What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe.

What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe. 1. Give an example of solid matter. 2. Give an example of liquid matter. 3. Give an example of gaseous matter. 4. Is all matter visible? 5. Does all matter take up space? Section 2-1 Interest Grabber

2–1The Nature of Matter A.Atoms B.Elements and Isotopes 1.Isotopes 2.Radioactive Isotopes C.Chemical Compounds D.Chemical Bonds 1.Ionic Bonds 2.Covalent Bonds 3.Van der Waals Forces Section 2-1 Section Outline

6 C Carbon 12.011 Section 2-1 An Element in the Periodic Table

Individual substances, Substance which cannot be broken down or subdivided by ordinary chemical means. Pure substances made up of only one type of atom

Anything that has mass and takes up space (volume). All matter is made up of atoms. Matter

Periodic Table, Biological Essentials

ATOMS The small units of matter 2 major Parts Nucleus (Protons+Neutrons) Electron cloud Atoms are smaller than cells

Structure of an atom Electron Cloud Nucleus

Nucleus +Found in the center of an atom. +Contains : protons (+ charge) protons (+ charge) neutrons (neutral charge) neutrons (neutral charge) +The nucleus has an overall positive charge(+). http://www.purchon.com/chemistry/atoms.htm

Electron Cloud (shells) --Found outside of the nucleus. --Made solely of electrons --Has a negative charge(-). http://www.purchon.com/chemistry/atoms.htm

 Located in the nucleus.  Positively (+)charged  subatomic particles.

Electrons Negatively (-) charged subatomic particles. http://www.purchon.com/chemistry/atoms.htm

The number of protons found in an Atom AKA the proton number Helps you locate an element on the periodic table. Atomic Number

12 C 6 ____Protons ____Neutrons _____Electron _____Atomic Mass Try to draw the carbon atom showing the electron levels! Identify the following for each of the elements listed.

35 Cl 17 12 C 6 23 NA 11 ____Protons ____Neutrons _____Electron _____Atomic Mass Identify the following for each of the elements listed.

31 P 15 16 O 8 209 Bi 83 ____Protons ____Neutrons _____Electron _____Atomic Mass

COMPOUNDS Dihydrogen Monoxide Conspiracy??? Dihydrogen Monoxide Conspiracy??? Current allegations suggest that the United States Environmental Protection Agency (EPA) may be conspiring to cover up the whole DHMO issue. Attempts by DHMO researchers to elicit comment from the EPA regarding the possible coverup were either ignored or dodged, leading researchers to infer the alleged cover-up. http://www.circus.com/~no_dhmo/ http://www.dhmo.org/coverup.html

COMPOUNDS A COMBINATION OF DIFFERENT ELEMENTS A COMBINATION OF DIFFERENT ELEMENTS THEY ARE MADE UP OF 2 OR MORE DIFFERENT KINDS OF ATOMS EXAMPLES: CO 2, H 2 O, & C 6 H 12 O 6

Any compound that does not contain the elements carbon and hydrogen is inorganic. Examples: >carbon dioxide >calcium carbonate > water >salts >Phosphates > bases and certain acids Inorganic Compounds

The Electron Shells P=___ N=___ (___e- )

Ions What is an Ion? A positively or negatively charged atom.

Isotope An Isotope is?

in text

Hydrogen atoms only need two electrons in their outer level to reach the noble gas structure of helium. Once again, the covalent bond holds the two atoms together because the pair of electrons is attracted to both nuclei.

in text

Atoms of the same element some-times form covalent bonds with each other. Hydrogen, H 2 Oxygen, O 2 Nitrogen Chlorine Diatomic Molecules

Nonradioactive carbon-12Nonradioactive carbon-13Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 8 neutrons 6 electrons 6 protons 7 neutrons Section 2-1 Figure 2-2 Isotopes of Carbon

Sodium atom (Na)Chlorine atom (Cl)Sodium ion (Na + )Chloride ion (Cl - ) Transfer of electron Protons +11 Electrons -11 Charge 0 Protons +17 Electrons -17 Charge 0 Protons +11 Electrons -10 Charge +1 Protons +17 Electrons -18 Charge -1 Section 2-1 Figure 2-3 Ionic Bonding

Water, Water Everywhere If you have ever seen a photograph of Earth from space, you know that much of the planet is covered by water. Water makes life on Earth possible. If life as we know it exists on some other planet, water must be present to support that life. Section 2-2 Interest Grabber

1. Working with a partner, make a list of ten things that have water in them. 2. Exchange your list for the list of another pair of students. Did your lists contain some of the same things? Did anything on the other list surprise you? 3. Did either list contain any living things? Section 2-2 Interest Grabber continued

2–2 Properties of Water A.The Water Molecule 1.Polarity 2.Hydrogen Bonds B.Solutions and Suspensions 1.Solutions 2.Suspensions C.Acids, Bases, and pH 1.The pH Scale 2.Acids 3.Bases 4.Buffers Section 2-2 Section Outline

Do Now: 1. “Get ready for class” 2. How long can you survive without food and water? HW: Webquest

Do Now: 1. “get ready for class” 2. How long can you survive without food and water? Food 30-40 days Water 5 days

Water is important It makes up 66-75% of your body 75% of Americans are chronically dehydrated. 37% of Americans, the thirst mechanism is so weak that it is often mistaken for hunger. Even MILD dehydration will slow down ones metabolism as much as 5%. Lack of water is the #1 trigger of daytime fatigue. (If you feel tired some morning, try drinking a pint of pure water....) research indicates that 8-10 glasses of water a day could significantly ease back and joint pain for up to 80% of sufferers. A mere 2% drop in body water can trigger fuzzy short memory, trouble with basic math, and difficulty focusing on the computer screen or on a printed page. According to some nutritionists, drinking 5 glasses of water daily decreases the risk of colon cancer by 45%, plus it can slash the risk of breast cancer by 79%, and one is 50% less likely to develop bladder cancer.

A.The Water Molecule 1.Polarity 2.Hydrogen Bonds B.Solutions and Suspensions 1.Solutions 2.Suspensions C.Acids, Bases, and pH 1.The pH Scale 2.Acids 3.Bases 4.Buffers 2–2 Properties of Water

Water Quality

The Importance of Water Properties of Water Composition and polarity Hydrogen bonding properties

Ions in Water

The Importance of Water

Properties of Water Chemical composition of seawater

The Importance of Water The Hydrologic Cycle

The Importance of Water Our Supply of Fresh Water

The Importance of Water Types of water: –surface water –runoff –drainage basin –groundwater –aquifers

Water formation Covalently bonded water has is neutral BUT due polar due to the uneven distribution of electrons between the oxygen and hydrogen atoms. Made of Hydrogen bonds

Hydrogen bonds Hydrogen bonds are an attraction between hydrogen (positively charged due to its small size) and the negative charge on another molecule. Hydrogen bonds are weak. The drawing below shows hydrogen bonds between water molecules..

Why are water molecules attracted to one another? (cohesive)

Salt Water formation In solution, crystals of salt separate and no longer exists as the usual atoms. Salt dissolves in water because the charged portions of the water molecule (H 2 0) have stronger attraction for the ions than they have for each other. Sodium loses the electron to form positive ion, Na+; chlorine gains one to make a negative ion, Cl-.

Cl - Water Cl - Na + Water Na + Figure 2-9 NaCl Solution

Section 2-2 Cl - Water Cl - Na + Water Na + Figure 2-9 NaCl Solution

Salt Water formation The mean electrical charge of a salt solution is zero, because there is one Na+ ion for every Cl- ion. Thus, they balance each other out. += H 2 0 + NaCl = Na+ Cl -

Solutions Solution: ions being gradually dispersed in the water……evenly throughout –Solute: The substance being dissolved –SOLVENT: the substance in which the solute is being dissolved. Ex: water, lipids(oils), Alcohol Suspensions: mixtures of water containing non-dissolved particles –Ex: blood

Copy these two Note cards down! FrontBack H+ HYDROGEN ION If in high concentration, solution is an ACID FrontBack OH- HYDROXIDE ION If in high concentration, solution is a BASE

pH: p H is the ratio of H+ (hydrogen) and OH- (Hydroxide) ions. When both are in equal concentration in pure Acidic SolutionNeutralBasic Solution the water has a pH less then 7. 0-6.5 pHs pH = 7the water has a pH above 7. 7.5-14 an excess of H+ ionsH+ = -OHan excess of OH- ions HCL  H+ Cl-H+ -OH  H20NaOH  Na+ -OH

Oven cleaner Bleach Ammonia solution Soap Sea water Human blood Pure water Milk Normal rainfall Acid rain Tomato juice Lemon juice Stomach acid Neutral Increasingly Basic Increasingly Acidic pH Scale

pH scale Acidity

pH scale alkalinity

Summary: Why are we going to use buffered stones in our aquarium?

MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 Carbon Compounds

Video 1 Click the image to play the video segment. Video 1 Atomic Structure

Video 2 Click the image to play the video segment. Video 2 Energy Levels and Ionic Bonding

Video 3 Click the image to play the video segment. Video 3 Covalent Bonding

Video 4 Click the image to play the video segment. Video 4 Enzymatic Reactions

Oven cleaner Bleach Ammonia solution Soap Sea water Human blood Pure water Milk Normal rainfall Acid rain Tomato juice Lemon juice Stomach acid Neutral Increasingly Basic Increasingly Acidic Section 2-2 pH Scale

Cl - Water Cl - Na + Water Na + Section 2-2 Figure 2-9 NaCI Solution

Section 2-2 Figure 2-9 NaCI Solution Cl - Water Cl - Na + Water Na +

Life’s Backbone Most of the compounds that make up living things contain carbon. In fact, carbon makes up the basic structure, or “backbone,” of these compounds. Each atom of carbon has four electrons in its outer energy level, which makes it possible for each carbon atom to form four bonds with other atoms. As a result, carbon atoms can form long chains. A huge number of different carbon compounds exist. Each compound has a different structure. For example, carbon chains can be straight or branching. Also, other kinds of atoms can be attached to the carbon chain. Section 2-3 Interest Grabber

1. On a sheet of paper, make a list of at least ten things that contain carbon. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. 3. If you know other elements that are in any items on your list, write those elements next to them. Section 2-3 Interest Grabber continued

Carbon Compounds include Examples are which contain CarbohydratesLipidsNucleic acidsProteins Function Examples are Building Blocks

Carbon Compounds include Examples are which contain CarbohydratesLipidsNucleic acidsProteins Sugars and starches Fats and oils DNA, RNAHair, Nails, Muscle, hormones Carbon, hydrogen, oxygen Carbon, hydrogen, oxygen Carbon,hydrogen, oxygen, nitrogen, phosphorus Carbon, hydrogen,oxygen, nitrogen, Function Examples are Main Energy Source backup energy Reproduction/ Regulation Support and Maintenance Building Blocks Glucose Glycerol, 3 fatty acids Nucleotides Amino Acids Monosaccharide's

2–3 Carbon Compounds A.The Chemistry of Carbon B.Macromolecules C.Carbohydrates D.Lipids E.Nucleic Acids F. Proteins

Go to Section: two more Note cards down! FrontBack Organic Compound C-H must be present In All living things C 6 H 12 O 6, CH 3, C 2 H 5 O 2 N FrontBack Inorganic Compound Does not contain both C-H NaCl, H2O, HCl

MethaneAcetyleneButadieneBenzeneIsooctane Section 2-3 Figure 2-11 Carbon Compounds

Organic Compounds Organic Compounds must contain carbon (C) and hydrogen (H) There are four major organic compounds: –Carbohydrates –Lipids –Proteins –Nucleic Acids

Organic Molecules CarbohydratesLipids ProteinsNucleic Acids

Carbohydrates Major energy source Ex. Bread, potato, rice, (ose) Glucose, maltose, lactose Organic compounds composed of carbon, hydrogen, and oxygen (CHO) with a 2 to 1 ratio of hydrogen to oxygen. The three basic types: – Monosaccharides- – Disaccharides - – Polysaccharides-.

Carbohydrates  Monosaccharides  Disaccharides  Polysaccharides What is their Function? Dietary examples? Building blocks Composed of? Made By what process?

Copy this Note card down! FrontBack Glucose C 6 H 12 O 6,

Isomers: Have the same chemical formula but different structural formula. Glucose, Galactose, Ribose, Fructose:::::: are all C 6 H 12 O 6

Monosaccharides simple sugars, monomer least complicated (C 6 H 12 O 6 ) Ex-glucose, galactose, and fructose. 3 Types of Carbohydrates glucose

C O C CH 2 OH C___H___O___

3 types of Carbohydrates polyOMERS. Disaccharides made when two Monosaccharides (C12H22O11) Ex-maltose, sucrose, and lactose.

Disaccharide formation

Starch Glucose Polysaccharide (Starch)

3 types of Carbohydrates polyMERS. Polysaccharides most complex carbohydrates. Plant= starch, cellulose Animal= glycogen. Polysaccharides are large molecules that make up chains of repeating units called polymers. CELLULOSE

What is their Function? Lipids are Backup energy source and insulator Dietary examples? oils, waxes, and fats Building blocks 1 glycerol with 3 fatty acids. Composed of?C_H_O Made By what process? Made by dehydration synthesis. Lipids

FrontBack Glycerol Building block of a LIPID Has an Alcohol functional group C 3 H 5 (OH) 3

FrontBack R Fatty acid Building block of a LIPID Has an ACID functional group Chemical formulas varies …? R: represents a variable

Lipids

Lipids are oils, waxes, and fats Backup energy source and insulator (CHO) Lipids are made up of 1 glycerol with 3 fatty acids. Made by dehydration synthesis.

Polyunsaturated fats are found in vegetable oils such as corn oil, safflower oil, soybean oil, and sunflower oil Saturated fats are usually solid or almost solid at room temperature. All animal fats, such as those in meat, poultry, and dairy products are saturated. Processed and fast foods are also saturated. Monounsaturated fats typically remain liquid at extremely low temperatures. These fats are also found in vegetable oils such as olive oil, peanut oil and canola oil. ) Monounsaturated fat lowers total blood cholesterol by lowering LDL cholesterol without lowering HDL cholesterol.

Lipids Hydrogenated vegetable oil (as in shortening and commercial peanut butters where a solid consistency is sought) started out as “good” unsaturated oil. However, this commercial product has had all the double bonds artificially broken and hydrogens artificially added (in a chemistry lab- type setting) to turn it into saturated fat that bears no resemblance to the original oil from which it came (so it will be solid at room temperature).

What is their Function? MOSTLY STRUCTURAL Countless Functions Dietary examples? Nuts, Meats, fish, poultry (Pigments, hormones, Cells and tissues antibodies, Muscles, ENZYMES) Building blocks AMINO ACIDS 1) Amino group 2) R-variable, re: it varies 3) Carboxylic acid group 4) Central Hydrogen Composed of?C_H_O_N Made By what process? Made by dehydration synthesis. Proteins

FrontBack Name: Amino Acid Are the building blocks of proteins 1) Amino group 2) R-variable, re: it varies 3) Carboxylic acid group 4) Central Hydrogen

Amino Acids 1.Circle the Carboxyl group 2.Square in the Amino Group 3.Triangle in the R-variable group

Proteins

Repair and replace tissue (CHON) Ex. Muscles, hair, your nails, hormones, and enzymes Proteins are made up of amino acids. A protein consists of of one or more polypeptides. Proteins

Amino Acids The building blocks of proteins.

Do Now Copy down the amino acid lysine in your notes. Now Place a: 1)Circle around Amino Group 2)Square around the acid group 3)Triangle around the variable

General structureAlanineSerine Section 2-3 Figure 2-16 Amino Acids Amino groupCarboxyl group

Amino Acids make protein. Acid group Amino group Variable  2 amino acids bonded together can form a protein.  188 amino acids bonded together can form a protein.  Human require 20 essential amino acids to survive.

LIPOPROTEINSLIPOPROTEINS: In the blood, cholesterol attaches to protein molecules of different densities to be carried through the blood vessels by special types of proteins, called lipoproteins. The amounts and types of lipoproteins are an important indicator of your heart disease risk. Low-density lipoprotein, LDL, is commonly termed "bad" cholesterol, because an excess of cholesterol carried by them can lead to the build up of plaque in the arteries. High LDL levels (above 160mg/dl) increase heart disease risk because they keep cholesterol in blood circulation and carry it to the arteries to be deposited. Excess body fat and a diet high in saturated fat tend to increase LDL levels. LDLs are not found in food, only in the body. High-density cholesterol, HDL, is considered "good" or protective cholesterol, because they carry cholesterol away from the arteries to the liver to be excreted from the body. Individuals with high HDL levels (above 35mg/dl) have a lower risk of heart disease. Regular exercise helps to increase HDL levels. HDLs are not found in food, only in the body.

What is their Function? Transfer genetic information examples?DNA, RNA Building blocks Nucleotides Composed of?C_H_O_N_P Made By what process? Made by dehydration synthesis. Nucleic Acids

( CHONP)( CHONP) Ex. DNA and RNA.Ex. DNA and RNA. Nucleic acids are the mostNucleic acids are the most complex of all biological compounds.complex of all biological compounds. They are extremely largeThey are extremely large molecules that may consistmolecules that may consist of hundreds of thousands of atoms.of hundreds of thousands of atoms. DNA and RNA both control heredity.DNA and RNA both control heredity.

Amino acids Section 2-3 Figure 2-17 A Protein

Matter and Energy Have you ever sat around a campfire or watched flames flicker in a fireplace? The burning of wood is a chemical reaction—a process that changes one set of chemicals into another set of chemicals. A chemical reaction always involves changes in chemical bonds that join atoms in compounds. The elements or compounds that enter into a chemical reaction are called reactants. The elements or compounds produced by a chemical reaction are called products. As wood burns, molecules of cellulose are broken down and combine with oxygen to form carbon dioxide and water vapor, and energy is released. Section 2-4 Interest Grabber

1. What are the reactants when wood burns? 2. What are the products when wood burns? 3. What kinds of energy are given off when wood burns? 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Section 2-4 Interest Grabber continued

2–4Chemical Reactions and Enzymes A.Chemical Reactions B.Energy in Reactions 1.Energy Changes 2.Activation Energy C.Enzymes D.Enzyme Action 1.The Enzyme-Substrate Complex 2.Regulation of Enzyme Activity Section 2-4 Section Outline

Reaction pathway without enzyme Activation energy without enzyme Activation energy with enzyme Reaction pathway with enzyme Reactants Products Getting into a Fight Is like a Chemical Reaction

Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Section 2-4 Figure 2-19 Chemical Reactions Getting into a Fight Is like a Chemical Reaction

Enzymes  Enzymes regulate the rate of a chemical reaction.  Enzymes are organic catalysts, substances that affect the rates of chemical reactions but are unchanged by the reactions.  Enzymes are named after the substrates, the substances they act upon.(with an “ase” ending)  An enzyme is a large complex protein  Some enzymes contain a non-protein component called a coenzyme.  3 Factors influence Enzyme action:

Do Now: Why is the way an enzyme works referred to as the “Lock and Key model”?

: Dehydration Synthesis: Building by removing water Lock and Key, ( enzymatic reaction)

: Hydrolysis: Using water and an enzyme to break bonds Lock and Key, ( enzymatic reaction)

Lock and Key, (animation )

The Three Factors that affect Enzyme action are: 1.Temperature 2. Enzyme and Substrate concentrations 3. pH level

Temperature

Enzyme-Substrate Concentration

pH Level

Enzyme Reactions: (Hydrolysis)

General Enzyme Reaction Enzyme looking For another reaction General Enzyme Reaction Enzyme looking For another reaction

Dehydration Hydrolysis Synthesis aka “digestion” Dehydration synthesis is a chemical reaction in which a large molecule is formed from smaller molecules by removing water. Example- 2 glucose combine by dehydration synthesis to create a maltose + H2O. http://faculty.nl.edu/jste/carbohyd.htm Hydrolysis occurs when large molecules are broken into smaller molecules. One or more bonds holding the larger molecule are broken. A molecule of water is added where each bond is broken to form two or more smaller molecules.

Glucose Substrates ATP Substrates bind to enzyme Substrates are converted into products Enzyme-substrate complex Enzyme (hexokinase) ADP Products Glucose-6- phosphate Products are released Section 2-4 Figure 2-21 Enzyme Action Active site

Video Contents Videos Click a hyperlink to choose a video. Atomic Structure Energy Levels and Ionic Bonding Covalent Bonding Enzymatic Reactions

Video 1 Click the image to play the video segment. Video 1 Atomic Structure

Video 2 Click the image to play the video segment. Video 2 Energy Levels and Ionic Bonding

Video 3 Click the image to play the video segment. Video 3 Covalent Bonding

Video 4 Click the image to play the video segment. Video 4 Enzymatic Reactions

Internet Career links on forensic scientists Interactive test Articles on organic chemistry For links on properties of water, go to www.SciLinks.org and enter the Web Code as follows: cbn-1022.www.SciLinks.org For links on enzymes, go to www.SciLinks.org and enter the Web Code as follows: cbn-1024.www.SciLinks.org Go Online

Section 1 Answers 1.Give an example of solid matter. Sample answers: books, desks, chairs 2. Give an example of liquid matter. Sample answers: water, milk 3. Give an example of gaseous matter. Sample answers: air, helium in a balloon 4. Is all matter visible? No 5. Does all matter take up space? Yes Interest Grabber Answers

Section 2 Answers Interest Grabber Answers 1. Working with a partner, make a list of ten things that have water in them. Possible answers: bodies of water, rain and snow, soft drinks and other beverages, juicy foods such as fruits, and so on. 2. Exchange your list for the list of another pair of students. Did your lists contain some of the same things? Did anything on the other list surprise you? Students’ answers will likely be similar, but not exactly alike. 3. Did either list contain any living things? Students’ lists may include plants, animals, or other living things.

Section 3 Answers Interest Grabber Answers 1. On a sheet of paper, make a list of at least ten things that contain carbon. Students will likely know that charcoal and coal contain carbon. They may also list carbohydrates (starches and sugars), oil, gasoline, wood, or carbon dioxide. 2. Working with a partner, review your list. If you think some things on your list contain only carbon, write “only carbon” next to them. Students will say that charcoal and coal contain only carbon. While these materials do contain small amounts of other elements, such as sulfur, they are composed mostly of carbon. 3. If you know other elements that are in any items on your list, write those elements next to them. Students may know that many carbon compounds also contain oxygen and/or hydrogen.

Section 4 Answers Interest Grabber Answers 1.What are the reactants when wood burns? Reactants are oxygen and cellulose. 2. What are the products when wood burns? Products are carbon dioxide and water. 3. What kinds of energy are given off when wood burns? Light and heat are given off. Some students may also mention sound (the crackling of a fire). 4. Wood doesn’t burn all by itself. What must you do to start a fire? What does this mean in terms of energy? To start a fire, you must light it with a match and kindling. You are giving the wood some energy in the form of heat. 5. Once the fire gets started, it keeps burning. Why don’t you need to keep restarting the fire? Once the fire gets going, it gives off enough heat to start more of the wood burning.

End of Custom Shows This slide is intentionally blank.

Go to Section: Isomers: Have the same chemical formula but different structural formula. Glucose, Galactose, Ribose, Fructose:::::: are all C 6 H 12 O 6

What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe.

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What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe.

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Presentation on theme: "What’s the Matter? All of the materials around you are made up of matter. You are made up of matter, as are the chair you sit on and the air you breathe."— Presentation transcript:

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