1. Chemical Compounds
Honors Chemistry

2. Metals Nonmetals Location: to the right of the staircase
Location: to the left of the staircase
Ion formation – tend to lose electrons resulting in positive charges
Nonmetals
Location: to the right of the staircase
Ion formation – tend to gain electrons resulting in negative charges

3. The Periodic Table +1 +3 -3 -2 -1 +2

4. Memorize!!!

5. a. Binary Compounds – only monatomic ions in compound sodium chloride
Ionic Compounds – look at charges; roman numerals needed for elements with more than one charge (polyvalent)
a. Binary Compounds – only monatomic ions in compound
sodium chloride
magnesium nitride
iron(III) sulfide
copper(I) oxide

6. Ionic Compounds
Binary Compounds
HF(g)
AlCl3
FeS
Cr2O3

7. Ionic Compounds
Ternary Compounds – contain 1/more polyatomic ions in compound
sodium carbonate
chromium(III) oxalate
ammonium sulfate

8. Note for polyatomic ions:
Ionic Compounds
Ternary
Co3(AsO4)2
CuSO3
Note for polyatomic ions:
-ate vs. –ite
per- and hypo-

9. 1 extra oxygen ClO4-1 perchlorate ClO3-1 chlorate 1 less oxygen
Anion
Description
Example
1 extra oxygen
ClO4-1
perchlorate
per_____ ate
ClO3-1
chlorate
the most common form
_______ate
1 less
oxygen
ClO chlorite
_______ ite
2 less
oxygens
ClO-1
hypochlorite
hypo_____ ite

10. Now try these…
sulfite
periodate
phosphite
bisulfite

11. Check for Understanding
magnesium hydride
calcium acetate
FeS2O3
SnI4

12. Salts
Ionic compound composed of a cation (positive ion) and an anion (negative ion) from an acid
NaCl
CaSO4
NaHCO3
NaHSO3

13. Hydrates – ionic compound with water bonded in its structure
anhydrate . xH2O
anhydrate  ionic compound
add prefix to indicate # of water molecules
CuSO4 . 5H2O
copper(II) sulfate pentahydrate

14. Hydrate Practice Ni(CH3COO)2  4H2O FeCl3  6H2O
lead (II) carbonate monohydrate
barium chloride dihydrate

15. Molecular Compounds – formed between 2 nonmetals
*Use prefixes
mono = 1 hexa = 6
di = 2 hepta = 7
tri = 3 octa = 8
tetra = 4 nona = 9
penta = 5 deca = 10
Binary Compounds: only 2 elements in the compound; use prefixes and –ide ending
CCl4
N2O5

16. More Practice
dihydrogen monoxide
nitrogen tetrabromide
S2O6

17. Acids – compounds that produce hydrogen ions in water
Mineral Acids
Binary Acids
1st word: prefix = hydro
root formed from anion
suffix –ide changed to -ic
2nd word: acid
HCl(aq)
HBr(aq)

18. Oxyacids 1st word: root from anion Suffix ate changed to ic
Suffix ite changed to ous
**Exceptions: if you have sulf or phos as roots, change the root to sulfur or phosphor
2nd word: acid
HNO3
HNO2
phosphorous acid

19. Organic Acids 1st word: root formed from anion
Suffix ate changed to ic
2nd word: acid
C6H5COOH(aq)
or HC6H5COO(aq)
acetic acid

20. Common Acids to Know HCl H2CO3 HClO4 H2SO4 H3PO4 HNO3
CH3COOH = HC2H3O2

21. Hydrocarbons
Saturated Hydrocarbons: compounds that contain all single bonds
Alkanes: each carbon is bonded to 4 atoms
aka paraffin series
Only contain single bonds
Molecular formula:
CnH2n+2

23. Unsaturated Hydrocarbons
Compounds that contain at least
one double bond or triple bond
Alkenes: compounds that contain a double bond
aka: olefins
Skeleton: C=C
Molecular formula = CnH2n

24. Unsaturated Hydrocarbons
Alkadienes: compounds that contain 2 double bonds
(C=C-C-C=C)
Alkatrienes: compounds that contain 3 double bonds
(C=C-C=C=C)
Conjugated alkenes: double bonds are alternating
(C=C-C=C-C)
Lycopene

25. Unsaturated Hydrocarbons
Alkynes: compounds that contain a triple bond
Hybridization: sp (linear)
Skeleton: CC
Molecular formula = CnH2n-2

26. Naming Alkanes (IUPAC)
Find the longest chain of carbon atoms. Choose the base name that describes the number of carbon atoms in this chain, with the ending -ane
# C atoms
Stem 1
meth 9
non 2
eth 10
dec 3
prop 11
undec 4
but 12
dodec 5
pent 13
tridec 6
hex 14
tetradec 7
hept 15
pentadec 8
oct 16
hexadec

27. Naming Alkanes (IUPAC)
Number the carbon atoms in this longest chain beginning at the end nearest the 1st branching.
If there is branching at equal distances from both ends of the longest chain, begin numbering at the end nearest the branch that is 1st in alphabetical order. 1 2 3 4

28. Naming Alkanes (IUPAC)
Assign the name (stem with yl ending) & position number to each substituent or branch. Arrange the substituents in alphabetical order.
The hydrocarbon branches are called alkyl groups:
-CH3 methyl -CH2CH2CH propyl
-CH2CH ethyl CH2CH2CH2CH butyl

29. Naming Alkanes (IUPAC)
Use the appropriate prefix to group like substituents: di = 2, tri = 3, tetra = 4, etc. Do not use these prefixes when alphabetizing attached groups
Write the name as a single word. Use hyphens to separate numbers & letters and commas to separate numbers. Do not leave any spaces.

30. Naming Organic Halides (Alkyl Halides)
The organic halides are named as halo- derivatives of the parent hydrocarbon. The prefix can be fluoro-, chloro-, bromo- or iodo-.

31. Naming Alkenes
Locate the carbon atoms in the longest carbon chain that contains the double bond. Use the stem with the ending –ene.
Number the carbon atoms of this chain sequentially, beginning at the end nearer the double bond. If the parent chain has more than 3 carbons, insert the number describing the position of the double bond (indicated by its 1st carbon location) before the base name.

33. Naming Alkenes
In naming alkenes, the double bond takes positional precedence over substituents on the carbon chain. The double bond is assigned the lowest possible number.

34. Alkene Examples

35. Alkene Examples

36. These are called stereoisomers
Naming Alkenes
Consideration must be given to compounds with different arrangements of groups on opposite sides of a double bond. This is known as geometric isomerism.
cis – adjacent to or same side
trans – opposite side
cis-2-butene
These are called stereoisomers
trans-2-butene

37. Alkene Examples

38. Naming Alkynes
Named just like the alkenes except the suffix –yne is added

39. Alkyne Examples

40. Diffusion and Effusion
Diffusion: the mixing of molecules of 2 or more gases due to their molecular motion (spontaneous)
Effusion is the movement of gas atoms or molecules through a small opening. Gases confined in a container randomly pass through a tiny opening in the container.
ex) hole in a tire; soda bottle (CO2 escaping)

41. Graham’s Law: The rate of effusion of a gas is inversely proportional to the square root of its molar mass.
He and SF6 demo