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Deutsch > Chem exam 1 > Flashcards

Chem exam 1 Flashcards

not to fail

1
Q

Saturated Solution

A

Contains the maximum amount of solute that will disolve in a given solution

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2
Q

Unsaturated Solution

A

Contains less solute than the solvent has capacity to disolve

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3
Q

Supersaturated

A

Contains more disolved solute than solvent has capacity to disolve

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4
Q

Solubility

A

The ability of a solute to disolve in a solvent
expressed as:
S = Mass of Solute (g) / Volume of Solution (L)

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5
Q

Heat of solution

A

gas becomes less soluble as temp increases.
Solid/Liquid solutions increase solubility as temp increases.

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6
Q

Pressure of a solution

A

does not affect solid/liquid solubility.
higher pressure increases solubility in gaseous solutions.

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7
Q

Ion-dipole

A

The charge of an ion is attracted to the positive side of a polar molecule

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8
Q

Dipole induced dipole

A

The partial charge on a polar molecule induces a temporary partial charge on a neighboring nonpolar molecule or atom.

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9
Q

Ion induced dipole

A

The charge of an ion induces a temporary partial charge on a neighboring nonpolar molecule or atom

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10
Q

molality (m)

A

mols of solute / mass of solvent (kg)

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11
Q

colligative property

A

properties that depend on the number of solute particles in a solution but do not depend on the nature.
* vapor pressure-lowering
* boiling point elevation
* freezing point deprevation
* osmotic pressure

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12
Q

IMFs

A
  • Hydrogen bonding- This is the strongest type of intermolecular force and occurs in molecules where hydrogen is directly bonded to highly electronegative atoms like O, N, or F.
  • Dipole-Dipole Interactions: These occur between the positive end of one polar molecule and the negative end of another polar molecule.
  • Ion-Dipole Interactions: These occur between ions and polar molecules.
  • Dipole-Induced Dipole Interactions (London Dispersion Forces): This is a type of van der Waals force where a polar molecule induces a temporary dipole in a neighboring nonpolar molecule, leading to an attractive force. This force is generally stronger in larger, more polarizable molecules.
  • Ion-Induced Dipole Interactions: These occur between an ion and a nonpolar molecule. The ion induces a temporary dipole in the nonpolar molecule, leading to an attractive force.
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13
Q

Raoults Law

A

Difference in vapor pressure of pure solvent and corresponding solution
𝑃𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛 = (𝜒𝑠𝑜𝑙𝑣𝑒𝑛𝑡)(𝑃𝑠𝑜𝑙𝑣𝑒𝑛𝑡)

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14
Q

boiling point elevation

A

ΔT b=i⋅Kb ⋅m

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15
Q

freezing point deprevation

A

ΔT f=i⋅Kf ⋅m

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16
Q

Osmosis

A

Osmosis is the movement of solvent molecules (usually water) across a selectively permeable membrane from an area of lower solute concentration to an area of higher solute concentration. The key factor in osmosis is the concentration of solutes, not the type of solute molecules.

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17
Q

Osmosis equation

A

π=i⋅M⋅R⋅T

Where:
π is the osmotic pressure,

i is the van’t Hoff factor (the number of particles into which the solute dissociates in the solution),

M is the molarity of the solution,

R is the ideal gas constant (approximately 0.0821 L·atm/(mol·K)),

T is the absolute temperature in Kelvin.

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18
Q

Van’t Hoff factor

A

The van’t Hoff factor (i) represents the number of ions that a molecule dissociates into when it dissolves in a solution.

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19
Q

Mass

A

Volume x Density

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20
Q

Colloid

A

a dispersion of particles of one substance throughout another substance
1 nanometer (nm) to 1 micrometer (μm).

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21
Q

Like disolves like

A

two substances of similar IMF and magnitude are more likely to be soluble with one another.

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22
Q

Hydrophillic

A

substances that “love” water
* Hydrophilic molecules are typically polar or ionic, meaning they have regions with partial positive and negative charges.
* They readily dissolve or interact with water molecules.
* Examples of hydrophilic substances include salts, sugars, and many biomolecules like proteins and nucleic acids.

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23
Q

Hydrophobic

A

substances that “fear” water and repel it.
* Hydrophobic molecules are often nonpolar and lack regions with significant positive or negative charges.
* They do not readily dissolve in water and may aggregate to minimize contact with water.
* Examples of hydrophobic substances include fats, oils, and certain types of molecules in cell membranes.

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24
Q

Semi Permeable membrane

A

A type of membrane that allows for certain substances to pass through and others to not.

25
Q

Chemical kinetics

A

The study of how fast reactions take place.

26
Q

Average reaction rate

A

The average reaction rate is a measure of how quickly a chemical reaction progresses over a specified period of time.

This is expressed by= Change in concentration of reaction or product / Change in time
​

27
Q

Insantaneous Reaction Rate

A

The instantaneous reaction rate refers to the rate of a chemical reaction at a particular point in time, usually at a specific moment during the reaction.

This is equal to the slope on any two given point on the concentration vs time graph

28
Q

Rate Law

A

Rate=k⋅[A]^m⋅[B]^n
* k=Rate constant a proportionality constant that depends on the specific reaction and temperature
* a proportionality constant that depends on the specific reaction and temperature
* m and n are the reaction orders with respect to reactants A and B, respectively.

29
Q

Rate Constant

A

represented as k. a proportional constant that depends on specific reaction and temperature. Shows speed

30
Q

Reaction Order

A

The reaction order refers to the power to which the concentration of a reactant in a chemical reaction is raised in the rate law equation.

31
Q

Zero order reaction

A

The rate is solely determined by the rate constant (k). The rate law for a zero-order reaction is:

rate=k

In a zero-order reaction, doubling or halving the concentration of the reactant does not affect the rate of the reaction. The rate is solely determined by the rate constant (k). The integrated rate law for a zero-order reaction is:

[A]=[Ao]-kt
[A]=given concentration of reactant
[Ao]= initial concentration of reaction
k=rate constant
t=time

units are expressed in M/s

32
Q

First order reaction

A

In a first-order reaction, the rate of the reaction is directly proportional to the concentration of a single reactant. The rate law for a first-order reaction is expressed as:

Rate= k x [A]
k= rate constant
[A]= concentration of reactant

In a first-order reaction, if the concentration of the reactant is doubled, the rate of the reaction will also double. The integrated rate law for a first-order reaction is:

ln([A])=−kt+ln([A]o)

[A]= concentration of reactant at time t
[A]o = concentration of initial reactant
k=rate constant
t=time
ln= natural logarithm

Units are expressed in s^-1

33
Q

Second order reaction

A

In a second-order reaction, the rate of the reaction is proportional to the square of the concentration of a single reactant or to the product of the concentrations of two reactants. The rate law for a second-order reaction can take two main forms:

rate = k x [A]^2

rate = k x [A] x [B]

[A] and [B] are the concentrations of the reactants

The integrated rate law for a second-order reaction with respect to a single reactant (A) is:
1/[A] = kt + 1/[Ao]

units are expressed in M^-1 x s^-1

34
Q

Half life

A

In the context of chemical reactions, particularly those involving first-order kinetics, the half-life is the time required for the concentration of a reactant to decrease by half.

this is shown by:

t 1/2 = 0.693/k

t 1/2 = half life
k = rate constant

35
Q

Collision theory

A
  • Reactions are a result of collisions
  • Collisions must have enough activation energy (Ae) to overcome the Activation energy barrier to proceed
  • The chemical reaction rate is porportional to the amount of effective collisions
  • very relevant to gas collisions
36
Q

Effective collision

A

collision that results in a reaction

37
Q

Transition state/activated complex

A

The transition state where a “species” is briefly created during the reaction.

38
Q

Energy Profile /
Reaction Coordinate
Diagram

A

Diagram showing a reaction
* reactants on left, products on right
* highest point is the transition state
* activation energy (Ea) is what must be reached for the reaction to occur

39
Q

Reaction mechanism

A

A reaction mechanism is a detailed step-by-step description of the series of elementary steps or molecular events that occur during a chemical reaction.

A+B –> C
C+b —> D

Overall reaction
A+2B —> D

40
Q

Intermediate

A

Intermediate species are transient molecular entities that are formed in one step of the reaction mechanism and consumed in a subsequent step. They do not appear in the overall balanced chemical equation for the reaction.

A+B –> C
C+b —> D

Overall reaction
A+2B —> D

example is C

41
Q

Elementary Reaction

A

Elementary steps are the individual, simple reactions that make up a chemical reaction mechanism. These steps involve the breaking and forming of chemical bonds between a small number of reactant molecules, leading to the formation of intermediate species or products.

=The amount of peaks on a diagram

42
Q

Unimolecular

A

Unimolecular refers to a type of chemical reaction or process in which a single molecular entity, such as a molecule or an ion, undergoes a transformation or decomposition. Unimolecular reactions involve the intramolecular rearrangement or dissociation of a single species without the direct involvement of other molecules.

43
Q

Bimolecular

A

Bimolecular refers to a type of chemical reaction or process that involves the collision or interaction between two molecular entities—such as two molecules or ions. In bimolecular reactions, the transformation or reaction occurs as a result of the collision or interaction between these two entities.

most common

44
Q

Termolecular

A

Termolecular reactions involve the simultaneous collision of three molecular entities (atoms, molecules, or ions) leading to a chemical transformation or reaction. Termolecular reactions are relatively rare compared to unimolecular and bimolecular reactions, primarily due to the increased complexity and lower probability of three particles colliding with the correct orientation and energy simultaneously.

45
Q

Rate determining/Rate limiting step

A

the slowest step in a reaction mechanism and governs the overall rate of the entire chemical reaction. It determines how quickly the reactants are transformed into products.

key characteristics:
* highest Ea
* slowest step
* The rate of the rate-determining step is often dependent on the concentrations of the reactants involved in that particular step.

46
Q

Catalyst

A

A catalyst is a substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with a lower activation energy, without being consumed in the overall reaction.

47
Q

Heterogenous Catalyst

A

Catalyst that is in a different state than the solution
(ex. solid in a liquid or gaseous solution)

48
Q

Homogenous Catalyst

A

Catalyst in the same state as the solution (ex. dissolved in solution)

49
Q

Chemical Equilibrium

A

Chemical equilibrium is a state in a chemical reaction where the concentrations of reactants and products remain constant over time. In other words, the forward and reverse reactions occur at the same rate

50
Q

Equilibrium Constant

A

The equilibrium constant (Kc) expression for a generic reaction:

solution / reactant:
[B]^b / [A]^a = Kc

51
Q

Reaction Quotient

A

Represented as Qc

  • If Q is less than K, the reaction will proceed in the forward direction to reach equilibrium, favoring the formation of products.
  • If Q is greater than K, the reaction will proceed in the reverse direction to reach equilibrium, favoring the formation of reactants.
  • If Q is equal to K, the system is at equilibrium.

Qc= [C]^c[D]^d / [A]^a[B]^b

52
Q

Heterogeneous
Equilibrium

A

Heterogeneous equilibrium refers to the equilibrium state in a chemical reaction that involves substances in different phases.

53
Q

Homogeneous
Equilibrium

A

Homogenous equilibrium refers to the equilibrium state in a chemical reaction that involves substances in the same phase.

54
Q

Arrhenius equation

A

The dependence of the rate constant of a reaction on temperature

k= A x e^-Ea/RT

Ea= activation energy
R= gas constant 8.314 J/K x mol
T= absolute temp
e = base of logorithm
A= collision frequency / frequency factor

OR

lnk = ln A - Ea/ RT

which can be rearranged to a linear fit as:

lnk = (-Ea/R)(1/T) + lnA

55
Q

Arrhenius equation (two temps)

A

ln k1/k2 = Ea/R (1/T2 - 1/T1)

56
Q

Exothermic vs endothermic on a diagram

A
  • Exothermic is when products have lower potential energy than the reactants
  • Endothermic is when producs have higher potential energy than the reactants.
57
Q

Describe the direction
1. Q>K
2. Q=K
3. Q<K

A
  1. reaction goes towards reactants
  2. reaction at equilibrium
  3. reaction goes towards products
58
Q
  1. Kc»>1
  2. Kc is not large
  3. Kc«<1
A
  1. reaction goes to completion
  2. Reaction occurs but doesnt go to completion
  3. reaction goes to completion, but at an insignificant amount

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