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

2. Atomic Theory & Bonding
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

3. 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-
Atoms can join together to form MOLECULES.
The oxygen molecules are O2
COMPOUNDS are made up of several (2+)atoms
Hydrogen and oxygen are atoms/elements
H2O is a compound

4. 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

5. 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)

6. 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
Periods are horizontal rows on the periodic table

7. 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

8. 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

9. - +

10. 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”

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

12. 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+

13. 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

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

16. 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?

17. 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

18. 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

19. 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!

20. 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!

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

22. Bonding Types:
When two atoms get close together, their valence electrons interact.
Recall that Ions form by the atom gaining or losing electrons to “fill or empty” the valence.
Metal Elements (left) “want” to lose electrons and Non-Metal Elements “want” to gain electrons
So if two Non-Metals meet at a bar?... but really, they both want more electrons so they make an agreement to SHARE and then they are both happy.

23. Bonding Types: Covalent Bonds: Formed between two or more non-metals
Electrons are shared between atoms
Hydrogen
Fluorine +
Electrons are shared
Hydrogen fluoride

24. Bonding Types:
When two atoms get close together, their valence electrons interact.
Ok so what if two metals walk into a bar? Well there would be a bar fight between the metals!
Metals “need” to get rid of electrons and there would be no way for them to strike a mutual deal
BUT if a Metal were to meet a Non-Metal at the bar it would be love at first sight. Well not quite, but they would be able to make each other happy since one “wants” to gain and the other “wants” to lose electrons

25. Electrons are transferred from the cations to the anion
Ionic Bonds:
Metals give electrons to non-metals (transfer of electrons)
cations (+ ions) and anions (- ions) form
For example, lithium and oxygen form an ionic bond in the compound Li2O
Lithium
Oxygen +
Electrons are transferred from the cations to the anion
Li+ O2- Li+
Lithium oxide,
Li2O

26. Lewis Diagrams: Like simplified Bohr diagrams
Only valence electrons are shown
Dots representing electrons are placed around the element symbols (on 4 sides, imagine a box around the symbol)
Electron dots are placed singularly, until the fifth electron is reached, then they are paired.
Example: Nitrogen atom

27. Lewis Diagrams:
Note: the Lewis diagrams are the same (except for the symbols) for elements in the same family because they have the same number of valence electrons

28. Lewis Diagrams for Ions:
For positive ions: one electron dot is removed from the valence shell for each positive charge of the ion.
For negative ions: one electron dot is added to each valence shell for each negative charge of the ion.
Square brackets and the charge are placed around each ion
Example: Nitrogen ion

29. Lewis Diagrams For Covalent Bonds:
valence electrons are drawn to show sharing of electrons.
Remember: All atoms “like” to have a full valence shell
The shared pairs (“bonding pairs”) of electrons are usually drawn as a straight line
“lone pairs” are the electrons not shared

30. Lewis Diagrams For Ionic Bonds:Be Cl
• •
• •
Each beryllium has two electrons to transfer away, and each chlorine wants one more electron
• •
• •
Since Be2+ wants to donate 2 electrons and each Cl– wants to accept only one, two Cl– ions are necessary
The ionic compound Beryllium chloride is formed 2+ –

31. Online Quiz via Classroom before next class!