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28 Cards in this Set
- Front
- Back
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3 factors affecting resonance stability? |
1. Smaller charge over big charges 2. Less distance between charges 3. Neg charge on more electronegative atom |
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What are the 3 intermolecular forces? Describe and arrange them in order of strength |
Van der waals < dipole-dipole < hydrogen |
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Planck's relation between energy and frequency ? |
E=hf H=6.6x10^-36 |
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Angular momentum formula |
L = nh/2π h = 6.6x10^-36 |
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Energy of electron: |
E= -Rh/2π Rh= 2.18x10^-18 |
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Planck's relation to wavelength formula E=hc/(wavelength) H = 6.6x10^-34 C = 3x10^8 |
E=hc/(wavelength)H = 6.6x10^-34C = 3x10^8 |
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Energy of electron transition |
E=-Rh[(1/nf^2)-(1/(ni^2)] |
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Max electrons in a shell. Subshell? |
Shell: 2n^2 Subshell: 4L+2 |
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Describe the definition and periodic table trends for the following: Zeff: Atomic Radii: Ionic Radii (metals and nonmetals): Electron affinity: Electronegativity: |
Zeff: Consistent down and up. Increase ➡️ Atomic radii: increase ⬇️ and ➡️ Ionic radii metals: Increase ⬅️ away from metalloid line Nonmetals: increase ⬅️ away from metalloid line Electron affinity: Increase ➡️ and decreases ⬇️ Electronegativity: Increase ⬆️ and ➡️ |
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What are the incomplete octets and the expanded octets? |
Incomplete : H-2 He-2 Li-2 Be-4 B-6 Expanded: P-10 S-12 Cl-14 |
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What are the 4 properties of ionic compounds |
1. High bp/mp 2. Dissolve readily 3. Good aq conductor 4. Solid crystal lattice |
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What electronegativity differences correspond to what kind of bonds? |
0.0 to 0.5 no polar covalent 0.5 to 1.7 polar covalent 1.7-2 ionic |
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Equation for dipole moment |
P= qd q=magnitude of charge D= distance |
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Difference between formal charge and oxidation number |
Formal charge: all electrons shared equally regardless of EN Oxidation number: More EN atom gets all of the electrons |
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What is kw |
Disassociation constant of water [H3O][OH] = 10^-14 at 298K |
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How can you estimate p values with a formula? |
P= m - 0.n (Nx10^-14) |
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How can you estimate p values just by looking at the log? |
Log 10=1 Log 1 = 0 Log .1 = -1 Log .01 = -2 |
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Relate Kw to ka and Kb |
Strong acid x weak conj base = 10^-14 Ka x Kb = Kw |
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What is the henderson hasselbach equation? When does ph=pka? |
Ph = pka + log [A/HA]. At half equivalence ph = pka |
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What is equivalence? |
When equal amount of titrand and titrant exist in solution |
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What are the strong acids and strong bases? |
Strong Acids: HCL, HBr, HI, HNO3, H2SO4, HClO4 Strong Bases. OH of Group 1 and 2 |
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Describe the 4 reactions between strong and weak acids and bases |
Strong acid + strong base = water + salt Strong acid + weak base = salt Weak acid + Strong base = salt + water Weak acid + weak base = either way depending which ka is higher |
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Describe the equivalence point in: 1.Strong acid vs strong base 2.Weak acid vs strong base 3.Strong acid vs weak base |
1. Eq at 7 2. Eq above 7 3 eq below 7 |
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What are the two major MCAT buffers? |
Acetic acid: CH3COOH ↔️ CH3COO- + Na Ammonia: NH3 ↔️ NH4Cl |
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Define the following terms and give their formulas 1. Gram equivalent weight 2. Equivalents in a given mass 3. Normality 4. Molarity |
1. Mass that will produce 1 mole of subject of interest Molar mass / n 2. Mass/GEW 3. Equivalents per liter Eq/L 4. Molarity: Normality/n Number of equivalent produced or consumed |
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Define electrolyte |
Solution that conducts. Strength depends on how likely solute is to dissolve |
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Describe the following reaction types Combination: Decomposition: Combustion: Single displacement: Double displacement: Neutralization: |
Combination: A+B➡️C Decomposition A➡️B+C (with heat) Combustion: CH4 (hydrocarbon) + O2 (oxidant) ➡️ CO2 + H2O Single displacement: A+BC➡️B +AC (common in redox) Double displacement: AB + BC ➡️ AD + BC (aka methathesis, one product typically precipitated out) Neutralization: HA + BOH ➡️ AB (salt) + H2O (sometimes) |
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Describe nomenclature for the following ions: Cations: Monanomic anions (H+, O2-) |
Cations: Roman numeral to indicate charge OR -ous lesser charge -ic greater charge M |
