3. Pg.1 of Elements,
Compounds & Mixtures
Draw a RED line between
COMPOUND and
MIXTURE
4. 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?
5. 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?
6. 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?
7. 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?
8. 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?
9. In Charge of Leading
Discussion
1. Log into Learning Point
2. Daily Assignments
3. This Week
4. Open “Elements, Compounds
and Mixtures” slide share
5. Use your abbreviation skills
6. R & R on pgs. 1,2 & 3
10. 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.
11. 1. One kind of atom
2. Pure (because all particles are the
same)
3. Smallest particle to retain
identity of the element
4. Separated only in nuclear
reactions
12. Particles look like:
Every atom looks
8 exactly the same
8 w/ the same
8 number of protons
Oxygen
1
1
1
Hydrogen
13. Example:
Aluminum: Every
atom of aluminum
in this can is
exactly the same
Your Example?
14. 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)
CO
4. Separated or rearranged in
chemical reactions
2
15. Particles look like: Every compound
looks exactly the
same w/ the same
set ratio
Carbon Dioxide –
CO2
Sodium Chloride -
NaCl
16. Example:
Salt: Every
molecule of the
compound NaCl is
exactly the same
Your Example?
17. 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
18. Particles look like:
Each particle keeps its
own identity….they are
just “blended” together
Mixture #1
Mixture #2
19. 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
Your Examples?
25. 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.
26. 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.
27. • Homogeneous: 2 or more
things evenly blended and
disappear into each other.
• Solute – Smaller quantity by %
• Solvent – Larger quantity by %
• Solution – a homogeneous
mixture
28. • Heterogeneous: 2 or more
things put together and still
can be seen.
• No set RATIO.
29. 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 .
30. 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.
31. Saturation Level What does this What does this look
mean? like? (color)
Unsaturated •Mixture contains more
solvent than solute
•Able to dissolve more
solute
Saturated •Mixture contains the %
of solute completely
dissolved by solvent
•No able to dissolve
more solute
Supersaturated
•Mixture contains the %
of solute unable to be
dissolved by the % of
solvent at the given
temp.
High temp usually = higher solubility
32. 1. We now know the definition of
Element, Compounds & Mixtures
2. What do their particles look like?
