Elements, Compounds & Mixtures Day 1 - 2013

You Will Need:1. Pencil, Colored pencils2. Element Booklet Directions stapled

to Bibliography - Due now3. Element Booklet – Put into Zip Loc

Bag - Due now 4. Elements, Compounds and

Mixtures – 1 sheet 2 sides – Bookshelf – This is only Part 1

5. Periodic Table – Pgs. 196-197 in the text book

1.Elements that have the same # of protons but a different E of neutrons are called ____________.

2.Why are Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium and Francium all in Family 1?

3.What does the atomic mass tell you about the atom of an element?

4.What family are the Halogens on the Periodic Table?

5.Which elements tend to gain electrons to complete their valance shell?

6.How many neutrons does Calcium contain?

7.What is the most common isotope of Silicon?

8.Why are the Rare Earth elements at the bottom of the Periodic Table?

9.Which scientist believed the atomic structure to look like a “Plum Pudding”?

10.Where are the transition elements located on the Periodic Table?

11.How many valence electrons does Oxygen have? How do you know?

12.Which family is also known as “INERT Gases”?

13.Why are the elements on the Periodic Table neutral?

14.How many valence electrons does Helium have? Why?

In Charge of Leading Discussion1. Log into Learning Point2. Daily Assignments3. This Week4. Open “Elements, Compounds

and Mixtures” slide share5. Use your abbreviation skills

1.Elements are pure substances made of only one kind of atom.

2.As we have learned, atoms are tiny structures found in all matter.

3.Most substances contain many different atoms.

4. It is how those atoms are arranged that determine whether you have an element, compound or mixture.

1. One kind of atom2. Pure (because all particles are

the same)

3. Smallest particle to retain element’s identity

4. Separated only in nuclear reactions

Particles look like:

Every atom looks exactly

the same w/ the same number of

protons

Oxygen

Hydrogen

11

1

88

8

Example:

Your Example?

Aluminum: Every atom of

aluminum in this can is exactly

the same

1. Two or more kinds of atoms chemically bonded

2. Pure (because all particles are the same)

3. Smallest particle to retain the Compound’s identity (SET RATIO of particles)

4. Separated or rearranged in chemical reactions CO

2

Particles look like:

Every compound looks

exactly the same w/ the

same set ratio

Carbon Dioxide – CO2

Sodium Chloride - NaCl

Example:

Your Example?

Salt: Every molecule of the compound NaCl is exactly the

same

1. Two or more elements and/or compounds blended together physically

2. Not pure (because all the particles are not the same)

3. Separation through distillation, magnetic, evaporation, density, or particle size

4. No set ratio

Particles look like:

Each particle keeps its own

identity….they are just “blended”

together

Mixture #1

Mixture #2

Examples:

Your Examples?

Heterogeneous: Different components are easy to see in

this type of blending

Homogeneous: Different components are difficult to see

because they are evenly distributed

Compound

Mixture

1. A solution is a mixture where all the components blend together to look like one substance.

2. A solution is a homogeneous mixture that appears to be a single substance.

3. The solution is composed of particles of two or more substances that are distributed evenly among each other and have the same appearance and properties throughout.

1. In solutions, the SOLUTE is the substance that is being dissolved and usually is the smaller quantity in the mixture.

2. The SOLVENT is the substance in the solution doing the dissolving and is usually the larger quantity in the mixture.

3. It is the SOLVENT that is doing the dissolving.

4. Go to page 144-145 in your textbook: Give examples of solutions in various states.

• Homogeneous: 2 or more things evenly blended and disappear into each other.

• Solute – Smaller quantity by %

• Solvent – Larger quantity by %

• Solution – a homogeneous mixture

• Heterogeneous: 2 or more things put together and still can be seen.

• No set RATIO.

Have you ever put sugar into lemonade and seen the grains of sugar sink to the bottom and not dissolve?

This is because the lemonade (solution) is supersaturated. In other words, there is not enough water (solvent) to completely dissolve the sugar (solute).

Temperature and Pressure can affect saturation levels as well.

1. Elements, Compounds & Mixtures - To be “on-time” Pg. 1 & ½ of Pg. 2