Chapter 1-9 The Molecular Chemistry Survival Guide Introduction to Chemistry PDF

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t1jU±±t©U 1jɔ!t

¾ j1H!v¾1v¾± Ȑ

!ľĞŤŃơƭƙǔU±ƭƵėǔ!ľĞĐŘśŃơƭơ

ȑȑ

!ľĞŤŃơƭƙǔUU±ƭƵėǔ!ľĞĐŘśŃơƭơ

ȒȔ

±ŲśƵďŃśŃƭǔ¾óďśĞ

Ȓȕ

!ľĞŤŃơƭƙǔUHŲƙŤƵśó±ľĞĞƭ

ȓȖ

!ľĞŤŃơƭƙǔUUHŲƙŤƵśó±ľĞĞƭ

ȕȏ ©ĞĐŲŤŤĞŦėĞė©ĞơŲƵƙĐĞơ

1

BY MELISSA MARIBEL

Sgfca Fge  Dea Aa

2

3

Ac Sce  Ie

4

The Pedc Tabe  Ted

5

Nag Cd



6

Checa Reac

7

Eca  Meca Fa

8

Sche



9

Red Reac



10

Sb  Ne Ic Reac

11

Theche



12

Eec Cfga



Eecagec Sec

13

14

Le Sce



15

Gae



Ieeca  Iaeca Fce

16

17

S



18

Phae Daga  Heag Ce

Lace Eeg  U Ce

19

20

Meca Oba The

21

Ncea Che



22

CHEMISTRY II STUDY CHECKLISTS BY MELISSA MARIBEL

23

Kineic



24

Coodinaion Chemi

25

Cal Field Theo



LE CHATELIERS PRINCIPLE

26

27 

Eilibim

28

Solion Eilibia  Solbili

29

Acid  Bae



30

K a  K b  BUFFERS



31

Tiaion



32

Themodnamic



33

Elecochemi

I



34

Nclea Chemi



ŤĞśŃơơóŤóƙŃďĞśɔĐŲŤ

MELISSAMARIBELCOM

CHEMISTRY I FORMULA SHEET ATOMIC STRUCTURE

36 1

PERCENT ABUNDANCE

Atomic Number  Protons  Electrons

Average Atomic Mass   x mass   x mass

Charge  Atomic Number  Electrons Mass Number  Protons  Neutrons

ISOTOPE NOTATION

A Z

NAMING COVALENT MOLECULAR COMPOUNDS PREFIXES

X

1

mono

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

10

deca

A Mass Number Z Atomic Number X Chemical Symbol

COMMON POLYATOMIC IONS NH4

Ammonium

NO3

Nitrate

OH

Hydroxide

NO2

Nitrite

CN 

Cyanide  Acetate

CO 3

C 2H 3O 

BrO 3  IO 3 ClO4

 2

Bromate Iodate Perchlorate

2 2

CrO 4

Cr2 O 7 Dichromate 2

SO 4

2

SO 3

3

Chlorate

PO 4

ClO 

Chlorite

PO 3

ClO 

3

Hypochlorite

Chromate

2

ClO 3 2

Carbonate

Sulfate Sulfite Phosphate Phosphite

MELISSAMARIBELCOM

37 2

THE METRIC SYSTEM Name

Symbol

Number

Tera

T

10

Giga

G

10

Mega

M

106

Kilo

k

103

Hecto

h

10

Deka

da

10

Deci

d

10

Centi

c

10

Milli

m

10

Micro

µ

10

Nano

n

10

Pico

p

10

Femto

f

10

12 9

2

1

1

2 3 6 9

12 15

DIMENSIONAL ANALYSIS Length 1 in  254 cm

Mass 1 kg  2205 lb

Volume 1 mL  1 cm

1 mi  1609 km

1 lb  4536 g

1 L  1057 qt

1 m  10936 yd

1 oz  283495 g

Time 1 min  60 sec

3

1 hour  60 min

1 tbsp  14787 mL

1 mi  16093 m

1 hour 3600sec

1 gal  4 qt 1 L  1 dm3

1 ft  12 in

3

1 ft 28317 L

PERCENT ERROR Percent Error 

 actual value  experimental value  actual value

PERCENT YIELD Percent Yield 

actual yield theoretical yield

x 100

x 100

MELISSAMARIBELCOM

38 3 TEMPERATURE

DENSITY

Density 

Mass Volume

Kelvin to Celsius:

Celsius to Kelvin:

C  K  273

K  C  273

Celsius to Fahrenheit:

Common Units:

gmL

Fahrenheit to Celsius:

F   18 x C   32

C  056 F 32

3

gcm

THERMOCHEMISTRY Specific Heat Capacity

Specific Heat Capacity of Water

Heat Capacity

Cwater     4184 J gC

q mC T

qC T

Work

Internal Energy

Bomb Calorimetry qcal   Ccal   T

w P V

 E  q w or  U qw

q   q   

cal   

rxn

q

rxn

 E mol Coffee Cup Calorimetry q     q    metal

water

Formula Expanded    x Cwater    x T water      water mmetal     x Cmetal     x  Tmetal      m

ENERGY CONVERSION FACTORS 1 calorie cal 1 kilocalorie kcal

1 cal  4184 J 1 kcal  4184 J 6

1 kilowatthour kWh

1 kWh  360 x 10 J

1 kilojoule kJ

1 kJ  1000 J

MELISSAMARIBELCOM

39 4 ENTHALPY

BOHRS MODEL 18  E  2179 x 10 J   1       1   2 ni n2f



Standard Enthalpy of Formation H  n   H       n   H freactants f products Bond Energy

RYDBERGS FORMULA 7

ELECTROMAGNETIC SPECTRUM c λ

E 

n

c V

8

c  2998 x 10 ms



ni2

1 n2f



8

or 30x 10 ms 34

h  6626 x 10 Js

E hⱱ ⱱ c concentration molL V volume L

Number of Photons 

1



ELECTROMAGNETIC SPECTRUM CONSTANTS

hc λ

h λ mv

1

109737 x 10 m 1  λ hc

 H n   H       n   Hproducts reactants

ⱱ



1 J  1

kgm 2 s2

E given Ephoton

QUANTUM NUMBERS Principal n Size Energy of Orbital n1 2 3

Angular Momentum l

Magnetic m l 

Orbital Shape

OrbitalOrientation

l 0 1 2 3

ml  l to l

Angular Momentum l s

l 0

p

l 1

d

l 2

f

l 3

Spin ms  Spin of electron ms  12

MELISSAMARIBELCOM

40 5

OXIDATION NUMBERS Type

Example

Oxidation number

FORMAL CHARGES Formal Charge  Valence Electrons  Bonding Electrons  Individual Electrons

BOND ORDER

BondOrder 

Bonding electrons  Antibonding electrons

2

ELECTRON GROUPS Electron Groups  bonds  lone pairs

MELISSAMARIBELCOM

41 6 ELECTRON GEOMETRY ELECTRONGROUPS

ELECTRONGEOMETRY

2

Linear

3

Trigonal Planar

4

Tetrahedral

5

Trigonal Bipyramidal

6

Octahedral

HYBRIDIZATION ELECTRONGROUPS

2

ELECTRONGEOMETRY Linear

HYBRIDIZATION

sp

3

Trigonal Planar

sp 2

4

Tetrahedral

sp 3

5

6

Trigonal Bipyramidal

Octahedral

sp3d

3

sp d 2

MELISSAMARIBELCOM

42

MELISSAMARIBELCOM

43 8 DILUTIONS

MOLARITY

Molarity M 

M1 V 1  M 2V2

mol of solute

or

L of solution

C 1V1 CV 2 2

MASS PERCENT COMPOSITION

MOLALITY Molality m 

mol of solute kg of solvent

Mass  

PERCENT BY VOLUME

vv  

Volume of solute Volume of solution

grams of solute mL of solution

x 100

mass of solute mass of solution

mm  

mass of solute mass of solution

ppm 

9

6

x 10 mass of solution

x 10

x 100

PARTS PER MILLION PPM mass of solute

x 100

PARTS PERBILLIONPPB ppb

x 100

PERCENT BYMASS

PERCENT BYMASSVOLUME mv  

mass of element mass of compound

MELISSAMARIBELCOM

44 9 BOYLES LAW

GAYLUSSACS LAW

P1

P1 V1  P2 V2

T1

CHARLESS LAW

V 1 T1



V2

COMBINED GAS LAW

P1 V1 T1



n2 a V2

 x V nb  nRT

AVOGADROS LAW

P2 V2

V1

T2

n1

IDEAL GAS LAW

T2

VAN DER WAALS

P 

T2



P2



V2 n2

GAS CONSTANTS R  0 0 8 20 6 

 PV  nRT   0 0 8 21

L at m mo l K L at m mo l K

PRESSURE UNITS CONVERSIONS 1 at m  760 t o rr 1 at m  760  m m Hg 1 at m   10 13 0 0 Pa 1 at m   10 1 3 kPa 1 at m  14 7 ps i

STANDARD TEMPERATURE  PRESSURE STP

Pr ess ur e  1 a tm Te mpe ra tu re  27 3 K Vo lum e  22 4 L mo l

MELISSAMARIBELCOM

45 10 AVERAGE KINETIC ENERGY

RATE OF EFFUSION MB

Ra te of Ef fu si o n A

KE avg 

Ra te of Ef fu si o n B

n

3RT

HYDROSTATIC PRESSURE

CLAUSIUS CLAPEYRON EQUATION

P2

ln   P1

Hva p R H

RT

CAPILLARY RISE

h

2Tco s r g

PA



PB



PC

PA  XA PTo tal

ln P   va p  ln A

P Ae



PARTIAL PRESSURE

  1  1      T T  1 2

 Hv ap  R T

 2d s i n

DALTONS LAW

PT ot a l

p h g

RT

BRAGG EQUATION

ROOT MEAN SQUARE VELOCITY u rm s

3 2

MOLE FRACTION

XA 

mo le s o f g as A to tal mo le s i n g as mi xt ure

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46 11 UNIT CELLS

S IMP L E C U B IC 

A T O MS P E R C E L L : 1

B O DY C E N T E R E D CU B IC  B CC  

F A C EC E N T E R E D C UB IC  F CC  

A T O MS P E R C E L L : 2

A T O MS P E R C E L L : 4

l2 r

4r

l

3

l 2r 2

FREEZING POINT DEPRESSION

BOILING POINT ELEVATION

Tf  K fm

Tb  K bm

RAOULTS LAW o

P s olu tion X s olv en t P s olv en t P  X P A

o

A A

OSMOTIC PRESSURE

 MRT

HEATING CURVE FORMULAS

q mC T qn

Hfu s i o n

qn

H va p

HENRYS LAW

C g k P g

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CHEMISTRYII FORMULA SHEET

47 1

KINETICS

Zero Order

First Order

Second Order

rate  k

rate  kA

rate  kA2

M s1

rate law

Units of rate constant

M s1

s1

integrated rate law

At   kt  A 0

ln A   kt ln A 0 t

Relationship between slope and rate constant k

k   slope

k   slope

halflife

t

12

A 0



2k

1

1 A t

 kt 

1 A 0

k slope

t12  0693 k

t 12 

1 A0 k

RATE OF REACTION rate of appearance 

change in concentration of product

rate ofdisappearance  

product



time interval

change in concentration ofreactant time interval

t





reactant

t

ARRHENIUS EQUATION VARIATIONS

k

Ea Ae RT

1 E ln k    a    ln A T R

ln

1 1   E a           T2 T1 k2 R

k1

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ANIONIC LIGANDS

48 2

NEUTRAL LIGANDS

Symbol

Name

Symbol

Name

F

fluoro

H2O

aqua

Cl 

chloro

NH3

ammine

Br 

bromo

CO

carbonyl

I

iodo

NO

nitrosyl

CN 

cyano

py

pyridyl

NO3

nitrato

en

ethylenediamine

OH 

hydroxo

O2

oxo

2 C2 O4

oxalato

2

carbonato

CO 3

MONODENTATE LIGANDS PREFIXES

POLYDENTATE LIGANDS PREFIXES

2

di

2

bis

3

tri

3

tris

4

tetra

4

tetrakis

5

penta

5

pentakis

6

hexa

6

hexakis

METAL NAMES Anion Name

Ion Co3

Cation Name

Pt 2 Cu

platinum II copper I

cuprate I

Fe 3

iron III

ferrate III

Ag

silver I

cobalt III

cobaltate III platinateII

argentate I

Metal copper gold iron lead

Anion Name cuprate aurate ferrate plumbate

tin manganese

stannate manganate

nickel zinc chromium

nickelate zincate chromate

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49 3 SPECTROCHEMICAL SERIES CN



Strongest

oct  E 

hc λ

NO 2 en NH 3

8

8

or 30x 10 ms

c  2998 x 10 ms

C2 O42 H2 O

34

h  6626 x 10 J s

F Cl  Br  Weakest

Red 5n m

0

45

62

ge an 0 nm

7

w

7

Green

Ye

57

m 2n

e

7

59

49

Blu

5

nm

45

492577 nm

llo

Vio

Or

59

l et

620700 nm

40

I

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50 4

EQUILIBRIUM

productscoefficient Reaction Quotient Qc  

coefficient

reactants

concentration

K  QFavors Reactants K  Q At Equilibrium KQFavors Products

x Pproduct

Reaction Quotient Qp  

Px reactant

x  coefficient

pressure

K 1Favors Reactants K 1 At Equilibrium K1Favors Products Equilibrium Constant Kc  

productscoefficient reactantscoefficient

concentration x

Equilibrium Constant Kp   x  coefficient

Pproduct Q  Ksp Forms Precipitate

x

Preactant

 Q  Ksp NoPrecipitate Forms

pressure

Kp Kc RT

P  MRT

n

R 00821 n  moles of products  moles of reactants

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51 5

ACIDS  BASES

pH   log H

pOH   log OH 

pOH OH   10

pH H  10

14 ...