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Anatomy and Physiology > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

Matter

A

Anything that has mass and occupies space

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2
Q

Weight

A

The pull of gravity on mass

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3
Q

States of Matter

A

Solid
Liquid
Gas

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4
Q

Energy

A

The capacity to do work or put matter into motion

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5
Q

Types of Energy

A

Kinetic

Potential

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6
Q

Forms of Energy

A

Chemical- stored in bonds of chemical substances
Electrical- Results from movement of charged particles
Mechanical- Directly involved in moving matter
Radiant- Travels in waves (ultraviolet light)

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7
Q

Energy form Conversion

A
  • May be converted from one form to another

- Conversion is inefficient (some energy is lost as heat)

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8
Q

Elements

A

Matter is elements

Cannot be broken into simpler substances by ordinary chemical methods

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9
Q

Human Body Elements (4)

A 
Oxygen
Carbon
Hydrogen 
Nitrogen
96% of the human body
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10
Q

Atoms (overall)

A

Building blocks for each element
Gives each element its physical and chemical properties
Smallest particles of an element with properties of that element

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11
Q

Atoms (make-up)

A

composed of subatomic particles- protons, neutrons, and electrons
Protons and Neutrons found in nucleus
Electrons orbit nucleus in an electron cloud

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12
Q

Atom (nucleus)

A

Almost entire mass of the atom
Neutrons- Carry no charge
Protons- Carry positive charge

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13
Q

Atom (electrons)

A

Electrons orbit within electron cloud

  • carry a negative charge
  • 1/2000 the mass of a proton
  • number of protons and electrons always equal
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14
Q

Atom (models)

A

Planetary model-2D simplified; outdated

Orbital model-3D current model, used by chemists

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15
Q

Isotyopes

A

Structural variations of atoms
Differ in the number of neutrons they contain
Atomic numbers same; mass numbers different

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16
Q

Atomic Weight

A

Average of mass numbers (relative weights) of all isotopes of an atom

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17
Q

Molecule vs. Compound

A

Molecule- 1 type

Compound- multiple types (at least 1)

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18
Q

Mixtures

A

Two or more components physically intermixed

-most matter exists as mixture

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19
Q

3 Types of Mixtures

A

Solutions
Colloids
Suspensions

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20
Q

Solutions

A

Homogeneous mixtures
Solvent- greatest substance, if a liquid; usually water
Solute- present in smaller amounts

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21
Q

Colloids

A

Heterogeneous mixtures

Larger solute particles do not settle out

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22
Q

Suspensions

A 
Heterogeneous mixtures (blood) 
Large, visible solutes settle out
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23
Q

Mixtures Vs. Compounds

A 
Mixture:
-No chemical bonding between components
-Can be separated 
-Heterogeneous or Homogeneous
Compound:
-Chemical bonding between components
-Can be separated
-All are homogeneous
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24
Q

Chemical Bonds

A

Energy relationships
Electrons can occupy up to 7 electron shells
Electrons in Valence Shell (outermost electron shell)
-have most potential energy
-are chemically reactive electrons

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25
Q

Chemically Inert Elements

A

Stable and unreactive
Valence shell fully occupied or contains eight electrons
Noble Gases

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26
Q

Chemically Reactive Elements

A

Valence shell not full

Tend to gain, lose, or share electrons (form bonds) with other atoms achieve stability

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27
Q

Types of Chemical Bonds (3)

A

Ionic
Covalent
Hydrogen

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28
Q

Ionic Bonds

A

Ions
-atoms gain or lose electrons and becomes charged
Transfer of electrons from one atom to another forms ions
-Anion (negative charge)
– atoms gains at least one electron
-Cation (positive charge)
– atoms loses at least one electron

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29
Q

Ionic Compounds

A

Most ionic compounds are salts
-when dry salts form crystals instead of individual molecules
Ex. NaCl (sodium chloride)

30
Q

Covalent Bonds

A

Formed by sharing of two or more electrons

Allows each atom to fill its valence shell at least part of the time

31
Q

Ionic Vs. Covalent

A

Ionic- giving

Covalent- sharing

32
Q

Hydrogen Bonds

A

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

  • not true bond
  • common in water
  • also acts as intramolecular bonds, holding a large molecule in a 3D shape
33
Q

Chemical Reactions

A

Occur when chemical bonds are formed, rearranged, or broken

-Reaction is the combination of formed, rearranged, or broken

34
Q

Patterns of Chemical Reactions

A

Synthesis (combination) reaction
Decomposition reactions
Exchange reactions

35
Q

Synthesis Reactions

A

A + B = AB

  • Atoms or molecules combine to form larger, more complex molecule
  • Always involve bond formation
  • Anabolic
36
Q

Decomposition Reactions

A

AB = A + B

  • Molecule is broken down into smaller molecules or its constituent atoms
  • -Reverse of synthesis reactions
  • Involving breaking of bonds
  • Catabolic
37
Q

Exchange Reactions

A

AB + C = AC + B

  • Also called displacement reactions
  • Involve both synthesis and decomposition
  • Bonds are both made and broken
38
Q

Energy Flow in Chemical Reactions

Two Types

A

All chemical reactions are either exergonic or endergonic

  • Exergonic Reactions- Exer- Exit leaving
  • -net release of energy
  • -products have less potential energy than reactants
  • -catabolic and oxidative reactions
  • Endergonic Reactions- Ender- Enter gaining/absorbing
  • -net absorption or energy
  • -products have more potential energy than reactants
  • -Anabolic reactions
39
Q

Reversibility of Chemical Reactions

A 
Chemical equilibrium
AB = A + B
A + B = AB
Many biological reactions are essentially irreversible
-due to energy requirements
-due to removal of products
40
Q

Rate of Chemical Reactions

A

Affected by

  • Rising Temperature = Rising Rate
  • Rising Concentration of Reactant = Rising Rate
  • Lowering Particle Size= Rising Rate
  • Catalysts: Rising Rate without being chemically changed or part of product
  • -enzymes are biological catalysts
41
Q

Biochemistry

A

Study of chemical composition and reactions of living matter

All chemicals either organic or inorganic

42
Q

Classes of Compounds

A

Inorganic- water, salts,and many acids and bases; does not contain carbon
Organic- carbohydrates, fats, proteins, and nucleic acids; contains carbon
Both equally essential for life

43
Q

Water in Living Organisms

A

Most abundant inorganic compound
Most important inorganic compound
-due to water’s properties

44
Q

Properties of Water

A

High heat capacity
-absorbs and release heat with little temperature change
-prevents sudden changes in temperature
High heat evaporation
-evaporation requires large amounts of heat
-useful cooling mechanism
Polar solvent properties
-universal solvent
-dissolves and dissociates ionic substances
-body’s major transport medium
Cushioning
-protects certain organs from physical trauma (cerebrospinal fluid)

45
Q

Salts

A

Ionic compounds that dissociate into ions in water

  • ions (electrolytes) conduct electrical currents in solution
  • ions plat specialized roles in body functions
  • ionic balance vital for homeostasis
46
Q

Acids and Bases

A 
Both are electrolytes
Acids- proton donors
- release in H+ solution
Bases- proton acceptors
-Take up H+ from solution
47
Q

pH: Acid base Concentration

A

-Free H+ of a solution measured on pH scale
-As free H+ increases, acidity increases
-As free H+ decreases alkalinity increases
pH= negative logarithm of H+ in mole per liter
pH scare ranges from 0-14

48
Q

pH: Levels

A 
Acidic Solutions
-rising H+, lower pH
-acidic pH = 0- 6.99
Neutral Solutions
- equal number of H+ and OH- 
- All neutral solutions are pH 7
-pure water is pH neutral
Alkaline (basic) Solutions
-lowering H+, higher pH
-Alkaline pH = 7.01-14
49
Q

Neutralization

A

Mixing acids and bases

  • forming water and a salt
  • neutralization reaction
50
Q

Acid-Base Homeostasis

A
  • pH change interferes with cell function and may damage living tissue
  • Even slight change in pH can be fatal
  • pH is regulated by kidneys, lungs, and chemical buffers
51
Q

Organic Compounds

A

Molecules that contain carbon
-except CO2 and Co, which are considered inorganic
-Carbon is electroneutral
Unique to living systems
Carbohydrates, lipids, proteins, and nucleic acids

52
Q

Carbohydrates

A 
Sugars and starches
Polymers
Three classes:
-Monosaccharides 
-Disaccharides 
-Polysaccharides
Function- cellular fuel 
-Ex. glucose
53
Q

Disaccharides

A 
Double sugars
Too large to pass through cell membranes
Important disaccharides
-sucrose 
-maltose
-lactose
54
Q

Polysaccharides

A

Polymers of monosaccharides
Important polysaccharides
-starch and glycogen
Not very soluble

55
Q

Lipids

A 
Insoluble in water 
Main Types:
-Triglycerides or neutral fats
-Phospholipids
-Steroids
-Eicosanoids
56
Q

Triglycerides

A

Energy storage
Insulation
Protection

57
Q

Phospholipids

A

Important in cell membrane structure

58
Q

Steroids

A

Interlocking 4-ring structure
Cholesterol, vitamin D, steroid hormones, and bile salts
Most important steroid is Cholesterol

59
Q

Eicosanoids

A

Prostaglandin (most important eicosanoid

-Role in blood clotting, control of blood pressure, inflammation, and labor contractions

60
Q

Other Lipids in the Body

A

Other fat-soluble vitamins (A, D, E, K)

Lipoproteins- transport fats in the blood

61
Q

Proteins

A 
Proteins are polymers
Amino acids (20 types) are the monomers in proteins
62
Q

Fibrous Proteins

A
  • Structural
  • Strandlike, water-insoluble, and stable
  • Provide mechanical support and tensile strength
  • Ex. keratin, elastin, collagen
63
Q

Globular Proteins

A
  • Functional
  • 3D structure
  • Specific functional regions (active sites)
  • Ex. antibodies, hormones, molecular chaperons, and enzymes
64
Q

Protein Denaturation

A

Proteins unfold and lose function-active sites destroyed
Can be caused by decreased pH or increased temperature
Usually reversible if normal conditions restore
Irreversible if changes extreme
-Ex. Cooking an egg

65
Q

Enzymes

A

Proteins that act as biological catalysts
-regulate and increase speed of chemical reactions
Lower the activation energy, increase the speed of a reaction

66
Q

Characteristics of Enzymes

A

Usually end in -ase
Often named for the reaction they catalyze
-Ex. hydrolases, oxidases

67
Q

Nucleic Acids

A 
Deoxyribonucleic Acid (DNA)
Ribonucleic Acid (RNA)
largest molecules in the body
68
Q

Deoxyribonucleic Acid (DNA)

A

Located within the nucleus
Utilizes 4 nitrogen bases
-Adenine (A), Guanine (G)
-Cytosine (C), Thymine (T)
–base pair rule- each base pair with its complementary base (A and T); (G and C)
Double-stranded helical molecule (double helix) in the cell nucleus
Provides instructions for all protein synthesis
Replicates before cell division ensuring genetic continuity

69
Q

Ribonucleic RNA

A 
Located outside the nucleus
Utilizes 4 nitrogen bases
-Cytosine (C), Guanine (G)
-Adenine (A), Uracil (U)
Single-stranded molecule
Three varieties of RNA carry out the DNA orders for protein synthesis
70
Q

Adenosine Triphosphate (ATP)

A

Chemical energy in glucose captured in this important molecule
Directly powers chemical reactions in cells
Energy form immediately usable by all body cells
Structure of ATP
-Adenine-containing RNA nucleotide with two additional phosphate groups

71
Q

Function of ATP

A

Phosphorylation:

  • Terminal phosphates are enzymatically transferred to and energize other molecules
  • Such “primed” molecules perform cellular work (life processes) using the phosphate bond energy

Anatomy and Physiology (27 decks)

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