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84 Cards in this Set
- Front
- Back
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The intermolecular forces that occur between polar molecules is called? |
dipole - dipole |
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Non-polar molecules do not have charged areas and are only capable of forming weak intermolecular forces called what? |
London Dispersion Forces |
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What is the uneven sharing of electrons between 2 atoms in a covalent bond called? |
Dipole |
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Difference between INTRAmolecular forces and INTERmolecular forces |
INTRAmolecular: forces HOLDING atoms TOGETHER to form molecule. INTERmolecule: forces BETWEEN molecules or atoms. (like interstate I-95) |
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Polar Molecule |
Has slightly positive side and slightly negative side. (like north and south pole on earth) |
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Dipole-dipole force |
when the positive side of a polar molecule attracts the negative side of another polar molecule. |
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Hydrogen bond |
an attraction between a slightly positive hydrogen of one molecule and a slightly negative atom (N, O or F) on another molecule. (special case of dipole-dipole) |
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Which is the strongest intermolecular force? |
Hydrogen bond |
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Which force is important in affecting the properties of water and biological molecules such as proteins? |
Hydrogen bonds |
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What 4 physical properties do IMF effect? |
Boiling Point Melting Point Evaporation Solubility |
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When does a temporary (instantaneous) dipole form between nonpolar molecules? |
When the electrons gather more on one end of the molecule than the other causing it to be slightly negative and the other end to be slightly positive. This can also cause neighbor molecules to become temp dipole. |
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London dispersion force |
The weak intermolecular force that results from the motion of electrons that creates temporary dipoles in molecules. |
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Which is the weakest of the IMFs |
London dispersion force |
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Which is the only force that works on noble gases and non-polar molecules? |
London dispersion |
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London force _________as the size of the molecule increases. |
Increases |
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London force increases as molar mass ________. |
gets larger |
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Stronger IMF = ______ Vapor Pressure |
Lower |
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Highest Vapor Pressure = ______ IMF |
Weakest |
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Stronger IMF = _______ boiling point |
Higher |
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______ IMF = Lower Boiling Point |
Weaker |
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3 Properties of Acids |
- pH values 0 - 7 - Taste and smell sour - Turn pH paper pink, red or orange |
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3 Properties of Bases |
- pH values greater than 7, up to 14 - Taste soapy and feel slippery - turn pH paper green, blue or purple |
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_____ Acids and Bases dissociate (break apart) 100% in solution |
Strong |
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Weak Acids and Bases dissociate ________ in solution |
much less than 100%. Only a small fraction break apart into constituent ions |
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What does an acid do when put in water? |
Breaks apart (dissociates) |
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Arrhenius Theory |
Acid Produces H3O+ (H+) in Sol'n Base Substance contains OH- and produces more OH- in water |
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Bronsted-Lowry Theory |
Acid - Proton Donor Base - Proton Acceptor |
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Conjugate Acid |
An acid that forms when a base gains a proton |
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Conjugate Base |
A Base that forms when an acid loses a proton |
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All arrhenius acids/bases are also _______ acids/bases |
Bronsted-Lowry |
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What do Inter Molecular Forces determine? |
Whether a substance is liquid, gas or solid. |
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Strength and attraction of Dipole-Dipole interaction depends on what? |
Size and Polarity of Molecule |
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The ___ bond is very polar |
O-H (there are 2 lone pairs on O atom) |
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Vapor Pressure |
The pressure exerted by the vapor when in equilibrium with its liquid. |
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Vapor pressures _______ with increasing temperatures |
increase |
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The temperature at which the vapor pressure of a liquid equals the external pressure |
Boiling point |
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Boiling point is effected by ____ and ____ |
IMF and Pressure |
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By adjusting the ____, a liquid can boil at any temperature. |
pressure |
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Heat of vaporization |
the amount of energy required to vaporize a mole of liquid at its boiling point. |
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Strong IMF have: __ Heat of Vaporization __ Boiling Points __ Vapor Pressures |
High Heat of Vaporization High Boiling Points Low Vapor Pressures |
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Surface tension |
The energy required to increase the surface area of the liquid. |
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Surface tension is dependent on ______ |
the strength of IMF |
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Viscosity |
The measure of the resistance to flow. |
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Viscosity depends on the strength of the ____ as well as the _____ of molecues |
IMF Size and Shape |
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For liquids, an increase in temperature will ____ the viscosity. |
Decrease (i.e. warming honey) |
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High IMF = ___ Viscosity
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High (generally) |
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Does cold honey have high or low viscosity? |
High |
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4 Properties of solids |
- Molecule, atoms or ions locked in Crystal Lattice - Particles CLOSE together - Forces that hold particles depend on type of solid - Highly ordered, rigid, incompressible, high densities. |
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4 Types of Crystalline Solids |
Ionic Molecular Metallic Network |
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Ionic Crystalline Solid (5 things about) |
- Solids contain ionic compound. - Bonding is ionic - High MP - Hard but brittle - Conduct electricity when molten or in solution |
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Molecular Crystalline Solid (5 things) |
- Solids have molecules or atoms arranged in regular pattern. - Low MP - Generally Insoluble in water - Non-conductor of electricity - Held by IMF |
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Metallic Crystalline Solid (3 things) |
- Have metal atoms arranged in regular pattern - properties of metals (malleable, ductile, conduct heat & electricity) - Bonding called metallic bonding |
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Network Crystalline Solid (3 things) |
- Solids held by covalent bonds. - Typically High MP - Hard but Brittle |
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Molecule that I think should be polar but is not |
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IMF's strongest to weakest |
Hydrogen-Bonding (strongest) Dipole-dipole London (weakest) |
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Examples of Ionic Crystalline Solids |
NaCl, K2SO4, CaCl, (NH4)3PO4 |
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Examples of Metallic Crystalline Solids |
Iron, Silver, Copper, others metals and alloys |
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Examples of Molecular Crystalline Solids |
H2, O2, I2, H2O, CO2, Ch3OH |
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Examples of Network Crystalline Solids |
Graphite, Diamond, Quartz, Feldspars, Mica |
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7 Strong Bases |
All of the soluble Hydroxides: LiOH NaOH KOH CsOH RbOH Sr(OH)2 Ba(OH)2 |
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7 Strong Acids |
HCl HBr HI HNO3 H2SO4 HClO4 HClO3 |
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Acids react with bases to give _____ and react with certain metals to give ______. |
- React with bases to give a salt and water. - React with certain metals to give a salt and H2 |
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Conjugate Acid Pair |
Acid-Base pair that differ by ONLY 1 proton (H+) |
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Amphiprotic
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can act as acid or base (i.e. water) |
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Acidic |
pH < 7 |
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Basic |
pH > 7
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pH formula |
pH = -log[H3O+] |
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pOH formula |
pOH = -log[OH-]
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pH + pOH = |
14 |
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[H3O+] = |
10 ^-ph |
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[OH-] = |
10 ^-poh |
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Suspensions (3 things) |
- Particle size is large, so some particles will settle and some stay suspended - Have tyndall effect - Easy to separate (filter) |
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Tyndall effect |
When light is scattered (i.e. when beam of light shows dust in the air) |
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Colloidal Dispersion (4 things) |
- small particles - particles don't settle or filter - can use centrifuge to separate - have tyndall effect (example - starch & water) |
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3 types of mixtures |
Suspensions Colloidal Dispersions Solutions |
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Solutions (4 things) |
- Particles very small <1 nm - Particles don't settle or filter - Homogenous mixture - No Tyndall effect |
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______ in pressure increases solubility of a gaseous solute in a liquid. |
Increase |
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Increase in temperature ________ solubility of a gaseous solute in a liquid.
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decreases |
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The missibility of two liquids is determined by? |
IMF Need to have like forces to work. Like dissolved like. |
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Non-Polar solutes will dissolve in what? |
non-polar solvents i.e. C10H8 will dissolve in CCl4 or C6H14 |
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Polar solutes will dissolve in what? |
polar solvents (i.e. water) |
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Ionic solutes will dissolve in what |
very polar solvents (i.e. water) Not all ionic compounds are soluble in H2O - see solubility rules |
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Two examples of acidic anhydrides |
CO2 and NO2 |
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Any _____ compound with a lone pair, will act as a base. |
Nitrogen. (i.e. NH3) |
