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Unit 5“Chemical Names
and Formulas”
ChemistryTroy High School
Mr. Blake
H2O
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Section 9.1Naming Ions
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Atoms and Ions• are
electrically neutral.–Same number of p+ and e-
• - atoms with a charge (+ or -)
• Made by gaining or losing .– Only electrons can move
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An Anion is…• A negative ion =
electrons.• Nonmetals gain electrons.• Charge is written as a superscript on the right.
F1- Has gained electron (-ide is new ending = )
O2- Gained electrons ( )
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A Cation is…• A positive ion =
electrons.• lose electrons
K1+ Has lost electron (no name change for positive ions)
Ca2+ Has lost electrons
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Predicting Ionic ChargesGroup 1A:Lose electron to form ions
H1+ Li1+ Na1+ K1+ Rb1+
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Predicting Ionic ChargesGroup 2A:Loses electrons to form ions
Be2+ Mg2+ Ca2+ Sr2+ Ba2+
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Predicting Ionic ChargesGroup 3A: Loses electrons to form ions
B3+ Al3+ Ga3+
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Predicting Ionic Charges
Group 4A: Do they lose 4 electrons or gain 4 electrons?
! Group 4A elements rarely form ions (they tend to share)
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Predicting Ionic ChargesGroup 5A: Gains _ electrons to form ions
N3-
P3-
As3-
Nitride
Phosphide
Arsenide
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Predicting Ionic ChargesGroup 6A: Gains electrons to form ions
O2-
S2-
Se2-
Oxide
Sulfide
Selenide
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Predicting Ionic ChargesGroup 7A: Gains _ electron to form ions
F1-
Cl1-
Br1-Fluoride
Chloride
Bromide
I1-Iodide
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Predicting Ionic ChargesGroup 8A: Stable noble gases
form ions!
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Predicting Ionic ChargesGroup B elements: Many transition elements have possible charge.
Iron (II) = Iron (III) =
Use of Roman numerals to show charges
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Naming Cations
• system – use roman numerals in parenthesis to indicate the charge value
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Naming cations• If the charge is always the
(like in the Group A metals) just write the of the metal.– Calcium =
• metals can have more than one type of charge.– Indicate charge as roman numeral in
after the name of the metal (Table 9.2, p.255)
– Iron (IV) =
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Predicting Ionic Charges Some elements also have more than one possible charge.Tin (II) = Lead ( ) = Pb2+
Tin (IV) = Lead ( ) = Pb 4+
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Predicting Ionic ChargesGroup elements: Some transition elements have only one possible oxidation state, such as these three:
Zinc = Silver = Cadmium =
**Do not use roman numerals for these
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Practice by naming these:• Na+ • Ca2+ • Al3+ • Fe3+ • Fe2+ • Pb2+ • Li+
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Write symbols for these:
• Potassium ion• Magnesium ion • Copper (II) ion• Chromium (IV) ion• Barium ion• Mercury (II) ion
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Naming Anions
• Anions are the same charge
• Change the ending to _
• F1- a Fluorine atom will become a ion.
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Practice by naming these:
• Cl- • N3- • Br- • O2-
• Ga3+
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Write symbols for these:
•Sulfide ion• Iodide ion•Phosphide ion•Strontium ion
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Polyatomic ions are…• Groups of atoms that together,
have an charge, and one name.• Usually end in – or - _
• Acetate: C2H3O2-
• Nitr : NO3-
• Nitr : NO2-
• Permanganate: MnO4-
• Hydroxide: OH- and Cyanide: CN-?
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• Sulf : SO42-
• Sulf : SO32-
• Carbonate: CO32-
• Chromate: CrO42-
• Dichromate: Cr2O72-
• Phosph : PO43-
• Phosph : PO33-
• Ammonium: NH41+
Know Table 9.3 on page 257
(One of the few positive polyatomic ions)
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H + Polyatomic ion =….
•If the polyatomic ion begins with H, then put “hydrogen” in front of the polyatomic ion: H1+ + CO3
2- → HCO31-
hydrogen + carbonate → hydrogen carbonate ion
• HSO3
• HPO4
• HCO3
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Helpful Hints on Oxy-Anions
1. _________: smaller # of oxygen2. _________: larger # of oxygen
Ex.
NO3- ____________________________
NO2- ____________________________
SO42- ____________________________
SO32- ____________________________
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A Guide to Determine Whether the –ate Formula is –XO3 or –XO4:
B C N
Cl
Br
I
Si P S
As Se
1
2
3
4
5
6
1 2 13 14 15 16 17 18
Transition Metals
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Section 9.2 Naming and Writing
Formulas for Ionic Compounds
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Writing Ionic Compound FormulasExample: Iron (III) chloride
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.
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Writing Ionic Compound Formulas
Example: Aluminum sulfide
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.
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Writing Ionic Compound Formulas
Example: Zinc hydroxide
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.
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Writing Ionic Compound Formulas
Example: Magnesium carbonate (note the 2 word name)
1. Write the formulas for the cation and anion, including CHARGES!
Mg2+CO32-
2. Check to see if charges are balanced.
They are balanced!
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Writing Ionic Compound Formulas
Example: Barium nitrate (note the 2 word name)1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.
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Writing Ionic Compound FormulasExample: Ammonium sulfate
1. Write the cation and anion with CHARGES!
2. Balance charges using the criss-cross method with subscripts, if necessary. Use parentheses if you need more than one of a polyatomic ion to balance subscripts.
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Writing Ionic Compound Formulas
Example: Aluminum phosphate
1. Write the formulas for the cation and anion, including CHARGES!
Al3+ PO43-
2. Check to see if charges are balanced.
They ARE balanced!
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Naming Ionic Compounds• 1. Cation , then anion
• 2. Monatomic cation = name of the element
• Ca2+ = ion
• 3. Monatomic anion = root + -ide
• Cl- =
• CaCl2 =
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Naming Ionic Compounds
• If the metal can have more than one charge ( ), use a Roman numeral in their name:
PbCl2 use the to find the
charge on the cation (chloride is always 1-)
(Metals with multiple oxidation states)
is the lead ( ) cation
PbCl2 = lead ( ) chloride
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Things to look for:
1) If cations have ( ), the number in parenthesis is their
.2) If anions end in –ide, they are
probably off the periodic table
( )3) If anion ends in -ate or –ite,
then it is
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Practice by writing the formula or name as required…
• Iron (II) Phosphate• Stannous Fluoride• Potassium Sulfide• Ammonium
Chromate• MgSO4
• FeCl3
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Section 9.3Naming and Writing
Formulas for Molecular
Compounds
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Molecular compounds are…• Made of only
• Smallest part is a • Can’t use charges to figure
out how many of each atom (there are no charges present / they share electrons)
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Molecular compounds are easier!• compounds use
to determine how many of each.• Figure out charges and criss-cross numbers.
• Molecular compounds: the name tells you the number of atoms.• Uses to tell you
the exact number of each element present!
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Prefixes (Table 9.4, p.269)
• 1 = mono-• 2 = di-• 3 = • 4 = tetra-• 5 = • 6 = hexa-• 7 = hepta-• 8 = octa-
• 9 = nona-• 10 =
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Prefixes• To write the name, include:
• One exception is we don’t write if there is only of
the element.• Normally, we do not have double vowels
when writing names (oa oo)
Prefix + name -ide
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Practice by naming these:
• N2O
• NO2
• Cl2O7
• CBr4
• CO2
• BaCl2
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Write formulas for these:• diphosphorus
pentoxide• tetraiodine nonoxide• sulfur hexafluoride• nitrogen trioxide• carbon tetrahydride• phosphorus trifluoride• aluminum chloride(Ionic compound)
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Section 9.4Naming and Writing Formulas for Acids
and Bases
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Acids are…• Compounds that give off
ions (H+) when dissolved in water (the Arrhenius definition)
• Formula starts with .• Always be some Hydrogen
next to an .• determines the
name.
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Rules for Naming acids: Name it as a normal compound first
• If the anion attached to hydrogen ends in -ide, put the prefix and change -ide to - acid
• In other words, if it’s just Hydrogen and one other nonmetal
• HCl = • H2S =
acid
acid
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Naming Acids• If the anion has oxygen in it, then it ends
in -ate or -ite2) Change -ate to -ic acid (use no prefix)
• Example: HNO3 Hydrogen + nitrate =
3) Change -ite to -ous acid (use no prefix)• Example: HNO2 Hydrogen + nitrite
=
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Naming Acids
Normal ending
____-ide
____-ate
____-ite
Acid name is…
hydro-___-ic acid
_____-ic acid
_____-ous acid
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Practice by naming these:
• HF• H3P
• H2SO4
• H2SO3 • HCN• H3PO4
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Writing Acid Formulas – in reverse!• Hydrogen will be listed first• The name will tell you the • Be sure the charges cancel out.
• Starts with hydro?• Anion is
, ends in –ide
• No hydro?1) -ate anion
comes from – ending
2) -ite anion comes from – ending
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Write formulas for these:
• hydroiodic acid• chloric acid• carbonic acid• phosphorous acid• hydrobromic acid
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Names and Formulas for Bases
• Base - an ionic compound that produces ions ( ) when dissolved in water (the Arrhenius definition)
• Named the same way as other ionic compounds:–Name of cation ( ) followed by
name of anion (which will be ).
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Names and Formulas for Bases
• NaOH =• Ca(OH)2 =
• To write the formula:
1) Write symbol for metal cation
2) Followed by hydroxide ion (OH1-)
3) Use criss-cross method to balance the charges.
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Practice by writing the formula for the following:
• Magnesium hydroxide• Iron (III) hydroxide• Zinc hydroxide
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Section 9.5The Laws Governing
Formulas and Names
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Some Laws:
Law of Proportions- in a sample of a chemical compound, the of the
are always in the proportions.
In every molecule of H2O (water), the mass ratio of H:O is 1:8
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Some Laws:Law of Proportions- Whenever two elements form than one compound, the masses of one element that combine with the mass of the other element are in the ratio of small .
H2O (water) and H2O2 (hydrogen peroxide)
2:1 2:2
2g:16g 2g:32g
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• https://www.youtube.com/watch?v=0OOcpiTiXzM
• Law of Definite Proportions - Law of Multiple Proportions
• by Brightstorm
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Summary of Naming and Formula Writing
• For naming, follow the flowchart- Figure 9.20, page 277
• For writing formulas, follow the flowchart from Figure 9.22, page 278
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Helpful to remember...1. In ionic compounds, the net charge is
_ (criss-cross method)2. Put -ide at the end of monatomic
3. An -ite or -ate ending means there is a ion that
has 4. Prefixes generally mean ;
they show the number of each atom
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Helpful to remember...5. A Roman numeral after the name
of a cation is the of the cation