Transcript Chapter 3 Molecules, Compounds, and Chemical Equations

Chapter 3
Molecules, Compounds, and
Chemical Equations
Molecular View of Elements and
Compounds
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How do atom join together to form
a compound?
compounds are made of atoms held together by chemical bonds
 ionic bonds result when electrons have been transferred between
atoms, resulting in oppositely charged ions that attract each other
 Metal + Nonmetal
 covalent bonds result when two atoms share some of their
electrons
 Nonmetal + Nonmetal

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Representing Compounds with
Chemical Formula
compounds are generally represented with a chemical formula
 all chemical formulas tell what elements are in the compound
◦ use the letter symbol of the element
 Empirical Formula describe the kinds of elements found in the
compound and the ratio of their atoms
◦ Simplest form of a molecule or compound
◦ they do not describe how many atoms, the order of
attachment, or the shape

◦ the formulas for ionic compounds are empirical
 Molecular Formula describe the kinds of elements found
in the compound and the numbers of their atoms
◦ they do not describe the order of attachment, or the
shape
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Chemical Formulas
Hydrogen Peroxide
Molecular Formula = H2O2
Empirical Formula = HO
Glucose
Molecular Formula = C6H12O6
Empirical Formula = CH2O
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Ionic Compounds
metals + nonmetals
 no individual molecule units,
instead have a 3-dimensional
array of cations and anions
made of formula units
 many contain polyatomic
ions
◦ Two or nonmetals are
bonded and carried
charge


Writing Formulas
for Ionic
Compounds
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Some Common Polyatomic Ions
Name
Formula
Name
Formula
acetate
carbonate
hydrogen carbonate
(aka bicarbonate)
hydroxide
nitrate
nitrite
chromate
dichromate
ammonium
C2H3O2–
CO32–
hypochlorite
ClO–
OH–
NO3–
chlorite
chlorate
perchlorate
sulfate
sulfite
NO2–
CrO42–
ClO2–
ClO3–
ClO4–
SO42–
SO32–
hydrogen sulfate
(aka bisulfate)
HSO4–
Cr2O72–
NH4+
hydrogen sulfite
(aka bisulfite)
HSO3–
HCO3–
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Examples
Complete the names of the following ions:
Ca2+
________
N3
_________
Al3+
__________
Se2
__________
Polyatomic ions
NH4+
_____________
CO32_______________
HPO42______________
CN_______________
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Writing Ionic compound
Identify the cation and anion
 Combine the cation and anion together to produce an electrically
charged compound.
◦ If the charges on the cation and anion are NOT equal in
magnitude, use the charge on the cation as the subscript for the
anion. Use the charge on the anion (omitting the negative sign) as
the subscript for the cation.
◦ Place parentheses around a polyatomic ion if you need more than
one of them in the final formula.
◦ Do not show the charges of the ions when you write the final
formula for the compound
 Make sure that the subscripts for the cation and anion are the
smallest whole number ratio.

Examples
What are the formulas and names for compounds made from the
following ions?

potassium ion with a nitride ion

Ammonium ion with a sulfide ion
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Examples

Write a formula for the combination of the following ions then give
a systematic name for each compound

NH4+ and SO42-

Al3+ and PO43-
Transitional Metal Cations

Metals with Invariant
Charge
◦ metals whose ions
can only have one
possible charge
 Groups 1A+1 & 2A+2,
Al+3, Ag+1, Zn+2, Sc+3
◦ cation name =
metal name with
Roman numeral in
parenthesis
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Examples

Write formulas and provide their names
1.
Pb4+ and S2-
2.
Cu2+ and F-
Example – Naming Binary Ionic with
Invariant Charge Metal CsF
1.
Identify cation and anion
Cs = Cs+ because it is Group 1A
F = F- because it is Group 7A
2.
Name the cation
Cs+ = cesium
3.
Name the anion
F- = fluoride
4.
Write the cation name first, then the anion name
cesium fluoride
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Example – Naming Ionic Compounds
Containing a Polyatomic Ion Na2SO4
1.
2.
3.
4.
Identify the ions
Na = Na+ because in Group 1A
SO4 = SO42- a polyatomic ion
Name the cation
Na+ = sodium, metal with invariant charge
Name the anion
SO42- = sulfate
Write the name of the cation followed by the name of the anion
sodium sulfate
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Name the following compounds
1.
TiCl4
2.
Au2S3
3.
MnO
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Practice - What are the formulas for
compounds made from the following ions?
1.
iron(III) ion with a bromide ion
2.
aluminum ion with a sulfate ion
3.
chromium(II) with hydrogen carbonate
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Hydrates



hydrates are ionic compounds containing
a specific number of waters for each
formula unit
water of hydration often “driven off ” by
heating
in formula, attached waters follow ∙
 CoCl2∙6H2O

in name attached waters indicated by
suffix -hydrate after name of ionic
compound
 CoCl2∙6H2O = cobalt(II) chloride hexahydrate
 CaSO4∙½H2O = calcium sulfate hemihydrate
Hydrate
CoCl2∙6H2O
Anhydrous
CoCl2
Prefix No. of
Waters
hemi
½
mono
1
di
2
tri
3
tetra
4
penta
5
hexa
6
hepta
7
octa
8
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Practice
1.
What is the formula of magnesium sulfate heptahydrate?
2.
What is the name of NiCl2•6H2O?
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Naming Covalent Compounds
N2F4
The first element listed is more
cationlike and takes the name of
the element.
The second element listed is more
anionlike and takes the name of the
element with an “ide” modification to
the ending.
The prefix is added to the front of each to indicate the number of
each atom.
dinitrogen tetrafluoride
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Naming Chemical Compounds
Binary Molecular Compounds
Whenever the prefix ends in “a” or “o” and the element name
begins with a vowel, drop the “a” or “o” in the prefix.
N2O4
dinitrogen tetroxide
Whenever the prefix for the first element is “mono,” drop it.
CO2
carbon dioxide
CO
carbon monoxide
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Subscript - Prefixes





1 = mono◦ not used on first
nonmetal
2 = di3 = tri4 = tetra5 = penta-
•
•
•
•
•
6 = hexa7 = hepta8 = octa9 = nona10 = deca-
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Name the following
1.
NO2
2.
PCl5
3.
I2F7
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Example – Binary Molecular
dinitrogen pentoxide
Identify the symbols of the elements
nitrogen = N
oxide = oxygen = O
 Write the formula using prefix number for subscript
di = 2, penta = 5
N2O5

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Write formulas for the following
1.
dinitrogen tetroxide
2.
sulfur hexafluoride
3.
diarsenic trisulfide
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Acids
acids are molecular compounds that form H+ when dissolved in
water
◦ to indicate the compound is dissolved in water (aq) is written
after the formula
 not named as acid if not dissolved in water
 sour taste
 dissolve many metals
◦ like Zn, Fe, Mg; but not Au, Ag, Pt
 formula generally starts with H
◦ e.g., HCl, H2SO4

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Acids
Contain H+1 cation and anion
◦ in aqueous solution
 Binary acids have H+1 cation and
nonmetal anion
 Oxyacids have H+1 cation and polyatomic
anion

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Naming Binary Acids
write a hydro prefix
 follow with the nonmetal name
 change ending on nonmetal name to –ic
 write the word acid at the end of the name
 E.g
HCl

HCN
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Naming Oxyacids
if polyatomic ion name ends in –ate, then change ending to –ic
suffix
 if polyatomic ion name ends in –ite, then change ending to –ous
suffix
 write word acid at end of all names
 E.g H2SO4
vs.
H2SO3

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Writing Formulas for Acids
when name ends in acid, formulas starts with H
 write formulas as if ionic, even though it is molecular
 hydro prefix means it is binary acid, no prefix means it is an oxyacid
 for oxyacid, if ending is –ic, polyatomic ion ends in –ate; if ending is
–ous, polyatomic ion ends in –ous
 E.g
Hydrosulfuric acid
vs.
Carbonic acid

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