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Opening Assignment
• What are the 4 main elements that make up 95% of the human body?
• Draw an atom of Carbon including the protons, neutrons, and electron shells. (Hint: Carbon has an atomic number of 6)
Opening Assignment
• What are the 4 main elements that make up 95% of the human body?
• Draw an atom of Carbon including the protons, neutrons, and electron shells. (Hint: Carbon has an atomic number of 6)
Anatomy and Physiology Honors Chapter 2 The Chemical Basis of Life
By Mrs. Shaw
Resources Hole’s Essentials of Anatomy and Physiology 9th Edition
Learning Goals for Lessons 2.1 and 2.2
Students will be able to:– Explain how the study of living things depends on the
study of chemistry.– Discuss how atomic structure determines how atoms
interact.– Describe the relationship between atoms and molecules.– Explain how molecular and structural formulas symbolize
the composition of compounds.– Describe the three types of chemical reactions.– Define pH.
Chemistry is . . . .
• Chemistry is the branch of science that considers the composition of matter and how this composition changes.
• This is essential to the study of anatomy and physiology because body structures and functions result from chemical changes within cells.
What’s the Matter?
• Matter is anything that has mass and takes up space.
• This includes all the solids, liquids, and gases in our surroundings and in our bodies.
Elements
• ELEMENT – single type of atom. As of 2010 there are 118 known elements (98 occur naturally on Earth)
Living organisms require about 20 elements. Oxygen, Carbon, Hydrogen, and Nitrogen make up more than 95% of the human body.
Atoms• ATOM-the smallest complete unit of elements
that maintain the characteristics of that element.
– Nucleus- The center of the atom, contains protons and neutrons
– Electron Cloud –Region surrounding the nucleus containing the electrons
The NucleusProton-A positively charged sub-atomic particle
(+). Atomic Mass = 1 amuThe number of protons is the same as the atomic
number
Li3
7 The atomic massThe atomic mass
The Atomic Symbol
The Nucleus
Neutrons –A sub-atomic particle in the nucleus--Has a mass equal to 1 atomic mass unit
--Neutron do not have a charge (0)To calculate the number of neutrons in an element…
Li3
7
The atomic number
The atomic massThe atomic mass
The atomic mass- The atomic number The number of neutrons
Li3
7
The atomic number
The atomic massThe atomic mass
7 (Atomic Mass)- 3 protons(Atomic #) 4 neutrons
WRITING RESPONSE
How many protons does Mg have?
How many neutrons does Mg Have?
WRITING RESPONSE
How many protons does Mg have?12
How many neutrons does Mg Have? 12
The Electron Cloud
• Electrons-• The number of electrons equals the number of protons• Sub-atomic particle with a negative charge (-)• Electrons behave as if in a 3-D orbit
• Valence Electrons– The outer most electrons– Valence electrons are responsible for bonding
WRITING RESPONSE
How many protons?
How many neutrons?
How many electrons?
WRITING RESPONSE
How many protons? 3
How many neutrons? 4
How many electrons? 3
Bohr Model• The first shell can have
2 electrons• The second shell can
have 8 electrons
Shells and the Electron Cloud
Let’s look at a few elements…
Hydrogen 1= Proton 1= electron
Let’s look at a few elements…
Helium 2=protons 2=neutrons2=electrons
Let’s look at a few elements…
Lithium 3=protons 4=neutrons3=electrons
Let’s look at a few elements…
Fluorine9=protons 10=neutrons
9=electrons
Let’s look at a few elements…
Argon18=protons 22=neutrons
18=electrons
IONSCharged particles that occur when an atom gains or loses an electron during chemical bonding.
• If the atom gains an electron- Negative charge• Ex: Cl-
• Most non-metals form negative Ions
• If the atom loses an electron- Positive Charge• Ex: Na+
• Most metals form Positive Ions
Losing an Electron = Positive ion Na+ has 11 protons but only 10 electrons
Gaining an Electron = Negative ion Cl- has 17 protons but has 18 electrons
Which shows a negative ion? Explain
Which shows a neutral atom? Explain
Which shows a positive atom? Explain
A
B
C
What would the charge be on an atom that lost an electron? Gained two electrons?
ISOTOPES
Atoms that have the same # of protons but have neutrons that have been added, resulting in a different atomic mass.
Electrons and bonding• Think about having two magnets. The closer they are to each
other the stronger the attraction is. There is a similar attraction between the negatively charged electrons and the positively charged nucleus.
• The outermost electrons (valence electrons) can be attracted to the nucleus of other atoms. This attraction is what causes a chemical bond.
Valence electrons 1
• The outer most electrons (valence electrons) are the only electrons involved in chemical bonding.
• Valence electrons have the most energy out of all the electrons in an atom.
• The number of valence electrons in each atom of an element can help determine the type and the number of bonds It can form.
Chemical bonding • Chemical bonding is the joining of atoms to
form new substances. A chemical bond is an interaction that holds two atoms together.
• Most atoms form bonds by gaining, losing, or sharing valence electrons until they fill their outer shell to become “happy” or stable.
Types of Chemical Bonds
• There are three types of chemical bonds we will discuss: ionic bonds, covalent bonds, and hydrogen bonds.
Covalent Bonds
• Covalent bonds happen when atoms share electrons.
• For example: Chlorine needs one electron to have a full outer shell so it can share 2 electrons with another Chlorine atom and become stable.
Covalent Bonds
• Another very important covalent bond is
Ionic Bonds
• Ionic bonds happen when electrons are transferred from one atom to another, causing the atom to become either positively charged or negatively charged.
• Na + Cl = Na Cl Table Salt
Ionic Bond
Losing an Electron = Positive ion Na+ has 11 protons but only 10 electrons
Gaining an Electron = Negative ion Cl- has 17 protons but has 18 electrons
This is the formation of a new substance through an Ionic Bond
Polarity and Hydrogen BondsDifferent types of chemical bonds share electrons to different degrees.
An ionic bond gains or loses electrons.
A covalent bond shares electrons.
A molecule formed when electrons are not shared equally. This results in the formation of a polar molecule hydrogen bond
Hydrogen Bonds
• The attraction of the positive hydrogen end of a polar molecule to the negative nitrogen or oxygen end of another polar molecule is called a hydrogen bond.
Hydrogen bonds• Hydrogen bonds are
important in protein and nucleic acid structure. In these cases, hydrogen bonds occur between polar regions within different parts of a single, very large molecule.
Molecules and Compounds
• When two or more atoms bond, they form a MOLECULE. They can be the same type of atom (Element)
• When atoms of two different types of elements bond, they form molecules called COMPOUNDS.
Formulas• A molecular formula presents the numbers
and types of atoms in a molecule.• Hydrogen Peroxide
• A structural formula shows the bonds that happen within a molecule
Elements, Compounds, and Mixtures
• http://www.bing.com/videos/search?q=mr%20lee%20elements%20compounds%20mixtures&qs=n&form=QBVR&pq=mr%20lee%20elements%20compounds%20mixtures&sc=0-28&sp=-1&sk=#view=detail&mid=20E281F99AE7071776D120E281F99AE7071776D1
Opening Assignment
1. Draw an atom of Nitrogen.2. How many bonds can an atom of Nitrogen
make?3. Differentiate from the 3 types of chemical
bonds: ionic, covalent, hydrogen.
Chemical Reactions
• Chemical reactions form or break bonds between atoms, ions, or molecules generating new chemical combinations.
Synthesis
• When two or more atoms bond to form a more complex structure the reaction is called synthesis. Synthesis requires energy!
Decomposition
• When the bonds within a molecule break so that simpler molecules, atoms or ions form, the reaction is called decomposition.
Exchange Reaction
• A third type of chemical reaction is an exchange reaction. In this reaction two different types of molecules trade positions.
Reversible Reactions
• Many chemical reactions are reversible. They are shown with a double arrow.
Carbonic Acid
Acids and Bases
• Some compounds release ions when they dissolve in water or react with water molecules.
• Since the resulting solution contains electrically charged particles it will conduct an electric current. Substances that release ions in water are called electrolytes.
Acids
• Acids are electrolytes that release hydrogen ions in water.
Bases• Electrolytes that release
ions that bond with hydrogen ions are called bases.
• For example sodium hydroxide releases hydroxide ions when placed in water. These hydroxide ions can bond with hydrogen ions to form water. This makes them a base.
ACIDS BASES
• All compounds can be classified in 2 broad categories:
• Organic compounds- Contain carbon and hydrogen atoms
• Inorganic compounds- Can have one or the other, but do not contain both carbon and hydrogen atoms
Organic Compounds• Most of your body’s molecules are organic
compounds.•
– Macromolecules are built from small organic compounds the same way a railroad train is built, by linking a lot of smaller units together into long chains.
•
Monomers and Polymers• Large carbon compounds are built up from smaller simpler
molecules called monomers (mono = one )• Monomers can bind to one another to form complex molecules
known as polymers (poly = many)• A polymer consists of repeated, linked units, which can also bind
forming large polymers called Macromolecules. (macro = large )
Dehydration Synthesis• Monomers link to form polymers through a chemical
reaction called condensation reaction or dehydration synthesis. During the formation of polymers, Water (H2O), is released or is by-product of the reaction.
Hydrolysis or DecompositionThe breakdown of some complex molecules, such as polymers, occurs through a process known as hydrolysis. (decomposition)
Hydrolysis is the reverse of a condensation reaction. The addition of water, to some polymers can break the bonds that hold them together
4 Main Macromolecules• There are four main types of macromolecules
found in living organisms: • Carbohydrates• Lipids • Proteins• Nucleic Acids
Carbohydrates– Carbohydrates
• Composed of carbon, hydrogen, and oxygen atoms in the proportion of 1 : 2 : 1
– General formula: (CH2O)n where n is the number of carbon atoms.
» Example: The sugar glucose is a small carbohydrate; its n equals 6. Therefore its chemical formula is C6H12O6.
• The building blocks (or monomers) of carbohydrates are monosaccharides.
Carbohydrates• Monosaccharides are simple sugars (saccharide = sugar). Examples:
– Glucose: commonly found in blood of animals– Galactose: a simple sugar found in milk – Fructose: commonly found in fruit
» Glucose and Fructose both have the formula C6H12O6, Sometimes compounds may have the same formula, however they have different structures/ arrangements. In such cases, those compounds are called isomers.
Carbohydrates• Disaccharides contain 2 monosaccharides joined by
dehydration synthesis. Examples: –Lactose: commonly found in milk, made up of
Galactose + Glucose–Sucrose: “table sugar”, transported in plants, made
up of Fructose + Glucose
Carbohydrates• Polysaccharides are carbohydrates formed from linking individual sugars into long chains. Examples:
– Starch: a common storage form of glucose in plants (breads, pasta, potatoes)
– Cellulose: a polysaccharide contained in the cell walls of plants; gives strength and rigidity to plant cells.
– Glycogen: a common storage form of glucose in animals (stored in the muscles and liver to be used as quick energy)
•
Lipids– Lipids (include fats, oils, waxes, etc.)
• Class of macromolecules that do not dissolve in water
• Lipids usually serve one of three functions: – Energy storage– structural support in cell membranes
(phospholipids)– serve as reactants ( starting materials) for
metabolic reactions
• Fatty acids are the building blocks (or monomers) that make up most lipids.
• Fatty acids are classified as either saturated or unsaturated.
Lipids– The classification depends on the proportion of hydrogen atoms
to carbon - carbon bonds in the molecule:– Saturated fatty acids have the maximum number of bonds
possible, they are full.» Saturated fats are usually solid at room temperature, and
most come from animal products.– Unsaturated fatty acids have double bond(s) in the carbon
chain and are not full.» Most unsaturated fats are liquid at room temperature, and
are usually referred to as oils.– Saturated animal fats are associated with circulatory disorders;
plant oils can be substituted for animal fats in the diet.
Lipids• A common lipid that contains fatty acids is a
triglyceride. Triglycerides (referred to as neutral fats) are glycerol linked to three fatty acids (in the shape of an “E”) by condensation reaction.
Proteins• Proteins are organic compounds composed mainly of
carbon, hydrogen, and nitrogen atoms.• Proteins are the construction materials for body
parts such as hair, skin, nails, and blood.
Proteins• Amino acids are the
building blocks (or monomers) that make up most proteins
– There are 20 different kinds of amino acids that humans use.
• One important group of proteins - enzymes - help control chemical reactions by acting as catalysts. Catalysts speed up reactions by lowering activation energy.
•
Nucleic Acids• Nucleic Acids are complex
organic molecules that store genetic information in the cell.
• Nucleotides are the building blocks (or monomers) that make up most nucleic acids.
–Nucleotides consist of a sugar (pentose) + base (nitrogenous) + phosphate.
•
Nucleic Acids• Three main types of nucleic acids
– DNA = Deoxyribonucleic acid» Is the genetic information inside the nucleus of cells
– RNA = Ribonucleic acid» Instructions which code for protein synthesis
– ATP = Adenosine triphosphate = has a slightly different structure than DNA and RNA. It contains a base + sugar + three phosphates
» ATP is used as energy for the cell
Macromolecules• http://
www.bing.com/videos/search?q=macromolecules+amoeba+sisters&FORM=VIRE1#view=detail&mid=28E79698F384F31B45C528E79698F384F31B45C5 (Amoeba Sisters – Review of Function)
• http://www.bing.com/videos/search?q=Macromolecules+Animation&FORM=RESTAB#view=detail&mid=3E26F3D92D4C97E606FB3E26F3D92D4C97E606FB (Review of structure)