1. Ch. 6-1: Atoms & Interactions
Biochemistry
Ch. 6-1: Atoms & Interactions

2. Properties of Matter Physical Properties
Properties that do not change the chemical nature of matter
Examples
Color, Smell, Freezing Point, Boiling Point, Melting Point, Polarity, and Density
Physical change – change in its state

3. Properties of Matter Chemical Properties
Properties that DO change the chemical nature of matter
Examples
PH, Combustion, reactivity with water, explosions!
Compounds put together that create a new compound

4. States of Matter Physical Changes Chemical Changes
Change in appearance
Solid, Liquid, Gas
Chemical Changes
Changes properties of matter all together
Ex. Spoiling Milk

5. Properties of Chemical Change
Forms or breaks chemical bonds
Energy is taken (endothermic) or energy is released (exothermic)
One or more new chemical substances are formed
The process is usually difficult to reverse

6. Examples of Chemical Change
Digestion
Photosynthesis
Respiration
Burning
Decomposition

7. Energy and Chemical Change
Any energy an object has because of its position is called Potential energy.
The energy in motion (actual) is called Kinetic energy.

8. Atoms: The building blocks of elements
Atom - smallest particle of an element that has the characteristics of that element

9. Structure of Atoms Protons: Neutron: Electron:
A particle located in the nucleus and has a positive charge
Neutron:
A particle located in the nucleus and has a neutral charge
Electron:
A particle located outside the nucleus and has a negative charge

10. Atoms
An atom that has either gained or lost an electron is called an Ion
Periodic Table
Atomic Mass: how much it weighs
Atomic Number: location on the periodic table (number of protons)
Isotopes: variations in elements based on number of neutrons

11. How to Read the Periodic Table of Elements

12. Atoms Electrons circle the nucleus in Energy Levels
Noble gases all have there outer most electron full of electrons.

13. 2 e-’s inner and 8 e-’s middle and 1 e- in the outer

14. 2 e-’s inner and 4 e-’s outer

15. Mass Number = Protons + Neutrons
Ex. Carbon
The atomic mass of carbon = 12 The atomic # of carbon = 6 = the # of protons
- neutrons = Mass Number - protons - neutrons = = 6

16. Ex: C12 : C 6 neutrons "normal"
Isotopes of an Element
Isotopes - atoms of the same element that have different numbers of neutrons.
Ex: C12 : C neutrons "normal"
C 13 or C14 : C 7 or 8 neutrons isotope

17. Molecules Compound vs. Element An element is made up of atoms
A compound is made up of different elements

18. Mixtures Solution Suspension
Homogenous (same) mixture of components that stay mixed
Sugar or Salt and water
Suspension
Mixture of two substances that may mix right away, but do NOT stay mixed up
Starch and water

19. Mixtures
Colloid
A suspension of small particles that are dispersed into another substance
Milk, foams
Paint,

20. Medium / Phases Dispersed phase Gas Liquid Solid Continuous medium
NONE (All gases are mutually miscible)
Liquid aerosol Examples: fog, mist, hair sprays
Solid aerosol Examples: smoke, cloud, air particulates
Foam Example: whipped cream, Shaving cream
Emulsion Examples: milk, mayonnaise, hand cream
Sol Examples: pigmented ink, blood
Solid foam Examples: aerogel, styrofoam, pumice
Gel Examples: agar, gelatin, jelly, opal
Solid sol Example: cranberry glass

21. Bonds
Ionic Bond
Sending an electron to an atom that is positively charged (opposing charges attract)
EX.
Na (+) = Cl (-)
Salt
H (+) = Cl (-)
Hydrochloric Acid

22. Types of Bonds Cation- Anion –
A positivily charged ion (more protons than electrons)
Anion –
Negatively charged ion that contains more electrons in its outer shell compared to the protons.

24. Bonds Covalent Bonds Sharing of electrons for the benefit of both EX.

25. Biochemistry
Ch. 6-2: Water & Diffusion

26. Properties of Water Polarity of water
Molecule with unequal distribution of charge.
Allows for cohesion of other water molecules
Allows water to dissolve many compounds
Ions and polar molecules easily dissolve in water

27. Bonds Hydrogen Weaker bond
It is the type of bonds that hold our DNA molecules together.
Must include a Hydrogen molecule
Causes water to expand when freezing

28. Properties of water Water Cohesion-
Water molecules binding to other water molecules
Hydrogen bonds attracted to each other and stick together!
Ions and polar molecules easily dissolve in water. The water molecules surround and separate the solute being dissolved.

29. Movement of Molecules discovered by Brown Called “Brownian Motion”.
Diffusion
The net movement of molecule from an area of high concentration to an area of low concentration.