Physical Science Properties of Matter, Solutions, Acids and Bases EOCT Review
1. Phase Changes Compare and contrast the atomic/molecular motion of solids, liquids, gases, & plasma.
A)Solids = vibrate; highly packed together; ______kinetic energy
B)Liquids= flow over each other; _____definite shape; more kinetic energy than solids
C)Gases = move everywhere; _____ definite volume or shape; highest kinetic energy
D)Plasma = gas that has been so energized that its atoms have been stripped of all or some of its electrons
E)Water is unique because in its solid state the molecules are a more open structure that is less ______than that of liquid state.
F)Particles in a gas, are moving very quickly and their only contact is when they collide.
G)During phase changes, the temperature stays the same but the energy decreases
H)When a flame symbol is on a bottle, it means the substance in the bottle is flammable
I)Evaporation is the process of a ______changing to a ______
Fill in the blanks:
- as temperature increases, the motion of the atoms ______
- describing a solid as a composition of particles closely situated in position giving a definite shape and definite volume and that little motion occurs between particles as compared to other phases of matter
- describing a liquid as a composition of particles free to move, giving a definite ______but not a definite ______and that particles have a ______range of motion as compared to solids
- describing a gas as a composition of particles that move more than the particles of either a solid or a liquid, giving no definite volume or shape, and colliding more randomly than the particles of solids and liquids
- Pressure is the ______exerted on a surface per unit area
2. Physical And Chemical Properties of Matter
J)Physical property/change = observable properties by the senses Physical property examples: boiling point, color, conductivity, density, malleability, mass, melting point, odor, shape, state of matter, weight.
K)Chemical property/change = characterizes how matter changes into entirely new substances.
L)Chemical property examples: ability to burn, ability to corrode, ability to support burning, reactivity with chemicals, reactivity w/light.
3. Relate temperature, pressure, and volume of gases to the behavior of gases.
A)Boyle’s law = inverse relationship between pressure and volume; hyperbola graph
B)Charles’ law = direct relationship between temperature and volume; straight-line graph
C)Gay-Lussac’s law = direct relationship between temperature and pressure; straight-line graph; the warmer something is the higher the pressure
4. Calculating heat capacity:understanding that phase changes require a gain or loss of energy
Q = m x Cp x Δt
Quantity of heat energy = mass x Specific Heat x Change in temperature
5. Solutions: Describe solutions in terms of solute/solvent, conductivity,& concentration.
A)Solute = ______in solution. Solvent = substance the solute is dissolved __
B)Mixing a powdered drink- makes the powder the solute and water the solvent
C)Increase in temperature causes solids to go into solution ______
D)______= solution holds all the solute it can
E)______= solution can hold more solute
F)______= solution holds more solute than normal.
G)______= less solute in solvent
H)______= more solute in solvent
I)Weak acids and bases are weak electrolytes in solution.
J)Strong acids and bases are strong electrolytes in solution.
K)Nonelectrolytes______conduct at all.
2)Observe factors affecting the rate a solute dissolves in a specific solvent.
A)As the temperature decreases, a solid ______its ability to go into solution
6. Demonstrate that solubility is related to temperature by constructing a solubility curve.
A)Solids ______solubility with temperature.
B)Gases ______solubility with temperature.
C)Solubility curve = shows the amount of dissolved solute changes with temperature.
Conductivity is the measure of a solution’s ability to conduct ______
Ionic compounds and acids yield solutions with high conductivity. A solution that conducts electricity is called an ______…if it does not it is called a nonelectrolyte.
**As the increase of OH- and H+ ions occur in a solution, the conductivity increases.
How can you make a substance dissolve faster?
1-______
2-______
3-______
Solubility Curves:Shows how the amount of dissolved solute changes with temperature (picture above)
Questions:
1)How much KCl is needed to make a saturated solution in 100g of water at 70 degrees? ______
2)How much KCl is needed to make a saturated solution in 200g of water at 10 degrees? ______
3)Is this saturated solution or an unsaturated solution: 20g of KCL in 100g of water at 30 degrees? ______
6. Acids and Bases: Compare& contrast the components and properties of acids and bases.
A)Acids = pH less than ___; litmus = ______.
B)Bases = pH more than ___; litmus = ______.
C)Taste = acids – tart or sour; bases – bitter.
D)Touch = acids – feel like water or may sting; bases – feel slippery or smooth.
E)Reaction with metals = acids react; bases don’t react.
F)Conductivity = both conduct electricity.
G)Litmus test = Acids turn blue litmus red; Bases turn red litmus blue.
H)Acids give off hydrogen ions (____) in solution.--Bases give off hydroxide ions (______) in solution.
I)Neutralization = reaction where acid and base react and form a salt and water.
J) Determine whether common household substances are acidic, basic, or neutral.
K) Soaps and cleaners are ______Juices and fruits are ______.