Chapter 3: States of Matter - Manchester High School 3.pdf · Section 1: Matter and Energy Kinetic...

S E C T I O N 1 : M A T T E R A N D E N E R G Y

S E C T I O N 2 : F L U I D S

S E C T I O N 3 : B E H A V I O R O F G A S E S

Chapter 3: States of Matter

Section 1: Matter and Energy

Key Terms

Plasma

Energy

Thermal Energy

Evaporation

Sublimation

Condensation


Kinetic Energy

* All matter is made up of atoms and molecules that act like tiny particles

* These tiny particles are always in motion. (High temp. equals faster movement)

* At the same temp, more massive particles move slower then less massive particles.


The states of matter are physically different

Solids - particles are in a fixed position

Liquids - closely packed, but they can still slide past each other

Gases - particles are in a constant state of motion


Solids have a definite shape and volume

Solids do not need a container to keep its shape

Particles in solids have almost no freedom to change position, but they vibrate.


Solids are divided into two categories

1. Crystalline - have an orderly arrangement of atoms or molecules

(Ex. Iron, diamonds, and ice)

2. Amorphous - composed of atoms or molecules that are in no particular order. Each particle is in a particular place, but the particles are not in an organized pattern.

(Ex. Wax and rubber)


Liquids change shape, not volume

Liquids have a definite volume, but change shape.

Particles in a liquid move fast enough to over come the forces of attraction between them.


Besides volume, another property of a liquid is surface tension.

Surface tension is the force acting on the particles at the surface of a liquid that cause a liquid, such as water, to form spherical drops.

Gases are free to spread in all directions

Gases expand to fill the available space. They change both shape and volume.


When gases are placed into a bottle, they are forced together. Once thy are released, they fill the available space.

Plasma is the most common states of matter.

Scientist estimate that 99% of the known matter is made up of plasma


Plasma is the state of matter that does not have a definite shape and in which the particles have broken apart.

Plasma also conducts electric currents

Natural plasmas are found in lighting, fire, and aurora borealis.


How is the glow of fluorescent lights caused?

By artificial plasma, which is formed by passing electric currents through gases.


Energy’s Role

Energy is the capacity to do work

Thermal energy is the total kinetic energy of a substance

All matter is made up of particles (atoms and molecules) that are in constant motion


Thermal energy is the kinetic energy of a substance’s atoms

At higher temperatures, particles of matter move faster. The more kinetic energy the greater the objects thermal energy.

Thermal energy also depends on the number of particles in a substance.


Temperature is a measure of average kinetic energy

The more kinetic energy the higher the energy

Since particles of matter are in constant motion, and not all particles are moving at the same speed, you measure the average kinetic energy.


Energy and Change of State

A change of state is the conversion of a substance from one physical form to another.

When we talk about change of state, the substance does not change only the energy changes.


Increase energy the particles move faster

Decrease energy the particles move slower

The temperature of a substance is a measure of energy

Solid Liquid Gas


Solid to Liquid = Melting

Liquid to Gas = Evaporation

Gas to Liquid = Condensation

Liquid to Solid = Freezing

Solid to Gas = Sublimation


Some changes of state require energy

Changes that require energy are called endothermic changes.

Evaporation is the change of a substance from a liquid to a gas


Boiling point is the temperature at which a liquid changes to a gas and is a characteristic property

Solids can also change to gases this is called sublimation.


Energy is released in some change of state

Changes that release energy are called exothermic changes

When water freezes or a gas becomes a liquid are examples of releasing energy

Condensation is the change of a substance from a gas to a liquid.


Temperature change verses change in state

Temperatures do not change during a state of change.


Conservation of Mass and Energy

Mass cannot be created or destroyed

Both in a chemical or a physical change, the total mass of matter stays the same before and after the change.


Matter changes but the total mass stays the same.

Energy cannot be created or destroyed.

Energy may be converted to another form during a physical or chemical change, but the total amount of energy present before and after the change is the same.

Section 2: Fluids

Key Terms

Fluid

Buoyant Force

Pressure

Archimedes’ Principle

Pascal

Pascal’s Principle

Viscosity

Section 2: Fluids

Fluids

Since both liquids and gases have the ability to flow they are referred to as fluids.

Fluids are able to flow because their particles can move past each other easily

Section 2: Fluids

Buoyant Force

Is the upward force that fluids exert on matter

What determines if something will float or sink?

Density and the buoyant force

Section 2: Fluids

Buoyancy explains why objects float

All fluids exert pressure, which is the amount of force exerted on a given area

Pressure of all fluids increase as the depth increases

Section 2: Fluids

Determining Buoyant Force

Archimedes’ principle states that buoyant force on an object in a fluid is an upward force equal to the weight of the fluid that the object displaces.

Section 2: Fluids

An object will float or sink based on its density

Since steel is almost eight times denser than water how do ships float?

Ships float because of their hollow shape. Remember that density equals mass

divided by volume.

Section 2: Fluids

Fluids and Pressure

Pressure is the amount of force exerted per unit area of a surface. The SI unit for pressure is Pascal (Pa)

Pressure is calculated by dividing force by the area.

Pressure = force/area (1 Newton/m2)

Section 2: Fluids

Fluids exert pressure evenly in all directions.

Pascal’s principle states that a change in pressure at any point in an enclosed fluid will be transmitted equally to all parts of the fluid

Hydraulic devices are based on Pascal’s principle. These devices use liquids to transmit pressure from one point to another.

Section 2: Fluids

Why are liquids used instead of gases?

Because liquids cannot be compressed or squeezed into a smaller place. Liquids transmit pressure more efficiently.

Section 2: Fluids

Fluids in Motion

Fluids move faster through smaller areas than through larger areas, if the overall flow rate remains constant

Viscosity is resistance to flow

Section 2: Fluids

Fluid pressure decrease as speed increases

Bernoulli’s principle states that as the speed of a moving fluid increases, the pressure of the moving fluid decreases.

Section 3: Behavior of Gases

Key Terms

Boyle’s Law

Charles’ Law

Gay-Lussac’s Law


Behavior of Gases

Gases are often forgotten because they are colorless and odorless. However, gases are very important


Properties of Gases

No definite shape or volume

Particles move rapidly in all directions

Fluids

Molecules are in constant motion, and they frequently collide with one another and with the walls of their container

Low density

Compressible

Spread out easily and mix with one another. Mostly empty space


Gases exert pressure on their containers

Gas under pressure will escape its container if possible


Gas Laws

The volume of a gas is the same as the volume of its container but there are other factors, such as pressure, to consider

The gas law describes how the behavior of gases are affected by pressure and temperature


Boyle’s Law relates the pressure of a gas to its volume

Boyle’s Law states that for a fixed amount of gas at a constant temperature, the volume of a gas increases as its pressure decreases, or the volume of a gas decreases as its pressure increases


Boyle’s Law

Pressure Volume

Pressure Volume


Charles’ Law relates the temperature of a gas to its volume

Charles’ Law states that for a fixed amount of gas at a constant pressure, the volume of gas increase as its temperature increases and the volume of a gas decreases as its temperature decreases


Charles’ Law

Temperature Volume

Temperature Volume


Gay-Lussac’s Law relates gas pressure to temperature

As temperature increases, the kinetic energy of the gas particles increase

Gay-Lussac’s Law states that the pressure of a gas increases as the temperature increases if the volume of the gas does not change


What does this mean?

If a pressurized container that holds gas is heated it may explode.

Chapter 3: States of Matter - Manchester High School 3.pdf · Section 1: Matter and Energy Kinetic...

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