1. The Human Organism and the Organization of Matter
Ch. 1: What’s the Matter?
The Human Organism and the Organization of Matter
Matter: anything that has volume & mass.
Ex. a desk
Ex. Pizza
Ex. silver necklace
Ex. oxygen

2. Mass: amount of matter found in an object.
measured using the triple beam balance or electronic balance.
The unit of measure is grams (g) Ex: The rock has a mass of 10.8g.
Weight: the pull of gravity on an object. Gravity acts on the mass of an object.

3. Volume amount of space taken up by an object or substance.
Regularly-shaped objects. ex: metric ruler (cm3)
V = length x width x height
Water displacement method - for irregularly-shaped objects
Use a graduated cylinder - for liquid (read the meniscus), unit of measure litre (l)
1ml = 1cm3

4. What do we do with volumes smaller than 1 L?
x10
x10
x10
x10
x10
x10
Kilo, Hecto, Deca, Unit (litres, meters), Deci, Centi, Milli
÷10
÷10
÷10
÷10
÷10
÷10
King Henry Died Uncle Didn’t Care Much
Often, we will be dealing with volumes which are less than 1 L.
Well, how many millilitres are there in 1L?
1L = 1000 mL
So in order to convert mL to L, you must divide the volume (mL) by 1000.
500mL = 0.5 L
300mL = ?

5. The Particle Model
A scientific model based on the idea that matter is made up of small particles that:
are extremely small.
are in constant motion.
when the temperature increases, the movement of these particles increases.
the particles may be held together by forces of physical attraction.

6. Phases/States of Matter
Particles in a:
Solid :
Bound by strong force of attraction, tightly packed, very organized
particles only vibrate, little movement.
Gives solids definite shape and volume
Liquid :
weaker attraction, very close with no arrangement
particles move about, slide past each other
takes shape of container, definite volume.
Gas:
No force of attraction, far apart,
Free movement at high speeds, take up all space given.
No definite shape or volume, taking space of container.

7. The Organization of Matter
Mixture
Pure Substance
Physical Separation
Hetero-geneous Mixture
Homo-geneous Mixture
Element
(Atom)
Ex. gold
Compound Ex. water
Chemical Separation

8. Pure Substance: Mixture:
composed of a single substance (one type of particle) with the same properties throughout
Ex: water (H2O)
Ex: table salt (NaCl)
Mixture:
combinations of two or more substances that are not chemically combined (mixed).
Easily separated
Ex: fruit salad
Ex: sugar in coffee
Ex: salt in water

9. A pure substance can be further broken down into an element or a compound……
Elements:
Pure substance that contains one type of atom/particle.
cannot be separated by chemical separation techniques.
Atoms: smallest particle of matter. The atomic model of matter.
Ex: Oxygen
Ex: Aluminum
Ex: Calcium
Ex: Copper
Particles making up matter are either molecules or atoms.

10. Recall, a pure substance can be further broken down into an element or a compound
Compounds:
substance made of two or more elements
can be separated into simpler substances
A molecule is formed when two or more atoms join together chemically. Ex: I Have No Bright Or Clever Friends; Iodine, Hydrogen, Nitrogen, Bromine, Oxygen, Chlorine, Florine
A compound is a molecule that contains at least two different elements.
All compounds are molecules but not all molecules are compounds.
Ex. Water (H2O)
Ex. Carbon dioxide (CO2)
Ex. Sugar (C6H12O6)
Ex. Salt (NaCl)

11. Element Compound Ex. oxygen & hydrogen Ex. water (H2O) NOTE:
With chemical reactions you can go from an element to compound & vise versa!!!
Element
Compound
Ex. oxygen & hydrogen
Ex. water (H2O) O O H H H H

12. State whether the following are examples of an element or a compound.
A gold ring
element
Rust (Fe2O3)
compound
Carbon monoxide (CO)
compound
Aluminum Foil (Al)
element
element
Calcium (Ca)

13. Ex #2
State whether the following are examples of an element or a compound or a mixture
A blueberry muffin
mixture
Chunky Soup
mixture
Salt (NaCl)
compound
Helium (He)
element
compound
Water (H2O)

14. Ex #3
State whether the following pictures represent an element or a compound or a mixture
Compound
Compound
Element
Mixture

15. Which statement best describes a compound.
Ex #4
Which statement best describes a compound.
A) A pure substance that has a high melting point.
B) A mixture that is formed by two or more elements.
C ) A pure substance that is formed by two or more elements.

16. Heterogeneous Mixture:
Mixtures: atoms and molecules together without forming chemical bonds. Requires at least two types of particles.
Heterogeneous Mixture:
Is made up of at least two substances that can be distinguished with the naked eye
mixtures that are not uniform
can see individual parts
Ex:Salad, chocolate chip muffin, vegetable soup, granite (biotite, quartz, feldspar), clouds
Homogeneous Mixture:
Mixture that looks uniform through-
out or like one substance
Ex: milk in coffee, sugar dissolved in
water, air, brass (copper and zinc)

17. Homogeneous Mixtures

18. Solution Contains a solvent and solute(s)
Solute: is a substance that dissolves in another substance.
Solvent: is a substance that can dissolve a solute.
Ex: saliva, sweat, tears, urine. For each of these examples water is the solvent and salt is one of the solutes.

19. Separating Mixtures Practically no pure substances in nature
Most separation techniques are physical separations
Get a pure substance when you can not physically separate any further.
Examples of use:
To make drinking water safe
To obtain gas from oil
To obtain precious metals (gold, silver) from various minerals

20. Separation Techniques
Decantation: The pouring off or out of a substance when constituents are separated by their densities. Usually used to separate heterogeneous mixtures.
Filtration: Passing a solid-liquid or solid-gas through filter paper. Can be used for heterogeneous or homogeneous.
Evaporation: Used to retrieve a solid that has dissolved. Usually used for solid in solution.
Distillation: Separate substances based on differing boiling points. Usually used to separate different liquids and/or a solid from a solution.
Centrifugation: Rapid spinning of a mixture to allow for decantation. Usually used for colloids.

21. Properties of Solutions
Concentration: the amount of dissolved solute in a given quantity of solution.
C is the concentration (in g/L)
m is the mass of the solute (in g)
V is the volume of the solution (in L)
Ex: 2 L of saltwater solution contains 5 g of salt. What is the concentration of the solution?
C = m V
m= 5 g C = m C= 5g C = 2.5 g C = 2.5 g/L V= 2 L V L L
FYI Energy drink companies study concentration of substances in human body to determine body requirements for refueling after extensive workouts.

22. Dilution: Decrease the concentration of a solution by adding solvent.
Solute = 13 g
Solution = 5 L
Solute = 13 g
Solution = 2 L
C = m = 13g = 6.5g/L
V L
C = m = 13g = 2.6g/L
V L

23. Procedure for making a specific concentration
Describe the procedure that would be used to prepare 250 ml of a sugar solution that has a concentration of 13 g/L.
BE SPECIFIC……
First, convert your volume from mL to L.
Find out you how much grams you need.
Step #1
250mL=0.25L
Step #2
C=m v
Write out procedure using a step by step method!
1. Pour half of the required volume (125 ml) into a beaker
2. Add the solute (3.25 grams) to the beaker
3. Mix them together
4. Add the solvent (liquid) until you reach the desired amount (250 ml)

24. Concentration in % Concentration can also be given in %.
The following are examples of items whose concentrations are given in %:
-hair dye
-wine
-beer
-rubbing alcohol
-nutritional food values

25. What does 12% on a wine bottle mean?
In this case, the label on the wine bottle means the wine contains 12% alcohol volume/volume
What does that mean?!
It means that for every 100mL of wine, there is 12mL of alcohol

26. But what if we need to know how much alcohol there is in the entire 750mL bottle?
What math operation do you think we should use?
CROSS-MULTIPLY & DIVIDE!
12mL = X
100mL mL
12x750/100=90mL of alcohol in the bottle

27. How can we convert concentration in % to g/L?
Example:
C= 25% m/v (mass/volume)
We know that 1L equals 1000mL.
So 25g = X
100mL mL
Once again, CROSS-MULTIPLY & DIVIDE.
25x1000/100=250g
Therefore, 250g/1000mL which equals 250g/L

28. Practice Problems
How much alcohol is present in 500mL of a 12% v/v wine bottle?
How much alcohol is present in 250mL of a 70% v/v bottle of rubbing alcohol?
Give the following concentrations in g/L
a) 17% m/v
b) 35% m/v
Do you see a pattern in your answers in #3?

29. Pure Substance: Elements
Elements are pure substances that are made up of only one constituent (substance).
Elements are placed into groups and families in the Periodic Table of Elements.
Their arrangement is based on similarities in properties that the elements share.

30. 25 elements are essential to life
The 4 major elements are carbon, oxygen, hydrogen and nitrogen
Make up 96% of matter on Earth.
Make up all molecules that form living organisms

31. Atoms & Molecules
An ATOM is the smallest particle of matter. It cannot be divided by chemical means.
A MOLECULE is a group of two or more atoms held together by chemical bonds.

32. The Atomic Model
An Atom is made up of a small (but heavy), positively charged Nucleus which consists of + charged Protons and neutral (no charge) Neutrons
The Nucleus is orbited by – charged Electrons

33. Properties of Pure Substances: Characteristic and Non-Characteristic properties
Non-characteristic property
Property that doesn’t help identify one substance
from another.
Ex: colour, shape, texture, state, mass, volume, temperature

34. Characteristic property
A characteristic property is one that helps us identify a pure substance or the group to which the pure substance belongs therefore it CAN identify a substance specifically.

35. Phase Changes are Physical Properties
Properties of Matter: Physical & Chemical
1) Physical Properties: Properties that do not change the chemical nature of matter.
usually those that we can observe with our senses
does not produce a new substance
must be measured at a specific temperature and
pressure.
Ex: melting point, boiling point, density, solubility, luster, malleability, ductility, thermal conductivity
Phase Changes are Physical Properties

36. Characteristic Physical Properties
Melting Point is the temperature range at which a solid changes state from solid to liquid. At the melting point the solid and liquid phase exist in equilibrium.
Going from a liquid back to a solid occurs at the same temperature range and it is referred to as the freezing point.
Ex: Water melts at 0oC
Ethanol melts at -117oC
Table salt melts at 801oC

37. Characteristic Physical Properties
2. Boiling Point when liquid is at the temperature at which the vapour pressure of the liquid equals the environmental pressure surrounding the liquid.
Ex: Water: 100oC, Ethanol 79oC, Table salt1465oC

38. Characteristic Physical Properties
3. Density: is the density of the substance, measured in g/cm3 or g/mL m
ρ V
Ex:
Water 1.0 g/mL
Ethanol 0.79 g/mL
Gold: 19.3 g/mL

39. Characteristic Chemical Properties Appendix on pg. 416 of textbook
2) Chemical properties: Properties that do change the chemical nature of matter.
relate to how the substance changes in composition or how it interacts with other substances.
produces a new substance
Help to identify a substance.
Many characteristic chemical properties are identified through reactions to indicators.
Fehling Reagent test:
Biuret Reagent test:
Reaction to litmus/pH paper:
Reaction of cobalt chloride paper:
Reaction to limewater:
Reaction of a glowing wood splint:
Reaction of a burning wood splint:
Reaction to an open flame:

40. Ex #1
You a leave a 2g copper penny outside. Over time, the penny becomes green in color & its mass is now 2.5g.
Which statements below are true?
TRUE
A) A chemical change occurred
B) A physical change occurred
TRUE
C) A compound was made
D) An element was made

41. production of two substances
Ex #2
You have 5g orange powder which you heat. As the powder is heated you noticed that a gas is given off & a silver liquid is produced. After heating you only have 1g of the orange powder left.
Which substance was definitely a compound? Why?
orange powder
decrease in mass
production of two substances

42. A grey colored solid is heated
A grey colored solid is heated. The following observations were recorded
Ex #3
Before Heating
After Heating
State
solid
Color
grey
black
Texture
smooth
granular
Mass
1.75g
2.5g
What statement is DEFINITELY true?
A) The solid after heating is an element
TRUE
B) The solid after heating is a compound
C ) The solid before heating is an element

43. Ex #4
In a lab you heat 50g of a white powder in an open container. Over time, you obtain a yellow substance with a mass of 65g.
Which statement is definitely FALSE?
A) The white powder could be an element
B) The white powder could be a compound
C) The yellow substance could be an element
D) The yellow substance could be a compound