Chemical Names and Formulas Chapter 9. Section 1 Naming Ions
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- Slide 1
- Chemical Names and Formulas Chapter 9
- Slide 2
- Section 1 Naming Ions
- Slide 3
- Section 1 Learning Targets 9.1.1 I can identify the charges of
monatomic ions by using the periodic table, and name the ions.
9.1.2 I can define a polyatomic ion and write the names and
formulas of the most common polyatomic ions. 9.1.3 I can identify
the two common endings for the names of most polyatomic ions.
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- Monatomic Ions Monatomic ion consist of a single atom with a
positive or negative charge resulting from the gain or loss of one
or more valence electrons.
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- Cations When the metals in Groups 1A, 2A and 3A lose electrons
they form cations with positive charges equal to the group number.
The names of these ions are the same as the element name with ion
after it.
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- Anions Nonmetals of Groups 5A, 6A, and 7A gain electrons to
form anions with negative charges. The charge of any ion of a Group
A nonmetal is determined by subtracting 8 from the group
number.
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- Group 7A so 7-8=-1; 6A so 6-8=-2; 5A so 5- 8=-3 The names of
these ions change. The endings are dropped and replaced by ide ion
(sulfur = sulfide ion). Groups 4A and 8A elements do not usually
form ions.
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- Examples: 1. Name the ions formed by these elements and
classify them as anions or cations: a) Selenium
____________________ b) Barium ____________________ c) Phosphorus
____________________
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- Examples: 2. Name the following ions: a) I -
____________________ b) N 3- ____________________ c) O 2-
____________________
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- This table can be found on page 254
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- Ions of Transition Metals The charges of the cations of many
transition metal ions must be determined from the number of
electrons lost.
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- Two methods classical (-ous and ic endings) or the stock system
(roman numerals). Preferred is the stock system because the roman
numeral tells the charge. So why do we use Roman numerals or the
classical method anyway?
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- This table can be found on page 255
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- Examples: 1. Name the following ions: a) Fe 3+
____________________ b) Cu + ____________________ c) Mn 4+
____________________ d) Sn 2+ ____________________ e) Pb 4+
____________________
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- Polyatomic Ions Polyatomic ion composed of more than one atom.
The names of most polyatomic anions end in ate or ite. There are
very few positive polyatomic ions.
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- Examples: 1. Write the symbol or formula (including charge) for
each of the following ions: a) Ammonium ion ____________________ b)
Chromate ion ____________________ c) Tin (II) ion
____________________ d) Nitrate ion ____________________
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- Examples: 2. Name the following ions: a) OH -
____________________ b) Pb 4+ ____________________ c) SO 4 2-
____________________ d) O 2- ____________________
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- Section 2 Naming and Writing Formulas for Ionic Compounds
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- Section 2 Learning Targets 9.2.1 I can apply the rules for
naming and writing formulas for binary ionic compounds. 9.2.2 I can
apply the rules for naming and writing formulas for compounds with
polyatomic ions.
- Slide 21
- Binary Ionic Compounds In the past anyone who created a
compound named it. Currently there is a system. Antione Lavoisier
decided it was too difficult to memorize unrelated names and
formulas.
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- Naming Binary Ionic Compounds Binary compound compound of two
elements and can be either ionic or molecular. To name binary ionic
compounds, place the name of the cation first followed by the anion
name.
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- Examples: 1. Write the names of the following binary ionic
compounds: a) NaCl ____________________ b) MgBr 2
____________________ c) SrO ____________________ d) Li 2 O
____________________ e) Be 3 N 2 ____________________
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- For transition metals you need to figure the charge of the
metal and put that in parentheses as a Roman numeral.
- Slide 25
- Examples: 1. Write the names of the following binary ionic
compounds: a) SnO 2 ____________________ b) Fe 2 O 3
____________________ c) MnO ____________________ d) MnO 2
____________________ e) Co 3 N 2 ____________________
- Slide 26
- Writing Formulas for Binary Ionic Compounds Write the symbol of
the cation and then the anion. Add what ever subscripts are needed
to balance the charges.
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- Examples: 1. Write the formulas for the compounds formed from
these pairs of ions: a) Ba 2+, S 2- ____________________ b) Ca 2+,
N 3- ____________________ c) Li +, O 2- ____________________ d) Cu
2+, I - ____________________
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- Examples: 2. Write the formulas for these compounds: a) Sodium
iodide ____________________ b) Potassium sulfide
____________________ c) Calcium iodide ____________________
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- For transition metals the Roman numeral tells the charge on the
metal cation. Then the same as before, balance the charges.
- Slide 30
- Examples: 1. Write the formulas for the following compounds: a)
Tin (IV) nitride ____________________ b) Copper (I) oxide
____________________ c) Copper (II) oxide ____________________ d)
Lead (II) sulfide ____________________ e) Iron (III) oxide
____________________
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- Compounds with Polyatomic Ions Write the symbol for the cation
followed by the formula for the polyatomic ion and balance the
charges. HINT: if you need more than one polyatomic ion use
parenthesis.
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- Examples: 1. Write the formula for the following compounds: a)
Ammonium nitride ____________________ b) Ammonium cyanide
___________________ c) Calcium carbonate ____________________ d)
Tin (IV) sulfite ____________________ e) Magnesium phosphate
__________________
- Slide 33
- Naming Compounds with Polyatomic Ions To name a compound
containing a polyatomic ion, state the cation first and then the
anion, just as you did for binary ionic compounds.
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- Examples: 1. Name the following compounds: a) Sn 2 (CO 3 ) 4
____________________ b) Mg(CN) 2 ____________________ c) Fe(NO 3 )
3 ____________________ d) (NH 4 ) 3 PO 4 ____________________ e)
CuSO 4 ____________________
- Slide 35
- Section 3 Naming and Writing Formulas for Molecular
Compounds
- Slide 36
- Section 3 Learning Targets 9.3.1 I can interpret the prefixes
in the names of molecular compounds in terms of their chemical
formulas. 9.3.2 I can apply the rules for naming and writing
formulas for binary molecular compounds.
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- Naming Binary Molecular Compounds Remember binary means 2.
Molecular compounds have covalent bonds not ionic like previous
sections.
- Slide 38
- A prefix in the name of a binary molecular compound tells you
how many atoms of each element are present in each molecule of the
compound. Ending is still ide so make sure youre telling the
difference between molecular and ionic.
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- Examples: 1. Write the name for the following binary molecular
compounds: a) NCl 3 ____________________ b) SO 3
____________________ c) NI 3 ____________________ d) N 2 O 3
____________________ e) N 2 H 4 ____________________
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- Writing Formulas for Binary Molecular Compounds Use the
prefixes in the name to tell you the subscripts of each element in
the formula. Then write the correct symbols for the two elements
with the appropriate subscripts.
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- Examples: 1. Write the formulas for the following binary
molecular compounds: a) Phosphorus pentachloride __________________
b) Iodine heptafluoride ____________________ c) Chlorine
trifluoride ____________________ d) Iodine dioxide
____________________ e) Diphosphorus trioxide
____________________
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- Section 4 Naming and Writing Formulas for Acids and Bases
- Slide 44
- Section 4 Learning Targets 9.4.1 I can apply three rules for
naming acids. 9.4.2 I can apply the rules in reverse to write the
formulas for acids. 9.4.3 I can apply the rules for naming
bases.
- Slide 45
- Naming Acids Acid a compound that contains one or more hydrogen
atoms and produces hydrogen ions (H + ) when dissolved in
water.
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- Rules for Naming Acids 1. When the name of the anion (X) ends
in ide, the acid name begins with the prefix hydro-. The stem of
the anion has the suffix ic and is followed by the word acid. HCl
(aq) (X = chloride) is named hydrochloric acid. H 2 S (aq) (X =
sulfide) is named hydrosulfuric acid.
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- 2. When the anion name ends in ite, the acid name is the stem
of the anion with the suffix ous, followed by the word acid. H 2 SO
3(aq) (X = sulfite) is named sulfurous acid.
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- 3. When the anion name ends in ate, the acid name is the stem
of the anion with the suffix ic followed by the word acid. HNO
3(aq) (X = nitrate) is named nitric acid.
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- Examples: 1. Write the names for the following acids: a) HNO 2
____________________ b) HCN ____________________ c) HMnO 4
____________________ d) H 2 S ____________________ e) HClO 4
____________________
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- Writing Formulas for Acids Use the rules for writing the names
of acids in reverse to write the formulas for acids.
- Slide 53
- Examples: 1. Write the formulas for the following acids: a)
Carbonic acid ____________________ b) Sulfurous acid
____________________ c) Hydroiodic acid ____________________ d)
Nitrous acid ____________________ e) Phosphoric acid
____________________
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- Names and Formulas for Bases Base an ionic compound that
produces hydroxide ions (OH - ) when dissolved in water. Bases are
named in the same way as other ionic compounds. The name of the
cation is followed by the name of the anion. Formulas are written
the same as for ionic compounds.
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- Examples: 1. Identify each compound as an acid or a base: a)
Ba(OH) 2 ____________________ b) HClO 4 ____________________ c)
Fe(OH) 3 ____________________ d) KOH ____________________
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- Examples: 2. Write the names for the following bases: a) Ba(OH)
2 ____________________ b) LiOH ____________________ c) Pb(OH) 2
____________________ d) Mg(OH) 2 ____________________ e) Al(OH) 3
____________________
- Slide 57
- Section 5 The Laws Governing Formulas and Names
- Slide 58
- Section 5 Learning Targets 9.5.1 I can define the laws of
definite proportions and multiple proportions. 9.5.2 I can apply
the rules for naming chemical compounds by using a flowchart. 9.5.3
I can apply the rules for writing the formulas of chemical
compounds by using a flowchart.
- Slide 59
- The Laws of Definite and Multiple Proportions The rules for
naming and writing formulas are possible because compounds form
from the elements in predictable ways. These ways are summed up in
two laws: the law of definite proportions and the law of multiple
proportions.
- Slide 60
- The Law of Definite Proportions States that in samples of any
chemical compound, the masses of the elements are always in the
same proportions.
- Slide 61
- The Law of Multiple Proportions States whenever the same two
elements form more than one compound, the different masses of one
element that combine with the same mass of the other element are in
the ratio of small whole numbers.
- Slide 62
- Practicing Skills: Naming Chemical Compounds Follow the arrows
and answer the questions on the flow chart to write the correct
name for a compound.
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- Examples: 1. Write the names for the following compounds: a)
NaClO 3 ____________________ b) HClO 4 ____________________ c) KHSO
4 ____________________ d) Cl 2 O ___________________
- Slide 66
- Examples: 1. Write the names for the following compounds: e)
SnO 2 ____________________ f) Ca(OH) 2 ____________________ g) K 2
CrO 4 ____________________ h) Fe(C 2 H 3 O 2 ) 3
____________________ i) SiCl 4 ____________________
- Slide 67
- Practicing Skills: Writing Chemical Formulas An ide ending
generally indicates a binary compound. Either ionic or covalent. An
ite or ate ending means a polyatomic ion that includes oxygen is in
the formula. An ic or ous ending shows that the compound may be an
acid.
- Slide 68
- Practicing Skills: Writing Chemical Formulas Prefix in a name
generally indicate the compound is molecular. A Roman numeral after
the name of a cation shows the ionic charge of the cation.
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- Examples: 1. Write the formulas for the following compounds: a)
Calcium bromide ____________________ b) Aluminum carbide
___________________ c) Tin (IV) cyanide ____________________ d)
Strontium acetate ____________________ e) Silver chloride
____________________
- Slide 72
- Examples: 1. Write the formulas for the following compounds: f)
Nitrogen dioxide ____________________ g) Lithium hydride
____________________ h) Sodium silicate ____________________ i)
Acetic acid ____________________ j) Hydrochloric acid
___________________