2–1 The Nature of Matter Section Outline A. Atoms

2–1 The Nature of Matter Section Outline 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

Matter –Anything that has mass and occupies space
1 The basic unit of matter is called the atom.

2, 3 Atomic Nuclei contain protons and neutrons.
Figure 2-2 Isotopes of Carbon Section 2-1 Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons 2, 3 Atomic Nuclei contain protons and neutrons. Protons 1+ charge size 1 amu nucleus Neutrons 0 charge size 1 amu in nucleus Electrons 1- charge size 1/1840 amu in electron cloud

4 Atoms are neutral because they contain the same # of electrons & protons.

5 Chemical elements are groups of atoms having the same atomic number, that is, atoms having the same number protons. These are all atoms of Carbon. All have atomic # 6.

C 6 12.011 6. Proton # = 6 : shown by the atomic number
An Element in the Periodic Table Section 2-1 6 C 12.011 Proton # = 6 : shown by the atomic number Also, C atoms have 6 electrons: Since atoms are neutral, if you know proton #, you also know electron #!

Figure 2-2 Isotopes of Carbon
Section 2-1 Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons 7 Isotopes are forms of the same element that have the same number of protons but a different number of neutrons.

Isotopes are identified by isotopic notation:
Figure 2-2 Isotopes of Carbon Section 2-1 Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14 6 electrons 6 protons 6 neutrons 6 electrons 6 protons 7 neutrons 6 electrons 6 protons 8 neutrons Isotopes are identified by isotopic notation: Carbon-12, carbon-13, carbon-14 OR 12C 13C 14C

9 Isotopes of the same element have the same properties because they have the same atomic number (the same number protons) 12C 13C 14C

10 Chemical compounds are groups of atoms held together by chemical bonds. Chemical compounds are more stable than individual atoms (except for noble gas atoms which have stable ---filled—valence electron shells. Chemical compounds allow atoms to obey the “octet rule”. (2 electrons in the outer electron shell in H and He, but 8 for other elements.

NaCl one Na ion bonded to one Cl ion
11 Chemical formulas show the numbers of different kinds of atoms bonded together in a single formula unit of a compound NaCl one Na ion bonded to one Cl ion Why do we know it’s composed of ions? Because Na is a metal—an electron donor—and Cl is a nonmetal—an electron acceptor if a metal is present to give it an electron.

12 Atoms in compounds are held together by chemical bonds—either ionic or covalent.

Figure 2-3 Ionic Bonding Section 2-1 13 Ionic bonds: attraction of negative ions to positive ions because a metal donates its electrons to a nonmetal atom, forming stable ions with complete valence shell octets. Sodium ion (Na+) Chloride ion (Cl-) Sodium atom (Na) Chlorine atom (Cl) Transfer of electron Protons +11 Electrons -11 Charge Protons +17 Electrons -17 Charge Protons +11 Electrons -10 Charge Protons +17 Electrons -18 Charge

13 Covalent bonds form when nonmetal atoms share electrons to fill their valence octets, linking atoms because both nuclei attract the shared electrons.

Figure 2-3 Ionic Bonding Section 2-1 14 Ions are atoms carrying a charge after losing or gaining valence electrons. Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na+) Chloride ion (Cl-) Transfer of electron Protons +17 Electrons -18 Charge Protons +11 Electrons -11 Charge Protons +11 Electrons -10 Charge Protons +17 Electrons -17 Charge

15. False. Atom that loses electrons becomes a positive ion.

16 Molecules (Not ionic compounds
16 Molecules (Not ionic compounds!) form when atoms are joined with covalent bonds.

17 A is false—2 shared electrons is a single covalent bond
D covalent bonds are formed when atoms share electrons b

18 Van Der Waals forces and dipole-dipole interactions hold atoms of nearby molecules together.
Occasionally, valence electrons are nearer one atom than the other in a covalent bond, creating areas partial charge.

Lesson 3: Chapter 2 The chemistry of Life
Watch movie on water, then answer questions on the worksheet together in your lab group BEFORE beginning the lab. Teacher will select one worksheet for grading, by random drawing. Complete water lab, then turn in one copy per lab group . Teacher will select one student’s report. Discuss the water movie & labs, and complete the 2.2 guided reading questions 1—8 as a class. Homework: guided reading & study workbook questions, pages 15—16, #9—21.

the strangest and most important molecule on earth!
Section Outline Section 2-2 2–2 Properties of Water, the strangest and most important molecule on earth!

Watch this movie from beginning to end.
Watch this movie from beginning to end. Then, the teacher will advance the movie one question at a time, giving time for you to write the answers to each question.

Guided reading & study workbook for section 2. 2, p 15--16 1
Guided reading & study workbook for section 2.2, p Water molecules contain 10 electrons, 1 for each H and eight for O. Water molecules also contain 10 protons True or False. Water molecules are neutral. True False

Is polar, with partial + & - charges.
2. Because water molecules have O at one end and H at the other, the entire molecule: Is positively charged Is negatively charged Is polar, with partial + & - charges.

3. Water is a polar covalent molecule because:
More electronegative O atoms are bonded to less electronegative H atoms O carries a δ- charge & H’s a δ+ charge The shared electrons of each O—H covalent bond are more strongly attracted to the O All of the above None of the above

Strongest triple covalent bond
2nd strongest double covalent bond 3rd strongest single covalent bond 4th strongest ionic bond 5th strongest Hydrogen bonds 6th strongest Dipole dipole interactions (polar molecules attracted δ+ to δ- ) OTHER than Hydrogen bonds 7th strongest Van der Waals forces (hydrophobic interactions of nonpolar compounds)

4. Which statement is True?
Hydrogen bonds are stronger than ionic bonds. Attraction of the H in one water molecule to O in another is a Hydrogen bond Hydrogen bonds are stronger than covalent bonds Hydrogen bonds are the strongest bonds BETWEEN different neutral molecules. Choices 2 and 5 are true

cohesion

5. Cohesion is: Attraction of δ+ and δ- atoms of water molecules to atoms or ions of other substances, like the glass in a graduated cylinder Attraction of δ+ H and δ- O of water molecules atoms in adjacent water molecules

5. Adhesion (exhibited by water adhering to the spider web) is:
Attraction of δ+ and δ- atoms of water molecules to atoms or ions of other substances, like the glass in a graduated cylinder Attraction of δ+ H and δ- O of water molecules atoms in adjacent water molecules

6. Water is cohesive (shown by water’s forming droplets) because:
δ+ H and δ- O atoms of water molecules are attracted to each other in the same molecule δ+ H and δ- O atoms of water molecules are attracted to each other in adjacent molecules

Surface tension versus capillary action

7. The rise of water in a narrow tube (like water rising in a thermometer) against the force of gravity is: surface tension capillary action specific heat

8 In plants capillary action:
Draws water upwards from the roots into the leaves through thin tubes called xylem Pulls sugar downwards from the leaves into the roots through thin tubes called phloem

Lesson on solutions and suspensions with homework correction slides Lesson on acids and bases Complete water labs & questions & acid/base questions. Tear off lab & questions through end page. Put rest back in notebooks. Homework: prep for a quiz on ch 2.1,2.2, tomorrow

Mixture: 2 or more substances combined but not chemically bonded
Mixture: 2 or more substances combined but not chemically bonded. They can be separated without another chemical reaction (a physical separation). e.g., sand and water can be separated with a filter inks in markers can be separated with chromatography Salt can be removed from water by evaporating the water

9. True or False. Sucrose (C6H12O6) is a mixture.

9. True or False. Sucrose (C6H12O6) dissolved in water is a mixture.

Mixtures may be heterogenous (nonuniform throughout) or homogenous (uniform throughout)
Another name for a homogeneous mixture is solution. Another name for a heterogeneous mixture is suspension.

10. This picture shows bananas mashed up in water. This mixture is a
suspension solution

11. World’s greatest solvent: water!
Water is known as the universal solvent because it can dissolve ionic compounds and polar covalent compounds. Ionic and polar covalent compounds are hydrophillic (water loving) Water can not dissolve nonpolar covalent compounds. Nonpolar compounds are hydrophobic (water hating)

12. A suspension is a: Homogeneous mixture Heterogeneous mixture
Unstable (particles settle out over time) Stable (a solution whose solutes do not settle out) 2 and 3

Parts of Solutions: Solvent: more abundant—does the dissolving
Solute: less abundant—gets dissolved

13. Two liters water are mixed with 0.3 liters salt. The water is the
solution solute solvent

14. Two liters water are mixed with 0.3 liters salt. The salt is the
solution solute solvent

concentration Molarity (M) = # moles solute/#L solution 3 Moles/0.5 L = 6 M 1 mole NaCl = 58.4 g 29.2 g/0.25 L = 0.5 moles/0.25 L= 2M

Aqueous solutions can be neutral, acidic, or basic.
These descriptions depend refer to the behavior of the solute when it is dissolved in water and to how this behavior alters the molar concentrations of these two ions in the aqueous solution: H+ protons OH1- hydroxide ions

1 out of over 500 million water molecules dissociates to H+ hydronium, OH- hydroxide
Neutral aqueous solutions and pure water contain equal numbers of both ions. 2H2O(l) → H3O+(aq) + OH–(aq)

14. Two water molecules can react to form:
2H2O(l) → H3O+(aq) + OH–(aq) Nonpolar compounds Hydronium & hydroxide ions

15. Water is neutral because it:
Is polar covalent Forms Hydrogen bonds Has equal numbers of hydronium & hydroxide ions Is nonpolar covalent

Acids increase the H1+ content of water in aqueous solutions
Acids increase the H1+ content of water in aqueous solutions. Bases increase the OH1- HCl  H+ + Cl- NaOH Na1+ + OH1-

pH Scale Section 2-2 The more H+ ions, the more acidic, the lower pH. The more OH1- ions, the more basic, the higher pH. Oven cleaner pH measures whether either H+ ions are greater (acidic) or the OH1- ions are greater (basic) Bleach Ammonia solution Increasingly Basic Soap Sea water Human blood Neutral Pure water Milk Normal rainfall Acid rain Increasingly Acidic Tomato juice Lemon juice Stomach acid

16. The pH scale indicates:
The acidity of an aqueous solution The basicity of an aqueous solution The concentration of H+ ions present relative to concentration of the OH- ions All of these.

17. Which of these aqueous solutions is most acidic?
pH9 pH11 pH7 pH5 pH3

pH 7 has 10 times less H+ than pH6 and 100 times less than pH5
pH Scale Section 2-2 pH 7 has 10 times less H+ than pH6 and 100 times less than pH5 Oven cleaner The pH scale is logarithmic. So, pH 0 has 10 times more H+ than pH1 and 100 times more than pH2. Bleach Ammonia solution Increasingly Basic Soap Sea water Human blood Neutral Pure water Milk Normal rainfall Acid rain Increasingly Acidic Tomato juice Lemon juice Stomach acid

18. How many more H+ ions does a solution with pH 4 have than one with pH 5?
1X more 10X more 100X more It has 1X less than pH5

19. Which statement is false?
Acidic solution pH is < 7 Acids add H+ to solutions Strong acids make solutions whose pH is Acidic solutions have higher concentrations of H+ than pure water

Life’s Backbone Interest Grabber
Section 2-3 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.

Interest Grabber continued
Section 2-3 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.

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

Concept Map Carbon Compounds Carbohydrates Lipids Nucleic acids
Section 2-3 Carbon Compounds include Carbohydrates Lipids Nucleic acids Proteins that consist of that consist of that consist of that consist of Sugars and starches Fats and oils Nucleotides Amino Acids which contain which contain which contain which contain Carbon, hydrogen, oxygen Carbon,hydrogen, oxygen, nitrogen, phosphorus hydrogen,oxygen, nitrogen,

Figure 2-11 Carbon Compounds
Section 2-3 Methane Acetylene Butadiene Benzene Isooctane

Figure 2-13 A Starch Section 2-3 Starch Glucose

Figure 2-16 Amino Acids General structure Alanine Serine Section 2-3
Amino group Carboxyl group General structure Alanine Serine

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

Interest Grabber Section 2-4 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.

Interest Grabber continued
Section 2-4 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?

2–4 Chemical Reactions and Enzymes
Section Outline Section 2-4 2–4 Chemical 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

Effect of Enzymes Reaction pathway without enzyme Activation energy
Section 2-4 Reaction pathway without enzyme Activation energy without enzyme Reactants Activation energy with enzyme Reaction pathway with enzyme Products

Figure 2-19 Chemical Reactions
Section 2-4 Energy-Absorbing Reaction Energy-Releasing Reaction Products Activation energy Activation energy Reactants Reactants Products

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

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

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

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

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

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

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

Interest Grabber 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 Section 1 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 2 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 3 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. Section 4 Answers

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2–1 The Nature of Matter Section Outline A. Atoms

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