SOCM EAP‐The Chemical Level of Organization PFN: …slides.jsomtc.org/SOMAPL12/SOMAPL12.pdf3 JSOMTC, SWMG(A) Slide 7 Agenda Communicate how the chemical properties of water make

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Slide 1JSOMTC, SWMG(A)

SOCMEAP‐The Chemical Level of

OrganizationPFN: SOMAPL12

Hours: 2.5


Terminal Learning Objective

Action: Communicate knowledge of “The Chemical Level of Organization”

Condition: Given a lecture in a classroom environment

Standard: Received a minimum score of 75% on the written exam IAW course standards


References

• Essentials of Anatomy and Physiology (6th

edition; 2013; Martini/Bartholomew)

2


Reason

As you begin your study of A&P, it is essential that you obtain a good understanding of the Chemical Level of Organization. Without it, you will not have established a bases from which to work. This could result in you having to struggle needlessly through the remainder of the A&P block.

As a SOCM Medic / Corpsman your knowledge of this chapter will enhance your patient treatment skills and your ability to communicate with other healthcare providers.


Agenda

Define the medical vocabulary components related to the chemical level of organization

Identify an atom and an element

Communicate the ways in which atoms combine to form molecules and compounds

Identify the use of chemical notation to symbolize chemical reactions


Agenda

Differentiate among the three major types of chemical reactions that are important to studying physiology

Identify the role of enzymes in metabolism

Differentiate between organic and inorganic compounds and communicate the physiological roles of inorganic compounds

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Agenda

Communicate how the chemical properties of water make life possible

Communicate the pH scale in the role of buffers in body fluids

Identify the structure and functions of carbohydrates, lipids, proteins, nucleic acids, and high‐energy compounds


The Medical Vocabulary Components Related to the

Chemical Level of Organization


Vocabulary Development

anabole a building up; anabolism

endo inside; endergonic

exo outside; exergonic

glyco sugar; glycogen

hydro water

lysis breakdown; hydrolysis

katabole a throwing down; catabolism

katalysis dissolution; catalysis

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Vocabulary Development

lipos fat; lipids

metabole change; metabolism

sakcharon sugar

mono single; monosaccharide

di two; disaccharide

poly many; polysaccharide


An Atom and an Element


Matter: Atoms and Molecules

Atoms

Smallest stable unit of matter

Subatomic particles

• Protons: (+) charge

• Neutrons: neutral

• Electrons: (‐) charge

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Structure of an atom

Nucleus

• Protons

• Neutrons

Electron Shell





Structure of an Atom Atomic number

• Equals number of protons

Atomic mass• Equals protons + neutrons

Isotopes of element• Reflects number of neutrons

Atomic weight• Averages isotope abundance

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Structure of an Atom

Electrons surround nucleus

Electrons are organized in shells

The outer shell determines the atom’s chemical properties



Atoms and Electron Shells



Key Note

All matter is composed of atoms in various combinations. The chemical rules governing the interactions among atoms alone and in combination establish the foundations of physiology at the cellular level.

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Check on Learning

What is the smallest, most stable unit of matter?

A. Proton

B. Cation

C. Atom

D. Element


The Ways in Which Atoms Combine to Form Molecules and Compounds



Chemical Bonds and Compounds

Atoms bond to each other in chemical reactions

Reactions transfer electrons

Electrons are gained, lost, or shared

Molecules or compounds result

• Compounds contain several elements

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Ionic Bonds Atoms gain or lose electrons Charged atoms are ion Ions bear (+) or (‐) charge

• Cations have (+) charge• Anions have (‐) charge

Cations and anions attract Ions form bonds





Covalent bonds Some atoms share electrons Shared electrons complete outer shell Sharing atoms bond covalently

• Single covalent bond One shared electron

• Double covalent bond Two shared electrons

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Matter: Atoms and Molecules Covalent Bonds



Non‐polar and Polar Covalent Bonds

Equal electron sharing

• Non‐polar covalent bonds

• Example: carbon‐carbon bonds

Non‐equal electron sharing

• Polar covalent bonds

• Example: oxygen‐hydrogen bonds



Hydrogen bonds

Weak attractive force

Between two neighboring atoms

• A polar‐bonded hydrogen, and

• A polar‐bonded oxygen or nitrogen

For example, between water molecules

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Matter: Atoms and Molecules Hydrogen Bonds


Check on Learning

Which of the following is not a type of chemical bond?

A. Ionic

B. Hydrogen

C. Covalent

D. Kinetic


The Use of Chemical Notation to Symbolize Chemical Reactions

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Chemical Notation

A chemical “shorthand”

Simplified descriptions of:

• Compounds

• Structures

• Reactions

• Ions

Abbreviations of elements

Abbreviations of molecules


Chemical Notation

2H + O H2O

What does the 2H represent?

• What does represent?

• Which is considered the reactant?

• Which is considered the product?


Chemical Reactions

Metabolism

All the chemical reactions in the body

Consumes reactants

Produces products

Breaks or makes chemical bonds between atoms

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Chemical Reactions

Basic Energy Concepts

Work—movement or change in matter’s physical structure

• e.g., running, synthesis of molecules

Energy—ability to do work

• Kinetic energy

• Potential energy


Chemical Reactions

Basic Energy Concepts (cont.)

Potential energy—stored energy

• e.g., a stretched spring, chemical bonding

Kinetic energy—energy of movement

• e.g., explosions, breaking chemical bonds


Check on Learning

In a chemical reaction, what are the interacting participants called, and what does the reaction generate?

A. Metabolites and energy

B. Catabolic and synthesis

C. Reactants and product

D. None of the above

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The Three Major Types of Chemical Reactions that are Important to

Studying Physiology


Chemical Reactions

Three types of reactions

Decomposition—breaks molecule into smaller pieces

Synthesis—assembles smaller pieces into larger one

Exchange—shuffles pieces between molecules


Chemical Reactions

Decomposition Reactions

In chemical notation:

• AB → A + B

• Releases covalent bond energy

Hydrolysis—Decomposition reaction with H and OH

• e.g., food digestion

Catabolism—Sum of all the body’s decomposition reactions

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Chemical Reactions

Synthesis Reactions


• A + B → AB

• Absorbs energy

Formation of new bonds

Dehydration synthesis

• Removal of H and OH between molecules

Anabolism—Sum of the body’s synthesis reactions


Chemical Reactions

Exchange Reaction


• AB + CD → AC + BD

Decomposition and synthesis


Chemical Reactions

Reversible Reactions

A + B ↔ AB

Equilibrium—Condition when the forward and reverse reactions occur at the same rate

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Chemical Reactions

Key Note

Things tend to even out, unless something prevents this from happening. Most reversible reactions quickly reach equilibrium, where opposing reaction rates are balanced. If reactants are added or removed, reaction rates change until a new equilibrium is established.


Check on Learning

What are the three types of chemical reactions important to the study of physiology?

A. Hydrolysis / Catabolism / Metabolite

B. Decomposition / Synthesis / Exchange

C. Enzyme / Chemical / Reversible

D. Non Reversible (stable) / Reversible (Unstable) / Metabolite (stable‐unstable)


The Role of Enzymes in Metabolism

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Enzymes and Reactions

Activation Energy ‐ Quantity of energy needed to start a chemical reaction

Catalysts reduce activation energy and accelerates the reaction

Enzymes catalyze cellular reactions


Enzymes and Reactions Enzymes and Activation Energy


Enzymes and Reactions

Exergonic—Reactions that release energy e.g., decomposition reactions (i.e., they are exothermic)

Endergonic—Reactions that consumeenergy

e.g., synthesis reactions (i.e., they are endothermic)

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Chemical Reactions

Key Note

Most of the chemical reactions that sustain life cannot occur under homeostatic conditions unless appropriate enzymes are present.


Check on Learning

What affect does lowering the activation energy by enzymes have in a cell?

A. The rate of a reaction proceeds

B. The direction of the reaction and the products that are formed

C. Enzymes can bring about a reaction that would otherwise be impossible

D. All of the above


Organic and Inorganic Compounds and the Physiological Roles of

Inorganic Compounds

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Inorganic Compounds

Nutrients

Essential elements and molecules obtained from the diet

Metabolites

Molecules synthesized or broken down by chemical reactions inside the body


Inorganic Compounds

Inorganic

Smaller molecules such as water and oxygen that lack carbon and hydrogen

Inorganic molecules do not have carbon

• The only exception is carbon dioxide

Organic

Larger molecules such as sugars, proteins, and fats composed largely of carbon and hydrogen

Organic compounds always have carbon

•Usually have hydrogen and oxygen also


Inorganic Compounds

Carbon Dioxide (CO2)

Gas produced by (animal) cellular metabolism

and released into the atmosphere via the lungs

Oxygen (O2)

Atmospheric gas consumed by (animal) cells in

order to produce energy

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Check on Learning

Which of the following substances is/are inorganic?

A. Carbon Dioxide

B. Oxygen

C. Water

D. All of the above


How the Chemical Properties of Water Make Life Possible


Inorganic Compounds

Water and its properties

Most important body chemical

Excellent solvent

High heat capacity

Essential chemical reactant

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Inorganic Compounds


Chemical Reactions

Key Note

Water accounts for most of your body weight; proteins, the key structural and functional components of cells, and nucleic acids, which control cell structure and function, work only in solution.


Check on Learning

What is/are the properties of water?

A. Water has a high heat capacity

B. Water is an excellent solvent

C. Water is an essential reactant in chemical reactions of living systems

D. All of the above

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The pH Scale in the Role of Buffers in Body Fluids


Inorganic Compounds

Inorganic Acids and Bases

Acid—Releases hydrogen ions (H+) into solution

• e.g., HCl → H+ + Cl‐

Base—Removes hydrogen ions from solution

• e.g., NaOH + H+ → Na+ + H•OH


Inorganic Compounds

pH (potentials of Hydrogen)

A measure of hydrogen ion concentration in a solution

•Neutral solution—pH = 7

• Acidic solution—pH below 7

• Basic solution—pH above 7

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Inorganic Compounds

pH and Hydrogen Ion Concentration


Inorganic Compounds

Buffers

Maintain pH within normal limits (pH 7.35 to pH 7.45)

Release hydrogen ions if body fluid is too basic

Absorb hydrogen ions if body fluid is too acidic


Inorganic Compounds

Salt

An ionic compound not containing H+ or OH‐

Salts are electrolytes

Electrolytes dissociate in water

• e.g., NaCl → Na+ + Cl‐

Electrolytes carry electrical currents in the body

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The Structure and Functions of Carbohydrates, Lipids, Proteins, Nucleic Acids, and High‐energy

Compounds


Organic Compounds

Organic Compounds

Contain carbon, hydrogen, and usually oxygen

Important classes of organic compounds include:

• Carbohydrates

• Lipids

• Proteins

• Nucleic acids


Organic Compounds

Carbohydrates (1:2:1) ratio

Most important energy source for metabolism

Three major types

•Monosaccharides (e.g., glucose)

•Disaccharides (e.g., sucrose)

• Polysaccharides (e.g., glycogen)

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Organic Compounds

Glucose


Formation and Breakdown of Complex Sugars


Organic Compounds

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Organic Compounds


Organic Compounds

Lipids

Water‐insoluble

Four important classes

• Fatty acids

Carboxylic acid group dissolves in solution

Hydrocarbon tail relatively insoluble

• Fats

Three Fatty acids attach to a glycerol base to form a triglyceride

Energy, insulation, and protection


Organic Compounds

Lipids

Four important classes (cont.)

• Steroids

Cholesterol (diet, liver)

Some Hormones (sex)

• Phospholipids

Water soluble head

Water insoluble tail

Most abundant lipid of cell membranes

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Organic Compounds


Organic Compounds Fatty Acids


Organic Compounds Triglycerides

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Organic Compounds

A Phospholipid Molecule


Organic Compounds

Proteins

Most abundant organic component in human body

About 400,000 different proteins

Contain carbon, nitrogen, oxygen, hydrogen, and sometimes sulfur


Organic Compounds

Proteins play vital roles

Support

Movement

Transport

Buffering

Metabolic Regulation

Coordination and Control

Defense

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Organic Compounds

Protein Structure

“R” groups interact with their neighbors and with solvent

Amino acid chain folds and twists into complex shape

Final shape determines function

High fever distorts shape (i.e., denaturing)

Distorted proteins don’t work exactly the same


Organic Compounds Proteins are built from amino acids


Organic Compounds

Peptide bonds join amino acids into long strings

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Organic Compounds


Organic Compounds

Enzyme Function

Substrates (reactants) bind to active site on enzyme surface

Binding lowers activation energy needed for reaction

Substrates react to form product

Product is released from enzyme surface


Organic Compounds

Enzyme function made simple

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Organic Compounds

Nucleic Acids

Large molecules

Built from atoms of C, H, O, N, and P (What are these elements?)

Store and process molecular information

Two classes of nucleic acids

• DNA (deoxyribonucleic acid)

• RNA (ribonucleic acid)


Organic Compounds

Structure of Nucleic Acids

Nucleotides contain a sugar, a phosphate, and a base

Sugar‐phosphate bonds link nucleotides in long strands

Hydrogen bonds hold two DNA strands in a double helix


Organic Compounds The Structure of Nucleic Acids

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Organic Compounds The Structure of Nucleic Acids


High‐Energy Compounds

Catabolism releases energy

Cells store energy in high‐energy compounds

High‐energy compounds drive endergonicreactions

ATP is the most important high‐energy compound in cells

ATP keeps cells alive!


High‐Energy Compounds Structure of ATP

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High‐Energy Compounds


Summary of Body Chemistry Organic Chemical Building Blocks


Chemicals and Cells

Biochemical building blocks

Cells

Miniature organism

Lipid membrane

Proteins

Nucleic acids

Carbohydrates

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QUESTIONS?


Terminal Learning Objective

Action: Communicate knowledge of “The Chemical Level of Organization”

Condition: Given a lecture in a classroom environment

Standard: Received a minimum score of 75% on the written exam IAW course standards


Agenda

Define the medical vocabulary components related to the chemical level of organization

Identify an atom and an element

Communicate the ways in which atoms combine to form molecules and compounds

Identify the use of chemical notation to symbolize chemical reactions

34


Agenda

Differentiate among the three major types of chemical reactions that are important to studying physiology

Identify the role of enzymes in metabolism

Differentiate between organic and inorganic compounds and communicate the physiological roles of inorganic compounds


Agenda

Communicate how the chemical properties of water make life possible

Communicate the pH scale in the role of buffers in body fluids

Identify the structure and functions of carbohydrates, lipids, proteins, nucleic acids, and high‐energy compounds


Reason

As you begin your study of A&P, it is essential that you obtain a good understanding of the Chemical Level of Organization. Without it, you will not have established a bases from which to work. This could result in you having to struggle needlessly through the remainder of the A&P block.

As a SOCM Medic / Corpsman your knowledge of this chapter will enhance your patient treatment skills and your ability to communicate with other healthcare providers.

35


BREAK!

SOCM EAP‐The Chemical Level of Organization PFN: …slides.jsomtc.org/SOMAPL12/SOMAPL12.pdf3 JSOMTC, SWMG(A) Slide 7 Agenda Communicate how the chemical properties of water make

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