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Bio 235 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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Biology 101 flashcards
1
Q

Ionic bond

A

An atom with an electric charge
One atom is the electron donor (loses electron), one an electron acceptor
Cation (lost negative electron) = POSITIVE charge
Anion (gained negative electron =more negative) = Negative charge
Example is sodium chloride

Opposites attract

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2
Q

Covalent bond

A

Strong bond involving shared electrons
If sharing one pair of electrons =single
If sharing two pair= double. Etc
Polar =unequal sharing of electrons, one atom has a stronger electronegativity (water)
Nonpolar= equal sharing of electrons between atoms that have equal pull

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3
Q

Hydrogen bond

A

Weak polar bond
In water causes surface tension (cohesion)

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4
Q

Matter exists in 3 states …

A

Solids, liquids, gases

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5
Q

Elements in the body

A

26 different chemical elements are normally found in the body.
Only four of those are considered “major elements” and constitute 96% of the body’s mass.
Oxygen, carbon, hydrogen, and nitrogen

8 others the “lessers” =3.6%
Calcium, phosphorus, potassium, sultry, sodium, chlorine, magnesium, and iron.

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6
Q

Atom

A

Smallest units of matter. Hydrogen atoms are the smallest atoms.

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7
Q

How many electrons can each shell hold?

A

First shell: 2
Second shell: 8
Third shell: 18

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8
Q

How do you determine the atomic number of an element?

A

By the amount of protons in its nucleus.

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9
Q

How do you determine the mass number of an atom?

A

It’s the sun of protons and neutrons.

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10
Q

Isotopes

A

Have a different number of neutrons than protons.

For example. In a sample of oxygen. Some atoms have 9 or 10 neutrons- but ALL HAVE 8 electrons and protons. The mass number determines the name of the isotope. For example (oxygen) O16 O17 O18

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11
Q

Ion

A

Is an atom that has a positive or negative charge because it has an uneven number of protons and electrons.

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12
Q

Molecule

A

When two or more atoms share electron(s). A molecule may include two atoms of the same kind. For example oxygen O2

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13
Q

Compound

A

Is a substance that contains atoms of two or more different elements. Most of the atoms in the body are joined into compounds.

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14
Q

Free radical

A

Is an atom or group of atoms with an unpaired electrons in the outer most shell. Example is superoxide which is the addition of an electron to an oxygen molecule.

Having an unpaired electron makes a free radical unstable, highly reactive, and destructive to nearby molecules.

Free radicals become stable by giving up their extra electron or pairing with an electron from another molecule, making them able to break apart important body molecules.

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15
Q

Octet rule

A

One atom is more likely to interact with another atom if it leaves both atoms with eight valence electrons.

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16
Q

Where are ionic bonds mostly found in the body?

A

Teeth and bones. Where they give great strength.

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17
Q

Electrolyte

A

An ionic compound that breaks apart into positive and negative ions in a solution.

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18
Q

Ions

A

Have a charge associated with them. For example if written as H+ (it’s because it donated its electron and gave up negativity)

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19
Q

Electonegativity

A

The power to attract electrons to itself (atom)

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20
Q

Polar covalent bond

A

Sharing of electrons between two atoms is unequal. The nucleus of one atom attracts the shared electrons more strongly than the other.

The molecule will have have a partial negative charge closer to the atom that attracts electrons more strongly (gaining negativity)

21
Q

Cohesion

A

The tendency of like particles to stay together.

22
Q

Energy

A

Capacity to do work

23
Q

Potential energy

A

Energy stores by matter due to its position

24
Q

Kinetic energy

A

The energy associated with matter in motion

For example the energy stored in water behind a dam, or stored in a person prepared to jump is potential energy. When the damn opens, or the person jumps potential energy is converted to kinetic energy.

25
Q

Chemical energy

A

Is a form of potential energy that is stored in the bonds of of compounds and molecules.

26
Q

Law of conservation of energy

A

Energy can not be created or destroyed, it may be converted from one form to another.

Generally releases heat.

For example energy from food can be converted to walking or talking.

27
Q

Exergonic energy

A

Releases more energy than absorbs

I’m general usually occur as nutrients. Such as glucose. If a molecule of glucose is completely broken down. It can be used to make 32 ATP.

28
Q

Endergonic reactions

A

Absorb for energy than they release.

29
Q

Activation energy

A

Collision energy needed to break the chemical bonds of reactants. Needed to start a reaction.

Temperature and concentration are factors.

The more particles of matter present in a confined space, the greater chance they will collide.
As temperature rises, particles move about more rapidly. The higher the temp. The more forcefully particles will collide=greater chance of reaction.

30
Q

Catalysts

A

Speed chemical reactions by lowering the amount of activation energy needed. Most important catalysts are enzymes.

Just lowers amount of energy needed to start the reaction.

31
Q

Anabolism

A

Building
Synthesis reaction
Enderogenic (absorb more than they release)

32
Q

Catabolism

A

Decomposition reactions
Exerogrnic (release energy)

33
Q

Oxidation-Reduction reactions

A

Essential to life, break down food molecules.

Oxidation refers to loss of electrons.

Reduction refers to the gain of electrons.

34
Q

Inorganic compounds

A

Lack carbon
Structurally simple
Molecules only have a few atoms
Cannot be used by cells to carry out complicated biological functions.

Water and many salts.

Ionic or covalent bonds

Inorganic compounds that contain carbon are: CO2, HCO-3, H2CO3

35
Q

Organic compounds

A

Always contain carbon
Usually contain hydrogen
Always have covalent bonds
Most are large molecules made up of long carbon atom chains.

36
Q

Solvent

A

Solution that Dissolves another substance called a solute.

Your sweat (solvent) and small amounts of salts (solute)

37
Q

Hydrophilic

A

Water loving
Solutes that are charged or contain polar covalent bonds are hydrophilic. Which means these solutes dissolve easily in water.

38
Q

Hydrophobic

A

Molecules with Non polar covalent bonds
Water fearing

39
Q

Water

A

Most important and abundant inorganic compound in all living systems.
-Universal solvent
-Serves as a medium for most chemical reactions
-Hydrolysis : helps break down molecules by adding water.
-Water can absorb or release a large amount of heat
-important component of mucus and other lubricating fluids.

40
Q

Mixture

A

Combination of elements or compounds that are physically blended together. But not bound by chemical bonds. For example air

41
Q

Colloid

A

Differs from a solution largely because the size of particles.
Colloids particles are large enough to scatter light. Usually appear translucent, or opaque.

42
Q

Solution

A

Once mixed together solutes in a solution remain evenly dispersed.
Because the particles are very small. The solution looks transparent.

43
Q

Suspensions

A

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

Blood is an example.

Colloids and solutions don’t settle.

44
Q

Mole

A

A unit of measurement that is equal to the sum of atomic mass(es) for a given element or compound.

45
Q

Acid

A

Is a substance that dissociates into one or more hydrogen ions, and one or more anions.

Because H+ is a single proton with one positive charge (gave away negativity) … An acid is a proton donor.

46
Q

Base

A

Removes H+ from solutions. And is therefore a proton acceptor.

Dissociate into one or more hydroxide (OH-) ions.

47
Q

Acid Base balance

A

Intracellular and extracellular fluids must contain almost balanced quantities of acids and bases. The more hydrogen ions in a solution the more acidic. The more hydroxide ions the more basic.

Ph is used to measure acidity.
A pH of 6 denotes 10 times more H+ than a pH of 7. A pH of 7 (such as water) is neutral

A pH below 7 =acidic
A pH above 7 =basic

48
Q

Buffer system

A

Functions to convert strong acids or bases into weak acids or bases.

Strong acids and bases ionize easily and can disrupt pH quickly and drastically. Where as weaker acids and bases can not.

49
Q

Carbonic acid-bicarbonate buffer system

A

Carbonic acid (H2CO3) can act as a weak acid, and bicarbonate (HCO3-) can act as a weak base. So this buffer system can compensate for either an excess or shortage of H+.

In example : for excess H+

H+ + HCO3- ->. H2CO3

If there is a shortage of H+ carbonic acid can function as a weak acid and provide hydrogen ions.

H2CO3 -> H+ + HCO3-

Bio 235 (2 decks)

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