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Chemistry

ch. 4

Subject: 
Physics
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Chemistry
Chlorides
Metal halides
Bases
Equilibrium chemistry
Oxidizing agents
redox
Chemical equation
Lead(II) chloride
Iron(III) chloride
Precipitation
Hydrogen chloride

Chapter 4 Practice Test 1. A 20.0-g sample of HF is dissolved in water to give 2.0 ? 102 mL of solution. The concentration of the solution is: a) 1.0 M b) 3.0 M c) 0.10 M d) 5.0 M e) 10.0 M Ans: d) 5.0 M Page: 4.3 2. Which of the following aqueous solutions contains the greatest number of ions? a) 400.0 mL of 0.10 M NaCl b) 300.0 mL of 0.10 M CaCl2 c) 200.0 mL of 0.10 M FeCl3 d) 200.0 mL of 0.10 M KBr e) 800.0 mL of 0.10 M sucrose ANS: b) 300.0 mL of 0.10 M CaCl2 PAGE: 4.3 3. What mass of calcium chloride, CaCl2, is needed to prepare 2.850 L of a 1.56 M solution? a) 25.9 g b) 60.8 g c) 111 g d) 203 g e) 493 g ANS: e) 493 g PAGE: 4.3 4. What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4? a) 168 mL

CHEM 1A midterm 2 2012

Subject: 
Chemistry
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Chemistry
Equilibrium chemistry
Bases
Physical chemistry
PH indicators
Acids
Phenolphthalein
Weak base
Acid dissociation constant
Methyl orange
Hydrazoic acid
PH

Chemistry 1A, Fall 2012 Midterm Exam #2 October 17, 2012 (90 min, closed book) Name:__________________________________ SID:___________________________________ GSI Name:________________ Discussion Day/Time: ________________ ? The test consists of 5 short answer questions and 22 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes may not be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice (1-22) 2-7 88 Titration Short Answer 6 Soda (1) Short Answer 4 Soda (2) Short Answer 4 Ocean Acidification Short Answer 4 Indicators Short Answer 4 Total 110

CHEM 1A midterm 2 key

Subject: 
Chemistry
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Chemistry
Equilibrium chemistry
Bases
PH indicators
Acids
Physical chemistry
Phenolphthalein
Weak base
Methyl orange
Acid dissociation constant
Hydrazoic acid
Carbonate

Chemistry 1A, Fall 2012 Midterm Exam #2 October 17, 2012 (90 min, closed book) Name:_____________KEY____________________ SID:___________________________________ GSI Name:________________ Discussion Day/Time: ________________ ? The test consists of 5 short answer questions and 22 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes may not be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice (1-22) 2-7 88 Titration Short Answer 6 Soda (1) Short Answer 4 Soda (2) Short Answer 4 Ocean Acidification Short Answer 4 Indicators Short Answer 4 Total 110

CHEM 1A midterm 2

Subject: 
Chemistry
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Chemistry
Equilibrium chemistry
Bases
Acid-base chemistry
Acids
Inorganic solvents
Tannic acid
Acid dissociation constant
Caffeine
Ammonia
PH
Buffer solution

Chemistry 1A, Fall 2011 Midterm Exam #2 October 18, 2011 (90 min, closed book) Name:__________________________________ SID:___________________________________ GSI Name:________________ ? The test consists of 4 short answer questions and 23 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes will NOT be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice 2-8 76 Cabbage juice 2 6 Kitty Litter 3 6 Nicotine 5 4 Caffeine 7 8 Total 100

CHEM 1A midterm 1 key

Subject: 
Chemistry
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Chemistry
Equilibrium chemistry
Bases
Acids
Smoking
Acid-base chemistry
Acid dissociation constant
Nicotine
Tannic acid
Caffeine
PH
Buffer solution
health

Chemistry 1A, Fall 2011 Midterm Exam #2 October 18, 2011 (90 min, closed book) Name:__________________________________ SID:___________________________________ GSI Name:________________ ? The test consists of 4 short answer questions and 23 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes will NOT be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice 2-8 76 Cabbage juice 2 6 Kitty Litter 3 6 Nicotine 6 4 Caffeine 8 8 Total 100 Useful Equations and Constants: pH = - log[H+] pX = - log X X = 10-pX Kw = 1?10-14 at 25?C PV = nRT ][ ][ log HA A pKpH a ?

CHEM 1A midterm 1

Subject: 
Chemistry
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Chemistry
Functional Groups
Antiseptics
Chemical bonding
Monomers
Superhard materials
Properties of water
Ether
Boron
Vapor pressure
Allene
Boiling point

Chemistry 1A, Fall 2012 Midterm Exam #1 September 19, 2012 (90 min, closed book) Name:__________________________________ SID:___________________________________ GSI Name:________________ Discussion Day/Time: ________________ ? The test consists of 4 short answer questions and 17 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes may not be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice (1-17) 2-6 51 Ethylene Glycol Short Answer 3 4 Boron Nitride Short Answer 4 4 Allene Short Answer 5 4 Cyanogen Short Answer 5 7 Total 70 Useful Equations and Constants: PV = nRT

CHEM 1A midterm 1

Subject: 
Chemistry
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Chemistry
DuPont
Synthetic fibers
Reducing agents
Hydrogen bond
Supramolecular chemistry
Kevlar
Properties of water
Hydrogen
Formamide
Formic acid
Nylon
Technology

Chemistry 1A, Fall 2011 Midterm Exam #1 September 20, 2011 (90 min, closed book) Name:__________________________________ SID:___________________________________ GSI Name:________________ ? The test consists of 4 short answer questions and 18 multiple choice questions. ? Put your written answers in the boxes provided. Answers outside the boxes may not be considered in grading. ? Write your name on every page of the exam. Question Page Points Score Multiple Choice (1-18) 2-7 55 Formic acid Short Answer 3 8 Hydrogen Storage Short Answer 3 4 Capsaicin Short Answer 5 4 Rubber Short Answer 7 4 Total 75 Useful Equations and Constants: PV = nRT

Chapter 10

Subject: 
Chemistry
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Chemistry
Thermodynamic properties
Chemical engineering
Materials science
Phase transitions
Enthalpy
Enthalpy of vaporization
Vapor pressure
Phase
Enthalpy of fusion
Dipole
Evaporation

Chapter 10 notes Claire Rafson 10.1-10.2 Intermolecular forces- occur b/w not in molecules. From solid to liquid to gas molecules remain in tact Forces: Dipole-dipole forces are forces that act between polar molecules Hydrogen bonding- strong form of dipole dipole with H and NOF London Dispersion- Present in all but ionic . noble gas and nonpolar and Polar. Big atom with a lot electrons LD can be stronger than dipole dipole Higher IMF = higher: surface tension, boiling/meltin point. Lower: vapor pressure Capillary action- polar liquids typically exhibit it 10.3- crystalline solids- highly regular arrangement of their components ionic and molecular amorphous solids- considerable disorder 10.5- Network atomic Solids- giant molecule Strong covalent bonds Silica- SiO2

Chapter 8

Subject: 
Chemistry
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Chemistry
Chemical bonding
Chemical bond
Valence electron
Lewis structure
Octet rule
Covalent bond
Ionic bond
Hydrogen bond
Lone pair
Formal charge
electron
Technology

Claire Rafson Chapter 8 Notes 8.1- Bond Energy- The strength of a bonding interaction. The energy required to break the bond. Why do bonds occur? So the system can achieve the lowest possible energy by behaving in this way. Ionic bonding- electrostatic attractions of the closely packed, oppositiyly charged ions. Ionic compound- Metal reacts with a nonmetal Coulombs law- interaction between pair of ions. E= (2.31X 10^-19 J* nm) (Q1Q2/r) A bond will form if the energy of the aggregate is lower than that of the separated atoms. Covalent bonds- type of bonding in which electrons are shared by nuclei. (i.e Hydrogen bonding) Polar Covalent Bond- Atoms are different enough that they have unequal sharing results. 8.2-

Chapter 7

Subject: 
Chemistry
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Chemistry
Physics
Atomic physics
Quantum chemistry
atoms
Molecular physics
Theoretical chemistry
electron
Energy level
Atomic orbital
Azimuthal quantum number
Aufbau principle
Technology

Claire Rafson Chapter 7: Atomic Structure and Periodicity 7.1- 7.3 Wavelength and frequency are inversely related C= speed of light = 2.9979 X 10^8 m/s Photoelectric effect- Einstein. Phenomenon in which electrons are emitted from the surgace of a metal when light strikes it. E=mc^2 ?. M= mass Dual nature of light Diffraction- light is scattered from a regular array of points or lines. Change in E= hv 7.4- quantum model- made by Bohr. Model for the hydrogen atom. Electron in a hydrogen atom moves around the nucleus only in certain orbits. Ground state- lowest possible energy state. 7.5- quantum mechanical model- Heisenberg, Broglie, and Schrodinger probability distribution- intensity of color is used to indicate probability value near a given point in space. 7.6-

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