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Physiology Exam 1 > Medical Biochemistry Chapter 2 > Flashcards

Medical Biochemistry Chapter 2 Flashcards

1
Q

life evocvled in what

A

water

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2
Q

organism typically contain

A

70tom 90%

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3
Q

Water is the perfect way, and what types of reactions occurs in aqueous solutions

A

solvent and chemical

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4
Q

Water has a what heat capacity

A

high

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5
Q

Water acts as a heat buffer to maintain internal temperatures

A

True

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6
Q

Is water more dense than ice?

A

yes

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7
Q

Water is a critical determinant of what?

A

structure and function of proteins, nucleic acids, and membranes

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8
Q

Water has a how many electron pairs and what geometrical shape does it have?

A

4 and tetrahedral

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9
Q

What does the elctronegavity of the oxygen have on water?

A

water serves as hydrogen bound donor and acceptor

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10
Q

Hexagonal ice forms a what lattice

A

regular

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11
Q

What is the entropy of hexagonal ice?

A

low

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12
Q

Why is ice more dense than water?

A

contains more hydrogen bond per water molecule

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13
Q

Ice doesn’t absorbs heat when melting which allows the delta S to be lesser?

A

False; Ice does absorbs heat when melting which allows the delta S to be greater

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14
Q

Water is a good solvent for

A

polar and charge molecules such as amino acids, peptides, alcohols, carbohydrates, nucleic acids

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14
Q

Water is a good solvent for

A

polar and charge molecules such as amino acids, peptides, alcohols, carbohydrates, nucleic acids

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15
Q

Water is a poor solvent for

A

non polar molecules such as non polar gases, aromatic rings, aliphatic chains, and lipids

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15
Q

Water is a poor solvent for

A

non polar molecules such as non polar gases, aromatic rings, aliphatic chains, and lipids

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16
Q

The high dielectric constant of water (ability to screen charges)

A

reduces the attraction between oppositely-charged ions in salt crystal

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17
Q

The stronger electrostatic interactions between the solvated ions and water molecules

A

lowers the energy of the system

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18
Q

What happens to the dissolving of NaCl?

A

entropy increases, spontaneous, positive enthalpy

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19
Q

Dissolved particles affect what?

A

boiling point. melting point, osmolarity, viscosity, surface tension, taste, and color

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20
Q

The cytoplasm of cells have

A

highly concentrated solutions and high osmotic pressure

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21
Q

What happens in hypotonic environments?

A

Water moves into he cel, stress the plasma membrane, and causes lysis

22
Q

What cells have prevented?

A

!. Bacteria and plants have rigid cell walls of sufficient strength to resist osmotic pressure
2. Some freshwater protists have an organelle that pumps water out of cell
3. In multicellular animals, blood plasma and interstitial fluid is maintained at as osmolarity close to cytosol. They also pump out ions into interstitial fluid, or pump water directly using aquaporins

23
Q

What does the effect of osmolarity depends on

A

number of dissolved particles and not their mass

24
Q

When water is a reactant, what happens to reactuons?

A

produced or consumed in reaction

25
Q

all forms can form

A

vam dẻ waals (weak bonds)

26
Q

all forms of weak attractions are based on

A

attraction between electrical charges

27
Q

What are bond measured in?

A

kJ or kcal

28
Q

Strong covalent bonds

A

493 kj/mol

29
Q

Weak bonds

A

4-30 kJ/ mol, broken by thermal energy.

30
Q

Hydrogen bonds

A

dipole movement of NH/OH molecules

31
Q

Ionic interactions

A

electrostatic interactions between permeantly charge species, or between the ion and a permanent dipole

32
Q

dipole interactions

A

electrostatic interactions between uncharged polar molecules

33
Q

Van der Waals interactions

A

weak interactions between all atoms, regardless of polarity, attractive and repulsive components

34
Q

Hydrophobic effect

A

the ordering of water molecules around non polar substances

35
Q

What is hydrogen bonds?

A

strong dipole-dipole or charge-dipole interaction that a rises between an acid and a base

36
Q

hydrogen bonds with neutral atom

A

2-6

37
Q

hydrogen bonds with one charged atom

A

12-21 kJ/mol

38
Q

regarding hydrogen bonds, what two most frequent electronegative bonded to?

A

nitrogen and oxygen

39
Q

When is hydrogen bonds are the most strongest?

A

when the bonded molecules are oriented to maximize electrostatic interaction

40
Q

In comparison to covalent bonds and hydrogen bonds, which one is weaker?

A

hydrogen is weaker and have a 2-21 kJ/mol, which indicates that the bond distance is greater with H bonds

41
Q

What is the source of unique properties of water?

A

H-bonds

42
Q

Why is H bond important?

A

structure and function of DNA, proteins, lipids, and sugars

43
Q

What is h bond involved in?

A

enzyme/substrate, hormone/receptors interactions, mRNA with tRNA

44
Q

What can water both serve as

A

h-bond donor and H-bond acceptor

45
Q

With four h-bonds per water molecules gives water its?

A

-high boiling
-high melting point
-large surface tension

46
Q

True or false: Hydrogen bonds between neighboring molecule are weak relative to the H-O covalent bonds

A

True

47
Q

Ionic bons

A

opposite charges attract, neutralized oppositely charged groups; 12-17 kJ/mol

48
Q

Where does van Der waals forces arise from?

A

nonspecific attractive forces that occurs when two atoms come close to each other, induces fluctuating charges caused by the nearness of the molecules

49
Q

Van der Waals radius

A

attractive and repulsive forces balance at a certain distance which is specific for each atom

50
Q

Organic molecules that tend to form H-bonds are

A

water soluble

51
Q

The energy of H-bonds is much greater Thant that of Van der Waals interactions

A

molecules will form H-bonds in preference of van der Waals interaction

52
Q

What cannot form H-bonds H-bonds?

A

Benzene and oil

53
Q

Nonpolar may seem ordered, however there’s a favorable entropy form water’s point of view

A

more self interactions; less clustering

54
Q

Polar molecules form

A

excellant H bond and soluble in water

Physiology Exam 1 (6 decks)

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