The Chemistry Of Life

Front 1

Define matter

Back 1

Matter is anything that has mass and takes up space. The various forms of matter are composed of one or more elements.

Front 2

What is the periodic table?

Back 2

Table of elements in order of Atomic number

Front 3

List the four most abundant elements in living things

Back 3

oxygen carbon hydrogen nitrogen

Front 4

Define compound and give an example.

Back 4

Compound is two or more elements in a fixed ratio CO2 is Carbon Dioxide

Front 5

Give an example of how the properties of a compound differ from the properties of the individual elements.

Back 5

Water is a liquid at room temperature but hydrogen and oxygen are both gases.

Front 6

Define Atom.

Back 6

Smallest piece or particle of an element

Front 7

List and describe the change of the three subatomic particles.

Back 7

Protons: Postive

Neutrons: Neutral

Electrons: negative

Front 8

Discuss the location of the subatomic particles.

Back 8

Neutrons and Protons are in the Nucleus and Electrons are found in the electron cloud

Front 9

What is the atomic number?

Back 9

The number of protons in each element also electrons Atomic mass is also found on the periodic table.

Front 10

Define isotopes and radioactive isotopes.

Back 10

Different forms of different numbers of neutrons

Front 11

List the three subatomic particles that make up an atom.

Back 11

Electrons neutrons protons

Front 12

Name the four most abundant elements of the human body.

Back 12

Oxygen carbon hydrogen nitrogen

Front 13

What part of an atom is involved in forming bonds?

Back 13

Electrons outer or valence electrons Valence electrons are involved in ionic and covelent bonds.

Front 14

Briefly describe ionic bonds.

Back 14

Ion -Atom that gives or receives electrons

Ionic Bonds - formed when one atom transfers more electrons to another

Front 15

Define Ion.

Back 15

Atoms with either a positive or negative charge.

Front 16

Explain how an ionic bond forms.

Back 16

An atom that loses elections becomes positive ion and atom that gains electrons become a negative ion

Front 17

When are covalent bonds formed?

Back 17

Formed when electrons are shared by the atoms each electron pair forms a covalent bond.

Front 18

How many covalent bonds can an atom form?

Back 18

Same as number of electrons needed to all its outer shell

Front 19

Describe van der Waals forces.

Back 19

Slight attraction between molecules that can develop between a positively charged regions of nearby molecules

Front 20

Define chemical reaction.

Back 20

Molecules become rearranged is exisiting bonds break and new bonds are formed.

Front 21

Briefly discuss the reactants and products of a chemical reaction.

Back 21

Reactant are the two things added together products are the answer

Front 22

Does the compound pictured here show covalent bonding or ionic bonding?

Back 22

covalent

Front 23

What is the importance of valence electrons?

Back 23

To bond to other elements

Front 24

Exothermic

Back 24

release more energy than absorbed HOT

Front 25

Endothermic

Back 25

absorbs more than it releases COLD

Front 26

What is a polar molecule?

Back 26

A molecule that has both negative or positive charges.

Front 27

Describe the polarity of water.

Back 27

The water molecule has more negative charge around the oxygen atom and has more positive charge around the hydrogen atoms

Front 28

Describe hydrogen bonds.

Back 28

The hydrogen atoms attract to the negative oxygen atoms

Front 29

List the four unique properties of water.

Back 29

1. Cohesion and adhesion

2.Specific heat capacity.

3. Lower density of ice compared to liquid water

4. Water's ability to dissolve other substances.

Front 30

Compare and contrast cohesion and adhession

Back 30

Cohesion - the attraction between molecules of the same substance.

Adhesion - the attraction between unlike molecules.

Front 31

Briefly describe why cohesion and adhesion are important in plants.

Back 31

Adhesion between water molecules and the walls of plant vessels draw water up out of the roots into stems and leaves.

Cohesion between water molecules hold the column of water together as it rises. Capillary reaction

Front 32

Describe surface tension.

Back 32

Surface tension pulls water molecules tightly together at the forming an invisible boundary.

Front 33

Where are hydrogen bonds formed?

Back 33

Between water molecules.

Front 34

Define specific heat capacity.

Back 34

Amount of heat energy required to raise temp. of 1 gram of material b y 1 degree celsius

Front 35

Why is water's high specific heat capacity important?

Back 35

Allows bodies of water to absorb large amounts of heat with only small changes in temperature.

Front 36

How is water involved in body temperature regulation in humans?

Back 36

Sweating lowers body heat when water evaporates off the surface of the skin

Front 37

Compare the density of ice with that of water.

Back 37

Ice has less closely packed molecules than liquid that is how it floats.

Front 38

Why is it important that ice floats

Back 38

Living organisms have access to nutrients at the bottom of the body of water. Ice insulates the liquid water.

Front 39

Define solution

Back 39

Solution - uniform mixture of two or more substances

Solvent - Does the dissolving for substance

Solute - Dissolves itself

Front 40

What is an aqueous solution?

Back 40

A solution where water is the solvent

Front 41

Name the ions that are formed when water molecules break apart in solution.

Back 41

Hydrogen ions (H+)

Hydroxide ions (OH-)

Front 42

Draw a pH scale (on the answer card)

Back 42

Front 43

Define acid and list some examples.

Back 43

Acids have a pH lower than 7 Acids are compounds that form H+ ions in solution.

Ex. Hydrochloric acid

Sulfuric acid

Cetric acid

Front 44

Define base and list some examples.

Back 44

Compounds that produce hydroxide ions

Bases have a pH higher than 7

Sodium hydroxide

Sodium bicarbonate or baking soda

Front 45

Define buffers and explain why are they important in living things.

Back 45

A weak acid or base that can react with strong acids or bases. To prevent sharp, sudden changes in pH

Buffers maintain homeostasis

Buffers maintain 7.35 - 7.45 in the bloodstream

Front 46

Describe unique property of water caused by its polarity and hydrogen bonding.

Back 46

Cohesion and adhesion

Specific heat capacity

Lower density of ice compared to liquid water

Water ability to dissolve other substances.

Front 47

How do pH values differ between acids and bases?

Back 47

pH 7- Acids form H+ ions

Base pH 7+ form hydroxide ions have pH 7+