Transcript Exam Review - Chemistry(CHEMISTRY )modified

Chemistry Exam
Review
Binary Ionic Compounds
(metal ion from groups 1 to3)
• contain only two atoms
– one metal + one non-metal
Naming:
1)
2)
3)
name the metal.
then name non-metal and change ending to “ide”
check for multivalent metals (use roman numerals)
** see next slide for details**
Formula:
1)
2)
3)
4)
write symbols (metal first, non-metal second)
write charges above
criss-cross numbers
simplify if possible (reduce to lowest terms)
Binary Ionic Compounds (Multivalent)
•
contain only two atoms
one metal (iron, cobalt, nickel, copper, gold, mercury, tin or lead) + one non-metal
Naming:
1)
name the metal
2)
reverse the criss-cross rule by putting the subscripts above each element symbol
where they originally came from
3)
check to see if the charge of the non-metal element matches its charge on the periodic
table…
a) if it does, change the charge of the METAL to Roman numerals and write it in
brackets BEHIND the name of the metal
b) if it does not, multiply BOTH the charge of the metal and non-metal by what the
non-metal’s charge should be (according to the periodic table) and change the
charge of the METAL to Roman numerals and write it in brackets BEHIND the name
of the metal
4)
then name non-metal and change ending to “ide”
Polyatomic compounds
•
more than two atoms (count the number of capital letters)
– metal ion + polyatomic negative ion (most are negative) OR
– polyatomic positive ion + non-metal ion OR
– polyatomic positive ion + polyatomic negative ion
Naming:
1)
2)
3)
name positive ion
then name negative ion – polyatomic ion names do not change, only change nonmetal ion’s name if it is an element from groups 5 to 7
check for multivalent metals (use Roman numerals)
Formula:
1)
2)
3)
4)
5)
write symbols
write charges
criss-cross numbers
when placing a subscript BEHIND a polyatomic ion, brackets must be placed around
the polyatomic ion formula
simplify if possible – remember ** polyatomic ion formulas cannot be changed! **
Binary Acids
• two 2 atoms
– starts with H+ ion + non-metal from groups 5 to 7
Naming:
1) H becomes "hydro"
2) name non-metal and change ending to "ic"
3) add the word “acid” to the end of the name
Formula:
1)
2)
3)
4)
write the symbols for each element
write charges
criss-cross numbers
add (aq) to the end of the formula
Examples:
• Give the formula:
hydrofluoric acid
• Give the name:
HCl(aq)
hydriodic acid
HBr(aq)
Oxyacids
• more than 2 atoms
– always starts with H + polyatomic ion containing oxygen is the second ion
• Naming:
1)
2)
3)
•
name the polyatomic ion
If ending of the polyatomic is "ate" change ending to "ic” and add the word “acid"
If ending of the polyatomic is "ite" change ending to "ous” and add the word
“acid“
Formula:
1) write symbols
2) write charges
3) criss-cross numbers
4) add (aq) to the end of the formula
Examples:
• Give the formula:
nitrous acid – HNO3(aq)
• Give the name:
H2SO4(aq) – sulfuric acid
chloric acid - HClO2(aq)
H3PO3(aq) – phosphorous acid
Molecular compounds
• two atoms
– only non-metals
• Naming:
1) Name first non-metal using prefixes (not
“mono”)
2) Name the second non-metal using all
prefixes
3) Change ending to “ide”
• Formula
1) Write symbols
2) Prefix tells how many of each atom
Balancing Chemical Equations
1) Cannot change any of the subscripts
2) Only add number to the front of the
molecules
3) Leave the simplest molecules or lone
atoms until last
4) Work on the most complicated
molecules first
Word/Chemical Equations
• Need same number and type of atoms
on reactant and product side of
equation Word Equation
Skeleton Equation
Balanced Equation
Types of Reactions
1) Synthesis reaction
• A + B  AB
2) Decomposition reaction
•
AB  A + B
3) Single displacement reaction
•
AB + C  AC + B or A + BC
4) Double displacement reaction
• AB + CD  AD + CB
Predicting Products
• Need same type and number of atoms
on reactant side and product side
• Identify which type of reaction it is
– Switch atoms accordingly
• Balance equation
Examples
• Na + O2 
• Na2S + Al 
• FeS
• Cl2 + NaBr 
• NaCl + Cu2SO4
• C4H6 + O2 

Acids/Bases/PH
Acid
Base
Neutral
Change in pH
from 1 to 2
pH scale
Change in the number of H+
ions
_______ times more ________
_______ times less _________
from 2 to 5
_______ times more ________
_______ times less _________
from 12 to 8
_______ times more ________
_______ times less _________
Solution A
ACID
Solution C
NEUTRAL
Solution B
BASE