1. All About Matter
SC2. Obtain, evaluate, and communicate information about the chemical and physical properties of matter resulting from the ability of atoms to form bonds.
a. Plan and carry out an investigation to gather evidence to compare the physical and chemical properties at the macroscopic scale to infer the strength of intermolecular and intramolecular forces.
b. Construct an argument by applying principles of inter- and intra- molecular forces to identify substances based on chemical and physical properties.
SC3. Obtain, evaluate, and communicate information about how the Law of Conservation of Matter is used to determine chemical composition in compounds and chemical reactions.
b. Plan and carry out an investigation to determine that a new chemical has been formed by identifying indicators of a chemical reaction (e.g., precipitate formation, gas evolution, color change, water production, and changes in energy to the system).

2. What is matter? Matter is the “stuff” that the universe is made of
Matter has mass and volume
MASS: measurement of the amount of matter
VOLUME: measurement of the amount of space that matter takes up

3. Where did it all come from?
Nobody knows the answer to this question – YET! (but we are close…)
The original composition of matter consisted of atoms of hydrogen (99% of the universe is still made of this)
All matter that exists today results from the process of NUCLEAR FUSION of smaller atoms combining together to form larger atoms.

4. KINETIC MOLECULAR THEORY OF MATTER
Matter is made up of very small particles which are in continuous random motion.

5. STATES OF MATTER Also referred to as “phases”
Based on particle arrangement
Based on energy of particles
Based on distance between particles

6. SOLID
Particles of solids are tightly packed, vibrating about a fixed position.
Solids have a definite shape and a definite volume.
Incompressible, have low kinetic energy and motion
Intermolecular forces are strong

7. LIQUID
Particles of liquids are tightly packed, but they are far enough apart to slide over one another.
Liquids have an indefinite shape and a definite volume.
Incompressible, have moderate kinetic energy and motion
Intermolecular forces are weaker

8. GAS Particles of gases are very far apart and move freely.
Gases have an indefinite shape and an indefinite volume.
Highly compressible, have high kinetic energy and motion
Virtually no intermolecular forces
A vapor is what you call the gaseous state of something that is normally a solid or liquid at room temperature.

9. PLASMA
Ionized gas
Very good electrical conductor and is affected by magnetic fields
Plasmas, like gases, have an indefinite shape and an indefinite volume.
Plasma is the most common state of matter in the universe

10. States of Matter SOLID LIQUID GAS PLASMA SHAPE SIZE PARTICLES
Definite
Indefinite
SIZE
PARTICLES
Tightly packed
Loosely arranged
Highly disordered
Disordered and ionized
STRUCTURE
Rigid
Fluid
SPECIAL TRAITS?
Resistant to changes in form
Surface tension
Highly compressible
Electrically conductive
EXAMPLE
Sugar
Water
Air
Lightning

11. PHASE CHANGES +Heat SOLID to LIQUID LIQUID to GAS SOLID to GAS Melting
Vaporization
Boiling
(from within)
Evaporation
(at the surface)
Sublimation

12. PHASE CHANGES -Heat GAS to LIQUID LIQUID to SOLID GAS to SOLID
Condensation
Freezing
Deposition

13. PHASE DIAGRAM

14. Heat in… Heat out… ENDOTHERMIC EXOTHERMIC
Term for any change in which heat is absorbed
These tend to feel cold because they absorb heat from our skin
Heat out…
EXOTHERMIC
Term for any change in which heat is released
These tend to feel warm because they release heat to our skin

15. HEATING/COOLING CURVE

16. Types of Matter MATTER PURE SUBSTANCES MIXTURES ELEMENTS COMPOUNDS
HOMOGENEOUS
HETEROGENEOUS

17. Types of Matter PURE SUBSTANCES
Have uniform and unchanging composition
Cannot be separated mechanically
Requires the substance to be changed chemically into other substances
Electrolysis

19. Pure Substances ELEMENT: cannot be separated into simpler substances
carbon, aluminum, oxygen (anything on the Periodic Table)

20. Pure Substances COMPOUND can be broken down chemically into elements
electrolysis
salt, sugar, water (anything that has a specific formula)

21. Types of Matter MIXTURES Have non-uniform or varying composition
Physical combination of substances, so they can be separated mechanically
Filtration, distillation, chromatography

22. DISTILLATION
FILTRATION
CHROMATOGRAPHY

23. Mixtures
HOMOGENEOUS
Composition appears uniform throughout; individual substances indistinct
Commonly referred to as solutions
KoolAid, air, alloys

24. Mixtures HETEROGENEOUS
Does not blend smoothly; individual substances remain distinct
cereal, pizza, iced tea

25. Mixtures HETEROGENEOUS Suspensions have particles that will settle
Muddy water, salad dressing
Colloids have particles that will scatter light
Milk, gels, aerosols

26. Properties of Matter
PHYSICAL properties are characteristics that can be observed or measured without changing the sample’s composition (what it’s made of)

27. Physical Properties
EXTENSIVE: dependent on the amount of matter present
mass, volume, length, molar amount
INTENSIVE: independent of the amount of matter present
density, color, odor, state

28. Properties of Matter
CHEMICAL properties are characteristics that can only be observed by changing a sample’s identity
flammability, reactivity, toxicity

29. Changes in Matter
PHYSICAL changes alter a material’s form without changing the composition
Cutting paper
Melting ice
Boiling water

30. Changes in Matter
CHEMICAL changes involve substances combining or breaking up to form new substances in chemical reactions
Burning paper
Rotting food
Rusting metal

31. Evidence of a Chemical Change
So how do you know if a chemical change has occurred?
You should observe at least one of the following characteristics:
Precipitation (two liquids mix and form a solid)
Gas evolution (fizzing, bubbling, or producing odors)
Color change (colors appear, disappear, or change)
Water production (solids can appear to liquefy)
Changes in energy (gets cold or warm, produces
light or sound)

32. It’s the LAW!
By carefully measuring the masses of substances before and after chemical reactions, it was observed that the total mass involved in the reactions remained constant (reactant mass = product mass)
The Law of Conservation of Matter (Mass) states that mass is neither created nor destroyed during a chemical reaction – it is conserved.