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human A&P 1 > Ch 2 > Flashcards

Ch 2 Flashcards

(103 cards)

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1
Q

Describe the 3 states of matter

A
  • solid: a definite shape and volume
  • liquid: a changeable shape but definite volume
  • gas: changeable shape and volume
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2
Q

Compare Kinetic and Potential energy and identify examples of each

A
  • kinetic: energy in action (a ball rolling)

- potential: stored energy (a ball at rest)

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3
Q

Know the 4 forms of energy used by humans and give examples

A
  • Chemical energy: adenosine triphosphate or ATP(energy in chemicals)
  • electrical energy: nerve impulses
  • mechanical energy: sound waves
  • radiant or electromagnetic energy: light rays
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4
Q

What are the major consequences of energy conversions?

A

you will always lose some energy that will create heat during the conversion

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5
Q

List the 4 major elements of the body and their symbols and state their common function

A
  • Carbon C: a component of all organic molecules, which include carbohydrate, lipids, proteins, and nucleic acids
  • Hydrogen H: a component of all organic molecules, as an ion, it influence the pH of body fluids
  • Oxygen O: a component of both inorganic and organic molecules. as a gas, it is needed for the production of cellular energy
  • Nitrogen N: a component of proteins and nucleic acids
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6
Q

Identify the remaining 9 minor elements by symbol and know their significance to the body

A
  • Calcium Ca: found as a salt in bones and teeth. its ionic form is required for muscle contraction, conduction of nerve impulses, and blood clotting
  • Phosphorus P: part of calcium phosphate salts in bones and teeth. also present in nucleic acids, and as part of ATP and phospholipids
  • Potassium K: its ion is the major positive ion in cells. necessary for conduction of nerve impulses and muscle contraction
  • Sulfur S: component of proteins, particularly muscle proteins
  • Sodium NA: as an ion, sodium is the major positive ion found in extracellular fluids. important for water balance, conduction of nerve impulses, and muscle contraction
  • Chlorine CL: its ion is the most abundant negative ion in extracellular fluids
  • Magnesium MG: present in bone. also an important cofactor in a number of metabolic reactions
  • Iodine: needed to make functional thyroid hormones
  • Iron Fe: component of hemoglobin and some enzymes
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7
Q

Describe the structural components of an atom. What makes it stable?

A

Neutrons, protons, and electrons

equal number of protons and electrons

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8
Q

Identify the characteristics of a suspension and be able to recognize examples.

A

Solute particles are very large, settle out, and may scatter light
ex: blood settles into plasma and red blood cells

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9
Q

Identify the characteristics of a colloid and be able to recognize examples

A

solute particles are larger than in a solution and scatter light; they do not settle out
ex: jello, milk, or paint

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10
Q

Identify the characteristics of a solution and be able to recognize examples

A

solute particles are very tiny, do not settle out or scatter light
ex: water

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11
Q

Be able to calculate molar concentrations of solutions

A

To find the molar concentration of a solution, simply divide the total moles of solute(its atomic weight in grams) by the total volume of the solution in liters

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12
Q

What is the chief difference between mixtures and compounds?

A
  • Mixtures do NOT allow chemical bonding between components

- Compounds do allow chemical bonding between components

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13
Q

What is the Octet Rule? How is it used to determine the type of chemical bond any element will form?

A

except for the first shell of electrons, atoms will interact to have 8 electrons in their valence shell

the atom will always try to stabilize the outer shell: A 4 will seek a 4, a 7 will seek a 1, and an 8 will try to stay separate

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14
Q

How does the Octet Rule apply to an element with 1 or 2 valence electrons?

A

the atom will give up their electron to another atom that wants it fill out it’s valence shell. this will give the atom a positive charge or a Cation

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15
Q

How does the Octet Rule apply to an element with 6 or 7 valence electrons?

A

the atom will take some electrons from another atom that wants to give them up. this will give the atom a negative charge or a Anion

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16
Q

Use the Periodic Table of Elements to predict if an element will gain or lose electrons and what type of chemical bond will be formed. (create examples)

A
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17
Q

Describe how an ionic bond is formed

A

An ionic bond can be formed after two or more atoms permanently lose or gain electrons to form an ion.

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18
Q

describe how a covalent bond is formed

A

formed by sharing of two or more valence shell electrons. allows each atom to fill its valence shell at least part of the time

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19
Q 
Know the difference between the following types of covalent bonds and recognize examples.
single -
double -
triple -
Nonpolar Covalent -
Polar covalent -
A
  • single: when a covalent bond forms to share 1 electron
  • double: when a covalent bond forms to share 2 electrons
  • triple: when a covalent bond forms to share 3 electrons
  • nonpolar covalent: electrons are shared equally. produces electrically balance (such as CO2)
  • polar covalent: unequal sharing of electrons produces polar molecules (such as H20)
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20
Q

Describe how a hydrogen bond is formed

A

attractive force between electropositive hydrogen of one molecule and an electronegative atom of another molecule.

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21
Q 
Describe the following types of chemical reactions and be able to give examples of each: Synthesis (combination) -Anabolism -
Decomposition -
Catabolism -
Exchange (displacement) -
Oxidation-reduction (redox) -
Reversible -
A

Synthesis (combination): smaller particles are bonded together to form larger, more complex molecules(amino acids bonding to form protein)
Anabolism: synthesis of larger molecules
Decomposition: bonds are broken in larger molecules, resulting in smaller less complex molecules(glycogen breaks down to glucose molecules)
Catabolism: breakdown of larger molecules
Exchange (displacement): bonds are both broken and made (a molecule from a major bond breaks off and joins a new molecule in bond)
Oxidation-reduction (redox): a reaction in which food fuels are broken down for energy
Reversible: all chemical reactions are theoretically reversible. chemical equilibrium occurs if neither a forward or revers reaction is dominant

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22
Q

Understand the importance of chemical equilibrium to metabolism.

A

it allows for a constant state of energy flow

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23
Q

Know the 4 factors that influence the rate of chemical reactions. Determine the impact when a factor is changed.

A
  • temperature(get from book) up: rate up
  • concentration of reactant up: rate up
  • particle size down: rate up
  • catalysts: rate up without chemically changed or part of product(ex. enzymes)
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24
Q

Know the differences between organic and inorganic compounds. Identify examples of each.

A
  • inorganic- does not contain both hydrogen and carbon at the same time(ex. water or salt)
  • organic compounds- always contain carbon and can also have hydrogen at the same time
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25
Know the 5 unique properties of water and the implications for the human body.
- High heat capacity: absorbs and releases heat with little temperature change - High heat of vaporization: evaporation requires large amounts of heat - Polar solvent properties: dissolves and dissociates iconic substances - Reactivity: critical part of hydrolysis and dehydration synthesis reactions - Cushioning: protects certain organs from physical trauma
26
Know the concept of the pH scale & identify if a solution is acidic, basic, or neutral
0-14 0-6 are acids 7 neutral compound 8-14 are bases
27
Know why a weak acid is a buffer
because it allows for a quick and easy neutralization of a base
28
Know why a weak base is a buffer
because it allows for a quick and easy neutralization of an acid
29
Understand how the carbonic acid-bicarbonate system maintains blood pH.
H2CO3 = HCO3- + H+ | this equation is the back and forth of blood pH
30
Know the bonding properties of carbon in organic compounds
- is electroneutral, share electrons; never gains or loses them - forms four covalent bonds with other elements
31
Name the 4 major organic molecules that are unique to living systems. Know their monomers.
- carbohydrates: carbon, hydrogen, and oxygen - lipids: carbon, hydrogen, and a little oxygen - proteins: - nucleic acids:
32
Identify the 6 most common functional groups inorganic compounds and state their significance
-Carbonyl: makes ketones and aldehydes -Hydroxyl: makes alchols -Sulfhydryl -Amino -Carboxyl: make organic acids(latic and acetic) -Phosphate (find other acids significance)
33
Identify the chemical reaction used to build polymers.
Dehydration synthesis
34
Identify the chemical reaction used to break down polymers.
Polymers are broken down into monomers via hydrolysis reactions, in which a bond is broken, or lysed, by addition of a water molecule
35
Name the 3 classes of carbohydrates.
- Monosaccharides - Disaccharides - Polysaccharides
36
Know the general functions of carbohydrates.
major source of fuel and is a structural molecule
37
``` State the importance of the following carbohydrates to cellular metabolism. Recognize examples. Monosaccharide – Isomer – Disaccharide – Polysaccharide – ```
- single chain structures, the building block, monomers, of the other carbohydrates. ex. Glucose and deoxyribose - have the same molecular formula, but their atoms are arranged differently, giving them different chemicals properties. ex. galactose and fructose - formed when 2 monosaccharides are joined by dehydration synthesis, a water molecule will be lost in the making. ex. sucrose, lactose, and maltose - are polymers of simple sugars linked together by dehydration synthesis. ex. starch and glycogen
38
Describe the general chemical structure of lipids. Name the 4 main types.
``` contains carbon, hydrogen, oxygen and sometimes phosphorus Triglycerides or neutral fats– Phospholipids– Steroids– Eicosanoids - ```
39
Know the chemical properties of the following lipids and how they are important to cells and tissues. Recognize examples: Triglycerides including saturated, monounsaturated and polyunsaturated fats - Phospholipids - Steroids - Eicosanoids -
- major form of stored energy in the body / fat deposits protect and insulate organs / has 3 fatty acid chains / fatty acids and glycerol / ex. fats - chief component of cell membranes / help transport lipids in blood / ha 2 fatty acid chains and 1 phosphate group with an attached nitrogen containing group - flat molecules made of 4 interlocking hydrocarbon rings / fat soluble and contain little oxygen / ex. cholesterol - derived from a 20-carbon fatty acids found in cell membranes / ex. prostaglandins
40
``` Describe the monomers of proteins. Include the following: Peptide bond – Amine group – Carboxyl group – Central carbon – R-group - ```
Carbon, oxygen, hydrogen, and nitrogen(2 also contain sulfur) - when the acid end of one amino acid links to the amine end of the next amino acid - NH2 - COOH - the carbon atom that is always in the middle of an amino acid - the molecules in the middle of an amino acid that connect the amine and acid groups together.
41
Know how each amino acid contributes to the physical and chemical properties of the protein.
a single change in the amino acid ladder can change the entire use of the protein strand.
42
Know the terms that describe the size of amino acid based molecules. Dipeptide – Tripeptide – Polypeptide –
- two united amino acids - three united amino acids - ten or more united amino acids
43
``` Know the four levels of protein structure and the functions gained at each level Primary – Secondary – a-helix b-pleated sheet Tertiary – Quaternary – ```
- the sequence of amino acids forms the polypeptide chain - the primary chain forms both spirals(A-helix) and sheets (B-pleated sheet). both are held together by hydrogen bonds - superimposed on secondary structure, both A and B are folded together in a compact globular molecule held together by intramolecular bonds. - two or more polypeptide chain, each with its own tertiary structure, combine to from a functional protein
44
Explain the differences between fibrous proteins and globular proteins. Know examples
Fibrous: structural proteins, form long strands, insoluble in water / ex, collagen Globular: functional proteins, form spherical proteins, are water soluble / ex. antibodies, regulate growth
45
Know how complementarity affects the functions of proteins.
46
What are molecular chaperones? Know their key functions.
molecular chaperones are proteins that assist the conformational folding or unfolding and the assembly or disassembly of other macromolecular structures
47
Be able to explain the importance of the Active Site to enzyme function. Include the substrate.
an enzymes functions depends on the presence of specific arrangements of atoms where catalytic activity occurs substrate is the substance enzymes work on in these sites
48
Know why most enzymes exist as a holoenzyme. State the significance of the enzyme components as they relate to homeostasis.
- some are pure protein, others consist of 2 parts: apoenzyme and a cofactor. these ones are holoenzyme. - by adding oxygen and removing hydrogen
49
Know the basic steps of enzyme activity
enzymes allow reactions to occur at normal body temperatures by decreasing the amount of activation energy needed. the enzyme speeds up reactions by lowering the barrier 1-substrate(s) bind to the enzyme's active site, temporarily forming an enzyme-substrate complex 2-the enzyme-substrate complex undergoes internal rearrangements that form the product(s) 3-the enzyme releases the product(s) of the reation
50
What happens when a protein becomes denatured?
the protein unfolds and loses it's three-dimensional shape
51
Describe the monomers and general structures of nucleic acids
composed of carbon, hydrogen, oxygen, nitrogen, and phosphorus DNA or deoxyribonucleic acid and RNA or ribonucleic acid
52
``` Compare and contrast RNA and DNA: location - size - structure - sugar - N - bases - Functions - ```
RNA DNA cytoplasm(area around nucleus) Nucleus single strand double strand straight or folded double helix ladder ribose deoxyribose Adenine(A), Guanine(G), Adenine(A), Guanine(G), cytosine(C), Thymine(T) cytosine(C), Uracil(U) carries out genetic instructions directs protein synthesis; replicates self before cell division
53
Know the concept of complementary base pairing between strands of DNA
bonding is specific, A always bonds to T, and G always bonds to C
54
Describe the structure and function of ATP
an adenine-containing RNA nucleotide to which two additional phosphate groups have been added. it is the primary energy-transferring molecule in cells and it provides a form of energy that is immediately usable by all body cells.
55
Define matter
anything that has space and has mass
56
Define mass
is the total amount of matter in the object
57
Define energy
the capacity to do work or to putter matter into motion
58
Define chemical element
the form stored in the bonds of chemical substances
59
Define physical properties
properties that we can detect with our senses or measure
60
Define chemical properties
properties that deal with atoms interacting with other atoms and account for the facts that iron rust, animals can digest food, and so on
61
Define atomic symbol
the one or two letter designation assigned to an element
62
Define Periodic table
an oddly shaped checkerboard that lists all of the known elements and helps explain their properties
63
Define atom
indivisible / a cluster of small particles called protons, neutrons, and electrons
64
Define protons
a subatomic particle with a positive charge / weighs 1 AMU
65
Define neutrons
a subatomic particle with a neutral charge / weighs 1 AMU
66
Define electrons
a subatomic particle with a negative charge / weighs 1/2000 AMU
67
Define electron shell/energy level
An energy level represents the 3-dimensional space surrounding the nucleus where electrons are most likely to be(also called the electron shell/cloud)
68
Define valence shell
the outer-most electron shell/cloud
69
Define atomic number
the number is equal to the number of protons in the atoms nucleus
70
Define atomic mass
the sum of mass from both protons and neutrons
71
Define atomic weight
An average of the weights (mass numbers) of all the isotopes of an element, taking into account their relative abundance in nature
72
Define isotope
an element that has the same number of protons and electrons, but has a different number of neutrons.
73
Define radioisotope
isotopes that exhibit radioactivity, the event in which their atoms decompose spontaneously into more stable forms
74
Define molecule
when two or more atoms are held together by a chemical bond
75
Define compound molecule
when two or different kinds of molecules bind together
76
Define molecular formula
a formula giving the number of atoms of each of the elements present in one molecule of a specific compound
77
Define molecular weight
the sum of atomic weights
78
Define mixture
substances composed of two or more components physically intermixed
79
Define solvent
the substance present in the greatest amount in a solution, the dissolving agent
80
Define solute
the substance present in smaller amounts in solutions, is dissolved in the solvent
81
Define molarity
means 'moles per liter', is a way to express the concentration of a solution
82
Define mole
is equal to the atomic weight or molecular weight in grams
83
Define Avogadro's number
6.02 x 10^23, the number of solute particles always found in 1 mole
84
Define reactive
the body's ability to react in a proper way to influence the environment
85
Define inert
lacking any active nature, usually applied to physiological inactivity or to inactivity of certain genes
86
Define ion
an atom that lost or gained an electron(s) and now has a + or - charge
87
Define cation
an atom that loses electrons and acquires a net positive charge
88
Define anion
the atom that gains 1 or more electrons, and gains a net negative charge
89
Define electronegativity
when an electron has 6 or 7 electrons and very strongly attracts more
90
Define chemical reaction
whenever chemical bonds are formed, broken, or rearranged
91
Define chemical equation
the written equation of a chemical change. H + H + O= H2O
92
Define reactants
the number and kinds of interacting substances
93
Define products
the chemical composition of the result of the reaction
94
Define salt electrolyte
salt is an ion, which makes it an electrolyte, that contains cations other than H+ and anions other than the hydroxyl ion OH-
95
Define acid
a substance the releases hydrogen ions H+ in detectable amounts. a proton donor
96
Define base
take up hydrogen ions H+ in detectable amounts, a proton acceptor
97
Define neutralization
when you mix acids and bases together
98
Define buffer
a chemical system that resists abrupt and large swing in pH of body fluids by releasing hydrogen ions when the Ph begins to rise and binding them when the pH drops
99
Define hydrophobic
tending to repel or fail to mix with water.
100
Define hydrophilic
having a tendency to mix with, dissolve in, or be wetted by water
101
Define macromolecule
large complex molecules containing thousands of atoms
102
define polymer
are chainlike molecules made of smaller, identical or similar subunits (monomers)
103
define monomer
a molecule that can be bonded to other identical molecules to form a polymer.

human A&P 1 (10 decks)

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