Mix and Flow of Matter Flashcards
Name and describe the three phases of matter
The three phases of matter are:
Solid: Particles are tightly packed, giving solids a fixed shape and volume. Example: ice.
Liquid: Particles are close but can move, so liquids take the shape of their container but keep the same volume. Example: water.
Gas: Particles are far apart and move freely, so gases have no fixed shape or volume and fill any container. Example: steam.
What is the “Particle Model of Matter”, what do we use it for
The Particle Model of Matter explains that all matter is made of tiny particles in constant motion, with forces of attraction between them. This model helps us understand changes in state (solid, liquid, gas), how temperature affects matter, and how substances interact, like dissolving or mixing.
Understand the 5 key ideas of the “Particle Model of Matter” – what is the main point of each key idea?
The Particle Model of Matter key ideas:
- Matter is made of particles.
- Spaces exist between particles.
- Particles are always moving.
- Heat makes particles move faster.
- Particles attract each other.
These ideas explain how particles behave in different states and when changing states.
Draw a diagram showing how the particles in each phase of matter are arranged
Name the process required to change back and forth between each phase of matter
Melting: Solid to Liquid
Freezing: Liquid to Solid
Vaporization: Liquid to Gas
Condensation: Gas to Liquid
Sublimation: Solid to Gas (Skips liquid phase)
Deposition: Gas to Solid (Skips liquid phase)
Describe what happens to the temperature of a substance when it is heated and undergoes all three phase changes – as you add heat, what happens to the temperature and phase of the substance?
The substance starts as a solid and begins to vibrate more as you add heat, until it reaches melting point, where it becomes a liquid. then as the heat continues to rise, the liquid reaches the boiling point where it begins to become gas.
Draw a flow chart including the 7 classifications of matter and understand what each one means
Pure Element: Substance that only has one type of atom
Pure Compound: Substance that has 2 or more types of atoms chemically combined in fixed proportions
Mixtures
—————————-
Colloid: Cloudy mixture
Suspension: A mechanical mixture that will separate over time
Mechanical: A mixture where you can clearly see the different parts
Solution: A mixture where you cannot clearly see the different parts
What is a pure substance? What are the two types of pure substances? Explain what a pure substance is using the particle model of matter
Pure substances have a uniform composition. There are Pure Compounds and Pure Elements. Pure element has only one type of atom whereas Pure compounds have 2 or more types of atoms in the composition
List the three types of mixtures
Mechanical Mixture
Suspension Mixture
Colloid Mixture
What are the characteristics of a homogeneous mixture? What example of homogeneous mixture did you make in the lab?
Homogeneous mixtures (Solutions or Colloids) have the same composition throughout the whole mixture
What are the characteristics of a heterogeneous mixture? Name some examples discussed in class
A Heterogeneous mixture has multiple parts which are all clearly visible. Things like salads, asphalt, and cereal are all heterogeneous.
Define the three types is “in-between” mixtures, name an example for each
What type of mixture is a solution? What is a solute? What is a solvent? What does dissolve mean?
Use the particle model of matter to explain how a solute dissolves into a solvent
List the factors that affect the rate of dissolving, and describe how each affects the rate of dissolving
Define “concentrated” and “dilute” solutions
What is the concentration of a solution?
Is it a qualitative or quantitative observation?
How is it calculated? For our purposes, what are the units?
What condition must be met in order to compare the concentration of two solutions?
Calculate the concentrations of the following salt solutions. Which salt solution is the most concentrated? Which is the most dilute (least concentrated)?
10 g of salt in 100mL of water
20 g of salt in 100mL of water
5 g of salt in 100mL of water
Concentration = mass of solute (g) / volume of solution (mL)
Most concentrated: 20 g in 100 mL (0.2 g/mL)
Most dilute (least concentrated): 5 g in 100 mL (0.05 g/mL)
Calculate the concentration of sugar in of the following solutions. Which sugar solution is the most concentrated? Which is the most dilute (or least concentrated)?
5 grams of sugar in 25 mL of water
20 grams of sugar in 200 mL of water
10 grams of sugar in 500 mL of water
Concentration = mass of solute (g) / volume of solution (mL)
Most concentrated: 5 g in 25 mL (0.2 g/mL)
Most dilute (least concentrated): 10 g in 500 mL (0.02 g/mL)
Use the particle model of matter to define saturated, unsaturated, and supersaturated solutions. How are they made in the lab? What key observation are you looking for when making each solution? What key conditions must be held constant when making them?
What is the “solubility” of a solute? Is it a qualitative or quantitative observation? How is it calculated and what are the units?
What conditions must be met when comparing the solubilities of different solutes? What happens to the solubility of a solute when the temperature changes, when the solvent changes
Calculate the solubility of the following saturated solutions of solute in water at room temperature:
17.5 g of sugar in 25 mL of water
20.0 g of baking soda in 200 mL of water
3.0 g of salt in 10 mL of water
Solubility = mass of solute (g) / volume of solution (mL) x 100 mL
Sugar: 70 g/100 mL
Baking soda: 10 g/100 mL
Salt: 30 g/100 mL
Define soluble vs insoluble
What is a fluid? List the properties of a fluid
Define viscosity. Explain viscosity using the particle model of matter. What observation do we use to assess a fluid’s viscosity?
What is the effect of temperature on the viscosity of a liquid? Use the particle model of matter to explain. How is viscosity related to temperature for liquids?
What is the effect of temperature on the viscosity of a gas? Use the particle model of matter to explain. How is viscosity related to temperature for gases?
Define density. Explain the density of different phases of a substance using the particle model of matter. How is density calculated? What are the units for density?
How can the density of a substance be changed?
Explain why different substances have different densities using the particle model of matter.
Describe how to calculate the density of a regular solid, of an irregular solid. What are the units for density of a solid?
Describe how to calculate the density of a liquid, of a gas. What are the units for density of a fluid (liquid or gas)?
Calculate the following densities:
A brick measures 30cm by 10cm by 15cm and has a mass of 850g.
A rock displaces a volume of water of 150 mL and has a mass of 125g.
A glass of orange juice has a volume of 300mL and has a mass of 375g.
Density = mass / volume
Brick: 0.189 g/cm³
Rock: 0.833 g/cm³
Orange juice: 1.25 g/mL
Define buoyancy of a fluid. What does the buoyancy of a fluid depend on?
What is gravity? What is mass vs weight? Why do we weigh less on the moon compared to here on earth?
What principle can be used to measure buoyancy? Define Archimedes’ Principle.
Which volume of displaced water would weigh more, 100mL or 200mL?
Which volume of water would exert the stronger buoyant force, 100mL or 200mL?
Define positive vs neutral vs negative buoyancy. How does the weight of the displaced fluid compare to the weight of the object? How does the density of the fluid compare to the density of the object?
Explain why certain objects float in water while others sink.
Describe examples of buoyancy in everyday life.
Can you explain why you can float more easily in the ocean than in a lake?
Can you explain why a ship will float on the ocean while a steel rod will sink?
What is the force acting on you or the ship? How can you measure the size of this force?
If you were an engineer, what would you have to ensure so that an object won’t sink?
Define compressibility of fluids. Using the particle model of matter, explain why gases are compressible while liquids are not. How do compressed gases and liquids transmit pressure?
Define pressure. What is the formula for pressure? What are the units for pressure?
How can pressure make an applied force greater?
What is Pascal’s Law? What is a hydraulic system? What is a pneumatic system? What are they used for? What decreases the efficiency of these systems?
