Lead II carbonate
SnO2
Period 8
Day 5 115
Acid - Compound that yields H+ ions (always
starts with an H) – molecular compounds that
act like ionics
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Non-binary: ate ending becomes ic,
ite ending becomes ous
HF
HBr
HNO3
HNO2
Naming:
Acids are named for their anions
Binary: hydro – anion base – ic
ending – the word “acid”
Non-binary: ate ending becomes ic,
ite ending becomes ous
Hydrochloric acid
Sulfurous acid
sulfuric acid
hydrofluoric acid
carbonic acid
HC2H3O2
HCl
H2SO3
# 2.57 (parts a-g) AND 2.58 (parts
a-e) AND 2.59 (parts a-f)
BINDERS!!!
Lead II carbonate
Phosphoric acid
H2SO4
SnO2
Periods 1 + 3
Day 5 11-5
Phosphorous acid
nickel III oxide
Pb(CO3)2
HClO3
Periods 3 + 8
Day 6 11-6
Ionic Compounds &
Polyatomic Ions
Oxyanions – polyatomic ions that contain
oxygen
ate = ending for most common ion (ClO3- Chlorate)
ite = ending for one less oxygen (ClO2- Chlorite)
hypo = prefix for another less oxygen (ClO Hypochlorite)
per = prefix for one more than most common (ClO4Perchlorate)
Molecule – group of atoms united by
covalent bonds (molecules =
molecular substance)
Empirical - simplified ratio
Molecular - How many atoms in a
single molecule (not
always a simplified ratio,
glucose = C6H12O6)
Empirical - Simplified ratio
Molecular - How many atoms in a
single molecule (not
always a simplified ratio,
glucose = C6H12O6)
Structural - Specifies which atoms are
bonded to each other
(organic chem)
Molecular Element – molecule of
atoms of same element – NOT a
compound - like O2, Cl2, O3
H BrONClIF = diatomic molecules
- these elements naturally occur
as diatomic molecules and not
singular atoms
Binary Molecular Compounds
Based on Prefixes
1. Less electronegative first – prefix only if
more than one atom
2. Second element – prefix, root of name,
ending ide (if only two elements)
3. o or a @ the end of prefix is dropped if name
begins with a vowel (monooxide,
monoxide)
Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca
1
2
3
4
5
6
7
8
9
10
Binary
Molecular
Compounds
– prefix
system
Binary Molecular Compounds
Write the Name:
N2O5
Dinitrogen pentoxide
SbF3
Antimony trifluoride
Write the Formula:
Germanium tetraiodide
GeI4
diphosphorous trioxide P2O3
Binary Molecular Compounds
Write the Name:
As2O5
diarsenic pentoxide
ICl3
iodine trichloride
Write the Formula:
carbon tetraiodide
CI4
dinitrogen trioxide
N2O3
Phosphorous acid
nickel III oxide
Pb(CO3)2
HClO3
Period 1
Day 6
11-6
Day 1 11-9
For each compound below, what
type is it (covalent, acid, or ionic),
and write the name.
NO2
HNO3
Co3(PO4)2
Green = halogens
Black = carbons
White = hydrogens
Red = oxygen
Blue = nitrogen
Grey / purple = metal
Formulas
Names
Day 2 11-10
For each compound below, what
type is it (covalent, acid, or ionic),
and write the name.
HC2H3O2
Cu3PO3
SF6
• Molecular compounds
− Nonmetals or nonmetals + metalloids
− Common names
− H2O, NH3, CH4
− Element furthest to the left in a period
and closest to the bottom of a group on
periodic table is placed first in formula
− If more than one compound can be
formed from the same elements, use
prefixes to indicate number of each
kind of atom
− Last element name ends in -ide
23
Molecular Compounds
HI
hydrogen iodide
NF3
nitrogen trifluoride
SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
24
Example 2.7
Name the following molecular compounds:
(a) SiCl4
(b) P4O10
Example 2.7
Strategy
We refer to Table 2.4 for prefixes.
In (a) there is only one Si atom so we do not use the prefix
“mono.”
Solution
(a)Because there are four chlorine atoms present, the
compound is silicon tetrachloride.
(b)There are four phosphorus atoms and ten oxygen atoms
present, so the compound is tetraphosphorus decoxide. Note
that the “a” is omitted in “deca.”
Example 2.8
Write chemical formulas for the following molecular
compounds:
(a) carbon disulfide
(b) disilicon hexabromide
Example 2.8
Strategy
Here we need to convert prefixes to numbers of atoms (see
Table 2.4).
Because there is no prefix for carbon in (a), it means that there
is only one carbon atom present.
Solution
(a) Because there are two sulfur atoms and one carbon atom
present, the formula is CS2.
(b) There are two silicon atoms and six bromine atoms present,
so the formula is Si2Br6.
29
An acid can be defined as a substance that yields
hydrogen ions (H+) when dissolved in water.
For example: HCl gas and HCl in water
•Pure substance, hydrogen chloride
•Dissolved in water (H3O+ and Cl−),
hydrochloric acid
30
31
An oxoacid is an acid that contains hydrogen,
oxygen, and another element.
HNO3
nitric acid
H2CO3
carbonic acid
H3PO4
phosphoric acid
32
Naming Oxoacids and Oxoanions
33
The rules for naming oxoanions, anions of
oxoacids, are as follows:
1. When all the H ions are removed from the “-ic”
acid, the anion’s name ends with “-ate.”
2. When all the H ions are removed from the “ous” acid, the anion’s name ends with “-ite.”
3. The names of anions in which one or more but
not all the hydrogen ions have been removed
must indicate the number of H ions present.
For example:
– H2PO4- dihydrogen phosphate
– HPO4 2- hydrogen phosphate
– PO43- phosphate
34
35
Example 2.9
Name the following oxoacid and oxoanion:
(a) H3PO3
Example 2.9
Strategy To name the acid in (a), we first identify the reference
acid, whose name ends with “ic,” as shown in Figure 2.15.
Solution
(a)We start with our reference acid, phosphoric acid (H3PO4).
Because H3PO3 has one fewer O atom, it is called phosphorous
acid.
A base can be defined as a substance that yields
hydroxide ions (OH-) when dissolved in water.
NaOH
sodium hydroxide
KOH
potassium hydroxide
Ba(OH)2
barium hydroxide
38
Hydrate – ionic substances that
absorb water into their solid
structures
Anhydrous substance – opposite of
hydrates (water-free)
1. Name ionic compound
2. use prefix to name hydrate
Name
CuSO4 • 5 H2O
Copper (II) sulfate pentahydrate
MgSO4 • 7 H2O
Magnesium sulfate heptahydrate
Formula
Calcium sulfate dihydrate CaSO4 • 2 H2O
Hydrates are compounds that have a specific
number of water molecules attached to them.
BaCl2•2H2O
barium chloride dihydrate
LiCl•H2O
lithium chloride monohydrate
MgSO4•7H2O
magnesium sulfate heptahydrate
Sr(NO3)2 •4H2O
strontium nitrate tetrahydrate
CuSO4•5H2O
CuSO4
41
42
Organic chemistry is the branch of chemistry that
deals with carbon compounds.
Functional Groups:
H
H O
H
H
C
OH
H
methanol
H
C
NH2
H
methylamine
H
C
C
OH
H
acetic acid
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