Nomenclature Review

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Nomenclature Review

• Unit 1 Review of AIM I and chemistry

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Diatomic elements

• Definition
• Elements that cannot exist by themselves in
  nature
• Instead, they are either found in a compound or
  bonded to themselves in a molecule

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Diatomic Elements

• Fantastic Seven - In Nature these form pairs of
  atoms making a molecule.
• Hydrogen - H2

Nitrogen - N2
Fluorine - F2
Oxygen - O2
Chlorine - Cl2
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Bromine - Br2
Iodine - I2
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Naming diatomics

• Name them the same as an element
• Look at the periodic table and write down the
  elements name
• Ignore that there is a subscript of two

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Monatomic ions

• Definition
• Monatomic ions are made from a single atom
• What is an ion?
• Formed when an element loses or gains electrons
• What are the two types of ions?
• Cations and anions

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Metals vs. nonmetals
Non-Metals (Right)
Metals (Left)
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Cations
Ca2

• Definition
• Metals
• Good conductors of electricity
• Luster
• Ductile
• Malleable
• Cations are elements that lose or have lost
  electrons
• They have a positive charge

Na1
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What charges do the cations have?
POSITIVE CHARGES!!
1
3
2
Can have any charge ranging from 1 to 7.
Can have any charge ranging from 1 to 7.
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How to name cations

• When writing the name of a monatomic cation, the
  element's name is written followed by the word
  ion.
• Example Mg2
• What would this be called?
• Try some on your own
• Li
• K
• Ca2

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Anions

• Definition
• Non-metals
• Not good conductors of electricity
• Non-lustrous
• Brittle
• Anions are elements that gain electrons
• They have a negative charge
• Does not include the noble gases!

Cl-1
O-2
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What charges do the anions have?
NEGATIVE CHARGES!!
4 Or - 4
1
0
3
- 3
-2
-1
2
Can have any charge ranging from 1 to 7.
Can have any charge ranging from 1 to 7.
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How to name anions

• When writing the name of a monatomic anion, the
  ending of the elements name is dropped and the
  suffix ide is added.
• Then, the word ion is written following.
• Example O-2
• What would this be called?
• You try some
• Br-
• N-3
• C-4

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Practice Identify if the following are elements,
cations, or anions. Then, name them accordingly.

• H
• H
• H-
• Ca2

Al3 S-2 F- He
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Binary Ionic Compounds

• Definition
• Ionic compounds consisting of two elements
• Always composed of a metal first (cation) and a
  non-metal second (anion)

Na1
Cl-1
Na Cl ? NaCl
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Naming binary ionic compounds

• The cation is always written first in the
  formula, therefore it is always named first. The
  name is written exactly as it is from the
  periodic table.
• The anion is always written second in the
  formula, therefore it is always named second.
  The ending of the name is dropped and the ending
  ide is added.
• Do not include the word ion anywhere this is
  not an ion anymore!
• Example NaCl ? Sodium chloride

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Some have special names

• These supersede any of the rules that were given
  to you
• H2O is water
• NH3 is ammonia
• CH4 is methane
• Remember - All other binary compounds have a name
  with a suffix ide.

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Shows how they like to bond
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Examples

• Name the following examples with your partner
• LiCl
• MgO
• CaF2
• Mg2S

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Special type of binary ionic compound the
transition metals

• Definition
• A metal that contains more than one charge
• Charges can range from 1 to 7
• We do not know what the charge by just looking at
  the periodic table
• The charge either has to be given to you or you
  will have to figure it out

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We need to know roman numerals
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Where are the transition metals located?
The transition metals are located in the center
of the periodic table, under the stair step and
the bottom two rows of the table.
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Naming rules for transition metals

• Similar to the rules from before
• Cation is named first, exactly as it appears on
  the periodic table
• NEW RULE use a roman numeral in parentheses
  after the cations name to show the charge of the
  cation
• Anion is named second, with the ending changed to
  ide.

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For example

• Cu2 bonds with O-2
• They form CuO
• We would call this Copper (II) oxide

O-2
Cu2
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How do we determine the charge of the transition
metal if it is not given to use in the problem?

• Lets do an example to figure this out
• Write the name for Cu2S
• What do we know?
• We know that Cu is Copper and S is Sulfur
• How many Cu do we have? How many S?
• Do we know the charge of Cu? What about S?
• So far we know that this is Copper (___) sulfide

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Lets keep going Cu2S

• Step 1 Determine the charge of the anion.
• What is the charge of S?
• Step 2 Multiply the charge of the anion by the
  subscript on the anion.
• Multiply the charge of S by the subscript of S?
• What do we get?

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Lets keep going Cu2S

• Step 3 Criss cross this charge up to the cation
  (make sure you write it as a positive number)
• Step 4 Divide the charge you wrote on the cation
  by the subscript on the cation
• YOUR ANSWER IS THE CHARGE OF THE CATION.

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Lets put all of the steps together

• What is the correct name for this molecule?
• PbO2

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One more type of ionic compound Ternary or
Polyatomics

• What is happening here?
• An ion is bonding with a polyatomic ion to form a
  polyatomic compound
• Three or more different elements are seen in the
  formula
• Most polyatomic anions contain one or more oxygen
  atoms
• Called oxoanions

MgSO4
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Naming rules for polyatomics

• Rules for naming a compound with a polyatomic
  ion
• Name the cation first. Use the name exactly as
  it appears on the periodic table.
• Name the polyatomic ion second!! (DO NOT change
  the ending to ide) Write the name as it appears
  on your polyatomic ion sheet.
• Our example would be called
• Magnesium sulfate

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Lets go backwards

• You are given the name and asked to write the
  formula
• We use what is called the criss-cross method for
  ionic compounds
• Example Magnesium oxide

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Criss-Cross

• Only used with ionic compounds
• First step write the symbols and charges of
  each element
• Example Magnesium oxide

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Criss-cross continued

• Second criss-cross
• The charge of the cation becomes the subscript of
  the anion
• The charge of the anion becomes the subscript of
  the cation
• Mg O

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Criss-cross

• Last step if your subscripts can reduce, then
  you must reduce them

Mg O
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Lets try some

• Aluminum fluoride
• Sodium carbide
• Strontium nitride

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What about polyatomics?

• Follow the same rules, except that you need to
  write your polyatomic in parentheses
• Example Magnesium phosphate

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Magnesium phosphate

• Step 1 Write down symbols and charges (put your
  polyatomic in parentheses)
• Step 2 Criss-cross
• Step 3 Reduce if needed

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Binary molecular compounds

• Definition
• Also called covalent compounds
• Composed of 2 non-metals (anions)
• NO METALS ARE INCLUDED!!

F-1
Cl-1
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Molecular Substances

• General Properties
• Nonconductors of electricity
• often insoluble in water
• low melting point
• low boiling point
• relatively easy to separate because of low
  intermolecular forces

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Greek Prefixes

• We need to learn Greek first!
• You are responsible for knowing the following
  Greek prefixes to use only with covalent
  compounds

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Naming covalent compounds

• The name of the first element in the compound is
  written first, exactly how it appears on the
  periodic table.
• If there is more than one of these atoms, a Greek
  prefix must be used to tell how many atoms are
  present.
• If only one atom is present WE DO NOT USE A
  GREEK PREFIX. This means that no covalent
  molecule starts with mono.

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Naming covalent compounds continued

• The name of the second element in the compound is
  written second.
• Use the name from the periodic table however,
  the ending is dropped and ide is added to the
  molecule.
• A greek prefix MUST ALWAYS be used to tell how
  many atoms of the second element are present in
  the compound, even if there is only one.

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Example

• CO2
• First elements name is?
• How many atoms of C are there?
• Do we need a prefix?
• Second elements name is?
• We change it to?
• How many atoms of O are there?
• Do we need a prefix?
• What is the name of this molecule?

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Try and name the following covalent compounds

• C4O5
• F3O
• I2F9

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PracticeIdentify if the following compounds are
ionic or covalent, then name accordingly.

• NaCl
• CO
• H2O
• CH4
• CaF2
• S2O3
• AlN

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Acids

• Definition
• Molecules that start with H
• When dissolved in water, acids break apart and
  add H to the water
• Two types
• Binary
• Ternary

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Binary Acid

• Made of two elements
• Hydrogen and one other nonmetal
• Naming
• Every binary acid starts with the prefix hydro-
• Then, you write the name of the non-metal from
  the periodic table, but change the ending to ic.
• Then write the word acid.
• Hydro_________ic acid

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Example

• HF
• - Hydrofluoric acid
• HCl
• - Hydrochloric acid

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You try some

• H4C
• H2S

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Ternary Acids also called oxoacids

• Made up of three or more elements
• Hydrogen bonded to a polyatomic ion
• Naming depends on the name of the polyatomic ion.

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If bonded to a polyatomic ion that ends in - ate

• - ate
• Then the name of the acid is the name of the
  polyatomic ion with the ending changed to ic
• Then, you add the word acid to it
• DO NOT USE HYDRO- FOR THESE!!!
• For example H2SO4
• This is Hydrogen bonded to SO4. What is the name
  of SO4?
• Sulfate ? so this becomes Sulfic acid.

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If bonded to a polyatomic ion that ends in - ite

• - ite
• Then the name of the acid is the name of the
  polyatomic ion with the ending changed to ous
• Then, you add the word acid to it
• DO NOT USE HYDRO- FOR THESE!!!
• For example H2SO3
• This is Hydrogen bonded to SO3. What is the name
  of SO3?
• Sulfite ? so this becomes Sulfous acid.

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• Oxoanions
• ate common ClO3- chlorate
• ite -1 oxygen ClO2- chlorite
• per__ate 1 oxygen ClO4- perchlorate
• hypo__ite -2 oxygens ClO- hypochorite

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Lets try naming acids

• HCl
• H3N
• HNO3
• HNO2
• H2CO3
• H3PO3

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A new type of molecule

• The hydrates
• What comes to mind when you hear the word hydrate?

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Hydrates

• Definition
• Water molecules that have adhered to ions or
  molecules becoming part of the crystal that is
  formed from a compound.
• Water attached to an ionic compound.

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Naming rules

• Same as before for the ionic compound
• Name the Cation first, exactly as it appears on
  the periodic table
• Name the Anion second, change the ending of its
  name to ide
• Use the greek prefixes to tell how many water
  molecules are attached.
• End with the word hydride.

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• For example
• NaCl H2O
• This is called Sodium chloride monohydride
• Try this example
• MgO 5 H2O
• This would be called ?

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Coordination compounds

• Type of complex
• Composed of a central atom (usually a metal)
• Surrounded by atoms or groups of atoms called
  ligands
• Recognized because it is usually written in
  square brackets
• Ni2 6 H2O ? Ni(H2O)62

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• Like an acid and base reaction where the metals
  behaves as a Lewis acid and accepts a pair of
  electrons from the Lewis base (ligand)
• Complex can be ionic or neutral
• Ionic called a complex ion
• Neutral called a coordination compound

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Naming rules

• Metal (the central atom) is always listed first
  in the brackets however, when naming the metal
  name is always given last
• Any material not listed within the brackets is
  named separately
• If everything in the formula is enclosed in one
  set of brackets, the entire name will be one word
• Use greek prefixes to tell how many of each
  element is present
• Ligand are listed alphabetically
• Anionic complex ions get a suffix of -ate

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Examples to help name

• Ni(H2O)4Cl2
• Nickel is the center metal we name it last
• Figure out its oxidation here so we know what
  charge we are using
• This is cationic (metal) does not end is ate
• We have four water and two chlorine (use our
  prefixes from the nonmetals to name these)
• Tetraaqua
• Dichloro
• So we get tetraaquadichloronickel(II)