1. Types of Matter

2. Types of Matter
All the matter in the universe is made up of particles.
2 general categories:
Pure substances
Elements
Compounds
Mixtures
Homogenous Mixtures
Heterogeneous Mixtures

3. Pure Substances
Made of only one kind of matter and has definite properties.
Every sample of a pure substance is the same.
2 kinds of Pure Substance:
Elements
Atoms – Neon (Ne)
Molecules – Oxygen (O2)
Compounds
Molecules – Water (H2O)
Ions – Sodium Chloride (NaCl)

4. Elements
Elements are pure substance that cannot be broken down into other substances.
Composed of atoms - the most basic units of matter.
All matter in the universe is composed of atoms.
Atoms are single units.
Neon (Ne)
Molecules are two atoms
of the same kind combined.
Oxygen (O2)

5. Compounds
A substance made of two or more elements that are chemically combined.
Have a definite ratio

6. Elements in a Compound
Water = H2O
2 Hydrogen (H)
1 Oxygen (O)

7. Compounds
Properties of a compound are always different from the properties of the elements that form them.
Carbon (C) = powdery black solid
Hydrogen (H) = invisible gas
Oxygen (O) = invisible gas
C12H22O11
(Table Sugar)

8. Mixtures
Two or more substances that are in the same place but are not chemically combined.
The individual substances keep their separate properties.
Sugar in lemonade may not be visible but you can taste it!
Can be separated.
Evaporation, separation, boiling
No definite ratio
Salt Water
Blood

9. Parts of a Mixture Solute – What is being dissolved.
Solvent – What is doing the dissolving (water)
Concentration – The amount of solute in a solvent.
Solution
Solute
Solvent
Salt Water
Salt
Water
Lemonade
Lemonade Mix

10. Mixtures Homogenous Mixtures: 2. Heterogeneous Mixtures: Solution
Evenly distributed
1 solute in a solvent
2. Heterogeneous Mixtures:
Suspension
Not evenly distributed
Multiple solutes in a solvent
Blood
(RBC + WBC +
Platelets + Plasma)
Salt Water
(NaCl + H2O)

11. Solubility
How well a type of matter can dissolve in a solvent is called solubility.
Two factors affect the rate at which solutes dissolve in solvents:
Temperature
The higher the temperature of the liquid solvent, the more solute can be dissolved.
The higher the temperature of a gas solvent, the less solute can be dissolved.
Pressure
The greater the pressure of the solvent, the more solute can be dissolved.

12. Solubility Curve Water NaNO3, NH4Cl, KClO3 45g 30°C
What is the solvent in this experiment?
What are the solutes?
At 75°C, how much KClO3 has dissolved?
90g of NaNO3 will dissolve at what temperature?
What is the relationship between the temperature of the water and the amount of solute that can be dissolved?
Water
NaNO3, NH4Cl, KClO3
45g
30°C
Higher the temperature, more solute dissolves