Unit 2: Study of Matter You may already know why ice floats.
Ironically, if the ice was dry, it would sink. What explains that?
Slide 2 Unit 2 Objectives Definitions: matter, element, compound,
mixture, (chemical) symbol, heterogeneous, homogeneous, metal,
nonmetal, metalloid, physical change, chemical change, nuclear
change, Laws of conservation, exothermic, endothermic, Kinetic
Molecular Theory, real gas, ideal gas, change of state, phase
diagram, triple point, critical point. Differentiate between
elements, compounds, and mixtures. Arrange a matter hierarchy.
Identify chemical symbols for elements. Separate mixtures
physically. Differentiate between hetero- and homogeneous mixtures.
Sepearate metallic, nonmetallic, and metalloid elements. Determine
the physical and chemical properties of a substance. Distinguish
chemical and physical properties from chemical and physical
changes. Perform calculations using the Law of Definite
Composition. Slide 3 Unit 2 Objectives Pt.2 The Kinetic Molecular
Theory (KMT) is based on the idea that particles in matter are
always in motion. The KMT can be applied to describe properties of
solids, liquids, and gases. Boiling, melting, freezing are among
the physical processes that can alter a substances state. How to
interpret a phase diagram. Identify the triple point and critical
point. (EFS D4) To use systems thinking and systems tools to
identify patterns, impacts, and relationships between a products
life cycle and the health of the system as a whole. Embed their
understanding of the Materials cycle principle in their work. (EFS
D5) Articulate how human choices regarding consumption, production,
distribution, and disposal of material goods affect our ability to
thrive over time. Slide 4 Essential Questions How do the types of
substances elements and compounds differ? How do the states of
matter differ according to the Kinetic Molecular Theory? GUIDING
QUESTIONS: What are the characteristics of elements and compounds?
Why cant a compound be separated by physical means? What are the
different categories of elements? How do the properties of the
general types of elements compare? What are the characteristics of
mixtures? What physical means are used to separate mixtures? What
are the distinctions between matter and energy? Why are chemical
and physical properties important? What is the importance of the
Laws of Conservation of Matter and Energy and Definite Composition?
How are physical, chemical, and nuclear changes distinguished? What
is the Kinetic Molecular Theory of Matter? How can the theory be
used to describe matter? How does a real gas differ from an ideal
gas? What is a change of state? What occurs when a substance
undergoes a change of state? What is a phase diagram and how is it
interpreted? Slide 5 Your Take How many atoms are in the body?(P3)
What is plasma? What is dark matter? How do we measure how much
matter is present? How are they able to organize the elements onto
a table? (P5) How is aluminum made? Are there more than the four
common states of matter? Can you turn lead into gold by firing
other atoms at it? (P7) How do they find new elements? Why could
lead be in our water? Cornstarch + Water = ??? Where did the names
of elements come from? Slide 6 Castagno Chemistry Challenge II
Rules: 1) Do NOT help anyone else. 2) You have a maximum of 10
minutes to complete the challenge. 3) Credit only goes to
COMPLETELY correct answers 1 st 2pts, 2 nd 1pt, 3 rd 0pts, 4 th
0pts Questions? Slide 7 The Challenge Organize the matter
hierarchy.matter hierarchy Slide 8 What Is Matter? As defined in
Unit 1, matter is anything that has mass and occupies space
(volume) There are 3 visible in this picture, sort of. Slide 9
Classification of Matter Can it be separated? Pure substances
Mixtures Can it be decomposed by ordinary chemical means? Is the
composition uniform? CompoundsElements Heterogeneous mixtures
Homogeneous Mixtures Forward Slide 10 Mixtures A mixture is a
combination of two or more substances. Substances can be elements
or compounds. Mixture can be easy to identify or not. Slide 11
Solid - Solid Jewelry alloys Rocks Slide 12 Solid - Liquid Iced Tea
Chocolate Milk Aka Powdered-drink mixes Slide 13 Liquid-Liquid
Liquid mixture Vinegar and other household liquids Slide 14 Liquid
- Solid Mercury in Silver dental amalgam (filling) Slide 15 Liquid
- Gas Fog Slide 16 Gas Liquid Carbonated- beverages Slide 17 Gas
Gas Atmosphere Slide 18 Mixtures II Separation Anxiety Mixtures can
be separated physically Filters based on particle size Distillation
based on boiling point Centrifuge based on density Back Slide 19
Homogeneous Mixtures Uniformity throughout the entire mixture. Back
Slide 20 Heterogeneous Mixtures Easy to identify different
materials within the sample. Different colors stand out Different
densities settle into layers Back Slide 21 Pure Substances FIXED
composition Each sample (like salt) has the same Composition
(make-up) Characteristics (color, density, etc.) Back Slide 22
Compounds Composed of chemically bonded atoms of different elements
Individual Molecules (water) Ionic crystals (salt) Back Slide 23
Elements (I) A pure substance composed of atoms that can not be
broken down into simpler, stable substances. Slide 24 Elements (II)
Symbols Every element is abbreviated with a symbol Saves space on a
periodic table Makes writing formulas much easier Some are common
or make sense C carbon Al aluminum But some seem very out of place
Slide 25 Elements (III) Symbols (II) Challenge #2 Thou fhouldeth
puteth thyne notebookf away. Medieval Matching Game Slide 26
Elements (IV) - Identification Challenge #3 Notebooks away! The
rare back-to-back challenge! Can you identify the elements as
metallic, nonmetallic, metalloid, or the single, very special,
undecided one?identify the elements Slide 27 Elements Examples 1)
Worlds largest gold bar, 250kg Estimated worth (9/30/13):
$10,663,679 ($42.53/g) 2) The Hope Diamond (carbon) Estimated
worth: $350,000,000 ($38,461,538/g) 3) Chunks of Boron Estimated
worth: $11.14/g (pure) Slide 28 Elements (V) - Metals As challenge
#3 revealed, the majority of elements are metallic. Typical
properties associated with them Conductors of heat and electricity
Malleable (sheets, foils) Ductile (wires) Slide 29 Elements (VI)
Nonmetals The second largest category of elements are nonmetallic
Opposite properties of the metals Poor conductors of heat and
electricity Brittle Typically break instead of flatten into sheets
or wires Of course, most nonmetals are gases so how can you flatten
a gas anyway? Slide 30 Elements (VIII) Metalloids Just a few
elements, located on the staircase, have intermediate properties.
Less malleable than metals Less brittle than nonmetals
Semiconductors Not as conductive as a metal, more conductive than a
nonmetal Slide 31 Elements (IX) Specialty Hydrogen! Typically non-
metallic with all associated properties However, it is believed to
behave as a metal inside the gas giants Jupiter and Saturn. This
metallic form helps explain the massive magnetic fields those
planets have. Back Slide 32 Check Yourself Challenge #4 - Notebooks
away! Class Quiz Slide 33 The Grand Unified States of Matter The
extremely rare double back- to-back Challenge #5 Notebooks out!
Describe as much as possible of the 4 examples of matter located on
the desks in the classroom. Slide 34 States of Matter So we know
there are 4 states of matter but do any others exist? Fundamental
(4) Solid, liquid, gas, plasma Non-classical (8*) Glass, plastic
crystal, liquid crystal, magnetically ordered (ferro-, antiferro,
ferri- magnet), Copolymers, Quantum spin liquids Low-Temperature
States (7*) Superfluid, Bose-Einstein Condensate, Fermionic
condensate, Rydberg molecule, Quantum Hall State, Strange matter
(quark), Photonic matter (formed September 2013) High Energy States
(3*) Quark-gluon plasma, color-glass condensate, gravitational
singularity (VERY high energy) Other proposed states (6*)
Degenerate matter, supersolid, string-net liquid, superglass, dark
matter, equilibrium gel Total: 4 + 8 + 7 + 3 + 6 = 28 (source:
wikipedia) Slide 35 Kinetic Molecular Theory Every state of matter,
from the normal to the strange, have one thing in common: Manner of
definition Each state of matter is defined by the movement of the
particles within. Slide 36 Kinetic Molecular Theory II The KMT is
what describes the movement It can be applied specifically to each
state of matter Slide 37 Gas The Kinetic Molecular Theory has 5
distinct points for gases 1) Individual particles are far apart
relative to their size 2) Collisions between particles and
containers are elastic (no energy loss) 3) Particles are in
constant motion 4) No forces of attraction between particles 5)
Temperature of the gas depends on the average kinetic energy of the
particles Slide 38 Gas II Steam and smoke are good examples. The
KMT describes 1) Indefinite shape (only containers define the
shape) 2) Indefinite volume (any amount fills a container) Slide 39
Gas III 3) Low density & 4) High compressibility Gas particles
are very far apart 5) Fluidity Gas particles always moving Slide 40
Gas IV 6) Expansion (Gas tanks) Volume can grow 7) Diffusion
(Scented candle) Spreading through an area 8) Effusion (flat tire)
Escape tiny opening Slide 41 Solid What explains solids always
keeping their shape? 1) Specific, repeating pattern of atom
arrangement 2) Particles vibrate in position Slide 42 Solid II Lack
of movement explains 1) Definite volume 2) Definite shape 3)
Incompressibility Close arrangement results in 4) Typically high
density (solid v liquid v gas of the same substance) Slide 43
Liquid Unlike solids, liquids particles are not in fixed positions
They do remain fairly close together This allows a liquid to take
any shape Slide 44 Liquid II Shifting positions explains Fluidity,
Indefinite shape Closeness of particles means Definite volume Still
fairly dense (usually less so than the solid, water is an
exception) Relatively incompressible Slide 45 Plasma Typical
properties of a gas except most/all particles are ionized (charged)
Extremely common, albeit temporarily seen on Earth Slide 46 St.
Elmos Fire* A weather phenomenon typically produced during
thunderstorms. There needs to be a sustained imbalance Of electric
energy often found in places we would consider a lightning rod.
When a limit is, reached, the energy is discharged into the glow of
fire. Slide 47 STOP! In the name of conservation! Challenge #6
Notebooks closed! There are two major laws (among many) that we
encounter in this class. What are they? Slide 48 Conservation of
Matter In chemical reactions, matter cannot be created nor
destroyed. 20g of reactants will form a minimum and maximum of 20g
product. Slide 49 Conservation of Energy The amount of energy
present in a system will remain constant. The energy present could
cause a change, such as melting of an ice cube, but overall energy
is conserved. Slide 50 Ch-ch-changes! Challenge #7 Notebooks away!
There are 6 changes of state between solid, liquid, and gas. Name
the transition AND the associated change (ie: L -> G) Slide 51
Properties The characteristics of substances are known as
properties Physical Chemical Forward Slide 52 Physical Properties
Can be described by sight or feel Color Texture or measured without
changing the substances identity Melting/Freezing Point, Boiling
Point Density Slide 53 Physical Changes When a substance changes
form but not identity Crush Tear Rip Boil Freeze Condense Melt
Sublimate Deposit Back Slide 54 Chemical Properties Ability of a
substance to undergo change to form a new substance Aka identity
changes Cannot be determined by simply looking at the substance
Slide 55 Chemical Changes The substance undergoing a transformation
into a new substance(s) Adding sodium to water causes this Back
Slide 56 Physical and Chemical Change Physical Change The substance
changes form Melt, Boil, Freeze, Condense, Sublimate, Deposit,
Crushed, Torn, Smashed Chemical Change The substance changes
identity React, Burn, Oxidize, Reduce Slide 57 Phase Diagrams
Challenge #8.1 Notebooks away! Describe what is happening from A to
B B to C C to D D to E E to F Slide 58 Phase Diagrams Challenge 8.1
Slide 59 Phase Diagrams Challenge #8.2 Notebooks away! Describe
what is happening from A to B B to C C to D D to E E to F Slide 60
Phase Diagrams Challenge 8.2 Slide 61 Phase Diagrams Challenge
Answers 8.1 A to B = solid heating B to C = melting C to D = liquid
heating D to E = boiling E to F = vapor heating 8.2 A to B = vapor
cooling B to C = condensing C to D = liquid cooling D to E =
freezing E to F = solid cooling Slide 62 Phase Diagram - Cooling A
cool curve is a graph which shows the temperature of a substance
decreasing over time. Phase changes that occur during this process
are Condensing Freezing Slide 63 Phase Diagram Cooling II Phase
changes occur during segments of no temperature change FREEZING
CONDENSING Solid Liquid Gas Slide 64 Phase Diagram Cooling III
Condensing (Gas to Liquid) The process of a gas becoming a liquid
Requires a LOSS of energy (cooling) Freezing (Liquid to Solid) The
process of a liquid becoming a solid Requires a LOSS of energy
(cooling) Slide 65 Phase Diagram - Heating A heating curve is a
graph which shows the temperature of a substance increasing over
time. Phase changes that occur during this process are Melting
Boiling Slide 66 Phase Diagram Heating II Phase changes occur
during segments of no temperature change MELTING BOILING Solid
Liquid Gas Slide 67 Phase Diagram Heating III Melting (Solid to
Liquid) The process of a solid becoming a liquid Requires a GAIN of
energy (heating) Boiling (Liquid to Gas) The process of a liquid
becoming a gas Requires a GAIN of energy (heating) Slide 68 Phase
Diagram - Review Whether heating (L) or cooling (R), CHANGES IN
STATE occur on the FLAT LINES Boiling/Condensing higher
Melting/Freezing lower BC MF Slide 69 Phase Diagram - Y Challenge
#9 Notebooks away! Slide 70 Phase Diagram - Y Label X, Y, Z, D, and
E X Z? Z X? X Y? Y X? Y Z? Z Y? Slide 71 Phase Diagram - Y Label X
= Solid Y = Liquid Z = Gas D = Triple Point E = Critical Point X Z
= sublimation Z X = deposition X Y = melting Y X = freezing Y Z =
boiling Z Y = condensation Slide 72 Phase Diagram Y II Area X is
always a solid Area Y is always a liquid Area Z is always a gas On
the line = both (equilibrium) Critical Point = liquid state cannot
exist beyond this temperature Triple Point = all 3 states of matter
in equilibrium Slide 73 Phase Diagram Y III Sublimation (Solid to
gas) The process of a solid becoming a gas by SKIPPING the liquid
state Requires a GAIN of energy (heating) Deposition (Gas to Solid)
The process of a gas becoming a solid by SKIPPING the liquid state
Requires a LOSS of energy (cooling) Note: Since the Y-diagram is a
pressure/temperature comparison, ANY change can occur by simply
altering the pressure.
