1. To get: Chromebook- Log into Classroom
To get out: Yellow Packet- Turn to pg 5- Introduction to chemistry
To Turn In: Observing Living Organisms Lab
(safety contract, info sheet)
Homework: Read pg (underline/highlight as you read and answer questions 1-8)

2. CHEMISTRY!?!!

3. Chemical Terms- Pg 5 Matter- anything that occupies and has
The “stuff” of the universe
All chemicals are matter just like all matter is basically chemical
Space
Mass

4. What makes up Matter? Atoms!
Atom- The smallest possible of an element that still has the properties of that element. Made of 3 particles: Proton- A subatomic particle in the nucleus with a single positive charge Neutron- A subatomic particle in the nucleus with a neutral charge Electron- A subatomic particle that quickly moves around the nucleus with a single negative charge little mass.
unit

5. **The proton and neutron together form the (atomic) nucleus.

6. Chemical Terms
Element- a pure substance made of the same types of atoms that cannot be broken down into other substances by chemical means.
Compound- a substance containing two or more elements that are chemically combined
A great example is WATER
Water is made of 2 Hydrogen atoms and 1 Oxygen atom (H2O)

7. Every element has a symbol containing 1 or 2 letters
Ex: Carbon = _________ Sodium= ________
Hydrogen= _________ Chlorine= _______
Oxygen = ________ Calcium= ________
Nitrogen= _________ Phosphorus= ________
Use the chart to fill in the symbols for each element.

8. Atomic Number: The # of in the nucleus—
different for each element.
protons

9. In a neutral uncharged atom, the # of protons = # of electrons
What is the charge on an atom with:
8 protons and 10 electrons? -2

10. What is the charge on an atom with
4 protons and 2 electrons? +2

11. Quick Review- Quiz on Google Classroom
What is the smallest unit of an element?
Where are Protons found?
What is the charge of a proton?
Where are Electrons found?
What is the charge of an electron?
What is the charge of an atom that has 5 protons and 6 electrons?

12. Electrons are arranged in energy levels (also called Orbitals or Electron Shells)
The number of Valence Electrons, electrons in the outer electron shell, determines how reactive an element is.
Atoms are most reactive when the outer shell is partially full (Atoms "want" to have a full outer shell!)

13. # of Electrons each energy level can hold:
1st Energy Level: 2 Electrons
2nd Energy Level: 8 Electrons
3rd Energy Level: 8 Electrons

14. Drawing a Bohr Model
Oxygen: Atomic #8
# Valence e-=
+ Vacanices= 6 2

15. Draw a Bohr model of Magnesium Atomic # 12
# Valence e-=
+ Vacanices= 2 6

16. Chemical Bonding
Atoms interact such that they all try to have 8 electrons in outermost orbit (energy level)
The attractive forces between atoms in a compound are chemical bonds 11

17. Chemical Bonding Vocab:
Molecule: A particle with 2 or more atoms bonded together
Compound: Molecule with at least 2 different elements. They can have very different properties from the elements that make them up.

18. An example:  Chlorine is a greenish gas while sodium is a soft, shiny metal.  When the two are combined, white sodium chloride (table salt) is made
NaCl

19. Chemical Bonding
Covalent Bonds - Two atoms share one or more pairs of electrons
Each ends up with 8 electrons in its outermost energy level (at least part of the time) 11

20. Draw a Covalent Bond
Hydrogen
Hydrogen + H H

21. Chemical Bonding
Ionic Bonds - One atom loses electrons; the other gains electrons
Ions: any atom/molecule with
Charge (positive or negative) 11

22. Chemical Bonding Atom that loses electrons has a net positive charge
Atom that gains electrons has a net negative charge
Unlike charges attract
An ionic bond is then formed from the attraction between the positive charge and negative charge 11

23. Sodium Chloride (NaCl)
Draw an Ionic Bond:
Sodium Chloride (NaCl)
Sodium (atomic number 11)
Chlorine (atomic number 17)