Course Information/ Syllabus

Course Syllabus

Mr. Talon’s 8^th Grade Science

This will be the very first page in your binder.

Bear Team

“The Earth does not belong to man - man belongs to the Earth”- Chief Seattle

“People are lonely and only animals with fancy shoes”- Jack Johnson

Personal Information: Email: mailto: talon.j@rochesterschools.com –Use this resource, if you don’t understand something I can try to help. I can at least tell you that I can help you the next day.

Material to be covered:

Awesome stuff!!

Ecology, Life structure, and Earth Science

KEY POINT: If you do as I ask you will pass!!! It’s really amazing. If you read the chapters, take notes, do all assignments and pay attention, you should do fine.

Makeup is mandatory. Detention will be given if too many assignments are being missed.

Grading- All areas are worth 20%

Tests-20% -This includes formal (standard tests) and informal assessment (essays, take-home tests)

Quizzes-20% -This is a shorter and less difficult test

Homework-20% -The reason for homework is to change some of the information in your short term memory to your long term memory so you don’t forget it.

Classwork- 20% -This included daily board work, participation exercises and sub work

Projects/ Papers/ Labs- 20%

Tests and Quizzes may be made up by doing TEST CORRECTIONS.

By doing test corrections you are proving to me that you know it and that you went back to the book, notes, or internet and learned what you missed. You can write me full sentences, or paragraphs explaining topics that you missed. Do not just re-write the question. I will be happy to average your old and new grade. If you got below a 60, I will average a 60 with your new grade.

It is my vow to teach you science material that is relevant to your life, important to know, and will make you a more educated and informed individual.

I will never fail a student who tries and puts in effort. This does not mean that I will pass you for trying at the last minute. Don’t come to me looking for extra credit at the last moment.

Chapter 3 Substances and Mixtures and vocab

Talon
All material was taken From Glencoe Science

Chapter 3 Vocab-

Substance- Matter with a fixed composition whose identity can be changed by chemical processes but not by ordinary processes

Solution- Homogeneous mixture whose elements and/or compounds are evenly mixed at the molecular level but are not bonded together.

Solute- Substance that dissolves and seems to disappear into another substance.

Solvent- Substance that dissolves the solute

Precipitate- solid that comes back out of it’s solution because of a chemical reaction or physical change

Aqueous- solution in which water is the solvent

Solubility- measure of how much solute can be dissolved in a certain amount of solvent

Saturated- describes a solution that holds the total amount of solute that it can hold under given conditions

Concentration- describes how much solute is present in a solution compared to the amount of solvent

Acid- substance that releases H+ ions and produces hydronium ions when dissolved in water. (H+ donor)

Base- substance that accepts H+ ions and produces hydroxide ions when dissolved in water (H+ acceptor)

pH- measure of how acidic or basic a solution is, ranging in a scale from 0-14.

Indicator- compound that changes color at different pH values when it reacts with acidic or basic solutions

Neutralization- reaction in which an acid reacts with a base and forms water and salt.

Ch 3 sec 1 Note Outline

From Glencoe Chemistry

Objectives: 1) Distinguish between substances and mixtures

2) Describe two different types of mixtures

3) Describe how solids, liquids, and gases can form different types of solutions.

What is a solution?

Lets start by re-defining substance

- Matter that has a fixed composition

- Elements are “pure substances” (atoms are the simplest forms of matter)

-Cannot be broken down by ordinary physical processes (boiling, changing pressure, cooling, sorting)

• Substances above pure elements could be broken down by chemical means

-Burning, reacting with other chemicals, reacting with light

• Examples of substances-

-Compounds such as water, carbon dioxide, and thousands of others

-Compounds have fixed composition, there is a fixed proportion of atoms in a substance.

• Mixtures are different than substances

-can be separated by physical processes ex. Salt water, sugar water

-Mixtures do not have fixed proportions of atoms within them.

• Heterogeneous mixture- “hetero”- different, a mixture that is visibly different in its parts.

• Homogeneous mixture- “homo” same, a mixture with the same consistency. Contains two or more substances that are evenly mixed at the molecular level. Ex. Shampoo, salt-water, sugar-water

• Another name for a homogeneous mixture is a solution

- When we dissolve one substance into another we form a solution. Evenly mixed at the molecular level but not bonded.

- Solute- the substance that dissolves

- Solvent- What dissolves the solute. (Hint: more letters more substance)

- Ex. In sugar water the sugar is the solute, the water is the solvent.

- In gasses or solid solutions the substance in greatest quantity is the solvent.

• Precipitates- A solid that falls out of solution as a result of a mixture cooling or a chemical reaction

-yellow color in lead nitrate reaction

-rock candy in the cooling of super-saturated sugar water

-Minerals in water react with soap to leave scum as a precipitate -Stalactites and stalagmites are precipitates of minerals in caves

Types of solutions

1) Liquid- Gas- Carbonated beverages

2) Liquid- Liquid- Most common, vinegar is acetic acid and water

3) Liquid- Solid- sugar water, salt water

4) Gaseous solutions- two gasses mixed together, the air we breathe.

5) Solid- solid- Brass, Steel, two solids are mixed to serve better purpose. (alloys)

Questions:

1) What is the difference between a substance and a mixture?

2) How do heterogeneous and homogeneous mixtures differ?

3) What are two ways that precipitates form?

4) What is the common name for a solid-solid solution of metals?

Chapter 3 chemistry solubility, substances, and mixtures

All material was taken from Glencoe Science, Chemistry.

Chapter 3 section 2 Chemistry- Solubility

Objectives:

• Explain why water is a good general solvent
• Describe how the structure of a compound affects which solvents it dissolves in.
• Identify factors that affect how much of a substance will dissolve in a solvent.
• Describe the concentration of a solution.

Solute- What you’re dissolving into the solvent (the sugar in sugar-water)

Solvent- Whatever there is more of. (The water in sugar-water)

Water is the Universal Solvent

• A solution in which water is the solvent is called aqueous.
• Water can dissolve so many solutes, chemists call it the universal solvent.

Review Covalent bonds

• Colvalent bonds share electrons.
• Nonpolar covalent bonds share electrons equally.
• Polar covalent bonds share electrons unequally.
• Water is a polar covalent bond. The electrons spend more time around the oxygen atom because it is more electronegative.
• The oxygen atom has a partial negative charge.
• The hydrogen atom has a partial positive charge.

Review Ionic Bonds

• Ionic Bonds transfer electrons.
• This results in a charge of the atoms involved due to the loss or gain of electrons.
• An atom that has lost of gained an electron is an ion.

Solubility of ionic compounds

• Water can dissolve ionic compounds because the partial charges of oxygen and hydrogen attract the ions.
• When dissolved the partially charged water molecules pull the ions apart. Figure 8 pg 71.

Solubility of molecular compounds (covalent)

• Water does dissolve molecules but does not break them apart like ions.
• Water just moves between the molecules.

What will dissolve?

• Only similar substance will dissolve into each other.
• “Like dissolves like”
• polar molecules dissolve polar molecules
• Nonpolar molecules dissolve Nonpolar molecules.
• Trying to mix Nonpolar with polar will not work- ex. Water and oil

Solubility- A measurement that describes how much solute dissolves in a given amount of solvent.

What can increase solubility?

• Increased temperature- speeds up the particle contact
• Stirring or shaking- puts particles in contact
• Increase the surface area of the solute (break up a cube of sugar)

Saturated solution-

• One that contains all of the solute that it can hold under the given conditions
• Hot solvents can hold more solute.

Concentration-

• The amount of solute compared to the amount of solvent
• Ex. Juice may say that it’s 15% Juice.

Questions you may ask yourself-

1. What properties of water make it the universal solvent?
2. Why does sodium chloride dissolve in water but vegetable oil does not?
3. What are two ways to increase the rate at which a substance dissolves?
4. What is the difference between a dilute solution and a concentrated solution?