1. D.S.Q 12/21/16
1. All substances are made up of a very small particle; what is that particle called?
2. Where can you find all of the elements listed?
3. Why do you think the periodic table was created?
1. Atoms
2. Periodic Table
3. To keep all the elements organized and to help scientists identify specific traits for each element.

2. D.S.Q. 12/22/16
1. What is an atomic nucleus made up of? (You should remember this from the video yest.)
2. Elements that have an atomic mass greater than 92 can only be found where?
3. To become positively charged, an atom must…?
1. Protons and neutrons
2. In a science lab
3. Lose an electron

3. D.S.Q. Element Symbol: Ba Element Name: __________
Atomic number: _________
Mass number:___________
# of protons: ____________
# of neutrons: ___________
# of electrons: __________
Element Symbol: Rn
Element Name: __________
Atomic number: _________
Mass number:___________
# of protons: ____________
# of neutrons: ___________
# of electrons: __________

4. D.S.Q. 1. What element has the symbol B?
2. What element has the symbol Na?
3. What element has the symbol K?
Sodium
Boron
Potassium

5. Combining Atoms Activity
Procedure
1. Use the Periodic Table and analyze the chemical formula to construct a model of each molecule with snap together cubes.
2. Fill in the number and type of each atom in the molecule in the substance composition column.
3. Fill in the boxes provided with the color noted in the KEY to represent the model.

6. D.S.Q
1. Label the two pictures as either a homogenous or heterogeneous mixture.
2. What are all these called in the image below.

7. Science Song !

8. Matter

9. Measuring Matter
Which weighs more, a pound of feathers or a pound of sand?
Weight is a measure of the force of gravity on an individual.
The force of gravity is greater on Earth than it is on the moon.

10. Measuring Matter
How can you weigh less on the moon than on Earth when nothing about you has changed?
Your weight depends on the gravitational force, however, your mass stays the same.
Mass is the amount of matter in an object.
Therefore, if you were to travel to the moon, the amount of matter in your body DOES NOT change

11. Mass The SI unit for mass is the Kilogram (kg)
Grams are also used to measure smaller units of mass
How do we convert grams to kilograms?
There are 1,000 grams in a kilogram. Or kilograms in a gram.
Kg = G ÷ 1,000
G = Kg x 1,000

12. Now you try! Object Mass (g) Mass (kg) Nickel 5 0.005 Baseball 150
Pineapple
1,600
Full can of soda
390
Inflated balloon 3

13. Answers
0.15
1.6
0.39
0.003

14. Volume The amount of space matter takes up
Solids, liquids AND gas all have volume!
The SI unit for volume is cubic meter (m³)
Other common units are:
Cubic centimeters (cm³)
Liters (L)
Milliliters (mL)

15. HOMEWORK:
1. What holds the hydrogen and oxygen atoms together in a water molecule?
2. Table sugar has the chemical formula C12H22O11. What is the ratio of carbon atoms to oxygen atoms in this compound?
3. Two formulas for compounds containing hydrogen and oxygen are H2O and H2O2. Do these formulas represent the same compound? Explain why or why not.

16. Changes in Matter

17. Changes of states How many states of matter are there?
3-solid, liquid and gas.
Suppose you leave a small puddle of liquid water on the kitchen counter. When you come back two hours later, the puddle is gone.
What happened to the water?
A physical change happened. The liquid water changed into water vapor (gas)

18. States of matter How do aluminum, water, and air differ?
Aluminum is an element
Water is a compound
Air is a mixture
How are these three types of matter different?
Aluminum is a solid
Water is a liquid
Air is a gas

19. States of matter continued
All particles of matter are constantly moving.
Every solid, liquid and gas around you is made up of moving particles that attract one another
What makes some matter a solid, some a liquid and some a gas?
It all depends on how close the particles in the matter are to one another and how fast they move.

21. Physical Properties
Is a characteristics you can observe or measure without changing the identity of the matter.
Ex. Gold is shiny

22. Size-Dependent Properties
Some physical properties, like mass and volume, depend on the size or amount of matter.

23. Size-Independent Properties
These physical properties do NOT depend on the amount of matter present.
Examples:
Melting point
Boiling point
Density
Electrical Conductivity
Solubility

24. Size-Independent Properties
Melting & Boiling Point:
The temperature at which a substance changes from a solid to a liquid is its melting point.
The temperature at which a substance changes from a liquid to a gas is its boiling point.

25. Notice the temp. doesn’t depend on how much water is in the beaker.

26. How is density determined?
Density is a measure of the mass of a material in a given volume.
You can find the density of a material by dividing its mass by its volume
Which objects will sink, which will float?
A block of wood and a block of iron
Wood would float, iron would sink because wood is less dense than water and iron is more dense than water
Density is a physical property
It is a size-independent property

27. Conductivity & Solubility
Conductivity is the ability of matter to conduct, or carry along, an electric current
Solubility is the ability of one substance to dissolve in another.

28. What happens to a substance in a physical change?
A physical change alters the form or appearance of matter but does not turn any substance in the matter into a different substance.

29. Change in shape & size Examples of changes in shapes and sizes.
When you chew food, you are breaking it down into smaller pieces.
When you pour juice from a bottle, you are changing the shape of the juice
If you fold clothes to fit them into a drawer, you are changing their shape.
Changes in shape and size are physical changes and the identity of the matter has not changed.

30. Examples of Physical Changes
melting point
electrical conductivity
color
density
boiling point
thermal conductivity
odor
hardness

31. Change in state of matter
Matter can change into different states of matter.
Ex. An ice cube is a solid, water is a liquid and water vapor is a gas
To change the movement of particles, thermal energy must be either added or removed.

32. Temperature & Thermal Energy
Temperature is a measure of how hot or cold something is.
Temperature and energy are related
For instance, the particles in warm air have greater energy, than the particles in cold air
Thermal energy is the total energy of the motion of all of the particles in an object
Thermal energy flows from warm cold

33. Thermal Energy & Changes in Matter
Thermal energy is a form of energy that is released or absorbed
Example: ice absorbs thermal energy from its surroundings when it melts and leaves the surrounding feeling cold.
The melting of ice is an ENDOTHERMIC CHANGE, a change in which energy is absorbed
Endothermic reactions usually feels cold because it is taking heat away from you.
An exothermic change releases energy
Exothermic reactions usually feels hot because it is giving heat to you

34. Adding thermal energy
When thermal energy is added to a solid, the particles in the solid move faster and faster and the temperature increases.
As the particles move faster and faster, they become tightly bonded
However, if they move to fast where they cannot stay tightly bonded, that is when melting point happens.

35. Adding thermal energy cont.
After the solid receives thermal energy, it turns into a liquid.
IN the liquid, the particles start moving even faster and the temp. increases even more
If the liquid gets to hot, where the particles can’t stay together anymore, it turns into a gas.

36. Adding thermal energy Cont.

37. Removing Thermal Energy
When thermal energy is removed from a gas, particles in the gas move more slowly and the temp. decreases.
Condensation occurs
Wait, what is condensation again?
Condensation is when a gas becomes a liquid

38. Removing Thermal Energy Cont.
After the gas has turned into a liquid, the more energy that is removed, the slower the particles move and the temp. decreases even more
Last step, freezing occurs and the particles are tightly packed together and vibrate in place.

40. Red=Endo…..Blue=Exo

41. Examples: Exothermic Processes Endothermic Processes freezing water
solidifying solid salts
condensing water vapor
making a hydrate from an anhydrous salt
forming an anion from an atom in the gas phase
Annihilation of matter E=mc2
splitting of an atom
melting ice cubes
melting solid salts
evaporating liquid water
making an anhydrous salt from a hydrate
forming a cation from an atom in the gas phase
splitting a gas molecule
separating ion pairs
cooking an egg
baking bread

42. How are changes in energy and matter related?
What is energy again?
The ability to do work
Every chemical and physical change in matter includes a change in energy.
Energy is NEVER created nor destroyed. It can only be transformed from one form to another

43. Chemical Property
Is a characteristic of matter that can be observed as it changes to a different type of matter.
Example: Burning paper

44. What happens to a substance in a chemical change?
Chemical change or a chemical reaction is a change in matter that produces one or more new substances
In some chemical changes, a single substance breaks down into two or more substances
Example: Hydrogen peroxide breaks down into water and oxygen gas when poured on a cut
Photosynthesis is a natural chemical change

46. Chemical Vs. Physical Change

47. Example of Chemical Changes

48. Law of Conservation of Mass
French chemist, Antoine Lavoisier, discovered that matter is not created nor destroyed in any physical or chemical change
Example:
Suppose you could measure all the carbon dioxide and water produced when methane burns.
What do you notice about the mass in the beginning and at the end? Is it the same amount of different?