Ch 10 Section 5 Flashcards

1
Q

water is the most abundant

A

liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

oceans, rivers, and lakes cover about

A

75% of earth’s surface

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

water is an essential component of all organisms: 70% to 90% of the mass of living things is

A

water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

the chemical reactions of most life processes takes place in water, and water is frequently a

A

reactant or product in such reactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

water molecules consist of two atoms of hydrogen and one atom of

A

oxygen united by polar-covalent bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

water molecule shape:

A

bent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

the angle between the two hydrogen-oxygen bonds is about

A

105 degrees

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

this is close to the angle expected for … of the oxygen-atom orbitals

A

sp3 hybridization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

the molecules in solid/ liquid wate rare linked by

A

hydrogen bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

the number of linked molecules decreases with increasing temperature because increases in kinetic energy make

A

hydrogen bond formation difficult

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

nevertheless, there are usually from … to … molecules per…

A

4 to 8; group in liquid water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

if it were not for these molecular groups, water would be a

A

gas at room temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

nonpolar molecules, such as methane, that are similar in size and mass to water molecules do not

A

undergo hydrogen bonding. they are gases at room temp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ice consists of water molecules in the

A

hexagonal arrangement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

the empty spaces between molecules in this pattern account for the relatively

A

low density of ice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

as ice is heated, the increased energy of the molecules causes them to

A

move and vibrate more vigorously

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

when the melting pt is reached, the energy of the molecules is so great that the

A

rigid open structure of the ice crystals breaks down, and ice turns into liquid water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

hydrogen bonds between molecules of liquid water at 0 degrees celsius are …. and more …. than those between molecules of ice at the

A

fewer; disordered; same temperature

19
Q

because the rigid open structure of ice has broken down, water molecules can

A

crowd closer together

20
Q

liquid water is

A

denser than ice

21
Q

as the liquid water is warmed from 0 degrees celsius, the water molecules

A

crowd still closer together

22
Q

water molecules are as tightly packed as possible at

A

3.98 degrees celsius

23
Q

at temperatures above 3.98 degrees celsius, the increasing kinetic energy of the water molecules causes them to

A

overcome molecular attractions

24
Q

the molecules move farther apart as the temperature continues to

A

rise

25
Q

as the temperature approaches the boiling point, groups of liquid water molecules absorb enough energy to

A

break up into separate molecules

26
Q

because of hydrogen bonding between water molecules, a high kinetic energy is needed, causing water’s boiling point to be

A

relatively high (100 degrees celsius) compared to other liquids that have similar molar masses

27
Q

at room temperature, pure liquid water is

A

transparent, odorless, tasteless, and almost colorless

28
Q

any observable odor or tase is caused by

A

impurities, such as dissolved minerals, liquids, or gases

29
Q

water freezes and ice melts at

A

0 degrees celsius at a pressure of 1 atm

30
Q

molar enthalpy of fusion of ice is

A

6.009 kJ/mol

31
Q

the molar enthalpy of fusion of ice is relatively larged compared with the molar enthalpy of fusion of

A

other solids

32
Q

water has the unusual property of …. in volume as it freezes, because its molecules form an..

A

expanding; open rigid structure

33
Q

ice at 0 degrees celsius has a density of only about …. wile liquid water at 0 degrees celsius has a density of

A

.917 g/ cm3 ; .99984 g/ cm3

34
Q

this lower density explains why ice floats in

A

liquid water

35
Q

the insulating effect of floating ice is particularly important int he case of

A

large bodies of water

36
Q

iv ice were more dense than liquid water, it would sink to the bottom of

A

lakes and ponds, where it would be less likely to melt completely

37
Q

the water of such bodies of water in temperature climates would eventually

A

freeze solid, killing nearly all the living things in it

38
Q

at 100 degrees celsius (boiling point at 1 atm) water’s molar enthalpy of vaporization is

A

40.79 kJ/ mol

39
Q

both the boiling pt and the molar enthalpy of vaporization of water are quite high compared with those of

A

nonpolar substances of comparable molecular mass, such as methane

40
Q

the values are high because of the strong hydrogen bonding that must be overcome for

A

boiling to occur

41
Q

the high molar enthalpy of vaporization makes water useful for

A

household steam-heating systems

42
Q

the steam (vaporized water) stores a great deal of

A

energy as heat

43
Q

when steam condenses in radiators, great quantities of

A

energy are released