Bio Exam Prep
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CHEMISTRY SEMESTER TWO EXAM NOTESCHAPTER 10- WATERWater and living thingsCellular RespirationC6H12O6(aq) + 6O2 (g) 6CO2(g) + 6H2O(l) + energy[pic 1]Photosynthesis[pic 2]6CO2(g) + 6H2O(l) C6H12O6(aq) + 6O2 (g)[pic 3][pic 4]WATER [pic 5][pic 6]Solid (ice) Liquid (water) Gas (water vapour)[pic 7][pic 8][pic 9] [pic 10][pic 11][pic 12][pic 13][pic 14][pic 15][pic 16]Specific Capacity Amount of energy required to raise the temperature of a substance of 1g by 1oC.Water has a high heat capacity- it take more energy to heat up 1g of water than 1g of anything else (eg. sand)Amount of energy required to raise temp= SHC x m x ∆T[pic 17][pic 18][pic 19][pic 20][pic 21]Water as a solvent Solvent + solute = solution A solution must be: Homogenous- solvent and solute distributed evenly throughout solution Solute particles must be too small to be seen Transparent in visible light. Why do substances dissolve?When one substance dissolves into another, the following occurs: The particles of the solute are separated from one anotherThe Particles of the solvent of separated from on anotherThe solvent and solute particles attract each otherA solute will dissolve if the attraction between the solute and solvent particles is strong enough to compete with the solute- solute and solvent-solvent forces of attractionAll substances that dissolve in water have ionic or polar covalent bondingMiscible- two liquids placed in same container they do not form separate layersImmiscible- form separate layers1) Dissolving Polar Covalent Compounds a) Hydrogen Bonds[pic 22] CH3CH2OH(l) CH3CH2OH(aq) [pic 23][The more –OH groups the more likely it is able to dissolve in water]H bonds of water break to make H- Bonds with the –OH group of another to dissolve it. b) Forming Ions [pic 24] HCl2(l) + H2O(l) H30+(aq) + Cl-(aq)[pic 25]
2) Dissolving Ionic CompoundsSolid ionic compounds contain + and – ions.In water the H+ is attracted to the – anion [pic 26][pic 27][pic 28] The O2- is attracted to the + cation [pic 29][pic 30][pic 31]This is called a Dissociation ProcessEg. NaCl(s) h20(aq) Na+(aq) + Cl-(aq) [pic 32]When an ionic compound dissolves in water, producing separate cations and anions.I.e. dissociated from the lattice.SOLUBILTY GUIDE FOR COMMON IONIC COMPOUNDSSoluble ionic CompoundsMost compounds of the following are solubleImportant exceptions Nitrate (NO3-)NoneEthanoate (CH3COO-) (acetate)None Sodium, Potassium (Na+, K+)NoneAmmonium (NH4)None Chloride (Cl-)AgCl, HgCl2, PbCl2 is slightly solubleBromide (Br-)AgBr, HgBr2, PbBr2 Iodide (I-)AgI, HgI2, PbI2Sulfate (SO4 2-)BaSO4,PbSO4, CaSO4 is slightly soluble. Insoluble ionic CompoundsMost compounds of the following are InsolubleImportant exceptions Sulfide (S2-) Na2S, K2S, Li2S, (NH4)2S, Carbonate (CO32-)Na2CO3, K2CO3, Li2CO3Phosphate (PO43-)Na3PO4, K3PO4, Li3PO4Hydroxide (OH-)NaOH, KOH, Ba(OH)2, Ca(OH)2 is slightly soluble