Download Prentice Hall Biology - Mayfield City Schools

Section Outline
Section 2-1
•
2–1 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
Go to
Section:
Matter –Anything that has mass and occupies
space
•1 The basic unit of matter is called the atom.
Go to
Section:
Figure 2-2 Isotopes of Carbon
Section 2-1
Nonradioactive carbon-12
6 electrons
6 protons
6 neutrons
Nonradioactive carbon-13
6 electrons
6 protons
7 neutrons
Radioactive carbon-14
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
Go to
Section:
4 Atoms are neutral because they contain the same #
of electrons & protons.
Go to
Section:
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.
Go to
Section:
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 #!
Go to
Section:
Figure 2-2 Isotopes of Carbon
Section 2-1
Nonradioactive carbon-12
6 electrons
6 protons
6 neutrons
Nonradioactive carbon-13
6 electrons
6 protons
7 neutrons
Radioactive carbon-14
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.
Go to
Section:
Figure 2-2 Isotopes of Carbon
Section 2-1
Nonradioactive carbon-12
6 electrons
6 protons
6 neutrons
Nonradioactive carbon-13
6 electrons
6 protons
7 neutrons
Radioactive carbon-14
6 electrons
6 protons
8 neutrons
8 Isotopes are identified by isotopic notation:
• Carbon-12, carbon-13, carbon-14 OR
13C
14C
• 12C
6
6
• 6
Go to
Section:
9 Isotopes of the same element have the same
properties because they have the same atomic
number (the same number protons)
•
•
Go to
Section:
12
C
6
13
C
6
14
C
6
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.
Go to
Section:
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.
Go to
Section:
12 Atoms in compounds are held together by
chemical bonds—either ionic or covalent.
Go to
Section:
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
Chloride ion (Cl-)
ions with complete valence shell octets. Sodium ion (Na+)
Sodium atom (Na)
Chlorine atom (Cl)
Transfer
of electron
Protons +11
Electrons -11
Charge
0
Go to
Section:
Protons +17
Electrons -17
Charge
0
Protons +11
Electrons -10
Charge
+1
Protons +17
Electrons -18
Charge
-1
13 Covalent bonds form when nonmetal atoms share electrons to fill
their valence octets, linking atoms because both nuclei attract the
shared electrons
Go to
Section:
.
Figure 2-3 Ionic Bonding
Section 2-1
14
Sodium atom (Na)
Ions are atoms carrying a charge after losing
or gaining valence electrons.+
Chlorine atom (Cl)
Sodium ion (Na )
Chloride ion (Cl-)
Transfer
of electron
Protons +11
Electrons -11
Charge
0
Go to
Section:
Protons +17
Electrons -17
Charge
0
Protons +11
Electrons -10
Charge
+1
Protons +17
Electrons -18
Charge
-1
15. False. Atom that loses electrons becomes a
positive ion.
Go to
Section:
16 Molecules (Not ionic compounds!) form
when atoms are joined with covalent bonds.
Go to
Section:
17 A is false—2 shared electrons is
a single covalent bond
b
A
•D covalent bonds are formed
when atoms share electrons
C
http://academic.brooklyn.cuny.edu/biology/bio4fv/page/covalent_bonds.html
Go to
Section:
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/nonunipass/Haine
sIMF/images/dipoledipole.jpg
Go to
Section:
Lesson 3: Chapter 2 The chemistry of Life
1. 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.
2. Complete water lab, then turn in one copy per lab group
. Teacher will select one student’s report.
3. 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.
Go to
Section:
Section Outline
Section 2-2
Go to
Section:
•
•
2–2
Properties of Water,
•
the strangest and most
important molecule on
earth!
http://www.wsi.nrcs.usda.gov/products/i
mages/wq_drop.jpg
http://www.sumanasinc.com/webcontent/ani
mations/content/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.
Go to
Section:
Guided reading & study workbook for section 2.2, p 15--16
1. 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.
1.True
2.False
Go to
Section:
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.
Go to
Section:
3. Water is a polar covalent molecule because:
1.More electronegative O atoms are bonded to
less electronegative H atoms
2.O carries a δ- charge & H’s a δ+ charge
3.The shared electrons of each O—H covalent
bond are more strongly attracted to the O
4.All of the above
5.None of the above
Go to
Section:
•
•
•
•
•
•
Strongest
2nd strongest
3rd strongest
4th strongest
5th strongest
6th strongest
• 7th strongest
•
Go to
Section:
triple covalent bond
double covalent bond
single covalent bond
ionic bond
Hydrogen bonds
Dipole dipole interactions (polar
molecules attracted δ+ to δ- )
OTHER than Hydrogen bonds
Van der Waals forces (hydrophobic
interactions of nonpolar compounds)
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
Go to
Section:
cohesion
Go to
Section:
5. Cohesion is:
1.Attraction of δ+ and δ- atoms of
water molecules to atoms or
ions of other substances, like
the glass in a graduated
cylinder
2.Attraction of δ+ H and δ- O of
water molecules atoms in
adjacent water molecules
Go to
Section:
5. Adhesion (exhibited by water
adhering to the spider web) is:
1.Attraction of δ+ and δ- atoms of
water molecules to atoms or
ions of other substances, like
the glass in a graduated
cylinder
2.Attraction of δ+ H and δ- O of
water molecules atoms in
adjacent water molecules
Go to
Section:
6. Water is cohesive (shown by water’s forming
droplets) because:
1.δ+ H and δ- O atoms of water
molecules are attracted to each
other in the same molecule
2.δ+ H and δ- O atoms of water
molecules are attracted to each
other in adjacent molecules
Go to
Section:
Surface tension versus capillary action
Go to
Section:
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
Go to
Section:
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
Go to
Section:
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
Go to
Section:
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
Go to
Section:
9. True or False. Sucrose
(C6H12O6) is a mixture.
se
50%
Fa
l
Go to
Section:
Tr
ue
1. True
2. False
50%
9. True or False. Sucrose (C6H12O6)
dissolved in water is a mixture.
se
50%
Fa
l
Go to
Section:
Tr
ue
1. True
2. False
50%
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.
Go to
Section:
10. This picture shows bananas
mashed up in water. This mixture is a
50%
50%
Go to
Section:
ut
io
n
so
l
su
sp
e
ns
io
n
1.suspension
2.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)
Go to
Section:
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
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Section:
20% 20% 20% 20% 20%
Parts of Solutions:
Solvent: more abundant—does the dissolving
Solute: less abundant—gets dissolved
Go to
Section:
13. Two liters water are mixed with 0.3 liters salt.
The water is the
1. solution
2. solute
3. solvent
Go to
Section:
ve
n
t
33%
so
l
ut
e
33%
so
l
so
l
ut
io
n
33%
14. Two liters water are mixed with 0.3 liters salt.
The salt is the
1. solution
2. solute
3. solvent
Go to
Section:
ve
n
t
33%
so
l
ut
e
33%
so
l
so
l
ut
io
n
33%
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
Go to
Section:
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
Go to
Section:
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)
Go to
Section:
14. Two water molecules can react to form:
2H2O(l) → H3O+(aq) + OH–(aq)
50%
50%
hy
...
&
um
on
i
Hy
dr
Go to
Section:
No
np
o
lar
co
m
po
.. .
1. Nonpolar
compounds
2. Hydronium &
hydroxide ions
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
ar
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Is
no
n
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eq
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um
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co
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po
l
Go to
Section:
Fo
rm
sH
yd
ro
va
l
...
25% 25% 25% 25%
Acids increase the H1+ content of water in
aqueous solutions. Bases increase the OH1HCl  H+ + ClNaOH Na1+ + OH1-
Go to
Section:
pH Scale
Section 2-2
Go to
Section:
Neutral
Increasingly Acidic
pH measures
whether either
H+ ions are
greater (acidic)
or the OH1ions are greater
(basic)
Increasingly Basic
Oven cleaner
Bleach
Ammonia solution
Soap
Sea water
Human blood
Pure water
Milk
Normal
rainfall
Acid rain
Tomato
juice
Lemon juice
Stomach acid
The more H+
ions, the
more acidic,
the lower pH.
The more OH1ions, the
more basic,
the higher pH.
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.
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Go to
Section:
25% 25% 25% 25%
17. Which of these aqueous solutions is most
20% 20% 20% 20% 20%
acidic?
pH
3
pH
5
pH
7
Go to
Section:
pH
11
pH9
pH11
pH7
pH5
pH3
pH
9
1.
2.
3.
4.
5.
pH Scale
Section 2-2
So, pH 0 has 10
times more H+
than pH1 and
100 times more
than pH2.
Go to
Section:
Neutral
Increasingly Acidic
The pH scale is
logarithmic.
Increasingly Basic
Oven cleaner
Bleach
Ammonia solution
Soap
Sea water
Human blood
Pure water
Milk
Normal
rainfall
Acid rain
Tomato
juice
Lemon juice
Stomach acid
pH 7 has 10
times less H+
than pH6 and
100 times less
than pH5
18. How many more H+ ions does a solution
with pH 4 have than one with pH 5?
25%
ss
...
It
h
as
1X
le
m
or
e
10
X
m
or
or
m
Go to
Section:
25%
e
25%
e
25%
10
0X
1X more
10X more
100X more
It has 1X less than
pH5
1X
1.
2.
3.
4.
19. Which statement is false?
1. Acidic solution pH is < 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
ha
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sa
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so
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Ac
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Go to
Section:
ut
io
n
pH
is
ut
io
ns
<7
25% 25% 25% 25%
Go to
Section:
pH
Go to
Section:
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.
Go to
Section:
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.
Go to
Section:
Section Outline
Section 2-3
•
2–3 Carbon
Compounds
A.
B.
C.
D.
E.
F.
Go to
Section:
The Chemistry of Carbon
Macromolecules
Carbohydrates
Lipids
Nucleic Acids
Proteins
Concept Map
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
Carbon,
hydrogen,
oxygen
Go to
Section:
Carbon,
hydrogen,
oxygen
which contain
which contain
Carbon,hydrogen,
oxygen, nitrogen,
phosphorus
Carbon,
hydrogen,oxygen,
nitrogen,
Figure 2-11 Carbon Compounds
Section 2-3
Methane
Go to
Section:
Acetylene
Butadiene
Benzene
Isooctane
Figure 2-13 A Starch
Section 2-3
Starch
Glucose
Go to
Section:
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Go to
Section:
Alanine
Serine
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Go to
Section:
Alanine
Serine
Figure 2-16 Amino Acids
Section 2-3
Amino group
Carboxyl group
General structure
Go to
Section:
Alanine
Serine
Figure 2-17 A Protein
Section 2-3
Amino
acids
Go to
Section:
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.
Go to
Section:
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?
Go to
Section:
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
Go to
Section:
Effect of Enzymes
Section 2-4
Reaction pathway
without enzyme
Activation energy
without enzyme
Reactants
Reaction pathway
with enzyme
Activation
energy
with enzyme
Products
Go to
Section:
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Absorbing Reaction
Energy-Releasing Reaction
Activation
energy
Products
Activation energy
Reactants
Reactants
Products
Go to
Section:
Figure 2-19 Chemical Reactions
Section 2-4
Energy-Absorbing Reaction
Energy-Releasing Reaction
Activation
energy
Products
Activation energy
Reactants
Reactants
Products
Go to
Section:
Figure 2-21 Enzyme Action
Section 2-4
Enzyme
(hexokinase)
Glucose
Substrates
Products
ADP
Glucose-6phosphate
Products
are released
ATP
Active site
Enzyme-substrate
complex
Substrates
are converted
into products
Go to
Section:
Substrates
bind to
enzyme
Figure 2-21 Enzyme Action
Section 2-4
Enzyme
(hexokinase)
Glucose
Substrates
Products
ADP
Glucose-6phosphate
Products
are released
ATP
Active site
Enzyme-substrate
complex
Substrates
are converted
into products
Go to
Section:
Substrates
bind to
enzyme
Figure 2-21 Enzyme Action
Section 2-4
Enzyme
(hexokinase)
Glucose
Substrates
Products
ADP
Glucose-6phosphate
Products
are released
ATP
Active site
Enzyme-substrate
complex
Substrates
are converted
into products
Go to
Section:
Substrates
bind to
enzyme
Figure 2-21 Enzyme Action
Section 2-4
Enzyme
(hexokinase)
Glucose
Substrates
Products
ADP
Glucose-6phosphate
Products
are released
ATP
Active site
Enzyme-substrate
complex
Substrates
are converted
into products
Go to
Section:
Substrates
bind to
enzyme
Videos
• Click a hyperlink to choose a video.
•
Atomic Structure
•
Energy Levels and Ionic Bonding
•
Covalent Bonding
•
Enzymatic Reactions
Video 1
Atomic Structure
•Click the image to play the video segment.
Video 2
Energy Levels and Ionic Bonding
Click the image to play the video segment.
Video 3
Covalent Bonding
Click the image to play the video segment.
Video 4
Enzymatic Reactions
Click the image to play the video segment.
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.
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
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.
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.
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.
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