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BioChemistry

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Matter

Matter = any material with Mass & Volume (i.e. takes up space)

Everything is made of matter

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What are the properties of matter?

  • Characteristics used to describe an object
  • Ex: color, odor, shape, size, texture, hardness, mass, weight, density

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Physical properties

  • Physical properties can be observed or measured without changing the identity of the matter.
  • Basically, properties you notice when using one of your five senses:
    • Feel - mass, volume, texture
    • Sight - color
    • Hear
    • Smell
    • Taste

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Physical vs. Chemical

  • Physical properties: observe without changing the identity of the substance
  • Chemical properties: observe only when the identity changes
  • How do you know if it is chemical or physical?
    • If it Changes for good, it’s CHemical

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Chemical properties

  • A common chemical property is reactivity.
    • Reactive to oxygen
    • Reactive to air
    • Reactive to water…
  • Notice that chemical properties aren’t EASY to observe, unlike physical properties.

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Chemical Changes

  • Chemical changes do alter the identity of a substance
  • In other words, a chemical change is when something changes into an entirely different substance
  • For example:
    • Iron rusting
    • Wood burning
    • Copper turning to brass
    • Baking a cake
    • spoiled milk

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Chemical properties-

  • These are properties that can only be observed by changing the identity of the substance.

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  • A piece of paper burns and turns to a black substance.
  • After the flame goes out you can no longer burn the new substance.

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  • The chemical properties have been changed.

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  • Milk needs to be in the refrigerator or else it will go bad.
  • If you've ever seen or smelled spoiled milk, it is not a pretty sight.
  • The milk gets a sour odor and becomes lumpy.
  • Unlike physical changes, you cannot reverse chemical changes.
  • You can melt ice to get water and freeze that water to get ice again.
  • You cannot make milk unspoiled.

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Matter

Solid

Liquid

Gas

- comes in 3 phases

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Solid

Definite Shape

Definite Volume

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Liquid

Indefinite Shape – takes the shape of the container

Definite Volume

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Gas

Indefinite Shape – takes the shape of the container

Indefinite Volume – can expand and be compressed

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States of Matter

Solid

Liquid

Gas

Definite Volume?

YES

YES

NO

Definite Shape?

YES

NO

NO

Result of a Temperature Increase?

Small Expans.

Small Expans.

Large Expans.

Will it Compress?

NO

NO

YES

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4th state: Plasma - formed at high temperatures; ionized phase of matter as found in the sun. Interesting but not so much to biology (If your dealing with plasma with living things, things have went terribly wrong)

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Three Main Phases

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Solid

Liquid

Gas

Melt

Evaporate

Condense

Freeze

Sublimation

Deposition

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Atoms

Atoms

The study of chemistry begins with the basic unit of matter, the atom.

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Atom

The smallest particle making up elements

PROTON

NEUTRON

ELECTRON

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Placed side by side, 100 million atoms would make a row only about 1 centimeter long.

Atoms contain subatomic particles that are even smaller.

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Atomic Structure

Sub-atomic Particles

Protons - p+ - positive charge, in nucleus 1 Atomic Mass Unit (AMU)

Electrons - e- negative charge, orbiting nucleus (Almost no mass)

Neutrons - n0 – no charge, in nucleus (1AMU)

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Atoms and the Periodic Table

Atomic number - Number of protons in an atom.

Neutrons – Atomic Mass – Protons

Atomic Mass – Protons + Neutrons

Electron – Equal to protons in a neutral atom

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Elements and Isotopes

Elements and Isotopes

Element - a pure substance that consists entirely of one type of atom.

ex.

        • C stands for carbon.
        • Na stands for sodium.

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Isotopes

Isotope - Atoms of the same element that have a different number of neutrons

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Elements and Isotopes

Because they have the same number of electrons, all isotopes of an element have the same chemical properties.

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Isotopes of Carbon

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Radioactive Isotopes

Some isotopes are radioactive, meaning that their nuclei are unstable and break down at a constant rate over time

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      • to determine the ages of rocks and fossils.
      • to treat cancer
      • to kill bacteria that cause food to spoil.
      • as labels or “tracers” to follow the movement of substances within an organism.

Radioactive isotopes can be used:

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Molecules and Compounds

Molecule – Atoms of the same element chemically combine. Ex. O2, N2, O3

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Compound - 2 or more different elements chemically combined to form a new substance with new properties. Ex. C6H12O6, H2O, CH4

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H2 + O H2O =

H

O

H

Chemical formula lists the number of different atoms in a single molecule

Structural formula shows the arrangement of the atoms in a single molecule

Molecules and Compounds

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Compounds

Inorganic Compounds

or

Organic Compounds

  • usually don’t contain Carbon
  • generally come from the earth
  • generally simple molecules
  • always contain C & H and usually O, N, sometimes S & P
  • originate in organisms
  • generally complex molecules

Biology!!

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Most Common Elements in Living Things

H

= Hydrogen

C

= Carbon

O

= Oxygen

S

= Sulfur

P

= Phosphorus

N

= Nitrogen

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Examples of Inorganic Compounds

H + O

= H2O = Water

H + Cl

= HCl = Hydrochloric Acid

C + O

= CO2 = Carbon Dioxide

Na + Cl

= NaCl = Common Table Salt

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Examples of Organic Compounds

C, H + O

Carbohydrates = Sugars, starches & cellulose

C, H + O

Lipids = Fats & Oils

C, H, O, N, & sometimes P + S

Proteins

C, H, O, N, + P

Nucleic Acids – DNA & RNA

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BioChemistry

Diga, diga, diga, diga, that’s all for today folks!