Classification of Matter
Properties and Changes
Kinetic Molecular Theory
Particle Drawings
Gas Laws
Phase Diagrams
100
The definition of matter.
Anything that is made of atoms, has mass, and takes up space.
100
The definition of the Law of Conservation of Mass.
In a physical or chemical change, mass is neither created nor destroyed.
100
Definition of kinetic molecular theory.
Matter is made up of particles and the particles are always moving.
100
The particles and movement of the particles in a solid, liquid, and gas.
100
The relationships between the following variables (direct or inverse):
- pressure and volume
- volume and temperature
- pressure and temperature
- pressure and volume = inverse
- volume and temperature = direct
- pressure and temperature = direct
100
X-axis and Y-axis on a phase diagram.
X-axis: temperature
Y-axis: pressure
200
The difference between a pure substance and a mixture.
A pure substance only has one type of particle while mixtures have more than one type of particle.
200
An example of the Law of Conservation of Energy.
Potential energy is converted to kinetic energy as you ski down a hill, but energy is not lost.
200
The shape and size of a crystal in comparison to the unit cell.
Larger but the same shape as the unit cell.
200
Diffusion versus effusion.
200
Two real-life examples of Boyle's Law, Charles's Law, or Gay-Lussac's Law. You must identify which laws you are providing examples of.
Boyle's Law: As the plunger on a syringe is pulled, increasing the volume, the pressure decreases, drawing in liquid
Charles's Law: a hot air balloon inflates as the gas inside is heated
Gay-Lussac's Law: the pressure inside an Instant Pot increases as the temperature is increased, cooking your food faster
200
State of matter when the temperature is 400 K and the pressure is 0.5 atm.
Gas.
300
The difference between a compound and a mixture.
Compounds have two or more elements chemically combined while mixtures have two or more pure substances physically combined.
300
Two physical properties and two chemical properties of iron.
Physical properties: size, color, magnetism, hardness
Chemical: ability to rust, ability to react with acid
300
A definition of kinetic energy and how it relates to particles at the same temperature.
Kinetic energy: energy of motion
Particles at the same temperature will have the same kinetic energy (kinetic energy and temperature are directly related).
300
An example of how you could decrease the pressure in a room.
Picture should show: increasing the amount of space, decreasing the number of particles, or decreasing the temperature.
300
If the initial temperature of 3.0 L of a gas is 298 K, at what temperature will the volume increase to 9.5 L?
940 K
300
Location of the triple point (letter, temperature and pressure) and a definition.
D, 273.2 K, 0.006 atm
The point where solid, liquid, and gas coexist in equilibrium.
400
An example of an element, a compound, a homogeneous mixture, and a heterogeneous mixture.
Element: carbon
Compound: H2O
Homogeneous mixture: air
Heterogeneous mixture: fruit salad
400
The difference between intensive and extensive properties plus an example of both for a pencil.
Intensive does not depend on the amount of substance (yellow color). Extensive depends on the amount of substance (mass, length).
400
Three assumptions about gases in kinetic molecular theory.
1. Gases are small, hard, spheres with insignificant volume
2. Gases are in constant, rapid, random motion
3. Collisions between gas particles are perfectly elastic
400
Illustration and description of the movement of the particles in a solution, colloid, and suspension
400
A gas is in a flexible 450 mL container, at a pressure of 1.0 atm and a temperature of 30 oC. If the temperature is decreased to -20 oC, and the pressure is increased to 5.5 atm, what will the volume of the container be?
0.07 L (70 mL)
400
Location of the critical point (letter, temperature and pressure) and what happens past the critical point.
E, 647 K, 218 atm
The sample can no longer become a liquid, instead becomes a supercritical fluid.
500
Three separation methods and and an example of when you would use each one.
Filtration- to separate a heterogeneous mixture of a liquid and solid (ex: sand and water)
Distillation- to separate a homogeneous mixture of two liquids with different boiling points (ex: water and alcohol)
Chromatography- to separate compounds with different polarity (ex: colored ink in a marker)
500
Three physical changes and three chemical changes.
Physical- breaking a toothpick, melting ice, blowing up a balloon.
Chemical- bleaching paper, hard boiling an egg, mixing vinegar and baking soda
500
The difference between a solution and a colloid, how you can tell the difference, and an example of both.
Solutions are homogeneous mixtures while colloids are heterogeneous mixtures.
Solutions will not exhibit the Tyndall effect while colloids will.
Salt water is a solution while jello is a colloid.
500
The velocity of helium gas (He) versus fluorine gas (F2) at the same temperature and the equation explaining why.
Picture should show He moving faster than F2 because of the equation KE = 1/2 mv2
500
What is the volume of a gas canister containing 3.55 moles of hydrogen gas at STP?
AND What are the two assumptions about ideal gases?
78.4 L
- the volume of the gas particles is negligible
- the gas particles do not experience any attractive intermolecular forces
500
Location and names of all the phase changes.
A: sublimation at temperature increases, deposition as temperature decreases
B: melting as temperature increases, freezing as temperature decreases
C: evaporation as temperature increases, condensation as temperature decreases