2.4 The Chemical Level Of Organization: Inorganic Compounds And Solutions

Front 1

What are inorganic compounds?

Back 1

Compounds that usually lack carbon and are structurally simple.

Front 2

What are some common inorganic compound types?

Back 2

Water and many salts, acids, and bases.

Front 3

Do inorganic compounds have ionic or covalent bonds.

Back 3

May have ionic or covalent.

Front 4

Which common inorganic compounds contain carbon?

Back 4

Carbon dioxide (CO2)

Bicarbonate ion (HCO3−)

Carbonic acid (H2CO3).

Front 5

What are the defining features of organic compounds?

Back 5

Always contain carbon

Usually contain hydrogen

Always have covalent bonds

Most are large molecules

Front 6

What is the most important property of water? Why is this important? (3 reasons)

Back 6

Its polarity.

1. Makes water an excellent solvent for other ionic or polar substances

2. Gives water molecules cohesion

3. Allows water to resist temperature changes

Front 7

What is the universal solvent?

Back 7

Water.

Front 8

Usually there is (less/more) solvent than solute in a solution.

Back 8

Usually there is more solvent than solute in a solution.

Front 9

What are common examples of hydrophilic solutes?

Back 9

Sugar and salt.

Front 10

What properties of solutes make them hydrophilic?

Back 10

Solutes that are charged or contain polar covalent bonds.

Front 11

What properties of solutes make them hydrophobic?

Back 11

Mainly nonpolar covalent bonds.

Front 12

What are common examples of hydrophobic compounds?

Back 12

Animal fats and vegetable oils.

Front 13

Table sugar (sucrose) easily dissolves in water but is not an electrolyte. Is it likely that all the covalent bonds between atoms in table sugar are nonpolar bonds? Why or why not?

Back 13

No. Because sugar easily dissolves in a polar solvent (water), you can correctly predict that it has several polar covalent bonds.

Front 14

What is hydrolysis?

Back 14

Decomposition reaction that breaks down large molecules into smaller molecules by the addition of water molecules.

Front 15

What are dehydration synthesis reactions?

Back 15

When two smaller molecules join to form a larger molecule, a water molecule is one of the products formed.

Front 16

Water is said to have a (high/low) heat capacity. What does this mean?

Back 16

Water is said to have a high heat capacity.

Water can absorb or release a relatively large amount of heat with only a modest change in its own temperature.

Front 17

Water's head of vaporization is (high/low). How do you know?

Back 17

Water's head of vaporization is high. Water requires a large amount of heat to change from a liquid to a gas.

Front 18

What is a mixture?

Back 18

A combination of elements or compounds that are physically blended together but not bound by chemical bonds.

Front 19

What is a colloid?

Back 19

Solute particles in a colloid are large enough to scatter light. Usually appear translucent or opaque.

Front 20

What is a suspension?

Back 20

Suspended material may mix with the liquid or suspending medium for some time, but eventually it will settle out.

Front 21

What does it mean to dissociate?

Back 21

When inorganic acids, bases, or salts dissolve in water, they separate into ions and become surrounded by water molecules.

Front 22

What is an acid?

Back 22

A substance that dissociates into one or more hydrogen ions (H+) and one or more anions.

Front 23

An acid is also referred to as what?

Back 23

As a proton donor.

Front 24

What is a base?

Back 24

Removes H+ from a solution, dissociates into one or more hydroxide ions (OH−) and one or more cations.

Front 25

A base is also referred to as what?

Back 25

A proton acceptor.

Front 26

What is a salt?

Back 26

When dissolved in water, dissociates into cations and anions, neither of which is H+ or OH−.

Front 27

The compound CaCO3 (calcium carbonate) dissociates into a calcium ion (Ca2+) and a carbonate ion (CO32−). Is it an acid, a base, or a salt? What about H2SO4, which dissociates into two H+ and one SO42−?

Back 27

CaCO3 is a salt, and H2SO4 is an acid.

Front 28

What is the pH scale?

Back 28

A measure of the concentration of hydrogen ions (H+) in a solution. The pH scale extends from 0 to 14, with a value of 7 expressing neutrality, values lower than 7 expressing increasing acidity, and values higher than 7 expressing increasing alkalinity.

Front 29

What is a buffer system?

Back 29

A weak acid and the salt of that acid (that functions as a weak base). Buffers prevent drastic changes in pH by converting strong acids and bases to weak acids and bases.

Front 30

What is an important buffer system in the body?

Back 30

The carbonic acid–bicarbonate buffer system.