1. What are atoms and how are they structured?
Bell Work
Thursday- 9/3
What are atoms and how are they structured?

2. Basic Chemistry Chapter 6 Section 1
5th century BC- Leucippus and Democritus first proposed the idea that all matter us made up of tiny, indivisible particles
1800s- scientists began to collect evidence supporting the existence of atoms
As technology improved, we were able to see that atoms are made up of even smaller particles

3. Atoms Atoms are the building blocks of matter
Three basic sub-atomic particles
PROTONS: positively charge; located in the nucleus
NEUTRONS: neutral; located in the nucleus
ELECTRONS: negatively charged; located outside nucleus

4. Atoms cont.
Atomic structure is a result of the attraction between protons and electrons

5. Atomic Structure Protons and neutrons are contained inside the nucleus
Protons are represented by atomic number
Number of neutrons can be predicted by subtracting the atomic mass from the atomic number and rounding to the nearest whole.
Number of electrons in a neutral atom should equal the number of protons

6. Oxygen Draw electronic configuration Remember energy levels
1st- 2 electrons
2nd- 8 electrons
3rd- 8 electrons

7. Oxygen Second energy level Protons (+ charge) Nucleus
First energy level
Electrons
Neutrons
(no charge)

8. Elements
Pure substances that cannot be broken down into other substances
Organized by characteristics on the Periodic Table

9. Periodic Table
Vertical- Groups
Horizontal- Periods

10. Isotopes
Proton number (atomic number) is equal to the number of electrons, but NEUTRON number can vary.
Atoms of the same element with different neutron numbers are called isotopes.
Changing neutron number can make the atom unstable and cause it to decay. When this happens, the isotope gives off radiation

11. Radioactive Isotopes
Changing the number of neutrons can affect the stability of the nucleus
When a nucleus breaks apart, it gives off radiation
Carbon-14 is a radioactive isotope found in all living things
Calculate age of object by measuring half life
Scientists know the amount of time it takes for half of Carbon-14 to decay
Calculate age by finding out how much Carbon-14 remains
Medical uses- other radioactive isotopes can be injected into a patient to diagnose disease and locate certain types of cancer
Cancer cells have a higher metabolic rate and therefore uptake the radioactive isotopes faster so you can see it in a scan

12. Compounds
A substance formed from two or more elements bonded in a specific ratio
Ex: CO2, NAOH, H2O, H2O2
Cannot be broken down into smaller parts physically; i.e. cannot be individually crushed or torn
Can be broken down chemically
Examples: Salt (NaCl), Water (H2O), Methane (CH4)

13. How many protons, neutrons, and electrons does Sulfur have?
Bell work 9/4
How many protons, neutrons, and electrons does Sulfur have?
Especially this Friday because
FSU football starts TOMORROW!!!

14. Electronic configuration

15. Atomic Structure and Octet Rule
Electrons travel outside the nucleus in energy levels
The first level holds up to two electrons
The second holds up to 8 electrons
The third holds up to 8
Full energy levels are more stable than partially filled ones
Bonds are formed between atoms with unfilled energy levels because unstable atoms tend to bond

16. Chemical Bonds Ionic Covalent
A bond formed when one atom donates one or more electrons to another atom.
Both atoms become charged and are called “ions”
The electrical charges of the atoms attract them to each other
A bond where a molecule is formed by two or more atoms SHARING electrons
Covalent bonds can be single, double, or triple bond depending on how many electrons are shared

17. Covalent Bonds
Two atoms will share one, two, or three electrons. The electrons travel between the electrons shells of both atoms.
Ex: H2O H2 O2
These electrons are shared

18. Covalent bond

19. Ionic Bonds
The atom with fewer electrons will donate to the atom with more electrons.
The atom that receives the electrons becomes negatively charged
The atom that donates the electrons becomes positively charged
The two atoms are attracted to each other, like magnets
Ex: Na+ Cl-

20. Van der Waals Forces
Electrons travel around the nucleus inconsistently.
This leads to temporary positive or negative areas.
When molecules come close together, these temporary positive and negative areas are attracted to each other
This causes molecules to be attracted to each other.
This attraction is known as van der Waals forces.
In water, this causes cohesion, which is the reason water beads together.

21. Carbon

22. Carbon

23. Aluminum

24. Aluminum

25. Potassium

26. Potassium

27. Potassium

28. Bonding
Use electron configuration to explain why Hydrogen and Oxygen bond together.

29. Covalent Bond

30. Bonding
Use electron configuration to explain why Sodium and Chlorine bond together.

31. Ionic Bond