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BIO 137 EXAM 1 CH 1, 2, 3 > CHAPTER 2 > Flashcards

CHAPTER 2 Flashcards

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Biology 101 flashcards
1
Q

Matter

A

anything that occupies space and has mass

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2
Q

Mass

A

the amount of matter in an object; remains constant

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3
Q

States of Matter

A

1) solid 2) liquid 3) gas

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4
Q

Solid

A

definite volume and shape

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5
Q

Liquid

A

definite volume, flexible/changing shape

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6
Q

Gas

A

no definite volume or shape

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7
Q

Energy

A

the capacity to do work or put matter into motion

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8
Q

States of Energy

A

1) Kinetic 2) Potential

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9
Q

Kinetic Energy

A

energy in action/motion

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10
Q

Potential Energy

A

capable of work, but currently inactive; stored energy; energy of position

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11
Q

Forms of Energy

A

1) chemical 2) electrical 3) mechanical 4) Radiant or Electromagnetic radiation

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12
Q

Chemical Energy

A

energy stored IN BONDS of chemical substances

ex: ATP most useful form of chemical energy in living systems

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13
Q

Electrical Energy

A

energy that results form movement or charged particles

ex: ions moving across cell membranes

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14
Q

Mechanical Energy

A

energy directly involved in moving matter

ex: legs pedaling a bike

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15
Q

Radiant Energy

A

or Electromagnetic Radiation.
Energy that travels in waves

ex: x rays, visible light, infrared, radio and ultraviolet waves

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16
Q

Can Energy be created or destroyed?

A

no, it can be converted from one form to another. conversion is inefficient and lose some energy in the form of heat.

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17
Q

Elements

A

composed of atoms and has its own unique physical and chemical properties

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18
Q

Physical Properties

A

observable with the senses and measurement

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19
Q

Chemical Properties

A

how atoms interact with other atoms

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20
Q

What are the major elements of the human body?

A

Oxygen- 65%
Carbon- 18.5%
Hydrogen- 9.5%
Nitrogen- 3.2%

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21
Q

Major elements make up what percent of body weight?

A

96%

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22
Q

Why are trace elements important?

A

essential parts of enzymes or are required to activate enzymes

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23
Q

What is the structure of an Atom?

A

it is composed of subatomic particles that differ in mass, charge and location in the atom

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24
Q

What is the mass, charge and location of a Proton?

A

1 amu, positive charge, and located in the atomic nucleus

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25
Q

what is the mass, charge and location of a Neutron?

A

1 amu, no charge, and located in the atomic nucleus

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26
Q

what is the mass, charge and location of an Electron?

A

0 amu, negative charge, and it orbits the nucleus

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27
Q

which subatomic particles account for 99.9% of an atoms mass?

A

the protons and neutrons. aka the nucleus

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28
Q

which subatomic particals determine the chemical behavior of an atom?

A

the electrons

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29
Q

Why are atoms electrically neutral?

A

there are always equal numbers of protons and electrons

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30
Q

What is the atomic NUMBER and where is it written?

A

the number of protons in the nucleus.

written as the left sub-script

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31
Q

What is the atomic MASS and where is it written?

A

the sum of protons and neutrons in the nucleus

written as the left post-script

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32
Q

Isotopes

A

elements that have the same number of protons and electrons but differ in neutrons

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33
Q

Radioisotopes

A

isotopes of atoms that decay spontaneously into more stable forms (radioactivity). can transform elements into different ones

34
Q

Molecule

A

particle composed of 2 or more atoms joined together by chemical bonds; atoms can either be the same or different

35
Q

What is the difference between molecules of an element and molecules of a compound?

A

molecules of an element are atoms of the SAME element joined.

molecules of a compound are composed of 2 or more DIFFERENT atoms that are chemically bonded.

36
Q

Mixture

A

substance composed of 2 or more components that are physically intermixed; include solutions, colloids and suspensions.

37
Q

Solvent

A

Substance present in the greatest amount that dissolves other substances i.e. water

38
Q

Solute

A

substance that is dissolved in a solvent, creating a solution

39
Q

Homogeneous Mixture

A

identical composition though out

ex: salt water

40
Q

Heterogeneous Mixture

A

composition is dissimilar in different areas of the mixture. samples vary in composition

ex: fruit salad jello

41
Q

What are the different types of mixtures?

A

1) solution 2) Colloids/Emulsions

3) Suspensions

42
Q

What are key characteristics of SOLUTION mixtures?

A 
homogeneous
can be gas, liquid or solid
small particle sizes
solvent: water
Usually transparent

ex: ocean (salt) water, air (H20)

43
Q

What are the key characteristics of COLLOID mixtures?

A 
also called EMULSIONS
heterogenous
exhibit sol-gel transformation
medium size particles that do not settle out over time
appear milky, almost translucent

ex: butter

44
Q

What are the key characteristics of SUSPENSION mixtures?

A

heterogeneous mixture
large particles that settle out over time

ex: sandy water

45
Q

Mixtures vs. Compounds

A

compounds: chemical bonding, can be hetero- or homogeneous
mixtures: separation by physical means, can be hetero- or homogeneous

46
Q

Chemical Bond

A

energy relationships between the electrons of reacting atoms

47
Q

Shell

A

orbits for electrons

48
Q

Valence Shell

A

atoms outermost energy level; chemically reactive

49
Q

Valence Electrons

A

electrons in the outermost energy level (valence shell); chemically reactive

50
Q

Which shell has the highest energy level and why?

A

the outer (valence) shell, becuase it is not as strongly bound to the nucleus, due to the distance

51
Q

Octet Rule/Rule of Eights

A

the tendency of atoms to interact in such a way that they have 8 electron in their valence shell.

52
Q

Chemically Inert Elements

A

atoms are filled to capacity (contains 8 electrons) therefore they are stable and unreactive

53
Q

Chemically Reactive Elements

A

the innermost energy level is not full; tend to gain, lose, or share electrons

54
Q

What are the different types of chemical bonds

A

1) ionic
2) covalent: polar and non-polar
3) hydrogen

55
Q

Ionice Bond

A

one atom donates one or more valence electrons and another atom picks up/adds one or more valence electrons, resulting in the formation of ions (hence IONIC bond)

56
Q

Ion

A

atoms/molecules with a positive or negative charge

57
Q

Anion

A

accepts/gains electrons and forms a net NEGATIVE charge

58
Q

Cations (ca+ions)

A

give up/lose electrons and form a net POSITIVE charge

59
Q

How to Ionic bonds form?

A

the net positive charge on on ion is attracted to the net negative charge on another ion., like magnets.

60
Q

How do Covalent bonds form?

A

when certain atoms interact and they share one or more valence electrons to fill their valence shells.

61
Q

How many electrons do single, double and triple covalent bonds share

A

1, 2 and 3 electrons

62
Q

What is the different between POLAR and NON-POLAR covalent bonds?

A

non-polar are balanced, polar have unequal electron pairing

63
Q

Polar Covalent Bonds

A

2 or more poles of charge
one atom is an electron “hog”
the two ends or poles of the molecule differ

Electronegative- attract electons
Electropositive- low electron attracting ability, usually lose electrons

64
Q

What is an example of a non-polar covalent bond?

A

CO2: O=C=O ( = meaning covalent bond)

65
Q

What are the characteristics of a Hydrogen Bond?

A

too weak to bind atoms
bonds form, break, and re-form
responsible for high surface tension of water

66
Q

Surface Tension

A

measurement of how difficult it is to stretch or break the surface of a liquid

67
Q

Cohesion

A

intermolecular attraction of like molecules to one another

68
Q

Adhesion

A

attraction between dissimilar molecules of surfaces

69
Q

Chemical Reactions

A

involve the formation and breaking of bonds between atoms.

involves the rearrangement of atoms to form different molecules

70
Q

How do reactants and products relate?

A

Reactants interact to yield the products

71
Q

What are the types of chemical reactions

A

1) Synthesis Reaction
2) Decomposition or Degradation Reaction
3) Exchange or Displacement Reaction
4) Oxidation Reduction Reaction

72
Q

Synthesis Reaction

A

to make or build something bigger

ex: AB+C+DEF= ABCDEF

73
Q

Decomposition Reaction

A

Degradation
break larger things down into smaller things

ex: ABCDEF -> ABC D EF

74
Q

Exchange Reaction

A

Displacement
combination of decomposition and synthesis

ex: ABC+DE -decomposition->A+B+C+D+E -synthesis-> ABDE+C

75
Q

Oxidation Reduction Reaction

A

one reactant loses electrons (oxidation) and the other reactant gains (reduction) the electrons.

76
Q

What are some examples of Oxidation-Reduction Reactions

A

Photosynthesis H2O+CO2–> C6H12O6+O2

Cellular Respiration C6H12O6+6O2 –>6CO2+6H2O+ATP

77
Q

Denaturation

A

when temperatures get so high it causes a change in the chemical structure of a substance

78
Q

Biochemistry

A

chemistry of living matter; organism possess inorganic and organic components

79
Q

Inorganic substances vs. organic substances

A

inorganic- water, salts, acids, bases and electrolytes

organic molecules- proteins, carbs, lipid, nucleic acids

80
Q

Acids

A 
proton donors (H+) 
release hydrogen and anions of the same type when dissolved in water
high [H+]  and low pH
81
Q

Bases

A

proton acceptors
release a cation and hydroxide ion when dissolved in water
slippery to the touch

82
Q

Electrolytes

A

minerals in your blod and other fluids that carry and electric charge

BIO 137 EXAM 1 CH 1, 2, 3 (6 decks)

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