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Anatomy and Physiology > Chapter 2- Chemical Basis Of Life > Flashcards

Chapter 2- Chemical Basis Of Life Flashcards

(104 cards)

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0
Q

Matter

A

Anything that takes up space and has mass

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1
Q

Electricity

A

The flow of electrons (energy)

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2
Q

Mass

A

A measure of the amount of matter an object contains

Stays the same regardless if changes in the objects position

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3
Q

Weight

A

The measure of how strongly an object is pulled by earths gravity and it varies with distance from earths center

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4
Q

Trace elements

A

Elements required by life in very minute quantities

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5
Q

Ultratrace elements

A

Element required by organisms in extremely minute quantities but are TOXIC at high levels (arsenic- Ar)

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6
Q

Compound

A

A pure substance composed of 2+ different elements combined in a fixed ratio (✔️molecule)

Ex: NaCl (sodium chloride)

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7
Q

Molecule

A

2+ atoms

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8
Q

Atom

A

Smallest possible unit of matter that retains chemical/physical properties of its element

Atoms of the same element share similar chemical properties

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9
Q

Subatomic particles

A

Neutrons, Protons, electrons

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10
Q

Electrostatic charge

A

✔️Two opposites attract each other

✔️Positive attracts negative

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11
Q

What is unique about hydrogen

A

It has only one electron and one proton, NO neutrons

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12
Q

Atomic nucleus

A

Where protons and neutrons are found; where mass of entire atoms is measured

Mass of 1 proton, one neutron= 1 Dalton

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13
Q

Where are electrons located

A

Orbit around the nucleus; held together by electrostatic attraction to positively charged nucleus

Mass so small, it’s not used to calculate atomic mass

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14
Q

Atomic number

A

DETERMINES the atom (unique to each)

Number of protons in an atom

All atoms of an element have the same atomic number (subscripts to the of the elements written symbol)

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15
Q

Mass number

A

Number of protons and neutrons in an atom (one of each has mass of approx 1 dalton)

Superscript to left or an elements symbol

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16
Q

Octet rule

A

1st shell- max 2 electrons
2nd shell- max 8 electrons
3rd shell- max 8 electrons

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17
Q

In what shell do electrons have most energy

A

The further out the shell, the more energy the electrons have because they aren’t being pulled into positively charged nucleus as strongly

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18
Q

Chemical reactions always go to the _________________? energy state

A

Chemical reactions always go to the LOWEST energy state

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19
Q

Inert

A

NOT reactive

Outermost shell is naturally full; ALL gasses (noble gasses)

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20
Q

Isotopes

A

Atoms of an element that have the same atomic number but different mass number

Different number of NEUTRONS

Under natural conditions, elements occur as mixtures of isotopes

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21
Q

Different isotopes of the same element react chemically in the ____________ way.

A

Different isotopes of the same element react chemically in the SAME way.

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22
Q

Radioactive isotope

A

Unstable isotope in which the nucleus spontaneously decays emitting subatomic particles and/or energy as radioactivity

Fixed half-life

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23
Q

What are two biological applications of radioactive isotopes

A
  1. Dating geological strata (layers) and fossils

2. Radioactive tracers

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24
Radioactive tracers
Trace steps of biochemical reaction or to determine the location of a particular substance within organism Useful bc they chemically react like the stable isotopes and are easily detected at low concentrations Diagnose disease Cause or cure cancer
25
Octet rule
Rule that valence shell is complete when it contains 8 electrons
26
Chemical bond
Attractions that hold molecules together
27
Covalent bond
✔️Strongest bond | ✔️Chemical bonds formed by sharing s pair of valence electrons
28
Carbon and silicon have 4 valence electrons, what is this called?
Tetravalent
29
Valence
Bonding capacity of an atom which is the number of covalent bonds that must be formed to complete the outer shell
30
Electronegative atom
The personality of some atoms to be attracted to electrons and pull them close to them!! EX: N2 and O2 !!!!!!
31
Dipole
Uneven distribution of the charge in a molecule
32
Hydrogen bond
✔️Weak bond ✔️form between molecules or diff parts of a large molecule ✔️Bond formed by the charge attraction when HYDROGEN is COVALENTLY bonded to an ELECTRONEGATIVE atom and is attracted to another electronegative atom ✔️indicated by dotted line in structural formula
33
Why is DNA hard to unravel?
Bc it has ALOT of weak hydrogen bonds which are strong when together bc there are so many
34
How many hydrogen bonds can a water molecule form with neighboring water molecules?
4
35
What holds DNA together?
Weak hydrogen bonds adenine----> thymine cytosine---> guanine
36
Ion
A charged atom or molecule
37
Ionic bond
✔️Formed by the electrostatic attraction (positive--->neg.) after the complete transfer of an electron from a donor atom to an acceptor. (Acceptors attract electrons bc electronegative) ✔️strong bonds in crystals not in water (salt dissolves in water bc ionic bonds dissociate into ions
38
Chemical reactions
Making and breaking chemical bonds leading to changes in composition of matter; reactants---> products Matter cannot be created nor destroyed
39
The relative concentration of reactants and products affects the reaction rate. The higher the concentration the ____________
....greater probability of a reaction
40
Completion in chemical reaction
All reactants are converted to products. (Majority are reversible)
41
Chemical equilibrium
The RATE of the forward reaction (speed/time) equals the RATE (speed/time) of the reverse reaction Dynamic- reactions continuing in both directions. Relative concentrations of reactants/products stay the same
42
Homogenous
Particles in a mixture are all spread out throughout; mixed together
43
Dissociation of water molecules
Occasionally, the hydrogen atom that is shared in a hydrogen bond between two water molecules, shifts from the oxygen atom to which its covalently bonded to the unshared orbitals of the oxygen atom to which its hydrogen bonded H2O-----> OH+H
44
What would happen if you took protein (slightly negative charge) and dumped it in acid?
The H+ ions (protons) will all pull the electrons toward them changing the shape of protein thus affecting its function DENATURED ENZYME
45
When does the #H+ = #OH-?
At equilibrium (pure water)
46
Brackets indicate
Molar concentration
47
[H+] + [OH-] = ? M?
1/10,000,000 M= 10-7 M
48
Acid
Substances that increase the [H+] of a solution; also removed [OH-] bc it combines with H+ to form H2O
49
Caustic
Either extremely acidic or extremely alkaline; will burn you
50
Base
Substances that reduce the relative H+ of a solution; may alternately increase OH-
51
LEO the lion says GER stands for ?
Lose electrons= oxidation Gain electrons= reduction Anything that breaks down into a positive and a negative
52
Salt
Substance formed by the reaction between an acid and a base
53
[H+][OH-]= ?
1.0 * 10-14
54
In what pH range are most biological fluids?
6 to 8
55
Each pH unit represents a ________ difference (logarithmic scale)
Tenfold Slight change in pH= large change in actual [H+]
56
Buffers
Minimizing wide fluctuations in pH to help organisms maintain the Psh of body fluids within the narrow range necessary for life Prevents sudden changes in pH Ex: Bicarbonate (buffer in blood)
57
How do buffers work?
They either donate H+ to the solution when they have been depleted or accept H+ from the solution when they are i know excess
58
Polymer
Large molecule consisting of many identical or similar subunits connected together Ex: protein consists of many amino acids
59
Monomer
Subunit or building block molecule of a polymer Ex: amino acids are the monomers of the polymer protein
60
Macromolecule
Large organic (carbon-containing) polymer
61
What are the four classes of macromolecules in living organisms
Carbohydrates Lipids Proteins Nucleic acid (DNA,RNA, and ATP)
62
Polymerization reactions
Chemical reactions that link 2+ small molecules to form molecules with repeating structural units (making a polymer)
63
Condensation reactions
Mose polymerization reactions in living things !!!! (Anabolism) Monomers are covalently linked, producing net removal of a water molecule for each covalent linkage One monomer loses OH and another loses H Requires energy
64
Hydrolysis
(Catabolism) A reactions process that breaks (splits) covalent bonds between monomers by the addition of water molecules Hydrogen fro water bonds with one monomer and remaining OH from water bonds with adjacent monomer Ex: digestive enzymes catalyze hydrolysis reactions which BREAK APART large food molecules into monomers that can be absorbed into the bloodstream
65
Carbohydrates
Organic (must have carbons and hydrogen to be organic) molecules made of sugars and their polymers
66
Monosaccharides
Simple sugars that are monomers or building block molecules in CARBOHYDRATES CH2O Major nutrients for cells ; glucose is most common
67
Where do carbs store energy
In their chemical bonds and it is harvested by cellular respiration
68
How do we get energy out of glucose?
Cellular respiration
69
Glycosidic linkage
Covalent bond formed by a condensation reaction between two sugar monomers
70
Preferential order of utilization
Body's favorite order of what macros to use first for energy Carbs --> protein --> fat
71
Polysaccharides
Macromolecules that are polymers of a few hundred or thousand monosaccharides Formed by linking monomers in enzyme-mediated condensation (joining by removing water) reactions
72
What's the most common storage polysaccharide in animals?
Glycogen Glucose polymer in animals stored in muscle and liver
73
Where is glycogen stored in humans?
The liver and muscles
74
Lipids
Diverse group of organic compounds that are insoluble in water (hydrophobic) but will dissolve in non polar (like dissolves like) solvents
75
What are the 3 important groups of lipids
Fats Phospholipids Steroids
76
What are fats composed of?
``` Glycerol- a three-carbon alcohol Fatty acid (carboxyl acid)- composer of a carboxyl group (COOH) head at one end and an attached hydrocarbon chain (tail) ```
77
Affinity
Attraction towards
78
Fats
(Tail) ``` Hydrocarbon chain (C-H) Hydrophobic and not water soluble ```
79
ester linkage
Bond formed between a hydroxyl group and a carboxyl group
80
Characteristics of fat:
✔️Insoluble to water ✔️variation among fat molecules is the fatty acid composition ✔️fatty acids in a fat may all be the same or some (all) may differ ✔️ vary in length ✔️ vary in number and location of carbon to carbon double bonds
81
Saturated fat
✔️No double bonds between carbons and fatty acid tail ✔️bonded to MAX number of hydrogens ✔️ solid at room temp ✔️most animal fats
82
Unsaturated fat
✔️one+ double bonds between carbons in fatty acid tail ✔️liquid at room temp ✔️plant fats
83
What are 4 useful functions of fats?
✔️energy storage (one gram stores twice as much energy as a gram of polysaccharide ✔️more compact fuel reservoir (store more energy for less weight than in plants) ✔️cushions vital organs (kidney) ✔️insulated against heat loss
84
Phospholipids
Compounds with molecular building blocks of glycerol, 2 fatty acids, one phosphate group, usually an additional small chemical group attached to the phosphate
85
How do phospholipids differ from fat?
The third carbon of glycerol is joined to a negatively charged phosphate group instead of another fatty acid
86
How is a cell membrane's phospholipid bilayer set up?
Has two layers of phospholipids. Each have a hydrophilic head polar head and two hydrophobic fatty acid nonpolar tails. The heads are facing outward toward extra|intra cellular areas and tails are facing inward
87
Steroids
Lipids which have 4 fused carbon rings with various functional groups attached Ex: cholesterol is important steroid
88
Cholesterol
Very important steroid ✔️adds stability to cell membrane (adds viscosity (thickness) to membrane) ✔️precursor to many other steroids (sex hormones etc)
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Fluid- mosaic
Characteristic of cell membrane to move Fluid- move all around Mosaic- all different components
90
Protein
Polymer of amino acids
91
Structure of amino acids
Carboxyl end (COOH) and an amino acid end (NH2) as well as a variable R group
92
Peptide
2+ amino acids
93
Peptide bond
Formed between the amino group (NH2) of one amino acid to the carboxyl group (COOH) of the next
94
How many kinds of amino acids are use in protein structure?
20
95
What are the four levels of protein structure?
Primary structure Secondary structure Tertiary structure Quaternary structure
96
Primary structure
The order of the amino acids in a peptide
97
Secondary structure
Coiled or FOLDED shape held together by hydrogen bonds
98
Tertiary structure
Further bending and folding
99
Quaternary structure
Between 2+ peptide chains
100
Will protein dissolve in water? Why/why not?
Yes bc proteins is polar and water is polar. Like dissolves like. The protein will bend on itself until is bonds with hydrogen in H2O
101
Protein conformation
✔️Overall protein shape | ✔️Cannot function properly if shape is altered
102
Denatured protein
An unraveled or destroyed protein Occurs when heat or changes in pH change protein shape
103
What are 6 functions of protein?
``` ✔️structural components ✔️enzymes for catalysis ✔️communication ✔️membrane transport ✔️cell recognition/protection ✔️movement ```

Anatomy and Physiology (16 decks)

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