s8p1a. matter describe matter and what is it composed of? page 11 matter is anything that has mass...

S8P1a. Matter

Describe matter and what is it composed of?

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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

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.

On page 12

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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.

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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

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

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.

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

Ions 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.

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.

On page 72Draw the electron arrangement of the following. Lithium Chlorine Sodium Sulfur

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.

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

Common 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

Common 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

Draw 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

Draw 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

Create 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

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?

Create 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

PHYSICAL 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

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 92

The freezing point and melting point are the same temperature.

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

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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

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

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?

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.