matter think – pair - share
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THINK. SHARE. What is matter?. What do you think?. What do you think?. Matter Think – Pair - Share. PAIR. Individually, think of what you know about “matter”. This was part of your 6 th grade science class. Write down what comes to mind when you think of “matter”. 5 - 7 minutes - PowerPoint PPT PresentationTRANSCRIPT
Matter Think – Pair - Share
Individually, think of what you know about “matter”. This was part of your 6th grade science class. Write down what comes to mind when you think of “matter”. 5 - 7 minutes
Now pair up with a partner (or team) and share your thoughts and ideas. One person serve are the recorder and put these on the construction paper.5 – 7 minutes
Each team will then share their information with the class. Tape the construction paper up for other students to see.
What is matter?
THINK
PAIR
SHARE
What do you think?
What do you think?
Matter: Properties and Change
Matter, is a substance that has mass and also volume. The volume is determined by the space it occupies, while the mass is defined as a measure of how much matter is in an object.
http://micro.magnet.fsu.edu/primer/java/scienceopticsu/powersof10/ size comparisons from milky way galaxy to quarks
http://www.youtube.com/watch?v=FSyAehMdpyI “The Nucleus: Crash Course Introduction To Chemistry” #1” 10:12
What is matter? Explain your reasoning.http://commons.wikimedia.org
Sunlight Water Electricity
Heat Smoke Earth’s Atmosphere
Early alchemists thought that everything was made of either earth, air, water or fire.
Why can you never trust an atom?
“The Elements” VHS 50:52http://youtu.be/zUDDiWtFtEM “The New Periodic Table Song 2:29
http://www.ncpublicschools.org/docs/accountability/testing/releasedforms/2009grade8periodic.pdf DPI periodic table
Element Information
An atom will have the same number of electrons as protons.
Chemistry Spoons Game
The first letter is always capitalized. In symbols with two or more letters, only the first letter is capitalized.
73
Atoms: most basic unit of matter; atoms make up everything
- An atom containing an equal number of protons (+) and electrons (-) is electrically neutral, otherwise it is positively or negatively charged and is known as an ion.
An atom is classified according to the number of protons (atomic #): - the number of protons (atomic #)
determines the chemical element,- and the number of neutrons
determines the isotope of the element. ( i.e. carbon 12 and 14)
Protons = positively chargedNeutrons = neutral (no) chargeElectrons = negatively charged
What particles are in the nucleus?
Lithium atom (atomic #3 = protons)
Atomic Mass = 7 (protons and neutrons)
Coach Lesson #1
How do sizes of atomic particles differ?
- Electrons are extremely small compared to all of the other parts of the atom.
- The mass of an electron is almost 1,000 times smaller than the mass of a proton.
(Quarks make up protons and neutrons.)
How is the size of atomic particles measured?
The nanometer is often used to express dimensions on an atomic scale:
- The diameter of a helium atom, for example, is about 0.1 nm, and that of a ribosome is about 20 nm.
2
(protons and neutrons)
Where are the protons and neutrons located?
Electron Orbitals/ Cloud/Energy Level/Shell Configurations
Valence electrons are those located in the outer most shell/level.
How many valence electrons are shown in this atom?
Atomic Structure of Helium1. How many protons(+) are in helium?2. How many neutrons (neutral) are in helium?3. How many electrons (-) are in helium?4. How many valence (outer level) electrons are
shown?
Name That Element
N
Lithium
- Protons = 3 (atomic number)
- Neutrons = 4
- Mass Number/Weight = 7 (protons and neutrons)
- Electrons = 3
* The number of protons (+) and
electrons (-) will be the same.
1. What period is lithium in?2. What group/family is lithium in?3. How many valence (outer) electrons does lithium have?
Lithium (Li): One neutron is not shown.
N
Elements above 92 are synthetic meaning they are “manmade” and not found in nature.
Name That Element
Atomic Structure of Carbon
1. How many protons (+) are shown?2. What is the atomic mass?3. How many neutrons (neutral) are shown?4. How many electrons (-) are shown?5. How many valence (outer level) electrons are shown?
Some sources have astatine as a metalloid while others do not.
Classifications of elements
Name That ElementAtom Diagram Practice
Atomic Structure of Boron
1. How many protons (+) are shown?2. How many neutrons (neutral) are shown?3. How many electrons (-) are shown?4. How many valence (outer level) electrons are shown?
A. What is the atomic number of boron?B. What is the mass number of boron?C. What family is boron in?D. What group is boron in?
“Build That Atom” Activityhttp://phet.colorado.edu/en/simulation/build-an-atom build an atom activity
“The Elements” VHS 50:52
Valence ElectronsThe valence is the number of outer shell/orbital electrons. These are the electrons available to take part in chemical reactions. The periodic trend for valence works well for the representative elements, which are in groups 1, 2, 13, 14, 15, 16, 17, and 18 (the ‘tall’ parts of the table). Reading left to right, the valence for each of the main groups increases from one to 8. The noble gas elements, with 8 valence electrons, are especially stable.
Helium only has 2 valence electrons. Why is it in group 18?
Why are the noble gasses the “happiest” elements?
Valence electrons can be determined by looking at the group/family.Group 1 = 1 valence (outer) electron Group 2 = 2 valence (outer) electrons Group 13 = 3 valence (outer) electrons, etc. (transition elements 3-12 will vary)
Valence electrons are what determine the bonding ability of an atom.
Periodic Table Color Coding Activity
Elements of the same period have the same number of electron orbitals/shells.
A group/family on the periodic table means the elements have similar chemical properties.
Essential mineral elements : (elements required by living organisms, other than the four elements carbon, hydrogen, nitrogen, and oxygen present in common organic molecules) nitrogen, phosphorus, potassium, calcium, magnesium, sulfur, boron, chlorine, iron, manganese, zinc, copper, molybdenum, and nickel.
Beneficial elements: elements which promote plant growth in many plant species but are not absolutely necessary for completion of the plant life cycle : Silicon, sodium, cobalt, and selenium
Essential nonmineral elements; (elements taken up as gas or water): hydrogen, oxygen, and carbon
Metals, Nonmetals and Metalloids
along zigzag line
Some sources show astatine as a metalloid while other do not.
Classifications of ElementsWhy is hydrogen not connected to group 1?
84Po
Polonium209
34Se
Selenium77
http://www.chemtopics.com/elements.htm interactive periodic table
Some periodic tables include astatine as a metalloid. Based on the site http://www.chemicalelements.com/groups/metalloids.html astatine is not a metalloid.
Classifications of elements
Metalloids
Metalloids are a chemical element with properties that are in-between or a mixture of those of metals and nonmetals. The seven elements commonly recognized as metalloids are boron, silicon, germanium, arsenic, antimony, polonium and tellurium. They or their compounds find uses in glasses, alloys or semiconductors. These are located along the zigzag line.
84Po
85jAt
Metalloids: located along the zigzag lineThe seven elements commonly recognized as metalloids are boron, silicon, germanium, arsenic, antimony, polonium and tellurium.
Group/Family 1 - 18
Period
http://www.chem4kids.com/extras/quiz_elemintro/q02_no.html on-line quiz use periodic table
Metals
Notice that the metalloids and nonmetals are not included. Compare this section of the periodic table to the complete periodic table of elements.
Metalloids & Nonmetals
Metalloids Nonmetals
Some sources show astatine as a metalloid while other do not.
Physical Properties: can be observed and measured without changing the kind of matter being studied; can be used to identify substances
Melting Point:- The temperature at which a solid can change to a liquid.- The temperature at which a pure substance melts is
unchanging under constant conditions.Boiling Point:
- The temperature at which a liquid boils.- A substance changes from a liquid to a gas.- Boiling temperature is unchanging under constant
conditions for a given substance.Density:
- a property that describes the relationship between the mass of a material and its volume
- Substances that have higher densities contain more matter in a given volume.
- The density of a substance will stay constant/the same.Color: may be used to identify substances but not always
Assessment Probe: “Floating Logs”Demo: Density BlocksExample: Man from Zambia
Physical Properties of Metals and NonmetalsSTC: “Finding the Conductor” 1.1
Physical Properties of Noble Gasses (Group/Family #18)
How are properties used to identify substances?
H
How are properties used to determine how elements and substances are used?
1. Why is aluminum used in airplanes?2. Why is helium used in balloons instead of oxygen or hydrogen?
Chemical Property: any of a material's properties that becomes evident during a chemical reaction; that is, any quality that can be established only by changing a substance's chemical identity
1. Can be used to help identify a substance
2. Usually involves the substance’s ability to react or not react with another specific substance
Examples
Reacting with Oxygen (oxidation): The ability of a substance to burn is a chemical property that involves a substance reacting quickly with oxygen to produce light and heat. (i.e. iron rusts or apples turn brown).
Reacting with Acids: The ability of a substance to react with an acid is a chemical property. Some metals react with various acids to form compounds. All metals do not react with all acids. Bases react with acids to form water and neutralize the acid.
Example: Man from Zambia
Reactivity: the tendency of a substance to undergo chemical reaction, either by itself or with other materials.; reactivity is a chemical property of an element
http://www.youtube.com/watch?v=Jy1DC6Euqj4 potassium reaction in water 20 sec.
http://www.youtube.com/watch?v=MTcgo46nxNE sodium reaction in water 48 sec.
These soft, silvery sodium chunks were cut with a knife and stored under oil. In air they turn white in seconds; exposed to water they generate hydrogen gas and explode in Flaming balls of molten sodium.
http://www.youtube.com/watch?v=1bJBueGSC9Mcalcium reactivity with oxygen 27 sec.
Physical & Chemical PropertiesSubstance Physical Property Chemical Property
Helium Less dense than air Nonflammable
Wood Grainy texture Flammable/combustible
Baking Soda White powder Reacts with vinegar to form bubbles
Powdered Sugar White powder Does not react with vinegar
Rubbing Alcohol Clear liquid Flammable/Combustible
Red Food Coloring Red color Reacts with bleach and loses color
Iron Malleable Reacts with oxygen (oxidation) to form iron oxide (rust)
Tin Malleable Reacts with oxygen to form tin dioxide
Physical or Chemical Property… What do you think?
1. Shape2. Density3. Acidity (below 7 pH)4. Solubility5. Basicity (above 7 pH)6. Combustibility7. Odor8. Melting point9. Reactivity10. Boiling point11. Color
Points to Consider
If the property changes, is a new substance formed? If not, it is a physical property.
If you still have the same substance after changing the property, it is a physical property.
Chemical vs Physical Changes (laptop review)
Chemical Change: - properties change and a different substance is
produced. - Chemical changes cannot be
reversed. - Examples: iron reacts with oxygen and water to
form iron oxide (rust);
silver reacts with oxygen to form silver oxide (tarnish)
Evidence of a chemical change:
1. Change in energy: temperature increase = exothermic chemical reaction
temperature decrease = endothermic chemical reaction
2. Color change: This is not when a color has been covered, for example dying, painting,
etc. 3. Formation of a gas: if in a solution, bubbles will
often times been seen when the gas is
formed
4. Formation of a precipitate: when two or more solutions are combined and a solid is
formed
STC: “The Burning Candle” 1.3 “Mixing the Solutions” 1.8 “Adding the Acid” 1.5
Physical Changes
Physical Change:
- The physical properties change but the type of substance stays the same.
- matter changes is size, shape or form
- There is no change in the chemical makeup of the substance(s) that are changed.
- Physical changes can be reversed.
- Examples: cutting, changes in states of matter (melting, boiling, freezing), etc.
http://glencoe.mcgraw-hill.com/sites/dl/free/0078617650/160350/00044680.html Brain Pop Chemical and Physical Changes program w/quiz
Phase Change
(dissolving a substance)
(mixing two or more substances)
Sublimation: when a substance changes directly from a gas to a solidExamples:- The forming of frost from water vapor
- When dry ice forms: Dry ice is frozen carbon dioxide. As it breaks down, it turns directly into carbon
dioxide gas rather than a liquid http://www.youtube.com/watch?v=8tHOVVgGkpk dry ice bubbles 2:20; also shows properties of polar molecules water and detergent (surface tension)
- Solid air freshenersApples brown (react with oxygen)
1. Is a phase change a physical or chemical change? Explain.2. What is the relationship between phase change and temperature?3. What effect does phase change have on the volume of the
substance/molecules? Density? Mass? Explain.
http://www.youtube.com/watch?v=czmQ2_ymaOo formation of ice crystals 37 sec.
Mini-Poster Analysis
Chemical Changes Require Chemical Reactions
Chemical Reaction: when a substance (or a few substances) change into another substance.
A chemical change involves a physical change, and can include but is not limited to the following:Examples: change in color, texture, physical state, odor, production of a gas, formation of precipitate, a change in its solubility, burning, rusting, etc. Chemical changes do not change the mass, because according to the Law of Conservation of Mass/Matter, during a chemical reaction the mass of the reactants of the formula will always equal the mass of the products
STC: “Reacting A Tablet” 1.7
Endothermic Reactions = temperature decrease; Exothermic Reactions = Temperature increase
MRE Lab
Chemical Reactions = Chemical Changes = New Substance(s) Formed
Chemical reactions are shown in the form of chemical equations.
Word equation: Sodium + Chlorine yields sodium chloride Chemical equation: 2Na(s) + Cl2 (g) 2NaCl(s)
reactants products
1. What is the mass of the reactants?2. What is the mass of the
products?3. Does this reaction meet the “Law
of Conservation of Mass/Matter”? Explain.
Law of Conservation of Mass/Matter: “Nuts & Bolts of Law of Conservation of Mass”- In a chemical equation, matter cannot be created or destroyed- The mass of the reactants will equal the mass of the products.
Coefficient = # of molecules in the compound
Subscript = # of atoms of the element
“Balancing Chemical Equations” practiceSTC: “Mixing the Solutions” 1.8
Balanced Chemical Equations
subscript
Hydrogen = 4Oxygen = 2
Hydrogen = 4Oxygen = 2
The coefficient shows how many total molecules are present. Multiply this by the subscript.
No subscript indicates that 1 atom is present.
Does this equation meet the “Law of Conservation of Mass/Matter”? Explain.http://www.youtube.com/watch?v=PlwuxpMh8nk “Simple Chemical Reactions” with Bill Nye 23:01
http://www.sciencespot.net/Media/blncact.pdf “Balancing Act”
Balance the following chemical equations.
Reactants Products
1. Na + Cl2 NaCl
2. H2 + Cl2 HCl
3. CO2 + H2 CO + H2O
4. NO + O2 NO2
5. Fe + 3O2 Fe2O3 Note: You may only add coefficients when balancing equations, not subscripts. One of the equations is balanced.
Check your equations.
Reactants Products
1. 2Na + Cl2 2NaCl
2. H2 + Cl2 2HCl
3. CO2 + H2 CO + H2O
4. 2NO + O2 2NO2
5. 4Fe + 3O2 2Fe2O3
Balanced chemical equations support the law of conservation of mass/matter. Explain why.The chemical reaction for photosynthesis
Reactants yield Products
Reactants6 carbon24 oxygen24 hydrogen
Products6 carbon24 oxygen24 hydrogen
Chemical Equation for Cellular Respiration
Reactants yield Products
Reactants6 carbon24 oxygen24 hydrogen
Products6 carbon24 oxygen24 hydrogen
Compounds and Mixtures
HeterogeneousElements combine to form compounds.
Cannot be changed into a simpler substance
Pure substances composed of two or more types of elements that are chemically combined
STC: “Our Ideas About Pure Substances and Mixtures”
What is the difference between a compound and a molecule?
1. A molecule is formed when two or more atoms join together chemically.
2. A compound is a molecule that contains at least two different elements.
- All compounds are molecules but not all molecules are compounds.
Example:
- Molecular hydrogen (H2), molecular oxygen (O2) and molecular nitrogen (N2) are not compounds because each is composed of a single element. They are diatomic molecules because in nature they do not exist as
individual atoms.
- Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds because each is made from more than one element.
- The smallest bit of each of these substances would be referred to as a molecule.
Compounds- A compound is a type of matter that forms when two or more different elements combine chemically. Two or more atoms bonded together is a molecule of the substance that is formed.
- When atoms combine chemically, they do not retain their original properties. How do the following compounds provide evidence of this?
In the compounds below, compare the properties of elements before and after chemical bonding has occurred.
Examples: Chemical formulas for common substances
H2O chemical formula for 1 water molecule
C12H22O11 sucrose NaHCO3 baking soda
NaCl table salt HC2H3O2 vinegar
O2 oxygen (diatomic element)
H2O water
NaClO household bleach NH3 ammonia
HCl hydrochloric acidCO2 carbon dioxide
NaCl sodium chloride (table salt)H2O2 hydrogen peroxide
Activity: Identification of Element & Compounds in Products “Analyzing Formulas” practice
Subscript: #of atoms present of the element to the left no # as with oxygen means there is 1 atom present
Water (H20)• Water is a compound formed
from two atoms of hydrogen and one atom of oxygen; H20
• In their form as elements, hydrogen and oxygen are gasses. They both are also highly flammable.
• When combined in this
2 to 1 ratio, they form a liquid that is not flammable.
_
+ +
_ and + indicates the charged area of the molecule
“Biological Molecules: “You Are What You Eat” complete study guidehttp://www.youtube.com/watch?v=H8WJ2KENlK0 (14:09)
Sodium Chloride: Table Salt (NaCl)Sodium Chloride (table salt) isa combination of 1 sodiumatom and 1 chlorine atom;NaCl.
• In their form as elements, sodium is a highly explosive solid that explodes in water and chlorine is a toxic gas.
http://www.youtube.com/watch?v=9bAhCHedVB4&safe=active
• When combined in a 1 to 1 ration, they form table salt which is a white solid that dissolves in water.
Sugar (C6H12O6) • What elements are in a molecule of sugar?
“A Compound Problem” Practice
What elements are in the compounds below and inwhat ratio? What are the properties of the elements?
Glucose and Fructose (sugar) Molecules
What elements are common is both of these compounds? How are they different?
Carbohydrate Compounds – the main source of energy for our bodies
What elements are in these molecules? What is a better source of carbohydrates, simple or complex carbohydrates?
What elements are in a molecule of protein?In nature, matter is continually recycled.
What elements are in the essential nutrient protein?
Lipids/Fats
What elements are in lipid molecules?
Common Name
Chemical Name Chemical Formula
white vinegar acetic acid CH3COOH + H2O
nail polish remover acetone CH3COCH3
ammonia ammonium hydroxide CH3 + H2O
boric acid boric acid H3BO3
marble,limestone,chalk calcium carbonate CaCO3
road salt calcium chloride CaCl2
garden lime calcium hydroxide Ca(OH)2
corn syrup glucose C6H12O6 + H2O
epsom salt magnesium sulfate MgSO4 + 7H2O
moth balls naphthalene C10H8
baking soda sodium bicarbonate NaHCO3
table salt sodium chloride NaCl
cane sugar sucrose C12H22O11
sulfuric acid sulfuric acid H2SO4
Common Chemicals
1. A molecule is what you get when any atoms join together.
2. A compound is what you get when atoms of two or more different elementsjoin together.
3. All compounds are molecules, but not all molecules are compounds.
- Water is a molecule because it is made from atoms that have been chemically combined. It is also a compound because the atoms that
make water are not all the same - some are oxygen and some are hydrogen.
- Oxygen in the atmosphere is a molecule because it is made from two atoms of oxygen. It is not a compound because it is made from atoms of
only one element - oxygen. This type of molecule is called a diatomic molecule, a molecule made from two atoms of the
same type.
Review: Molecules & Compounds
1. A molecule is what you get when any atoms join together.
2. A compound is what you get when atoms of two or more different elementsjoin together.
3. All compounds are molecules, but not all molecules are compounds.
- Water is a molecule because it is made from atoms that have been chemically combined. It is also a compound because the atoms that
make water are not all the same - some are oxygen and some are hydrogen.
- Oxygen in the atmosphere is a molecule because it is made from two atoms of oxygen. It is not a compound because it is made from atoms of
only one element - oxygen. This type of molecule is called a diatomic molecule, a molecule made from two atoms of the same type.
The Difference Between Compounds and Mixtures
Mixture - A physical blend of two or more substances that are NOT chemically combined. Compound - A substance that contains two or more elements CHEMICALLY combined in a fixed proportion. The elements do not retain their original properties. Compound is chemically combined, mixture is not chemically combined.
*Cake would be a compound because all of the ingredients are together to make batter you cannot see the individual components (eggs, flour, sugar, etc.) *Trail mix would be a mixture because you can see every individual item (M&M, peanuts, raisins, pizza, etc.)
“Introduction to Matter” Mini-poster examples
- tin + copper = pewter - copper + tin = bronze (more) (less) (more) (less)
- Steel is an alloy of iron, with carbon being the primary alloying element.- The air you breathe is made up of about 21% oxygen, 78% nitrogen, and small
amounts of other gases like argon, carbon dioxide and methane.
STC lab activities: “Comparing the Two Mixtures” 1.6 “Filtering a Mixture” 1.2 “Separating a Mixture” 1.4
Ways to separate mixtures:- Filtration (separates large particles from small) - Magnet- Evaporation (use boiling point) - Sifting- Centrifuge (use density)
Mixture
Homogenous or Heterogeneous Mixtures… Do you know?
#1 M & M #2 Salad #3 Kool Aid drink #4 Fruit Loops
#5 Milk #6 Cake Batter #7 Chocolate Chip Cookie
#9 Trail Mix #10 Tap Water #11 Smoke #12 Clear Seawater
#8 Hot Chocolate
