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Biochemistry LEC > Module 2: Water > Flashcards

Module 2: Water Flashcards

1
Q

the bonds that hold atoms to atoms
and make compounds

A

Intramolecular bonds

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2
Q

3 types of intramolecular bonds

A

covalent, ionic, and metallic

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3
Q

a bond in which a pair or pairs of electrons is shared by
two atoms

A

Covalent Bond

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4
Q

covalent bonds between two atoms that have a difference in
electronegativity

A

Polar

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5
Q

covalent bonds between two atoms that have equal
electronegativity

A

Nonpolar

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6
Q

a bond that holds atoms together in a compound;
the electrostatic attraction between charged ions

A

Ionic Bond

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7
Q

a bond resulting from the attraction between positive ions and surrounding mobile electrons

A

Metallic Bond

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8
Q

Forces occur between molecules

A

Intermolecular forces

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9
Q

the weakest intermolecular force and
consist of dipole-dipole forces and dispersion forces

A

Van der Waals forces

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10
Q

result of electron movement within the molecule,
producing a temporary induced dipole with neighboring molecules

A

London dispersion forces

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11
Q

List examples of London Dispersion Forces

A

Halogens, Nobel Gases, Gases, Hydrocarbons

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12
Q

strength of dispersion forces tends to increase with

A

increased molecular weight

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13
Q

The strength of dispersion forces tends to increase with
increased molecular weight, this is because

A

larger electron clouds that are easier to polarize

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14
Q

Why are molecules that have permanent dipoles attracted to each other?

A

positive end of one is attracted to the negative end of the other

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15
Q

True or False? The more polar the molecule the higher its boiling point

A

True

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16
Q

These interactions will occur between partial positive and partial negative charges on different molecules

A

Dipole-dipole interaction

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17
Q

Occurs between molecules containing a hydrogen bonded to fluorine, oxygen, or nitrogen

A

Hydrogen Bonding

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18
Q

True or False? Presence of hydrogen bonding in a molecule indicates a high boiling point.

A

True

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19
Q

Occurs between an ionic and polar compound

A

Ion-dipole interactions

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20
Q

two attractive forces in ion-dipole

A
  • Between a cation and partial negative end of a polar molecule
  • Between an anion and partial positive end
    of a polar molecule
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21
Q

Why are ion-dipole interactions important in solutions of ions

A

strength of these forces is what makes it possible for ionic substances to dissolve in polar solvents

22
Q

List the intramolecular forces from strongest to weakest

A

metallic bond, ionic bond, polar covalent bond, nonpolar covalent bond

23
Q

List the intermolecular forces from strongest to weakest

A

Hydrogen Bonding, Dipole-Dipole attraction, London dispersion attraction

24
Q

Resistance of a liquid to flow

A

viscosity

25
Q

related to the ease with which molecules can move past each other

A

viscosity

26
Q

True or false? Viscosity increases with stronger intermolecular forces and decreases with higher temperature

A

True

27
Q

results from the net inward force experienced by the molecules on the surface of a liquid

A

Surface tension

28
Q

True or False? As temperature decreases, surface tension increases

A

True

29
Q

What is the value of Blood pH?

A

7.4

30
Q

When a solution contains equal amounts of [H+] and [OH-], it is said to be

A

Neutral

31
Q

Solutions with an excess of H+ are

A

Acidic

32
Q

Solutions with an excess of OH- are

A

basic

33
Q

how strongly the atoms pull electrons

A

Electronegativity

34
Q

the weak attraction between the hydrogen atom of one
water molecule and the oxygen atom of another

A

Hydrogen bond

35
Q

Water molecules tend to stick together

A

cohesion

36
Q

what is being dissolved

A

Solute

37
Q

the solute in the solvent

A

Solution

38
Q

a measure of the relative amounts of acids and bases in a solution

A

pH scale

39
Q

pH greater than 7

A

basic

40
Q

Pure water pH = 7

A

neutral

41
Q

pH lower than 7

A

acidic

42
Q

help maintain a relatively constant hydrogen ion concentration

A

Buffers

43
Q

the capacity of a buffer to maintain a specific pH

A

Buffering capacity

44
Q

a condition that occurs when human blood pH falls below 7.35

A

Acidosis

45
Q

if blood pH rises above 7.45

A

Alkalosis

46
Q

-something that has a proton and is willing to give it up.
- or may be defined as a hydrogen ion donor

A

Acid (HA)

47
Q
  • something that has a place to put a proton
  • as a hydrogen ion acceptor
A

Base

48
Q

_____ completely dissolves in H2O

A

Strong acids

49
Q

_____don’t completely dissolve in H2O

A

Weak acids

50
Q

Organic acids (compounds with carboxyl groups) are referred to as

A

weak acids

51
Q

is used for calculating the pH and concentration of a buffer

A

Henderson-Hasselbalch Equation

Biochemistry LEC (4 decks)

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