1. Unit 3: Introduction to Chemistry What is chemistry?

2. What we will be learning over the next 6 weeks
Before Christmas Break
History of the Atomic Theory
The Atom & It’s Subatomic Particles
Reading Element Squares & The Periodic Table
Determining number of subatomic particles
Valence Electrons & The Bohr Model
After Christmas Break
Elements, Substances, Compounds, & Mixtures
Physical & Chemical Changes
Chemical Reactions
How to Write Chemical Formulas
Balancing Chemical Equations
What we will be learning over the next 6 weeks

3. During notes, write the red info on the inside tab.
Bellwork:
Pick up handouts.
Cut foldable out like the example.
Fill in planner for the week.
History of the Atomic Theory Prezi
During notes, write the red info on the inside tab.
Activity:
Use your foldable to complete the timeline.
TURN IT IN WHEN DONE.

4. Bellwork: Pick up notes & activity.
Did you get your timeline turned in yesterday?
Atom’s Family Challenge Powerpoint

5. The Atomic Theory states...
Fill this in for Bellwork
All matter is made up of atoms.
All atoms of a given element are identical.
Compounds are formed when atoms of different elements combine in fixed amounts.
An atom cannot be created or destroyed, just rearranged in a chemical reaction.

6. Fill this chart in as we go through the notes.
Charge
Location
Discovered By
Proton
Neutron
Electron
Atoms are known as the building block of matter.
They are made of 3 subatomic particles...

7. Carbon atoms make up width of 1 strand of human hair.
1,000,000
Carbon atoms make up width of 1 strand of human hair.
1 trillion atoms
to make one human cell
500 years
Amt. of time it would take you to count the atoms in a grain of salt.

11. outside of the nucleus in electron orbits/levels
Check your chart.
Charge
Location
Discovered By
Proton
positive (+)
inside the nucleus
Rutherford
Neutron
no charge
Chadwick
Electron
negative (-)
outside of the nucleus in electron orbits/levels
Thomson
Atoms are known as the building block of matter.
They are made of 3 subatomic particles...

12. Periodic Table-
Arrangement of all chemical elements. Each element represents one atom of the given element. The table is arranged in order by increasing atomic number.

13. Atomic Number=
# of protons=
# of electrons
Remember: APE
Mass Number=
# of protons +
# of neutrons
Remember: MAN

14. 4 Steps to Determining the Number of Protons, Electrons, and Neutrons
Look up the givens on the periodic table: atomic number & mass number (Hint: this is the decimal--round the number to a whole number)
Fill in the number of protons and electrons (Hint: same as the atomic #)
Mass #- atomic #= # of neutrons
Check your math. A=P=E & the protons & neutrons should=mass #
4 Steps to Determining the Number of Protons, Electrons, and
Neutrons

15. Bellwork:
Pick up handouts.
Grab scissors, glue, & map pencils.
Have your notes on your desk.
Start cutting.

16. History of The Periodic Table
Originally proposed by Dmitri Mendeleev (1869)
Grouped elements according to their atomic mass, as he did he noticed that families had similar chemical properties.
Changes made by Henry Moseley (1914)
Organized table by atomic number.
–Columns then contained elements with similar properties
This is what we follow today!
History of The Periodic Table

17. Getting to Know The Families vs. Periods
Families/Groups
are the vertical columns (up & down).
There are 18 families.
They are grouped because they have similar properties & the same # of valence electrons.
Periods
are the horizontal rows (left to right).
There are 7 periods.
They are grouped because they have the same # of electron orbitals. They do not share similar properties
Getting to Know The
Families vs. Periods

18. Important Families to Know Periodic Table Song
Alkali Metals
Group 1A. Is the most reactive group.
Always bonded with other elements.
Elements: Li, Na, K, Rb, Cs, Fr
Alkaline Earth Metals
Group 2A. Never found freely in nature.
Found in foods.
Elements: Be, Mg, Ca, Ba
Halogens
Group 17/7A. The most active non-metals. Bond with alkali metals.
Elements: F, Cl, Br, I
Noble Gases
Group 18/8A. Stable elements that exist on their own. (Small amts.)
Elements: He, Ne, Ar, Kr, Xe

20. Take 5 minutes and see if you can answer these questions.
Let me know when you are ready to check your answers.

21. Time to color! Cut out. Glue into the correct column. 5 minutes!
Color the METALS some shade of GREEN!
Color the METALLOIDS YELLOW!
Color the NON-METALS some shade of pink.
Time to color!
Cut out.
Glue into the correct column.
5 minutes!

22. Metals •Metals are good conductors of heat and electricity.
•Metals are shiny.
•Metals are ductile (can be stretched into thin wires).
•Metals are malleable (can be pounded into thin sheets).
•Metals are corrosive. (A chemical property of metal is its reaction with water)
Metals

23. Non- Metals •Non-metals are poor conductors of heat and electricity.
•Non-metals are not ductile or malleable.
•Solid non-metals are brittle and break easily.
•They are dull.
•Many non-metals are gases.
Non- Metals

24. •Metalloids (metal-like) have properties of both metals and non-metals.
•They are solids that can be shiny or dull.
•They conduct heat and electricity better than non- metals but not as well as metals.
•They are ductile and malleable.
Metalloids

25. # of Electrons Each Level Can Hold
The electrons found in the outermost energy level used for bonding.
The Bohr model shows the location of ALL electrons in the different energy levels.
Valence Electrons
# of Electrons Each Level Can Hold
1st Level
2 electrons
2nd Level
8 electrons
3rd Level