(Ionic, Covalent and Metallic)...The strength of a metallic bond is determined by number of outer...
Transcript of (Ionic, Covalent and Metallic)...The strength of a metallic bond is determined by number of outer...
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Chemical Bonding (Ionic, Covalent and
Metallic)
Name_________________
Quiz Date _____________ Test Date______________
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____________________ is the mutual attraction between the nucleus and valence electrons of different atoms. Atoms bond to become more ______________!
What are the 3 bond types? 1) Def: ____________________________________________________ ________________________________________________________ ________________________________________________________ 2) Def: ____________________________________________________ ________________________________________________________ ________________________________________________________ 3) Def: ____________________________________________________ ________________________________________________________
Types of Covalent Bonds 1) Equal sharing of electrons between atoms in a compound, no positive or negative poles exist = _________________________________________ 2) Unequal sharing of electrons within a molecule, positive and negative ends exist = _________________________________________________
Occurs Between Role of the Electrons
Example
Covalent Bonding
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Determine Bond Type from Electronegativity Differences Try It – Practice Problems: Determine the BOND Polarity: 1) H – S (2.2, 2.6) 5) Cs – S (0.8, 2.6) 2) S – Cl (2.6,3.2) 6) O – O (3.4,3.4) 3) Rb – Se (0.8,2.6) 7) F – I (4.0,2.7) 4) C – I (2.6,2.7) 8) Ca – N (1.0,3.0) Other Types of Covalent Bonds:
Memorize this Diagram!!
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Key Terms to Know: *________________________ = neutral compound consisting of nonmetals covalently bonded *_________________________________ = smallest representative unit of a molecular compound, can exist independently
What are these elements called? Def: ___________________________ ___________________________ ___________________________ Define these: Bond Length:_________________________________________________ _____________________________________________________________ Bond Angle:__________________________________________________ _____________________________________________________________ Bond Energy:________________________________________________ _____________________________________________________________
As bond length increases, bond energy decreases. As bond length increases, bond strength decreases.
**Think about it!!!** What relationship do each of the above have? What is the relationship between bond length and bond strength for each?
Memorize These!!
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What are polyatomic ions? DEF: Ex:
Properties of Covalent Compounds Dot Diagrams and Structural Formulas - Molecules It is important to follow the Octet Rule - ____________________________ _____________________________________________________________ The following elements are exceptions to this rule: (MEMORIZE THESE!) Let’s Try It – Practice Problems! Examples:
1. NH3
2. CH4
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3. H2O
4. BF3
5. CO2 VSPER Theory: ______________________________________________ _____________________________________________________________ _____________________________________________________________ Define and draw a picture for each of the following: Lone pair: Shared pair: Def: Def: Picture:
Molecular Geometry (Shapes)
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VSEPR - Shapes Table ****The five shapes you need to know are…****
Shape # Bonds to
Central Atom # Lone Pairs to Central Atom
Examples
Linear 2 atoms together or 2
bonds to central atom
0
Bent 2 2
2 1
Trigonal Planar 3 0
Trigonal Pyramidal
3 1
Tetrahedral 4 0
Let’s Try It – Practice Problems! 1. NH3 2. CH4 3. H2O 4. BF3 5. CO2
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Molecular polarity: What does Molecular Polarity depend upon? 1) 2) 3) Molecular polarity influences intermolecular forces. Nonpolar molecule: Polar molecule: Polar or non-polar?
____________ _________ ______________
Think about it: Review Questions for studying on your own 1) What shapes are ALWAYS polar molecules?
2) What guarantees that a compound will be polar?
Molecular Polarity
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Intermolecular Forces: ________________________________________ _____________________________________________________________ _____________________________________________________________ The 3 intermolecular forces are 1) 2) 3) Type Definition Examples
Let’s Try It! – Determine the IMF(s) Present H2O Molecular Polarity =
Dispersion Forces Dipole-Dipole H-Bonding
SCl2
Intermolecular Forces The glue that holds the molecules together
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PF3
CF4 Relating properties to IMF’s:
1. Stronger bonds/imf’s
2. Weaker bonds/imf’s
3. Solubility Let’s Try It! - Practice Problems
1. Would the following be soluble in each other? - H2O and CF4
2. Which would have the higher boiling point? - H2O or PF3
3. Which would have the lower melting point? - CO2 or NH3
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Definition Role of the
Electrons Example
How does this picture explain metallic bonding? ________________________ ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ Properties of Metallic Compounds
Metallic Bonding
The strength of a metallic bond is determined by number of outer electrons Softer metals can be combined with harder metals. The strongest metals are the transition metals
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Definition Role of the
Electrons Example
The simplest combining ratio of ions in a compound that does not exist independently is called a _______________________________. Determining the formula unit
(Remember that the compound is neutral overall = no charge) Let’s try it! Determine the formula unit for each! 1) Potassium and Fluorine 2) Calcium and Iodine 3) Magnesium and Nitrogen 4) Calcium and nitrate 5) Sodium and phosphate
Ionic Bonding
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Drawing Structures - Dot Diagrams for Ionic Compounds Ex: NaCl Ex: CaBr2 Ionic Compounds form solid crystals. Crystal lattice: ___________________________________________ _______________________________________________________
Lattice energy: ___________________________________________ ________________________________________________________ ________________________________________________________
Crystal Lattice – all (+) ions are completely surrounded by (-) ions and vice versa
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Properties of Ionic Compounds