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Chemistry Workbook Chapter 2 Matter
Spring 2016
Chapter 2
Matter
2.1 Classification of Matter
Anything that has mass and volume is matter. Matter is also
defined as anything with the property of inertia.
PA Standards
Mass is a measure of the quantity of matter. Mass of a body is not
affected by temperature, location, or any other factor. Weight,
Classify physical or chemical changes.
however, change with location. The law of conservation of mass,, CHEM.A.1.1.1 (3.1.12 B.2) (3.1.10 E.1)
states that for any system closed to all transfers of matter and
between homogenous
energy (both of which have mass), cannot be created of destroyed, Differentiate
and heterogeneous and how mixtures
only transferred.
can be separated. CHEM.A.1.2.2.
(3.4.10 A.8)
Histograms
The purpose of a histogram is used to graphically summarize
and display information with a data set. The vertical axis of
the histograms is labeled the frequency or number of points,
Describe ways that quantify the
properties of matter (e.g., density,
solubility coefficients) CHEM.A.1.2.4
(3.4.12 A.8)
Describe the effects of error in
measurement. (3.1.10 E.3)
times. The horizontal is the response. The purpose is to tell
the most common response, distribution, accuracy of data.
Mass Activity
Objective: Prove the law of conservation of matter states that
matter cannot be created or destroyed ONLY transferred.
Ice cube melting in water
Online Textbook http://www.ck12.org/user%3AY3NoYXBpcm9AYmVuc2FsZW1zZC5vcmc./book/Honors-Chemistry-BHS/
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Properties of Matter
Matter is anything that has mass and takes up space. It includes all the physical “stuff” around
us—rocks, houses, water, air, people, ants, trees, etc. All matter can exist as a solid, a liquid, or a
gas. Matter includes all the things we can weigh (to find the mass) and measure to find the volume
(because they take up space). The properties of matter can be divided into two categories:
physical properties and chemical properties.
Physical properties of matter refer to characteristics of a substance that can be observed
WITHOUT changing the actual “makeup” of a substance. An example is odor. When you smell
water or isopropyl alcohol, neither of these substances changes into something else.
Chemical properties of a substance allow it to change into another kind of substance. The
flammability of isopropyl alcohol is an example of a chemical property. When alcohol is burned, the
alcohol actually turns into something else. s are observable characteristics of a substance that can
be used to CHANGE the makeup of the substance.
Sample Problem Is it a chemical or physical property?
A. Aluminum foil can be crumpled into a ball.
B. Aluminum can be corroded by oxygen to form aluminum oxide.
C. Aluminum can be "destroyed" by hydrochloric acid (HCl), forming aluminum chloride and hydrogen gas.
D. waters boiling point of 100°C
E. Argon is a colorless liquid at room temperature
F. separates into oxygen and hydrogen gases due to electricity
G. is able to erode rocks over time
Physical and Chemical Changes
Physical changes are those changes that do not result in the production of a new substance. If
you melt a block of ice, you still have H2O at the end of the change. If you break a bottle, you still
have glass. Painting a piece of wood will not make it stop being wood. Some common examples
of physical changes are; melting, freezing, condensing, breaking, crushing, cutting, and
bending. REVERSIBLE
A chemical change is also called a chemical reaction. A chemical reaction is a process that
occurs when one or more substances are changed into one or more new substances. When
you burn a log in a fireplace, you are carrying out a chemical reaction that releases
carbon. Common examples of chemical changes are; digestion, respiration. IRREVERSIBLE
Physical and Chemical Changes Practice
a. frying an egg
___________________b. melting snow
___________________
c. toasting bread
___________________d. souring of milk
___________________
e. brewing Tea
___________________f. growing a plant
___________________
g. melting Nickel
___________________h. magnetizing Iron
___________________
i. getting a suntan
___________________j. putting on Makeup
___________________
k. tarnishing silver
3
___________________ l. melting cheese
3
___________________
Classification of Matter
http://www.chem.purdue.edu/gchelp/atoms/elements.html (Notes)
There are three kinds of matter – elements, compounds and mixtures. An element is something
that you can find on the periodic table. It cannot be broken down into other substances.
Whereas a compound is a substance that is made up of two or more element that are
chemically combined. A mixture, on the other hand, is a substance that isn’t chemically
combined and can made in a of the three ways
Elements


consists of only _______ kind of atom,
__________ be broken down into a simpler type of matter by either physical/chemical means
Compounds




consists of atoms of two or more different elements ________________,
can be broken down into a __________ type of matter (elements) by chemical means only.
has properties that are ___________ from its component elements, and
always contains the __________ ratio of its component atoms.
Mixtures




consists of _______________ different elements and/or compounds physically intermingled,
can be _____________ into its components by physical means, and
often ____________ many of the properties of its components
Can be either heterogeneous or homogeneous.
Matter Classification Homework
Classify as Element. Compound, or mixture
a. Orange Juice__________________
b. Milk __________________
c. salt
d. Pepsi__________________
__________________
e. Butter Finger__________________
f. Hershey Kiss____________
g. Ranch dressing________________
h. Aluminum Foil ___________
i. Fruity Pebbles_________________
j. chalk __________________
k. Iron Nail
l. water __________________
__________________
Chemistry Workbook
Spring 2016
2.6 Homogenous Mixture
http://www.ducksters.com/science/chemistry/chemical_mixtures.php
Homogeneous mixtures - Any material that contains only one phase would be considered
homogeneous. Substances like sugar, and solutions like salt water, are all considered
homogeneous because they are uniform.
2.7 Heterogenous Mixture
(Notes)
Heterogeneous mixtures - Heterogeneous mixtures are made up of more than one phase and
they can be separated physically. The chocolate chip cookie, and tossed salad are examples of
heterogeneous mixtures.
Heterogeneous or Homogeneous Practice – draw a picture of the mixtures below
a. ice cream
b. coffee
c. salad dressing
Heterogenous
d. soda
e. cake icing
f. motor oil
g. saltwater
Homeogenous
(Notes)
2.4 Solid, Liquid and Gas
http://www.ck12.org/user:Y3NoYXBpcm9AYmVuc2FsZW1zZC5vcmc./book/Honors-Chemistry-BHS/section/2.4/
Matter typically exists in one of three states: solid , liquid , or gas . The state a given
substance exhibits is also a physical property. Some substances exist as gases at
room temperature (oxygen and carbon dioxide), while others, like water
and mercury metal, exist as liquids. Most metals exist as solids at room temperature. All
substances can exist in any of these three states.
Liquids have the following characteristics:
Gases have the following characteristics:
Solids are defined by the following characteristics:
Solids Liquids and Gases Practice
Determine whether the molecules below are a solid, liquid, or gas. Then decide whether they
are an element, compound or a mixture.
Solid
________
_______
_______
________
________
_______
Liquid
Gas_________________________________________________________________________________________________
Element
Compound
Mixture
________
_______
_______
________
________
_______
Phase Changes
(Notes)
Eureka 18 https://www.youtube.com/watch?v=eWQuE0X-sTI
Liquid
Gas
Ice
All matter can move from one state. Melting point to measure the temperature at which a
sold turns into a liquid. Whereas, freezing point is when a liquid turns into a
sold. The boiling point is when a liquid turns into a gas. Some of you may
have also seen a solid become a gas. It's a process called sublimation.
While condensation is when a gas turns into a liquid.
CHEMISTRY TERM
Melting
Freezing
Boiling/Vaporization
Condensation
Sublimation
PHASE CHANGE
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Heating Curve Activity
Objective: Observe changes in the state of matter by preparing a heating curve.
Identify the
melting and boiling point of water. When a solid is heated, the temperature of the solid increases,
indicating an increase in the kinetic energy of the particles. The temperature will continue to rise until
the melting point is reached. Likewise when a liquid reaches the point where it turns into a gas, the
kinetic energy increases until the boiling point is reached.
Procedure of the investigation:
1.
Retrieve an iced test-tube from Shapiro and measure the temperature every minute until it reads 0C for 3
consecutive minutes. Start time ____________
Fill a 125 mL Erlenmeyer flask with 125 mL of water.
Place the test-tube in the water bath and continue reading the temperature every minute until you have
reached boiling for 3 consecutive times.
2.
3.
Data:
Time
0 min
1 min
2 min
3 min
4 min
5 min
6 min
7 min
8 min
9 min
10 min
11 min
12 min
13 min
14 min
15 min
Temperature
Phase
Time
16 min
17 min
18 min
19 min
20 min
21 min
22 min
23 min
24 min
25 min
26 min
27 min
28 min
29 min
30 min
31 min
Temperature
Phase
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Discussion Questions:
1.
2.
3.
4.
Label A, B, C, D E Melting Point (Blue) and Boiling Point (Red).
Label A, B, C, D E Solid, Liquid, Gas
Where is water gaining energy? __________ Color Red
Where is water neither gaining nor losing energy? _________ Color Yellow
5. A sample of water in a pan is brought to a boil. Does the temperature of the boiling water
gradually increases?_____________________________
6. A sample of water is brought to a boil. What are the bubbles inside ___________
7. When gaseous water condenses to liquid water, does the water absorbs energy from the
surroundings or does the water releases energy to the surroundings
8. Where would the distance between the water molecules increase?__________________
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2.8 Particle Diagrams
(Notes)
https://dashboard.dublinschools.net/lessons/?id=7572c239bdb545af210f38a7e8eee87a&v=2
Chemistry Workbook
Everything around you is made of particles so tiny that we cannot see them even with the most
powerful microscope. These particles are arranged and move differently in each state of matter.
Take water as an example; the size, shape and chemical composition of the water particles
remains the same whether it is solid water (ice) or gaseous water (steam) - but how those particles
move and are arranged is different for each state.
Sample Problem
The circle on the left shows a magnified view of a very small portion of liquid water in a closed container.
What would the magnified view show after the water evaporates? Classify as physical or chemical change
and Mixture, compound or element?
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Particle Diagram Practice
Which number belongs to the corresponding description?
Elementary substance = E
Compound = C
Homogeneous mixture = HOMO
Heterogeneous mixture = HETERO
______________
_____________
____________ ___________
_____________ _____________
______________
_____________
____________ ___________
_____________ _____________
2.9 Elements to know
Column 1
Aluminum
Antimony
Argon
Arsenic
Barium
Beryllium
Bismuth
Boron
Bromine
Calcium
Carbon
Cesium
Chlorine
Chromium
Cobalt
Copper
Fluorine
Francium
Gallium
Column 2
Al
Sb
Ar
As
Ba
Be
Bi
B
Br
Ca
C
Cs
Cl
Cr
Co
Cu
F
Fr
Ga
Germanium
Gold
Helium
Hydrogen
Iodine
Iron
Krypton
Lead
Lithium
Magnesium
Manganese
Mercury
Neon
Nickel
Nitrogen
Oxygen
Phosphorus
Platinum
Plutonium
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Column 3
Ge
Au
He
H
I
Fe
Kr
Pb
Li
Mg
Mn
Hg
Ne
Ni
N
O
P
Pt
Pu
Potassium
Radium
Radon
Rhodium
Scandium
Selenium
Silicon
Silver
Sodium
Strontium
Sulfur
Tin
Titanium
Tungsten
Uranium
Xenon
Vanadium
Zinc
Zirconium
K
Ra
Rn
Rh
Sc
Se
Si
Ag
Na
Sr
S
Sn
Ti
W
U
Xe
V
Zn
Zr
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2.15 Separation of Mixtures
(Notes) http://www.bensalemsd.org/Page/6652
1. Distillation
 Distillation is a technique used to separate two liquids with
________________________
 When the first liquid starts to boil, it _________________ and reaches the condenser
 Water _________________ on the outside and return to the liquid state and be
collected at the other end
2. Evaporation
 Evaporation can be used to separate a ____________
from a ____________ in a homogeneous solution
 The solution is heated until all of the liquid evaporates
and only the ______________ is left behind
3. Crystallization is the process through solute crystallizes
forming a precipitate after all of the water has evaporated.
 First __________________ is used.
 The solution is heated until all of the liquid evaporates
and only the solid is left behind
The solute substance then _______________.
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4. Filtration
 A filter is a ______________ or layer than allows some
substances to pass through while blocking others
 You use to __________________ mixtures; separate
______________ solids from liquids
 Same as using a coffee filter
5. Decanting – Decanting means you are pouring off a liquid
without disturbing the sediment or other
liquid layers.
 Using the __________, you separate
two substances.
 Pour off the __________ __________ substance first.
6. Magnetism Two substances can be separated by their
magnetic properties if one substance is magnetic and the other is not
 The magnet will then __________ one substance but not the other
 iron, nickel, cobalt, chromium, manganese are
magnet elements
7. Manually
 Pick the _____________
pieces out by hand.
 It involves _____________
separating each of the
component elements of a Mixture..
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How Much Iron Is In Your Cereal Activity
Purpose:
Each box of cereal indicates the percentage of FDA recommended vitamins and minerals. FDA states
that everyone should have 18 mg of iron. If a box states that each serving contains 100% of FDA
recommended values than it contains 18 mg. Since mixtures conserve there physical properties, can
you find out how much iron is in your cereal by using the elements physical and c
Depending on the cereal, most of them are a heterogeneous mixture; therefore, the separate
components conserve their physical properties. As a result, iron can be separated out of the
mixture due to the uneven distribution of the cereal. Add enough warm water to fill the beaker
containing the cereal to the 750-mL mark. Drop in a large magnetic stir bar and place the beaker on
the magnetic stirrer for a few minutes. Remove the bar and observe the amount of iron on the stir
bar.
View under stereoscope
Particle Diagram
Discussion Questions
1. We use these properties to separate these components?
2. Is cereal a homogeneous or heterogeneous mixture?
3. What is the law of conservation of matter and how does it apply to this activity?
4. Did the cereal undergo a chemical or a physical change?
5. Why is iron an essential part of our diet?
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Making and Separating your Solution
Instructions: You will weigh out 5 grams samples: copper salt and wax. Combine them with 30 mL of
water to obtain your mixture. You must write a procedure detailing how you plan to separate the three
substances. These samples will be combined and it will be your job to use your knowledge of separation
techniques to separate each substance from the others. At the end, you will find the mass of your final
samples and calculate the percent difference between your initial and final mass.
Write your procedure below of this paper and give it to me.
Procedure:
Separation of wax
1.
2.
3.
4.
Results 5 grams before
?
grams after
?
grams after
% error OV – TV x 100 =
TV
Separation of Copper salt
1.
2.
3.
4.
Results 5 grams before
% error OV – TV x 100 =
TV
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HOW TO WRITE AN ABSTRACT 20 Points
Please Edit Find 12 errors below
Introduction statement (reel the readers in with how the overall theme/hypothesis applies to life)
The objective of the lab is …………
My hypothesis for this lab is ………….because………………
I accomplished this by….(explain you procedure BRIEFLY)
Our data showed, based on graphs, (validate hypothesis, explain graphs, slope)
In conclusion, ……(summarize the objective and hypothesis)
Real life statement (connect the introduction statement to the last statement)
Solutions Abstract
Elements, compounds and mixtures are everywhere. What defines a mixture is its ability to be
separated by chemical means. The objective of the experiment was to prepare and separate a
homogenous solution of wax, salt and iron. My hypothesis is that since this solution is a compound, it
can be separated. I accomplished this by making a homogeneous compound of 5.0 grams of wax, 5.0
grams of copper salt and pinch of iron. In order to separate, the iron was first removed using
filtration. Next, the wax was chemically picked out or it can be separated from the mixture through
magnetism. In order to filter the wax from the mixture, salt must first be insoluble in water. Since
filter paper only allows solutes though, the saltwater solution will pass through and the wax will stay
behind. Finally, the salt can be separated from water through filtration. During evaporation, the
solute evaporates leaving solid particles behind to decant. Our data showed that we recovered 4.8
grams of wax and 5.3 grams of salt. Since matter be created or destroyed, our data showed
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