Chapter 2. Atom Element = the smallest unit of matter that cannot be broken down = a pure substance...
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Transcript of Chapter 2. Atom Element = the smallest unit of matter that cannot be broken down = a pure substance...
![Page 1: Chapter 2. Atom Element = the smallest unit of matter that cannot be broken down = a pure substance made of only one kind of atom.](https://reader035.fdocuments.us/reader035/viewer/2022062422/56649edb5503460f94bebbc5/html5/thumbnails/1.jpg)
Chapter 2
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AtomElement
= the smallest unit of matter that cannot be broken down
= a pure substance made of only one kind of atom
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Protons = positive electric charge (1+)
Neutrons = neutral charge (0)Electrons = negative charge (1-)
Atoms are composed of even smaller parts, called subatomic particles.
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Each element has a unique number of protons = atomic number.
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• Atoms have equal numbers of P and e- – The atomic number = tells the number of
protons and the number of electrons
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•Mass number = the sum of the number of protons
and neutrons in the nucleus of an atom.
# Neutrons = Mass # - Atomic #
# protons?# electrons?# neutrons?
Carbon =
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• Atoms of a given element may differ in the number of neutrons = isotopes.
• In nature, an element occurs as a mixture of isotopes.– For example, 99% of carbon atoms have 6
neutrons (12C).– Most of the remaining 1% of carbon atoms
have 7 neutrons (13C) while the rarest isotope, with 8 neutrons is 14C.
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6 C Carbon 12.01
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Electron ShellsEnergy Levels
1st Shell = 2 electrons2nd Shell = 8 electrons3rd Shell = 8 electrons (stable)
PN
e-
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Atoms are mostly “empty space”
If Nucleus= golf ball ----------------------------------------------------- e-
1km (10 football fields)
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Electron ShellsEnergy Levels
Valence Electrons = electrons in outer energy shell
Valence Electrons do the interaction during chemical reactions.The nuclei do not come close enough to interact.
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Groups/Families
Periods (+ Protons/electrons)
(Reactivity/Valence e-)
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? ? ? ? ? ?
?1 2 3 4 5 6 7
2/8Valence Electrons?
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Atom Interaction?
~ 50 trillion cellsEach cell 1,000’s atoms
Valence Electrons
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• Atoms want to be “stable” = full valence shell.
• Share or transfer electrons.
• To become stable, atoms will hold together by chemical bonds.– The strongest chemical bonds are covalent
bonds and ionic bonds.
Chemical bonds
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ChemicalBond
SingleAtoms
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• A covalent bond is the sharing of a pair of electrons by two atoms.
Hydrogen
H H
H2 Subscript (2 atoms)
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“Hydrogen Molecule” (H2)
Single Covalent
Double Covalent
Two or more atoms held together by covalent bonds constitute a molecule
“Oxygen Molecule” (O2)
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• Ionic bond = one atom strips an electron completely from the other.
NaCl
Ions = charged atoms or molecule
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• YouTube - Carl Sagan on the chemical elements
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BalloonVan de Graff Machine
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Top 4 Atoms found in Organisms?
O = 65%C = 18.5%H = 9.5%N = 3.3%
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AstronomersLife evolved in water
~75% Earth Cells 70-95% Water
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H2O
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Polar Covalent Bond = electrons not shared equally
-
+
“Polar Molecule”
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• Hydrogen bonds = a weak chemical attraction between polar molecules.
H+ O-
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Up to 4 per water molecule
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Cohesion = water molecules bonding to each other.
“Surface tension” prevents
stretch or break the surface
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Adhesion = clinging of one substance to another (polar polar).
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Solution = homogenous mixture.
Solute = Solvent =
Water is the “solvent” of life
dissolving agentsubstance dissolved
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Forms hydrogen bonds with charged and polar covalent molecules.
Solvent?Solute?
“Dissolve”
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pHHydrogen Ion
H+
“Dissociation”
H2O <=> H+ + OH-
Acid = any compound that forms hydrogen ions (H+) ions in solution
Base = any compound that forms hydroxide ions (OH-) in solution
pH scale = concentration of H+ in a solution
Buffers = weak acids or bases that prevent sudden changes in pH
“Homeostasis”
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pH
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Hydrogen Ion
H+
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• Dissociation
H2O <=> H+ + OH-
• In pure water only one water molecule in every 554 million is dissociated.
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pH scale = concentration of H+ in a solution
0 - 14
7 = neutral (H+ = OH-)
0-6 = acidic (H+)8-14 = basic (OH-)
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Base = any compound that forms hydroxide ions (OH-) in solution
Acid = any compound that forms hydrogen ions (H+) ions in solution
Factor of 10
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Cell pH = 6.5 – 7.5
“Homeostasis”
Buffers = weak acids or bases that prevent sudden changes in pH
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CARBON COMPOUNDS“ORGANIC CHEMISTRY”
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96%
-------------------
-------------------
4%
-------------------
Life dependson 25 elements
“Trace elements”
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• Although cells are 70-95% water, the rest consists mostly of carbon-based compounds.
• Proteins, DNA, carbohydrates, and other molecules are all composed of carbon atoms bonded to each other and to atoms of other elements.
“CARBON COMPOUNDS”
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Organic chemistry = the study of carbon
compounds (organic compounds).
HONSP
C bonds with:
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3-D
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Hydrocarbons “Petroleum”
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Functional groups unique properties
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Macromolecules
Form
MONOMERS
POLYMERS
“Single”
“Multiple”
Large Carbon Based Molecules
B
ond
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MACROMOLECULES
Elements Monomers Example
Carbohy-drates
C,H,O
1:2:1
Monosac-
carhides
Starch
Glucose
Sucrose
Lipids C,H,O Glycerol
Fatty Acids
Fats
Oils
Cholesterol
Proteins C,H,O,N Amino
Acids
Insulin
Hemoglobin
Nucleic
Acids
C,H,O,
N, P
Nucleotides DNA
RNA
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1. CARBOHYDRATES
“Sugar”
Main source of energy
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GlucoseC6H1206
Monomer =
“Monosaccharide”
1:2:1
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“Polysaccharide”
Starch Glucose Glucose
Polymer =
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Monomers:
2. LIPIDS (fats, oils, waxes)
Glycerol
Fatty Acid
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Monomer
Polymer
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Straight
Kinked
Solid at room Temp (Bad)
Liquid at Room Temp (Good)
Double bond prevents “packing”
Store energy
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Steroids
Cholesterol
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3. PROTEINS
AA—AA—AA—AA
Monomer =Amino Acids
“Peptide” Bond
Polymer =“Polypeptide”
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20 different Amino Acids
“R Group”
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Proteins:Control rate of reactionsRegulate cell processesForm bone and muscleTransport substances into and out of the cellFight disease
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4. NUCLEIC ACIDS
Monomers =Nucleotides
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Monomer
Monomer
Polymer =Nucleic Acids (DNA/RNA)
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• YouTube - Carl Sagan on the chemistry of life on Earth/ other planets
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CHEMICAL REACTIONS AND ENZYMES
Energy = the ability to move or change mater
Chemical reactions = chemical bonds between atoms are broken and new ones formed
Chemical equations: Reactants ProductsNaCl Na+ + Cl-
Metabolism = all the chemical reactions that occur in an organism
Activation energy = the energy needed to start a chemical reaction
Enzyme = a substance that increases the speed of chemical reactions
Speeds-up reaction by reducing activation energy
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Chemical reactions = chemical bonds between atoms are broken and new ones formed
Reactants Products
NaCl Na+ + Cl-
Chemical equations:
Energy is released or stored
Na + Cl Na+Cl-
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Energy Releasing Reaction
“Bonds Broken”
NaCl Na+ + Cl-
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Energy Absorbing Reaction
“Bonds Formed”
Na + Cl Na+Cl-
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Metabolism = all the chemical reactions that occur in an organism
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Activation energy = the energy needed to start a chemical reaction
“Push” needed
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Cells require activation energy
Enzyme = a substance that increases the speed of chemical reactions
“catalyst”
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Speeds-up reaction by reducing activation energy
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1. Substrate binds to enzyme
2. Substrate is converted toproducts
3. Productsare released
4. Active siteis availablefor anothersubstrate
active sitesubstrate
induced fit
Enzymes are unaffected by the reaction and arereusable
Reaction rate issubstrate concentrationdependant
denature
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End in “-ase” AmylaseCatalase