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CHEM 105 LECTURE > Midterm Exam 3 > Flashcards

Midterm Exam 3 Flashcards

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1
Q

chemical reactions

A
  • represented by chemical equations
  • shows relationship between reactants&raquo_space;> products
  • involves breaking & forming of bonds (can be covalent or ionic)
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2
Q

what are the rules to balancing a chemical equation?

A
  • CANNOT add new reactants or products
  • CANNOT change formula of a reactant or product
  • coefficients are REDUCED to the SMALLEST WHOLE NUMBERS
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3
Q

what are the four types of chemical reactions?

A
  1. synthesis (condensation)
  2. decomposition
  3. single replacement
  4. double replacement
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4
Q

synthesis

A
  • also known as CONDENSATION
  • example: A + B = C
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5
Q

decomposition

A
  • opposite of synthesis
  • example: AB = A + B
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6
Q

single replacement

A
  • single exchange only
  • example: A+ BC = AC + B
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7
Q

double replacement

A
  • double exchange
  • example: AB + CD = AD + CB
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8
Q

how is water involved in terms of chemical reactions?

A
  • has many interactions in both chemistry and biochemistry
  • HYDROLYSIS: water (hydro) is being used to SPLIT (lyse) a molecule
  • acid (hydrogen ions H+) catalyzes hydrolysis of an ester - turns into a carboxylic acid
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9
Q

hydration

A

process where water IS ADDED to a double bond (within an ALKENE) in the presence of an ACID (H+) to form an ALCOHOL

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10
Q

dehydration

A
  • the oppostive of hydration
  • process where ALCOHOL LOSES WATER in the presence of an ACID (H+) *and heat to form an ALKENE
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11
Q

reduction

A
  • the GAIN of ELECTRONS
  • the LOSS of OXYGEN
  • the GAIN of HYDROGEN
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12
Q

oxidation

A
  • the LOSS of ELECTRONS
  • the GAIN OF oxygen
  • THE LOSS OF HYDROGEN
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13
Q

redox

A

meaning that reduction and oxidation ALWAYS OCCUR TOGETHER

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14
Q

combustion

A

specific oxidation reaction: when oxygen reacts with ORGANIC chemicals
- will always produce carbon dioxide & water

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15
Q

what do the alcohols oxidize into?

A

primary alcohols - ALDEHYDES
secondary alcohols - KETONES
tertiary alcohols - DOES NOT OXIDIZE
*aldehydes can oxidize into carboxylic acids

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16
Q

catalytic hydrogenation

A

hydrogen gas can be added to a double bond (alkene) in the presence of platinum (going from unsaturated to saturated)

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17
Q

what are the gas properties?

A
  • gases behave similarly regardless of their nature
  • gas particles DO NOT interact with one another
  • FREE to move about a container
  • they COLLIDE with container walls: makes PRESSURE
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18
Q

pressure

A

the force of collisions that take place between gas particles and an object

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19
Q

what are factors we have to consider in regards to pressure?

A

volume & temperature
GREATER VOLUME, PRESSURE DOWN
LOWER VOLUME, PRESSURE UP
GREATER TEMP, PRESSURE UP
LOWER TEMP, PRESSURE DOWN

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20
Q

atmospheric pressure

A

refers to the force applied on the earth’s surface

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21
Q

what are some important units to remember in terms of atmospheric pressure (what is the standard temperature & pressure)?

A

1 mmHg = 1 torr
1 atm = 760 torr = 760 mmHg

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22
Q

vapor pressure

A

when a liquid is placed in a closed container: will begin to EVAPORATE until a maximum pressure is reached
- changes with TEMPERATURE

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23
Q

boiling point

A

temperature when a liquid’s vapor pressure = atmospheric pressure

24
Q

Boyle’s Law

A

P1V1 = P2V2
(inital) (final)

25
Q

mixtures

A

contains two or more substances

26
Q

homogeneous mixtures

A

UNIFORMLY DISTRIBUTES the substances they contain
- these are also called SOLUTIONS!!!

27
Q

heterogeneous mixtures

A

DOES NOT uniformly distribute the substances they contain

28
Q

solvent

A

the component present in the greatest amount (water)

29
Q

solute

A

the component dissolved in the solvent (sugar dissolving in water)

30
Q

how does a solution form?

A
  • both solute and solvent particles are around the same size
  • both have to INTERACT with each other
  • interactions are NON-COVALENT (ionic bonds, dipole-dipole bonds, hydrogen bonds)
31
Q

like dissolves like

A

can help predict if the substance is soluble or insoluble

32
Q

solubility

A

the amount of solute that will dissolve in a solvent at a given temperature

33
Q

what happens when two homogenous mixtures react together?

A

they form a solid PRECIPITATE

34
Q

alkanes (hydrocarbons)

A

will EASILY MIX, but DO NOT DISSOLVE in water

35
Q

nonpolar hydrocarbons

A

cluster together through LONDON FORCES

36
Q

polar hydrocarbons

A

cluster and interact through H-BONDING

37
Q

how are biochemical compounds classified?

A
  • HYDROPHILIC: love water - compounds soluble in water
  • HYDROPHOBIC: hate water - compounds insoluble in water
  • AMPHIPATHIC: compounds that have both hydrophilic/phobic parts
38
Q

hydrophilic

A
  • often have compounds that resemble water
  • form typical H-BONDS
39
Q

hydrophobic

A
  • these are basic FATTY ACIDS that have long hydrocarbon chains
40
Q

amphipathic

A
  • can be originated from hydrophobic fatty acids with the added conversion of NaOH
41
Q

amphipathic nature

A
  • nonpolar interior: hydrophobic
  • polar exterior: hydrophilic
42
Q

concentration

A

refers to the amount of solute that is dissolved in a solvent

43
Q

saturated concentration

A

solvent that holds the MAXIMUM amount of solute that can be dissolved at a particular temp

44
Q

unsaturated concentration

A

holding LESS than a saturating amount of solute within a solvent

45
Q

what are the calculations for concentration?

A
  1. weight/volume
    % = g of solute/mL of solution x 100
  2. volume/volume
    % = mL of solute/mL of solution x 100
  3. weight/weight
    % = g of solute/g of solution x 100
46
Q

molarity

A

commonly used to report concentration

46
Q

what are the formulas for concentration?

A

ppt = g of solute/mL of solution x 10^3

ppm = g of solute/mL of solution x 10^6

ppb = g of solute/mL of solution x 10^9

46
Q

M equivalent

A

g of solute/L of solution

47
Q

equivalent (eq)

A

number of moles of charges that one mole of a solute contributes to a solution

48
Q

dilution

A

easy way to reduce the concentration of a solution by adding more solvent

V(original) x C(original) = V (final) x C(final)

49
Q

suspensions

A

contains large particles suspended in a liquid
- VISIBLE particles to the naked eye
- will SETTLE due to gravity after enough time
- can be separated from the liquid

50
Q

colloids

A

contains larger particles larger than solutions but SMALLER than suspensions
- NON-VISIBLE particles to the naked eye
- will NOT SETTLE upon standing

51
Q

diffusion

A

substances move from areas of higher concentration to areas of lower concentration

52
Q

semipermeable membranes

A

allow only SOLVENTS (water) to pass through while SOLUTES cannot pass

53
Q

solvent molecules (diffusion)

A

pass from side of lower solute concentration to the side of higher solute concentration to reach equilibrium

54
Q

osmosis

A

net movement of water from a solution of lower concentration to a solution of higher concentration

55
Q

blood plasma concentration

A

isotonic - same concentration inside and outside the cell
hypertonic - greater concentration with water flowing OUT (crenation)
hypotonic - lower concentration with water flowing IN (hemolysis)

CHEM 105 LECTURE (17 decks)

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