1. Properties of Matter
Review Answers

2. 1. Hope you reviewed all of your vocabulary flashcards!!!
2. a. physical change
b. chemical property
c. physical change
d. chemical property
e. physical property
f. chemical change

3. 3. D Closer to 7 the weaker the solution
4. B
5. A Farther from 7 the stronger solution
6. C
7. pure water (Very rare to have pure H2O)

4. 8. Diffusion cannot take place in a solid substance because it can only occur in fluids (liquids and gasses) where the molecules can move freely.
9. Oil (C6H14) will not dissolve in water because it is a covalent compound and it has neutral charges. Covalent compounds do not have charges that the Polar water molecules can attract to pull the substance apart.

5. 10. When a chemical change occurs a totally new substance with different chemical and physical properties is created. The evidence that a chemical change occurred includes smoke, flame/sparks, gasses are produced, a temperature change (colder or hotter), and formation of new substances.
During a physical change only physical properties are altered. The substance remains the same.

6. 11. Kinetic Theory (4 Parts)
All matter is composed of atoms and molecules that behave like tiny particles that are always in motion.
2. If you increase the temperature of these tiny particles they will move faster.
3. At the same temperature, the more massive particles will move slower than the less massive particles.
4. Particles move from and area of high concentration to and area of low concentration until equilibrium is reached.

7. 12. If I burn a match, the mass of the products will always be equal to the mass of the reactants.
13. I know this because the Law of Conservation of Mass states that mass cannot be created or destroyed. Mass can change forms!

8. 14. NaCl, CaCl2, Al2S3 (Any ionic compounds).
15. Ionic compounds break up easily in water because they are made up of ions which have charged particles. Covalent compounds are not made up of charged particles and do not typically break up in water. In order for electric current to flow (conductivity) there needs to be charged particles present.

9. 16. From the list below decide if each is an Intrinsic or Extrinsic property. Write “I” for intrinsic and “E” for extrinsic.
a. Weight= extrinsic
b. Odor= intrinsic
c. Volume= extrinsic
d. Mass= extrinsic
e. Hardness= intrinsic
f. Malleable= intrinsic

10. 17. In sections B and D phase changes are
occurring and the energy is being used to weaken/strengthen bonds or break/reform bonds.
18. At section “B” you have melting when energy increases and freezing when energy decreases.
At section “D” you have evaporation when energy increases and condensation when energy decreases.
19. A=solid, C= liquid, E= gas

11. 20. Bromine would have 7 valence e-, tends to gain 1e- so it would form ions with the oxidation # -1, would most likely form compounds with H+1 or any other +1 ions, is a non-metal, will not conduct electricity, is either a liquid or gas at room temp., has a low M.P. and B.P., it has 4 energy shells and is highly reactive.

12. Most are liquids or gases @ room temp.
21.
Metals
Non-Metals
Conductive
Non-Conductive
High M.P. and B.P.
Low M.P. and B.P.
Malleable / Ductile
Brittle
Luster
Dull
room temp.
Most are liquids or room temp.

13. 22.
liquid gas (throughout) =
gas liquid =
solid liquid =
liquid solid =
liquid gas (surface) =
solid gas =
vaporization
condensation
melting
freezing
evaporation
sublimation

14. 23.-25. Solid Strong Bonds Low Energy Gas No Bonds High Energy Liquid
Medium bonds
Medium Energy
Plasma
Few bonds
Very High Energy

15. 22. If a block of copper measures 2. 00 cm wide x 4. 00 cm long x 5
.   If a block of copper measures 2.00 cm wide x 4.00 cm long x 5.00 cm high and weighs 356 g, What is its’ density? Use DUFAs to solve
Volume= 40 cm3 mass 356 g D=M/V
Density= 8.9 g/cm3

16. 23. What is the mass of 8.20 mL sample of mercury, if the density of mercury is 13.6 g/ml? Use DUFAs to solve.  
Volume=8.20 ml D= 13.6 g/mL Mass=D x V
Mass= g

17. Energy Level of Molecules Strength of Bonds Between Molecules
23.
State of Matter
Energy Level of Molecules
Strength of Bonds Between Molecules
Solid
Lowest
Strongest
Liquid
Medium
Gas
Highest
Weakest