2

1
Section Outline
Section 2-1

• 21 The 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

2
Matter Anything that has mass and occupies space

• 1 The basic unit of matter is called the atom.

3
Figure 2-2 Isotopes of Carbon
Section 2-1
Nonradioactive carbon-12
Nonradioactive carbon-13
Radioactive carbon-14
6 electrons 6 protons 7 neutrons
6 electrons 6 protons 6 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
4 Atoms are neutral because they contain the
same of electrons protons.
5
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.
6
An Element in the Periodic Table
Section 2-1
6
C
12.011

• 6. 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 !

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

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

• Isotopes are identified by isotopic notation
• Carbon-12, carbon-13, carbon-14 OR
• 12C 13C 14C
• 6 6 6

9
9 Isotopes of the same element have the same
properties because they have the same atomic
number (the same number protons)

• 12C 13C 14C
• 6 6 6

10
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
---filledvalence 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.

11
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 its composed of ions? Because Na
  is a metalan electron donorand Cl is a
  nonmetalan electron acceptor if a metal is
  present to give it an electron.

12
12 Atoms in compounds are held together by
chemical bondseither ionic or covalent.
13
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.
Figure 2-3 Ionic Bonding
Section 2-1
Sodium ion (Na)
Chloride ion (Cl-)
Sodium atom (Na)
Chlorine atom (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
14
13 Covalent bonds form when nonmetal atoms share
electrons to fill their valence octets, linking
atoms because both nuclei attract the shared
electrons.
15
14 Ions are atoms carrying a charge
after losing or gaining valence electrons.
Figure 2-3 Ionic Bonding
Section 2-1
Sodium atom (Na)
Chlorine atom (Cl)
Sodium ion (Na)
Chloride ion (Cl-)
Transfer of electron
Protons 17 Electrons -18 Charge -1
Protons 11 Electrons -11 Charge 0
Protons 11 Electrons -10 Charge 1
Protons 17 Electrons -17 Charge 0
16
15. False. Atom that loses electrons becomes a
positive ion.
17
16 Molecules (Not ionic compounds!) form when
atoms are joined with covalent bonds.
18
17 A is false2 shared electrons is a single
covalent bond

• A
• C

• D covalent bonds are formed when atoms share
  electrons

• b

http//academic.brooklyn.cuny.edu/biology/bio4fv/p
age/covalent_bonds.html
19
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.

http//www.chem.unsw.edu.au/coursenotes/CHEM1/nonu
nipass/HainesIMF/images/dipoledipole.jpg
20
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 students
  report.
• Discuss the water movie labs, and complete the
  2.2 guided reading questions 18 as a class.
• Homework guided reading study workbook
  questions, pages 1516, 921.

21
Section Outline
Section 2-2

• 22
• Properties of Water,
• the strangest and most important molecule on
  earth!

http//www.wsi.nrcs.usda.gov/products/images/wq_dr
op.jpg
22
http//www.sumanasinc.com/webcontent/animations/co
ntent/propertiesofwater/water.html

• 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.

23
Guided reading study workbook for section 2.2,
p 15--161. Water molecules contain 10
electrons, 1 for each H and eight for O. Water
molecules also contain 10 protonsTrue or False.
Water molecules are neutral.

1. True
2. False

24
2. Because water molecules have O at one end and
H at the other, the entire molecule

1. Is positively charged
2. Is negatively charged
3. Is polar, with partial - charges.

25
3. Water is a polar covalent molecule because

1. More electronegative O atoms are bonded to less
   electronegative H atoms
2. O carries a d- charge Hs a d charge
3. The shared electrons of each OH covalent bond
   are more strongly attracted to the O
4. All of the above
5. None of the above

26

• 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 d to d- ) OTHER than
  Hydrogen bonds
• 7th strongest Van der Waals forces (hydrophobic
• interactions of nonpolar compounds)

27
4. Which statement is True?

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

28
cohesion
29
5. Cohesion is

1. Attraction of d and d- atoms of water molecules
   to atoms or ions of other substances, like the
   glass in a graduated cylinder
2. Attraction of d H and d- O of water molecules
   atoms in adjacent water molecules

30
5. Adhesion (exhibited by water adhering to the
spider web) is

1. Attraction of d and d- atoms of water molecules
   to atoms or ions of other substances, like the
   glass in a graduated cylinder
2. Attraction of d H and d- O of water molecules
   atoms in adjacent water molecules

31
6. Water is cohesive (shown by waters forming
droplets) because

1. d H and d- O atoms of water molecules are
   attracted to each other in the same molecule
2. d H and d- O atoms of water molecules are
   attracted to each other in adjacent molecules

32
Surface tension versus capillary action
33
7. The rise of water in a narrow tube (like
water rising in a thermometer) against the force
of gravity is

1. surface tension
2. capillary action
3. specific heat

34
8 In plants capillary action

1. Draws water upwards from the roots into the
   leaves through thin tubes called xylem
2. Pulls sugar downwards from the leaves into the
   roots through thin tubes called phloem

35
10-1-09

• 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

36
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

37
9. True or False. Sucrose (C6H12O6) is a
mixture.

1. True
2. False

38
9. True or False. Sucrose (C6H12O6) dissolved
in water is a mixture.

1. True
2. False

39
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.

40
10. This picture shows bananas mashed up in
water. This mixture is a

1. suspension
2. solution

41
11. Worlds 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)

42
12. A suspension is a

1. Homogeneous mixture
2. Heterogeneous mixture
3. Unstable (particles settle out over time)
4. Stable (a solution whose solutes do not settle
   out)
5. 2 and 3

43
Parts of Solutions

• Solvent more abundantdoes the dissolving
• Solute less abundantgets dissolved

44
13. Two liters water are mixed with 0.3 liters
salt. The water is the

1. solution
2. solute
3. solvent

45
14. Two liters water are mixed with 0.3 liters
salt. The salt is the

1. solution
2. solute
3. solvent

46
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

47
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

48
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)
49
14. Two water molecules can react to form
2H2O(l) ? H3O(aq) OH(aq)

1. Nonpolar compounds
2. Hydronium hydroxide ions

50
15. Water is neutral because it

1. Is polar covalent
2. Forms Hydrogen bonds
3. Has equal numbers of hydronium hydroxide ions
4. Is nonpolar covalent

51
Acids increase the H1 content of water in
aqueous solutions. Bases increase the OH1-

• HCl ? H Cl-
• NaOH? Na1 OH1-

52
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
53
16. The pH scale indicates

1. The acidity of an aqueous solution
2. The basicity of an aqueous solution
3. The concentration of H ions present relative to
   concentration of the OH- ions
4. All of these.

54
17. Which of these aqueous solutions is most
acidic?

1. pH9
2. pH11
3. pH7
4. pH5
5. pH3

55
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
56
18. How many more H ions does a solution with
pH 4 have than one with pH 5?

1. 1X more
2. 10X more
3. 100X more
4. It has 1X less than pH5

57
19. Which statement is false?

1. Acidic solution pH is lt 7
2. Acids add H to solutions
3. Strong acids make solutions whose pH is 11--14
4. Acidic solutions have higher concentrations of H
   than pure water

58
(No Transcript)
59
pH
60
Lifes Backbone
Interest Grabber
Section 2-3

• 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.

61
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.

62
Section Outline
Section 2-3

• 23 Carbon Compounds
• A. The Chemistry of Carbon
• B. Macromolecules
• C. Carbohydrates
• D. Lipids
• E. Nucleic Acids
• F. Proteins

63
Concept Map
Section 2-3
Carbon Compounds
include
that consist of
that consist of
that consist of
that consist of
which contain
which contain
which contain
which contain
64
Figure 2-11 Carbon Compounds
Section 2-3
Methane
Acetylene
Butadiene
Benzene
Isooctane
65
Figure 2-13 A Starch
Section 2-3
Starch
Glucose
66
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Alanine
Serine
67
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Alanine
Serine
68
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Alanine
Serine
69
Figure 2-17 A Protein
Section 2-3
Amino acids
70
Matter and Energy
Interest Grabber
Section 2-4

• Have you ever sat around a campfire or watched
  flames flicker in a fireplace? The burning of
  wood is a chemical reactiona 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.

71
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 doesnt 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 dont you need to keep restarting the fire?

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Section Outline
Section 2-4

• 24 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

73
Effect of Enzymes
Section 2-4
Reaction pathway without enzyme
Activation energy without enzyme
Activation energy with enzyme
Reactants
Reaction pathway with enzyme
Products
74
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Releasing Reaction
Energy-Absorbing Reaction
Activation energy
Products
Activation energy
Reactants
Reactants
Products
75
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Releasing Reaction
Energy-Absorbing Reaction
Activation energy
Products
Activation energy
Reactants
Reactants
Products
76
Figure 2-21 Enzyme Action
Section 2-4
Enzyme (hexokinase)
Glucose
Substrates
ADP
Products
Glucose-6- phosphate
ATP
Products are released
Active site
Substrates bind to enzyme
Enzyme-substrate complex
Substrates are converted into products
77
Figure 2-21 Enzyme Action
Section 2-4
Enzyme (hexokinase)
Glucose
Substrates
ADP
Products
Glucose-6- phosphate
ATP
Products are released
Active site
Substrates bind to enzyme
Enzyme-substrate complex
Substrates are converted into products
78
Figure 2-21 Enzyme Action
Section 2-4
Enzyme (hexokinase)
Glucose
Substrates
ADP
Products
Glucose-6- phosphate
ATP
Products are released
Active site
Substrates bind to enzyme
Enzyme-substrate complex
Substrates are converted into products
79
Figure 2-21 Enzyme Action
Section 2-4
Enzyme (hexokinase)
Glucose
Substrates
ADP
Products
Glucose-6- phosphate
ATP
Products are released
Active site
Substrates bind to enzyme
Enzyme-substrate complex
Substrates are converted into products
80
Video Contents
Videos

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

81
Video 1
Video 1
Atomic Structure

• Click the image to play the video segment.

82
Video 2
Video 2
Energy Levels and Ionic Bonding
Click the image to play the video segment.
83
Video 3
Video 3
Covalent Bonding
Click the image to play the video segment.
84
Video 4
Video 4
Enzymatic Reactions
Click the image to play the video segment.
85
Internet
Go Online

• 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.
• For links on enzymes, go to www.SciLinks.org and
  enter the Web Code as follows cbn-1024.

86
Section 1 Answers
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

87
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.

88
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.

89
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
doesnt 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 dont you
need to keep restarting the fire? Once the fire
gets going, it gives off enough heat to start
more of the wood burning.
90
End of Custom Shows

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