- Page 5 and 6: CHEMISTRY
- Page 7 and 8: the complete high school study guid
- Page 9 and 10: In each chapter, you’ll find the
- Page 11 and 12: UNIT 3:ATOMIC THEORY ANDELECTRON CO
- Page 13: UNIT 10:ACIDS AND BASES 38328. Prop
- Page 16 and 17: Chapter 1INTRODUCTIONTO CHEMISTRYWH
- Page 18 and 19: TYPES OF CHEMISTRYChemistry has dif
- Page 20 and 21: Background research involves review
- Page 22 and 23: The scientific process isn’t alwa
- Page 24 and 25: SCIENTIFIC THEORIESAND LAWSAfter co
- Page 26 and 27: LAWA rule based on observation of a
- Page 28 and 29: 1. Chemistry is the branch of scien
- Page 30 and 31: Chapter 2CONDUCTINGEXPERIMENTSDESIG
- Page 32 and 33: A VARIABLE is a factor thatcan alte
- Page 34 and 35: COLLECTING DATAGood data is specifi
- Page 36 and 37: LINE GRAPHS show the relationship b
- Page 38 and 39: DRAWING CONCLUSIONSYou have reached
- Page 40 and 41: 1. Data is either quantitative, in
- Page 42 and 43: formed. This allowed the knowledge
- Page 44 and 45: CONCLUSION/EVALUATION: Presents a s
- Page 46 and 47: SYSTEMATIC ERRORSA systemic error a
- Page 50 and 51: CALCULATING PERCENT ERRORPERCENT ER
- Page 52 and 53: 1. As a scientist, it’s important
- Page 54 and 55: Chapter 4MEASUREMENTThe Internation
- Page 56 and 57: DIMENSIONAL ANALYSISDIMENSIONAL ANA
- Page 58 and 59: If you have something measured in k
- Page 60 and 61: If you go to the moon, you will sti
- Page 62 and 63: moleculesstop movingcompletelyPRESS
- Page 64 and 65: Rules for Significant Figures1.All
- Page 66 and 67: DIFFERENT ACCURACIESWhat happens wh
- Page 68 and 69: 1. Mass is the amount of matter in
- Page 70 and 71: Chapter 5LAB SAFETY ANDSCIENTIFIC T
- Page 72 and 73: Don’t eat, drink, or chew gum in
- Page 74 and 75: When Working with ChemicalsRead eve
- Page 76 and 77: SAFETY SHOWER : Use only ifa chemic
- Page 78 and 79: An ERLENMEYER FLASK looks like abea
- Page 80 and 81: A PIPETTE is a long, thin tube with
- Page 82 and 83: WEIGHING BOAT ORWEIGHING PAPER is u
- Page 84 and 85: 1. Safety first! Always pay attenti
- Page 86 and 87: 72
- Page 88 and 89: Chapter 6PROPERTIES OFMATTER ANDCHA
- Page 90 and 91: EXTENSIVE AND INTENSIVE PROPERTIESP
- Page 92 and 93: REACTIVITY: the likelihood of a sub
- Page 94 and 95: FOR EXAMPLE: Burning a logchanges i
- Page 96 and 97: w1. How is a physical property diff
- Page 98 and 99:
1. You can see, touch, smell, hear,
- Page 100 and 101:
Chapter 7STATES OFMATTERSTATES OF M
- Page 102 and 103:
A LIQUID is a substance that flows
- Page 104 and 105:
COMPRESSIBILITYMeasures the change
- Page 106 and 107:
CONDENSATION is the opposite of vap
- Page 108 and 109:
A phase diagram is usually set up s
- Page 110 and 111:
A SOLID is on the lower left end of
- Page 112 and 113:
1. The state of an object is not al
- Page 114 and 115:
Chapter 8ATOMS, ELEMENTS,COMPOUNDS,
- Page 116 and 117:
A NEUTRAL ATOM (an atom without an
- Page 118 and 119:
COMPOUNDS AND MIXTURESA COMPOUND is
- Page 120 and 121:
If you’re talking about a pizza,
- Page 122 and 123:
EXTRACTION is the actof isolating o
- Page 124 and 125:
1. Matter is anything that has mass
- Page 126 and 127:
112
- Page 128 and 129:
Chapter 9ATOMICTHEORYTHEORY DEVELOP
- Page 130 and 131:
Dalton’s theory didn’t get ever
- Page 132 and 133:
Atoms are made of mostly empty spac
- Page 134 and 135:
Because Rutherford knew the charge
- Page 136 and 137:
1. John Dalton2. True. They have di
- Page 138 and 139:
HUH?!The units of measurement for a
- Page 140 and 141:
The Electromagnetic SpectrumWavelen
- Page 142 and 143:
A quantum is like a penny. Apenny i
- Page 144 and 145:
However, the energy of the light mu
- Page 146 and 147:
So that means:A photon = a quantumP
- Page 148 and 149:
1. Quantum theory explains the beha
- Page 150 and 151:
Chapter 11THEPERIODIC TABLEDifferen
- Page 152 and 153:
123456711HHydrogen1.00783LiLithium6
- Page 154 and 155:
In many cases, the letters in a che
- Page 156 and 157:
NEUTRAL ELEMENTS,ISOTOPES, AND IONS
- Page 158 and 159:
ISOTOPESISOTOPES are atoms of the s
- Page 160 and 161:
Hydrogen has three isotopes:Protium
- Page 162 and 163:
A positively charged ion (+), or CA
- Page 164 and 165:
1. There are 118 known elements.2.
- Page 166 and 167:
Elements in the periodic table are
- Page 168 and 169:
1HHydrogen1.00783LiLithium6.94111Na
- Page 170 and 171:
FAMILIES INTHE PERIODIC TABLEA fami
- Page 172 and 173:
ALKALI METALSElements in this group
- Page 174 and 175:
What about the two rows of elements
- Page 176 and 177:
Atomic RadiusATOMIC RADIUS is a mea
- Page 178 and 179:
Ionic radius INCREASES for nonmetal
- Page 180 and 181:
FOR EXAMPLE: Two elements of chlori
- Page 182 and 183:
RecapTrends in the periodic tableTr
- Page 184 and 185:
1. The periodic table is governed b
- Page 186 and 187:
Chapter 13ELECTRONSENERGY LEVELSThe
- Page 188 and 189:
Electrons in the outermost energy l
- Page 190 and 191:
The most likely place to find a pho
- Page 192 and 193:
1. When an electron moves from a hi
- Page 194 and 195:
Chapter 14BONDINGCHEMICAL BONDSWhen
- Page 196 and 197:
Atoms bond to complete their outer
- Page 198 and 199:
Nonmetal atom + electron (e - ) ➜
- Page 200 and 201:
Ammonium hydroxide is a neutral com
- Page 202 and 203:
FOR EXAMPLE: Determine how ions bon
- Page 204 and 205:
A crystal lattice may be drawnlike
- Page 206 and 207:
BUT, if you had two Cl ions, they w
- Page 208 and 209:
The easiest way to see how covalent
- Page 210 and 211:
How to Draw a Lewis Dot Diagramfor
- Page 212 and 213:
Oxygen (O 2 ) forms a diatomic mole
- Page 214 and 215:
Hydrogen bonds with itself to have
- Page 216 and 217:
1. The octet rule states that eleme
- Page 218 and 219:
Chapter 15VALENCE SHELLELECTRON PAI
- Page 220 and 221:
How the Structures Are FormedAtoms
- Page 222 and 223:
In a polar covalent bond, the side
- Page 224 and 225:
This drawing of hydrogen chloride (
- Page 226 and 227:
In the model, the straight bondsare
- Page 228 and 229:
The geometric shape, which is linea
- Page 230 and 231:
1. Molecular geometry is the three-
- Page 232 and 233:
Chapter 16METALLIC BONDSANDINTRAMOL
- Page 234 and 235:
TYPE OF BONDCOVALENT METALLIC IONIC
- Page 236 and 237:
Intermolecular forces from weakest
- Page 238 and 239:
The two hydrogen-positive dipoles w
- Page 240 and 241:
INTERMOLECULAR FORCESAND STATES OF
- Page 242 and 243:
You can also use the electronegativ
- Page 244 and 245:
1. Metallic bonds are formed when t
- Page 246 and 247:
Chapter 17NAMINGSUBSTANCESChemical
- Page 248 and 249:
The Roman numerals match the number
- Page 250 and 251:
BINARY COMPOUNDS are created whentw
- Page 252 and 253:
The information is in the periodic
- Page 254 and 255:
A TERNARY SALT is a compound made u
- Page 256 and 257:
TERNARY ACIDS are acids formed from
- Page 258 and 259:
NAMING MOLECULARCOMPOUNDSMolecular
- Page 260 and 261:
CALL MESTANNIC.CALL MESTANNOUS.246
- Page 262 and 263:
1. Iron (III) ion OR ferric ion, le
- Page 264 and 265:
The number of atoms in 12 grams (g)
- Page 266 and 267:
FOR EXAMPLE: What is the mass of a
- Page 268 and 269:
2 (atomic mass H) + 1 (atomic mass
- Page 270 and 271:
Calculating GramsYou can convert to
- Page 272 and 273:
1 mol of CO 2 has 1 mol carbon atom
- Page 274 and 275:
Using Molecular Massto Calculate Mo
- Page 276 and 277:
1. The number of atoms in 1 mol of
- Page 278 and 279:
To find the percent composition,1.
- Page 280 and 281:
Hint:Add all of the percentagesof e
- Page 282 and 283:
FINDING THEEMPIRICAL FORMULAAn EMPI
- Page 284 and 285:
Round to the nearest whole number.1
- Page 286 and 287:
1. Percent composition of a compoun
- Page 288 and 289:
Chapter 20CHEMICALREACTIONSCHEMICAL
- Page 290 and 291:
The chemicals on the left side of t
- Page 292 and 293:
Steps for balancingchemical equatio
- Page 294 and 295:
5. Multiply the element or compound
- Page 296 and 297:
TYPES OF CHEMICALREACTIONSSYNTHESIS
- Page 298 and 299:
DOUBLE REPLACEMENT/METATHESIS: Two
- Page 300 and 301:
FOR EXAMPLE: Potassium bromide reac
- Page 302 and 303:
1. Scientists use chemical equation
- Page 304 and 305:
Chapter 21CHEMICALCALCULATIONSScien
- Page 306 and 307:
DIMENSIONAL ANALYSISA problem-solvi
- Page 308 and 309:
Mass (g) of compound A(periodic tab
- Page 310 and 311:
716.0 g CO 2 is created from 236.5
- Page 312 and 313:
To solve mass-to-volumestoichiometr
- Page 314 and 315:
Known: 12.3 L H 2 gasSulfuric acid
- Page 316 and 317:
EXCESS REAGENTReactants that are le
- Page 318 and 319:
In reactions occurring in an actual
- Page 320 and 321:
56 g H 2 SO 4 × 1 mol H 2SO 498.08
- Page 322 and 323:
1. Stoichiometry is the quantitativ
- Page 324 and 325:
310
- Page 326 and 327:
Chapter 22COMMON GASESIDENTIFYING C
- Page 328 and 329:
Common Gases at Room TemperatureH 2
- Page 330 and 331:
FOR EXAMPLE: If you have a balloon
- Page 332 and 333:
EVANGELISTA TORRICELLI (1608-1647)w
- Page 334 and 335:
1. Gases are less dense, have molec
- Page 336 and 337:
Principles that compriseKinetic Mol
- Page 338 and 339:
Collision of Gas ParticlesTemperatu
- Page 340 and 341:
1. Gases constantly move in straigh
- Page 342 and 343:
As the pressure on a gasAs the pres
- Page 344 and 345:
V ~ T, assuming that pressure and a
- Page 346 and 347:
P ~ T, assuming that volume and amo
- Page 348 and 349:
The formula for the combined gas la
- Page 350 and 351:
AVOGADRO’S LAWItalian scientist A
- Page 352 and 353:
The gas particles have no forces ac
- Page 354 and 355:
FOR EXAMPLE: A sample of nitrogen g
- Page 356 and 357:
FOR EXAMPLE: Calculate the density
- Page 358 and 359:
P ETHANE = nRT V=(7.93 mol) (.0821
- Page 360 and 361:
1. Gas laws describe the movement a
- Page 362 and 363:
Chapter 25SOLUBILITYSOLUBLE VS INSO
- Page 364 and 365:
Things to know!Aqueous solution: a
- Page 366 and 367:
The molecules within the solid sucr
- Page 368 and 369:
FOR EXAMPLE: Carbon dioxide (CO 2 )
- Page 370 and 371:
There are four typesof colloids:SOL
- Page 372 and 373:
Oil-and-vinegar suspension: The lar
- Page 374 and 375:
1. A substance that is soluble will
- Page 376 and 377:
PRECIPITATION REACTIONS are one of
- Page 378 and 379:
SOLUBILITY RULESSolubility rules he
- Page 380 and 381:
ELECTROLYTIC PROPERTIESSolutes in a
- Page 382 and 383:
Pressure affects gases when mixed w
- Page 384 and 385:
1. Dissociation of ions occurs when
- Page 386 and 387:
Chapter 27CONCENTRATIONSOF SOLUTION
- Page 388 and 389:
MOLALITY gives you the number of mo
- Page 390 and 391:
FOR EXAMPLE: Calculate the molality
- Page 392 and 393:
DILUTIONSChemists sometimes need to
- Page 394 and 395:
Start with the NaCl because that is
- Page 396 and 397:
1. Concentration tells you the amou
- Page 398 and 399:
Chapter 28PROPERTIESOF ACIDS ANDBAS
- Page 400 and 401:
Hydrogen (H + ) is also called a pr
- Page 402 and 403:
reacts with certain metals to produ
- Page 404 and 405:
Carbonates and hydrogen carbonates:
- Page 406 and 407:
1. Acids are substances that dissoc
- Page 408 and 409:
Common Substancesand Their pH Value
- Page 410 and 411:
Chemists use logarithms for pH beca
- Page 412 and 413:
FOR EXAMPLE: The concentration of a
- Page 414 and 415:
But when sulfuric acid is added int
- Page 416 and 417:
pH in our livesSome plants, like ra
- Page 418 and 419:
1. pH is a measure of hydrogen ions
- Page 420 and 421:
When you put them together, that cr
- Page 422 and 423:
OH - accepts a proton in the revers
- Page 424 and 425:
The formula to find K a:K a = [prod
- Page 426 and 427:
w1. What is the difference between
- Page 428 and 429:
1. Arrhenius acids are substances t
- Page 430 and 431:
The burette contains the solution o
- Page 432 and 433:
Titration stoichiometry can be summ
- Page 434 and 435:
1. A titration is an experiment per
- Page 436 and 437:
422
- Page 438 and 439:
Chapter 32CHEMICALEQUILIBRIUMCHEMIC
- Page 440 and 441:
ACID-BASE REACTIONSWeak acids and b
- Page 442 and 443:
In this equation, water moves from
- Page 444 and 445:
Dinitrogen tetraoxide (N 2 O 4 ) is
- Page 446 and 447:
K b = base dissociation constant =
- Page 448 and 449:
Because solids are not included in
- Page 450 and 451:
FOR EXAMPLE: At the start of this r
- Page 452 and 453:
ConcentrationIn this graph, morerea
- Page 454 and 455:
1. Chemical equilibrium is a dynami
- Page 456 and 457:
Chapter 33LE CHÂTELIER’SPRINCIPL
- Page 458 and 459:
What happens if you remove C from t
- Page 460 and 461:
The beakers below illustrate the re
- Page 462 and 463:
What happens if you decrease the te
- Page 464 and 465:
1. Le Châtelier’s Principle stat
- Page 466 and 467:
Chapter 34THE FIRST LAW OFTHERMODYN
- Page 468 and 469:
Almost every chemical reaction abso
- Page 470 and 471:
To calculate the heat change, you n
- Page 472 and 473:
This graph shows the phase changes
- Page 474 and 475:
ENTHALPYScientists have developed a
- Page 476 and 477:
1. Balance the equation.P 4(s) + 5O
- Page 478 and 479:
When you are working with equations
- Page 480 and 481:
FOR EXAMPLE: Calculateof methane.H
- Page 482 and 483:
1. Reverse the second equation so t
- Page 484 and 485:
1. The Law of Conservation of Energ
- Page 486 and 487:
Chapter 35THE SECOND LAW OFTHERMODY
- Page 488 and 489:
Things to know!Solids have the most
- Page 490 and 491:
FOR EXAMPLE: Calculate the standard
- Page 492 and 493:
If you want to know the standard-st
- Page 494 and 495:
1. Gibbs free energy ( G) is used t
- Page 496 and 497:
Common reaction ratesand their spee
- Page 498 and 499:
Reaction rates can be graphed. A re
- Page 500 and 501:
Different ways that collisions can
- Page 502 and 503:
CATALYST A catalyst is a substance
- Page 504 and 505:
Activation energy is also related t
- Page 506 and 507:
FOR EXAMPLE: In the reaction NO 2 +
- Page 508 and 509:
1. The reaction rate is the change
- Page 510 and 511:
mass-to-massstoichiometry, 292-296m
- Page 512 and 513:
gloves, 57graduated cylinders, 65gr
- Page 514 and 515:
isotopes, 144-147neutral elements,
- Page 516:
Vvalence electrons, 156, 174, 181va