Term
| What makes water unique/essential to life? |
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Definition
solid form is less dense than the liquid form
high specific heat
excellent solvent
high boiling and melting point |
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Term
| Why does water have such strong intermolecular forces? |
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Definition
| It is highly polar and has hydrogen bonding |
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Term
| What is an intermolecular force? |
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Definition
a nonbionding force
the force exists between molecules
they influence the physical properties of the substance |
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Term
| What is an intramolecular force? |
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Definition
a bonding force
these forces exist within each molecule
they influence the chemical properties of a substance |
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Term
| What elements must be present for a Hydrogen bond to occur? |
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Definition
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Term
| What do H-bonds to to melting and boiling points? |
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Definition
| they elevate melting and boiling points |
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Term
| Why is ice less dense than water? |
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Definition
| the bent shape of water and the Hydrogen bonding arrangement make a hexagonal crystal structure when solid that is less dense than liquid |
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Term
| Why is ice important to aquatic life? |
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Definition
| It insulates water beneath, allowing aquatic life to survive winters |
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Term
| Why do we flash freeze our food? |
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Definition
because ice crystals will rupture tissues and the slower the freezing, the larger the crystals/tissue rupture will go
flash freezing makes smaller crystals |
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Term
| Why do substances form a meniscus? |
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Definition
| due to capillary action and adhesive forces, the liquid has adhesive forces and is attracted to the container |
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Term
| What kind of molecules have London (dispersion) forces as the primary intermolecular force? |
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Definition
| non-polar molecules have this |
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Term
| why do London forces occur? |
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Definition
| they occur because of the instantaneous dipoles created by random electron movement and are relatively weak forces with low boiling/melting points |
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Term
| can a dipole in one molecule induce a dipole in a neighboring molecule? |
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Definition
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Term
| What do London forces have to do with Molar mass? |
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Definition
| they increase as molar mass increases, so boiling points and melting points also increase with molar mass |
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Term
| what does surface area have to do with london forces and melting and boiling points? |
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Definition
| the greater the surface area, the greater the london forces and melting and boiling points |
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Term
| Rank in order of strongest to weakest the commong bonding/nonbonding forces |
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Definition
Ion-dipole
H bond
Dipole-dipole
Dipole-induced dipole
ion-induced dipole
dispersion |
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Term
| what molecules or ions can polar solvents dissolve? and non-polar solvents? |
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Definition
polar solvents can dissolve polar molecules or ions
non-polar solvents dissolve non-polar solutes |
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Term
| What is the difference between temperature and heat? |
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Definition
Heat is a flow of energy due to a temperature difference
Temperature is a measure of the random motions of the components of a substance |
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Term
| what is the specific heat? |
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Definition
| the amount of energy required to raise the temperature of one gram of a substance by one degree celsius? |
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Term
| what is the equation to find amount of heat? |
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Definition
Q=s*m*Δt
where Q = amount of heat
s = specific heat
m - mass
and Δt = change in temperature |
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Term
| what is the heat of fusion? |
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Definition
the energy required to melt 1 mole of a solid
specific to the substance |
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Term
| what is the heat of vaporization? |
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Definition
| the energy required to boil one mole of a liquid |
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Term
| why is the high specific heat of water important? |
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Definition
| it moderates temperature fluctuations and the high heat of vaporization has strong cooling effect |
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Term
| what is hard water, what ions are involved, and why is it a problem? |
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Definition
water with high amounts (>300 ppm) of Ca2+, Mg2+, and to a lesser extent Fe2+
It's a problem because it forms mineral deposits when it evaporates and it prevents proper lathering of soap and fomrs insoluble "soap scum" (spots on your dishes/dirty shower)
it's also a problem b/c to treat it we put phosphates in detergents which, when released into the environment, can cause eutrophication in ponds/aquaecosystems |
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Term
| What steps to we take to soften water? |
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Definition
we use ion exchange resins that exhange Ca2+ and Mg2+ for K+ or Na+
we also use charcoal filters (household ones use an ion exhange resin to soften water) |
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Term
| what is the structure of soap |
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Definition
| it has a non-poar tail and a polar head (like a phospholipid bilayer) |
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Term
| cholera, typhoid, cryptosporidiosis and ecoli in water |
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Definition
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Term
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Definition
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Term
| how to calculate ppm and ppb and what they mean |
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Definition
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Term
| groudwater contamination by fertilizers, pesticides, gasoline additives, volatile organic compounts (VOCs) |
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Definition
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Term
| steps of wastewater treatement |
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Definition
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Term
| how charcoal finters/household filters work |
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Definition
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Term
| bottled water vs tap water industry and expense |
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Definition
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Term
| treated water, natural and municipal sources |
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Definition
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Term
| bottled water, is it safer than tap? |
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Definition
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Term
| environmental cost of plastic used in manufacturing and transportation |
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Definition
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Term
| Describe a saturated and an unsaturated hydrocarbon |
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Definition
* saturated has every possible bond given to hydrogen
*unsaturated does not have all given to hydrogen, some double/triple bonds or other elements |
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Term
| What is the difference between an aliphatic or aromatic hydrocarbon? |
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Definition
both contain six membered carbon rings
Aliphatic can be saturated or unsaturated
saturated = alkanes, unsaturated = alkenes or alkynes and have double or triple bonds
may be chains or rings (ring molecules have 2 less H than chain so the ends can join)
chains may be straight or branched
Aromatics contain 1 or more 6 C unsaturated rings (benzene rings)
chemical reactions different than alkenes
resonance hybrid
all C-C bond lengths and bond angles are identical |
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Term
| how stable are hydrocarbons and how do they break down? |
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Definition
| they are very stabble but burn with substantial release of heat |
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Term
| what is the general formula for an alkane |
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Definition
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Term
| What is the general formula for an alkene? |
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Definition
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Term
| What is the general formula for a cyclohexane? |
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Definition
| CnH2n (but it's in a ring) |
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Term
| what is the general formula for alkynes? |
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Definition
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Term
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Definition
| a molecule with the same molecular formula but different arrangements of the atoms |
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Term
| what are the prefixes from 1-10 carbons |
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Definition
| meth, eth, prop, but, pent, hex, hept, oct, non, dec |
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Term
| know how to draw alkanes, alkenes, cycloalkanes, and alkynes including numbering, suffixes, and branching |
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Definition
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Term
| what kind of ring and electrons are associated with aromatics? |
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Definition
| they have a 6-membered flat ring with delocalized electrons |
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Term
| what are some specific aromatics? |
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Definition
| benzene, toluene, styrene, and phenol |
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Term
| what are the functional groups |
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Definition
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