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Grade 9 Science: Unit 2: Chapter 1:

Matter

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Chapter 1: Matter

Summary of Chapter

This chapter is about matter, from the different types of matter and their classifications, to physical and chemical properties of matter, as well as physical and chemical changes in matter

Basic Intro video (coming soon)

These two laws below define matter.

Fundamental Law of Matter:

Matter is anything with a mass (weight) and a volume (takes up space). It, like energy, cannot be created or destroyed.

Particle Theory of Matter:

All matter is made of particles.
Particles have space between them.
Particles are always moving.
Particles move faster and get farther apart when heated.
Particles are attracted to each other.
All Particles of the same substance are identical.

Content

Section 1: Classification of Matter

Matter is anything with a mass (weight) and a volume (takes up space). It, like energy, cannot be created or destroyed.

Types of Matter

Key Terminology of this Chapter:

Pure Substance: Made of only one kind of matter. Can only be split by chemical means.

Element: The most basic and pure type of matter: Everything we currently know is made of some combination of one or more elements on the 118 elements on the Periodic Table. Examples of elements include: Carbon, Oxygen, Hydrogen. Can only be split by advanced chemical means., such as particle accelerators.

Molecule: A combination of 2 or more atoms of the same element. Example: Ozone (O3) has 3 oxygen molecules. Can only be split by chemical reactions.

Compound: A combination of 2 or more different elements. Examples include: Glucose ( C6H12O6), with 24 atoms: 6 carbon, 12 hydrogen, and 6 oxygen; Carbon Dioxide (CO2) , with 3 atoms, 1 carbon and 2 oxygen. Can only be split by chemical reactions.

Mixture: Made of more than one kind of matter. Some of these mixtures can be split apart by physical means, others require chemical means.

Homogeneous Mixture: A mixture where all constituents (parts) have been mixed to the extent where the mixture appears as one uniform substance not distinguishable into its separate components, appearing evenly throughout. Many homogeneous mixtures require chemical means to separate. Examples of homogeneous mixtures include air, steel, and tap water.

Solution: A homogeneous mixture which is composed of a solute and a solvent. The solvent is the substance that dissolves the solute(s) . For example, in saltwater, water, the solvent, dissolves salt, the solute. Water is known as a "universal solvent" because of its ability to make so many solutions.

Alloy: A combination of metals or a combination of a metal with one or more other elements. Examples: Steel: Iron (which is a metal) and Carbon, Sterling Silver (silver and copper combination, both are metals)

Colloid: A combination of 2 or more different elements. Examples include: Glucose ( C6H12O6), with 24 atoms: 6 carbon, 12 hydrogen, and 6 oxygen; Carbon Dioxide (CO2) , with 3 atoms, 1 carbon and 2 oxygen. Can only be split by chemical reactions.

Emulsion: A combination of 2 or more different elements. Examples include: Glucose ( C6H12O6), with 24 atoms: 6 carbon, 12 hydrogen, and 6 oxygen; Carbon Dioxide (CO2) , with 3 atoms, 1 carbon and 2 oxygen. Can only be split by chemical reactions.

https://sciencenotes.org/what-is-an-emulsion-definition-and-examples/

Aerosol: A combination of 2 or more different elements. Examples include: Glucose ( C6H12O6), with 24 atoms: 6 carbon, 12 hydrogen, and 6 oxygen; Carbon Dioxide (CO2) , with 3 atoms, 1 carbon and 2 oxygen. Can only be split by chemical reactions.

Foam: A combination of 2 or more different elements. Examples include: Glucose ( C6H12O6), with 24 atoms: 6 carbon, 12 hydrogen, and 6 oxygen; Carbon Dioxide (CO2) , with 3 atoms, 1 carbon and 2 oxygen. Can only be split by chemical reactions.

Heterogeneous Mixture: A mixture where all constituents (parts) are not mixed to the point where it is a homogeneous mixture, or a mixture where the components simply cannot be mixed in that way. In many cases, the separate parts are easily visible, and can be easily separated by physical means. Examples include: Pizza (its toppings are easily visible), over saturated sugar water (some sugar is visible at the bottom).

Suspension: A homogeneous mixture which is composed of a solute and a solvent. The solvent is the substance that dissolves the solute(s) . For example, in saltwater, water, the solvent, dissolves salt, the solute. Water is known as a "universal solvent" because of its ability to make so many solutions.

Mechanical Mixture: A combination of metals or a combination of a metal with one or more other elements. Examples: Steel: Iron (which is a metal) and Carbon, Sterling Silver (silver and copper combination, both are metals)

Section 2: Properties of Matter

Seeing as everything tangible, everything with a mass and volume is made of matter, ways to distringuish between different types of matter are needed. There are two different kinds of properties of matter: Physical properties, and chemical properties.

Physical Properties of Matter

Physical properties of matter are either determined how our five senses perceive the object (qualitative) or measured and assigned a numeric or other value (quantitative)

Examples of Qualitative Properties:

Clarity: The way light passes through the object. An object can be fully see-through and allow all or most visible light to pass through (transparent), partially see-through and allow some visible light to pass through (translucent), or not allowing any visible light to pass through it (opaque). Examples: glass is transparent, tinted glass is translucent, and wood is opaque.

Crystal Form: The shape that a particle of a solid takes. For example sugar crystals are cubical.

Density: The ratio of an object;s mass to its volume (D = mass / volume). Objects with more mass per volume are more dense, and objects with less mass per volume are less dense. For example, iron would sink in water because iron has more mass per the same volume. Objects more dense than water sink, while objects less dense than water float.

Ductility: The ability of a substance to be drawn into wires. Metals are usually very ductile, e.g copper.

Hardness: Technically speaking, how resistant a solid is to scratching or breaking (can also be considered a quantitative property as there is a scale for hardness: the Mohs scale of hardness). For example pure gold is not very hard, (which is why it is usually combined with other metals), but diamond is very hard, being the hardest mineral.

Lustre: How shiny an object. Shinier objects are described as more lustrous, while dull objects are less lustrous. For example, a cut and faceted gem is very lustrous, but unpolished wood is not very lustrous

Malleability: Ability of an object to be bent, shaped, formed, molded, etc. For example, wet clay is very malleable, while diamond is virtually unmalleable.

State: What state of matter an object is in: solid, liquid, gas, plasma, etc.

Solubility: Ability of a substance to dissolve (usu. in water), essentially how good of a solute it is. For example, salt is soluble in water.

Viscosity: Resistance of a fluid to flow. Substances which are more resistant to flow are more viscous, while less flow-resistant substances are less viscous. For example, honey is very viscous, while water is not very viscous. When fluids get hotter they get less viscous as the bonds that hold the molecules get weaker. As gases get more viscous, they get thicker, and as liquids get more viscous, they become more runny.

Examples of Quantitative Properties:

Melting Point: The minimum temperature required to melt a solid (turn it into liquid). For example water melts at 0*C, salt melts at 800*C

Boiling Point: The minimum temperature required to boil a liquid (turn it into a gas). For example, water boils at 100*C, oxygen boils at -183*C

*Some qualitative properties can also measured by numerical values. For example hardness does have a scale, known as the Mohs Hardness Scale (see below image: Fig 1)

Chemical Properties of Matter

Chemical properties are usually harder to be assessed than physical properties, they usually require the object to be altered in some way. There are four main examples of chemical properties.

Examples of Chemical Properties:

Stability: How reactive a substance is. The more reactive a substance is, the less stable it is, and vice versa. For example, sodium is extremely reactive and unstable, while helium is unreactive and very stable.

Flammability: How easily an object can catch fire when exposed to a certain temperature. Flammables have a flash-point (minimum ignition temperature when exposed to an ignition source) below 37.8*C. Flammable materials can catch fire in normal working temperatures when exposed to flame. For example Ethanol at 17*C can catch fire if exposed to flame.

Combustibility: How easily an object will ignite when exposed to intense heat and/or pressure. For example, the gas (propane, etc) in gas cylinders is under high pressure and very combustible. A material is combustible when its flash-point is higher than 37.8*C. For example, formaldehyde can catch fire if exposed to an ignition source, and it is stored at over 70*C

Toxicity: How harmful a substance is to health. It may alter/interfere with/stop metabolic processes in the body or cause harmful chemical reactions. For example, heavy metals like mercury and lead are extremely toxic because they interfere with key metabolic processes and destroy biological molecules.

Difference between Combustibility and Flammability in detail: Useful Links

https://www.ccohs.ca/oshanswers/chemicals/flammable/flam.html

https://www.highspeedtraining.co.uk/hub/difference-between-flammable-and-combustible/

Section 3: Changes in Matter

Matter is constantly changing between different types, both in nature, and in human-caused situations. There are different types of these changes.

Physical Changes in Matter

Physical changes in matter involve chemicals/materials being rearranged in a new way, but still retaining the essential properties of the chemical/matter. The resulting chemical/material is chemically identical to the original chemical/material. These changes are reversible

Signs of a Physical Change:

Change in state (For example, ice melting)
Change in shape or form (For example, ripping paper)
Easily reversible (For example: freezing liquid water: can be melted again to restore liquid water)
No new substance formed (For example cutting up cookie dough)

Everyday physical changes:

Cutting something up, folding it or bending it
Melting, freezing, boiling

Chemical Changes in Matter

A chemical change is when new substances are created, the change is not easily reversible, and a chemical reaction has occurred.

Signs of a Chemical Change:

Formation of a new substance(s) and/or substance removed (baking soda and vinegar forming carbon dioxide, water, and sodium acetate)
Chemically caused color change (Copper turning green as it oxidizes/rusts)
Gas created (Water undergoing a decomposition reaction into hydrogen gas and oxygen gas)
A solid created from non-solids (precipitate formation)
Not easily reversible (For example, Burning bread)
Smell/odor production (For example, Sulfurous compounds making a powerful odor when eggs rot and their chemical composition changes)
Temperature change (For example, exothermic (give off heat) or endothermic (absorb heat) chemical reactions)

Everyday chemical changes:

Cooking something (with heat)
Burning
Rusting
Rotting

Activities:

Activity 1: Chemistry:

brief 1 sentence description.

Link to the assignment:

Make a Copy of the document

Activity 2: Chemistry:

brief 1 sentence description.

Link to the assignment:

Make a Copy of the document

Biomes Activity: Your Local Biome

Do some research on what biome you are located in

Suggestions for recording:

Think of the answers to these questions:

What biome are you located in
What level of diversity is in this biome

a. Do some research, what biome and ecozone is the nature area in?

What are the threats to this biome?
How can we protect this biome?

Chapter Quiz

This short quiz is to test your knowledge on the biodiversity chapter in the ecology unit.

It will be out of 45 points. + 2 bonus points

Good luck! Remember, this isn't a real quiz. Just to test your knowledge on the unit. So don't stress, just keep calm, and don't worry. This whole site was intended as a study aid. If you do well, good job! Kudos to you. If you don't do so well, it just means you may need to study the section again.

Don't cheat. Please. The chapter quizzes are built into the site as Google Forms, unlike the unit tests, which are external, secure links.

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