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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
What is cholesterol and what does it look like?
A waxy, fat-like substance, found in the cells in your body -27 carbon compound with a hydrocarbon tail
26
What is the difference between dietary fats and oils?
Dietary fats: solid at room temperature Oils: liquid at room temperature
27
What is the Concentration equation
M=n/v M=Molar concentration n=moles of solute V= liters of solution
28
What is morality?
A unit of concentration expressed as the number of moles in a dissolved solute per liter of solution
29
How do you find the mass percent and what is it?
-mass percent=(mass of chemical divided by total mass of compound)x100
30
What is volume percent and how do you find it?
The ratio of the volume of the solute to the total volume of solution -volume percent=(Volume of solute/volume of solution)x100
31
What is the mass/volume percent of solution defined as?
The ratio of the mass of solute that is present in a solution relative to the volume of solution as a whole
32
What is percentage concentration?
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
33
What is ppm and ppb?
Ppm: 1 part per million = Ppb: 1,000 parts per billion
34
What is the dilution equation?
(C1)(V1)=(C2)(V2)
35
What are the two parts of a solution?
A solute and a solvent
36
What is a solvent?
A liquid that causes a solute
37
What is a solute?
What “disappears” in the solvent
38
What are the 3 types of mixtures?
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
What is the difference between unsaturated, saturated, and supersaturated?
Unsaturated: below the curve Saturated: on the curve Supersaturated: above the curve
40
What is the relationship between solubility and temperature?
The solubility of most solid or liquid solutes increases with increasing temperature
41
What is Henry’s law?
If the pressure of a gas over liquid increases then the amount of gas dissolved in the liquid will increase (carbonated drinks)
42
What are the 4 types of electrolytes?
-Potassium (K) -Sodium (Na) -calcium (Calcium) -Magnesium (Mg)
43
What is the equivalent charge conversion for ions with -1 and +1?
1x1=1
44
What is the equivalent charge conversion for ions with -2 and 2+?
1/2x2=1
45
How do you find ppm?
(Mass of solute)/(mass of solution)x 10^6
46
How do you find ppb?
(Mass of solute)/(mass of solution)x 10^9
47
How do you find the morality?
(Mol of solute)(liters of solution)
48
What is osmosis?
Something moving from a higher concentration to a lower concentration (drop of food dye)
49
What does dilution mean?
The addition of a solvent that decreases the solute in the solution (water to orange juice)
50
What is osmotic pressure?
The minimum pressure added to the solution to halt the flow of solvent molecules
51
What is isotonic?
Equal osmotic pressure
52
What is hypotonic?
Solutions with lower osmotic pressure (water go in cell)
53
What is hypertonic?
An external solution that has a high solute concentration (water goes out)
54
What is hemolysis?
A blood cell burst (from hypotonic)
55
What is cremation?
A blood cell shrivel (hypertonic)
56
What happens during diffusion?
Particles in high concentration areas move toward low concentration
57
What happens during dialysis?
Remove waste products and excess fluid
58
What is active trasnsport?
Uses atp to get across cel membrane
59
What is passive transport?
Does not use atp to get across cell membrane
60
How do molecules use osmosis to transport across cell membrane?
they move from a region of higher water concentration to a region of lower water concentration
61
What is the equilibrium constant equation?
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
Something that has a pH value less than 7 indicates
It’s acidic
63
Something with a pH greater than 7 indicates
It’s a base
64
If a pH is 7 it is
Neutral
65
What is a base?
A substance that neutralize an acid by reacting with hydrogen ions
66
What is an acid?
A hydrogen containing substance that is capable of donating a proton
67
What are the strong acids?
HCl/Hydrochloric Acid HNO3/ Nitric Acid H2SO4/Sulfuric Acid HBr/ Hydrobromic Acid HI/ Hydroiodic Acid HClO4/ Perchloric Acid HClO3/ Chloric Acid
68
What are the strong bases?
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
What are weak bases?
NH4OH/Ammonium hydroxide N(CH3)3/Trimethylamine C5H5N/Pyridine H2O/water
70
What is a Neutralization reaction?
An acid and a base react to form water and a salt
71
What is the equilibrium constant?
A number that expresses the relationship between the amounts of products and reactions present
72
how the equilibrium value relates to what is predominant at equilibrium
A large value of the equilibrium constant K means that products predominate at equilibrium
73
What is Le Chatelier’s principle?
The variables will shift as equilibrium shifts
74
What is Acid Dissociation Constant?
A measure of the extent to which and acid dissociate in the solution and therefore its strength
75
What are conjugate acid and base pairs
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
What happens during the Autoionization of water?
a proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻)
77
what is the relationship between pKa and acid strength?
Lower the pKa value the stronger the acid
78
What is the relationship between Ka and Acid strength?
The higher the Ka the stronger the Acid
79
What is the relationship between pKa and pH?
pKa indicates whether an acid is a strong acid or a weak acid
80
What is a buffer?
a solution that can resist pH change upon the addition of an acidic or basic components.
81
How does the buffering system in blood work?
The Carbonic Acid-Bicarbonate buffer system is the most important buffer for maintaining the pH homeostasis of blood
82
How do buffers relate to Le Chateliers principle?
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
How to calculate pH?
pH=-log[H3O+]
84
How do you calculate morality?
Morality = mol/liters
85
While do you find the molarity after mixing solution?
M1V1=M2V2
86
Large Ka is a blank acid and small Ka is a blank acid
Strong, weak
87
How do you find the pKa?
-log of Ka
88
How can you tell if it is a conjugate base?
Take away the hydrogen
89
If a reaction is exothermic it will go to the…
Left
90
If a reaction is endothermic it will go to the
Right

Chem 1110 (9 decks)

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