1. Atomic Theory Review Basic Atomic Structure: A Look Inside the Atom
Watch the Video Linked above Before starting these notes.

2. Assessment – Criterion Based
(0)
Beginning (1)
Developing (2)
Accomplished (3)
Exemplary (4)
<50%
50-65%
65-75%
75-90%
90-100%
I have not achieved a standard described by any of the descriptors to the right.
I am able to:
state scientific knowledge
apply scientific knowledge and understanding to suggest solutions to problems set in familiar situations
interpret information to make judgments.
outline scientific knowledge
apply scientific knowledge and understanding to solve problems set in familiar situations
interpret information to make scientifically supported judgments.
describe scientific knowledge
apply scientific knowledge and understanding to solve problems set in familiar situations and suggest solutions to problems set in unfamiliar situations
analyse information to make scientifically supported judgments.
explain scientific knowledge
apply scientific knowledge and understanding to solve problems set in familiar and unfamiliar situations
analyse and evaluate information to make scientifically supported judgments.

3. Learning Outcomes for this Section
“B” (Beginning), “D” (Developing), or “A” (Accomplished) based on your level of understanding. Outcomes with * indicates that this is an “E” (Exemplary) goal (>90%)
KNOW B D A
LEARNING OUTCOME
I can explain how matter is classified (vocab: atom, ion, molecule, compound)
I can describe the structure of an atom (nucleus, electron, proton, neutron)
I can tell you all of the diatomic elements * as well as S8 & P4
I can describe trends in the periodic table (# of valence electrons, size, reactivity) DO
I can calculate the number of neutrons, electrons, or protons in an atom
I can calculate the number of neutrons, electrons, or protons in an ion if given the ion charge
I can calculate the number of neutrons, electrons, or protons and can explain ion charge and how this relates to its properties
I can draw & label the structure of an atom or ion (vocab: proton, electron, neutron, nucleus, energy shells)
I can classify an element as a metal, non-metal, or metalloid

4. Atomic Theory & The Periodic Table
What is an Atom?
smallest particle of an element that still has the properties of that element
An atom = proton(s) & electron(s) & neutron(s) (PEN)
Fun Fact:
50 million atoms, lined up end-to-end = 1 cm

5. An ELEMENT is made up of one type of atom
The element, oxygen, is O
IONS are atoms with a charge.
The ion of oxygen is O2-

6. 8 Elements that are never found alone form Diatomic MOLECULES.
H2, N2, O2, F2, Cl2, Br2, F2, H2
Make Up Your Own Acronym. You will need to know these

7. COMPOUNDS are made up of several (2+)atoms
Hydrogen and oxygen are atoms/elements
H2O is a compound

8. Classification of Matter
Mixture
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent

9. Classification of Matter
Mixture
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
Has mass and volume
Exists in 3 states; solid, liquid, gas
Annotate
Draw
Examples

10. Classification of Matter
Mixture
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
made of only one type of atom or only one type of molecule
Unique physical and chemical properties

11. Classification of Matter
Mixture
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
made up of two or more different substances
the physical combination in which the identities are retained
*mixed in the form of solutions, suspension and colloids.

12. Classification of Matter
Mixture
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
Made up of many identical molecules
Each molecule contains more than one type of atom
There are a specific number of each atom in each molecule
Atoms are joined by chemical bonds

13. Classification of Matter
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
Two of the SAME elements bonded to form a Molecule
The bond is covalent
They never occur naturally alone
*this has nothing to do with how they combine with other elements in compounds

14. Classification of Matter
Pure Substance
Element
Diatomic Elements
Compound
Ionic
Covalent
Chemical bond resulting from transfer of electrons
+ and – ions attracted to each other
metal + and non-metal -
Chemical bond resulting from sharing of electrons
Atoms attached to each other
Non-metals only

15. Electrons (negative charge) exist in the space surrounding the nucleus
Structure of an Atom:
The nucleus is at the centre of an atom
composed of protons (positive charge) and neutrons (neutral charge)
Electrons (negative charge) exist in the space surrounding the nucleus

16. area surrounding the nucleus
Subatomic Particles:
Atoms are made up of smaller particles known as sub-atomic particles.
Name
Symbol
Charge
Location
Atomic Mass
Proton p 1+
nucleus
1 AMU
Neutron n
Electron e 1–
area surrounding the nucleus
1/1836 (0)

17. Families of the Periodic Table:
Columns of elements are called groups, or families
All elements in a family have…
similar properties
bond with other elements in similar ways
have the same number of valence electrons
Family names (on the periodic table!):
Group 1 = alkali metals
Group 2 = alkaline earth metals
Group 17 = the halogens
Group 18 = noble gases

19. Periods on the Periodic Table
Periods are horizontal rows on the periodic table.
Have the same number of electron “shells” (row 1 =1, row 2 = 2….)
Do you remember
how many electrons
can fit in each shell?

20. Where are the following?
INCREASING REACTIVITY
Where are the following?
Atomic Number
Period
Group/Family
Metals
Non-metals
Transition metals
Metalloids
Alkali metals
Alkaline earth metals
Halogens
Noble gases

21. Periodic Table & Ion Formation:
Atoms gain and lose electrons to form ions
Metals lose electrons & become positive ions (cations)
Some metals can have more than one charge (multivalent)
ie. Iron, Fe, loses either 2 (Fe2+) or 3 (Fe3+) electrons
Non-metals gain electrons & become negative ions (anions)
Atoms do this in an attempt to have the same number of valence electrons as the nearest noble gas – to become stable

22. - +

23. Numbers to Remember :
Atomic number = # of protons = # of electrons in atoms In ATOMS: # of protons = # of electrons in every atom AND ONLY IN ATOMS!!! (not ions) *this keeps the atom neutral since protons are (+)ive and electrons are (-)ive
Positive Ions
Metals generally form positive Ions
They have only a few electrons in their valence so they tend to lose electrons to be “happy”
Negative Ions
Non-Metals generally form negative Ions
They have almost a full valence so they tent to gain electrons to be “happy”

24. Try These: Element Atomic Number # of Protons # of Electrons Charge
Carbon atom
Nitrogen atom
Nitrogen Ion
Calcium atom
Calcium Ion
Phosphorous atom
Phosphorous Ion

25. Try These: Element Atomic Number # of Protons # of Electrons Charge
Carbon atom 6
Nitrogen atom 7
Nitrogen Ion 10
+7 + (-10) = -3
Calcium atom 20
Calcium Ion 18
+20 +(-18) =2+
Copper 29
Copper Ion
? multivalent
Cu1+ =28
Cu2+ = 27 1+ 2+

26. You are doing Great! Lets Keep Going
Mass Number = The mass number is the ACTUAL mass of 1 atom
= #Protons + # Neutrons (since both have mass)
Atomic Mass = This is AVERAGE mass of the ISOTOPES of an element
Found on the periodic table and generally has a decimal.
This would be impossible in realty since the mass of an atom comes from protons and neutrons that each weight 1amu and you can’t have part or a proton or neutron BUT it is also impossible to take a sample of an element and have only 1 atom! That same will contain many atoms and will contain a variety of the isotopes of the atoms of that element!
Isotope = Same element (same atomic number / # of protons)
= Different mass number because Different # of NEUTRONS

28. Don’t confuse this with what you see in each box of the periodic table

29. Practice:
Determine the number of protons neutrons and electrons for the symbol above?
If an element has 15 protons 17 neutrons and 18 electrons, write is isotope notation below?

30. Practice:
Determine the number of protons neutrons and electrons for the symbol above?
Protons = 29 (bottom number is atomic number)
Neutrons = 35 (64-29 = 35 since top number is mass number)
Electrons = 29 ( no charge was indicated for P = e- )
If an element has 9 protons 10 neutrons and 10 electrons, write is isotope notation below? -1

31. If you are confused – Video Links Below
Difference between Mass Number and Atomic Mass
Isotopes Explained
Isotope Notation and Practice
Otherwise Watch this before Moving on
Valence Electrons and the periodic Table

32. Bohr Diagrams:
Bohr diagrams show how many electrons appear in each electron shell around an atom.
Each shell holds a maximum number of electrons (2, 8, 8, 18, 18)
Electrons in the outermost shell are called valence electrons
Except for the transition elements, the last digit of the group # = # of valence electrons
Note: Think of the shells as being 3D like spheres, not 2D like circles!

33. Bohr Diagrams What element is this?
It has = 18 electrons, and therefore 18 protons
It has 8 electrons in the outer (valence) shell
18 p
22 n
Argon!

34. Bohr Diagrams for the first 20 elements
Note: The noble gas elements have full electron shells, and are very stable.

35. Annotate your Periodic Table Assignment