General Chemistry Flashcards
What is Half life?
Zero Order: t=[reactants]/2K 2nd Order: t=1/k[Reactants]
What Ksp?
Solubility product When this is high most soluble
What does Diamagnetic mean?
Element that electrons are paired example in Hund’s rule
What is the difference between beta, alpha, and gamma decay?
Alpha Decay: atomic #-2 (z-2) and mass-4(a-4) Beta Decay: MOST PENETRATING atomic# -1(z-1) or atomic #+1(z+1) Gamma Decay: Nothing
What is Electrolysis
Redox RXN Need electron enegry to induce rxn Reduction is cathode Oxidation is the anode
What are elements are liquid at room temp?
BR2 and Hg, everything else solids but Cl, G, N,O and noble gases
What is Avogadro’s number?
6 x 10^23 molecules/moles
What is the standard enthalpy of formation for any element?
0
What is an Ionic compound?
Metal + Nonmetal, except NH4Cl
Name intermolecular forces form weakest to strongest?
London Dispersion, Dipole-Dipole, Hydrogen Bonding, Ionic bonding
Differences between Ionic compounds, molecular solid, and covalent bond networks
IC: High melting points MS: Low boiling points and held together by dispersion and d-d ex sugars, ice, sulfur CBN: stronger than ionic bonds ex diamond, graphite, asbestos
When dealing with rate law how does the balanced equation help?
It doesn’t
Which is stronger bond metalloid + nonmetal or nonmetal + nonmetal
Metalloid + Nonmetal
If temperature is the same, what does it mean for the molecules?
They all have the same average kinetic energy
Avogadro’s Law
All gases contain equal number of molecules at the same temperature and pressure
What is Hendreson Hasselback equation?
pH=pKa+ log base/acid
What is the Oxidation number of Oxygen, Elements, Hydrogen
H= +1 except hydrides=-1 e.g. LiH O= -2 except in peroxides= -1 Element= 0
Are Ionic compound molecules? What kind of array are they in?
No they are not molecules. They are in a crystal lattice.
What is the difference between polar and no polar bonds?
Nonpolar covalent bonds are a type of chemical bond where two atoms share a pair of electrons with each other. Polar covalent bonding is a type of chemical bond where a pair of electrons is unequally shared between two atoms.
What is the rate constancy?
.0821
What is the ideal gas law?
PV=nRT
Allotropes
Different forms of the same element
Oxidation Numbers of these molecules: PO4(Phosphate), KMnO4(permanganate),
PO4(Phosphate):-3 KMnO4(permanganate): -1
What is the temperature of and endothermic and exothermic RXN?
Endo: Lower Exo: Higher
Equation for taking a liquid to a gas
q=m(Delta)H make sure to divide mass by moles to get the correct units
Equation for pH and pOH
pH= -log[H+] pOH= -long[OH]
Specific Heat equation
(Delta)H=mc(delta)T C specific heat compacity
Gas Density Equation
P(MW)=DRT
Units for rate laws
1st order= sec^-1 2nd order= M^-1 sec^-1 Change the M^n to equal up to the rate order…basically add the exponents to equal the number of the rate order
VSPER(name EVERYTHING)
VSPER(Name just basic structures)
Explan Graphs of Rate order
*Nuclear decay is similar to 1st order
When a ion has a large - charge, what does that mean?
It has gained electrons causing it to increase in size
What is Aufbau principle?
determine the electron configuration of an atom, molecule or ion
Which elements are usually souble and insolube?
Solube: Group 1A metal, NH4, & NO3
Insouble: Ag, Hg, Pb, BaSO4, CaCO3
Oxidation Numbers of these molecules: HCO3(bicarbonate), NH4(ammonium)
HCO3(bicarbonate):-1 NH4(ammonium):+1
Oxidation Numbers of these molecules: C2H3O2(Acetate), NO2(Nitrite), ClO3(chlorate),
C2H3O2(Acetate):-1
NO2(Nitrite):-1
ClO3(chlorate):-1
Oxidation Numbers of these molecules: CLO4(Perchlorate), NO3(Nitrate), CH2O4(Oxalate),
ClO4(Perchlorate): -1
NO3(Nitrate): -1
CH2O4(Oxalate): -2
Oxidation Numbers of these molecules: Cr2O7(Dichromate), O2(Peroxide), OH(Hydroxide)
Cr2O7(Dichromate): -2
O2(Peroxide):-2
OH(Hydroxide):-1
Oxidation Numbers of these molecules:
SO3(Sulfite), SO4(Sulfate)
SO3(Sulfite):-2
SO4(Sulfate):-2
What is colligative properties?
Depends ONLY on # of particles in a solution, not solutes
ex: VP lowering, BP elevating
What is Molarity?
Moles of solute/Kg Solvent
Depends on temperature
What is the equation of find a boiling point or freezing point of molecule?
Boiling point-(Delta)T= Kb*m*i
freezing point- Boiling point-(Delta)T= Kf*m*i
*Take these and added to the correct tempearture of ºC
What is an equalibrium system?
OMIT solids and liquids from expression
K=Products/Reactants
When equation reversed(products to reactants)
Knew=(Koriginal)1/2
If reaction doubled= (K)2
What is an atom?
Basic Building block of Matter
smallest chemical unit of element
Explain Protons, neurtons, electrons
Atomic #(z)=Protons- + charge, 1 amu
Mass #- Atomic #= Neutrons, neutral, and a little bigger than protons
Atomic#= - charge, smalles, has calence elctrons
What are valence electrons?
Farthest from nucleucs= weaker attactiong
Able to leave and influence other atoms
Determin reactivity of atom
What is Atomic Mass Unit?
1.66 x10^-23 grams
What are isotopes?
Same # of protons but different neutrons
same # of + and -
Keeps chemical properties
What is Balmer Series?
4 wavelengths in visible region
upper leves of n
What is atomic Emission Spectra?
Most atoms in this state at room temp, but electrons ccan hbe excited to higher energy level and emit enegery as protons
What is the equation for Atomic Emission Spectra?
E=hc/lamda
H- Plank constant= 6.62606957 × 10-34 m2 kg / s
C= velocity of light= 3.0x10^8
Lamda= wavelength
What are the Quantum Number?
n, l, ml, ms
they explain the postiion and energy of electrons
What is Pauli exclusion principle?
No two electrons can have the same set of 4 quatum numbers
What is the principal quatam number?
N
the larger N is the energy level and radius
N max= 2n^2
What happens with shell energy with more distance from the radius?
they decrease in energy
enegry distance bw 4 &3 less than 1 & 2
What is the Azimuthal Number?
Angular momentum
l
subsells/sublevels
Intergers of l= 0-n-1
l=0(s),1(p),2(d), 3(f)
max # of electrons= 4l+2
What is Magnetic #?
Ml
Orbital region w/ in subshel may contain no more than 2 electrons
Ml= l to -l
Ml possible values= 2l+1
What are the orbitals of s, p, d, f?
s-1
p-3
d-5
f-7
What is Spin Number?
ms
Spin of particle is intristric angular momentum
Characteristic of particle
does NOT spin of axis
Spin orientation= +1/2 and -1/2
What is Hunds rule?
orbitals are filled by max number of half filled oritals with parallel spin
What effect do paired and unpaired electons have on molecules?
chemical and magnetic properties
What is paramagnetic?
unpaired electrons, magnetic field align the spin and attract atom
What is diamagnetic?
no unpaired electrons, slightly repelled by a magnetic field
How to find atomic radii?
Atomic radius decreases across period and inc down a group
What is ionization energy?
energy needed to remove electon form atom/ion
closer and tightly bound harder to remove
more energy to remove the 1st ionization energy
inc left ot right across period
dec down a group
group 1 lowest
What is elctron affinity?
Energy changes that occurs when elctron added
how easy an atom can accept electron
strong attaction greater electron affinity
What is electronegativity?
Attaraction an atom has for electons in a chemical bond
better for bonding, relates to ionization
inc form left ot right across period
decreasd down group
Properities of metals
Left and middle of table
solids at room temp except Hg
High MP & density
malleabality
ductitle
larger atomic radius
low ionization and elctroneg
good conduct of heat and electricity
G 1a IIa most reactive
Properties of nonmetals
Brittle at solid state
no metallic luster
high ionzation and electroneg
poor conductors of heat & electricity
upper right of periodic table
Properties of metalloids/semimetals
Zig zag line elements
varerity of properites
characteristics of metals and nonmetals
Good semiconductors
reavtive depending on element
Boron, Silicon, Germanium. Arsenic, Antimony, & Tellurium
What are alkali metals?
Group 1A, similar to metals
low densities
losely bounded elctron
largest radi
low ionzation and elctro negative
react w/ nonmetals and halogens
What aer alkaline earth
Group IIA
Smaller radi than alkali metals
2 electrons in outer shell
low electonegativity
What are halogens?
Group VIIA
highly reactive
gases, liquids and solid at room temp
high electronega
reactive with alkali and alkline earth metals
Waht are noble gases?
Inert gases
Group VIII
non reactive
low bp
gases at room temp
high ionzation
What are tranzaiton metals
Hard elements
High BP and MP
Across periods orbitals fill
low ionzation enrty
can lose numerous electrons
make complex ions with h2o or nonmetals
lower solubilites
What are the difference between ionic, covalent, and polar covalent bonds
I- electron is taken from low ionzation to another with high elect aff
C- electron pair shared
Polar- part covalent part ionic
What is ionic Bonding
Complete transfer of atom
Cation- lose elctron +
Anion gain electron -
High BP and MP
conduct eletricity in liquid and aq state
make crtstal lattice
What is Covalent bond
similar electronegative interaction
renergy required>energy relesased
weak intermolecular forces
low MP
Does not conduct electricity
What are the differences in Bond Length?
Short the better
shortest is triple bond
What is your center atom in Lewis structures?
least electronegative
end postion usually H, F, Cl, Br, I
What is formal charge equation?
V-1/2Nbonding - Nnonbonding
v= valence electrons
will determine best resonace structure
more negative the better resonace
Exception to octet rule
Atom Beyond III period
What is the differenct between nonpolar covalent and corrdinate covalent?
Nonpolar- b/w same electroneg, bond equal sharing, occurs in diatomic molecule(made with 2 atoms)
Coordinate- shared pair form lone paori of one atom
What are the shapes of s and p orbitals?
S orbital n=1, l=0 spherical symmetry
P orbital l=1 double shape
What is Dipole-Dipole?
+ region close to - region of another molecule
makes attractive forces
NOT in gas
High BP than nonpolar
What is Hydrogen Bonding?
Strong form of d-d
Bond w/ high electroneg atom
interatis w/ partial(-) chage of olther molecules
inc BP and hard to break enegry for it
ex H20,-OH, NH, COOH
What is Disperison Forces?
Equally shared covalent bonds has rapid polarization/ counter polarization of electron cloud
London forces- short lived dipoles
Weakest intermolecular force
Formula for Moles
Mol= weight of sample(g)/ molecular weight(g/mol)
What is equivalent weight?
Measure of reactive capacity
equivalent weight= wight of compouns/gram equivalent weight
What is gram equivalent weight?
determin the number of equivalents a compound contains
Molar mass/ n
n=# of Hs per molecule
What is the Law of constant compostion?
any sample of a give compound will contain smae element in identical mass ratio
What is empirical and molecular formula?
E- simplest whole # ration of elements
M- exact # of atomof each element
What is perecnt compostion?
Weight percent in specific compound
% compound= (mass of X informula/formula weight of compound) *100
What is combination reaction?
2+ reactants form 1 product
S + O2 to SO2
What is decmposition reaction?
One compound to 2+ substance
by heat or electrolysis
2HgO to 2Hg +O2
What is single displacement reaction?
Atom/ion replaced by another element
redox rxn
ZN + CuSO4 to Cu + ZnSO4
What is double displacement reactions?
metasthesis reaction
2 diffrent compouns displace each other make 2 new compounds
What is a net ionic equation?
Displacements use ions and can be rewritten into these
only show participating molecules
What is a spectator ion?
Don’t take part of overall reaction, but stay in solution
usually in displacement reaction
What is the equation for percent yield?
(actual yield/theroretical yield)*100
What is the defintiton of rate?
Disapparenc of reactants over time
appearnce of products over time
What is rate law?
Foward irreversible reaction
rate proportional to product of concentration to some power
Rate=K[A]^x[B]^y
What is zero order reactions?
Constant rate
indendent of reactant concentration
rate=K
unit=msec^-1
What are 1st order reactions?
rate proptional to one reactant concnetration
rate=k[A]
unit=sec^-1
What are 2nd order reaction?
rate porptional to 2 reactant or to sauware of concnetration of single reactant
rate=k[A]^2
unit: m^-1 sec^-1
What are height order reaction or mixed order reaction?
High= order 2+
Mixed= fractional order
What is the collision theory of chem kinetics?
Molecules must collide for reaction to occur
Rate of reaction is porption # of collison per second between reacting molecules
What is an effective collison?
Makes products
collide at correcto orientation
eable to break old bonds and form new bonds
What is activation energy/energy barrier?
min energty need for collison for a rxn to happen
What is the rate of reaction?
rate=fz
z=total number of collision per sec.
f=fraction of collison effective
What is the Transition State Theory
molecules collide with sufficient energy
old bonds weaken
new bonds form
dissociates into product and new bonds full form
What effects rate of reaction
Reactant concentration, tmep, medium and catalyst
How does reactant concentration affet the reaction rate?
High concentration high # of effective collision
all rates will increast but zero order
How does temperature affect rxn rate?
Rate will go up as temp rises
temp: avg kinetic energy
How does medium affet reaction rate?
aq solutions may speed it p
can be solid, liquid or gas
How do catalyst affect reaction rate?
Inc rxn w/o being consumed
lower activation energy
inc collison by changing orientation
reduce intrmolecular bonding
energy barrie lower
forces more toward equalibrium
What is the law of mass action
one step reaction
when two rates = each other
Kf=Kr[BC/A] basically products/reactants
Kc=equilibrium contant c=conentration p= pressure
What is reacation quotient?
Q
mesuare of degree to which a reaction has gone to completion
Qc=([CcDd]/[AaBb]
Qc=Kc constant at equalibrium
What are the properties of the equilibrium constant?
Pure solids and liquids not in the constanct
It is a given temp
Very large compared to 1, very little reactat compared to products
very small compared to 1, very little products compared to reactants
Close to 1, equal amounts reactants and products
What is Le Chatelier’s Principle
System to which stress is applied tends to change to releive the applied stress
effected by change in concentration, pressure, volume, and temperature
What is the effect of concentration in Le Chatelier’s Principle?
Inc reactact more products will be made
equlibrium shifts right
Decrease reactants will shift equlibrium toward reactants
What is the effect of pressure/ volume in Le Chatelier’s Principle?
Solid and liquid NOT effected
Pressure and volume invertedly related
High pressure low # of moles(reduces volume)-relieves stress
High Volume low pressure-shift toward products
What is the effect of temperture on Le Chatelier’s Principle?
Product: exothermic
Reactants: endothermic
Dec temp reaction to right
Inc temp reaction to left
Only one to change the value of the equlibrium constant
What is the Law of Conservation of Energy
states that the total amount of energy remains constant in an isolated system.
It implies that energy can neither be created nor destroyed, but can be change from one form to another.
What are the various system in thermochemistry?
Isolated-cannot exchange energy or matter
closed-can exchange but not matter
open-cahnge exvhange both matter and energy
What is a isothermal, adibatic, iosbric process?
Iso-temp constant
adibatic-no heat exchange occurs
iso-constant pressure
What is enthaply?
express hear changes at constant pressure
What is the change in enthaply?
heat absored or evolved by the system at constant pressure
It depend on intial and final
Hrxn=Hproducuts-Hreactants
H+ endothermic
H- exothermic
What is the enthaply standard heat formation?
enthalpy change that would occur if one mole of compound were formed directly from its element in ther standard states
elemnt is standard state=0
Hf
What is enthaply standard heat of reaction?
Hypothetical enthaply change that would occur if the reaction were carried out under standard condtions
=Sum of Hf products- Hf of reactants
What is Hess Law?
enthalpies of eactions are additive
What is Bond dissociation Energy in enthalpy?
average of energy requiresd to break a particular type of bond in one gaseous molecules
h=hbonds broken + hbonds formed
What is enthalpy heat of combustion?
usually fast and spontaneous and usally combustion
What is entropy?
measures disorder/randomness
units:energy/temp:J/k:cal/k
high order low entropy
low order high entropy
*sublimtaion greatest entropy change
What is the formula for entrop state fucntion?
S=Sfinal-Sintial
qrev/T
Qrev= heat added to system
T= absolute temperature
What is the standard entropy change for a reaction?
Sum of Sproduct-Sum of Sreactants
What is the second law of theromdynamics
All spontaneous process proceed such that entrop of the system plus it surrounds increae
Suniverse=Ssystem+Ssurroundings>0
What is Gibbs Free Energy?
Spontaneity of Reaction
combines two factors that affect the spontaneity of rxn;change in enthalpy and changes in entropy
What does (Delta)G mean?
Maximum amount of energy release by process. at constant tmeperature and presssure
(Delta)G= (Delta)H-T(Delta)S
What will be the reaction if (Delta)G is negative, postive, and zero?
Negaitive- spontaneous
Postive-not spontaneous
0-state of equilibrium
What would be the reactions for
(Delta)H (Delta)S
- +
+ -
+ +
- -
-+ spontaneous at all tem
+-nonspontaneous at all temperatures
++sponatneous only at high temp
-sponatneous only at low temp
If reaction nonspontaneous what will be the reverseal reactions
reversal will be sponatanous
What is standard free energy of (Delta)G?
Defined as the process occuring at 25c 1 atm pressure for which concentration of any solution invlver ar 1 mM
Most stable form 0
=sum of products-sum of reactants
What is the eaulibrium contant for (Delta)Grxn?
=-RTlnKeq
Keq-equilibrium constant, r-gas constant, t temp in K
What is the raction quotient in Gibbs Energy?
This happens after rxn starts
(Delta)G=(Delta)Gº+RTQ
What is STP?
Standard Temp and pressure of gases
273K
1atm
What is Boyle’s Law?
Gas at constant tempature
volume and pressure inversely proportional
What is the EQUATION for Boyle’s Law?
P1V1=P2V2
What is Charles and Gay-Lussac Law?
at constant pressure
volume gas directly porptional to absoulte temperature
What is avogadro’s principle?
Gass at constant temp and pressure
volume directly porptional to moles of gas present
can be used to kinetic rate law
What is the EQUATION for Charles law?
V1/T1=V2/T2
What is the EQUATION for avogadro’s principle?
N1/V1=N2/V2
What is the ideal gas law?
Shows relation bw pressure, volume, temp, and moles of gas
Ideal Gas Law equation
PV=NRT
R=gas constant=8.21x10-2 L*atm/mol*KJ=8.314 J/K*mol
How to find density of gas?
P(MM)/RT
V2=V1(P1/P2)(T2/T1)-can be used to find molar mass
d=m/V2
How are real gases effecte by pressure?
high pressure- molecules closer together until it becomes liquid
moderately-volume less bc of intermolecular attraction
extremely high-takes up more space!
What is the effect of tempurature of real gas?
low temp low velocity-attractive forece become important
Closer the gas is to BP less ideal it is
What is Dalton’s Law?
2+gases in one vessel w/o chem interation will be have independitly
Both exert partial pressure
How to find partial pressure?
Pa=PtxA
xA=Moles of A/total moles
What is the Kinetic Moleculear Theory of Gases?
Molecular behavior based on motion of individual molecules
Assumption 1 of kinetic moleular theory
Particles volumes are negligible compared to container volume
Assumption 2 of kinetic molecular theory
atoms/molecules exhibit no intermolecular attraction/repulstion
Assumption 3 of kinetic moleuclar theory
Continous, radom, collisons with other particles and container walls
Assumption 4 of Kinetic Molecular Theory
Collision between any 2 gases are elestic(no overall gain/loss of energy)
Assumption 5 of kinetic molecular theory
Average of Kinetic energy proptional to absolute temp and same for all gas at given
Kinetic Molecular Theory of Gases Equation
Kinetic Energy=1/2(mv2)=3/2(kT)
k=boltzmann constant=1.23x10-23
What is Maxwell-Boltzman Curve?
shifts right as temp inc
inc temp inc in speed
What is Graham’s law of Diffusion?
heavier gas molecule diffuse more slowly than lighter ones
differing avg speed
Equation Graham’s Law of Diffusion and Effusion
r1/r2=(MM2/MM1)1/2
r=diffusion rates
What is Graham’s law of Effusion?
Flow of gas particles under pressure from one compartement to another through a small opening
What is amorphous solid?
no ordered 3d arrangement, but molecules fixed into place
What is a crystalline?
possesse an order structure
3d arrangments
Properties of ionic solid
high BP and MP
poor electrical conductivity
strong electrostatic interaction
Properties of metallic solids
metals packed closed together
high MP and BP
strong covalent attraction
What is vapor pressure?
equalibrium bw evaporation adn condestion rates are equal
When does vapor presure increase?
when temperature increases
When vapor pressure of liquid = external pressure
boiling point
What is depostition?
gas to solid
What is Gibbs Function
thermodynatimic criterion for each above equilibria of gas-liquid, liquid-solid, gas-solid
What is the phase diagram
Define triple poitn and critical point of phase diagram
tp-phases at equilibrium
cp-temp and pressure no distinction bw liquid and gas
What is Raoult’s Law?
USe on of mixtures to get the relation of one in the souliton
find relationship betweek vapor pressure of vapor and concentraion of liquid
Raoult’s graph
What is equation for freezing/boiling point depression?
Kf*m
Kf=proportionality constanct
m=molality of solution
What is osmotic pressure?
Gives enough pressure to counterbalance the tendency to go through a membrane
depens on amount of solute
Equation for osmotic pressure
Π=MrT
M=molarity
r=idal gas constant
t=kevlin
In osmotic pressure what is dirrecly proptional
molarity and osmotic pressure
What is vapor-pressure lowering?
Similar to raoult’s law
solute add to pure solven vapor pressure decreases
Equation for Vapor pressure decrease
P=xbPºA
xb=mole raction of soulte B in solvent
xb=1-xa
P°a=vapor pressure of pure solvent
What is a non ionic solution?
solvation involves van der wals between solute and solvent
General Rule of solutions
inoic and polar souble in polar
nonpolar dissolve in nonpolar
What does saturated mean referring solutions?
when max added
solution at equlibrium
What does dilute mean referring to solutions?
propotion of solute:solvent small
releative term
What does concentrated mean referring to solution?
Proportion of solute to solvent large
Aqueous solution rule 1
Sals of alkali metal soulble in H2O
Aqueous solution rule 2
All ammounium salt H2O soluble
Aqueous solution rule 3
All chlorides, bromides, iodies soule in H2O
EXCEPT: Pb, Hg2, Ag
Aqueous solution rule 4
All salts of SO4 ion souble
Ca, Sr, Ba, Pb
Aqueous solution rule 5
MEtal oxides INSOULBE
except CaO, SrO, BaO
Aqueous solution rule 6
All Hydroxides insouble
except alkli metals, Ca, Sr, Ba
Aqueous solution rule 7
All carbonates, Phosphates, sulfides, and sulfites are insoulbe
exepte alkali metals and ammonium
Ending of element with lesser or greater charge
- ous lesser charge
- ic greater charge
Monatomic anions ending
-ide
Polyatmic anions(oxyanions)
Less oxygen -ite
more oxygen -ate
Four oxyanions prefix
Hypo-less oxygen
Per-more oxygen
Polyatomic anions that gain 1 or more H prefix
Hydrogen or dihydorgen
add in front of name
Ion charges on left of peroidc charges
usually positive
Ion charges on the right of the periodic table
usually negative ions
How are groups set up with ion charges/
usually the same
What are electrolytes?
electial conductivity of aq governed by precence and concentratio of ion in solution
How do strong electrolytes dissociates?
consitutent + ion
What are non electolytes
Compound that do no ionize in aq and retain molecular structure
limited solubility
What is an aquesus solution?
They dissolve in water
Equation for precent composition by mass
(Mass of solute/mass of solution)x100
Mole fraction equation
moles of compoiund/# of total moles of everything in system
What is molarity?
of moles solute per liter of solution
depend on volume of solution
What is molality
moles of solute/ kg of solvent
What is normality?
of gram equivalent weight
meausre reatvitiy of molecule
What is dilution
a solution is diluted in a solven
solvent added to a solution with high concnetration to get a lowere concnetration
Equation for dilution
MiVi=MfVf
M=molarty
V=volume
Solubility product constant
for ion and saturated solution
=[An+]m[Bm-]n
m and n are charges
Qsp>Ksp
precipitation will occur
Qsp-ion constant
Ksp-solubility constant
Qsp<ksp>
</ksp>
dissolution happen until soultion saturatied
Qsp=ion constant
Ksp=souilbility product constant
Qsp=Ksp
eqalibrium solution satureted
dissolves equal it preciptatin out of solution
General formula for slightly soulble salt MX3
MX3
Ksp=27x4
General formula for slighlty souble salt of MX2
Ksp=4x3
x= molar solubility
What factors affect solubility?
Temp of solution solvent
gasp phase solut is the pressure
other substances added
What is the common ion effect?
Example of Le Chateleir’s Principle
decution recation to solubility
if something is added to soultion
General formula of slightly soulble salt of general formmula MX
Ksp=x2
When anion becomes acid suffix?
-ide
Anion with a prefix of hydro acid end
-ic
Acids formed form oxyanions endings
called oxyacids
anion ending in -ite new ending is -ous
anion end in -ate ending is ic acid
How to measure dissaccocitaion of acid?
Ka= [product][product]/[HA]
HydrogenA+H2O-H30+A
Ka= acid dissociation constant
How to measure the dissociation of a base?
Kb=[B][OH]/[BOH]
What is hydrolysis?
reverse reaction salt ions react with water to give back the acid/ base
What is acid equivalent?
One mole of H+ ions
What is base equivalent?
equal to one mole of OH- ion
What does polyvalent?
each mole of acid/ base liberates more than one acid/base equivalent
Common polyvalent acids
H2SO4,
H3PO4
H2CO3
What is amphoteric or amphiprotic species?
One taht can act either as an acid/base, depending on its cehmical enviornment
example water
What is amphortic?
partially dissociated conjugate base of polyprotic acid
ex: HSO4, can gain or lose H
and hydroxides of cerain metals
What is a titration?
Prodedure used to determine the molarity of acid or base
What is equivalence point?
number of acids equivalents equals the number of base equivalents added
What is end point?
when the indicatior actually changs color
What is buffer solution
consistes of mixture of weak acid ann its salt
mixture of weak base and its salt
resist changes in pH
What does polyprotic acid mean
specific acids that are capable of losing more than a single proton per molecule in acid-base reactions
What are the oxidations of Group 1A and 2A
Group 1=+1
Group 2=+2
Oxidation number of group 7A in a compound
is -1
except with element higher electro negativity
Wht is half reaction method?
separte equation into two half reactions
oxidation part
reduction part
then add the needed H and e to each equation
What are the two types of electrochemical cells?
Galvanic cells/voltaci cells
electrolytic cells
What kind of reaction occurs in galvanic cell?
has negative G, so it is sponateous
negative pole of battery
What are half cells?
Separate by energy
What kind of reaction is in eletrolytic cells?
positive G
non spontaneos
postive pole of battery
What is Faraday’s Constant?
One elctron chargexby avagadors number
1F= 96,487 coulombs
Which direction does the electron go in a battery?
anode to cathode
What is Eº?
Standard reduction potential
What happens in high and low Eº?
high: greater tendency for reduction
low: greater tendency for oxidation
What is standard electromotive force?
Difference in potential between two half cells
emf/Eºcell
What does emf equal?
Eºred+Eºoxid
Equation of Emf and Gibbs Free energy
G=-nFECell
Effect of conecntraon on EMF
Nernst equation
Ecell=Eºcell-(RT/nF)(ln(reaction quotient))
HOw can emf be measeured?
By voltmeter
Realtionshp between EMF and the Equalibrium
G=-RTlnKeq
r=gas constant
nFEcell=RTlnKeq
What is mass defect?
Difference bw them protons and neurtons
What is fusion?
small nuclei combine to into large
What is fission?
Large nucleus splint into small nuclei
rarely spoontaeous
What are chain reations in reference to fissions?
neutrons cause them by splitting and they cause others neutrons to split causeing a chain reaction
What is Baryon number conservation?
the total number of neutons plus protons remains the same, even if neutrons converted to protons
Name some strong acids
HBr. HCl, HNO3, H2SO4, HClO4
What is Ka = to in acid/base equations?
Ka=Products/reactants
