Science Test Review | Matter

* school science matter chemistry

[2026-01-08 Thu]

1. Understand the importance of safety in scientific investigations, recall the laboratory safety rules and common WHMIS symbols.

1.1. WHMIS

W orkplace H azardous M aterials I nformation S ystem

1.2. HHPS

H azardous H ousehold P roduct S ymbols.

1.3. If a substance has a WHMIS or HHPS symbol on it, what makes that substance dangerous?

More sides = more danger. It means that something is flammable, corrosive, toxic, …

1.4. What are some of the lab safety tools that can be found in the lab?

Goggles
Lab coat
Gloves

2. Define matter and explain the difference between qualitative and quantitative properties.

2.1. What is matter?

Anything that has mass and take up volume.

2.2. What are the different states of matter and how do they differ?

2.2.1. Solid

Particles are closely packed together and do not move much. Has fixed shape and volume.

2.2.2. Liquid

Particles are spaced apart and flow. Has no fixed shape, but fixed volume.

2.2.3. Gas

Particles are far apart. No fixed shape and volume.

2.3. What are qualitative and quantitative properties? Give examples for each.

2.3.1. Qualitative Properties

Your 5 senses. Cannot be measured numerically. Eg; odour, beauty, …

2.3.2. Quantitative Properties

Properties that can be objectively measured. Eg; length(cm), mass,

3. Distinguish between and provide examples of physical and chemical properties of matter? Distinguish between physical and chemical changes and be able to predict whether a physical or chemical change has occurred.

3.1. What is a physical property? Give examples of physical properties.

A physical property describes a substance/object. Eg: malleability, lustre, ductility, …

3.2. What do these physical properties mean?

Property	Meaning
Lustre	Shiny-ness
Clarity	Clear-ness/transparency
Viscosity	Ability to flow/pour
Hardness	Relative ability to be scratched/scratch another
Malleability	Ability to be hammered int oa sheet or molded.
Ductility	Ability to be drawn into a strand
Conductivity	Ability to allow electrons to flow through

3.3. What is a chemical property? Give examples of chemical properties (i.e., reactivity, flammability, acidity, etc.)

A chemical property describes how a substance reacts to other substances. Eg: Acidity, how it reacts with bases. Reactivity: How readily a substance interacts with others.

3.4. What are physical and chemical changes? How do they differ?

3.4.1. Physical Changes

Alter a substances form(like shape, state, size). But do not add a new substance.

3.4.2. Chemical Changes

Changes that create a new substance.

3.5. In a given situation, how do you know if a physical or chemical change is taking place? (Indicators of a chemical change)

A chemical change is usually indicated by:

Changes in odour
Changes in color
Precipitate(solid) formation
Gas bubbles
Light/energy.

4. In a given situation, how do you know if a physical or chemical change is taking place? (Indicators of a chemical change)

4.1. What are the five postulates of the particle theory of matter? (Recall S.T.A.M.P)

All matter is made up of particles.
All particles have space between them.
All particles are attracted to eachother.
Particles move faster as temperature increases.
Particles are always moving

4.2. What happens to the particles of a substance when they change state?

The particles stay the same, but their arrangement and spacing can change. Eg: Water particles move faster and further apart when boiled.

5. Distinguish between a mixture and a pure substance. Differentiate between mechanical mixtures and solutions and provide examples of each. (p. 175-177)

5.1. What are the different types of matter? Provide examples of each.

(see: Matter)

5.1.1. Pure Substances

Elements

Elements are made of one type of particle. Each particle is made up of one element of the periodic table.
Compound

Compounds are made of multiple different types of atoms bonded together.

5.1.2. Mixtures

Mechanical(Heterogenous) Mixtures

Mechanical mixtures are mixtures in which you can see the different components and they remain seperate.
Solution(Homogenous) Mixtures + Alloys

Solutions are combinations of two or more substances where the components are evenly distributed and you cannot differentiate them with the naked eye. Alloys are homogenous mixtures of two or more elements with at least one metal created by melting and mixing them.

6. Use the Particle Theory of Matter to account for differences in the densities of substances at a given temperature and as their temperature changes. Explain how water is unique in this regard (p.193, 196-197)

6.1. Why are solids of a substance more dense than liquids of the same substance that have the same volume?

Solids are more dense because particles are more closely packed together.

6.2. How is the density of a substance impacted by temperature changes?

Increasing the temperature causes the particles to move faster and go farther apart, decreasing density.

6.3. What is unique with regards to water and its density at different temperatures?

Water has a unique molecular structure. When frozen, it forms a crystal lattice. It is less dense at lower temperatures while most things are denser at low temperatures.

7. Solve simple density problems using the GRASP format. Express the results of these calculations to the appropriate number of significant figures and with the correct units of measurement. (p.192-195)

7.1. What does GRASP stand for?

-w Givens

Requirements
Analysis
Solution
Paraphrase

7.2. How do you calculate mass, volume, and density of a substance?

\begin{equation}{\frac{\text{Mass}}{\text{Volume}}} = \text{Density} \end{equation} \begin{equation}\text{Density} \cdot \text{Volume} = \text{Mass} \end{equation} \begin{equation}{\frac{\text{Mass}}{\text{Density}}} = \text{Volume} \end{equation}

7.3. What are the significant figures rules?

Non-zero digits are always significant
Zeros between non-zero digits are significant
Leading non-zero digits are significant
Leading zeroes are not significant
Trailing zeroes are significant if the number is written with a decimal point
Trailing zeroes in a whole number without a decimal point are insigificanat

7.4. How many significant figures do you put in your final answer?

When answering a question, you round to the one with the least sig figs.

7.5. Know how to convert between units (E.g., 1000g = 1kg or 1000mL = 1L)

This is easy.

8. Characterise elements as metals, nonmetals or metalloids and locate them on the Periodic Table

8.1. Which elements are metals.

Items left of the staircase

8.2. Which elements are nonmetals?

Nonmetals are right of the staircase.

8.3. What are the properties of metals, nonmetals, and metalloids?

Metals are usually shiny, malleable, ductile, and conductive, relatively dense.
Nonmetals are usually the opposite: brittle, poor conductor, less dense.

9. Distinguish between groups and periods and explain the significance of each. Compare similarities in properties both between and within the following groups: alkali metals, alkaline earth metals, halogens and noble gases.

9.1. What is the difference between a group and a period?

Group = Column
Period = Row

9.2. What are the names of Groups 1, 2, 17, and 18?

1=Alkali Metals
2=Alkali Earth Metals
17=Halogens
18=Noble gases

9.3. What are the properties of alkali metals, alkaline earth metals, halogens, and noble gases?

Alkali Metals are shiny, soft, very reactive, and low density.
Alkaline earth metals are harder and less reactive
Halogens are very reactive and poisonous
Noble gases arent reactive at all

10. Define atomic number and mass number. Use the atomic number and mass number to calculate the number of subatomic particles in an atom of a given element.