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45 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Carbon prevalence
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Makes up less than 1% of earth's crust, what is most prevalent?
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Si, Al, and O2 |
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Are all compounds containing carbon considered organic?
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No, what doesn't get included?
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pure carbon compounds (such as graphite, diamond, Bucky Balls, nanotubes), CO2, calcium carbonate, etc. |
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Why is carbon so special?
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Can form strong single bonds with itself.
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What are isotopes, ions, and elements?
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differing number of neutrons are isotopes
differing number of electrons are ions elements differ by number of protons |
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How do you calculate formal charge?
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(Valence) - (# of bonds) - (# non-bonded electrons)
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# of bonds & lone pairs?
Boron Carbon Nitrogen Oxygen Fluorine |
3, 0
4, 0 3, 1 2, 2 1, 3 |
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Draw out memorized set of periodic table
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H——————————————He
Li—Be———B—C—N—O—F—Ne Na————————P—S—Cl—Ar K————————————Br—Kr |
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What 2 factors contribute to a bond dipole?
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Differences in electronegativity
Bond length |
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When you see Na-sth or K-sth...
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Cross out spectator ion from group 1 and write in charge on anion
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What moves in resonance?
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electrons (NEVER move the charge)
Which ones? |
lone pairs & pi bonds |
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To start on resonance problems...
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move electrons towards positive charge
Why? |
Because positive and negative attract. |
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What are road blocks in resonance structures?
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sp3 hybridized atoms
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How do I choose the major resonance contributor?
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#1: Octet Rule
If octet rule is fulfilled for multiple structures, where should the negative charge be? |
On the most electronegative atom. Also, minimize separation of charge. |
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What is an empirical formula?
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simplest, whole-number ratio of elements in a compound
With what else could you determine molecular formula? How? |
molar mass Divide molar mass by empirical mass to get factor by which to multiply empirical numbers. |
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Molar Mass of
Hydrogen? Carbon? Nitrogen? Oxygen? |
1 g/mol
12 g/mol 14 g/mol 16 g/mol |
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What is a molecular formula?
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The total number of each element in a molecule of a compound.
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What is a structural formula?
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Elucidates the Lewis structure of the molecule.
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Rules for writing condensed structural formula?
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CH2's in a row counted and written as (CH2)n
CH3's connected to same carbon written as (CH3)n |
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What is deuterium and its symbol?
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Heavy hydrogen (1 neutron), D (must still be drawn in on line-angles)
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Arrhenius acids and bases
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Acids dissociate in H2O to give H3O+
Bases dissociate in H2O to give OH- |
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Lewis acids and bases
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Acids accept electrons (electrophiles)
Bases donate electrons (nucleophiles) |
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Bronsted-Lowry acids and bases
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Acids donate protons
Bases accept protons |
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What is the difference between 2 conjugates (acid/base)?
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1 proton
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What is the periodic trend for acid strength?
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When the proton of interest is bonded to different elements, acidity increases left to right, top to bottom
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What other factors increase acidity of a molecule?
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Electron-withdrawing groups (halogens, NO2, C=O) near acidic proton. More electronegative = stronger effect.
How? |
They help stabilize the conjugate base. |
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During acid comparisons...
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check to see if molecule may be a carboxylic acid (acidic) or an alcohol (NOT acidic).
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What are the strong acids?
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HCl
HBr HI H2SO4 HNO3 HClO4 |
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Strong acid creates..
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Weak conjugate base
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Strong base creates...
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strong OR weak conjugate acid
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Weak acid or base creates..
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Weak OR strong conjugate
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What strong bases have we seen up until now?
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hydroxide and alkoxides are the weakest of the strong bases (anything above that on the table will be strong)
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pKa
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refers to acid strength
< 0 - very strong 0-5 moderately strong 5-15 moderately weak 15+ weak (higher Ka = lower pKa = stronger acid) |
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pKa of CH4
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45-50
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pKa of NH3
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about 35
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pKa of terminal alkyne
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about 25
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pKa of alcohol
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15-18
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pKa of water
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15.7
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pKa of phenol
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10
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pKa of carboxylic acid
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4-5
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How do I rank a series of bases in order of increasing/decreasing basicity?
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1. Convert to acids
2. Determine approx. pKa 3. W/in category, rank on electron-withdrawing groups 4. Reverse acid strength order |
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How do I determine if a base is strong enough to quantitatively deprotonate an acid?
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If you start from the acid in question, go across to its conjugate. Conj. will not be strong enough, and you will have equilibrium.
Any base that is stronger than the conjugate (higher on the list that orders acids and bases), will be able to completely deprotonate the acid. |
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degenerate orbitals
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orbitals with identical energies (p. 4)
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covalent bonding
ionic bonding |
occurs through sharing of electrons
attraction of oppositely charged ions (usually forms 3D lattice structure) |
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polar covalent bond
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electrons shared unevenly
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What makes a molecule stable?
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Dispersion of charge therefore...
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having resonance structures makes a molecule incredibly stable |
