Standard: 7. PS1.6 Create and interpret models of substances whose atoms represent the states of matter with respect to temperature and pressure.

Day 1 Matter

Matter is the general word for what makes up things. The matter that makes up a balloon is not the exact same matter that makes up air in the balloon. Matter is makde up of smaller particles . These particles cannot be seen with your eyes. These tiny particle's are called atoms.

Matter is defined as something that has mass and takes up space. Mass is how much matter is in an object. Mass can be measured on a balance. Mass is different than weight. Weight is a measurement of gravity acting on the mass of an object. Since gravity is different for various planets your weight would be different on each one. Weight is measured with a scale.

Activity 1- At the top of your paper write the word Mass. Go to the following site and draw the balance. Measure the mass of five different items and write them down. link  

Volume of matter is how much space the object takes up. If the object is square you can use the formula length x width x height to determine the volume of that item. For things that are irregular, you can use water displacement. Ask your teacher to demonstrate this concept using a graduated cylinder. Have you ever jumped into the bath tub and noticed the water level go up? The amount that it goes up is equal to the volume of your body. 

Activity 1- Write the word volume on your paper. Draw a graduated cylinder. Practice reading a graduated cylinder at the following link. link 

Activity 2- Draw the chart below. Measure a marble, an eraser and a rock using a graduated cylinder. 

water object add the object     difference

25ml rock

25ml eraser

25ml marble

Density is another property of matter. Density is how tightly packed the particles are is the sample. For example, if you have a cotton ball and a brick, which one do you think is more dense? If you have ever thrown things into a pool you have seen density in action. If the item is less denser than water it will float. If it is denser than water it will sink. To determine the density you first measure the mass. Next you find the volume of that item. Now divide the mass by the volume. Mass divided by volume equals density. 

Activity- Draw the following chart on your paper. Complete your measurements.

                   Physical properties of a Penny

Property               Observations and measurements

Physical State

mass

volume

Magnetism

Conductor of electricity

density

Handout copy - Labs for property of matter link 

Matter is anything that takes up space. You are made of all kinds of different matter. Matter falls into four basic categories or states: solid, liquid, gas, and plasma. Solids, like an ice cube or your desk, have a definite shape and volume. Remember volume is how much space something takes up. The particles in a solid barely move. In a liquid, like milk or soda, the particles move a little faster. Liquids do not have a definite shape but they do have a a definite volume. For example, lets say you  pour 1/2 cup of milk into a round container and a 1/2 cup of milk into a square container. The liquid takes on the shape of the container. But the volume of milk stays the same. You still are using the same amount of liquid. The next type of matter is a gas. Helium and the air you breathe are kinds of gasses. They do not have a specific shape or a specific volume. Think of the propane tank on your barbecue. The gas inside have been pumped in but if you open the top the gas escapes. It will keep spreading out so you can't measure the volume. The particles are moving much faster than a liquid. The last example of matter that we are going to talk about is plasma. The atoms or particles are super heated and they begin to lose parts of the atom called electrons. As they fly off they create a type of light. Some examples of plasma are lightening, fire, the gas in a neon sign and the sun to name a few.  Matter can change from one state to another by adding energy in the form of heat. If you add heat an ice cube will change from a solid to a liquid. If you remove the energy of a gas by cooling it down it will turn into a liquid. Things to remember about matter:

• matter is made up of tiny particles

• the particles have space between them

• the particles are in constant motion

• the particles attract each other

• matter can change from one state to another by adding energy or taking it away

Activity 1: At the top of your paper write Physical States of Matter.

Make three columns and label them solid, liquid, gas. Draw an apple, a glass of water, and a helium filled balloon in the correct column. Below each one draw the particles for each state in a circle. Add the following choices to each one. You can use an answer more than once.

-has a definite shape

-has a definite volume

-shape depends on the container shape

- no definite shape

Activity 2:Answer the following questions from the reading:

 What are the four states of matter?

    Does a liquid have a definite shape?

    How do they change states?

    In which state do the particles begin to fall apart?

    In which state are the particles moving the slowest?

     Link to reading handout: docs.google.com/document/d/1Yw0RkreMUp1yLCZYFBG7_EI9u_6v8pbIhR7lp6VJgL8/edit?usp=sharing 

Activity 3: Make vocab cards from the reading above. Include a picture and a definition. 

Activity 4: group activity- link 

Activity 5: Brain Pop: States of Matter- Watch the video and take notes - draw the particles in each state 

Activity 6. Game www.brainpop.com/games/mattersorter/ 

Day 2  

Create a list of the physical properties below

Important physical properties of matter

• color

• mass

• density

• smell

• volume

• melting point

• boiling point

• solubility

• electrical conductor or insulator

• magnetic

• crystal shape

lab- add one drop of food coloring to 15 ml of cold water and one drop of warm water. What happens? explain your answer using your notes

Activity 1. Quizziz : Physical versus Chemical properties of matter

Examples of chemical properties:

• Flammability

• How easily a substance can ignite or sustain a combustion reaction. For example, butane gas is flammable when mixed with air.

• Toxicity

• The result of a chemical reaction or set of reactions that can cause harm. For example, skin damage from sodium hydroxide is a chemical property.

• Reactivity

• A substance's ability to interact chemically with another substance. This can happen when substances are mixed together or come into contact.

• Acidity

• Related to the hydrogen ion concentration of a solution. 

oxidation-It is defined as a process that occurs when atoms or groups of atoms lose electrons. Another way to define oxidation is when a chemical species gains oxygen or loses hydrogen. 

Changing states of matter  

Phase Transitions Between States of Matter

Temperature and pressure changes may cause phase transitions between states of matter.

Changes in temperature and pressure causes matter to change from one state to another. This change is called a phase transition or phase change. Examples of phase transitions including the melting of ice (a solid) into water (a liquid) and the boiling of water into water vapor (a gas). Here are the names of the phase transitions between solids, liquids, gases, and plasma:

• Melting: Phase transition from solid to liquid.

• Freezing: Phase transition from liquid to solid.

• Vaporization: Phase transition from liquid to gas.

• Condensation: Phase transition from gas to liquid.

• Sublimation: Phase transition from solid to gas.

• Deposition: Phase transition from gas to solid.

• Ionization: Phase transition from gas to plasma.

• De-ionization or recombination: Phase transition from plasma to gas.

Activity 1- make vocabulary cards for the words above

Activity 2- click on the image and copy onto your notes. link 

Activity 3 Play the game link 

Activity 4- Watch the video and take the quiz link 

Standard: 7.PS1.1 Develop and use models to illustrate the structure of atoms, including the subatomic particles with their relative positions and charges

Day 3  What are atoms? 

Do you like mysteries? Are you curious? Humans are curious. Someone always wants to know something that is not easy to detect or to see what can't be seen. For example, people began wondering about matter more than 2,500 years ago. Some of the early philosophers thought that matter was composed of tiny particles. They reason that you could take a piece of matter cut it in half, cut that piece in half again and continue to cut it again and again. Eventually you would be able to cut anymore. You would only have one particle left. They name these particles atoms, a term that means, "cannot be divided".

Bill Nye: Introduction to the atom

Activity 1. Watch the episode and complete the handout. 

videowww.youtube.com/watch?v=ogPNZ_MXksM 

handout:docs.google.com/document/d/1GAIm295jziJZaz-_4FGwC5x_tADk6m9EzadNz1AZux4/edit?usp=sharing 

Activity 2. Draw the time line below in your note book or paste the one from the bottom. Cut along the solid line to create flap for each scientist.

Read the information and fill in each flap. 

Day 4 Thinking about matter 

Democritus, a Greek philosopher, co-originated the thought (with his teacher, Leucippus) that all matter is composed of indivisible elements. Atomos=undividable

Shape

Dalton: John Dalton, a British chemist and physicist, developed a theory that matter is simply composed of atoms of different weights and is combined in ratios by weight. Also proposed that these atoms are spherical, and are in motion

Electrons discovered 

Thompsons plum pudding model- J. J. Thomson discovered the electron in 1897 through his studies of cathode rays, which he found were composed of negatively charged particles much smaller than atoms.

Structure of an atom developed (1909-1911) 

Ernest Rutherford known as the father of nuclear physics, developed the theory for the structure of the atom. He used a gold foil experiment, observing the scattering of alpha particles, and demonstrated for the first time the existence of the atomic nucleus. In 1911, Ernest Rutherford suggested that atoms also contain a central positive charge, making up most of their mass.

Bohr improves the atomic model 

Neils Bohr developed the Bohr atomic model, with electrons travelling in orbits around the nucleus, and chemical properties being determined by how many electrons are in the outer orbits. He also integrated the Planck quantum theory, stating that when electrons change orbits they emit a quantum of discrete energy.

The neutron is discovered 

James Chadwick discovers the neutron component of the atomic nucleus, explaining the nuclear fission of uranium 235. In 1932, James Chadwick was able to calculate the mass (and prove the existence) of neutrons by firing them at paraffin wax and determining the energy of the protons they displaced. This also made it possible to produce elements heavier than uranium in the lab.

reading- History of Atoms

Add the following to your flap: link 

Activity 3: Watch the Brain Pop and write 5 notes. Atomic Models  

Use your notes to take the quiz.

What are the parts of an atom? Dogs teaching chemistry link 

 Activity 4. Watch Brain Pop and take notes. Atoms 

Activity 5: Write cards for the following words

Vocab: atoms, protons, neutrons, electrons, ions, isotopes

To draw an atom:

Put the correct number of protons and neutrons in the nucleus

Put the electrons on the different energy levels.

Activity 6:video history of atoms 

Activity 7: Lab: atom activity link 

You and your partner take turns reading the slides. Copy down the information found on slides 22-26 in your notebook.

Activity 8. Quizziz lesson and notes link 

Day 5

Standard: 7.PS1.5 Use the periodic table as a model to analyze and interpret evidence relating to physical and chemical properties to identify a sample of matter. 

What do the elements represent? link 

Activity 1: Lab: Take your bag of Legos and sort them. Try to make as many categories as you can. Create a chart in your notebook and draw each piece.

Activity 2: Periodic table  https://www.brainpop.com/science/matterandchemistry/periodictableofelements/  Watch the video and write down 8 things that you learn in the video. Use your notes and take the quiz.

In the periodic table of the elements, elements are arranged in a series of rows (or periods) so that those with similar properties appear in a column. Elements of the same period have the same number of electron shells; with each group across a period, the elements have one more proton and electron and become less metallic.

The periodic table has eight main groups: 1, 2, 13, 14, 15, 16, 17, and 18 (previously numbered Ia, IIa, IIIa, IVa, Va, VIa, VIIa, and 0, respectively). Each group consists of elements that have similar electronic structures characterized by completely filled inner electron shells and by a number of electrons in their outermost shells equal to the group number.

The alkali metals, found in group 1 of the periodic table (formerly known as group IA), are very reactive metals that do not occur freely in nature. These metals have only one electron in their outer shell. Therefore, they are ready to lose that one electron in ionic bonding with other elements. As with all metals, the alkali metals are malleable, ductile, and are good conductors of heat and electricity. They are also reflective. The alkali metals are softer than most other metals. Cesium and francium are the most reactive elements in this group. Alkali metals can explode if they are exposed to water.

The alkaline earth elements are metallic elements found in the second group of the periodic table. All alkaline earth elements have an oxidation number of +2, making them very reactive. Because of their reactivity, the alkaline metals are not found free in nature.

One characteristic of metals is their ability to be deformed without breaking. Malleability is the ability of a metal to be hammered into shapes. Ductility is the ability of a metal to be drawn into wire. Because the valence electrons can move freely, metals are good heat conductors and electrical conductors.

Non-metals are the elements in groups 14-16 of the periodic table. Non-metals are not able to conduct electricity or heat very well. As opposed to metals, non-metallic elements are very brittle, and cannot be rolled into wires or pounded into sheets. The non-metals exist in two of the three states of matter at room temperature: gases (such as oxygen) and solids (such as carbon). The non-metals have no metallic luster, and do not reflect light. They have oxidation numbers of ±4, -3, and -2.

Activity 3.  Draw one of the elements on the table. Label the atomic number, mass, symbol. How many protons, neutrons, and electrons are in your element?

 Day 6 Protons, neutrons, electrons, and isotope

The atomic number will tell you how many protons and electrons are in each atom. To determine the number of neutrons, round the mass to the nearest whole number and subtract the atomic number. 

Isotopes are variants of a particular chemical element which differ in neutron number, although all isotopes of a given element have the same number of protons in each atom. The term isotope is formed from the Greek roots isos and topos, meaning "the same place"; thus, the meaning behind the name is that different isotopes of a single element occupy the same position on the periodic table. This is the reason mass number is presented in a decimal form. 

Activity 1 Brain Pop: Isotopes 

Activity 2 Websites for explanations: website 

Activity 3: Draw a model of hydrogen, oxygen, carbon, sodium, chlorine.

While many elements differ dramatically in their chemical and physical properties, some elements have similar properties. We can identify sets of elements that exhibit common behaviors. For example, many elements conduct heat and electricity well, whereas others are poor conductors. These properties can be used to sort the elements into three classes: metals (elements that conduct well), nonmetals (elements that conduct poorly), and metalloids (elements that have properties of both metals and nonmetals).

Activity 4: Complete pages 1-3 of the project-exploring atoms (copy can be found below) using the interactive periodic table below 

http://www.ptable.com

http://www.chemicalelements.com/ 

Atoms Family Song https://www.youtube.com/watch?v=Le9a8C0Pk2c

Another song https://www.youtube.com/watch?v=d3YR8e_iHlk

Activity 5: Using the information below, complete the Unit 2 physical and chemical changes worksheet ( copy can be found at the bottom of this page)

Activity 6: Elements- cell phones and the body

a; read the article and complete the handout

b: use the second handout and work with a partner to research one element found in the body. Put the information on a google slide and share it with me.

We are all just stardust

Day 7: Physical and Chemical Properties

Basically, physical properties are those which you can observe and measure without changing the chemical identity of your sample. Physical properties are used to describe matter and make observations about it. Examples of physical properties include color, shape, position, volume and boiling point.

Physical properties may be subdivided into intensive and extensive properties. An intensive property (e.g., color, density, temperature, melting point) is a bulk property that does not depend on the sample size. An extensive property (e.g., mass, shape, volume)  is affected by the amount of matter in a sample.

by Anne Marie Helmenstine, Ph.D.

Updated August 02, 2018

Activity 1 Watch the video and take the quiz link 

Chemical properties are any of the properties of matter that may only be observed and measured by performing a chemical change or chemical reaction. Chemical properties cannot be determined by touching or viewing a sample; the structure of the sample must be altered for the chemical properties to become apparent.

Examples of Chemical Properties

Here are some examples of chemical properties.

Reactivity with other chemicals

Toxicity

Flammability

Heat of combustion

Oxidation states

Chemical stability

Types of chemical bonds that will form

Activity 1 Watch the video and take the quiz 

More information go to https://opentextbc.ca/chemistry/chapter/physical-and-chemical-properties/ 

Day 6 Physical and chemical changes- Generation Genius

Matter is capable of undergoing changes, which are classified as either physical or chemical. Physical changes in matter are often reversible: An ice cube can melt into liquid water, and then the liquid water can be frozen back into an ice cube. Chemical changes, on the other hand, are not reversible: A log burned in a fire turns to ashes, but the ashes cannot be changed back into a log. What Is a Physical Change?

In a physical change, the material involved in the change is structurally the same before and after the change. Types of some physical changes are texture, shape, temperature, and a change in the state of matter. A change in the texture of a substance is a change in the way it feels. For instance, a block of wood may feel rough when you run your finger across it but rubbing the wood with sandpaper smooths the surface so it no longer feels rough. The wood itself has not changed during sanding to become a new material, only the texture of the surface changed. A piece of metal may be heated in a fire until it glows, but the metal is the same material before heating and after cooling. Similarly, when a material changes phase like going from a solid to a liquid, it only changes physically; the substance is still the same.

 A chemical change occurs when the composition of a substance is changed, which requires the breaking and forming of chemical bonds during a chemical reaction. This results in the rearranging of atoms in substances to form the products of a chemical reaction, which are brand new molecules that cannot be easily reverted back to their original state.

Sometimes it is difficult to tell if a chemical reaction has taken place. To help determine whether there has been a reaction, chemists consider the basic indicators that a reaction has occurred, such as a change in temperature, a change in color, the development of an odor, the formation of a precipitate, or the formation of a gas.  

Lab: see below- class reading sheet

Standard: 7.PS1.2 Compare and contrast elemental molecules and compound molecules.

Day 7 To understand about molecules, let’s say that you have something which is having two or more elements like Oxygen (O2 – in which you have two oxygen chemically bonded) is a molecule.They are the same they are an elemental molecule. 

Same for compounds, let’s say if you have two or more molecules. If you take H2O, where you have two Hydrogen and one Oxygen chemically bonded, then you can call it as a compound. Now, if you take another example like CaCl2, i.e., Calcium and Chlorine, then these are different molecules that come together to create a compound.

Let’s try one more. (Pause if you need to think about it.) For CH4, we have Carbon and four Hydrogen atoms. So, we have more than two elements that make it a molecule, but they are also different. So it’s a compound as well.

If we take something like P4 as an example, we have four Phosphorus atoms chemically bonded. So basically, two or more elements give us a molecule. But in this case, they are all the same, and we don’t have different components. Therefore, it can’t be a compound. P4 is just a molecule.

Brain Pop: Chemical bonds https://www.brainpop.com/science/matterandchemistry/chemicalbonds/

Activity 13: Read pages 260-265 in the blue 8th grade science book. Complete the note taking sheet ( a copy can be found at the bottom of the page)

What is a monoatomic atom? In physics and chemistry, monatomic is a combination of the words "mono" and "atomic", and means "single atom". It is usually applied to gases: a monatomic gas is one in which atoms are not bound to each other. All chemical elements will be monatomic in the gas phase at sufficiently high temperatures.

What is a diatomic element?

Key Points

Diatomic elements are pure elements that form molecules consisting of two atoms bonded together.

There are seven diatomic elements where the elements are the same: hydrogen, nitrogen, oxygen, fluorine, chlorine, iodine, bromine.

These elements can exist in pure form in other arrangements. For example, oxygen can exist as the triatomic molecule, ozone. 

Many compounds are diatomic, such as HCl, NaCl, and KBr. Diatomic compounds consist of two of the same or two different elements.

Activity 1: Have your group come up with a sentence that uses the first letter of the seven diatomic elements. 

Activity 2: complete page 4 of your project-exploring atoms.

Activity 3: Sorting activity

Day 8 Standard: 7.PS1.4 Analyze and interpret chemical reactions to determine if the total number of atoms in the reactants and products support the Law of Conservation of Mass.

chemistry link 

The law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations. According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.

Labs: steel wool, vineagar and water balloons, slime

Activity 16 :Watch the following Brain Pop and write 5 notes. Take the quiz using your notes. Brain Pop: Conservation of mass https://www.brainpop.com/science/matterandchemistry/conservationofmass/Activity 17: Watch the following Brain Pop and write 8 notes. Take the quiz using your notes. Chemical equations https://www.brainpop.com/science/matterandchemistry/chemicalequations/ Counting Atoms

It is important to be able to interpret and understand chemical formulas….this means being able to count the atoms of each element in a compound

Rules for Counting Atoms… 

1. Symbols: - Each CAPITOL letter means that there is a NEW ELEMENT Ex) Li2Cl3  is made of LITHIUM and CHLORINE

Na2SO4  is made of SODIUM, SULPHUR and OXYGEN

2. Subscripts: - A NUMBER that comes after a SYMBOL and BELOW. - The subscript only affects the element it COMES AFTER.Ex) Li2Cl3  has 2 LITHIUM atoms and 3 CHLORINE ATOMSNa2SO4 has 2 SODIUM atoms, 1 SULPHUR atom and 4 OXYGEN atoms

.3. Brackets: - A SUBSCRIPT OUTSIDE a bracket affects ALL the elements INSIDE the bracket…(ie. MULTIPLY!!!)Ex)

 Al(SO4)3 has 1 ALUMINUM atom, 3 SULPHUR atoms and 12 OXYGEN atoms. There’s 3 of everything in the brackets!

4. Coefficients: - A “FULL SIZE” number in FRONT of a chemical FORMULA. - MULTIPLIES everything in the formula:

Ex) 2Na2SO4  has 4 SODIUM atom, 2 SULPHUR atoms and 4 OXYGEN atoms 2Al(SO4)3 has 2 ALUMINUM atom, 6 SULPHUR atoms and 24 OXYGEN atomsvideo counting atoms  video 2 -counting atoms  https://www.youtube.com/watch?v=wV2TUHjgPLQ

• Activity 1: Complete the handout How to Count atoms in a compound. ( a copy can be found at the bottom of the page)

Day 9 Standard: 7.PS1.3 Classify matter as pure substances or mixtures based on composition.

Activity  Watch the following Brain Pop. Click on the activities tab and write vocabulary cards for each term. 

Compounds and mixtures https://www.brainpop.com/science/matterandchemistry/compoundsandmixtures/ 

Study jams http://studyjams.scholastic.com/studyjams/jams/science/matter/mixtures.htm

A pure substance contains only one kind of molecule, and a mixture is a combination of two or more pure substances. Distilled water, aluminum foil and table sugar are each made from only one type of particle. However, salt water is a mixture because it contains salt as well as water. Both pure substances and mixtures can exist as solids, liquids or gases. Most ordinary things are mixtures with at least two types of molecules. For example, air is a mixture of pure substances, including nitrogen, oxygen and carbon dioxide. Apple juice is another common mixture that includes particles of water, sugar, flavoring and vitamins.

Many substances in nature are not pure substances, instead they are mixtures. And lemonade is a mixture - a combination of two or more elements and/or compounds. Lemonade is comprised of ingredients (such as water, sugar and lemon juice) that have their own chemical formulas. The sour taste of lemon is caused by the presence of organic acids. The major acid in lemons is citric acid (C₆H₈O₇) which makes up around 5 to 6% of the lemon's juice. Other acids are also present, although in much lower concentrations than citric acid. Malic acid(C₄H₆O₅) is one of these, present at around 5% of the concentration of citric acid.

Lemons contain high levels of vitamin C, also known as ascorbic acid (C₆H₈O₆). The levels in lemon are around 50mg per 100g.

Simple sugars are called monosaccharides and glucose is one of them with a chemical formula C₆H₁₂O₆. This means that in one molecule of sugar there are six carbon atoms, twelve hydrogen atoms and six oxygen atoms. Lastly, water as we all know has a chemical formula of H₂O.

Lab: you and your partner will analyze a common household product and list the compounds present. 

Activity 1: Notes on mixtures. Reading activity is located at the bottom. 

Activity 2. Lab- Separating liquids activity sheet below

Activity 3: https://prezi.com/6trjfq6cafze/element-compound-mixture-the-game/

mixtures vs pure substance quiz https://www.quiz.biz/quizz-367168.html#debutform367168

Going Beyond- Whole Lotta Rules Going On

The process of naming compounds is just a set of rules. We're going to show

you some of the basics. There are some advanced ways of naming things that

we're going to skip right now. 

When you have two different elements, there are usually only two words in the compound name. The first word is the name of the first element. The second word tells you the second element and how many atoms there are in the compound. The second word usually ends in IDE. That's the suffix. When you are working with non-metals like oxygen (O) and chlorine (Cl), the prefix (section at the beginning of the word) of the second element changes based on how many atoms there are in the compound. It's like this... 

Let's put these ideas together! Remember, we're

only talking about simple compounds with no metal elements. Most simple

compounds only have two words in their names. Let's start with carbon monoxide

(CO). That name tells you that you have one carbon (C)

atom and one oxygen (O) atom (you can also use the prefix MONO to

say one atom). Remember that the second word ends in -ide. So... 

(1) Carbon+ (1) Oxygen = Carbon monoxide (CO)

Now we'll build on that example. What if you have one carbon (C) and two oxygen (O) atoms? 

(1) Carbon + (2) Oxygen = Carbon dioxide (CO2)

One last example and we'll call it quits. Now you have one carbon (C) and four chlorine (Cl) atoms. 

(1) Carbon + (4) Chlorine = Carbon tetrachloride (CCl4)

You should be getting the idea now. The compound name can tell you how many atoms are inside. Take a look at some of the examples and see if you understand what is happening in the name. 

Blend space lesson links: what are atoms?  https://www.tes.com/lessons/HuUEPTsGQpI22w/copy-of-atoms

Acids and bases:game

great website link