Covalent Bonding Test Questions – Flashcards
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1. Transfer of electrons 2. Crystal lattice 3. Conductor in water 4. Brittle 5. Anion/Cation 6. High melting/boiling points 7. Stack
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Ionic Bonding
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1. Sharing of Electrons 2. Insulator 3. Polar/nonpolar 4. Low melting/boiling points 5. Do not stack
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Covalent Bonding
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1. Represents covalent bonding 2. Has octet for each atom except hydrogen
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Lewis Structures
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When two electrons from each atom are shared - 4 electrons shared total
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Double Covalent Bond
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1. Electrons shared equally
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Nonpolar Covalent Bonds
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1. Electrons shared unequally 2. Electrons shifted toward more electronegative atom
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Polar Covalent Bonds
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Molecules
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What Do Covalent Bonds Exist As
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1. Lower melting and boiling point 2. Non-conductors of electricity 3. Exist in all three states at room temp 4. Have common names 5. Have definite lengths and strengths
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Covalent Bond Properties
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1. The shorter the bond length, the stronger the bond 2. The longer the bond length, the weaker the bond 3. The more electrons shared, the stronger the bond 4. The less electrons shared, the weaker the bond
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Covalent Bond Length & Strength Relationship
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When more than one Lewis Electron Dot Structure is possible
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Resonance
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Some molecules share to have less than 8 or more than 8 valence electrons
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Exceptions To Octet Rule
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Ions that have covalent bonding within to hold them together so that they may bond together ironically
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Polyatomic Ions
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Carbon dioxide
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CO2
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Sulfur dioxide
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SO2
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Nitrogen Triflouide
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NF3
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Carbon tetrachloride
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CCl4
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Diarsenic trioxide
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As2O3
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Carbon monoxide
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CO
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Dihydrogen oxide
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H2O
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Chlorine Triflouide
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ClF3
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Diphosphorous Trioxide
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P2O3
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Disulfur decaflouride
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S2F10
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Hydrobromic acid
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HBr
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Hydroflouric acid
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HF
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Hydroiodic acid
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HI
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Perchloric acid
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HClO4
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Chloric acid
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HClO3
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Chlorous acid
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HClO2
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Hypochlorous acid
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HClO
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Nitrous acid
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HNO2
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Sulfurous acid
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H2SO3
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Phosphorous acid
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H3PO3
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Methane
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CH4
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Water
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H2O
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Ammonia
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NH3
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Glucose
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C6H12O6
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Carbonic acid
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H2CO3
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Phosphoric acid
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H3PO4
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Hydrochloric acid
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HCl
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Sulfuric acid
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H2SO4
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Nitric acid
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HNO3
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Acetic acid
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HC2H3O2
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When parallel orbitals overlap and share electrons
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Pi Bond
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Single covalent bonds - occur when pair of shared electrons is in an area centered between two atoms
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Sigma Bond
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Consists of one sigma bond and at least one pi bond
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Multiple Covalent Bond
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States that atoms lose, gain, or share electrons in order to acquire a stable electron configuration of a noble gas
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Octet Rule
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1. Subtract the atom with the highest Electronegativity from the atom with the lowest Electronegativity in each bond of a molecules 2. If between .4 - 1.7, it is polar 3. If between 0- .4, nonpolar 4. If 1.7 and greater, it is mostly ionic
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Calculate A Bond Polarity From Electronegativities
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Shared & unshared electron pairs want to get as far from each other as they can
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VSEPR Theory
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Valence shell electron pair repulsion theory
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What Does VSEPR Stand For
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Linear
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AB2
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Bent
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AB2E2
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Trigonal Planar
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AB3
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Tetrahedral
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AB4
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Pyramidal
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AB3E
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Trigonal bipyramidal
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AB5
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Octahedral
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AB6
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You treat the molecule as several smaller molecules, going one by one and finding each smaller molecule
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How Do You Find The Shape of A Very Large Molecule
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1. If the electrons are shared equally in all of the bonds in the molecule, then the electrons are distributed evenly in the whole molecule, making it nonpolar - if all bonds nonpolar, molecule nonpolar 2. If the molecule has polar bonds and they cancel out because of symmetry, then the molecule is nonpolar 3. If the bond polarities are not symmetrically arranged, then the molecule will be polar
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How To Determine Molecular Polarity From Bond Polarity & Shape
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1. The shorter the bond length, the stronger the bond 2. The longer the bond length, the weaker the bond 3. The more electrons shared, the stronger the bond 4. The less electrons shared, the weaker the bond
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Covalent Bond Length & Strength Relationship
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?
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How Are Bond Polarity & Molecular Polarity Related
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Name based on number of bonds
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Hybridization
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Base this strictly off of the number of bonds connected to the central atom
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Finding Molecular Shapes
