Chapter 6 Notes The Chemistry of Life

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Chapter 6 NotesThe Chemistry of Life

• Section 6.1 Atoms and Their Interactions

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Take 5

• ____________ is the condition that results from
  changes in the independent variable.
• __________ results in an increase in the amount
  of living material and the formation of new
  structures.

3
Take 5

• An atom of Fluorine has nine electrons. Its
  second energy level has ________ electrons.
• How many electrons can a carbon atom share?
• What kind of bond is formed when two atoms share
  electrons, such as with hydrogen and oxygen in
  water?

4
Take 5

• Water dissolves many ionic and molecular
  compounds because of its __________.
• Show the bond between magnesium and Sulfur.
• Name two types of carbohydrates.

5
Take 5

• What are the two components of a lipid?
• What are the 3 components of a nucleotide?
• What do nucleotides make up? Give 2 examples.

6
Take 5

• Draw Neon and show the energy levels.
• Show me a covalent bond between two carbon atoms.
• Show me an ionic bond between NaCl

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I. Elements

• Natural elements in living things
• Element _________________________
• ________________________________
• Four elements make up ______ of the mass of the
  human body _________________
• Look at page 142, Table 6.1. It shows some common
  elements along with their symbols, found in the
  human body.

A substance that cant be broken down into
simpler chemical substances.
9 6
C, H, O , N
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Elements in the Human Body
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I. Elements

• Trace Elements
• ______________________________
• ________________________________
• (Table 6.1)

Elements that play a vital role in maintaining
healthy cells, but are needed in very small
amounts
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II. Atoms The Building Blocks of Elements

• Atom the smallest particle of an __________ that
  has the characteristics of that element.
• The structure of an atom
• The center of an atom is the ___________.
• The nucleus is made up of _________ (p) which
  are positively charged and __________ (n) which
  are neutral or have no charge.

Element
Nucleus
Protons
Neutrons
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II. Atoms The Building Blocks of Elements

• 3. Elements are arranged on the Periodic table
  according to the number of ________ they
  naturally have. This number is called the
  __________ ____________.
• 4. The region of space surrounding the nucleus
  contains extremely small, negatively charged
  particles called __________ (e-). This region is
  also known as the __________ ___________.

Protons
Atomic Number
Electrons
Electron Cloud
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? Atomic Number for Carbon Therefore,
there are 6 protons in the nucleus.
6
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How many Protons are in the following Elements???
Helium Calcium
Neon

He 2
Ca 20
Ne 10
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II. Atoms The Building Blocks of Elements

• Electron energy levels (pg. 143, fig 6.2)
• 1. Within the electron cloud, there are energy
  levels which the electrons move in.

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E1 2 electrons E2 8 electrons E3 18
electrons E4 32 electrons
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Draw the energy levels of each atom
Nitrogen
Iron (Fe)
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III. Isotopes of an Element

• Isotope atoms of the same element that have the
  same number of ________, but a different number
  of ___________.
• Scientists refer to isotopes by stating the
  combing total of ___________ and __________ in
  the nucleus.
• For example Carbon-12 (naturally occurring
  element)
• Carbon-14 (contains 2
  more neutrons)
• - The nucleus is ___________ and tens to break
  apart and give off ______________.

protons
Neutrons
protons
Neutrons
unstable
radiation
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IV. Compounds and Bonding

• Compound a substance that is composed of
  ________ of two or more __________ elements that
  are chemically combined. Ex NaCl _______
• How and why do elements combine?
  _______________________________
• ________________________________
• For many elements, an atom becomes ________ when
  its outermost energy
• level is __________.

atoms
different
Sodium Chloride
Atoms combine with each other only when the
resulting compound is more stable than the
individual atoms.
stable
full
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IV. Compounds and Bonding

• How covalent bonds form
• Covalent Bond _____________________
• The electrons being shared ____________ around
  both elements holding them ___________ together
• A ________________ is a group of atoms held
  together by covalent bonds. Ex ____________
  (_______)

The force between two atoms that share electrons
move
close
molecule
H2 O
water
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IV. Compounds and Bonding

• Examples of covalent bonds
• a. Two hydrogen atoms

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IV. Compounds and Bonding

• b. Two Carbon Atoms

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IV. Compounds and Bonding

• How ionic form
• Ionic bond _______________________
• ___________________________________
• Ion ____________________________
• These bonds are ________ abundant in living
  things than covalent molecules, but ions are
  important in _________ processes
• Examples of ionic bonds

The attractive
force between two ions of opposite charge
A charged atom that gained or lost electrons
less
biological
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IV. Compounds and Bonding

• A. Table salt NaCl
• B. MgS

Na 11 Cl 17
Mg 12 S 16
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V. Chemical Reactions

• Chemical reactions occur when ______ are formed
  or broken, causing substances to __________ into
  different substances.
• All the chemical reactions that occur within an
  organism are referred to as that organisms
  ________________.
• Writing chemical equations
• Basic Setup
• _________ ?_________ NaCl ? NaCl

bonds
recombine
metabolism
Reactants
Products
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V. Chemical Reactions

• 2. In chemical reactions, it is important to
  understand that atoms are neither _________ nor
  __________, they are simply rearranged.

created
destroyed
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VI. Mixtures and Solutions

• Mixture a combination of substances in which
  the __________ components retain their own
  __________. Ex _____________________
  ____
• Solution a mixture in which one or more
  _________ (solutes) are distributed _________ in
  another substance (solvent). In other words, one
  substance is __________ in another and will not
  settle out of solution.
• Ex _____________________________

individual
properties
Mixing sand and sugar, salt and pepper
substances
evenly
dissolved
Sugar and water, food coloring and water
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VI. Mixtures and Solutions

• Acids and Bases
• Chemical reactions can only occur when conditions
  are __________. One condition that is very
  important is the ____ of the solution.
• The pH is a measure of how _________ or _________
  a solution is.
• Look on page 150, fig 6.11 for the pH scale
  ____________ is acidic, ________ is neutral,
  ________ is basic.
• An acid is any substance that forms hydrogen ions
  (H) in water. EX _________________

right
pH
acidic
basic
0 to 6
7
8-14
HCl ? (H) (Cl-)
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VI. Mixtures and Solutions

• 5. A base is any substance that forms
  hydroxide ions (OH-) in water
• EX ___________________________
• 6. If the hydrogen ions equal the hydroxide
  ions the solution is neutral and the pH of 7.
• 7. So
• If H gt OH- then solution is acidic
• If H lt OH- then solution is basic
• If H OH- then solution is neutral

NaOH ? (Na) (OH-)
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pH of common substances
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Concentration of H ions
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Section 6.2

• Water

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I. Water and Its Importance

• Water is polar
• Polar Molecule ____________________
• __________________________________.
• These molecules have a __________ end and a
  ______________.
• Polar molecules attract other __________
  molecules as well as _________ ________
• Look at page 153, fig 6.12. Water is a polar
  molecule.

A molecule with
unequal distribution of charge
Positive
negative
polar
Charged ions
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I. Water and Its Importance

• When two water molecules come in close contact,
  the negative ___________ end is attracted to the
  other water molecules positive ___________ end.
  This attractions of opposite charges forms a
  ________ bond called a ____________.
• Because of waters polarity, it..
• Is the ____________ ____________
• Can move up plants by ________ ________

oxygen
hydrogen
weak
Hydrogen bond
Universal solvent
Capillary action
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Water is a universal solvent!!!!!
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I. Water and Its Importance

• Water resists temperature changes
• Water requires ______ heat to increase its
  temperature than other liquids. Why?
  __________________________________________________
  __________________
• When water cools, it gives _____ a lot of
  ___________.
• Because water takes longer to heat up and cool
  down, it is like an _______ that helps maintain a
  __________ environment when conditions fluctuate
  outside and within our own ______________.

more
Because of the hydrogen bonds between each
molecule. As you heat up water, the bonds must
be broken to move around.
off
heat
insulator
steady
Bodies/cells
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I. Water and Its Importance

• Water expands expends when it freezes
• - As water begins to _________ more and more
  _____________bonds are formed and the water
  molecules become more ________ apart. When this
  happens as a piece of ice forms, it becomes
  ________ ________ than the surrounding liquid
  water, therefore ice ___________________!

freeze
hydrogen
spread
Less dense
floats
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II. Diffusion
Just Know and understand the definition of
Diffusion!!!!!

• Early observations Brownian motion
• (1827) Was one of the first to observe the random
  motion of molecules and substances.
• The process of diffusion
• Diffusion ________________________
• ___________________________________
• Diffusion is a ___________ process because it
  relies on the random _________ of atoms and
  molecules

The net movement of particles from
an area of higher concentration to an area of
lower concentration.
slow
motion
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Diffusion
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Section 6.3

• Life Substances

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I. The role of Carbon in Organisms

• Molecular Chains
• Biomolecule large ____________ compounds (
  contains 10s, 100s, to 1000s of carbon atoms)
• Polymer a large molecule formed when ________
  smaller molecules bond together.

organic
many
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I. The role of Carbon in Organisms

• The structure of carbohydrates
• Carbohydrate a biomolecule composed of
  ________________________________
• _____________________________ (CHO ratio)
• Functions of carbos ___________________
• Two types of carbohydrates
• _______________
• A _______________ is a ____________ (small) sugar
• EX glucose and fructose

carbon, hydrogen, and oxygen that has or can be
reduced to a 121 ratio
Stores energy for the cell
Sugars
simple
monosaccharide
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I. The role of Carbon in Organisms
Disaccharide

• A __________ is _____ monosaccharide's linked
  together
• EX glucose fructose sucrose (table sugar)(pg
  159, 6.17)
• _______________
• Starches are ________________. The are polymers
  composed of many monosaccharide subunits.
• EX glycogen cellulose (pg 159 6.17)

2
Starches
polysaccharides
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Carbohydrate- sugar
Monosaccharide

• Glucose is stored
• In a plant as starch
• In an animal as glycogen

The formula for glucose (C6H1206) is shown above.
(121)
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I. The role of Carbon in Organisms

• Structure of Lipids
• Lipid large biomolecules that __________
• ___________________________________
• It can ______ reduced to a 121 ratio
• The are _________ in water because their
  molecules are __________ and repel water
• EX _____________________________
• ___________________________________
• Functions of lipids __________________
• __________________________________

are made mostly of carbon and hydrogen
with a small amount of oxygen.
not
Insoluble
nonpolar
Fats, oils, waxes, and steriods
energy storage,
insulation, protective coverings
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I. The role of Carbon in Organisms

• 5. Components of a lipid
• a. ________________________
• b. ___________________ (pg 160, 6.2)
• 6. Lipids can be saturated, unsaturated, or
  polyunsaturated.
• - Saturated All of the ______ atoms are
  _______ bonded together the molecule is now
  ____________ with hydrogen atoms

Three fatty acids
one glycerol molecule
carbon
Single
saturated
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I. The role of Carbon in Organisms

• Unsaturated when a _______ bond exists between
  two of the carbon atoms the molecule now has
  ________ hydrogen atoms
• Polyunsaturated when _________ double bonds
  exist between the carbons even __________
  hydrogen is present now.
• The structure of proteins
• Protein ________________________________
• ___________________________________

double
less
many
less
A large, complex polymer composed of carbon,
hydrogen, oxygen, nitrogen, and sometimes sulfur.
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I. The role of Carbon in Organisms

• Components of a protein __________
• ___________________________
• The amino acids are linked together by covalent
  ___________ bonds.
• Proteins come in a large variety of _______ and
  _________. The number and order of the
  ____________ determines its function.
• Functions of proteins
• a. Gives structure and ____________. Ex
  _________
• b. Help ____________ contact.

Amino acids
peptide
shapes
sizes
Amino acids
Hair, fingernails, horns, hoofs
support
muscles
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I. The role of Carbon in Organisms
oxygen

• Transport ____________ in your bloodstream. Ex
  ______________
• Provide ______________ EX _____________
• Carry out ______________ EX ___________
• An _____________ is a protein that changes the
  __________ of a chemical reaction.
• - Without the ________ of enzymes, we would not
  be able to __________ our food fast enough to
  feed our body.

hemoglobin
antibodies
immunity
reactions
enzymes
enzyme
rate
help
digest
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I. The role of Carbon in Organisms

• The structure of nucleic acids
• Nucleic acid a complex biomolecule that
  ________________________________.
• Components of a nucleic acid ______________
  (which have C, H, O, N, P)
• A nucleotide is made up of (page 163, fig 6.24)
• ________________________
• ________________________
• ________________________

Store cellular information in the form of a code
nucleotide
sugar
Nitrogenous base
Phosphate group
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I. The role of Carbon in Organisms

• Examples
• _______ (deoxyribonucleic acid)
• Contains our __________ ________ ( how to make
  all of our proteins)
• ______ (ribonucleic acid)
• - Take the code from ______ and actually take
  part in making our ______________.

DNA
Genetic code
RNA
DNA
proteins