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Mixtures – Picked up yesterday

Test #3 Retakes1. 1 opportunities remain

Update Log #41. Assignment Log #4 – Update

w/new assignment

Pg.1 of Elements, Compounds & Mixtures

Draw a RED line between COMPOUND and MIXTURE

1. What families make up the Transition Metals?

2. Where would I find the Halogens on the P.T.?

3. What is the valence of Silicon?

4. What subatomic particle determines the charge of the atom?

5. When an atom is “charged”, what do we call this particle?

6. How are Elements and Compounds different?

7. How are Elements and Compounds the same?

8. Why are mixtures not “pure”?9. Name any 3 ways to separate a

mixture? 10.What does having a “set ratio” mean

for compounds?11.If I am looking at B10, B11 and B12,

how do I know the atom is Boron?

13.If I have dissolved 3.5 mL of HCl in a solution containing 165 mLof H2O, which component of this mixture is the solute and which is the solvent? How do you know?

14.Give an example of a heterogeneous mixture.

15.Give an example of a homogeneous mixture.

16.How are these two types of mixtures similar?

17.KNO3 = element, compound or mixture?

18.Bronze = element, compound or mixture?

19.Hamburger = homogeneous or heterogeneous mixture? Why?

20.What is the valence of Na and what family does this element belong to?

21.What is the valence of Barium?22.Which family is the most reactive

nonmetals on the P.T.? Why?

Look at the particles for each type of matter….Why did we draw a red line to separate the left from the right side of the chart?

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

and Mixtures” slide share5. Use your abbreviation skills6. R & R on pgs. 1,2 & 3

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

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

Most substances contain many different atoms.

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 identity of the element

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 identity of the compound (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

Categorize as either Atom, Element,

Molecule or Compound

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

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

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 which the solute is dissolved and usually is the larger quantity in the mixture.

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

• 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.

Discuss and Generate 3 bullets of information.

Turn to pgs 144-145 in your text book. There you will find a chart with examples of different solutions having different states. Complete the chart.

When coming up with your example, you may discuss as a group and use the same example.

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 also affects saturation levels.

Saturation Level

What does this mean?

What does this look like? (color)

Unsaturated

Saturated

Supersaturated

•Mixture contains more solvent than solute

•Able to dissolve more solute

•Mixture contains the % of solute completely dissolved by solvent

•No able to dissolve more solute•Mixture contains the % of solute unable to be dissolved by the % of solvent at the given temp.High temp usually = higher

solubility

1. We now know the definition of Element, Compounds & Mixtures

2. What do their particles look like?

1. Elements, Compounds & Mixtures - To be “on-time” Pgs. 1-4

2. Have a good weekend!