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Chemistry of Life
Chapter 2
Elements
Simplest form of matter
Made of atoms of one type
Cannot be chemically broken down into
simpler substances
About 117 known elements
The Periodic Table of Elements
Each element has unique properties
>90% of the Human
Body
Carbon
Nitrogen
Oxygen
hydrogen
Elements/Atoms
Atoms
Smallest unit of an element
Still has chemical properties of that
element
Examples
Element oxygen – oxygen atoms
Element carbon – carbon atoms
Subatomic Particles
Subatomic
particle
Position/
Charge
Details
PROTONS NUCLEUS/
+
Atomic # = # of protons
# protons = # electrons (neutral element)
Atomic mass= # protons + # neutrons
Stay in clouds
-charge attracted to + charge of protons
Outermost shell electrons---chemical
rxns.
Inner shell electrons---held tightly
NEUTRONS NUCLEUS/
none
ELECTRONS CLOUD/
-
IONS
Elements with a + or – charge
Unequal # of protons and electrons
Lost electrons------- (+) charge
Ca +2
Gained electrons------ (-) charge
Cl –2
Isotopes
Elements with
same # of protons and electrons
Diff # of neutrons
Radioisotopes
Unstable nuclei break down
Release radiation
Uses:
Medical tagging/tracing
Fossil dating
What are isotopes used
for in medicine
Thyroid Scan
-radioactive iodine
Cancerous portion-failure to uptake iodine
PET
radioactive medicine is tagged to a natural
chemical (glucose)
As tracer is broken down positrons are
made
Scan detects different levels of positrons
PET Scans
Used for
• epilepsy (what part of the brain is being
affected)
• Alzheimer’s disease
• Cancer
• Heart disease
A Thyroid scan is a nuclear
medicine examination that uses the
emissions of gamma rays from
radioactive iodine to help
determine whether a patient has
thyroid problems, including
hyperthyroidism, cancer, or other
growths.
The scanner detects the location
and intensity of the gamma rays
emitted
Positron emission tomography (PET) scan of a person on cocaine
Cocaine has other actions in the brain in addition to activating reward. Scientists have the ability
to see how cocaine actually affects brain function in people. The PET scan allows one to see how
the brain uses glucose; glucose provides energy to each neuron so it can perform work. The scans
show where the cocaine interferes with the brain's use of glucose - or its metabolic activity. The
left scan is taken from a normal, awake person. The red color shows the highest level of glucose
utilization (yellow represents less utilization and blue shows the least). The right scan is taken
from a cocaine abuser on cocaine. It shows that the brain cannot use glucose nearly as effectively
- show the loss of red compared to the left scan. There are many areas of the brain that have
reduced metabolic activity. The continued reduction in the neurons' ability to use glucose
(energy) results in disruption of many brain functions.
Chemical Bonds
Attraction, sharing, or transfer of outer shell electrons
Energy bonds one atom to another
Energy stored in the molecule, energy is released when molecule breaks apart
3 Types:
Ionic
Covalent
Hydrogen
Ionic Bonds
Transfer of electrons
Sodium (Na+) + Chloride (Cl-)
Sodium chloride (NaCl)
Sodium Ion: Electron donated by Sodium
Chloride Ion: Electron accepted by Chloride
Covalent Bonds
Electrons shared
Helps fill electron shells
Examples
H-H (H2) and H-O-H (H2O)
Which of the above is a compound?
Single, double, triple
Polar Covalent: if UNEQUAL SHARING
Hydrogen Bonds
Hydrogen atoms bonded to oxygen or
nitrogen
Example: Strong force between water
molecules
Think about surface tension…
Chemical Reactions in
Living Cells
Help form new molecules for
Cell growth
Cell development
Cell maintenance
Allow storage or release of energy
Acids and Bases
ACIDS-
dissociate in H20
release H+
HClH+ + Cl-
BASES-
Take up H+ ions OR
Release –OH ions
NaOH Na+ + -OH
pH
pH = - [log H+]
pH scale = 0 – 14
Indicates how acidic or basic
High H+ = Very Acidic = LOW pH
Low H+ = Weakly Acidic = HIGH pH
or Very Basic
pH of body fluids
narrow range!
Normal blood pH = 7.4 (slightly alkaline)
Acidosis pH < 7.35
Alkalosis pH > 7.45
BUFFERS-maintain pH
[H2CO3] – [HCO3]
carbonic acid- H+ donor
Bicarbonate - H+ acceptor
Body’s pH
pH controls the speed of biochemical
reactions
low pH (too acidic) – body is slowly stewing
in poisonous wastes
Forces body to borrow minerals from vital
organs to neutralize the acid
Electrolytes
Salts, acids, bases
Dissociate in water
Release ions
Electrolyte balance
affects vital organs (heart, brain etc.)
Organic Compounds
Carbon atoms combined with Hydrogen
Usually Oxygen also
May contain Nitrogen, Sulfur, & Phosphorous
Macromolecules
Macromolecule Example Subunit(s)
Carbohydrates Polysaccaride Monosaccharide
Lipids Fat Glycerol + fatty
acids
Proteins Polypeptide Amino acid
Nucleic Acids DNA, RNA Nucleotide
Carbohydrates
Contain Carbon, Hydrogen, & Oxygen
H:O 2:1
Function: Source of Energy
3 Types :
Monosaccharides (1 sugar, simple)
Disaccharides (2 sugars, simple)
Polysaccharides (Multiple sugars, complex)
Monosaccharides
3-7 Carbons
Simplest form: glucose
Disaccharides
Double sugar
Know 3 types:
Sucrose(table sugar)= glucose + fructose
Lactose(milk sugar) = glucose+galactose
Maltose(malt sugar)=glucose + glucose
Polysaccharides
Many glucose molecules
Complex Carbohydrates
Examples
Starch
Glycogen
Cellulose
Pectin
chitin
Lipids
Fats and Oils
Contain carbon, hydrogen, and oxygen
Not in fixed ratio
Fatty acid + glycerolTG(Fat) + H2O
Non-polar (do not dissolve in water)
Functions:
Long-term energy and carbon storage
Parts of cell membrane
Types of Fats
Saturated: Butter and lard, solid at room temp
Single bonds only
Unsaturated: Olive oil, corn oil etc, liquid at room temp
Some double or triple bonds
Phospholipids : form cell membrane
Cholesterol: hormone development, cell membrane
Proteins
Made of Amino Acids
Functions
Structural components of cell
Messengers
Receptors (receive messages)
Defense
Enzymes (help with cellular reactions)
Amino Acids
Contain carbon, hydrogen, oxygen,
nitrogen
Building blocks of proteins
Peptide Bond –
Bond amino acids together to make
protein!
Protein Structure
Primary: Long polypeptide chain
Secondary: folded long polypeptide chain
Tertiary: more complex folding
Globular or spiral structure
Determined by amino acid sequence
Determines function
Quarternary: combined tertiary
Enzymes
Are a type of protein
Speed up chemical reactions (ex:
lactose)
Nucleic Acids
DNA and RNA
Stores genetic info
Contains info to
make protein for the
body.
Nucleic Acid Structure
Made of nucleotides (4 possibilities)
Each nucleotide has 3 parts:
5-carbon sugar (pentose)
A phosphate group
A nitrogen base (more on this…)
Nitrogen Bases
Purines (2 Rings):
Adenine (A)
Guanine (G)
Pyrimidines (1 Ring):
Cytosine (C)
Thymine (T)
replaced in RNA by Uracil (U)
DNA
Deoxyribonucleic acid
Double helix
Each helix/strand is made of:
Nucleotides
Each DNA nucleotide has:
A 5-carbon sugar (deoxyribose)
A phosphate group
A nitrogen base (A, T, G, C)
DNA Base Pairing
Hydrogen bonds
A and T (double bond)
G and C (triple bond)
Bonding b/w nitrogen base
Sugar phosphate backbone
RNA
Ribonucleic acid
Single stranded
Each strand is made of nucleotides
Each nucleotide is made of:
A ribose sugar
A phosphate group
A nitrogen base (A, U, G, C)
ATP
adenosine triphosphate
A nucleic acid that stores energy
contains 3 phosphate groups
Made in the mitochondria of every cell as
it carries out cellular respiration
Cells need energy from ATP to make
carbs/proteins, for muscle contraction
and for nerve impulse conduction