1. BIOCHEMISTRY I

2. A sense of scale

3. Matter: the physical component that makes up everything
Takes up space
Has mass
Everything excluding empty space and energy.

4. PARTICLE THEORY OF MATTER
All matter is made up of particles
All particles in a pure substance are identical (no two different pure substances have the same particles)
3. All particles have space between them
All particles are always moving – more energy
(heat) produces more movement
5. All particles are attracted to one another
If a solid absorbs heat, it may become a
liquid. If a liquid absorbs heat, it may
become a gas.
VIDEO:

5. Atom: most basic unit of matter (the particles)!
CHEMISTRY OF LIFE
Atom: most basic unit of matter (the particles)!
composed of a nucleus (protons & neutrons) and electrons.
Particle
Charge
PROTON +
NEUTRON
NEUTRAL
ELECTRON -

6. Element: simplest form of a substance
CHEMISTRY OF LIFE
Element: simplest form of a substance
A pure substance consisting of ONE type of atom.
Is distinguished by its atomic number.
Each element has a specific symbol.
Examples: Hydrogen (H), Carbon (C), Oxygen (O), Phosphate (P), Sulphur (S), Neon (Ne), Helium (He), Nitrogen (N), etc.
Where can we find information about different elements?...

7. CHEMISTRY OF LIFE
THE PERIODIC TABLE OF ELEMENTS!!!

8. CHEMISTRY OF LIFE
In Biology, we deal mostly with elements within the elements within the first 4 rows (periods) of the Periodic Table.
Bulk Elements: C, H, O, N – make up the majority of every living thing.
Ex. 96% of human body
Minerals:
Ma, Mg, P, K, Ca (3.5%)
Fe, I (trace elements – tiny amounts)

9. REPRESENTING AN ATOM A Bohr Diagram
Find the element on the periodic table.
Determine the number of electrons (same as atomic #)
Determine the number of Neutrons
(Atomic Mass – Atomic #)
Write the number of Protons (P) and Neutrons (N) in the “nucleus.”
Draw appropriate number of orbitals around the nucleus (1, 2, or 3)
First orbital – 2 electrons max
Second orbital – 8 electrons max
Third orbital – 18 electrons max

10. Bohr Diagrams
Carbon

11. Bohr Diagrams
Chlorine

12. Only shows the OUTER electrons of an atom.
REPRESENTING AN ATOM
A Lewis Dot Diagram
Only shows the OUTER electrons of an atom.
The shell of the outer electron is called the VALENCE shell, and the electrons are called VALENCE electrons
These are the electrons which react with other atoms.

13. Lewis Dot Diagrams
Carbon

14. Lewis Dot Diagrams
Chlorine

15. ISOTOPES
atoms of the same element that HAVE A DIFFERENT NUMBER OF NEUTRONS
Some isotopes are radioactive. This means that their nuclei is unstable and will break down at a CONSTANT RATE over time.
There are several practical uses for radioactive isotopes:
CARBON DATING
TRACERS
KILL BACTERIA / CANCER CELLS

16. COMPOUNDS
a substance formed by the chemical combination of 2 or more elements in definite proportions
Ex: water, salt, glucose, carbon dioxide
H20
CO2
NaCl

17. Inorganic - usually "support" life
TWO TYPES OF COMPOUNDS
Organic - Contain C, H, and O in some ratio (usually referred to as chemicals of life)
Carbohydrates, Proteins, Lipids, Nucleic Acids
Inorganic - usually "support" life

18. Chemical bonds hold the atoms in a molecule together.
There are 2 types of chemical bonds IONIC and COVALENT

19. The Periodic Table Atoms generally want a FULL valence shell!
Column 1  1 outer electron, forms a 1+ charge
Column 2  2 outer electrons, forms a 2+ charge
Column 3  3 outer electron, forms a 3+ charge
Column 4  4 outer electrons, no charge, covalent bonding
Column 5  5 outer electron, forms a 3- charge
Column 6  6 outer electrons, forms a 2- charge
Column 7  7 outer electron, forms a 1- charge
Column 8  8 outer electrons, neutral, no charge
The middle
section of transition metals fits here. It is NOT important for our biology lesson.

20. - one atom donates an electron to another atom
There are two types of chemical bonds:
1. Ionic Bonding
- one atom donates an electron to another atom
positive ion (lost electrons)
negative ion (gained electrons)

22. Covalent Bonding
involves sharing electrons
between atoms
VIDEO:

23. Water is essential to living systems
Water is made up of polar molecules.
-ve
“Hydrogen Bonding”
+ve

24. Water Solutions
Why is water important?

25. Water regulates temperature

26. Water expands as it freezes

27. Water participates in life’s chemical reactions
Cellular respiration Photosynthesis

28. Water is cohesive

29. Water dissolves many substances

30. So stay hydrated!!!
Hydrated 
Dehydrated 

31. A universal solvent
Water is known as the universal solvent because is dissolves many substances
Substances are divided into two categories based on whether or not they dissolve

32. Hydrophilic Substances
Dissolve well in water
Ex. Sugar, salt
‘hydrophilic’ means “water-loving”
These substances are made of polar molecules or ions
Ex. Sugar (sucrose) and table salt

33. Hydrophobic Substances
Do not dissolve well in water
Dissolve well in other hydrophobic substances
Ex. Vitamins ADEK – fat soluble
‘hydrophobic’ means “water-fearing”
Hydrophobic materials often protect against water

34. MIXTURES
Water is not always pure. It is often found as part of a mixture.
A mixture is a material composed of TWO OR MORE ELEMENTS OR COMPOUNDS THAT ARE PHYSICALLY MIXED
Ex: salt & pepper mixed, sugar and sand – can be easily separated

35. SOLUTION
Two parts:
SOLUTE – SUBSTANCE THAT IS BEING DISSOLVED (SUGAR / SALT)
SOLVENT - the substance in which the solute dissolves
Materials that do not dissolve are known as SUSPENSIONS.
Blood is the most common example of a suspension.
Cells & other particles remain in suspension.

36. FORMULA
The chemical symbols and numbers that compose a compound ("recipe")
Structural Formula – Line drawings of the compound that shows the elements in proportion and how they are bonded
Molecular Formula – the ACTUAL formula for a compound
C2H6O

37. ACIDS & BASES
Acids: always (almost) begin with "H" because of the excess of H+ ions (hydrogen)
Ex: lemon juice (6), stomach acid (1.5), acid rain (4.5), normal rain (6)
Facts about Acids
Acids usually taste SOUR.
You eat acids daily (coffee, vinegar, soda, spicy foods, etc…)

38. Bases usually feel SLIPPERY to touch and taste BITTER.
ACIDS & BASES
Bases: always (almost) end with -OH because of the excess of hydroxide ions (Oxygen & Hydrogen)
EX: oven cleaner, bleach, ammonia, sea water, blood, pure water
Facts about Bases
Bases usually feel SLIPPERY to touch and taste BITTER.

39. Neutralization Reactions
When an acid reacts with a base to produce a salt and water.

40. pH SCALE measures degree of substance alkalinity or acidity
Ranges from 0 to 14
0 – 5 strong acid
6-7 neutral
8-14 strong base