Studied by 15 peopleMetal + Acid > ?
example reactants: Mg(s) + HCl(aq) > ?
Salt + Hydrogen gas
example products: MgCl2 + H2 (g)
Metal + HOT water (steam) > ?
example reactants: Mg(s) + H2O(g) > ?
Metal oxide + Hydrogen gas
example products: MgO (s) + H2 (g)
Metal + COLD water > ?
Metal hydroxide + Hydrogen gas
IODIFORM TEST
Methyl ketone + 3 I2 + 4 NaOH > ?
Carboxylate + 3 NaI + 3 H2O + CHI3 (IODIFORM; YELLOW PPT)
IONIC period 3 chloride + Water > ?
example reactants: NaCl(s) + H2O > ?
NEUTRAL SOLUTION of ions
example products: Na+ (aq) + Cl- (aq)
COVALENT period 3 chloride + Water > ?
ACIDIC SOLUTION, white fumes of HCl
PCl5 (s) + 4H2O (l) > ?
H3PO4 (aq) + 5HCl (g)
SiCl4 (l) + 2H2O (l) > ?
SiO2 (s) + 4HCl (g)
Na2O (s) + H2O (l) > ?
2 NaOH (aq)
MgO (s) + H2O (l) > ?
Mg(OH)2 (s)
SiO2 (s) + HOT 2 NaOH (aq) > ?
Na2SiO3 (aq) + H2O (l)
SO2 (g) + H2O (l) > ?
H2SO3 (sulfurous acid) (aq)
SO3 (g) + H2O (l) > ?
H2SO4 (sulfuric acid) (aq)
P4O10 (g) + 6 H2O > ?
4 H3PO4 (phosphoric acid) (aq)
Carboxylic acid + NaOH (any strong base) > ?
carboxylate + H2O
carboxylic acid + K2CO3 (weak base) > ?
carboxylate + H2O (l) + CO2 (g)
carboxylic acid + Na (s) > ?
carboxylate + hydrogen gas
alcohol + Na (s) > ?
carboxylate + hydrogen gas
carboxylic acid + LiAlH4 (in dry ether) > ?
alcohol + H2O
PRIMARY alcohol + acidified K2Cr2O7/hot acidified KMnO4 (oxidizing agent) > ?
carboxylic acid (aldehyde if distilled after first oxidation) + H2O
SECONDARY alcohol + acidified K2Cr2O7/hot acidified KMnO4 (oxidizing agent) > ?
ketone + H2O
TERTIARY alcohol + acidified K2Cr2O7/hot acidified KMnO4 (oxidizing agent) > ?
no reaction
dehydration of alcohol
alcohol (H2SO4 (conc., reflux, 180˚C) > ?
alkene + H2O
mole (definition)
the amount of substance which contains 6.02×10²³ particles (atoms, ions, molecules, electrons, formula units)
Avogadro’s constant (definition)
the number of particles equivalent in a mole of those particles. 6.022 × 10²³ PARTICLES(atoms+ions) FORMULA UNITS(ionic) MOLECULES(covalent)
unified atomic mass unit (definition)
one twelfth of the mass of a carbon-12 atom
Relative atomic mass (definition)
the weighted average mass of atoms of an element to the unified atomic mass unit. Unit is g/mol
relative formula mass (definition)
the weighted average mass of one formula unit (ionic compound) compared to the value of the unified atomic mass unit. Unit is g/mol
relative molecular mass (definition)
the weighted average mass of a molecule in a given sample for that molecule compared to the value of the unified atomic unit. for covalent compounds. unit is g/mol
Atomic number (definition)
number of protons in the nucleus of an atom
Nucleon number (definition)
Sum of the protons and neutrons in the nucleus (mass number)
Isotopes (definition)
atoms with the same number of protons but different numbers of neutrons
S orbital (shape)
sphere
P orbital (shape)
dumb-bell
electron configuration
1s2s2p3s3p4s3d4p4d4f
elect config of chromium
[Ar]4s^1 3d^5
elect config of copper
[Ar]4s^1 3d^10
First Ionization energy (definition)
the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive one ions.
Second ionization energy (definition)
the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous positive two ions.
first ionization energy equation
sodium ex. ~ Na(g) > Na+ (g) + e-
second ionization energy equation
Na+ (g) > Na(2+) (g) + e-
first ionization energy periodic trends
INCREASES across period, DECREASES down group
effective nuclear charge periodic trend
INCREASES across period, DECREASES down group (shielding effect)
atomic radii (definition)
One-half the distance between the nuclei of identical atoms that are bonded together
atomic radii periodic trend
DECREASES across period, INCREASES down group
cations are smaller than their elements (true/false)
TRUE ~ less electrons = greater Zeff = valence e pulled closer
anions are larger than their elements (true/false)
TRUE ~ lower Zeff + spin-pair repulsion
what is equilibrium
the point in an equilibrium reaction in which the forward and backward reactions are equal and opposite
what is dynamic equilibrium
moving forwards and backwards, the concentration of reactants and products remain constant
the Kc equilibrium constant is for..
AQUEOUS solutions, expressed as molarity (mol/dm³)
the Kp equilibrium constant is for..
GASES, expressed as partial pressures of gases
what is Kc for this reaction?
aA + bB > cC + dD
Kc = ( [C]^c x [D]^d ) / ( [A]^a x [B]^b )
Kc is affected by a change of temperature. t/f
TRUE
Kc is NOT affected by a change in concentration of reactants or products. t/f
TRUE
Kc is NOT affected by a change of pressure
TRUE this only affects gases
Kc is NOT affected by adding a catalyst
TRUE
Le chateliers principle about equilibrium
when a change is applied to a system in dynamic equilibrium, the system reacts in such a way as to oppose the effect of the change. ex. if the concentration of a substance is increased then the concentrations of the other species will change to keep the equilibrium constant the same
What is Kp for this reaction
aA + bB > cC + dD
( (PressureC)^c x (PressureD) ^d ) / ( (PressureA)^a x (PressureB)^b) )
increasing conc of reactants shifts equilibrium..
to the RIGHT (products side)
increasing conc of products shifts equilibrium..
to the LEFT (reactants side)
decreasing conc of reactants shifts equilibrium..
to the LEFT (reactants side)
what is the only factor affecting the equilibrium constants? (Kc & Kp)
temperature
increasing the pressure shifts equilibrium..
to the side with FEWER gaseous molecules
decreasing the pressure shifts equilibrium..
the side with MORE gaseous molecules
what happens when pressure changes in an equilibrium reaction but both sides have equal moles of gases?
NO CHANGE
increasing temperature in an EXOTHERMIC reaction shifts equilibrium..
to the LEFT (reactants side)
decreasing temperature in an EXOTHERMIC reaction shifts equilibrium..
to the RIGHT (products side)
increasing temperature in an ENDOTHERMIC reaction shifts equilibrium..
to the RIGHT (products side)
decreasing temperature in an ENDOTHERMIC reaction shifts equilibrium..
to the LEFT (reactants side)
what is the role of a catalyst?
Provides an alternative reaction pathway involving a lower activation energy
what is a homogenous catalyst?
catalyst is in the same state of matter as reactants
what is a heterogenous catalyst?
catalyst is in a different state of matter as reactants
catalysts shift equilibrium. t/f
FALSE. they only lower Ea
what is the Haber Process? what are the conditions?
N2 (g) + 3H2 (g) > 2NH3 (g) . 20000kPa, 380-450 degrees C, IRON CATALYST
is Haber process exo or endothermic
exothermic
why does the Haber process require a catalyst?
we want to increase the yield of ammonia but if we increase temperature equilibrium favors the reactants. so our only option is using a catalyst to lower activation energy and therefore yielding more product.
enthalpy (definition)
a measure of the heat content of a substance at constant pressure
what is a bronsted-lowry acid
a molecule or ion that is a proton (H+) donor
what is a bronsted-lowry base
a molecule or ion that is a proton (H+) acceptor
when will equilibrium of acid-base reactions occur
if either the acid or base (or both) are weak
what is a strong acid?
an acid that dissociates completely in aqueous solution
what is a weak acid?
an acid that dissociates partially into ions in aqueous solution.
how is the strength of an acid/base measured?
degree of dissociation
what are the strong acids?
HCl, HBr, HI, H2SO4, HClO3, HClO4
dissociation of H2SO4 equation
H2SO4 (aq) + H2O (l) > 2H+ (aq) + SO4(2-) (aq)
what is a strong base?
a base that dissociates completely in aqueous solution
are insoluble/slightly soluble bases weak or strong?
WEAK because they are adding few OH- ions into the solution
what are the strong bases?
NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
is ammonia a weak or strong base
weak
what is self-ionization of water
when two water molecules produce a hydronium (H3O+) and a hydroxide (OH-) ion
self ionization of water (equation)
2H2O(l) = H3O+ (aq) + OH- (aq)
if [H3O+] > [OH-] then solution is..
acidic
if [H3O+] < [OH-] then solution is..
basic
if [H3O+] = [OH-] then solution is..
neutral
formula to find pH
-log[H3O+]
formula to find [H+]
10^-pH
electrical conductivity for strong and weak acids/bases
strong acids/bases generate more ions so they conduct more electricity than weak acids/bases
reactivity of strong and weak acids/bases
strong acids/bases are more reactive with metals than weak acids/bases bc of more ions
what is an acid-base indicator
a dye or mixture of dyes that changes color over a specific pH range
ammonia (weak base) dissolving in water
NH3 (aq) + H2O (l) = NH4+ (aq) + OH- (aq)
Note
Flashcard