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UNIT 2 Physical Properties of Matter

Describe the properties of gases, liquids, solids, and plasma.

Use the Kinetic Molecular Theory to explain properties of gases.

Explain the properties of liquids and solids using the Kinetic Molecular Theory.

Explain the process of melting, solidification, sublimation, and deposition in terms of the Kinetic Molecular Theory.

Use the Kinetic Molecular Theory to explain the processes of evaporation and condensation.

Operationally define vapour pressure in terms of observable and measurable properties.

Operationally define normal boiling point temperature in terms of vapour pressure.

Interpolate and extrapolate the vapour pressure and boiling temperature of various substances from pressure versus temperature graphs.

Personal Response SheetAnswer the following questions below as best you can. During this topic of study you will revisit these questions and answer them again and by doing so be able to gauge your learning development.

1. Why does water evaporate faster on a warmer day than a colder day?

The increase in heat means that the particles have more kinetic energy. By having more kinetic energy, the IMF’s can be broken, causing the water to evaporate.

2. Perfume is placed in a sealed plastic bag so well that it can’t escape through the seal. When you smell the bag you can smell the perfume. Why can you still smell the perfume?

The perfumes particles are so small that they are able to diffuse through the tiny holes in the plastic bag. The particles want to move from an area of high concentration to an area of low concentration.

3. Explain why a thermometer rises when placed in warm water and drops when placed thereafter in cold water.

When placed in the warm water, the particles gain kinetic energy causing them to move around more quickly. As they move around more quickly, they cause the liquid to expand and the result is that the liquid will rise in a thermometer. When it cools, the particles will lose kinetic energy and their movement will decrease, resulting in the liquid dropping.

4. A balloon is filled with air. It is then placed in the freezer. What will happen to it? Why will this happen?

The balloon will shrink because the particles will lose kinetic energy as they cool down. As the particles lose energy, their movement decreases and the particles will move closer together, taking up less space.

5. An unopened bag of Old Dutch chips is placed near a warm air vent. What do you think will happen to the size of the bag over the next hour?

The size of the bag will increase, and possibly pop open. This will happen because the air in the bag will gain kinetic energy. This will increase the movement of the particles, and will cause the particles to move further apart.

Personal Response Sheet6. Two people are standing on opposite ends of a large swimming pool. While both

standing up one person bangs two rocks together above the water but the other does not hear it. When they both go under water and bang the rocks the other can now hear it. Explain why.

Gr. 11 Chemistry Physical Properties of Matter

Sound is transmitted by particles. The sound wave can travel faster through a liquid than a gas because the particles are closer together in a liquid than in a gas.

7. Explain why water boils at lower temperatures (ex. 90 °C) on the top of a mountain when at sea level in boils at 100 °C.

For water to boil, the vapour pressure of the water has to equal the atmospheric pressure. On a mountain, the atmospheric pressure is less than at sea level. This means that for water to boil, the vapour pressure does not have to be as high as it would be at sea level. With the vapour pressure being less, less kinetic energy is required to reach that level resulting in a lower boiling point.

8. A can of coke expands when frozen in the fridge. Explain why.

Coke is made up of water, and when water freezes it expands.

9. A car tire becomes somewhat flatter on a cold day but once the car starts traveling down the road it goes back to its original size. Explain why.

On a cold day, the particles in the tire will lose kinetic energy and the movement of the particles will decrease causing the tire to become flatter. As the tire drives down the road, the friction from the road will increase the kinetic energy of the particles, causing them to move faster, resulting in the tire expanding.

10. Explain why you can hear sounds easier on cold winter days than warm summer days.

Sound is transmitted through particles. On a cold winter day, the particles will have less energy and will be closer together. This will allow the sound waves to travel at a faster rate than on a warm day where the particles will be further apart.


Classifying Matter

Physical and Chemical PropertiesCharacteristic Property: a quality or attribute used to identify a substance. Very specific (melting point).


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How can one tell if something is a physical or chemical property? How do we know?

Physical Property: original substance is not changed chemically into a new substance.

Chemical Property: original substance is changed during the process and a different substance with new chemical properties is produced.

Examples of Physical and Chemical Properties:

Characteristic Physical Properties Characteristic Chemical Properties

colour, volume degree of reactivity

texture, shape reacts with O2 in air

mass, density produces CO2

state, temperature flammability

melting/boiling point

ductility

Intensive Physical Properties: properties that do not depend on the amount of matter present. Ex. density, colour, melting point, specific heat.

Extensive Physical Properties: properties that depend on the amount of matter present. Ex. mass, volume.

Physical or Chemical Properties Practice Problems

1. What other word could be used instead of the word “property”?

characteristic


2. What is one example of an extensive and intensive physical property?

intensive – densityextensive – mass

3. Identify each of the following properties as physical (P) or chemical (C):P a. hardness C e. catches fire in waterP b. solubility in water C f. inert to everythingC c. flammability P g. malleabilityC d. sensitivity to light C h. explodes in water

4. In each case, identify the underlined property as a physical or chemical property. Give a reason for your choice.

a. The normal colour of the element bromine is red-orange. physicalb. Iron is transformed into rust in the presence of air and water.

chemicalc. Dynamite can explode. chemicald. Aluminum metal, the shiny “foil” you use in the kitchen, melts at

660˚C. physicale. Dry ice sublimes at -78˚C. physicalf. Methanol (methyl alcohol) burns in air with a colourless flame.

chemicalg. Sugar is soluble in water. physicalh. Hydrogen peroxide, H2O2, decomposes to form oxygen, O2, and water

H2O. chemical

*Complete “Physical vs. Chemical Change” worksheet*


Comparing Solids, Liquids, and GasesArrange the following list of things as solids, liquids, or gases.

plasticine sponge honeywater tomato sauce airtoothpaste copper penny baking powdercloth oxygen nitrogen

SOLIDS LIQUIDS GASES

plasticine water oxygentoothpaste tomato sauce air

cloth honey nitrogensponge

copper pennybaking powder

Differences Between Solids, Liquids, and Gases

Criteria Solids Liquids GasesTakes the shape of its container Has a mass Has a shape Takes up space


Three States of Matter

SOLID LIQUID GAS

Properties of Solids, Liquids, and Gases

Property Solid Liquid Gas


vibraterotate

translational

vibrate

rotate

moving in straight lines (translational)

vibrate

Shape Has a definite shape

Takes the shape of the container

Takes the shape of the container

Volume Has a definite volume

Has a definite volume

Fills the volume of its container

Arrangement of particles Fixed, very close Random, close Random, far apart

Interaction between particles

Very strong Strong Essentially none

Movement of particles Very slow Moderate Very fast

Compressibility Cannot be compressed

Slightly compresses Easily compresses

Density Very dense Slightly less dense than solids Not dense

Diffusion Cannot diffuse easily Diffuses easily

Diffuses easily (more than a

liquid)

Examples ice, salt, iron water, oil, vinegar water vapour, helium, air

* Use “Physical Properties of Matter Demo” to explain concepts while filling in the chart*


Plasma

Scientists recognize a fourth state of matter known as plasma.

What is Plasma? A gaseous mixture of positive ions and electrons. Due to the unstable nature of these particles, the only way to have large

number of these energetic particles co-existing together is at temperatures over 100 million degrees Celsius.

Plasmas are the most common form of matter in the universe, comprising 99% of the visible universe, but are the least common on Earth.

Plasmas DO NOT occur naturally on Earth except in the form of lightning bolts.

Examples: aurora borealis, lightening, fluorescent lights.

Similarities between gas and plasma: both do not have a definite volume or shape

Differences between gas and plasma: due to the charges of plasma, it is electrically conductive and responds strongly to magnetic

fields and electrical currents.

*Oobleck and Glurch Activity**Complete “The Four States of Matter” assignment*


Solids, Liquids, and Gases Review Questions

1. Why doesn’t the density of solids and liquids change (hint: density=mass/volume)?

The mass and volume of solids and liquids are both definite.

2. Why does the density of a gas change?

Mass and volume are not definite and can change.

3. Explain in your own words what is meant by the shape of solids being definite.

The molecules are “locked” in position.

4. What is meant by the shape of liquids being indefinite?

Molecules are free to move, and take the shape of the container.

5. What is meant by the shape of gases being indefinite?

Molecules are free to move, and take the shape of the container.

6. Explain why solids are not classified as fluids?

Solids do not have the ability to flow.

7. Explain why most solids are denser than most liquids at the same temperature.

Particles are closer together; have a fixed position.


Kinetic Molecular TheoryThe kinetic molecular theory describes the behaviour of molecules in terms of particle motion. There are several assumptions that are made:

1. All matter is composed of particles.

2. Particles are in constant motion. The amount of motion depends greatly on the kinetic energy of a substance.

3. Collisions between atoms are elastic.i.e. no change in energy takes place and particles bounce off each other without losing energy, only changing direction.

Elastic Collisions: no loss of energy, only a change in direction.

Non-elastic Collisions: loss of energy

4. Energy of the particle is proportional to the temperature of the particle i.e. as the temperature increases, the particles speed increases, thus increasing the kinetic energy.


SOLIDGAS

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melting

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Changes of State


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Vapour PressureVapour: gaseous state of a substance which is liquid or solid at room temperature.

Vapour Equilibrium: the state in which evaporation and condensation are taking place at the same rate. rate condensation = rate of evaporation

water level is constant

Vapour Pressure: the pressure (force per unit area) generated by a vapour in equilibrium with its liquid. Vapour pressure is a characteristic physical property, and is also a measure of the size or strength of the intermolecular forces (IMF) of a liquid.

Melting Point: temperature at which the structure of a solid collapses and the solid changes to a liquid.

Normal Melting Point (n.m.p.): the temperature at 101.3 kPa at which solid changes into liquid. Ex: Water n.m.p. = 0˚C

Boiling Point: temperature at which the vapour pressure of the liquid is equal to the atmospheric pressure.

Normal Boiling Point (n.b.p.): the temperature at which the vapour pressure of the liquid is equal to 101.3 kPa. Ex: Water n.b.p. = 100˚C if the vapour pressure is 101.3 kPa and the atmospheric pressure is also 101.3 kPa.

Heat: the measure of the quantity of energy in a system. It can only be measured when energy is being transferred from one object to another.


*Can demo*

Unit = J (joules) Instrument = Calorimeter

Temperature: the measure of the intensity of the energy in the system. It is related to the average speed of the motion of atoms and molecules.

Unit = ˚C (degree Celsius) or K (Kelvin)Instrument = thermometer

Vapour Pressure

Low Vapour Pressure: strong intermolecular forces (IMF’s) slow rate of evaporation (water) non-volatile (low volatility) high boiling point

High Vapour Pressure: weak IMF’s high rate of evaporation (acetone, nail polish remover) volatile (high volatility) low boiling point

How Does Temperature Affect Vapour Pressure?As you increase the atmospheric pressure, the boiling point increases, and vice versa. Why?The boiling point occurs when the vapour pressure of the liquid equals the atmospheric pressure. As atmospheric pressure increases, vapour pressure increases. For vapour pressure to increase, the temperature (kinetic energy) must go up, i.e. higher boiling point.


*Complete “Changes of State Worksheet”*

Vapour Pressure Graphs

You will notice that regardless the substance there is a similar trend in the vapour pressure as temperature increases. We can use this graph to determine the normal boiling point of each substance and the temperature each will boil, at various pressures.

1. What is the normal boiling point of ethanol?~ 77°C

2. If the pressure in a city is 90 kPa, at what temperature will water boil?~96°C

3. Which substance has the largest forces of attraction at 60°C?Acetic acid


*Complete “Vapour Pressure Graphs Worksheet”*

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