Transcript Chemical Compounds Powerpoint

Chemical
Compounds
Honors Chemistry
Metals
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
The Periodic Table
+1
+2
+3
0
-3
-2 -1
CATION
“cat”ion
ca+ion
ANION
“ant”ion
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
Ionic Compounds
Binary Compounds
HF(g)
AlCl3
FeS
Cr2O3
Ionic Compounds
Ternary Compounds – contain 1/more
polyatomic ions in compound
sodium carbonate
chromium(III) oxalate
ammonium sulfate
Ionic Compounds

Ternary
Co3(AsO4)2
CuSO3
Note for polyatomic ions:
-ate vs. –ite
per- and hypo-
Anion
Description
Example
per_____ ate
1 extra
oxygen
ClO4-1
perchlorate
_______ate
the most
common form
ClO3-1
chlorate
_______ ite
1 less
oxygen
ClO2-1
chlorite
hypo_____ ite
2 less
oxygens
ClO-1
hypochlorite
Now try these…
 sulfite
 periodate
 phosphite
 bisulfite
Check for Understanding
 magnesium
 calcium
 FeS2O3
 SnI4
hydride
acetate
Salts
 Ionic
compound composed of a cation
(positive ion) and an anion (negative
ion) from an acid
 NaCl
 CaSO4
 NaHCO3
 NaHSO3
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
Hydrate Practice
 Ni(CH3COO)2
 FeCl3
 lead
 4H2O
 6H2O
(II) carbonate monohydrate
 barium
chloride dihydrate
Molecular Compounds –
formed between 2 nonmetals
*Use prefixes
mono = 1
di = 2
tri = 3
tetra = 4
penta = 5
hexa = 6
hepta = 7
octa = 8
nona = 9
deca = 10
Binary Compounds: only 2 elements in the
compound; use prefixes and –ide ending
CCl4
N2O5
More Practice
 dihydrogen
 nitrogen
 S2O6
monoxide
tetrabromide
Acids – compounds that
produce hydrogen ions in water
1.
Mineral Acids
Binary Acids
1st word:
prefix = hydro
root formed from anion
suffix –ide changed to -ic
2nd word:
acid
a.
HCl(aq)
HBr(aq)
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
Organic Acids
 1st
word: root formed from anion
Suffix ate changed to ic
 2nd word: acid
C6H5COOH(aq)
or HC6H5COO(aq)
acetic acid
Common Acids to Know
 HCl
 H2CO3
 HClO4
 H2SO4
 H3PO4
 HNO3
 CH3COOH
= HC2H3O2
Hydrocarbons
Saturated Hydrocarbons:
compounds that
contain all single
bonds
1.
Alkanes: each carbon
is bonded to 4 atoms
– aka paraffin series
– Only contain single
bonds
Molecular formula:
CnH2n+2
Unsaturated
Hydrocarbons
Compounds that contain at least
one double bond or triple bond
Alkenes: compounds that contain a double
bond
1.
•
•
•
aka: olefins
Skeleton: C=C
Molecular formula = CnH2n
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
Unsaturated Hydrocarbons
2.
Alkynes: compounds that contain a triple
bond
–
–
–
Hybridization: sp (linear)
Skeleton: CC
Molecular formula = CnH2n-2
Naming Alkanes (IUPAC)
1.
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
# 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
Naming Alkanes (IUPAC)
Number the carbon atoms in this longest chain
beginning at the end nearest the 1st branching.
2.
•
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
Naming Alkanes (IUPAC)
3.
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
-CH2CH2CH3
propyl
-CH2CH3
ethyl
-CH2CH2CH2CH3
butyl
Naming Alkanes (IUPAC)
4.
Use the appropriate prefix to group like
substituents: di = 2, tri = 3, tetra = 4, etc. Do not
use these prefixes when alphabetizing attached
groups
5.
Write the name as a single word. Use hyphens
to separate numbers & letters and commas to
separate numbers. Do not leave any spaces.
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-.
Naming Alkenes
1.
2.
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.
http://wps.prenhall.com/wps/media/objects/476/488316/index.html
Naming Alkenes
3.
In naming alkenes, the double bond takes
positional precedence over substituents on
the carbon chain. The double bond is assigned
the lowest possible number.
Alkene Examples
Alkene Examples
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-2-butene
cis – adjacent to or same side
trans – opposite side
These are called stereoisomers
trans-2-butene
Alkene Examples
Naming Alkynes
 Named
just like the alkenes except the
suffix –yne is added
Alkyne Examples
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)
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
Effusion =
r1

r2
1
M
M2
M1