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Chem 1110 > Exam 3 > Flashcards

Exam 3 Flashcards

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1
Q

What is the combined gas law equation?

A

P1V1/T1= P2V2/T2

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2
Q

What is the definition of pressure

A

The amount of force applied perpendicular to the surface of an object per unit area

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3
Q

What does Kinetic molecular theory explain?

A

That matter is always in motion, have negligible volume, have negligible intermolecular forces

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4
Q

What is Boyles law?

A

The volume is inversely proportional to the pressure. (Ex: when value increase pressure decreases)

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5
Q

What is Charles law?

A

The volume of an ideal gas is directly proportional to the absolute temperature at constant pressure (ex: the colder a ball is the less gas it has)

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6
Q

What is Gay Lussac’s Law?

A

Means that the pressure increases while temperature increases and vice versa (ex: atoms move faster when hot and slower when cold)

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7
Q

What is the combined gas law?

A

That gas pressure, volume, and temperature are constant (ex: balloon gas decrease as the temperature decreases and in turn the volume decreases)

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8
Q

How are boiling point and vapor pressure related?

A

Boiling will happen when vapor pressure is equal to atmospheric pressure

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9
Q

What are the 5 types of attractive forces between molecules?

A

London forces, dipole-dipole forces, hydrogen bonding, ion-dipole forces, ionic attractions

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10
Q

What is London force?

A

-The weakest intermolecular force.
-It temporarily makes attractive force that form temporary dipoles (making a dipole dipole force)

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11
Q

What is a dipole dipole force?

A

-An attractive force between a positive and negative of a polar molecule.
-Strength range from 5kj to 20kj per mole

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12
Q

What is hydrogen bonding forces?

A

-It is a special type of dipole dipole force that occurs between hydrogen and a highly electronegative atom (O,F,CL, etc.)
-stronger than general dipole dipole force

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13
Q

What is an ion dipole force?

A

-An attractive force that results from attraction between an ion and a neutral molecule that has a dipole
-strongest of the intermolecular forces

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14
Q

What is ionic attraction force?

A

When two opposite ions attract
It is a strong force

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15
Q

What is the difference between intramolecular forces and intermolecular forces?

A

Intramolecular: within the molecule
Intermolecular: between the molecule

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16
Q

How do you find the highest boiling point of alkanes

A

The boiling point increases with increasing molecular weight

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17
Q

How do we identify H-FON, Polar molecules, and nonpolar molecules?

A

-H-Fon is hydrogen bonding (H bonded to F,O,N)
-Polar Molecules is dipole-dipole force and London dispersion force
-non polar molecules is London dispersion force

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18
Q

What is the golden rule of solubility?

A

Like dissolves like (polar dissolve polar, nonpolad dissolve non polar)

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19
Q

What is hydrophilic?

A

Attracted to water (polar atoms lots of Ns and Os)

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20
Q

What is hydrophobic?

A

Resists water (nonpolar atoms it’s of carbons and hydrogen)

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21
Q

What is hydration in terms of chemistry?

A

A chemical reaction in which a substance combines with water

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22
Q

What are amphipathic compounds?

A

Chemical compounds that have both polar and nonpolar portions in their structure (ex: detergent)

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23
Q

What is the difference between Michelle and a bilayer

A

Micelle interior is completely non polar while bilayers enclose an aqueous compartment called liposomes

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24
Q

How can you identify a steroid molecule?

A

17 carbon atoms arranged in four rings around A,B,C,D

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25
Q

What is cholesterol and what does it look like?

A

A waxy, fat-like substance, found in the cells in your body
-27 carbon compound with a hydrocarbon tail

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26
Q

What is the difference between dietary fats and oils?

A

Dietary fats: solid at room temperature
Oils: liquid at room temperature

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27
Q

What is the Concentration equation

A

M=n/v
M=Molar concentration
n=moles of solute
V= liters of solution

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28
Q

What is morality?

A

A unit of concentration expressed as the number of moles in a dissolved solute per liter of solution

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29
Q

How do you find the mass percent and what is it?

A

-mass percent=(mass of chemical divided by total mass of compound)x100

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30
Q

What is volume percent and how do you find it?

A

The ratio of the volume of the solute to the total volume of solution
-volume percent=(Volume of solute/volume of solution)x100

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31
Q

What is the mass/volume percent of solution defined as?

A

The ratio of the mass of solute that is present in a solution relative to the volume of solution as a whole

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32
Q

What is percentage concentration?

A

1: the mass of the solute divided by mass of solution x10^2
2: the volume of the solute divided by the volume of the solution
3: the mass of the solute divided by the volume of the solution

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33
Q

What is ppm and ppb?

A

Ppm: 1 part per million =
Ppb: 1,000 parts per billion

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34
Q

What is the dilution equation?

A

(C1)(V1)=(C2)(V2)

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35
Q

What are the two parts of a solution?

A

A solute and a solvent

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36
Q

What is a solvent?

A

A liquid that causes a solute

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37
Q

What is a solute?

A

What “disappears” in the solvent

38
Q

What are the 3 types of mixtures?

A

Solution: a homogenous mixture of two or more substances (salt and water)
Colloid: a mixture of two or more substances but can be separated (mayo)
Suspension: a heterogenous mixture of a finely distributed solid in a liquid (flour and water)

39
Q

What is the difference between unsaturated, saturated, and supersaturated?

A

Unsaturated: below the curve
Saturated: on the curve
Supersaturated: above the curve

40
Q

What is the relationship between solubility and temperature?

A

The solubility of most solid or liquid solutes increases with increasing temperature

41
Q

What is Henry’s law?

A

If the pressure of a gas over liquid increases then the amount of gas dissolved in the liquid will increase (carbonated drinks)

42
Q

What are the 4 types of electrolytes?

A

-Potassium (K)
-Sodium (Na)
-calcium (Calcium)
-Magnesium (Mg)

43
Q

What is the equivalent charge conversion for ions with -1 and +1?

A

1x1=1

44
Q

What is the equivalent charge conversion for ions with -2 and 2+?

A

1/2x2=1

45
Q

How do you find ppm?

A

(Mass of solute)/(mass of solution)x 10^6

46
Q

How do you find ppb?

A

(Mass of solute)/(mass of solution)x 10^9

47
Q

How do you find the morality?

A

(Mol of solute)(liters of solution)

48
Q

What is osmosis?

A

Something moving from a higher concentration to a lower concentration (drop of food dye)

49
Q

What does dilution mean?

A

The addition of a solvent that decreases the solute in the solution (water to orange juice)

50
Q

What is osmotic pressure?

A

The minimum pressure added to the solution to halt the flow of solvent molecules

51
Q

What is isotonic?

A

Equal osmotic pressure

52
Q

What is hypotonic?

A

Solutions with lower osmotic pressure (water go in cell)

53
Q

What is hypertonic?

A

An external solution that has a high solute concentration (water goes out)

54
Q

What is hemolysis?

A

A blood cell burst (from hypotonic)

55
Q

What is cremation?

A

A blood cell shrivel (hypertonic)

56
Q

What happens during diffusion?

A

Particles in high concentration areas move toward low concentration

57
Q

What happens during dialysis?

A

Remove waste products and excess fluid

58
Q

What is active trasnsport?

A

Uses atp to get across cel membrane

59
Q

What is passive transport?

A

Does not use atp to get across cell membrane

60
Q

How do molecules use osmosis to transport across cell membrane?

A

they move from a region of higher water concentration to a region of lower water concentration

61
Q

What is the equilibrium constant equation?

A

Kc=[c]^c x [D]^d
——————-
[A]^a x [B]^b
A,B =products
C,D= Reactants
[A]= equilibrium concentration of A in moles
a= number of moles of A

62
Q

Something that has a pH value less than 7 indicates

A

It’s acidic

63
Q

Something with a pH greater than 7 indicates

A

It’s a base

64
Q

If a pH is 7 it is

A

Neutral

65
Q

What is a base?

A

A substance that neutralize an acid by reacting with hydrogen ions

66
Q

What is an acid?

A

A hydrogen containing substance that is capable of donating a proton

67
Q

What are the strong acids?

A

HCl/Hydrochloric Acid
HNO3/ Nitric Acid
H2SO4/Sulfuric Acid
HBr/ Hydrobromic Acid
HI/ Hydroiodic Acid
HClO4/ Perchloric Acid
HClO3/ Chloric Acid

68
Q

What are the strong bases?

A

LiOH/Lithium hydroxide
NaOH/ Sodium Hydroxide
KOH/ Potassium hydroxide
RbOH/ Rubidium Hydroxide
CsOH/ Caesium Hydroxide
Sr(OH)2/ Strontium Hydroxide
Ba(OH)2/ Barium Hydroxide

69
Q

What are weak bases?

A

NH4OH/Ammonium hydroxide
N(CH3)3/Trimethylamine
C5H5N/Pyridine
H2O/water

70
Q

What is a Neutralization reaction?

A

An acid and a base react to form water and a salt

71
Q

What is the equilibrium constant?

A

A number that expresses the relationship between the amounts of products and reactions present

72
Q

how the equilibrium value relates to what is predominant at equilibrium

A

A large value of the equilibrium constant K means that products predominate at equilibrium

73
Q

What is Le Chatelier’s principle?

A

The variables will shift as equilibrium shifts

74
Q

What is Acid Dissociation Constant?

A

A measure of the extent to which and acid dissociate in the solution and therefore its strength

75
Q

What are conjugate acid and base pairs

A

An acid and a base which differ only by the presence or absence of a proton are called a conjugate acid-base pair. Thus NH3 is called the conjugate base of NH4+, and NH4+ is the conjugate acid of NH3. Similarly, HF is the conjugate acid of F–, and F– the conjugate base of HF

76
Q

What happens during the Autoionization of water?

A

a proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻)

77
Q

what is the relationship between pKa and acid strength?

A

Lower the pKa value the stronger the acid

78
Q

What is the relationship between Ka and Acid strength?

A

The higher the Ka the stronger the Acid

79
Q

What is the relationship between pKa and pH?

A

pKa indicates whether an acid is a strong acid or a weak acid

80
Q

What is a buffer?

A

a solution that can resist pH change upon the addition of an acidic or basic components.

81
Q

How does the buffering system in blood work?

A

The Carbonic Acid-Bicarbonate buffer system is the most important buffer for maintaining the pH homeostasis of blood

82
Q

How do buffers relate to Le Chateliers principle?

A

The carbonic acid-bicarbonate chemical buffering systems help to maintain blood pH and is a good example of Le Chatelier’s principle at work in the human body

83
Q

How to calculate pH?

A

pH=-log[H3O+]

84
Q

How do you calculate morality?

A

Morality = mol/liters

85
Q

While do you find the molarity after mixing solution?

A

M1V1=M2V2

86
Q

Large Ka is a blank acid and small Ka is a blank acid

A

Strong, weak

87
Q

How do you find the pKa?

A

-log of Ka

88
Q

How can you tell if it is a conjugate base?

A

Take away the hydrogen

89
Q

If a reaction is exothermic it will go to the…

A

Left

90
Q

If a reaction is endothermic it will go to the

A

Right

Chem 1110 (9 decks)

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