1. Putting Atoms Together
Chapter 7

2. Terminology Molecule –
Ex. Air = roughly 80% _______________ molecules, _____ oxygen molecules, and trace amounts of H2O and CO2
two or more atoms of the same or different elements that are chemically joined together in a unit.
nitrogen
20%

3. Terminology
notation that indicates the type and number of atoms in a pure substance
Chemical Formula –
- small numbers written ____________, in chemistry usually indicates a charge 
– small number ___________, tells us how many atoms there are 
Diatomic Elements –
Superscript
above/after
Mg2+
Subscript
below/after
O2 = 2 oxygen atoms
Elements that exist as molecular elements consisting of 2 atoms.

4. * 7

5. Molecular compounds
Sharing is caring!

6. Terminology
What do we call rxn’s that release energy/heat?
What do we call rxn’s that require it?  
Molecular Compounds – Compound consisting of two or more different elements with neutral charges that are bonded together.
Involves two _______________ (includes hydrogen) elements joining together and sharing their ________ electrons to fill their outer __________________ (shell).
non-metal
valence
energy level
A simulation of the reaction: 2H2 + O2   ®    2H2O  

7. hydrogen oxygen valence 2 8 sharing of electrons
Means electrons “LEAN” or migrate towards one molecule creating partial + and - charges
Forces that hold atoms together
Represent “potential” energy
Illustration to the right shows two __________ molecules and a single _______ molecule. Hydrogen wants to have a full ________ shell (first shell can hold a max. of __) meanwhile the oxygen atom also wants to have a full valence shell (2nd shell can hold __). Therefore a ____________________ occurs.
hydrogen
oxygen
valence 2 8
sharing of electrons
2 H O  H2O

8. dependent on arrangement fixed amounts
A key aspect of molecular compounds is the fact they are ______________________ ____ ____________________. Only certain combinations in __________ _______________________ are found in nature.
Ex.
The above example highlights the fact that a change in ______________________________________ dramatically changes the ______________________________________________
dependent on arrangement
fixed amounts
O2 = Oxygen Gas, meanwhile O3 = Ozone
configuration
compound and how it affects us.

9. Bohr-Rutherford Lewis dot diagrams
These molecules can be drawn as __________________________________________ diagrams or as ____________________________________ with the shared pair of electrons represented by a _____, 2 pairs by a ______, or 3 sets of shared electrons by _____. The most that will ever be shared is 3.
Bohr-Rutherford
Lewis dot diagrams

10. Ionic Compounds

11. TERMINOLOGY metal Cation Anion
Compound consisting of a positively charged (cation) and negatively charged (anion) ion.
Def.
Involves a ___________ + a _____________ joining together, with the metal _____________ its ___________ _________ and the __________ taking them.
Def. Ion –_________________________________  2 forms 1.) _________ = Positive 2.) _________ = Negative
metal
non-metal
giving away
valence
electrons
non-metal
a particle that has a + or - charge
Cation
Anion

12. Why does the metal always give away its valence electrons and the non-metal always take them?
Think about this silently (use your notes or textbook as a reference)

13. ANSWER
It is easier for a metal to give up 3 or 4 electrons than try to take enough to fill its valence shell.
For non-metals, they generally only need 1 or 2 extra’s to fill their shells, so it is easier for them to take 2 than give up 6.

14. Sodium Atom, Na Sodium Ion, Na+ Chlorine Ion, Cl- Chlorine Atom, Cl
Sodium Atom, Na
Sodium
Ion, Na+
Chlorine
Ion, Cl-
Chlorine Atom, Cl
+ Charge (Protons)
- Charge (Electron)
Ionic charge

15. Draw Diagram from text (pg. 260) Copy the Bohr-Rutherford
Create a Lewis Dot Diagram

16. Sodium Ion, Na+ Chlorine Ion, Cl-

17. HW  Q 1-8 on page 261

18. Periodic Table Worksheet
REVIEW

19. Metals
1. _______ are located on the left side of the periodic table, with __________ located on the right side. They are separated by a “________” that touches the __________.
2. Horizontal rows are known as ________ and tell us the number of ______ _____ or ______ an element has.
non-metals
staircase
metalloids
periods
Energy levels
shells

20. Families
columns
3. ________ or groups are vertical ________ on the periodic table and tell us how many valence _________ an element has.
4. ATOMS have the same number of Protons as they do ______ _______, so their charge is neutral, this information is detailed in the ______.
electrons
atomic number
charge

21. charge valence electrons cations anions
5. IONS have a positive or negative _______ because they have given up their _______ _________ or taken valence electrons from an atom of another element in order to fill/empty their outer energy shell.
6. Positive ions are known as _______ (think the t looks like a +) while negative ions are called _______ (has two n’s for negative).
valence electrons
cations
anions

22. Magnesium Atom Symbol = Period # = # of energy levels = Group # =
# of Valence Electrons =
Member of the _____________ Family
Draw a Bohr-Rutherford Diagram

23. Lithium Atom Symbol = Period # = # of energy levels = Group # =
# of Valence Electrons =
Member of the _____________ Family
Draw a Lewis-Dot Diagram

24. Argon Atom Symbol = Period # = # of energy levels = Group # =
# of Valence Electrons =
Member of the _____________ Family
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

25. Fluorine Atom Symbol = Period # = # of energy levels = Group # =
# of Valence Electrons =
Member of the _____________ Family
Number of Neutrons =
Draw a Lewis Dot diagram

26. ION REVIEW Neon Helium phosphorus -3
a) An ION of fluorine is going to mimic (look like) an atom of ______.
b) An ION of beryllium is going to mimic an atom of __________________.
c) An ION of ____________ has to gain 3 electrons to mimic argon. Its ionic charge will be ____.
Neon
Helium
phosphorus -3

27. Aluminum
d) An ION of _________ has to give up 3 electrons in order to mimic an atom of neon. Its charge will be ___.
e) An Ion of Oxygen has to ____ ___ electrons to mimic _____. Its ionic charge will be ___. +3
gain 2
neon -2

28. Calcium Atom Symbol = Atomic # = # of Protons = # of Electrons =
Ionic Charge =
Atomic Mass =
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

29. Oxygen ION Symbol = Atomic # = # of Protons = # of Electrons =
Ionic Charge =
Atomic Mass =
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

30. chlorine ION Symbol = Atomic # = # of Protons = # of Electrons =
Ionic Charge =
Atomic Mass =
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

31. aluminum ION Symbol = Atomic # = # of Protons = # of Electrons =
Ionic Charge =
Atomic Mass =
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

32. Potassium ION Symbol = Atomic # = # of Protons = # of Electrons =
Ionic Charge =
Atomic Mass =
Number of Neutrons =
Draw a Bohr-Rutherford Diagram

33. Questions from reading
How do atoms become more stable?
When metals mix with another metal is it called an ________.
When metals mix with non-metals it is called an __________ compound.
What happens with the electrons in these compounds?
When two non-metals mix it is called an ____________ compound.

34. Ionic compounds
Names & Formulas

35. REview metal Cation Anion
Compound consisting of a positively charged (cation) and negatively charged (anion) ion.
Def.
Involves a ___________ + a _____________ joining together, with the metal _____________ its ___________ _________ and the __________ taking them.
Def. Ion –_________________________________  2 forms 1.) _________ = Positive 2.) _________ = Negative
metal
non-metal
giving away
valence
electrons
non-metal
a particle that has a + or - charge
Cation
Anion

36. NAMING
Ionic compounds are easily identified by the presence of a ___________ (first term). Any time you see a metal as the first term, you should automatically be thinking IONIC! Additionally, there is never a __________________ reference in the compound name (so no _________________). The nice thing about naming Ionic molecules is we __________ need to worry about numbers (subscripts).
metal
NUMERICAL
PREFIXES
DO NOT

37. 2 Potassium Oxygen Potassium ox”ide’ Example  K2O
Determine how many elements (each capital letter represents a new element) are present in the compound (_______) and locate them on the periodic table. Is there a metal..? If so it must be a Ionic Compound.
Identify which of the elements is the metal (it must go first). __________________
Identify the non-metal element (it goes 2nd). ____________________
Write the name of the metal, than the name of the non-metal (but change the ending of the non-metal to “IDE”). ___________ _____________ 2
Potassium
Oxygen
Potassium ox”ide’

38. Try these… Li2O MgF2 NaCl K3N CaS Be3P2 LiBr Na2O Lithium oxide
CaS
Be3P2
LiBr
Na2O
Lithium oxide
Magnesium flouride
Sodium chloride
Potassium nitride
Calcium sulphide
Berylium phosphide
Lithium bromide
Sodium oxide

39. WRITING chemical FORMULAS for Ionic Compounds
Since the electrons are ____________ and electrical _______ are present we need to reference the Periodic Table in order to determine how many of each element there is going to be. ____________________________!
given/taken
charges
THE CHARGES MUST BALANCE

40. Step 1: Locate the elements in the Periodic Table- ensure one is a metal, and one is a non-metal. Write down their chemical symbol.
Step 2: Determine the “charge” each element carries when its forms an ionic bond (remember: STABLE)
Step 3: Backcross the “charges“ to SUBSCRIPTS for each element +1 -2
Rb O
Ex.
Rubidium
fluoride +1 -2
Rb O
Rb2O1
“charges it up” _____ _____ 
“backcross it down”

41. Compound Sodium chloride Magnesium nitride Calcium fluoride
Francium phosphide
CHARGE
FORMULA
Na+1 Cl-1
Mg+2 N-3
Ca+2 F-1
Fr+1 P-3
Mg3N2
CaF2
Fr3P
NaCl