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Biology-149 > Chapter 2: The Chemical Basis of Life > Flashcards

Chapter 2: The Chemical Basis of Life Flashcards

Atoms, Molecule, and Water

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1
Q

What are the three types of matter?

A

Solid, liquid and gas.

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2
Q

Atoms

A

The smallest functional unit of matter that forms all chemical substances.

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3
Q

Element

A

A pure substance made of only one kind of atom.

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4
Q

Compound

A

Two or more different elements.
Example: H2O

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5
Q

Molecule

A

Same atoms that are connected
Example: O2

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6
Q

What are the three subatomic particles?

A

Protons, Neutrons, and Electrons

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7
Q

Protons

A

Positive Charge and found in the nucleus

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8
Q

Neutrons

A

No charge/ Neutral and are found in the nucleus.

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9
Q

Electrons

A

Negative charge and found on orbitals. Participate in chemical reactions.

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10
Q

How many electrons can the first orbital hold?

A

2 Electrons

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11
Q

The more electrons you have the more…?

A

Power

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12
Q

Valence Electrons

A

The electrons on the outer shell that are important for chemical bonds.

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13
Q

To fill the outer shell

A

atoms will share, gain or lose electrons.

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14
Q

Atomic number

A

Represents the number of protons

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15
Q

Mass number

A

The sum of protons and neutrons.

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16
Q

To find the number of neutrons you must…?

A

subtract mass number and atomic number.

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17
Q

Four elements that most abundant in life are

A

Hydrogen, Oxygen, Nitrogen and Carbon

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18
Q

Molecular formula

A

contains chemical symbols of the elements in the molecule.

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19
Q

What are isotopes?

A

The same number of protons, different number of neutrons.
Sometimes radioactive
Used for carbon dating.

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20
Q

Electronegativity

A

The measure of an atom’s ability to attract electrons in a bind with another atom.

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21
Q

Octet Rule

A

Determines bonding behavior.
Stable or “complete” when the valence shell has 8 electrons.
Unstable or “incomplete” when the shell has less than 8 electrons.

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22
Q

Types of molecular bonding

A

Ionic Bonds
Covalent bonds
Hydrogen bonds

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23
Q

Ionic bonds

A

Atoms take an electron from another.
These are bond attractions between ions of opposite charge.
These compounds are called salts.

24
Q

Cation

A

Positive charge ion

25
Q

Anion

A

Negative charge ion

26
Q

Covalent Bonds

A

A bond forms when elements SHARE a pair of electrons.
Strongest bonds.
Occurs between atoms with unfilled valence electron shells.

27
Q

Polar Covalent Bonds

A

Unequal sharing of electrons.
Creates polarities (difference in electric charge)

28
Q

Non-polar Covalent Bonds

A

Equal sharing of electrons, no charge difference. Happens with atoms with similar electronegativities.

29
Q

Why are covalent bonds strong chemical bonds?

A

The shared electrons behave as if they belong to each atom.

30
Q

Hydrogen Bonds

A

The hydrogen atom from one polar molecule is attracted to an electronegative atom of another.

31
Q

Chemical Reaction

A

When one or more substances are changed into other substances.

32
Q

Properties of Chemical Reactions

A

Require a source of energy (heat)
In living organisms, they often use an enzyme as a catalyst (an agent that speeds up a chemical reaction)
They tend to proceed in a particular direction but will eventually reach equilibrium.
It usually occurs in liquids.

33
Q

What will dissolve in water?

A

Ions and molecules with polar covalent bonds.

34
Q

Solution

A

Solutes in a solvent

35
Q

Hydrophobic

A

lacking affinity for water (dislikes water, does not mix, nonpolar)

36
Q

Hydrophilic

A

having an affinity to water (to like water, polar)

37
Q

Amphipathic

A

Both hydrophilic and hydrophobic

38
Q

Hydrogen bonding explains most of the water’s life’s supporting properties…

A

Water as a solvent
Cohesion
Water moderates temperature
Ice floats

39
Q

Concentration

A

The amount of a solute dissolved in a unit volume of solution.

40
Q

Molarity

A

Number of moles of a solute dissolved in water.

41
Q

Cohesion

A

attraction of identical molecules

42
Q

Water molecules stick together as a result of?

A

Hydrogen Bonding

43
Q

Surface Tension

A

The measure of how difficult it is to stretch or break the surface of a liquid.

44
Q

Adhesion

A

Ability to stick to polar surfaces.

45
Q

Water moderates temperature

A

Because of hydrogen bonding, water has a resistance to temperature change.
Highest heat capacity of any liquid.

46
Q

Ice Floats

A

Water is less dense as a solid than as a liquid, this allows fish and other organisms to survive under ice. Water expands when frozen.

47
Q

Heat of Vaporazation

A

Energy to boil

48
Q

Heat to fusion

A

Energy to melt.

49
Q

Acid

A

pH = 0-7
High hydrogen concentrations
Donates protons/hydrogen atoms.

50
Q

Bases (Alkaline)

A

pH= 7-14
Low hydrogen concentrations
Accepts protons/hydrogen ions

51
Q

Neutral

A

pH= 7.0

52
Q

pH scale

A

Describes how acidic or basic a solution is. A measure of the concentrations of hydrogen bonds.

53
Q

The pH of a solution can affect:

A

The shapes and functions of molecules
The rates of many chemical reactions
The ability of two molecules to bind together.
The ability of ions or molecules to dissolve in water. Small changes in pH can have a big impact on biological processes.

54
Q

Buffers are composed of

A

weak acid/base and its salt.

55
Q

The function of a buffer is

A

to reduce the change in pH when an acid or base is added.

56
Q

Waters important functions

A

Participates in chemical reactions
Provides force or support
Removes toxic waste
Evaporative cooling
Lubrication
Cohesion and Adhesion

Biology-149 (16 decks)

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