THE STORY CONTINUES…

…STATES OF MATTER Unit 1 (LESSON 5)

Unit 1 – LESSON 5 “STATES of MATTER”

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

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

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

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

GASES: Kinetic-Molecular Theory of Matter

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)

LIQUID: Kinetic-Molecular Theory of Matter

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

SOLID: Kinetic-Molecular Theory of Matter

Summary: Kinetic-Molecular Theory of Matter

“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)

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

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

TYPES SOLIDS: CRYSTALLINE and AMORPHOUS CRYSTAL and AMORPHOUS ALLOTROPES

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

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

PROPERTIES of LIQUIDS: ADHESION, COHESION & SURFACE TENSION and VISCOSITY http://apod.nasa.gov/apod/ap130424.html SURFACE TENSION

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

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

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]

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

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

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

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

“4th” State of Matter: PLASMA

THE END FOR NOW… UNIT 1 (LESSON 5)

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

THE STORY CONTINUES…

…CHANGING STATES OF MATTER Unit 1 (LESSON 6)

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

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

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

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

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

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

MELTING and VAPORIZATION:

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

BOILING; MELTING and SUBLIMATION:

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

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

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

CONDENSATION and FREEZING:

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

LATENT HEAT:

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

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

Law of Conservation of Energy:

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

Law of Conservation of MASS:

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

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

BALANCING EQUATIONS (STOICHIOMETRY):

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