Gen Chem Flashcards
A first order rate law can be identified by the presence of _
One reactant
A second order rate law can be identified by the presence of __
Two Reactants
How would you sequentially determine the rate law for a multi-step mechanism?
Look at reactant 1 and see if there are any related changes in rate. Then look at reactant 2 and see if there are any related changes in rate
Trigonal Planar geometry uses ___ angles and the planar geometry allows for __ stabilization.
120 degree ; resonance
Trigonal pyramidal geometry leads to __ bond angles which are __ degrees.
distorted ; <120
The sigmoidal shape of an oxyhemoglobin dissociation curve is due to __ binding and eventual __.
Cooperative ; Saturation
Carbon monoxide poisoning results in a left shift. This is because CO increases __ binding affinity. As a result, saturation occurs quicker as CO results in fewer available __.
O2 ; bind sites
Cooperative Binding
When something (i.e. Oxygen) is bound to a subunit subsequently its affinity for additional i.e. oxygen increases and it can bond more readily to additional i.e. oxygen.
If concentration is __ than solubility than a precipitate will form
greater than
If concentration is __ to solubility then it can be considered as saturated.
=
If concentration is __ solubility then it can be considered unsaturated.
less than
Ideal gases have 1) __ molecular volume 2) ___ intermolecular forces and 3) their Kinetic Energy is proportional to __.
negligible ; negligible ; temperature
Liquids are incompressible, however, __ can be compressed.
Gases
In order for an object to float the density of the object must be __ than that of the fluid. If it was to sink then the density of the object must be __ than that of the fluid.
less ; greater
The electron configuration can be determined by the ___.
Atomic number ( then + or - any charges)
The maximum number of electrons in an atomic energy level is __
2n^2
The maximum number of electrons in a subshell is __
4l+ 2
According to the Heisenberg Uncertainty Principle we are unable to measure position and momentum both __ and __. This is due to an error in one variable as we attempt to measure the other.
exactly ; simultaneously
The atomic number indicates the ___.
Number of protons (A in A/Z)
The atomic weight is the ___ of isotopes. It is also the amount, in grams, for 1 mole.
average
The atomic mass is the mass number. This means that it indicates the number of __ and __.
Protons and Neutrons (note: # protons = # electrons if atom is neutral)
Charge is determined by __
electrons
Atomic number is determined by __
protons
Isotopes are determined by __.
Neutrons
Planck’s equation measures ___. Its formula includes planck’s constant and frequency __.
Energy ; E= hf
As the principal quantum number (n) increases the energy of the electron becomes less __ .
negative
The energy of a photon can be measured using what equation:
E = hc / wavelength
When n=1 (lower) goes to n=3 (higher) what occurs?
AHED (Absorb Light ; Higher Potential energy ; Excited ; Distant from Nucleus)
According to Pauli’s exclusion principle ___
No two electrons in a given atom can be described by quantum numbers (n, l, ml, ms) that are exactly the same
The angular momentum (l) is limited by the ___. It determines the shape and number of subshells.
Principle quantum number (n)
Magnetic Quantum number (ml) specifies __ and ranges between __.
the orbital within a subshell ; - l to + l including 0
Spin Quantum number (ms) can either be ___ or ___.
+ 1/2 or -1/2
If electrons are paired that means they are in the __ orbital with __ spins.
same ; opposite
If the electrons are parallel than they are in __ orbitals with ___ spins.
different ; same
Aufbau Principle suggests the following rule for filling shells and subshells__
N+ 1
If something is paramagnetic that means it is __ magnet and has all __ electrons.
attracted to ; unpaired
If something is diamagnetic that means it is __ magnet and has all __ electrons.
repelled from ; paired
Atomic radius __ left to right. It __ top to bottom.
decreases; increases
Ionic radius is bigger in __ than neutral atoms and is smaller in ___.
anions ; cations
Ionization energy ___ left to right. It __ top to bottom.
increases ; decreases
Electron affinity ___ left to right. It __ top to bottom.
increases; decreases
Electronegativity __ left to right. It __ top to bottom.
Increases ; Decreases
The oxidation number of a ion is equal to __. It describes the degree of oxidation.
the charge of the ion
Intramolecular bonding is “within” and examples include __ which have strong electrostatic attraction & electronegativity differences and __ which have weak electrostatic attraction and moderate electronegativity differences .
ionic ; polar covalent
Intramolecular bonding also includes ___ which is when electrons in a bond come from one atom and __ which has neutral atoms, negligible electrostatic attraction and a small electronegativity difference.
coordinate covalent ; covalent
In terms of intramolecular strength rank the following: covalent, polar covalent, ionic
Ionic > Polar Covalent > Covalent (based on electrostatic attraction)
In terms of intermolecular strength rank the following: dipole-dipole, dispersion, ion-dipole, hydrogen bonding.
Ion Dipole > Hydrogen Bonding > Dipole- Dipole > Dispersion
Hydrogen bonding requires N O or F and is a ___ interaction.
very strong dipole
Ion-dipole involves strong electrostatic attraction, fully charged ions and __.
solvation
Ionic bonds form between __ ions. Polar covalent bonds form between atoms with ___ .
fully charged ; different electronegativity
Coordinate covalent bonds occur when the electrons come from __ . Covalent bonds form between atoms of ___.
a single atom ; similar electronegativities
Tetrahedral Electronic Geometry (Associated Groups, Hybridization and Bond Angles)
4;Sp3; 109.5
Trigonal Planar (Associated Groups, Hybridization and Bond Angles)
3; sp2; 120
Trigonal bipyramidal (Associated Groups, Hybridization and Bond Angles)
5; sp3d; 90,120,180
Charge is determined by the number of __
Electrons
Atomic number is determined by the number of __
Protons
Isotopes have the same atomic number but different __ due to a difference in the number of neutrons.
Mass Number
E=hf where h is planck’s constant and f is frequency in J*s.
Planck’s equation for determining energy
L= nh/ 2pi where h is planck’s number and n is the principal quantum number measures
Angular momentum
E= -Rh/ n^2 where RH = 2.18 x 10^-18 J and the __ changes as n changes.
Energy of the electron
The equation for the electromagnetic energy of a PHOTON.
E= hc / wavelength
If we go from n=1 as the lower initial energy level to n=3 a higher final energy level what can we expect to happen?
Absorption of light, higher potential, excited, distant from nucleus
The maximum number of electrons in a shell can be described as __
2n^2
If two electrons are said to be PAIRED what does this mean about their orbital and spin?
They have the same orbital but are opposite spins
If two electrons are said to be PARALLEL what does this mean about their orbital and spin?
They are in different orbitals but have the same spins
The maximum number of electrons in the subshell can be defined by the equation 4l+2. This means that which quantum number limits the number of electrons within a subshell?
l which is the angular momentum
According to Pauli’s exclusion principle what is true of 2 electrons in a given atom ?
No 2 electrons can be described with the exact same quantum mechanical numbers
If it is said to be paramagnetic what does that mean for the electrons?
Attracted to magnet and all unpaired electrons
If it is said to be diamagnetic what does that mean for the electrons?
Repelled from magnet and all paired electrons
Effective Nuclear Charge (Zeff) __ left to right and __ from top to bottom.
increases ; increases
Atomic radius __ left to right and __ top to bottom.
Decreases; Increases
deltaG < 0
Q < Keq
forward reaction occurs
deltaG > 0
Q > Keq
reverse reaction occurs
deltaG = 0
Q =Keq
dynamic equilibrium- forward and reverse still occuring
equilibrium is reached when entropy is at its maximum and free energy is at its minimum
Calculate Keq
I Products I / I ReactantsI
Law of Mass Action
Keq >1
more products
Law of Mass Action
Keq ~ 1
equal amount of products and reactants
Law of Mass Action
Keq <1
more reactants
Law of Mass Action
Keq «<1
negligible in comparison to initial concentration
In one direction it is written as Keq, the equilibrium constant for the reverse reaction is written as __
1/ Keq
If a reactant is added or a product is removed what impact would this difference in concentration have __
Qc < Keq
Forward
Up QC until equilibrium
If a reactant is removed or a product is added what impact would this difference in concentration have __
Qc > Keq
Reverse
Qc until equilibrium
If a reaction undergoes compression (volume down, pressure up) the reaction moves in the direction with __
less moles of gas
If a reaction undergoes expansion (volume up, pressure down) then it moves in the direction of __
more moles of gas
If a reaction is endothermic then dH>0 and heat is _
a reactant
Temperature does not change Qc or Qp but it does effect
Keq
If a reaction is exothermic then dH<0 and heat is _
a product
If temperature increases in endothermic conditions or temperature decreases in exothermic conditions the reaction will shift to the __
right
If temperature decreases in endothermic conditions or temperature increases in exothermic conditions the reaction will shift to the __
left
The kinetic product is easier to reach the transition state. It is higher in __ __ , forms quicker and can form at __ temperatures
free energy ; low
The thermodynamic product is more slow and stable. It is __ in free energy and is high in heat transfer. It is spontaneous which means that deltaG is __.
lower ; negative
What does not appear in the equilibrium constant (Keq) equation?
pure solids and pure liquids
Collision Theory
rate proportion to number of collisions / second
Arrhenius Equation
as the frequency factor Ea increases the rate constant (k) increases
if T increases, the exponent becomes less negative (smaller) and constant (k) increases
Ea can be increased by increasing the number of molecules in the vessel
Transition State Theory
+ deltaG endergonic : energy absorbed
- deltaG exergonic: energy given off
Ea can be lowered without deltaG
Reaction Rates: Concentration
increased concentration:
increase collisions, increase freq. factor, increased rate except 0 order reactions
Reaction Rates: Temperature
incr. rate ; incr. KE
Reaction Rates: Change in Medium
aqueous / non aqueous
physical state
polar/nonpolar
Reaction Rates: Catalysts
homogenous: same phase
heterogenous: different phase
lower Ea no change in Keq
does not transform nonspontaneous to spontaneous
Zero Order Rate law
constant rate not dependent on concentration of reactant
changes only be change in Temp or catalyst
conc. v time linear ; slope = -k
rate = k[A]^0 [B]^0
First Order Rate Law
nonconstant rate and dependent on concentration of reactant
conc. v time nonlinear ; slope ln[A] = -k
rate = k[A]^1 or rate = k[B]^1
Second Order Rate Law
nonconstant rate and dependent on concentration of reactant
conc. v time nonlinear ; slope 1/[A] = k
rate = k[A]^1 [B]^1 or rate = k[A]^2 or rate = k[B]^2
Broken Order Reaction
noninteger orders
Mixed Order Reaction
rate order changes over time
