GENERAL CHEMISTRY-UNIT 5 REVIEW-Bonding
Bonding
Define and Know the following
Ionic
Naming rules
Cation
Anion
Electrostatic Attraction
Ionic Bond & characteristics
Lattice Energy
Covalent
Naming rule
Electronegativity
Electronegativity Difference
Covalent Bond & characteristics
Polar covalent bonds
Non-polar covalent bonds
Molecule
Octet Rule (stable octet, stable duet)
Valence Electrons
Resonance
Bond Polarity
Dipole
Diatomic Atoms
Metallic Bond & Characteristics
Electron-Sea
Lewis Structures
Valence Electrons
How may does each atom need? (hydrogen?)
Draw a Lewis Structure (electron dot diagram)
Shared pairs (Bonding pairs)
Unshared (Nonbonding pairs)
Single/Double/Triple Bonds
Recognize Lewis structure
Intermolecular Forces
London Dispersion Forces
Dipole-Dipole
H-bonding
VSEPR – Valence Shell Electron Pair Repulsion Theory
Linear
Bent
Trigonal Planar
Trigonal Pyramidal
Tetrahedral
Molecular Polarity - predict
Nonpolar: must be both of the following:-Symmetry in Shape AND
-Symmetry in Atoms
Polar :
No symmetry in shape or atoms
1. Using your electronegativity and bond character charts determine the types of bonds (nonpolar covalent,
polar covalent, or ionic) that will form between the following atoms:
Atoms
Electronegativity difference
Bond Type
Oxygen and Oxygen
Sulfur and Oxygen
Lithium and Oxygen
Iron and Fluorine
Titanium and Oxygen
2.
For each of the following molecules: 1) draw the Lewis Structure ( electron-dot diagram), 2) write down how many
valence electrons are in each compound, 3) determine the polarity type of the bonds inside the molecule using the
Electronegativity Table From the notes, 4) determine the shape of the molecule using the VSEPR Table from the
notes, and 5) determine whether the molecule is a polar or nonpolar molecule using the symmetry/assymetry
guidelines from the table.
NO3 -1
CF4
Bonds: __________________________
Bonds:_________________________
Shape:___________________________
Shape:_________________________
Molecules:_______________________
Molecule:_______________________
IMF:____________________________
IMF:___________________________
PCl3
SBr2
Bonds: __________________________
Bonds:_________________________
Shape:___________________________
Shape:_________________________
Molecules:_______________________
Molecule:_______________________
IMF:____________________________
IMF:___________________________
3. What is the force that holds an ionic compound together? Explain.
4. What are three different types of intermolecular forces of attraction and rank them from strongest to weakest.
5. Are intermolecular forces stronger or intramolecular forces?
6. What is the Kinetic-Molecular Theory? How are energy and intermolecular forces related?
7. Which transition metals do not need a roman numeral, because their charge never changes?
8. What charge do the alkali metals always form? Alkaline-Earth? Halogens?
9. Which elements are diatomic? What does this mean?
10. What is the shape and strongest intermolecular force present for each of the following compounds? You may
find it useful to draw Lewis structures for some of these molecules:
Chemical Formula
a. water
Molecule Polarity?
IMF
_______________
________________
b. carbon tetrachloride _____________
______________
________________
c. nitrogen trichloride
_______________
________________
_________________
_______________
________________
_________________
c. HCN
______________
SHAPE
______________
________________
________________
11. Using the space below, explain the difference between an ionic and covalent compounds.
12. Identify the following compounds as Ionic, Covalent & write the correct chemical formula or name:
sodium sulfide: ____________________________________________________________________
sulfur dioxide: _____________________________________________________________________
zinc oxide: _______________________________________________________________________
K3PO4: __________________________________________________________________________
Fe2O3: ___________________________________________________________________________
Ca(OH)2: _________________________________________________________________________
heptasilicon tribromide: ___________________________________________________________
Mercury (II) chloride:________________________________________________________________
N2O5: ___________________________________________________________________________
AuS: ____________________________________________________________________________
chromium (III) nitrate: _______________________________________________________________
Ba3(PO4)2 : ________________________________________________________________________
13. What is wrong with the following compounds. Correct the error:
monosilicon heptachlorine:__________________________________________________________
Ba2S2:_______________________________________________________________________________________________________________
MgN2O6:_______________________________________________________________________________
iron oxide: ______________________________________________________________________
aluminum (III) oxide: _____________________________________________________________
Cr(NO3)2 was named chromium nitrate: ______________________________________________
SrBr2 was named strontium sulfur bromine: ____________________________________________
heptacarbon monooxygen: _________________________________________________________
Bonding Review Answers:
1. O & O Nonpolar; S & O Polar; Li & O Ionic; Fe & F Ionic; Ti & O Ionic
2. Lewis Structures:
NO3- Bonds: (weakly) polar
Shape: trigonal planar
Molecules: non-polar
PCl3-Bonds: Polar
Shape: trigonal pyramidal
Molecules: Polar
CF4- Bonds: (strongly) polar
Shape: tetrahedral
Molecules: non-polar
SBr2-Bonds: (weakly) polar
Bent -- 2 shared + 2 Unshared @ Sulfur
Polar - because it is bent
GENERAL CHEMISTRY-UNIT 5 REVIEW-Bonding
Bonding
Define and Know the following
Ionic
Cation: positively charged ion due to losing electrons
Anion: negatively charged ion due to gaining electrons
Electrostatic Attraction: forces between unlike charges organizing the ions of ionic substances into a rigid, organized threedimensional arrangement
Ionic Bond & characteristics
Ionization Energy energy required to remove electrons
Electron Affinity ability of atoms to attract electrons
Lattice Energy energy given off when ions of opposite charge bond together
Unit Cell smallest structure of an ionic compound
Covalent
Electronegativity attraction for electrons in a chemical compound
Electronegativity Difference
Covalent Bond & characteristics
Polar covalent bonds
Non-polar covalent bonds
Molecule smallest structure of a covalent compound
Bond Strength vs. Bond Length the stronger the bond the shorter the bond length, triple bonds are stronger than double, etc.
Octet Rule (stable octet, stable duet)
Valence Electrons electrons located in the outermost energy level, are involved in chemical bonding/reactions
Resonance
Coordinate Covalent Bond: when two atoms have a covalent bond where the two electrons that are shared by the atoms in the bond
come from only one of the atoms
Bond Polarity
Dipole
Diatomic Atoms
Bond Energy (aka bond dissociation energy)
Exothermic vs. Endothermic
Metallic Bond & Characteristics
Electron-Sea: valence e- very mobile between metallic bonds, not belonging to any one atom, smallest structure of metallic compounds
Lewis Structures
Valence Electrons
How may does each atom need? (hydrogen?)
Draw a Lewis Structure (electron dot diagram)
Shared pairs (Bonding pairs)
Unshared (Nonbonding pairs)
Single/Double/Triple Bonds
Recognize Lewis structure