final exam key terms | CHEM 1045 - General Chemistry Lab, Quizzes of Chemistry

Download final exam key terms | CHEM 1045 - General Chemistry Lab and more Quizzes Chemistry in PDF only on Docsity! TERM 1 pure substance DEFINITION 1 a type of matter that has a fixed composition TERM 2 element DEFINITION 2 substance that cannot be broken down into a simpler substance TERM 3 compound DEFINITION 3 substance that is composed of two or more elements chemically combined in a fixed proportion by mass. TERM 4 mixture DEFINITION 4 a substance that consists of two or more pure substances that are physically combined TERM 5 % composition of a component DEFINITION 5 (mass of component / total mass of sample) X 100 TERM 6 % error DEFINITION 6 (original mass of sample - total mass of collected sample) original mass of sampleanswer X 100 TERM 7 Law of Conservation of Mass DEFINITION 7 the sum of the individual masses of the components that are collected must equal the mass of the original sample of mixture. TERM 8 Filtration DEFINITION 8 Can be used to separate a liquid and solid. TERM 9 precipitate DEFINITION 9 a reaction where aqueous solutions of two ionic compounds react to form an insoluble product. a precipitate forms where there is a combo of ions that form an insoluble compound TERM 10 Polar Molecule DEFINITION 10 Water is a polar molecule. The electrons in the water are not evenlydistributedover the molecule. Uneven distribution of negative and positive charges TERM 21 combination reaction DEFINITION 21 A + B ----> ABH2 + O2 -----> 2H2Oh2 is oxidized and o2 is reduced TERM 22 decomposition reaction DEFINITION 22 AB ----> A + B2 KClO3 -----> 2 KCl + 3 O2Cl has been reduced and oxygen has been oxidized TERM 23 single-replacement reaction DEFINITION 23 A + BC ----> AB + C2 Al + 6 HCl ------> 2 AlCl3 + 3 H2aluminum is oxidized and hydrogen is reduced TERM 24 titration DEFINITION 24 the known concentration of one solution is used to determine the unknown concentration of a second solution TERM 25 equivalence point DEFINITION 25 the number of moles of added base is stoichiometrically equivalent to the moles of acid being titrated TERM 26 standard solution DEFINITION 26 one whose concentration isaccuratelyknown TERM 27 how do you find the moles of HCl? DEFINITION 27 M (HCl) X V (HCl) = n (HCl) TERM 28 How can the molarity of NaOH be found? DEFINITION 28 M (NaOH) = moles NaOH volume (L) NaOH TERM 29 monoprotic DEFINITION 29 one ionizable hydrogen atom. 1:1 ratio TERM 30 diprotic DEFINITION 30 two ionizable hydrogen atoms TERM 31 molarity DEFINITION 31 concentration measured by the number of moles of solute per liter of solution TERM 32 gas discharge tubes DEFINITION 32 lamps can be made by passing high voltage electric current thought gas-filled glass tubes. The gas filled tubes are gas discharge tubes. Used for decorativepurposes---fluorescent coatings and colored glass provide a wide range of colors. TERM 33 Planck's Law DEFINITION 33 change in E=(hv)/cV(nu) = E2-E1 h= 6.626 X 10^-34 J/Hz c= 3.00 X 10^8 m/s h c= wavelength X frequency TERM 34 Rydberg Eqn DEFINITION 34 R= 0.0109737 nm^-1 TERM 35 Relationship between energy and frequency of light? DEFINITION 35 energy is directly proportional to the frequency of light TERM 46 interatomic distances DEFINITION 46 thedistancesbetween any pair of atoms (bonded or not) in a molecule TERM 47 ideal molecular geometry DEFINITION 47 a chemical structure in which the central atom in a molecule has no unshared electron pairs. Has a high degree of symmetry. TERM 48 isomers DEFINITION 48 compounds with the same molecular formula but different structural formulas. TERM 49 optical isomers DEFINITION 49 they can be detected using polarized light. mirror images of each other TERM 50 superimposible DEFINITION 50 identical models of each other TERM 51 nonsuperimposible DEFINITION 51 when you exchange a pair of atoms on one of the models but not the other TERM 52 chiral DEFINITION 52 mirror images. nonsuperimposible. asymmetric TERM 53 Charles' Law DEFINITION 53 for a fixed number of moles of a gas at constant pressure, volume is directly proportional to temperature. V1/V2 = T1/T2 TERM 54 Boyle's Law DEFINITION 54 for a fixed number of moles of gas at constant temperature, volume isinverselyproportional to pressure. P1V1=P2V2 TERM 55 Avogadro's Law DEFINITION 55 for a gas at constant temperature and pressure, volume is directly proportional to the number of moles of gas. V1/V2=n1/n2 TERM 56 ideal gas law DEFINITION 56 PV=nRTR=0.0821 L X atm/mol X K