Unit 4- Mixture and
Compounds Notes
Model So Far…..
• Key Concept 1: Everything has been a simple “pure”
particle…..
What are the two categories of
“stuff” that exist?
REVIEW FROM UNIT 1
c
• Key Concept 2: Matter is anything made of
atoms.
• Matter has observable and measurable
qualities.
– Key Concept 3: Two basic types of
properties of matter: physical properties
and chemical properties.
– Key Concept 4: All matter can undergo
change: physical change or chemical
change
REVIEW FROM UNIT 1
Properties
–Key Concept 5: Physical properties can be
observed without changing the
substance(use your senses).
–Key Concept 6: Chemical properties are
determined by trying to change the
make-up of a substance (only evident at
the particle level).
RIVIEW FROM UNIT 1
Change
– Key Concept 7: Physical change- the original
substance still exists (its particles are still the
same); it has simply changed form.
– Key Concept 8: Chemical change- takes place
on the molecular level and produces a new
substance (chemical changes are accompanied
by physical changes) (hard to undo).
What are some properties of….
Sugar
Salt
Iron
Key Concept 2: Water vs. Ethanol
Property
Appearance
Odor
Flammability
Density
Melting Point
Boiling Point
Chem/Phys
Water
Ethanol
What happens to the properties if I
mix water and ethanol?
• Solubility?
• Density?
• Boiling points?
• Physical Change, not chemical
• Crude Oil and fractional distillation
What happens if I mix sulfur (S) and
iron (Fe) together?
• Chemical Change
Change and Properties
• Key Concept 3: Physical change- mixed two
particles together, but no reaction.
– Some properties are the same as the original
substance (MP and BP), and other are a mix of
those properties(density).
• Key Concept 4: Chemical change- mixed
particles react to form a new product.
– All the physical and chemical properties have
changes.
We made mixtures
“Elemental”
“Mixture”
Is the new product a mixture?
“Elemental”
“Compounded”
End of Day
Key Concept 5
A type of matter
Examples: steel, air, water,
vegetable soup
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Heterogeneous
Characteristics of mixture
Key Concept 6:
Homogenous- “homo” same or alike
Heterogeneous- “hetero” different
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Heterogeneous
Heterogeneous
Mixture
Heterogeneous Mixture
Key Concept 7: Heterogeneous mixtures- are
composed of large pieces that are easily separated
by physical means.
• You can see with your eyes (you might need a
microscope for some) that the composition is not
the same throughout
• Components are distinguishable
• Examples: fruit salad, vegetable soup, etc.
Heterogeneous Mixture
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Homogenous
Mixture
Heterogeneous
Heterogeneous
Mixture
Homogenous Mixture
Key Concept 8: Homogenous mixtures- looks the
same throughout but can be separated by physical
means.
• If you break a piece of homogeneous matter into
smaller pieces, each piece will have the same
properties as every other small piece.
• If you look at one of the pieces under a
microscope, it is impossible to distinguish one part as
being a different material from any other part.
• Examples: air and glass
Homogenous Mixture
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Heterogeneous
Homogenous
Mixture
Solution
Heterogeneous
Mixture
Solution
Everyday definition
• Answer to a problem
• A type of liquid
Chemistry
• Key Concept 9:
Solution- uniform
mixture that can
contain solid, liquid, or
gases
Solution = Homogenous mixture
They are synonyms
How a solution is made?
• Solution consist of a
solvent and solute.
• Key Concept 10:
Solvent- the substance
that dissolves the solute
to form a solution; most
plentiful substance in
the solution.
• Solute- one or more
substance dissolved in a
solution.
How a solution is made?
Important vocabulary
Soluble
Insoluble
Alloy
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Pure Substance
• Key Concept 11: Pure Substance- Consists of
only one component with definite physical
and chemical properties.
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Element
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Element
• Key Concept 12: Elements- composed of 1
type of atom
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Element
Compound
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Compound
• Key Concept 13: Compound – is composed of
two or more different elements chemically
bonded together.
Demo 3
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Element
Compound
Can be separated
only by chemical
means.
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Can be separated
using physical
means.
Key Concept 14: Make a 4 column T chart
Pure Substances
Mixtures
Element Compound Homo. Mixture
Heter. Mixture
Example for T chart
•
•
•
•
•
•
•
•
•
•
Water
Ethanol
Water mixed with ethanol
Sulfur
Iron
Iron Sulfide
Sugar
Sea Water
Vegetable Soup
Orange Juice
BIG IDEA for Unit 4
• Key Concept 1: Everything has been a simple
“pure” particle….. But now we need to
illustrate matter as either a mixture
(homo/hetero) or a pure substance
(compound/element).
Separating Techniques
• The primary concept of chemistry is the
classification of matter.
• You have learned that matter can be a pure
substance or a mixture that is homogenous or
heterogeneous.
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Element
Compound
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Separating Techniques
Key Concept 15:
Why is this
important to
understand
separation
techniques?
Why is are separation
techniques important?
• “For some 1.1 billion people, sufficient, safe,
acceptable, accessible and affordable water
for life is a hope for the future, not a reality
for the present.”
• 17 % OF HUMANITY WITHOUT ACCESS TO
CLEAN WATER !!
Why is this important
Why is this important
PBS News Hour: Haiti
Why is this important
Why is this important
Why is this important
Why is this important
• 0.7% sodium hypochlorite liquid solution used
to treat drinking water at "point of use“.
Electrochlorination is the process of
producing hypochlorite by running an
electric current through salt water.
NaCl + H2O + ENERGY → NaOCl + H2
Why is this important
Why is this important
NaCl + H2O + ENERGY → NaOCl + H2
Why is this important
Separating Techniques
• Settling
– Used to separate substances with different
weights
• Sifting
– Used to sort solids by size.
Separating Techniques
• Decanting: Used to separate an
insoluble solid from a liquid by
carefully pouring off the liquid.
Based upon differences in
density.
Separating Techniques
• Key Concept 16: Filtration
– Used to separate a liquid
and an insoluble solid.
• Alum
– Added to a liquid to promotes coagulation of
suspended particles which is then filtered.
Separation Techniques
• Key Concept 17: Evaporation: Used to
separation of a liquid and a soluble solid.
Separation Techniques
• Crystallization: Slow formation of a solid from
a warm solution that is cooled.
Separation Techniques
• Key Concept 18: Distillation: Used
to separation two miscible liquids,
that have different boiling points.
• If two liquids are miscible they
form a homogeneous mixture
when added together.
Miscible = Mix M&M
• It is made possible due to the fact
that each liquid has its unique
boiling point.
Separation Techniques
• Key Concept 19: Separating
Funnel: used in separate the two
immiscible liquids with different
densities.
"water is immiscible with suntan oil”
“alcohol is miscible with water”
Separation Techniques
• Key Concept 20: Magnetism: used to
separate out any substance based on its
magnetic properties.
Separation Techniques
• Paper Chromatography: used to
separate soluble substances from
one another based upon
differences in size as a solvent
moves over paper.
Defining a process with
word you don’t know
Miscible
Immiscible
Solute
Soluble
Insoluble
Why is this important
• How is your drinking water cleaned?
End of Day
Practice Problems 4ASpeed Dating
Reading Atoms From
Democritus to Dalton
These Key Concepts will be summarized from
the reading:
•
•
•
•
•
Key Concept 21: Empedocles
Key Concept 22: Democritus
Key Concept 23: Torricelli & Bernoulli
Key Concept 24: Priestley
Key Concept 25: Lavoisier
Goal of this reading: Understand some key
hypothesis that will allow us to get out of the
particle model.
Dalton
• Key Concept 26: Dalton
Dalton’s atomic theory
• Key Concept 27: Dalton's atomic theory had
four main concepts:
– All matter is composed of indivisible particles
called atoms.
– All atoms of a given element are identical;
atoms of different elements have different
properties.
– Chemical reactions involve the combination of
atoms, not the destruction of atoms.
– When elements react to form compounds, they
react in defined, whole-number ratios.
Dalton’s atomic theory vs.
Atomic Theory
Practice Problems B- # 1-3
End of Day
Water?
Question still to answer?
• Density- Practice Problems Unit 1C
Particle diagram illustrating density
What substance has the greatest density and
how do you know?
Iron (Fe)
Aluminum (Al)
Is everything a simple particle?
• One of the greatest challenges early chemists
faced was trying to find a way to connect the
mass of a substance to the number of
particles in the sample.
• If we knew how atoms combined together, we
could deduce the mass of different types of
atoms.
Battle of understanding
simple combinations
Coming to Understand Simple
Combinations
• Read out loud as a group taking turns.
• Go in a circle each person reading a
paragraph.
• Answer each key questions on the paper as
you go.
• Whiteboards/poster and markers are available
at lab table 6.
End of Day
Guy-Lussac Experimental Evidence
Guy-Lussac found that one volume of
water vapor was not produced, but
two equal volumes.
Avogadro’s Hypothesis
• Key Concepts 28: Avogadro assumed
– Equal volumes of gases have equal numbers of
molecules.
– These particle can be split into half-particle during
chemical reactions (particles of some gaseous
elements must contain two atoms.)
– That particle of elemental gases could contain
more than a single atom.
Avogadro’s Hypothesis
• Two volumes of hydrogen react with one
volume of oxygen to produce two volumes of
water when hydrogen and oxygen can be split
into half-molecules!
Avogadro’s Hypothesis
• If we accept Avogadro’s Hypothesis, we can
compare the mass of various gases and
deduce the relative mass of the molecules.
• To do this, we pick a weighable amount of the
lightest element (how about 1.0) then use
mass ratios to assign atomic masses to the
other elements.
Molecular vs. Compound
• Key Concept 30: A molecular is made of one
or more elements (7 + 1).
Dalton, Gay-Lussac, and
Avogadro
NOS?
Homework- Due
• Write a letter as if you were Avogadro to
Dalton and Guy-Lussac.
• You will need to explain how your hypothesis
can be used to explain Dalton's density
problem and excepts Guy-Lussac law of
combining volumes.
• Couple of paragraphs
End of Day
Is everything a simple particle?
• One of the greatest challenges early chemists
faced was trying to find a way to connect the
mass of a substance to the number of
particles in the sample.
Avogadro’s Hypothesis
• If we accept Avogadro’s Hypothesis, we can
compare the mass of various gases and
deduce the relative mass of the molecules.
• To do this, we pick a weighable amount of the
lightest element (how about 1.0) then use
mass ratios to assign atomic masses to the
other elements.
• 36:30 to 37:50
• https://www.youtube.com/watch?v=ADYiwJ6
exf4
Relative Mass
• To assign relative masses to elements it is
necessary to know that the samples being
compared have the same number of
particles
– If particles are all the same size, the same size
sample would have the same number of
particles
– If particles are different sizes, the same size
sample would have different numbers of
particles
Particle diagram illustrating density
What substance has the greatest density and
how do you know?
Iron (Fe)
Aluminum (Al)
ANSWER
• The best way is…..
– If it is a gas (same number of particle per unit
volume)
– If it is a liquid or gas (different number of particle
per unit volume due to how close the atoms are
and the size of the atoms)
PIQ- next class period
Review Practice Problems A & B
A type of matter
Examples: steel, air, water,
vegetable soup
Homogenous
Pure
Substance
Element
Compound
Heterogeneous
Homogenous
Mixture
Solution
Solvent + Solute
Heterogeneous
Mixture
Out of the particle level
Our model has to change…….
Elements
Compounds
Mixtures
Ionic Compounds vs. Molecular Compounds
Ionic vs. Molecular
Compound Demos
Ionic vs. Molecular
Properties Summary
State
(Room Temp.)
Ionic
Compounds
Molecular
Compounds
Solubility in
water
Conductivity
Boiling
Point
Melting
Point
Strength of
Intermolecular
Forces
End of Day
Understanding chemical bonding
starts with a very important
question?
What type of compound is it?
What type of compound is it?
Ionic Compound
vs.
Molecular Compound
What type of molecule is it?
Ionic Compound
• There is a transfer of
electrons that forms an
ionic bond.
Molecular Compound
• There is a sharing of
electron through a
covalent bond.
Properties Review
What is different about these two compounds:
NaCl (table salt)
vs.
C6H12O6 (sugar)
Get out Demo Sheet- Properties Review
What if we just look at the compounds that conducted
electricity
Compound
Conductivity
Tap water (H2O and salts)
Yes
Sodium Chloride (NaCl)
Yes
Magnesium Sulfate (MgSO4)
Yes
Potassium Chloride (KCl)
Yes
What do these compounds have in common?
What is an ionic compound?
• How would you define a salt?
– A salt is just an ionic compound
• So what is an ionic compound?
– Key Concept 31: Ionic Compound: consists of a
metal and a non-metal bound together in a lattice
structure by ionic bonds.
Ionic Compounds
• Ionic Compound = metal + nonmetal
or cation + anion
Ionic Compounds
• Key Concept 32
– Cation – positively charged ion
– Anion – negatively charged ion
• Polyatomic Ions
–
–
–
–
“Poly” = many
“atomic” = atoms
Ion = charged
Polyatmoic ion = many atoms bonded together having
an overall charge
– See periodic table
WE NEED A TOOL TO DETERMINE
IF AN ELEMENT WILL BE A
CATION OR ANION
• This is a “tell”…..
• We have a tool and it is called the periodic
table.
• Why this tool works won’t come until Unit 6
& 7 next semester.
• Right now I just need you to correctly use the
tool.
Ionic Compounds
• Ionic compounds consist of a cation (metal)
bonded with an anion (non-metal).
• Key Concept 33: Polyatomic ions themselves
are not ionic compounds, but they form ionic
bonds when paired with a metal.
Properties of ionic compounds
• When compounds conduct electricity they are
also called electrolytes.
• Where have you heard the term electrolyte
before?
Key Concept 34 : Properties of ionic compounds
A. Conductivity
– Ionic compounds conduct electricity because of the
presence of ions.
B. Solubility
– Ionic compounds are soluble in water.
Properties of ionic compounds (cont)
C. Melting Point
– Ionic compounds have a very high melting point
because of the bond strength within the compound
D. Intermolecular Forces
– Ionic compounds have very strong intermolecular
forces causing a very high bond strength
– This causes all ionic compounds to be found in the
solid state at room temperature
Ionic Bonding
• Key Concept 35: Ionic Bond– forms through a
transfer of electrons that causes an attraction
between 2 oppositely charged ions.
• Review: What is an ion?
– Different number of electrons from protons
– Not a neutral atom
– Contains a charge
Ionic Bonding (cont)
• Ionic bond is formed through electrostatic
attraction between 2 oppositely charged ions
• These ions are attracted to one another and
form what is called a lattice or crystalline
structure
Why do these properties exist?
• Key Concept 36: This lattice structure and strong
interaction between ions is what causes the high
bond strength and high melting point and solid
state at room temperature
• When ionic compounds interact with water, the
ions are more attracted to the water molecules
so the lattice dissociates
• Key Concept 37: The dissociation of the ions is
what causes ionic compounds to conduct
electricity
dissociation animation
Key Concept 38: Properties of Molecular
Compounds
A. Conductivity
– Molecular compounds do not conduct electricity
B. Solubility
– Molecular compounds are generally not soluble in
water
Properties of Molecular compounds (cont)
C. Melting Point/Boiling Point
– Molecular compounds have a very low melting point
or boiling point because of the bond strength within
the compound
D. Intermolecular Forces
– Molecular compounds have very weak intermolecular
forces causing low bond strength
– This causes most molecular compounds to be found in
the liquid or gas state at room temperature
Bonding in Molecular Compounds
• Molecular compounds contain covalent bonds
• Key Concept 39: Covalent bond– the sharing of
electrons in an atom to form a bond.
Bonding
Chemistry is about stability
• Some molecules are more stable when they are found as
diatomic – two of the same element covalently bonded
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Bonding
Time to process and organize
Make some type of graphically
organizer over the properties of
ionic compounds vs. molecular
compounds
Get Creative
End of Day
Basic properties of ionic
and molecular compounds
•
•
•
•
•
•
Composition
Conductivity
Solubility
Melting/Boiling Points
Intermolecular Forces
Types of Bonds
Bonding – can be modeled with people!
Ionic Bond
vs.
Covalent Bond
What other information do
we need to know?
Ionic Compounds
• How to name and write the
formulas
• Use common ions to predict
the products of a chemical
formulas
Molecular Compounds
• How to name and write
formulas
• Draw Lewis Structures (NOT
UNTIL NEXT SEMESTER)
90%
10 %
Why is naming important?
• What does your name mean to you?
• Where did your name come from? Would
anyone like to share?
• In other cultures, names can come from
tradition and have different meanings.
• We are going to look at a few different
cultures and how they determine names
Spain
• Most people have one or two given names, followed
by two surnames.
• The first surname (considered the primary surname)
is inherited from the father's paternal surname
• The second is inherited from the mother's paternal
surname.
• Women usually keep their names when they marry.
• Example - If José Lopez Garcia marries María Reyes
Cruz, both will keep their surnames unchanged. If
they have a child named Tomás, his full name will be
Tomás Lopez Reyes.
Africa
• Traditional African given names often reflect
the circumstances at the time of birth.
– time or day when the child was born.
– birth order of the newborn,
– describe the parents' reaction to the birth
– descriptive of the newborn or of desired
characteristics
• Example: Esi "Sunday“ Mosi "first born"
Chinese
• A modern Chinese name consists of a
surname (xìng 姓) and a given name (míng 名
or míngzì 名字), usually presented in that
order.
• When transcribed into western writing, the
characters of the given name are often written
separately.
• Sometimes the first character of the given
name is shared by all members of a
generation in a family
Navajo
• Navajo name is considered so precious it’s only used during
ceremonies, meaning a day-to-day conversation in a Navajo
family may go something like “Mother, go get Son.”
• The Salish tribe follows a “naming trail” in which the name
given to a baby by his parents at birth (usually a virtue or
trait the parents hope for the baby) is eventually replaced
at adolescence with another name that is given by the
tribal leader at a ceremony called the Jump Dances.
• This name usually represents a talent or strength for which
the child is known.
• Navajo naming is done through ceremony and names are
symbolic of traits, tribes, animals, or virtues
Chemistry
• In chemistry, compounds and elements are
named using the IUPAC system of naming
– International union of pure and applied chemistry
• This system ensures that everyone in every
language will know what a compound is based
on its name
• There are a set of rules for naming different
types of compounds
Naming Rules – Ionic Compounds
• There are 3 different “types” of naming rules for
ionic compounds based on what metals and
nonmetals are involved
– Type A: metal (cation) + nonmetal (anion)
• NaCl
– Type B: metal (cation) + polyatomic ions (anion)
• CaCO3
– Type C: transition metal (cation) + nonmetal/ or polyatomic (anion)
• CuCl
Pass out- Formula to Name
Graphical Organizer
Glue it on a new clean page
Key Concept 40: Formula to Name– Ionic
Compounds
Type A
Metal + Nonmetal
1. Name the metal
2. Name the nonmetal
3. Change the ending of the nonmetal to “ide”
Example: NaCl – sodium chloride
Naming Rules – Ionic Compounds
Type B
Metal + Polyatomic ion
1. Name the metal
2. Name the polyatomic ion, DO NOT change
the ending
Example: CaCO3 – calcium carbonate
EXCEPTION ALERT!!
• There is 1 polyatomic ion that is a cation,
which means it is NOT a metal
• NH4+ - ammonium
• Example: NH4NO3 – ammonium nitrate
Naming Rules – Ionic Compounds
Type C
Transition Metal + Nonmetal
1. Name the transition metal
2. Figure out the charge of the transition metal
and place in Roman numerals in parenthesis
3. Name the nonmetal:
• If it is a regular nonmetal – change the ending to “ide”
• If it is a polyatomic ion – DO NOT change the ending
Example: CuCl – copper (I) chloride
Ionic Compounds- Formula to
Name Practice
• What naming type should I follow (A, B, or C)
and then determine the correct name.
• NaF
• KSO4
• CaCl2
• NH4NO3
Pass out- Name to Formula
Graphical Organizer
Glue it on a new clean page
Key Concept 41: Name to Formula
– Ionic Compounds
1. Refer to the periodic table for the proper
symbols and oxidation number.
2. Using the oxidation numbers determine what
neutral compound will form (draw out if
needed).
3. Use subscripts to indicate the number of
each atom needed (if more than one
polyatomic exist, put the polyatomic in
parenthesis).
Here is a tell…… how to determine
oxidation numbers.
Oxidation Numbers
• We won’t get to why this trend exists on the
periodic table until Unit 6 & 7.
• Right now, use the periodic table as a tool and
the understanding of WHY will come next
semester.
Ionic Bonding (cont)
• Work with your shoulder partner to determine
the most likely charge for the following:
– Chlorine
– Sulfur
– Sodium
– Nitrogen
– Aluminum
– Potassium
Ionic Bonding (cont)
Ionic Compounds- Name to
Formula Practice
• Lithium Chloride
• Magnesium Sulfide
• Calcium Nitride
Ionic Compounds- Name to
Formula Practice
• Copper (II) sulfate
• Copper (I) sulfate
• Aluminum hydroxide
Ionic Compounds- Ions to Names
Bonding With A Classmate
Go bond until the bell….
Watch the clockClosure is Be the Teacher
Change name tags every third bond
End of Day
What other information do
we need to know?
Ionic Compounds
• How to name them
• Use common ions to predict
the products of a chemical
reaction
Molecular Compounds
• How to name them
• Draw Lewis Structures
(NEXT SEMESTER)
90%
10 %
Key Concept 42: Formula to Name
• The rules for molecular compounds are much
easier than ionic (no exceptions)
1. Name First Element (Use prefix on first element
if more than one)
2. Use prefix name second element
3. Change suffix to –ide.
Example: N2O5
NO2
Naming Rules- Molecular Compounds
• Greek Prefixes
1 = mono
2 = di
3 = tri
4 = tetra
5 = penta
6 = hexa
7 = hepta
8 = octa
9 = nona
10 = deca
Key Concept 43: Name to Formula
1. Refer to the periodic table for the proper
symbols
2. Use prefix in the name to determine
subscripts needed.
Example: triphosphorus hexafluoride
carbon dioxide
You have seen molecular
represented like this
Speed Dating
Understanding chemical bonding
starts with a very important
question?
What type of molecule is it?
Tomorrow Combined Practice
End of Day
Properties of Water - demos
• How many drops of water can a penny hold?
• Will a needle float or sink in water?
Properties of Water
• Why can this bug
“walk” on water?
• Why does water form
a meniscus with glass?
Properties of Water
• Why did the top of the penny hold so many
drops of water?
• Why can the bug walk on water?
• Why did the needle float at first in the water?
• Key Concept 44: Surface tension – an inward
force that tends to minimize the surface area
of a liquid; it causes the surface to behave as if
it were a thin skin
Properties of Water
• Water has polar, covalent bonds and interacts
with other water molecules by hydrogen
bonding
• Hydrogen bonding is an intermolecular force
and is part of the reason for water having the
properties we just saw
• Key Concept 45: The intermolecular forces in
water is called hydrogen bonding. These
intermolecular forces are very strong for a
liquid.
Covalent bond
Hydrogen bond
Properties of Water
• Why does water form a meniscus?
• Key Concept 46: Capillary action – ability of a
liquid to move up a surface against the forces
of gravity.
• With water, this is due to the water molecules
hydrogen bonding with the glass molecules
Properties of Water
• Because of the surface tension and hydrogen
bonding, water has a very high specific heat
capacity
– amount of heat energy required to raise the
temperature of an object by a given amount.
Properties of Water
• These properties of water help answer many
different questions about the “odd” behavior of
water under different circumstances
• Why are snowflakes shaped the way they are?
• Why do oil and water not mix?
• Why do ionic compounds dissolve in water and
conduct electricity?
• Why does solid water (ice) float in liquid water? (with
other substances, the solid state is more dense than
the liquid state).
Crash Course
• https://www.youtube.com/watch?v=HVT3Y3_
gHGg
Four different fact from the video
•
•
•
•
Key Concept 47:
Key Concept 48:
Key Concept 49:
Key Concept 50:
Understanding chemical bonding
starts with a very important
question?
What type of molecule is it?
Combined Practice: Rotation Station
END OF UNIT 4