


Anything that has mass and occupies space
Some matter is changed chemically to produce
energy
Energy used to carry out cell activities

Exists in 3 states
 Solid – definite volume, definite shape
 Liquid – definite volume, indefinite
shape
 Gas – indefinite volume, indefinite
shape

Chemical and Physical Properties

Physical Properties – physical appearance or
characteristic of a substance
 Color
 Boiling or Melting Point
 Hardness

Chemical Properties – how one kind of matter reacts
with other matter
 Burning of a substance

Physical and Chemical Changes

Physical Changes – appearance changes, matter does not
 Change of State
 Freezing – from liquid to solid
 Melting – from solid to liquid
 Evaporation – from liquid to gas
 Condensation – from gas to liquid
 Sublimation – from solid to gas
 Change in size – cutting paper

Chemical Change – matter changes
 Iron reacts with oxygen to produce rust
 Law of Conservation of Matter – matter is neither created
nor destroyed, only changes form

Atom – tiny unit of matter

Composed of:
 Protons - + charge, 1amu, in nucleus
 Neutron – no charge, 1amu, in nucleus
 Electron - - charge, 0 amu, in electron cloud

Element – Substance containing only one type
of atom

Atoms of same elements have the same number of
protons – called Atomic Number
 Hydrogen – 1 proton
 Oxygen – 8 protons



Sum of protons + neutrons determines Atomic Mass
Number
Isotopes – atoms that have the same number of
protons but different numbers of neutrons
Number of electrons = Number of protons; result
atom is electrically neutral

Elements are arranged according to atomic
number in the Periodic Table
Element Symbols
1st one or two letters of English name
Hydrogen H
Helium He
Others from Latin or foreign language names
Silver
Ag Argenitum (Latin)
Tungsten
W
Wolfran (German)
1st letter always capitalized, 2nd is lower case
Atoms want to be stable, want a complete
outer energy level
Combine with other elements; both become
stable
Compound – substance formed when 2 or
more elements bond chemically
Stability by sharing or transferring electrons
Covalent Bond – electrons are shared
Molecule – bonded set of atoms
Ionic Bond – electrons are transferred
Ion – electrically charged atom
Negative Ion – gain electrons
Positive Ion – loses electrons
Bond forms due to attraction of
oppositely charged ions
Covalent Bonds – Water (H2O)
Ionic Bonds – Sodium Chloride (NaCl)
Chemical Formula – Expression of chemical
makeup of a compound
Shows kinds and number of atoms
H2O – 2 atoms hydrogen; 1 atom oxygen
Coefficients show number of molecules
2H2O – 2molecules; 4 atoms H; 2 atoms O
Composed of 2 or more substances that can be
separated by physical means
Homogeneous – every part looks same
Heterogeneous – some sections look different
Types
Solution
Suspension
Colloid
Solution
Homogeneous mixture where one
substance is dissolved in another
Solute – Substance dissolved
Solvent – Substance doing the
dissolving
Suspension
Heterogeneous mixture of substances larger
than molecules or ions
Particles may settle
Some stay suspended; cloudy appearance
Example - Blood
Colloid
Homogeneous mixture with particles
larger than in solution but smaller than a
suspension
Clusters of atoms, ions or molecules
Examples – Gelatin, Homogenized Milk
Most atoms in Human Body
Hydrogen
Oxygen
Carbon
Nitrogen
Inorganic Compounds
Primarily composed of elements
other than Carbon
Organic Compounds
Contain the element Carbon
Most abundant inorganic compound in living
organisms
Composed of Hydrogen and Oxygen
Universal Solvent – dissolves many
substances due to polarity of water
Dissolves ionic compounds to produce
ions called electrolytes
Doesn’t dissolve covalent compounds
very well
Dissociates to form H+ and OH- ions
Both are equal in distilled water
Gives us the pH scale
Below 7 – acidic
Above 7 – alkaline
7 - neutral
Polarity of water
Causes hydrogen bonding – bond between H of
one and O of another.
Results in water’s unique properties
Boiling and Freezing Points
Cohesion – attracted to other water molecules –
water droplets
Adhesion – attracted to other similar molecules
– allows movement of water in plants
Inorganic even though it contains
carbon
Source of Carbon and Oxygen in
organic compounds by way of
photosynthesis
Contain the element Carbon
Has 4 electrons in outer energy level
Can form 4 bonds – either with other
carbons or other elements
Originally believed to have to come
from living organisms
Many have been synthesized
Often described by structural formulas
Show kinds of atoms
Show number of atoms
Show how atoms are attached to each
other
Organic Compound important to Life
Carbohydrates
Proteins
Lipids
Nucleic Acids
Processes (reactions) important to organic compounds
Dehydration Synthesis
Production of a more complex molecule from 2 or
more simpler molecules by removing a water
molecule
Hydrolysis
Breakdown of a more complex molecule into
simpler molecules by the addition of a molecule of
water – usually during digestion
Composed of Carbon, Hydrogen, and Oxygen
Hydrogen: Oxygen ratio always 2 to 1
Used for energy source, structure, and energy
storage
Classes
Monosaccharides
Disaccharides
Polysaccharides
Monosaccharides – single sugars
Most have formula C6H12O6 –different
structures
Examples – glucose, fructose, galactose
Glucose – food product of photosynthesis
Disaccharides – double sugars
Composed of 2 monosaccharides that combine by
dehydration synthesis
Molecular formula – C12H22O11
Examples
Sucrose (Table Sugar) – Glucose + Fructose
Lactose (Milk Sugar) – Glucose + Galactose
Polysaccharides – many sugars
Made of many monosaccharides that combine
during a series of dehydration syntheses
Types
Cellulose – structural compound in plants
Starch – energy storage in plants
Glycogen – energy storage in animal livers;
called “animal starch”
Composed of Carbon, Hydrogen, Oxygen, and
Nitrogen; sometimes Sulfur
Made up of 20 different Amino Acid joined
together by dehydration synthesis reactions.
Peptide Bonds join the amino acids – amino
group of one amino acid attaches to carboxyl
group of another amino acid
Used to build and repair cells; also function as
enzymes.
Types
Dipeptide – 2 amino acids
Polypeptide – many amino acids
Amino Acid Structure
3 basic parts around a central Carbon
Amino Group – NH2
Carboxyl Group – COOH
R-Group – a simple H or group of Carbon
and Hydrogen atoms
Hydrogen forms the 4th bond.
Enzyme - protein molecule that acts as an organic
catalyst – changes the rate of chemical reaction
Acts on a Substrate – Material to be changed
Often described as a “Lock and Key” operation
Lock – substrate
Key - enzyme
Contain Carbon, Hydrogen, and Oxygen
Larger number of Hydrogen atoms and lower
number of Oxygen atoms than carbohydrates
Insoluble in water
Most composed of Fatty Acids
Primary function is energy storage but help form cell
membranes
Fatty Acids
Large straight chain hydrocarbon with a
carboxyl group at one end
Carboxyl Group – Hydrophilic
Hydrocarbon Chain – Hydrophobic
Saturated Fatty Acid
Unsaturated Fatty Acid
Kinds
Triglycerides – 3 fatty acids bonded to a
glycerol by dehydration synthesis
Oil – Liquid at room temperature
Fat – Solid at room temperature
Wax – Long fatty acid bonded to long alcohol
Steroids – Rings of 4 Carbons; hormones, nerve
tissue, some plant and animal poisons
Triglyceride
Phospholipids
Complex molecules that store and transmit
important information about the cell
Involved with transmission of characteristic
during cell reproduction
Types
Deoxyribonucleic Acid – DNA
Ribonucleic Acid – RNA
DNA and RNA – composed of thousands of
nucleotides
Nucleotides – composed of 3 parts formed by
dehydration synthesis
Parts
5-Carbon Sugar – Ribose or Deoxyribose
Phosphate Group
Nitrogen Base – Guanine, Cytosine, Adenine,
Thymine, or Uracil
Deoxyribonucleic Acid
Stores information essential for cell activities
Found mostly in the cell nucleus
Ribonucleic Acid
Stores and transfers information to make
proteins