Chapter 3 Water And Life

Front 1

Polar molecule

Back 1

The opposite ends have opposite charges

Front 2

Four emergent properties of water

Back 2

Cohesive behavior, ability to moderate tempurate, expansion upon freezing, versatility as a solvent

Front 3

Cohesion

Back 3

When Hydrogen bonds hold water molecules together

Front 4

Adhesion

Back 4

An attraction between different substances. Ex. Water and plant cells

Front 5

Surface tension

Back 5

The measure of how hard it is to stretch or break the surface of a liquid. It is related to cohesion

Front 6

Moderation of temperature by water

Back 6

Water absorbs hear from warmer air and releases stored heat to cool air. Water can absorb or release a large amount of heat with only a slight change in its own temperature.

Front 7

Kinetic energy

Back 7

The energy of motion

Front 8

Thermal energy

Back 8

The total kinetic energy associated with random movement of atom or molecules (matters volume)

Front 9

Temperature

Back 9

The average kinetic energy of the molecules in a body of matter

Front 10

Heat

Back 10

The transfer of thermal energy from one body of matter to another

Front 11

Calorie

Back 11

The amount of heat required to raise the temperature of 1g of water

Front 12

Joul

Back 12

Is another unit of energy where 1J= .239 calories. Or 1cal=4.184J

Front 13

Specific heat

Back 13

The amount of heat that must be absorbed or loft for 1g of that substance to change its temperature.

Front 14

Evaporation

Back 14

Transformation of a substance from liquid to gas

Front 15

Heat of vaporization

Back 15

The heat a liquid must absorb for 1g to be converted to gas

Front 16

Evaporative cooling

Back 16

The process of a liquid evaporates it's remaining surface cools

Front 17

Evaporative cooling

Back 17

Helps stabilize temperatures in organisms and bodies of water

Front 18

Solution

Back 18

A liquid that is homogenous mixture of substances

Front 19

Solvent

Back 19

The dissolving agent of a solution

Front 20

Solute

Back 20

Substance that is dissolved

Front 21

Aqueous solution

Back 21

One in which water is the solvent

Front 22

Hydration shell

Back 22

When an ionic compound is dissolved in water each ion is surrounded by a sphere of water molecules called a hydration compound.

Front 23

Hydrophillic

Back 23

Substance that has an affinity for water

Front 24

Hydrophobic

Back 24

Substance is one that does not have an affinity for water

Front 25

Molecular mass

Back 25

The sum of all masses of all atoms in a molecule

Front 26

1mol

Back 26

6.02 x 10^23

Front 27

Avocados number

Back 27

6.02 x 10^23 daltons=1g

Front 28

Molarity

Back 28

The number of moles of solute per liter of solution

Front 29

Hydrogen (H+)

Back 29

The hydrogen atom leaves it's electron behind and is transferred as a proton

Front 30

Hydronium

Back 30

The molecule with the extra proton is now a hydronium ion (H+)

Front 31

Hydroxide ion OH-

Back 31

The molecule that lost the proton

Front 32

Water in a state of dynamic equilibrium (pic)

Back 32

Front 33

Though statistically rare, the dissociation of water molecules has a great effect on organisms

Back 33

In pure water 554 million water molecules dissociated

Front 34

Concentrations of H+ OH-

Back 34

Are equal in water

Front 35

Acid

Back 35

Any substance that increases the H+ concentration of a solution

Front 36

Base

Back 36

Any substance that reduces the H+ concentration of a solution

Front 37

Examples of pH levels (pic)

Back 37

Front 38

Buffers

Back 38

Substances that minimize changes in concentrations of H+ and OH- in a solution

Front 39

Fossil fuels

Back 39

CO2 is a main product of fossil fuel combustion. 25% of human generated CO2 is absorbed by the oceans.

Front 40

Ocean acidification

Back 40

Yhe proccess in which CO2 is dissolved in sea water forms carbon acid

Front 41

hydrophilic

Back 41

ionic and polar substances; they have an affinity for water due to electrical attractions and hydrogen bonding

Front 42

hydrophobic

Back 42

non-polar and nonionic substances; they will not easily mix with or dissolve in water

Front 43

molecular mass

Back 43

the sum of the mass of all atoms in the molecule

Front 44

mole (mol)

Back 44

is the amount of a substance that has a mass in grams numerically equivalent to its molecular mass.

Front 45

molarity

Back 45

refers to the number of moles of a solute dissolved in 1 liter of solution

Front 46

buffers

Back 46

regulate an organism's pH

Front 47

hydrogen bonding between polar water molecules

Back 47

creates a cohesive liquid with a high specific heat and high heat vaporization, both of which help to regulate environmental temperature.

Front 48

Ice

Back 48

floats and protects oceans and lakes from freezing

Front 49

The polarity of water

Back 49

makes it versatile solvent

Front 50

The H+ in a solution

Back 50

is expressed as pH and determines if a solution is acidic, neutral or basic

Front 51

A water molecule consists of

Back 51

two hydrogen atoms, each bonded to a more electronegative oxygen atom by a polar covalent bond

Front 52

the polar molecule

Back 52

has a V shape with partial positive charge on each hydrogen atom and a partial negative charge associated with the oxygen

Front 53

Creates a structural organization that leads to emergent properties of water?

Back 53

Hydrogen bonds

Front 54

hydrogen bonds are

Back 54

electrical attractions between the hydrogen atom of one water molecule and the oxygen atom of a nearby water molecule

Front 55

how many water molecules can hydrogen bond to one water molecule?

Back 55

four

Front 56

thermal energy is a measure of

Back 56

kinectic energy (the energy of motion) associated with the random movement of atoms and molecules.

Front 57

temperature measures

Back 57

the average kinetic energy of molecules in a body of matter

Front 58

thermal energy reflects

Back 58

total kinetic energy in that matter, which relates to volume of body of matter.

Front 59

the thermal energy that transfers from warmer to cooler body of matter is defined as

Back 59

heat

Front 60

How is heat measured?

Back 60

a calorie calorie is the amount of heat it takes to raise 1 g of water 1 degree celsius. A kilocalorie is 1,00 calories, the amount of heat required or released to change the temperature of 1 kg of water by 1 degree Celsius. A joule equals 0.239 cal; one calorie is 4.184 j

Front 61

a calorie (cal) is?

Back 61

the amount of heat it takes to raise 1g of water1 degree celsius

Front 62

What is the amount of amount absorbed or lost when 1 g of a substance changes its temp by 1 degree celsius?

Back 62

Specific heat

Front 63

What is water's specific heat of 1 cal/g degrees celsius?

Back 63

is unusually high compared with other common substances

Front 64

why does water absorb or release a relatively large quantity of heat as its temperature changes?

Back 64

heat must be absorbed to break hydrogen bonds, before water molecules can move faster and the temperature can rise, and conversely, heat is released when hydrogen bonds form as water molecules slow down when the temperature of water drops.