1. Fundamentals of Chemistry Unit 2 Notes Matter & Energy

2. Matter – anything that has mass and takes up space.
Law of Conservation of Mass/Matter
- Matter cannot be created or destroyed in an ordinary chemical reaction just rearranged to form different substances
Matter can be described using properties..

3. PROPERTIES
CHEMICAL
PHYSICAL
INTENSIVE
EXTENSIVE

4. Characteristics of Matter
Physical Properties
-Characteristics of a substance that can be observed without the production of a new substance.
Examples:
-Color,smell, taste, hardness, density, texture, melting/boiling/freezing points, magnetic attraction, solubility, electrical conductivity, temperature, state or phase

5. Two types of Physical Properties
1. Extensive
-Depends on the particular sample
-for example: volume, mass, weight, shape, etc…
2. Intensive
-Depends on the type of matter  NOT how much there is
-For example: color, melting point, specific heat, density, appearance, etc…

6. Chemical Properties
-describes how a substance reacts or fails to react with other substances to produce new substances.
Examples:
-Oxidation, Corrosion, Hydrolysis,
Combustion, Flammability, Reaction to Acid or Base.

7. Two Types of Changes 1. Physical Change
- an alteration of a substance that only changes the physical properties of the substance.
*Does not change the chemical composition of the matter!!

8. 2. Chemical Change
-an alteration of the chemical composition of a substance that results in the formation of a new substance
-ALWAYS forms a new substance that has different physical and chemical properties than the original substance.
*Also known as a chemical reaction.

9. Kinetic Theory
-All matter is made of tiny particles in constant motion.
Potential Energy (PE)
-energy due to the position or condition
-at the atomic level: the distance between the particles
closer= low PE farther = high PE
Kinetic Energy (KE)
-energy due to motion
 Faster=high KE Slower= low KE

10. Based upon particle arrangement
Based upon energy of particles
Based upon distance between particles
AKA POTENTIAL AND KINETIC

11. Solid Gas State or Phase Particle level picture Particles description
Keep Volume?
Keep shape?
Solid
Liquid
Gas
Arranged in orderly pattern
Yes
Yes
Touching, but not tightly packed
Yes No
Far apart and rarely touching No No

12. SOLIDS Particles are tightly packed, vibrating about a fixed position
definite shape
definite volume
Heat

13. LIQUID
Particles are tightly packed, but are far enough apart to slide over one another
indefinite shape
a definite volume
Heat

14. GAS Particles are very far apart and move freely indefinite shape
indefinite volume
Heat

15. Solid Gas State or Phase Particle Movement Amount PE Amount KE Example
Liquid
Gas
Vibrate only
Very Low
Low
Ice
Vibrate & move past each other
Low
Medium
Water
Move freely
High
High
Vapor

16. Plasma
- extraordinary state of matter
- consists of high energy particles
- electrons are stripped from their nuclei
-examples: fluorescent lights
stars
lightning
*Most Abundant State of Matter in the Universe!*

17. STATES OF MATTER LIQUID PLASMA SOLID GAS
Tightly packed, in a regular pattern
Vibrate, but do not move from place to place
Close together with no regular arrangement.
Vibrate, move about, and slide past each other
Well separated with no regular arrangement.
Vibrate and move freely at high speeds
Has no definite volume or shape and is composed of electrical charged particles

18.
ANIMATION

21. Phase Changes – Changes of State
Adding or removing energy (heat) to a substance causes phase changes
The particles potential energy is changed (increased or decreased).
During a phase change, temperature does NOT change

22. Phase changes Melting S Δ L (adding energy)
Freezing L Δ S (removing energy)
*Melting point & freezing point of a substance occur at the same temperature.

23. Phase changes Boiling L Δ G (adding energy)
Condensation G Δ L (removing energy)
Evaporation L Δ G (adding energy)
*Difference between boiling & evaporation:
-Boilinga specific temp. below the surface
-Evaporation any temp. at the surface

24. Phase changes Deposition G Δ S (removing energy) -Examples: snow frost
Sublimation S Δ G (adding energy)
-Examples: solid CO2 (dry ice)
solid air fresheners

25. AB -heat Δ KE -move faster -temp.  -solid BC -heat Δ PE
Liquid
Melting
Solid AB
-heat Δ KE
-move faster
-temp. 
-solid BC
-heat Δ PE
-get farther apart
-temp. stay same
-melting CD
-heat Δ KE
-move faster
-temp. 
-liquid

26. DE EF -heat Δ PE -heat Δ KE -get farther apart -move faster
Gas
Boiling DE
-heat Δ PE
-get farther apart
-temp. stay same
-boiling EF
-heat Δ KE
-move faster
-temp. 
-gas

27. A C B E D F CD
-KE 
-slows down
-temp. 
-Liquid AB
-KE 
-slows down
-temp. 
-Gas BC
-PE 
-closer together
-temp. stays same
-Condensation

28. A C B E D F EF
-KE 
-slows down
-temp. 
-Solid DE
-PE 
-closer together
-temp. stays same
-Freezing

29. What is the boiling point? What is the melting point?
Freezing Point &
Freezing
Melting Point
Melting
What is the boiling point?
What is the melting point?
What is the freezing point?

30. If melting & freezing points are at the same temp
If melting & freezing points are at the same temp. how do you know which?
-depends on whether adding or removing energy

31. What is this substance?
-Water
How do you know?
-Boiling & melting & freezing points of water

32. Matter
Pure Substances
Mixtures
Elements
Compounds
Homogeneous
Heterogeneous

33. Pure Substances
-made of only one type of matter
Mixtures
-a physical combination of two or more substances
-no particular ratio of particles
Element
-made of only one type of atom
-cannot be broken down into simpler substances under normal laboratory conditions

34. Compound
- Atoms of two or more elements, chemically combined in a definite ratio.
Homogeneous Mixtures
-two or more substances, physically combined in no definite
-The same throughout.
-Must be a SOLUTION
Heterogeneous Mixture
-two or more substances, physically combined in no definite ratio
-Different throughout

35. Classifications of Mixtures
Solutions – Particles are Very tiny, will not separate by filtering, will not settle out when allowed to stand, particles too small to scatter light, (-) Tyndall effect. Ex. Kool Aid, brine
Colloids – Particles are tiny, will not separate by filtering, will not settle out when allowed to stand, particles will scatter light, (+) Tyndall effect. Ex. Milk, whipped cream, aerosols
Suspension – Particles visible with unaided eye, will separate when filtered, will settle out if allowed to stand, particles will scatter light, (+) Tyndall effect. Ex. Muddy water, snow globe

36. Solutions SOLUTION – a solute dissolved in a solvent.
The solvent is the part in greater quantity.
For example: In a solution of salt water, salt is the solute and water is the solvent.
ELECTROLYTE - a solution that conducts electricity in water or molten form.
Salt water will conduct electricity.(Electrolyte)
Sugar water will not.

37. Soluble Able to dissolve.
Solute ions (for example: Na+1 and Cl-1) become surrounded by solvent molecules (H2O).
(Opposite charges attract!)
“Like dissolves Like”
Polar dissolves Polar
Ex. Salt in Water
Nonpolar dissolves Nonpolar
Ex. Oil in Gasoline

38. H2O
H =
O = - + + - + - - + - - + - + + -
NaCl
Na =
Cl = + -

39. CLICK HERE

40. Solutions are Homogeneous Mixtures
The solution is well stirred during its formation.
The particles will not come out of solution no matter how long it is allowed to stand.
The solution is clear and transparent.
A solution is considered to be in one phase and will not filter unless extremely fine filter paper is used.

41. Types of Solutions Gas-Gas Carbon dioxide, Nitrogen, Oxygen (air)
Liquid-Gas Water Vapor in Air
(moist air)
Gas-Liquid Carbon dioxide in Water (soda water)
Liquid-Liquid Acetic acid in Water
(vinegar)
Solid-Liquid Sodium chloride in Water
(brine or salt water)
Solid-Solid Copper in Silver (Sterling Silver)

42. Solubility
The amount of solute that dissolves in a given quantity of solvent at a given temperature.
Usually expressed in grams of solute per 100g of solvent.

43. Solution Concentrations
Saturated Solution – Contains the maximum amount of solute for a given amount of solvent at a constant temperature.
Unsaturated Solution - Contains less solute than a saturated solution.
Supersaturated Solution – Contains more solute than is should be able to hold at a given temperature. (Unstable)

44. Factors that affect solubility…
The nature of the solute and solvent.
Some chemicals are just more soluble than others.
2) Temperature and pressure.
3) The amount of solute already dissolved.
Solubility can be increased by…
Stirring the solution
decreasing the particle size of the solute
increasing temperature

45. Solubility
Refers to the maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure.
g solute / 100 g solvent
Saturated vs Unsaturated vs Supersaturated

46. Definitions Solutions can be classified as saturated or unsaturated.
A saturated solution contains the maximum quantity of solute that dissolves at that temperature.
An unsaturated solution contains less than the maximum amount of solute that can dissolve at a particular temperature

47. Definitions
SUPERSATURATED SOLUTIONS contain more solute than is possible to be dissolved; excess solute will precipitate out of a supersaturated solution, leaving a crystallized solid and a saturated solution.
Supersaturated solutions are unstable. The supersaturation is only temporary, and usually accomplished in one of two ways:
Warm the solvent so that it will dissolve more, then cool the solution
Evaporate some of the solvent carefully so that the solute does not solidify and come out of solution.

51. ON THE CURVE = SATURATED
BELOW CURVE = UNSATURATED
ABOVE CURVE = SUPERSATURATED
Note: you may be asked sometimes how much more solute should be used to make something saturated.

52. What are the units for solubility?
What is the solubility of NaCl at 600C?
What is the change in solubility of NaNO3 from 150C to 600C?
How much more KI can be dissolved in 100 grams of water at 300C than KNO3?
If 60 grams of NaCl were placed into a beaker with 100 grams of water at 350C and then stirred, what type of solution would result?