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Classification of Matter -
All matter can be classified as either a mixture or a pure substance. Mixtures are homogeneous or heterogeneous, and pure substances are either elements or compounds.
Difference Between Pure Substances & Mixtures -
A pure substance contains only one kind of molecule, while a mixture is a combination of two or more pure substances.
Examples of Mixtures: Steel & Chocolate Chip Cookies
Examples of Pure Substances: Oxygen & H₂O
Difference Between Elements & Compounds -
An element is made up of only one kind of atom, while a compound contains the atoms of two or more elements.
Example of an Element: Carbon
Example of a Compound: Copper
Difference Between Homogeneous & Heterogeneous Mixtures -
A homogeneous mixture is a type of mixture in which every part of the solution has the same properties. A heterogeneous mixture is a type of mixture in which the components can be seen, as there are two or more phases present.
Example of a Homogeneous Mixture: Kool-Aid
Example of a Heterogeneous Mixture: Chocolate Chip Cookie

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Physical properties can be measured or observed without changing the chemical nature of the substance - properties that you can see. Physical properties include: appearance, texture, color, odor, melting point, boiling point, density, solubility, polarity, and many others.

Chemical properties are properties or characteristics of substances that are observed during a reaction in which the chemical composition or identity of the substance is changed - properties that are observed while there is a chemical reaction occurring. Chemical properties include: toxicity, coordination number, flammability, enthalpy of formation, the heat of combustion, oxidation states, chemical stability, and the types of chemical bonds that will form.

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3 Common Examples -
• Lightning
• Auroras
• Stars / Sun
Physical Properties -
• Hot ionized gas
• Consists of charged particles, neutrals, and fields that exhibit
collective effects
• Plasmas carry electrical currents and generate magnetic fields
• Plasmas are the most common form of matter, comprising more than
99% of the visible
universe.
• Plasma is highly conductive.
Forces of Attraction (Intermolecular Forces) -
Electrically charged gaseous particles that are strongly influenced by electromagnetic phenomenon.

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3 Common Examples -
• Wood
• Metals
• Rocks
Physical Properties -
• Highly compacted particles
• Own specific boiling and melting points
• Malleable and ductile
• Specific shape and form
• Specific volume
Forces of Attraction (Intermolecular Forces) -
• Take up little intermolecular space
• Very strong intermolecular forces

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Definition: a theory that proposes the existence of distinct, separable, independent components - the atoms of each element are very similar, but the composition of the atoms differ.
3 Parts:
1) All matter is made of atoms.
2) Atoms are indivisible and indestructible.
3) Compounds are formed by a combination of two or more different
kinds of atoms.

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Definition: the smallest particle of an element that can exist either alone or in combination.
Structure: Atoms are made up of three particles: protons, neutrons and electrons. The positively charged nucleus (the center of an atom) consists of protons and neutrons that are surrounded by a number of electrons. The number of electrons is equal to the number of protons.

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3 Common examples -
• Water
• Milk
• Blood
Physical Properties -
• Takes the shape of it's container
• Close to being incompressible
• Usually have a boiling point above room temperature
• Definite volume
Forces of Attraction: (Intermolecular Forces) -
The intermolecular bonds in liquids are very weak, but they are strong enough to keep the particles together.

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3 Common examples -
• Oxygen
• Helium
• Nitrogen
Physical Properties -
• Certain pressure
• Specific number of particles
• Temperature can differ
• Easy to compress
• Expand to fit their container
Forces of Attraction: (Intermolecular Forces) -
The average kinetic energy of the particles in a gas is great enough to overcome the forces of attraction between them. The molecules of a gas move apart when they collide.