s8p1a. matter describe matter and what is it composed of? page 11 matter is anything that has mass...
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S8P1a. Matter
Describe matter and what is it composed of?
Page 11
Matter is anything that has mass and takes up space.Examples: book, toy, car, paperNon-examples: heat, light
Matter is made of tiny indivisible particles called atoms. They are the basic building blocks of all matter.
For many years, people have wondered what matter is made of including Democritus, Lavoisier, Dalton, Thompson, Rutherford and Bohr.
On page 10, create a t-chart and identify each of the following as an example of matter or not an example of matter.
Water, juice, plant, lightning, electricity, magnetism, force, heat,air, helium, oxygen, time, sound, clothes, sunlight, energy, inertia
Matter Not Matter
Page 13
The nucleus is the small dense, positively charged center of an atom. It contains the most of the atom’s mass. It contains protons and neutrons.
Protons are positively charged particles located inside the nucleus.
Neutrons are neutrally charged particles located inside the nucleus.
Electrons are negatively charged particles found in electron clouds outside the nucleus.
Page 61
There are two kinds of pure substances: elements and compounds.
An element is matter made up of only one kind of atom. There are over 100 known elements. About 90 of them are found naturally on Earth and the other 20+ are synthetic (man-made).
All known elements are arranged in a chart called the periodic table of elements. Each element on the chart has a chemical symbol with one to three letters.
The periodic table is arranged in rows called periods and columns called groups or families. There are 7 periods and 18 groups.Elements in the same group share similar properties.
Page 63
Each element has an atomic number and an atomic mass.
The atomic mass is the average of all of the isotopes of an element.
The atomic number is ALWAYS the number of protons. It is also the number of electrons in a neutral atom.
To determine the number of neutrons, you must subtract the atomic number from the atomic mass.
For example, Copper has an atomic number of 29 and an atomic mass of 63. It has 29 protons , 29 electrons and 34 neutrons.
On page 60Identify the group/family number of the following elements:1. Lithium 4. Beryllium2. Xenon 5. Hydrogen3. Gold
Identify the period number of the following elements:6. Arsenic 9. Xenon7. Palladium 10. Mercury8. Argon
Identify the group/family name of the following elements:11. Lithium 14. Beryllium12. Xenon 15. Aluminum13. Gold
On page 62, draw and complete the table below.
Describe how the periodic table is arranged/organized.
Element Name # of protons # of electrons # of neutrons
Aluminum
Barium
Neon
Tin
Platinum
Titanium
Zirconium
Page 65
About 75% of all the elements are metals. They generally have a shiny or metallic luster and are good conductors of heat and electricity. All metals except mercury are solid at room temperature. Metals are located on the left side of the Periodic Table.
Nonmetals are elements that are usually dull in appearance. Most are gases and poor conductors of heat and electricity. Nonmetals are located on the right side of the Periodic Table.
Metalloids are elements that have characteristics of metals and nonmetals. They are found between the metals and the nonmetals along a zig-zag line.
On page 64, identify whether the following elements are metals, nonmetals or metalloids.Hydrogen, Helium, Lithium, Beryllium, Boron, Argon, Potassium, Mercury, Calcium, Oxygen, Sulfur, Zinc, Gold, Xenon, Neon
Metal Nonmetal Metalloid
Page 67
Each element has a unique # of protons which is the atomic number. Every single atom of that element must have the same number of protons.
Atoms of one element must have the same # of protons, but can have a different # of neutrons.
Isotopes are atoms with the same # of protons and a different number of neutrons. This gives an isotope a different atomic mass.
For example Hydrogen sometimes has an atomic number of 1, 2 or 3. This is because the number of neutrons may vary.
Page 69
When referring to an isotope, you state the element name followed by its atomic mass.
For example:Hydrogen-1 or Hydrogen-2 or Hydrogen-3
protons = 1 protons = 1 protons = 1 electrons = 1 electrons = 1 electrons = 1 neutrons = 0 neutrons = 1 neutrons = 2
Note: Mass numbers are decimals because some isotopes are more common than others. The one listed in the periodic table is the most common isotope.
1H
Hydrogen1.001
1H
Hydrogen2.001
1H
Hydrogen3.004
On page 66, determine the number of protons, electrons and neutrons for the following isotopes.
Carbon -12 Carbon-13 Carbon-14
Protons
Electrons
Neutrons
Chlorine 35 Chlorine 37
Protons
Electrons
Neutrons
Iron-54 Iron-56 Iron-57 Iron-58
Protons
Electrons
Neutrons
On page 66, determine the number of protons, electrons and neutrons for the following isotopes.
Carbon -12 Carbon-13 Carbon-14
Protons 6 6 6
Electrons 6 6 6
Neutrons 6 7 8
Chlorine 35 Chlorine 37
Protons 17 17
Electrons 17 17
Neutrons 18 20
Iron-54 Iron-56 Iron-57 Iron-58
Protons 26 26 26 26
Electrons 26 26 26 26
Neutrons 28 30 31 32
Page 71Ions are atoms that have a charge. They may be positively or negatively charged.
Ions that have a positive charge are called cations. They form when an atom loses electrons. Number of Electrons < Number of Protons
Ions that have a negative charge are called anions. They form when an atom gains electrons.Number of Electrons > Number of Protons
Only the electrons change. The protons and neutrons stay the same.
Ions with opposite charges attract therefore cations and anions attract each other. Moving ions conduct electricity
On page 70, determine the number of protons, electrons and neutrons for the following. Remember: Only the electrons change. The protons and neutrons stay the same.
P P -3
Protons
Electrons
Neutrons
Ca Ca +2
Protons
Electrons
Neutrons
K K +1
Protons
Electrons
Neutrons
Cl Cl -1
Protons
Electrons
Neutrons
Mg Mg +2
Protons
Electrons
Neutrons
Sc Sc +3
Protons
Electrons
Neutrons
On page 70, determine the number of protons, electrons and neutrons for the following. Remember: Only the electrons change. The protons and neutrons stay the same.
P P -3
Protons 15 15
Electrons 15 18
Neutrons 16 16
Ca Ca +2
Protons 20 20
Electrons 20 18
Neutrons 20 20
K K +1
Protons 19 19
Electrons 19 18
Neutrons 20 20
Cl Cl -1
Protons 17 17
Electrons 17 18
Neutrons 18 18
Mg Mg +2
Protons 12 12
Electrons 12 10
Neutrons 12 12
Sc Sc +3
Protons 21 21
Electrons 21 18
Neutrons 24 24
Electron Levels
Page 15
Electrons surrounding an atom are located in regions around the nucleus call “energy levels”. They represent 3-D spaces surrounding the nucleus.
The first energy level is closest to the nucleus with each level moving a little farther away. Each energy level can accommodate or “hold” a different number of electrons before additional electrons go into the next level.
Page 15
1st Level = 2 electrons max.2nd Level = 8 electrons max.3rd Level = 8 electrons max.4th Level = 18 electrons max.5th Level = 18 electrons max.6th Level = 32 electrons max.7th Level = 32 electrons max.
The electrons in the farthest (outer) level are called valence electrons. Elements in the same group have the same number of valence electrons.
S8P1a., S8P1f., S8P1d
States of Matter 11/ /13
Compare and contrast the particle movement in the different states of matter?
Page 77
A state of matter is the physical form in which matter exists. There are four states (phases) of matter : solid, liquid, gas and plasma. Matter often changes state when heat is added or taken away.
A solid is a substance with a definite shape and a definite volume. The particles in a solid are packed closely together and maintain a rigid form without a container. They vibrate slowly against one another.
A liquid is a substance with a definite volume, but not a definite shape. The particles in a liquid move faster and freely past one another, but are still close to one another. Liquids take the shape of the container they are in.
Page 79
A gas is a substance that does not have a definite shape or a definite volume. Gas particles move very fast and bounce off of one another. Gases fill the container they are in.
Summary: Describe the particle movement in the states of matter.
On page 76Identify whether each of the following are solids, liquids or gases in the table below.
Milk toy car helium hydrogen water ice steam sugar salt pepsi oxygen
Solid Liquid Gas
On page 78Compare and contrast the characteristics and the particle position and movement in the 3 common states of matter
Solid Liquid Gas
Shape
Volume
Particle Position
Particle Movement
Miscellaneous
S8P1d. Properties of Matter 11/ /13
What are the various properties of matter and how can I distinguish between physical and chemical properties of matter? A property is a characteristic of matter.
A physical property is a characteristic that can be observed or measured without changing the identity of a substance. Examples: density (mass/volume), electrical conductivity, hardness, pH, state of matter and luster
A chemical property is a characteristic that describes how a substance will interact with other substances during a chemical reaction. Examples: reactivity, the ability to burn and rustSummary: What are the various properties of matter and how can I
distinguish between physical and chemical properties of matter?
Page 83
Page 85Common Physical PropertiesDensity is the amount of mass in a given volume.Density = mass or D=m volume VThe density of water is 1.0 g/cm3
pH is a measure of how acidic or basic a solution is ranging in a scale from 0 to 14. The values are the concentration of hydrogen ions in a solution. neutral acidic (acid) 7 basic (base) 0 14Most acidic Most basicHigh concentration Low concentrationof hydrogen ions of hydrogen ions
Page 87Common Chemical PropertiesTarnishing – the reaction between sulfur in the air and metals.
Rusting – the reaction between oxygen and metals.
Combustibility – the reaction between oxygen and fuel that results in fire.
Flammability – the ability to burn
Reactivity – the ease and speed with which an element combines, or reacts (bonds), with other elements and compounds
Page 82Draw the pH scale and illustrate each item on it in its appropriate place on the scale and classify each of the following materials as an acid or base.
pH Acid or Base
Baking soda 8.5
Lemon 2
Ammonia 11.5
Milk 6.5
Soap 10
Drain cleaner 14
Water 7
Banana 5.2
Vinegar 2.8
Page 82Draw the pH scale and illustrate each item on it in its appropriate place on the scale and classify each of the following materials as an acid or base.
pH Acid or Base
Baking soda 8.5 base
Lemon 2 acid
Ammonia 11.5 base
Milk 6.5 acid
Soap 10 base
Drain cleaner 14 base
Water 7 neutral
Banana 5.2 acid
Vinegar 2.8 acid
Page 84Create a two-column table and classify each of the terms below as either a physical property or a chemical property.
reacts with base to form water Boiling pointdensity Taste reacts with an acid colorflammability melting point luster reacts to oxygensolubility hardness odor reacts with water to form gas
Physical Property Chemical Property
S8P1.d & S8P1.e Changes in Matter 11/ /13
What types of changes can matter undergo? What happens to matter when it undergoes changes?
Page 89
Matter can change. The types of changes matter undergoes are classified into two groups: physical changes and chemical changes.
A physical change alters the physical properties of a substance without changing the identity of the substance. Physical changes cause a change in properties such as volume, mass, or state of matter. Many physical changes can be reversed.Examples: melting, evaporating, freezing, cutting
A chemical change occurs when a substance is changed into a new substance with different properties. During a chemical change, the identity of a substance is changed. Examples: burning, rusting, baking, combusting
Page 91
A chemical reaction is the process by which new substances are formed during a chemical change. Some signs that indicate a chemical reaction has occurred include the forming of gases, a change in color, the release of heat, or the emission of light.
Another sign of a chemical reaction is the formation of a precipitate. A precipitate is a solid that forms from a chemical reaction that takes place in a solution.
It is very difficult or impossible to reverse the effects of a chemical change.
Summary: EQ - What types of changes can matter undergo? What happens to matter when it undergoes changes?
page 88Create a two-column table and classify each of the descriptions below as either a physical change or a chemical change.
Iron rusts sodium hydroxide dissolves in water milk goes soura match ignites and burns an ice cube melts to form a puddle of water icicles form at the edge of a roof chocolate bar melts in the sun water is heated and changed into steam vinegar and baking soda reactacid on limestone produces carbon dioxide gas wood and leaves rota tea kettle begins to whistle
Physical Change Chemical Change
Page 90PHYSICAL OR CHEMICAL CHANGE?
YESPHYSICAL CHANGE
NOCHEMICAL CHANGE
QUESTION: AFTER THE CHANGE IS IT THE SAME SUBSTANCE?
EVIDENCE OF A CHEMICAL CHANGE
BUBBLING
TURNS CLOUDY
TEMPERATURE CHANGES EXOTHERMIC – ENERGY IS EXITING - GETS HOTTER
ENDOTHERMIC – ENERGY IS ENTERING – GETS COOLER
COLOR CHANGE
CHANGE IN SMELL OR TASTE
Page 93
The transformation of matter from one state to another is called a phase transition. Phase transitions occur at precise points when the energy of motion in the atom is too much or too little for the atom to remain at that state.
Summary: EQ-Water can be found in solid, liquid and gas forms. How does that happen?
Phase Transition Description
Melting (add heat) Solid to Liquid
Evaporation (heat added) Liquid to Gas
Sublimation (heat added) Solid to Gas (skipping Liquid)
Condensation (heat removed) Gas to Liquid
Freezing (heat removed) Liquid to Solid
Deposition (heat removed) Gas to Solid (skipping Liquid)
EQ-Water can be found in solid, liquid and gas forms. How does that happen?
On page 92The following processes are phase transitions. Identify the type of transition.
Phase Transition
Water droplets coat your cold soda can on a hot day.
A cloud releases rain.
Solid dry ice steams in air.
Glaciers floating in the ocean are shrinking.
Morning dew disappears from the grass by midday.
A cloud releases snow.
Substances and MixturesDistinguish between pure substances and mixtures?
Page 17
All forms of matter can be classified into two groups: pure substances and mixtures.
A pure substance is one having a homogeneous composition. There are two types of pure substances: elements and compounds.
An element is matter that is made of only one kind of atom. An atom is the smallest unit of an element.
A compound is matter that is formed when two or more elements join (bond) chemically (a chemical reaction). They cannot be broken apart. A molecule is the smallest unit of a compound that has all the properties of the compound.
On page 16Identify whether each of the following are elements or compounds in the table below.
H H20 Ca Na NaCl CO2 CoFe2S OH CH4 NaOH CO SiO2
Element Compounds
Page
A molecule is the smallest unit of a compound that has all the properties of the compound. The makeup of a molecule is shown in a chemical formula. A chemical formula uses chemical symbols and subscripts to identify the number and types of atoms of each element that make up a compound.
A subscript is a small number written to the right and slightly below a chemical symbol to tell the number of atoms of that element is in the substance.
The chemical formula for water is H20.This means one molecule of water has 2 Hydrogen atoms and 1 Oxygen atom.
On page 96Determine the number of atoms of each element present in each of the following compounds.1. CO2. CO2
3. H2O2
4. NaCl5. NaOH6. C12H22O11
7. FeS2
8. Fe2O3
9. C2O10.Na2O11.CH4
Page 99
Elements can combine in different ways to form either compounds or mixtures. A mixture forms when two or more substances combine without joining chemically. They are not bonded together.
Because they are not bonded chemically, the parts of a mixture retain their own individual identities and properties and can be separated.
A mixture that is unevenly mixed is called a heterogeneous mixture. Ex. Trailmix. A mixture that is mixed evenly is called a homogeneous mixture. Ex. Kool-Aid
Summary: EQ- How can matter be classified?
On page 98Identify whether each of the following are heterogeneous or homogeneous mixtures in the table below.
Vegetable soup Chex Mix coffee cake batter chocolate chip cookie milk salt water pizza spaghetti & meatballs cereal in milk taco salad
Heterogeneous Mixture Homogeneous Mixture
S8P1g. Conservation of Matter
During a change in matter, how does the amount of matter compare before and after it changes?
Page 101
The law of conservation of matter states that, during a chemical reaction, matter cannot be created or destroyed.
Even though the matter may change from one form to another, the same number of atoms exist before and after the changes take place.
Reactant – the substances there before a reaction occurs.
Product – the substances there after the reaction takes place.
MASS OF REACTANT = MASS OF PRODUCT
UNDERSTANDING CHEMICAL REACTIONS &THE LAW OF CONSERVATION OF MATTER
2H2 + O2 2H20Reactants Products
A coefficient shows the number of molecules. 2H2 means 2 hydrogen molecules for a total of 4 hydrogen atoms.
A subscript shows how many atoms are in a formula. In O2, the 2 means 2 atoms of oxygen.
4K + O2 2K2025g + 5g 30g
If 25g of Potassium is reacted with 5g of Oxygen, how much Potassium Oxide is produced?
Page 103
Page 100 – Write the questions and answer each.How many different elements are present?N2 CaF2 CO2 NaSO3 CaCO3 SiO2
How many molecules are present?2H2O 5Be2Br 8CO2 3NaCl O2 MgS
How many total atoms are present?2H2O 2Be2Br 7CO2 6NaCl 4O2 2MgS
Using this reaction, answer the following questions.Li2O + MgCl2 2LiCl + MgOName the first reactant.Circle the second reactant.Underline the first product.Name the second product.How many Mg atoms are on the reactant side? the product side? How many Chlorine atoms are on the reactant side? the product side?
page 102 – Write each chemical reaction (and question) and determine the missing value?
2Mg + O2 2Mg023g + ?g 38g
2KCl + Li2O K2O + 2LiCl21g + 4g ?g + 12g
If 23g of Magnesium is reacted with Oxygen to produce 38 g of Magnesium Oxide, how much Oxygen was used in the reaction?
Using the numbers provided, determine how much K2O is produced in the reaction.