Module 7 (Part II)
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Last updated 1:53 AM on 3/3/23
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21 Terms
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VSEPR Model
\-Valence Shell Electron Pair Repulsion model
\-based on arrangement that MINIMIZES REPULSION of shared & unshared electron pairs around central atom
\-bond angles & unshared electron pairs help determine shape of molecule
-shared electron pairs are pushed slightly together by lone pairs b/c lone pairs contribute to repulsion
\-electron pairs are located in a molecule as far apart as they can be
\-based on arrangement that MINIMIZES REPULSION of shared & unshared electron pairs around central atom
\-bond angles & unshared electron pairs help determine shape of molecule
-shared electron pairs are pushed slightly together by lone pairs b/c lone pairs contribute to repulsion
\-electron pairs are located in a molecule as far apart as they can be
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bond angle
\-electron pairs repel each other and cause molecules to be in fixed positions relative to each other
\-angle formed by 2 terminal atoms w/ central atom is called bond angle
\-angle formed by 2 terminal atoms w/ central atom is called bond angle
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2 electron groups
0 lone pairs
0 lone pairs
\-linear
\-180 degrees
\-180 degrees
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3 electron groups
0 lone pairs
0 lone pairs
\-trigonal planar
\-120 degrees
\-120 degrees
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3 electron groups
1 lone pair
1 lone pair
\-bent
\-
\-
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4 electron groups
0 lone pairs
0 lone pairs
\-tetrahedral
\-109.5 degrees
\-109.5 degrees
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4 electron groups
1 lone pair
1 lone pair
\-trigonal pyramid
\-
\-
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4 electron groups
2 lone pairs
2 lone pairs
\-bent
\-
\-
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electronegativity & bond character
\-**equal** sharing of electrons results in **nonpolar** covalent bond
\-**unequal** sharing of electrons results in **polar** covalent bond
\-bonding is often not clearly ionic or covalent
\-the greater the electronegativity difference → the greater the ionic character
\-**unequal** sharing of electrons results in **polar** covalent bond
\-bonding is often not clearly ionic or covalent
\-the greater the electronegativity difference → the greater the ionic character
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polar covalent bonds
\-electrons spend more time around more electronegative atom
\-results in partial charges at the ends of the bond
\-results in partial charges at the ends of the bond
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nonpolar covalent bond
\-between 2 identical or very similar atoms
\-not great electronegativity difference
\-electrons shared equally & charge is balanced evenly
\-not great electronegativity difference
\-electrons shared equally & charge is balanced evenly
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determining bond character according to EN difference
\- > 1.7 = mostly ionic
\- 0.4 - 1.7 = polar covalent
\- < 0.4 mostly covalent
\- 0 nonpolar covalent
\- 0.4 - 1.7 = polar covalent
\- < 0.4 mostly covalent
\- 0 nonpolar covalent
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polar molecules
\-molecules are polar when electrons are shared unequally btwn atoms (contain polar bonds)
\-this causes molecule to have partial neg charge on part of atom w/ more electrons (more electroneg atom)
\-non-polar molecules aren’t attracted by an electric field
\-polar molecules align w/ an electric field & are called **dipoles**
\-this causes molecule to have partial neg charge on part of atom w/ more electrons (more electroneg atom)
\-non-polar molecules aren’t attracted by an electric field
\-polar molecules align w/ an electric field & are called **dipoles**
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organic compound exceptions
\-all carbon-containing compounds
\-EXCEPTIONS:
-carbon oxides (ex. CO2)
-carbonides (carbon + a metal)
-carbonates (CaCO3)
\-EXCEPTIONS:
-carbon oxides (ex. CO2)
-carbonides (carbon + a metal)
-carbonates (CaCO3)
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organic compound structure
\-carbon nearly always shares its electrons & forms 4 covalent bonds
\-in organic compounds, carbon usually bonded to H or elements near carbon on periodic table (N, O, S, P, & halogens)
\-bc C forms 4 bonds → forms complex, branched-chain structures, ring structures, & even cage-like structures
\-in organic compounds, carbon usually bonded to H or elements near carbon on periodic table (N, O, S, P, & halogens)
\-bc C forms 4 bonds → forms complex, branched-chain structures, ring structures, & even cage-like structures
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hydrocarbons
\-simplet organic compounds
\-contain ONLY elements C & H
\-contain ONLY elements C & H
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saturated hydrocarbon
\-contains only single bonds (ALKANES)
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unsaturated hydrocarbon
\-contains at least one double or triple bond (ALKENES & ALKYNES)
\-watch names of alkenes & alkynes
-ex. (alkene example) 1-Butene → double bond is btwn 1st & 2nd carbon, but 2-Butene → double bond is btwn 2nd & 3rd carbon
\-watch names of alkenes & alkynes
-ex. (alkene example) 1-Butene → double bond is btwn 1st & 2nd carbon, but 2-Butene → double bond is btwn 2nd & 3rd carbon
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alkanes
\-one single bond btwn atoms
\-simplest hydrocarbons
\-name ends in -*ane*
\-General formula: **C(n)H(2n+2)** where n=# of C
\-simplest hydrocarbons
\-name ends in -*ane*
\-General formula: **C(n)H(2n+2)** where n=# of C
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alkenes
\-double covalent bonds btwn carbon atoms
\-name ends in -*ene*
\-for alkenes w/ only one double bond & 4 or more C, general formula: **C(n)H(2n)** where n=# of C
\-name ends in -*ene*
\-for alkenes w/ only one double bond & 4 or more C, general formula: **C(n)H(2n)** where n=# of C
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alkynes
\-triple covalent bonds btwn carbon atoms
\-name ends in -*yne*
\-General formula: **C(n)H(2n-2)** where n=# of C
\-name ends in -*yne*
\-General formula: **C(n)H(2n-2)** where n=# of C