Tuesday 03/26/2013: CHARACTERISTICS OF MATTER and SOLUTIONS Review

General/Background Information

PHYSICAL PROPERTY: characteristic of matter that can be observed or measured without changing the sample’s composition (e.g. color, state, melting point, boiling point, density).

PHYSICAL CHANGE: any change that alters the size or amount of a substance without changing the sample’s composition.

CHEMICAL PROPERTY: characteristic of matter that describes its "potential" to undergo some chemical change or reaction (e.g. reactivity with other substances, potential to ignite or explode, remains unchanged in the presence of water).

CHEMICAL CHANGE: the ability of a substance to combine with or change into one or more other substances (a new substance is formed).

INTENSIVE PROPERTY: [physical] does not depend upon the sample size and can be used to identify substances (e.g. color, odor, luster, malleability, ductility, conductivity, hardness, melting/freezing point, boiling point, density).

EXTENSIVE PROPERTY: [physical] depends upon sample size and cannot be used to identify substances (e.g. mass, volume, state).

PURE SUBSTANCE: element or compound

MIXTURE: physically mixed – heterogeneous or homogeneous

Using the above information and your prior knowledge, complete the following charts with a check mark (P) in the proper column(s).

STATE OF MATTER / Solid / Liquid / Gas
1.Definite shape & volume
2.
3. No definite shape or volume
4. Particles vibrate in place
5.
6. Particles move extremely fast and in a straight line until they “bump” into each other or the sides of the container.
7.
8. Particles able to move around each other, but still attracted to each other
9. Tight packing of particles makes it incompressible
10. Definite volume, but not shape
11. Virtually incompressible because of the way particles move around each other
12. Space between particles allow compressibility

Only one checkmark per change or property of matter for the tables below:

CHANGES IN MATTER / Physical / Chemical / PROPERTY OF MATTER / Chemical / Physical (intensive) / Physical (extensive)
Boil / Blue solution
Crumple / Turns blue in air
Crush / 32 grams of silver
Explode / Shaped into sheets
Burn / Bubbles when mixed
Ferment / 13.5 g/cm3
Freeze / Boils at 357ºC
Grind / Gets COLD when mixed
Condense / White powder
Melt / Conducts heat
Oxidize / Colorless gas
Rot / Melts at 185ºC
Corrode / 14 mL green liquid
Rust / Melting point
Tarnish / Length
Vaporize / Yellow solid

For the following problems(Only one check mark per sample of matter)

CLASSIFICATION OF MATTER / Pure Substance / Mixture
Element / Compound / Heterogeneous / Homogeneous
Aluminum chloride
Air
Iron
CuCl2(aq)
CuCl2(s)
Vinegar & Oil
Sodium
NaCl(s)
Steel
Hot tea
Iced tea
Penny ($0.01)
H2O
Water vapor
Muddy water
Ammonia - NH3(aq)
Cough syrup

Solutions EOC review

Solubility Rules Chart

Solubility Rules for Ionic Compounds in WATER
This information is also found in the back of the EOC periodic table
Compounds / Solubility / Exceptions
Salts of alkali metals and ammonia / Soluble / Some lithium compounds
Nitrate salts and chlorate salts / Soluble / Few exceptions
Sulfate salts / Soluble / Compounds of Pb, Ag, Hg, Ba, Sr, and Ca
Chloride salts / Soluble / Compounds of Ag, and some compounds of Hg and Pb
Carbonates, phosphates, chromates, sulfides, and hydroxides / Most are Insoluble / Compounds of the alkali metals and ammonia
Student Practice
Directions: Identify whether the following are soluble or insoluble in water.
Chemical Formula Name Solubility
1. NH4CH3COO Ammonium acetate ______
2. Ba(OH)2 Barium hydroxide ______
3. FeCO3 Iron (II) Carbonate ______
Directions: Answer the following.
1.  Why does grinding up a solid into smaller pieces speed up the dissolving of a solid in liquid?
2.  You can make most solids dissolve faster in a liquid by ______the temperature.
3.  You can make most gases dissolve faster in a liquid by ______the temperature.
4.  (a) Explain why a bottle of soda fizzes when you first open it. (b) How is pressure affecting the solubility of carbon dioxide gas?

Types of Solutions

On a solubility curve, the lines indicate the concentration of a ______solution - the maximum amount of solute that will dissolve at that specific temperature.

Values on the graph (above/below) ______a curve represent unsaturated solutions - more solute could be dissolved at that temperature.

Values on the graph (above/below)______a curve represent supersaturated solutions- contains more dissolved solute than a saturated solution at the same temperature.

Label the following solutions as saturated or unsaturated. If unsaturated, write how much more solute can be dissolved in the solution.

Solution / Saturated, Unsaturated, Supersaturated?
a solution that contains 70g of NaNO3 at 30°C (in 100 mL H2O)
a solution that contains 50g of NH4Cl at 50°C (in 100 mL H2O)
a solution that contains 20g of KClO3 at 30°C (in 100 mL H2O)