Chemical Names

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Chemical Names Formulas

• Chapter 9

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Warm Up

• Take 7 min to finish Homework

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Go Over

• ChemQuest 21
• Skill Practice 19-21
• More Ionic Bonding Practice

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Time to Review Ionic Bonding

• IB QUIZ NEXT CLASS
• This should go quick. All of this has been
  taught. Some of these slides you have already seen

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Ionic Bonding Between Metals and Nonmetals
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Monatomic Ions

• Ions consisting of one atom
• Determined by using the periodic table

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• Transition Metals - the charge must be provided
• Ex.)
• Fe(III) has a 3 charge
• Fe(II) has a 2 charge
• Reference Table 9.2, p.255 for trans. metal
  names and charges
• Stock Name vs. Classical Name
• Ex) Copper(I) ion (stock name) and Cuprous ion
  (classical name)

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Polyatomic Ions

• Tightly bound group of atoms that behave as a
  unit and carry a charge
• Treated the same as monatomic ions when writing
  chemical formulas and naming (also called
  tertiary compounds)
• Ex.)

(PO4)3-
Phosphate
(CO3)2-
Carbonate
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Polyatomic Ions
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Types of Compounds

• Ionic
• Metal Non-Metal
• Molecular
• 2 Non-Metals

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Ionic Compounds

• Ionic bond forms between ions (atoms w/ a charge
  b/c they have extra or missing e-)
• Represented by chemical formulas (or formula
  units)
• Ex) NaCl
• Typically solids at room temperature
• Occurs between oppositely charged ions
  (opposites attract)
• Include a cation an anion
• Cation charges
• Anion - charges

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• In an ionic compound, the atoms combine in ratios
  to balance the charges (neutral compound)
• Ex.) How many Mg will react w/ S?

Mg2 S2- ? MgS
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Criss-Cross Method

• An easier way to determine the subscripts
• Use it if it makes sense to you. Otherwise,
  continue balancing the charges

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Criss-Cross Method

• How many B will react w/ S?
• B3 S2-

B3
S2-
B2S3

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Notice when you write the formula the cation
(metal) goes 1st
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Examples
What is the formula when Al and F combine? Al3
F1-
Al3
F1-
AlF3

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1
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Examples
LiBr

• Lithium and Bromine

CaS
Calcium and Sulfur
Zn3P2
Zn (II) and Phosphorus
Na3PO4
Sodium and Phosphate
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Naming Ionic Compounds

• Binary compounds - composed of 2 elements
• 1st write the name of the cation
• 2nd write the name of the anion
• Replace the ending with -ide

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Examples

• Al2O3

Aluminum Oxide
NaCl
Sodium Chloride
Calcium Oxide

• CaO

Iron(II) Sulfide

• FeS

Copper(II) Bromide
CuBr2
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Naming Ionic Compounds with Polyatomic Ions

• composed of 3 or more different elements
• 1st write the name of the cation
• 2nd write the name of the polyatomic ion

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Examples

• Al(NO3)3

Aluminum Nitrate
Na(OH)
Sodium Hydroxide
Ca(SO4)
Calcium Sulfate
Fe(CrO4)
Iron(II) Chromate
Cu3(PO4)
Copper(I) Phosphate
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Naming Race Worksheet

• Second Page (Front/Back) of packet
• Work with ONE partner OR by yourself
• Do all 45
• Get answers checked by me
• First group done

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Naming Acids

• Use the template below to name acids

Anion ending Example Acid name Example
- ide HCl Chloride Hydro( )-ic acid Hydrochloric acid
- ite H2SO3 Sulfite ( ) ous acid Sulfurous acid
- ate HNO3 Nitrate ( ) ic acid Nitric acid
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Properties of IB

• Properties
• - Electrically neutral compounds
• - High boiling/melting point (BP/MP)
• - Form crystal solids which are brittle
• - Dissolve in Water
• - Conduct electricity in molten or dissolved
  state

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Ionic Compounds

• Dissociate into ions when they dissolve
• So,
• NaCl Na Cl-
• AlCl3 Al3 3Cl-
• Note The number of each ion becomes a
  coefficient (3Cl-)
• Ions have a charge, so the charge MUST be written

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Write the equation when the following ionic
compounds dissolve in water

• MgO
• Na3P
• Fe2O3
• Mg(NO3)2
• FeSO4

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Work on Ionic Bonding Practice

• First Page (Front/Back) of Packet

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STOP

• Complete any unfinished worksheets

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Molecular Compounds

• Compounds composed of molecules (usually 2 or
  more non-metals)
• Represented by molecular formulas
• Ex) H2O
• Typically exist as gasses or liquids at room
  temperature
• Diatomic molecules
• H2, N2, O2 , F2 , Cl2 , Br2 , I2

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Naming Molecular Compounds

• Binary molecular compounds - composed of 2
  non-metals
• Use prefixes to distinguish between different
  compounds (Table 6.5, p.159)
• Atom which is furthest to the left is written
  first

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Prefix Number
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10
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Examples

• SO3

Sulfur trioxide
CO
Carbon Monoxide
OF6
Oxygen Hexafluoride
P2Br4
Diphosphorus tetrabromide
S3I8
Trisulfur Octiodide
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Examples

• Name the following acids
• HBr
• HNO2
• H2SO4
• Write the formula for the following acids
• Hydrofluoric acid
• Phosphorous acid

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The Law of Definite Proportions

• the masses of the elements are always in the same
  proportions in any sample of a chemical compound

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161
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The Law of Multiple Proportions

• Comparison of the ratios of one element in 2
  different compounds containing that particular
  element

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Example

• A sample of water contains 16 g of oxygen,
  whereas a sample of hydrogen peroxide contains 32
  g of oxygen. What is the ratio of oxygen in the
  two compounds?