2. THE STORY CONTINUES…

3. …STATES
OF MATTER
Unit 1
(LESSON 5)

4. Unit 1 – LESSON 5
“STATES of MATTER”

5. MATTER: all matter is composed of small particles (atoms or molecules)
Kinetic-Molecular Theory of Matter states:
(1) the DISTANCE between particles determines
the state of the substance
(2) particles are in constant motion
(3) the MOTION of particles is different for each
state of matter

6. MATTER: Kinetic-Molecular Theory of Matter …
describes the characteristics of the states of matter
explains the behavior of matter by examining the molecular forces between particles and their energy
matter maintains the same chemical composition regardless of the state matter in which it exists
(e.g.) water is H2O whether it’s a solid, liquid or gas

7. MATTER: Kinetic-Molecular Theory of Matter …
particles of substances at a given temperature have the SAME average KINETIC ENERGY…
… this is due to the strength of the intermolecular attraction between particles
(e.g.) ROOM TEMPERATURE (20o C): some substances are solids, some liquids and others gases

8. GASES: Kinetic-Molecular Theory of Matter …
have the WEAKEST intermolecular forces
particles are FAR APART moving freely in all directions in a translational (straight line/linear) motion
when particles “COLLIDE” energy is transferred between the particles, but is NOT LOST

9. GASES:
Kinetic-Molecular Theory of Matter

10. LIQUID: Kinetic-Molecular Theory of Matter …
have STRONGER intermolecular forces than gases
particles are still CLOSE TOGETHER, but are now in partial disorder as they move about
particles are FLUID (able to flow from place to place)

11. LIQUID:
Kinetic-Molecular Theory of Matter

12. SOLID: Kinetic-Molecular Theory of Matter …
have the STRONGEST intermolecular force between the particles
particles are CLOSE TOGETHER arranged in an ordered pattern
particles have kinetic energy and are ALWAYS VIBRATING

13. SOLID:
Kinetic-Molecular Theory of Matter

14. Summary: Kinetic-Molecular Theory of Matter

15. “3” Principle States of Matter:
Solid (definite shape & volume; atoms held tightly
together w/ a vibrational motion)
Liquid (definite volume; shape of container; atoms
loosely held together, atoms sliding over
one another)
Gas (shape & volume of container; atoms NOT held
together and moving in ALL directions)

16. “3” Principle States/Phases of Matter:
Solid
Liquid
Gas

17. TYPES of SOLIDS:
CRYSTALLINE (true): regular, orderly, repeating, crystalline lattice pattern
ALLOTROPES  same element, same state of matter, different atomic form
(e.g.) Carbon [C]: graphite, diamond,
nanotubes and buckyballs
AMORPHOUS: long, intertwining chains or strands of atoms

18. TYPES SOLIDS: CRYSTALLINE and
AMORPHOUS
CRYSTAL and AMORPHOUS
ALLOTROPES

19. PROPERTIES of LIQUIDS:
ADHESION: a force that attracts particles of different substances to each other
COHESION: a force that attracts particles of the SAME substance to each other
SURFACE TENSION  the attraction of water molecules to each other at the surface
VISCOSITY: the resistance of a liquid to flow

20. PROPERTIES of LIQUIDS: ADHESION, COHESION & SURFACE TENSION and VISCOSITY
ADHESION and COHESION
VISCOSITY

21. PROPERTIES of LIQUIDS: ADHESION, COHESION & SURFACE TENSION and VISCOSITY
SURFACE TENSION

22. PROPERTIES of GASES:
EXPANSION: the spreading out of molecules filling a container regardless of its size due to the spacing between gas molecules
COMPRESSION: the compaction of same amount of gas molecules in a smaller container due to the spacing between molecules
DIFFUSION: the process where one gas mixes with another [SOLIDS and LIQUIDS can also diffuse]
EFFUSION: the process where gas escapes through a very small holes in a container

23. PROPERTIES of GASES:
DIFFUSION and EFFUSION  state the HEAVIER the gas’s molecular MASS, the SLOWER the diffusion (mixing) and effusion (escaping) of the gas molecules

24. MEASUREABLE PROPERTIES of GASES:
PRESSURE and VOLUME (Boyle’s Law): as VOLUME increases PRESSURE decreases
[when TEMPERATURE remains CONSTANT]
PRESSURE and TEMPERATURE: as TEMPERATURE increases PRESSURE increases
[when VOLUME remains CONSTANT]
VOLUME and TEMPERATURE (Charles’s Law): as TEMPERATURE increases a “flexible” VOLUME increases
[when PRESSURE remains CONSTANT]

25. MEASURABLE PROPERTIES of GASES:
PRESSURE and VOLUME (Boyle’s Law)  as the VOLUME INCREASES PRESSURE DECREASES when TEMPERATURE is kept CONSTANT

26. MEASURABLE PROPERTIES of GASES:
PRESSURE and TEMPERATURE  as the TEMPERATURE INCREASES PRESSURE also INCREASES when VOLUME is kept CONSTANT

27. MEASURABLE PROPERTIES of GASES:
VOLUME and TEMPERATURE (Charles’s Law)  as the TEMPERATURE INCREASES VOLUME also INCREASES when PRESSURE is kept CONSTANT

28. PLASMA “4th” State/Phase of Matter:
ionized atoms stripped of their electrons (negatively charged subatomic particles of an atom) leaving positively charged nuclei tightly packed together
the state of matter of the stars and stellar nebulae
makes up 99% of the matter in our universe
also found in the outer-most layer of earth’s atmosphere = ionosphere
ionized gases are found in fluorescent and neon signs and lightning

29. “4th” State of Matter: PLASMA

30. THE END
FOR NOW…
UNIT 1
(LESSON 5)

31. COMING SOON
“CHANGES of STATE”
UNIT 1
(Lesson 6)

32. THE STORY CONTINUES…

33. …CHANGING STATES OF MATTER
Unit 1
(LESSON 6)

34. “CHANGING STATES of MATTER”
Unit 1 – LESSON 6
“CHANGING STATES of MATTER”

35. STATE OF MATTER depends on the BALANCE between TEMPERATURE and ENERGY
changing temperature causes a gain or loss in energy
changing the amount of energy causes a change in the motion of the particles
changing motion of the particles changes the distance and attraction of the particles to each other

36. What DOES CHANGE when changing States of Matter:
the energy of the particles (gain or lose)
the motion of the particles (fast or slow)
the attraction of the particles (more, less or none)
the distance of the particles (close or farther apart)
without a change in temperature and energy (outside forces) , matter would remain in its current state due to INERTIA

37. MELTING occurs when: temperature of a SOLID is raised
the SOLID’S particles gain energy
the particles of the SOLID move faster
the attraction of the SOLID’S particles weakens
the distance of the particles become farther apart  turns into a LIQUID

38. VAPORIZATION occurs when:
temperature of a LIQUID is raised
the LIQUID’S particles gain energy
particles of the LIQUID move faster
the attraction of the LIQUID’S particles weakens
the distance of the particles become farther apart  turns into a GAS

39. FORMS of VAPORIZATION:
EVAPORATION = changing of the SURFACE molecules only of a liquid into a GAS BEFORE reaching the boiling point temperature
BOILING = changing of ALL the liquid’s molecules throughout the liquid into a GAS AFTER reaching the boiling point temperature

40. MELTING and VAPORIZATION:

41. SUBLIMATION occurs when:
temperature of a SOLID is raised
the SOLID’S particles gain energy
particles of the SOLID move faster
the attraction of the SOLID’S particles weakens
the distance of the particles become farther apart  turns DIRECTLY into a GAS

42. BOILING; MELTING and SUBLIMATION:

43. CONDENSATION occurs when:
temperature of a GAS is lowered
the GAS’S particles lose energy
the particles of the GAS move slower
the attraction of the GAS’S particles strengthens
the distance of the particles become closer  turns into a LIQUID

44. FREEZING occurs when: temperature of LIQUID is lowered
the LIQUID’S particles lose energy
particles of the LIQUID move slower
the attraction of the LIQUID’S particles strengthens
the distance of the particles become closer  turns into a SOLID

45. DEPOSITION occurs when:
temperature of a GAS is lowered
the GAS’S particles lose energy
particles of the GAS move slower
the attraction of the GAS’S particles strengthens
the distance of the particles become closer  turns DIRECTLY into a SOLID

46. CONDENSATION and FREEZING:

47. LATENT HEAT:
“hidden heat” providing the energy for the molecules to be “rearranged” without making them move faster, which allows for continued melting/freezing or boiling/condensation without the overall temperature of the substance changing
HEAT of FUSION  going from a solid to a liquid and a liquid to a solid
HEAT of VAPORIZATION  going from a liquid to a gas and gas to a liquid

48. LATENT HEAT:

49. LATENT HEAT (hidden heat of physical changes):
the heat that is absorbed or released when a substance undergoes a physical phase change but does NOT make the substance change temperature
the heat of the water in
our atmosphere that
creates weather
patterns and provides
the powerful energy of
lightning and
thunderstorms

50. Law of Conservation of Energy:
the TOTAL amount of ENERGY ALWAYS STAYS THE SAME regardless of how many times it undergoes a physical or chemical change
ENERGY can change FORM, but it can NEVER be CREATED or DESTROYED

51. Law of Conservation of Energy:

52. Law of Conservation of MASS:
during a CHEMICAL REACTION, MATTER can NEVER be CREATED or DESTROYED
the TOTAL MASS ALWAYS STAYS THE SAME regardless of how many times it undergoes a CHEMICAL change
the ATOMS of the MATTER become REARRANGED, but their QUANTITIES remain CONSTANT

53. Law of Conservation of MASS:

54. Balancing Chemical Equations or STOICHIOMETRY:
occurs when the REACTANTS (left side) are EQUAL TO the PRODUCTS (right side) of a CHEMICAL EQUATION
both sides MUST contain THE SAME ELEMENTS and THE SAME number of ATOMS per ELEMENT

55. BALANCED EQUATION CONSERVATION of MASS 2 2 H = 2 4 2 4 1 2 2
Balancing Chemical Equations or STOICHIOMETRY: H2O  H2 + O2
BALANCED EQUATION
CONSERVATION
of MASS
REACTANT / original substances
PRODUCT / new substances 2 2
H =
O = 2 4
H =
O = 2 4 1 2 2
1st check for SAME “TYPE OF ATOMS” (ELEMENTS)
2nd check for SAME “NUMBER” OF ATOMS (exact count)
REMEMBER when balancing the equation:
ONLY change the coefficient count; NEVER the subscripts

56. BALANCING EQUATIONS
(STOICHIOMETRY):

57. THE
END of
Unit 1
(LESSONS #1-6)