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Q4 > Q4- GEN CHEM > Flashcards

Q4- GEN CHEM Flashcards

1
Q

A substance which speeds up a reaction but is chemically unchanged as it ends

A

Catalyst

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2
Q

The process of speeding up a reaction by using a catalyst

A

Catalysis

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3
Q

Types of catalyst

A

Homogeneous Catalyst, heterogeneous catalyst

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4
Q

When a catalyst and the reactants are in the same physical state or phase, the reaction is considered

A

Homogenously catalyzed/ homogeneous Catalyst

Additional info: this happens mostly with gaseous catalyst-reactant pairs.

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5
Q

When the catalyst and the reactant are in different phases, the reaction is said to be

A

Heterogeneously catalyzed
Additional info: common heterogeneous catalyst mostly include inorganic or a non carbon containing solid like elemental metals, sulfides and metallic salts.

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6
Q

proteins that function as catalyst in all living systems. They are natural catalysts found in the body.

A

Enzymes

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7
Q

They are responsible for many essential

A

Biochemical reactions

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8
Q

They have components called ______ binding sites or an active site, where molecules involved in a reaction under catalysis become attached

A

substrate

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9
Q

_____ ___ of Thermodynamics states that energy cannot be created or destroyed.

A

First Law

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10
Q

The _______ ___ of thermodynamics states that a spontaneous process will increase the ENTROPY of the universe.

A

second law

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11
Q

If the system becomes less ordered, the entropy________.

A

increases

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12
Q

If the system becomes more ordered, the entropy _________

A

decreases

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13
Q

Comparing entropies

The greater the number of possible microstates for a system, the higher the entropy. Microstate refers to the arrangement of the energy of each molecule in the whole system at one instant. It is directly related to the amount of the substance.

A

A. Number of Possible Microstates

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14
Q

Comparing entropies

Different phases have different entropies. Gases have higher entropy than liquids and liquids have higher entropy than solids.

A

B. Phases

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15
Q

the process of changing solid to liquid

A

Melting

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16
Q

the process of changing liquid to gas

A

Evaporation

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17
Q

the process of changing liquid to gas

A

Evaporation

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18
Q

the process of changing gas to liquid

A

Condensation

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19
Q

the process of changing liquid to solid

A

Freezing

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20
Q

Comparing entropies

The higher the temperature, the higher the entropy

A

C. Temperature

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21
Q

Comparing entropies

Compared to a pure substance, in which all particles are identical, the entropy of a mixture of two or more different particle types is greater. This is because of the additional orientations and interactions that are possible in a system comprised of nonidentical components

A

D. Mixture vs pure solvent

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22
Q

Comparing entropies.

When a solid dissolve in a liquid such as sodium chloride in water, the particles of the solid experience both a greater freedom of motion and additional interactions with the solvent particles. This corresponds to a more uniform dispersal of matter and energy. The process of dissolution therefore involves an increase in entropy.

A

E. Dissolved Substances vs. Precipitate

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23
Q

Comparing entropies.

The side of the equation with more moles of gas has a higher total entropy. This is because a greater number of moles indicates a greater number of gas particles and a greater number of arrangements of the gas particles.

A

F. Presence of gas

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24
Q

What formula is this?
∆S reaction= ∆Sproducts - ∆Sreactant

A

Formula of entropy

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25
Q

The symbol for entropy is

A

S

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26
Q

standard entropy of a substance is given by the symbol

A

S°

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27
Q

Standard entropy is the entropy of a substance at 25°C and 1 atm of pressure. The units for entropy are J/K mol

A

Read carefully 🐯

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28
Q

Generally, a reaction is said to occur _____________ if the entropy increases. Entropy (S) is a measure of the disorder in a system.

A

spontaneously

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29
Q

Are attractive forces BETWEEN molecules

A

Intermolecular forces
They are important because they determine some physical properties of molecules like boiling point, melting point, and density

30
Q

Hold atoms together in a molecule

A

Intramolecular forces

31
Q

Van der waals forces
Between polar molecules

A

Dipole-Dipole Interaction

32
Q

Van der waals forces
Between polar and non polar molecules

A

Dipole-induced dipole interaction

33
Q

Van der waals forces
Between non polar molecules

A

Dispersion forces

34
Q

the relative tendency of an atom to attract electrons to itself when chemically combined with other atoms

A

Electronegativity Values

35
Q

__________ of Molecules depends on:

Electronegativity (EN) Difference

Geometrical Shapes of Molecules

A

Polarity

36
Q

Electronegativity Difference (ΔΕΝ) and

Type of Bonds

A

lonic Bond ≥ 1.7

Polar Covalent 0.5-1.6

Nonpolar Covalent ≤ 0.4

37
Q

formed when electrons are shared unequally by two atoms in a compound, forming an electric dipole

A

Polar Covalent Bond
An atom with higher EN value becomes the partially negative pole
And with lower EN value becomes partially positive

38
Q

Between ion and polar molecules

A

Ion-dipole interaction

39
Q

Between polar molecules (H must be attracted to O, N or F or another molecule)

A

Hydrogen bond

40
Q

the ability water has to flow upward against the force of gravity, due to cohesion and adhesion

A

Capillary Action

41
Q
  1. Capillary Action
  • sticking together of two like molecules
A

• Cohesion (cohesive)
-2 water molecules are cohesive due to the hydrogen bonds

42
Q
  1. Capillary Action
  • sticking together of two unlike molecules
A

• Adhesion (adhesive)
Ex: A water molecule being attracted to a sugar molecule (Like making Kool-aid)
Add: 1. Polarity

43
Q
  • a measure of the force necessary to stretch or break the surface of a liquid
A

Surface tension

44
Q
  • amount of heat that must be absorbed or lost before it actually changes temperature
A

Specific Heat

45
Q

-The cooling of a surface occurs when the liquid evaporates

A

Heat of Vaporization

46
Q
  • a measure of how compact the atoms or molecules are within a substance or how much mass there is in a given space (volume)
A

Density

47
Q
  • a liquid that dissolves a particle (solute)
A

Solvent

48
Q
  1. Universal Solvent
    - particle or liquid that gets dissolved in the solvent
A

Solute

49
Q

-A unique temperature and pressure at which three phases (usually solid, liquid, and gas) can exist together

A

Triple Point

50
Q

The temperature and pressure at which gas and liquid merge together to form a supercritical fluid. Beyond this temperature, no amount of pressure will condense the gas to a liquid

A

Critical Point

51
Q

At 1 atm pressure, the temperature at which the solid melts to liquid.

A

Normal Melting Point

52
Q

At 1 atm pressure, the temperature at which the liquid vaporizes to become a gas

A

Normal Boiling Point

53
Q

A measure of kinetic or translational energy

A

Heat

54
Q

Measure of warmth and coldness

A

Temperature

55
Q

■The _______ ______ is a graph which represents how a sample changes phases. As heat is added over time, the sample changes temperature and phase accordingly.

A

heating curve

56
Q

It is a “map” that tells us which state(s) of matter (solid, liquid, gas) exist for a given set of temperature and pressure conditions.

A

Phase diagram

57
Q

is the amount of energy needed to completely make a solid into a liquid

A

Heat fusion

58
Q

is the amount of energy needed to completely make a liquid into a gas

A

Heat vaporation

59
Q

A ratio comparing the amount of solute to the amount os solution

A

Concentration

60
Q

A homogeneous mixture of one substance(the solute) dissolved in another substance (the solvent (

A

Solution

61
Q

mass solute (g)/ mass solution (g) × 100

A

Percent mass

62
Q

volume solute (ml)/volume solution (ml) × 100

A

Percent volume

63
Q

Expresses the concentration of solution as the mass of solute in a given mass of solution

A

Ppm

64
Q

Typically used for very small Concentration

A

Ppb

65
Q

Moles • grams/1mole= grams

A

Mass to moles

66
Q

An expression of moles/Liter of the solute

A

Molarity

67
Q

Another quantitative expression of the concentration of the solution

A

Molality

68
Q

The study of quantities of materials consumed and produced in chemical reactions.

A

Stoichiometry

69
Q

The minimum energy required for a reaction to take place

A

Activation energy

70
Q

The measure of how much exposed has which is expressed in square units

A

Surface area

71
Q

Those that result in a chemical reaction and a new product is formed.

A

Effective Collisions

72
Q

A collision is considered __________ when one doesn’t lead to product formation

A

Ineffective

Q4 (2 decks)

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