bond•When elements are bonded together, the more electronegative element attracts the electrons
Example: HF•Flourine is more electronegative.•The electrons in the bond are attracted towards the fluorine atom
Polar Bond (Dipole Moment)
ENH = 2.1 ENF = 4.0
∆EN H-F = 4.0 - 2.1 = 1.9
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(Continued) This is not a complete transfer of an electron from hydrogen to
fluorine; it is merely a drifting of electrons toward fluorine
When a charge separation of this type is present, the molecule possesses an electric dipole, so called “dipole moment” and the bond is called a POLAR COVALENT BOND
H : F ClCl
:
Polar Covalent Covalent
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Polar Covalent Compound
0.5 < Electronegativity difference < 1.7
This difference is great enough for the bonding electron pair to spend more time near the more electronegative atom than the less electronegative atom.
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(Continued)
Example: Water (H2O)∆EN = 1.24 (which is between 0.5 and 1.7)
Polar Covalent BondOxygen = a slightly negative chargeHydrogen = a slightly positive chargeSince the hydrogen does not completely transfer its
electron to the oxygen, the their respective charges are indicated as + (the indication of partial positive charge) and - (indication of partial Negative charge).
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O
H H
+ +
-
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∆EN3.3
Comparison of Ionic, Non-polar covalent and Polar covalent bonding
1.7 0.5 0
[Na]+[Cl]- H+ - Cl- Cl - Cl
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Summary
Chemical Bonds are formed between the atoms in molecules
The bonds are formed from the valence electrons of the atoms and the resulting bond allows each atom to achieve a noble gas configuration (the most stable arrangement of electrons around the atom: Octet Rule)
The types of bonding can be classified as:1. Covalent (non-metal bondin; 0<∆EN<0.5)
2. Polar covalent bonds (non-metal bonding with a dipole moment; 0.5<∆EN<1.7)
3. Ionic (metals + non-metals; 1.7 <∆EN< 3.3)
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Questions Complete the chart:
Identify each compounds as ionic or covalent: CCl4,HCI, MgF2,
H2O,NH3, NaCl, OH, H2
Show how the bond forms between Li+Cl, Mg +O (Follow the Octet Rule) as well as Li + O