1. Chapter 5-The Structure of Matter
Molecules and Compounds
Ionic and Covalent Bonding
Naming Compounds

2. Compounds and Molecules

3. Remember from Chapter 2…
A compound is a substance made of atoms of two or more different elements that are chemically combined by chemical bonds
Mixtures are made of different substance that are just placed together; each substance in the mixture keeps its own properties

4. What is a chemical bond?
An attractive force between the nuclei and valence electrons of different atoms that binds them together
Bonds form in order to…
decrease potential energy (PE)
increase stability

5. Ne Stability Stability is the driving force behind bond formation!
Octet Rule
most atoms form bonds in order to have 8 valence e-
full outer energy level
like the Noble Gases! Ne
Stability is the driving force behind bond formation!

6. Becoming Stable
All neutral atoms want to be stable like a noble gas
They either GAIN or LOSE electrons
CATION: Positively Charged
ANION: Negatively Charged Na Cl =
Loses electron; becomes +
Gains electron; becomes -

7. Becoming Stable
CATIONS: Have more positive charge than negative, they LOSE electrons
ANIONS: Have more negative charge than positive, the GAIN electrons Na Cl =
Loses electron; becomes +
Gains electron; becomes -

8. What’s the charge? The charge on an ion.
Indicates the # of e- gained/lost to become stable. 1+ 4- 2+ 3+ 4+ 3- 2- 1-

9. Stability
Transferring e-
Sharing e-

10. Ionic and Covalent Bonding

11. Covalent Bonds
Nonmetal + Nonmetal
Bonds form by SHARING ELECTRONS

12. Ionic Bonds
Metal + Nonmetal
Bonds form by TRANSFERRING ELECTRONS

13. What’s the charge? The charge on an ion.
Indicates the # of e- gained/lost to become stable. 1+ 4- 2+ 3+ 4+ 3- 2- 1-

14. How do ions bond? +1 -1 Review: cations + anions
What is the ionic charge of Na? +1
What is the ionic charge of Cl? -1
The final compound MUST be neutral!!

15. Continued… Na+1 + Cl-1 = NaCl (neutral) Cs+1 + O-2 = Cs2O (neutral)
Metals
Non metals
Na+1 + Cl-1 = NaCl (neutral)
It takes 1 positive Na to balance the 1 negative Cl
Cs+1 + O-2 = Cs2O (neutral)
It takes 2 positive Cs to balance the 1 negative O
We use the subscripts to depict how many atoms of each element must be used for the compound

16. Crossing Charges Na+1 + Cl-1 Na Cl = NaCl
Switching the superscripts to make new subscripts also works:
Na+1 +
Cl-1 Na Cl =
NaCl

17. Try these…
Cs+1 + O-2 =
Mg+2 + S-2 =
Be+2 + N-3 =

18. Not all ions are single elements:
Different ions
Not all ions are single elements:
We’ve seen some ions made of single elements, but…
Some are made of more than a single element (polyatomics)
SO4-2
CO32-
OH-
NO3-
More than 1…atom

19. Naming binary ionics (nomenclature)
Write the name of the cation (metal), just the way it is
Write the name of the anion (non metal), change the ending to “ide”
Nitrogen – nitride
Oxygen – oxide
Chlorine – chloride
Carbon - carbonide

20. Name the following compounds:
Lets practice…!!
Name the following compounds:
MgCl
CaBr2
CaO
SrF2

21. Give compound formulas for the following:
Let’s practice more…!!
Give compound formulas for the following:
Potassium iodide
Aluminum sulfide
Sodium chloride
Magnesium nitride

22. Naming compounds with polyatomic anions
Write the name of the cation (metal), just the way it is
Isolate the polyatomic anion – determine its name
Write the name of the polyatomic anion, just the way it is
The ones to the right are the
ones you need to know

23. Name the following compounds:
Let’s practice…!!
Name the following compounds:
Ca(OH)2
Na2(CO3)

24. What about polyatomics that look similar, but are different
Most polyatomic look very similar, but have different numbers of oxygens
SO3 and SO4
Is a trick to it
Hypo – “little”
Ite
Ate
Hyper – “lots”

25. That’s right, more practice…!!
Name the following compounds:
Na (ClO3)
Na(C2H3O2)
Mg3(PO4)2
Ca(SO4)
Mg(OH)2
Na(NO3)

26. Stock system of nomenclature
For transition metals…
Some transition metals carry more than one charge
Ex: Fe+1, Fe+2, Fe+3…Cu+1, Cu+2
Is depicted with Roman numerals
Ex: Fe+2 – Fe(II), Fe+3 – Fe(III)
Ex: Cu+2 – Cu(II), Pb+3 – Pb(III)
Some metals always have a definite charge
Al+3, Zn+2, Ag+1

27. Stock system of nomenclature
For transition metals…
Transition metals charge can change so it is always written in the name.
Example: Copper (II) Chloride
Cu+2 +
Cl-1 Cu Cl =
CuCl2

28. Practice with transitions…!!
Name the following compounds or give formulas:
Copper (II) oxide
CuBr2
Tin (IV) iodide
FeS
Iron (II) chloride
Fe2O3

29. Let’s practice…!!
NaI
K2O
Ca(OH)2
CaCl2
Na(NO3)
K2S
Ca3(PO4)2
KClO3

30. Covalent Bonds
Nonmetal + Nonmetal
Bonds form by SHARING ELECTRONS

31. Covalent Bonds
Electrons are shared from the valence shell, still want it full!
But electrons are not always shared equally…
When two Chlorine atoms bond, electrons are equally attracted to the positive nucleus of each atom---NON- POLAR Covalent bond
When not shared equally-Polar Covalent bond

32. What makes a Covalent Bond
Non-metal + non-metal
Some examples below
Can share more than one pair of electrons
single bond shares one pair electrons
double bond shares two pairs electrons
triple bond shares three pairs electrons

33. Naming Covalent Compounds
Covalent compounds have different rules than ionic compounds
Prefixes are only used for the first atom if it is more than one
Second element is named using a prefix to indicate how many
Second element’s name ending is changed to “ide”
The “a” and “o” at the end of the prefix is dropped when used in the name, followed by a vowel

34. Naming Covalent Compounds
Write the more metallic element first.
Add subscripts according to prefixes.

35. Covalent Bonds
Two nonmetal atoms form a covalent bond because they have less energy after they bonded
H H H : H = HH = H2
hydrogen molecule

36. Diatomic Molecules Gases that exist as diatomic molecules
Are: Br2, I2 , N2, Cl2, H2, O2, F2
octets
       
 N   N   N:::N
 
triple bond

37. Molecular Formulas
The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2

38. Learning Check
Use the name of the element to name the following diatomic molecules.
H2 hydrogen
N2 nitrogen
Cl2 _______________
O2 _______________
I2 _______________

39. Solution
Use the name of the element to name the following diatomic molecules.
H2 hydrogen
N2 nitrogen
Cl2 chlorine
O2 oxygen
I2 iodine

40. Naming Binary Covalent Compounds
Two nonmetals
Name each element
End the last element in -ide
Add prefixes to show more than 1 atom (don’t use mono on first element but use all others)
Prefixes
mon penta 5
di 2 hexa 6
tri 3
tetra 4

41. Learning Check
Fill in the blanks to complete the following names of covalent compounds.
CO carbon ______oxide
CO2 carbon _______________
PCl3 phosphorus _______chloride
CCl4 carbon ________chloride
N2O _____nitrogen _____oxide

42. Solution CO carbon monoxide CO2 carbon dioxide
PCl3 phosphorus trichloride
CCl4 carbon tetrachloride
N2O dinitrogen monoxide

43. Learning Check A. P2O5 1) phosphorus oxide 2) phosphorus pentoxide
3) diphosphorus pentoxide
B. Cl2O7 1) dichlorine heptoxide
2) dichlorine oxide
3) chlorine heptoxide
C Cl2 1) chlorine
2) dichlorine
3) dichloride

44. Solution A. P2O5 3) diphosphorus pentoxide
B. Cl2O7 1) dichlorine heptoxide
C Cl2 1) chlorine

45. Some examples… Give the name for As2O5 SO3 ICl3 PBr5
Two arsenic atoms as indicated by the subscript – “di”
Five oxygen atoms as indicated by the subscript – “penta”
Diarsenic pentoxide
Notice the oxygen changes to oxide
SO3
ICl3
PBr5
Sulfur trioxide
Iodine trichloride
Phosphorous pentabromide

46. Try these… CI4 PCl3 N2O3 P2O3 CSe2 S2Cl2 Carbon tetriodide
Phosphorous trichloride
Dinitrogen trioxide
Diphosphorous trioxide
Carbon diselinide
Disulfur dichloride

47. Let’s try it backwards…
Phosphorus pentabromide
Sulfur trioxide
Trinitrogen pentachloride
PBr5
SO3
N3Cl5

48. Naming Acids
Honors Only

49. Definition Acid Compound that forms H+ in water.
Formula usually begins with ‘H’.
Examples:
HCl, HNO3, H2SO4

50. Acid Names

51. Acid Names HBr H2CO3 -ide  hydrobromic acid H2SO3 -ate
 carbonic acid
-ite
 sulfurous acid

52. Acid Formulas hydrofluoric acid sulfuric acid nitrous acid -ide  HF
-ate
 H2SO4
-ite
 HNO2