All matter is made up of tiny particles that are constantly moving.
There are spaces between the particles, which can vary in size depending on the state of matter.
The temperature of a substance affects the speed of the particles; higher temperatures result in faster-moving particles.
The particles are attracted to each other, with this attraction varying in strength between different types of matter.
The arrangement of particles determines the state of matter—solid, liquid, or gas.

All matter is made up of tiny particles (atoms/compounds/ions)

Example 1 drop of water is made of millions of particles

When heated, the particles gain energy and move apart, leading to a change in state, such as ice melting into water. As temperature increases, the kinetic energy of these particles also increases, resulting in a transition from a solid to a liquid, and eventually, to a gaseous state.

Each type of matter is made up of unique particles, different from other types of matter
All particles have spaces between them. The size of the space changes with different states.

Particles far apart are gasses

Particles spaced are liquid

Particles tightly packed are solid

Particles are attracted to each other. The closer they are, the stronger the attraction.

Particles are always moving. The speed is directly related to the tempicher: increasing temperature = increasing speed.

Solids - particles vibrate

Liquids - particles slide

Gas - particles move quickly, in straight lines.

We can use the particle theory to explain what is happening as matter changes states

S - what is happening to the spaces? increased / decreased

A - how is the attraction changing? increased / decreased

M - how has the movement changed? increased / decreased

E - what happened to the energy?

Physical properties

Physical properties definition: properties of matter that can be observed with 5 senses, without changing the substance.

The 2 kinds of physical properties

Quantitative
Qualitative

Qualitative properties

Colour - the colour
State - state of matter (liquid, solid and gas)
Clarity - appearance of being clear
Odor - smell

Quantitative

Taste - flavour sweet, sower, spicey?
Texture - feel of the surface
Lustre - shininess
Malleability - can you hammer it into a sheet?
Flexibility - easiness to bend
Ductility - easiness to stretch
Melting - temperature where substance melts (melting point of water is 0 degrees celsius)
Boiling point - temperature where substance boils (boiling point of water is 100 degrees celsius)
Solubility - ability of substance to dissolve in a solvent (water)
Hardness - how hard substance is. (diamonds are the hardest)
Electrical conductivity - measure of a substance (conductivity electricity
Viscosity - Measure of how easy liquid flows (water has a low viscosity)Little piece of paper in your hair
Density - Amount per unit volume
Ahestion - Measure of attraction between different materials
Cohesion - Measure of attraction between the same materials

Molecular (covalent) compounds

Recap: ionic compounds are formed between metal ions and non metals ions. The metal gives its electron(s) to the nonmetal, they are then attracted by strong electrostatic forces

Molecular compounds form when two or more nonmetals SHARE pairs of electrons to fill their valence shells, and become stable.

The shared pair (2) of electrons is called a covalent bond

Properties of molecular compounds

Molecular compounds are attracted to other molecular compounds by intermolecular forces that are weak compared to electrostatic forces of ionic compounds

Melting and boiling points tend to be low - does not require a lot of energy to charge state - solid - liquid - gas

Many covalent compounds are gas liquid at room temperature or much lower

Solubility - some molecular compounds will dissolve in water (ex: sugar), many will not (ex: co2, oil)

Conductivity - molecular compounds NEVER conduct electricity

Ionic compounds are made when metal atoms and non-metal atoms interact. Here's a simpler breakdown:

How Ions Form:
- Non-metal atoms gain electrons to become negative ions.
- Metal atoms lose electrons to become positive ions. They have a positive charge equal to the number of electrons they lost.
Formation of Ionic Compounds:
- Ionic compounds are formed between these metal and non-metal ions.
- For example, if there are X metal ions (positive) and Y non-metal ions (negative), the relationship is that we need enough ions to balance the charges so that the total positive charge equals the total negative charge. Sometimes, you may need more than one of each ion.
Electron Transfer:
- Metals transfer their electrons to non-metals, creating ions that stick together because of strong attraction known as electrostatic forces.
Properties of Ionic Compounds:
1. They have very high melting and boiling points. For instance, table salt melts at about 840°C and boils at 1464°C.
2. They are solid at room temperature.
3. They dissolve in water and usually conduct electricity when they are dissolved or melted because their ions can move freely.

What is Matter?
Matter includes anything that takes up space and has mass, like mud, a person, oxygen, sodium, and carbon dioxide.

What is Not Matter?
Things like heat, light, and electricity are not matter.

Types of Matter:

Pure Substances: Only one type of particle (e.g., elements like oxygen and compounds like water).
Mixtures: Two or more different substances mixed together.
- Mechanical Mixtures (like pizza) have visible different components.
- Solutions (like coffee with milk) look uniform and the same throughout.

Separating Mixtures: