Gen Chem Flashcards by Magda Wojtara

A first order rate law can be identified by the presence of _

One reactant

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A second order rate law can be identified by the presence of __

Two Reactants

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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

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Trigonal Planar geometry uses ___ angles and the planar geometry allows for __ stabilization.

120 degree ; resonance

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Trigonal pyramidal geometry leads to __ bond angles which are __ degrees.

distorted ; <120

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The sigmoidal shape of an oxyhemoglobin dissociation curve is due to __ binding and eventual __.

Cooperative ; Saturation

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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

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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.

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If concentration is __ than solubility than a precipitate will form

greater than

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If concentration is __ to solubility then it can be considered as saturated.

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If concentration is __ solubility then it can be considered unsaturated.

less than

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Ideal gases have 1) __ molecular volume 2) ___ intermolecular forces and 3) their Kinetic Energy is proportional to __.

negligible ; negligible ; temperature

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Liquids are incompressible, however, __ can be compressed.

Gases

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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

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The electron configuration can be determined by the ___.

Atomic number ( then + or - any charges)

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The maximum number of electrons in an atomic energy level is __

2n^2

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The maximum number of electrons in a subshell is __

4l+ 2

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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

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The atomic number indicates the ___.

Number of protons (A in A/Z)

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The atomic weight is the ___ of isotopes. It is also the amount, in grams, for 1 mole.

average

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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)

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Charge is determined by __

electrons

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Atomic number is determined by __

protons

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Isotopes are determined by __.

Neutrons

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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

Gen Chem Flashcards

(104 cards)