Do Now

Please take 2 minutes to answer this question:

• Why do we need to study (review) chemistry in our anatomy/physiology class?

Do Now Objectives Matter & Energy Demo Matter

Do Now

Please take 2 minutes to answer this question:

• What is the most common element in the universe?

• What are humans made up of?

Do Now Objectives Matter & Energy Demo Matter

Anatomy & Physiology Textbook Analysis• New Material!!!!!!• What are the main topics for this chapter?• List three things that you think are important

in this chapter:• Chose a problem from the back of the chapter

that you feel is impossible for you to answer right now. Also, choose one that you can answer.

Objectives

Concepts of Matter and Energy• Differentiate clearly between matter and

energy.• List the major energy forms and provide one

example of how each energy form is used in the body.

Matter and Energy• Matter – anything that occupies space and

has mass (weight)• Energy – the ability to do work• Turn and talk about different kinds of

energies:• Chemical Electrical• Mechanical Radiant

Demonstration

• Feeling energy!• List all the types of energy needed in order for you to feel the electrical pulse of the machine:

Composition of Matter• Elements

• Fundamental units of matter• 96% of the body is made from four elements

• Carbon (C)• Oxygen (O)• Hydrogen (H)• Nitrogen (N)

• Atoms• Building blocks of elements

Chemistry’s Role in Human Anatomy

Chemistry is involved in:1. Growth2. Interaction with the environment3. Reproduction4. Movement

Atoms• The basic unit of matter• Made up of protons, neutrons, and electrons • nucleus = the center of the atom, contains the

protons (positively charged particles) and the neutrons (no charge) Protons and neutrons have roughly the same

mass• Have the same number of electrons (negative

charge) and protons (positive charge) so the overall charge on the atom is neutral (no charge)

Atomic Structure

• Nucleus• Protons (p+)• Neutrons (n0)

• Outside of nucleus• Electrons (e-)

Figure 2.1

Electrons

• Negatively charged particles • 1/1840 the mass of the neutrons/protons• Move around outside the nucleus in orbitals/shells

The first orbital (energy level) holds 2 electrons Every other orbital can hold up to 8 electrons** Orbitals want to be full, because then the atom is stable

• The number of electrons in an atom’s outer shell determines its chemical properties**

Elements• A pure substance that consists entirely of one type of

atom • Represented by one or two letters

Examples: Carbon = C, Hydrogen = H, Sodium = Na, Chlorine = Cl • Determined by the number of protons in an atom –

called the atomic number Examples: carbon has 6 protons, oxygen has 8 p, hydrogen has 1 p

• More than 100 known elements but only 13 make up most of the mass of the human body

Biochem intro

• http://www.youtube.com/watch?v=itWLaLat8LU

Identifying Elements

• Atomic number• Equal to the number of protons that the atoms

contain• Atomic mass number

• Sum of the protons and neutrons

IonsIon = atom that has a positive or negative charge because it gained or lost an electron to fill its outer orbital

Most common ions in the body:Sodium Na+

Potassium K+

Calcium Ca2+

Magnesium Mg 2+

Chlorine Cl-

Bicarbonate HCO3-

Biphosphate HPO42-

Sulfate SO42-

Do Now

Please take 2 minutes to answer this question:

• What elements make up most of the human body?

• How do we get these elements on a regular basis?

• Which element has 6 protons?

Do Now Objectives Matter & Energy Demo Matter

Principle Elements in the Human Body

1) Oxygen (O) 65% of body weight• Component of water, essential for respiration

2) Carbon (C) 18.6%• Found in all organic molecules

3) Hydrogen (H) 9.7%Component of H2O and most other compounds in the body

4) Nitrogen (N) 3.2%• Found in proteins and nucleic acids

Principle Elements in the Human Body

• 5) Calcium (Ca) 1.8%• Found in bones and teeth, necessary for membrane function,

nerve impulses, muscle contraction, and blood clotting

• 6) Phosphorous (P) 1%• Found in bones and teeth, nucleic acids, and ATP

• 7) Potassium (K) 0.4%• Necessary for membrane function, nerve impulses, and muscle

contractions

• 8) Sodium (Na) 0.2%• Necessary for membrane function, nerve impulses, and muscle

contractions

Principle Elements in the Human Body

• 9) Chlorine (Cl) 0.2 %• Important for membrane function and water absorption, major component of

stomach acid

• 10) Magnesium (Mg) 0.06%• Required for the activation of many enzymes

• 11) Sulfur (S) 0.04%• Found in many proteins

• 12) Iron (Fe) 0.007%• Essential for oxygen transport

• 13) Iodine (I) 0.0002%• Component of hormones of the thyroid gland

Isotopes• Atoms of the same element (have the same # of

protons) that differ in the number of neutrons• Represented by adding together the # of protons

and neutrons to determine the mass number (ex. Flourine-18)

• Different isotopes of a single element have the same chemical properties because they have the same numbers of protons and electrons**

Isotopes and Atomic Weight

• Isotopes

• Have the same number of protons• Vary in number of neutrons

Figure 2.3

Isotopes and Atomic Weight

• Atomic weight• Close to mass number of most abundant isotope• Atomic weight reflects natural isotope variation

Radioactivity

• Radioisotope• Heavy isotope• Tends to be unstable• Decomposes to more stable isotope

• Radioactivity• Process of spontaneous atomic decay

Do Now

• How are energy and matter related?• What is the human body mostly made of?• What is the most common element in the

universe?• Why did you feel the electricity yesterday?

Objectives

• Explore the need to know basic biological chemistry.

• Review and refresh chemical processes involved in the human body.

• Explore how atomic structure affects atoms, molecules and eventually the human body.

**Radioactive Isotopes• Isotopes whose nuclei are unstable and break

down at a constant rate over time, giving off matter or energy or both in the form of radiation

• Used for:1. Treating cancer and killing bacteria2. Following movements of atoms in

body tissues (PET Scan)

Molecules and Compounds

• Molecule – two or more like atoms combined chemically

• Compound – two or more different atoms combined chemically

Chemical Compounds• A substance formed by the combination of 2 or more

elements in definite proportions• Chemical formulas are used to show what is in a

compound Example: H2O, NaCl, CO2

• The chemical properties of a compound are very different from the properties of the atoms on their own

• Molecule = the smallest unit of most chemical compounds (but only for covalently bonded compounds)

Chemical Reactions

• Atoms are united by chemical bonds• Atoms dissociate from other atoms when

chemical bonds are broken

Electrons and Bonding

• Electrons occupy energy levels called electron shells

• Electrons closest to the nucleus are most strongly attracted

• Each shell has distinct properties• Number of electrons has an upper limit• Shells closest to nucleus fill first

Electrons and Bonding

• Bonding involves interactions between electrons in the outer shell (valence shell)

• Full valence shells do not form bonds

Inert Elements• Have complete valence shells

and are stable• Rule of 8s

• Shell 1 has 2 electrons• Shell 2 has 10 e

• 10 = 2 + 8• Shell 3 has 18 e

• 18 = 2 + 8 + 8Figure 2.4a

Reactive Elements

• Valence shells are not full and are unstable

• Tend to gain, lose, or share electrons• Allows for bond formation,

which produces stable valence

Quick group question

• Please take 2 minutes to answer these questions:• What are neutrons?• How are they related to atomic mass?

Chemical Bonds• A link that holds atoms together in a

compound • Formed between electrons • Formed to try and achieve stability by filling

outer energy level (orbital, shell)• Where the POTENTIAL ENERGY of a

compound is stored• Two types: covalent bonds and ionic bonds

Covalent Bonds

• Formed by the sharing of electrons between 2 atoms

• Can be single, double, or triple• Produces a tight link between atoms

Example: H20

Covalent Bonds

• Atoms become stable through shared electrons• Single covalent bonds share one electron• Double covalent bonds share two electrons

Do Now

Please take 2 minutes to answer this question:• How are chemical bonds like human

relationships?• What kind of an element are you (positively

charged, negatively charged or neutral)? Explain….

Objectives

Content:• Review reactive elements and valence “shells”.• Distinguish among the different kinds of chemical

bonds

Language:• Summarize the processes needed for synthesizing

molecules, by creating a table with the definitions of synthesis, decomposition and exchange.

IonsIon = atom that has a positive or negative charge because it gained or lost an electron to fill its outer orbital

Most common ions in the body:Sodium Na+

Potassium K+

Calcium Ca2+

Magnesium Mg 2+

Chlorine Cl-

Bicarbonate HCO3-

Biphosphate HPO42-

Sulfate SO42-

Ionic Bonds

• Formed by the transfer of 1 or more electrons from 1 atom to another

• Involves ions that are attracted to each other because of their opposite charges

Example: NaCl

Chemical Bonds

• Ionic Bonds• Form when electrons are completely

transferred from one atom to another• Ions: Charged particles

• Anions are negative• Cations are positive

Chemical Reactions• Process that changes one set of chemicals into another

set of chemicals• Metabolism: sum of all the chemical reactions in the

body that provide energy to maintain homeostasis and perform vital functions

• Reactants – elements or compounds that enter into chemical reactions

• Substrate – reactant in a biological reaction• Products – elements or compounds that are produced by

chemical reactions

Types of Chemical Reactions • Decomposition Reaction (Catabolism): breaks

molecule into smaller fragmentsExample: DigestionAB A + B

• Synthesis Reaction (Anabolism): assembles larger molecules from smaller components

Example: Hair GrowthA + B AB

Synthesis and Decomposition Reactions

Reaction Video

• http://www.youtube.com/watch?v=g-biRwAVTV8

Inorganic Compounds• Small molecules that do not contain Carbon and

Hydrogen atoms togetherExamples:1. Water2. Carbon Dioxide3. Oxygen4. Salts5. Acids and Bases

Types of Chemical Reactions • Exchange Reaction: reacting molecules are rearranged

Example: Sodium Bicarbonate + Hydrochloric Acid in stomach form salt, water, and CO2

AB + CD AC + BD

• Reversible Reactions (Equilibrium Reactions): actually two simultaneous reactions

Example: conversion of ATP to ADP, CO2 in the blood

A + B AB

Types of reactions

• http://www.youtube.com/watch?v=tE4668aarck

Energy and Work

• Work: movement or change in the physical structure of matter

• Energy: the capacity to perform work• Two types of energy:

1) Potential – stored in chemical bonds2) Kinetic – energy of motion

• Conversion of potential energy to kinetic energy is not 100% efficient – much of the energy is lost as HEAT

Energy in Reactions• Energy is released when a bond is broken• Energy is absorbed when a bond is

formed• All energy absorbing reactions need a

source of energy to start, which is called activation energy

Drop & Think

•Describe how our body breaks down and puts together chemicals!

•What do we call these type of reactions?

Do Now

• Please take 2 minutes to answer this question:• What have been your favorite parts of

this class?• What are the parts you have liked the

least?

Objectives

Content:• Review reactive elements and valence “shells”.• Distinguish among the different kinds of chemical

bondsLanguage:• Summarize the processes needed for synthesizing

molecules, by creating a table with the definitions of synthesis, decomposition and exchange.

Chemicals of the Human Body

• Nutrients: essential elements and molecules obtained in the diet

• Metabolites: all the molecules synthesized or broken down by the chemical reactions in our bodies

• Two categories: inorganic and organic compounds

Biochemistry: Essentials for Life

• Organic compounds• Contain carbon• Most are covalently bonded• Example: C6H12O6 (glucose)

• Inorganic compounds• Lack carbon• Tend to be simpler compounds• Example: H2O (water)

Water• Water is the most abundant compound in

living things (60-80% of human body) Example: provides cushioning for organs

• Water is essential for many chemical reactions in the body

Example: making carbohydrates and proteins

Water II• Water is an excellent solvent, enables many

nutrients to be transported throughout the body

Example: blood plasma

• Water has a high heat capacityExample: distributes body heat, helps you adapt to temperature

Chems in the body!

• http://www.youtube.com/watch?v=t5lXqRlKKdw

Mixture

• A substance composed of two or more elements or compounds that are mixed together but not chemically combined

• Two types of mixtures that can be made with water are solutions and suspensions

Solution• A mixture in which components are evenly

dispersed, commonly in liquid formExample: putting salt into a beaker of water

• solute – the substance that is dissolved (salt)• solvent – the substance in which the solute is

dissolved (water)

Do Now

• Please take 2 minutes to answer this question:• What is neutral pH?• What can you do when you feel the

stomach acid burning (heart burn)? – why does it work?

Suspension

• Mixtures of fluid and non-dissolved material

• Motion of fluid molecules keep materials from settling out

Example: blood

Carbon Dioxide and Oxygen

• Cellular respiration is the conversion of glucose into ATP

• ATP is the only energy source that cells use• Oxygen is an essential reactant in cellular

respiration• Carbon dioxide is a waste product of

cellular respiration

Carbon Dioxide and Oxygen

• Carbon dioxide is dissolved in blood plasma as carbonic acid or the bicarbonate ion

• Oxygen is attached to hemoglobin of red blood cells

Salts• Ionic compound containing a positive ion (not

H+) and a negative ion (not OH-)• When salts dissolve in water, ions become

electrolytes• Electrolyte: substance that conducts an electrical

current in solution• Common salts in the body: NaCl, Ca2CO3,

KCl, Ca(PO4)2

Salts

Functions in the Human Body:1) Na+ and K+ are essential for nerve transmission2) Fe2+ in hemoglobin helps transport

oxygen3) Zn2+ and Cu2+ assist in the function of

enzymes

Drop & Think

•Why do we need salts in the body?

•How do we get these salts?

Chems in body?

• http://www.youtube.com/watch?v=0JZPNmkV3zE

Acids and Bases

• Acids and bases are considered electrolytes (dissociate in water and conduct electrical current)

• When mixed, neutralization occurs, and a salt and water are formed

H20 ↔ H+ + OH-

• Water molecules “liberate” the ions from the acids and bases

• H+ one of the most reactive ions in nature

pH

• Measures relative concentration of hydrogen ions• pH 7 = neutral• pH below 7 = acidic• pH above 7 = basic• Buffers: chemicals

that can regulate pH change

Figure 2.11

pH Scale• Measurement system used to measure the amount

of H+ ions in a solution• Ranges from 0-14 • The lower the # the higher the acidity (higher

number of H+ ions)• The higher the # the higher the alkalinity

(lower number of H+ ions)• Distilled (pure) water has a neutral pH of 7

Scale explained

• http://www.youtube.com/watch?v=uba-T01uF3U

• http://www.youtube.com/watch?v=yodcYTUZjC8

pH Scale Continued…

• Each step on the scale represents a factor of 10 in the concentration of H+ ions

• A solution with pH 5 is 10x more acidic then a solution with pH 6 (has 10x as many H+ ions)

• A solution with pH 4 is 100x more acidic than a solution with a pH 6 (has 100x as many H+ ions)

Acids

• Any compound that forms H+ ions in solution

• Have pH values below 7• Sour, react with metals, “burn”• Examples: hydrochloric acid, acetic

acid, carbonic acid

Do Now

• What is the normal pH of human blood?

• Is it a base or an acid?• Why is carbon so important in our bodies?

Bases

• A compound that forms OH- ions in solution

• Have pH values above 7• Bitter taste, feel slippery• Examples: bicarbonate, ammonia,

magnesium hydroxide

Regulation of pH in the Body

• Human blood has a normal pH range of 6.5 - 7.5

• This is necessary to maintain homeostasis!• Enzymes used to speed up biological reactions

only work in a very specific pH• pH is regulated by the kidneys, lungs, and

buffers

Buffers• Dissolved compounds that help prevent sharp

swings of pH (weak acids and bases)• When pH rises, they bind H+ to lower pH• When pH drops, they release to H+ to raise pH• Example: reversible reaction involving carbonic

acid and bicarbonate ion in blood

Weak Base Weak Acid

Organic Compounds

• Compounds that contain carbon• 5 major organic compounds found

in living things:1. Carbohydrates2. Lipids3. Nucleic acids4. Proteins5. ATP

Carbon’s Importance in Human Biology

• Four electrons in last energy level• Forms four covalent bonds• Bonds well with other carbon atoms• Bonds can be single, double, or triple• Can form long chains or ring structures

Macromolecules

• Giant molecules made from thousands of smaller molecules through polymerization

• Polymerization is the joining together small units to build larger ones

• Monomers = smaller unit• Polymer = larger unit, macromolecule

Do Now

• What is the difference between saturated and unsaturated fats?

• How will you prepare for your test?• Who has finished their poster?

Objectives

Content:• Compare and contrast different type of

macromoleculesLanguage:• Summarize the naming process for

macromolecules so that by looking at them, their group can be determined.

Carbohydrates

• Contains C, H, O (often end in suffix “– ose”)• 1:2:1 ratio• Monomers are called monosaccharides or simple

sugars Examples: glucose, fructose, lactose, sucrose

• Polymers are called polysaccharidesExamples: glycogen, cellulose, starch

Function of Carbohydrates in the Body

• Monosaccharide glucose is the most important metabolic fuel in the body

• Simple sugars (mono- and di-): source of energy (roughly 50% of our diet)

• Polysaccharides (glycogen in humans): food storage in liver and skeletal muscle

Lipids• Mostly C and H with a few O• Monomers (not true monomers) – glycerol + fatty acids• Generally not soluble in water• Five main categories of lipids:

1. Fats2. Oils3. Waxes4. Steroids5. Hormones

Fatty Acids

• Long chains of carbon atoms• Saturated – all single bonds between

carbons (i.e. saturated with hydrogens)• Unsaturated – at least one double

bond in carbon chain• Polyunsaturated – more than 1 double bond

Saturated Fatty Acids

• More hydrogen atoms• More energy (Why?)• Mostly animal fats• Usually solid at room temperature

Unsaturated Fatty Acids

• Fewer hydrogen atoms• Less energy• Mostly plant fats (olive oil (mono-), corn

oil, (poly-))• Usually called oils instead of fats• Liquid at room temperature

Function of Lipids in the body

• Insulation against heat loss• Protection from mechanical damage• Energy storage• Major structural part of biological membranes• Steroids are basis for hormones produced by the

adrenal gland and reproductive system• Cholesterol (a steroid based molecule) is essential

for Vitamin D and bile production

Bio Style?

• http://www.youtube.com/watch?v=nt9u7CfVoc4

Objectives

Content:• Complete biochem pre-test (open

notebook) using the guided notes from prior lectures.

• Utilize each other as partners in learning.

• Prepare for “real” test

Proteins• C, H, O, N, sometimes S or P• The most diverse macromolecule• Monomers – 20 different amino acids

• The body can make 10, the other 10 must be obtained in the diet, “essential”

• The order and number of amino acids determine which protein is made (that information is stored in DNA)

Function of Proteins

• Structural – muscles, fingernails, hair, ligaments

• Transport substances across membranes• Fight disease (antibodies)• Control chemical reactions: enzymes

Enzymes I• Proteins that speed up the rate of

chemical reactions (catalysts)• Catalyst: something that speeds up a

reaction but does not change or get used up• Make many chemical reactions

possible• Very, very specific – one enzyme to

one reaction

Enzymes

• Active sites are sites where reactants and substrates can be brought together to react and form products

• Enzymes affected by temp, pH, etc.• Denaturation: protein changes shape and

can’t function properly (ex. cooked egg white)

Nucleic Acids

• C, H, O, N, P• Monomers = nucleotides• Polymers = DNA and RNA

Nucleic Acids

• Provide blueprint of life• Nucleotide bases

• A = Adenine• G = Guanine• C = Cytosine• T = Thymine• U = Uracil

• Make DNA and RNA

Nucleic Acids

• Deoxyribonucleic acid (DNA)• Organized by

complimentary bases to form double helix

• Replicates before cell division

• Provides instruction for every protein in the body

Figure 2.18c

Function of Nucleic Acids

DNA:• Stores and transmit hereditary or genetic

information• Provides the directions for making all the

proteins in the body (growth and development)

RNA:• Carries out instructions for making

proteins

ATP• High energy but unstable compound• Created during anaerobic and aerobic respiration

from glucose• It is the only type of energy that cells can directly use• Without ATP:

1) Molecules could not be made or broken down2) Substances would not be actively transported across

membranes3) Muscles could not contract4) Nerves could not send impulses

Do Now

• Will you perform better on this test than the 1st one?

• How did you prepare for your test?

Objectives

Content:• Complete biochem REAL-test• Preview the next unit of study in our

class.