Download Ionic compounds

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2.3 atomic number, mass number, and isotopes
2.4 the periodic table
2.5 molecules and ions
2.6 chemical formulas
Molecular formula
Molecular models
Ionic formulas
2.7 naming compounds
Ionic compounds
Molecular compounds
Acids and bases
 Homework
Hydrated
p72: 2.26, 2.34, 2.36, 2.44, 2.46, 2.50
p73: 2.57 (a,e,f,g,h,i,j,k,l,m) 2.58(b,c,d,g,h,i,k
2.59(a,b,d,g,h,j) 2.60(a,e,f,g,h,k), 2.94
Dr. LAILA AL-HARBI
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By the end of this chapter you should:
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Know atomic number, mass number, and isotopes
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Be able to distinguish between molecules (diatomic
& polyatomic ) , ions ( cation 7& anions)
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Know different Chemical formulas
Know how to Name Ionic & covalent compounds
Dr. LAILA AL-HARBI
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Protons and electrons are the only particles that have a charge.
Protons and neutrons have essentially the same mass.
The mass of an electron is so small we ignore it.
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Atomic number (Z) = number of protons in nucleus)
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Mass number (A) = number of protons + number of neutrons
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= atomic number (Z) + number of neutrons
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Note that th № of P= № of e-
Dr. LAILA AL-HARBI
Mass Number
A
Atomic Number
Z
X
Element Symbol
Symbols of Elements
All atoms of the same element have
the same number of protons: The
atomic number (Z)
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The mass of an atom in atomic
mass units (amu) is the total
number of protons and neutrons in
the atom.
Dr. LAILA AL-HARBI
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Isotopes are atoms of the same element with different
masses.
Isotopes have different numbers of neutrons.
Hydrogen
1
1
2
1
H
235
92
Deuterium
3
1
H (D)
U
238
92
Tritium
H (T)
U
Chemically, isotopes are not very different from each other.
Dr. LAILA AL-HARBI
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Give the number of protons, neutrons and electrons in each of
the following species
20
11
Na
Mass Number
Atomic Number
Number of electrons
Number of protons
Number of neutrons
22
11
Na
17
8
O
22
20
11 Na
11 Na
17
8
14
6
C
O
14
6
C
20
22
17
14
11
11
8
6
11
11
8
6
11
11
8
6
20-11 = 9 22-11=11 17-8=9 14-6=8
Dr. LAILA AL-HARBI
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a.
b.
c.
d.
The nucleus of an atom
contains:
protons and neutrons.
protons and electrons.
electrons and neutrons.
air.
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a.
b.
c.
d.
Atoms with identical
atomic numbers but
different mass
numbers are called:
mutants.
isomers.
Isotopes.
symbiots.
Dr. LAILA AL-HARBI
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Elements arranged in order of increasing atomic number.
Horizontal Rows in periodic table are called periods.
Vertical Columns are groups or families; elements have similar properties.
representative elements: A Group; transition elements: B Group
These five groups are known by their names
Dr. LAILA AL-HARBI
Main-group elements [1A to 8A]
Dr. LAILA AL-HARBI
Noble Gas
Period
Halogen
Group
Alkali Earth Metal
Alkali Metal
Transition metals
Nonmetals are on the right side of the
periodic table (with the exception of H).
Metalloids border the stair-step line
(with the exception of Al, Po, and At).
Metals are on the left side of the chart
Dr. LAILA AL-HARBI
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Molecules is an aggregate of two or more atoms in a definite
arrangement held together by chemical forces.
I. Diatomic molecules
Some elements exist as diatomic molecules:
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II. Polyatomic molecules that contain more than two atoms
O3 , H2O
Dr. LAILA AL-HARBI
An ion is an atom, or group of atoms, that has a net
positive or negative charge.
cation – ion with a positive charge
If a neutral atom loses one or more electrons
it becomes a cation.
Na
11 protons
11 electrons
Na+
11 protons
10 electrons
anion – ion with a negative charge
If a neutral atom gains one or more electrons
it becomes an anion.
Cl
17 protons
17 electrons
ClDr. LAILA AL-HARBI
17 protons
18 electrons
A monatomic ion contains only one atom
Na+, Cl-, Ca2+, O2-, Al3+, N3A polyatomic ion contains more than one atom
OH-, CN-, NH4+, NO3How many protons and electrons are in
119
50
4+
Sn
?
50 protons, 46 (50 – 4) electrons
78
34
How many protons and electrons are in Se
34 protons, 36 (34 + 2) electrons
Dr. LAILA AL-HARBI
2-
?
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a.
b.
c.
d.
Positive ions are called:
positrons.
anions.
cations.
nucleons.
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a.
b.
c.
d.
The elements located in
group 7A of the periodic
table are called:
alkali metals.
noble gases.
chalcogens.
halogens.
What are the ions present in the compound (NH4)2SO4 ?
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NH3, H2, and SO2
N3–, H+, S2–, O2–
NH42+ and SO4–
NH4+ and SO42– (3 IONS)
(NH4+)2 and SO42–
Dr. LAILA AL-HARBI
Selenium (34Se) element is:
(a) a nonmetal
(b) found in group 6A
(c) both a and b
Which of the following sets of
elements is expected to have
similar chemical properties?
a) Sulfur and phosphorous
b) Sulfur and oxygen
c) Sulfur and argon
Gallium (Ga) element is found
in the periodic table in(a)
period 3, group 1B
(b) period 3A, group 4
(c) period 4, group 1A
(d) period 4, group 3A
Dr. LAILA AL-HARBI
Molecular formulas give the actual numbers and types
of atoms in a molecule.
E.g. CH4, H2O2, C2H4, C6H12O6
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Empirical formulas give the smallest whole number
ratio of atoms in a molecule. The empirical formula of
many compounds is the same as the molecular formula
E.g. CH4, HO, CH2, CH2O
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Ionic formulas: the number of electrons lost & gained
must be equal, so + and -charge cancel out.
Dr. LAILA AL-HARBI
Write the molecular formula of methanol and chloroform
shown in the figures
H
H
O
Cl
C
Cl
Cl
C
H H
Molecular formulas
CH4O
CH3OH
H
Molecular formulas
CHCl3
Dr. LAILA AL-HARBI
molecular
empirical
1
H2O
6
H2O
CH2O
C6H12O6
3
O3
O
2
N2H4
NH2
Dr. LAILA AL-HARBI
Write the Empirical formulas for the following molecules
 Acetylene C2H2 divided by 2 CH
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Glucose C6H12O6 divided by 6 CH2O
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Nitrous oxide N2O , the Empirical formulas is same as
molecular formula N2O
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Caffeine C8H10N4O2 divided by 2 C4H5N2O
Dr. LAILA AL-HARBI
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1) Write down formulas of ions
2) Combine the smallest number of ions to give the
charge sum equal to 0; if the charges are not equal, find
the lowest common multiple
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E.g. Predict the formula for the compound formed from
the following elements:
Potassium bromide K+ Cl– = KCl
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Zinc iodide
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Aluminum oxide
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Zn+2 I– = ZnI2
Al+3 O–2 = Al2O3
2 × +3 = +6
Al3+
3 × -2 = -6
Al2O3
O2Dr. LAILA AL-HARBI
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Write the formula of
magnesium nitride?
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Write the formula of
a)chromium sulfate ,
b)titanium oxide?
2 × +3 = +6
3 × +2 = +6
2 × -3 = -6
3 × -2 = -6
Cr 2(SO4)3
SO42-
Cr 3+
Mg 3N2
2 × +4 = +8
Mg 2+
Examples 2.4
4 × -2 = -8
Ti 2O 4
N3-
Ti 4+
O 2-
Practice exercise 2.4
Dr. LAILA AL-HARBI
 Ionic
compounds
 Molecular compounds
 Ionic compounds
consist of metals ( positive ions (cations) and negative ions
(anions).
A. Naming Cations
1. Fixed charge metals:
Cations have same name as the metal element. (Groups1A, 2A,
3A , transition metals ) have specific charge.
Ag+ silver ion
Zn2+ zinc ion ,
Al3+ Aluminum ion
Li+ lithium ion
Ca2+ calcium ion
Dr. LAILA AL-HARBI
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2. Variable charge metals:
If the metal has more than one oxidation state, the charge is
indicated by a Roman numeral in parenthesis after the metal
name.
Most of the transition metals are variable charge metals.
E.g. Common metals which exist in more than one positive
state:
Fe2+ iron(II)
,Au+ gold(I), Cu+ copper(I) ,
Fe3+ iron(III) Au3+ gold(III) Cu2+ copper (II)
Hg2 +2mercury(I)
Hg2+ mercury (II)
3. Polyatomic cations: consist of nonmetals:
H3O+ hydronium ion
NH4+ ammonium
Dr. LAILA AL-HARBI
Variable charge metals
Dr. LAILA AL-HARBI
Some Cations of variable charge have name for each
oxidation state
 Example
Fe2+ iron(II) ferrous , Fe3+ iron(III) ferric
Cu+ copper(I) cuprous , Cu2+ Copper (II) cupric
Hg2 +2mercury(I) mercurous
Hg2+ mercury (II) mercuric
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Dr. LAILA AL-HARBI
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1. monoatomic anions: change ending to -ide
E.g. Oxygen→ Oxide
Sulfur → Sulfide
Hydrogen →Hydride
chlorine → Chloride
Florine → Floride
Bromine → Bromide
Polyatomic anions: most end in -ate or -ite; usually contain O
(oxy)
 Know polyatomic anions on handout.
 Carbonate CO3-2 , Nitrate NO3- , Sulfate SO4-2 ,
 Phosphate PO4-3
Cyanide CN- , Hydroxide OH- , Oxide O2-2
See table 2.3
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Dr. LAILA AL-HARBI
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Ionic compounds names start with the positive ion
(metal) (include Roman numeral in parenthesis ONLY IF
metal has variable charge) followed by the negative ion
(nonmetal).
NaCl
Sodium Chloride
BaCl2
Barium Chloride
K2O
Potassium oxide
KNO3
Potassium Nitrate
Na2CO3
Sodium Carbonate
FeCl2
Iron(II) Chloride → ferrous Chloride
FeCl3
Iron(III) Chloride → ferric Chloride
Cr2S3
Chromium(III) Sulfide
(NH4)3PO4 Ammonium Phosphate
Dr. LAILA AL-HARBI
Dr. LAILA AL-HARBI
Metals
Positive ion
Cation
Non metals
Negative ion
Anion
( 1A , 2A ,3A & transition metals)
Fixed
charge
metals
Cations have
same name as the
metal element
Ag+ silver ion ,Zn2+ zinc ion ,
Al3+ Aluminum ion , Li+ lithium
ion , Ca2+ calcium ion
monoatomic
anions
Variable
charge
metals (STOCK SYSTEM)
If the metal can form more than 1 cation, the
charge is indicated by a Roman numeral in
parenthesis after the metal name.
Polyatomic
anions
Fe2+ iron(II)
,Au+ gold(I),
Cu+ copper(I) ,
Fe3+ iron(III) Au3+ gold(III) Cu2+ copper (II)
Hg2 +2mercury(I)
Hg2+ mercury (II)
Dr. LAILA AL-HARBI
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Name the following compounds
Cu(NO3)2
Cupper(II)nitrate
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Name the following
compounds
PbO
Lead(II) oxide
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Li SO3
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Lithium sulfite
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KH2PO4
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Potassium dihydrogen phosphate
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NH4ClO3
NH4 is not metal but NH4ClO3
ionic compound
Ammonium chlorate
Example 2.5
PRACTIES EXERICISE 2.5
Dr. LAILA AL-HARBI
Write the chemical formula
for the following compounds
 Mercury(I)nitrite
Hg2 (NO2)2
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Cesium sulfide
Ce2S
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Write the chemical formula for
the following compounds
Rubidium sulfate
Rb 2 SO4
Barium hydride
BaH 2
Calcium phosphate
Ca3 (PO4)2
Example 2.6
PRACTIES EXERICISE 2.6
Dr. LAILA AL-HARBI
Molecular compounds
• nonmetals or nonmetals + metalloids
• common names
 H2O water
 NH3 ammonia
 CH4 methane
 H2S hydrogen sulfide
 SiH4 silane
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 B2H6 diborane
1) Name 1st element & use a prefix (table 2.4) to
indicate the number of atoms.
.
2)Name 2nd element & include prefix for number
of atoms (see table 2.4).
3) Change ending of 2nd element to –ide.
Dr. LAILA AL-HARBI
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Note that mono- is never used for the first element
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For oxides, the ending “a” in the prefix is omitted.
N2O4 dinitrogen tetroxide not (dinitrogen tetraoxide)
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For oxides, the ending “o” in the prefix is omitted.
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N2O dinitrogen monoxide not (dinitrogen monooxide )
Dr. LAILA AL-HARBI
Molecular Compounds
HI
hydrogen iodide
NF3
nitrogen trifluoride
Br2O7
Dibromine heptaoxide
SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
ICl3
Iodine trifchloride
Dr. LAILA AL-HARBI
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Iron (III) sulfide → Fe2S3
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Tetrasulfur octoxide → S4O8
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Silver dichromate → Ag2Cr2O7
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Aluminum hydride → AlH3
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Sodium phosphide → Na3P
Cobalt (III) nitrite → Co(NO2)3
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Diphosphorus pentasulfide → P2S5
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Sulfur hexafloride SF6
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Dinetrogen pentoxide P2O5
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Disulfur pentafluoride S2F10
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Tin(IV) chloride → SnCl4
Chromium(III) thiocyanate →
Cr(SCN)3
Lead(IV) oxide → PbO2
Calcium phosphite →Ca3(PO3)2
Arsenic(V) sulfide → As2S5
manganese(VII) oxide → Mn2O7
IONIC COMPOUNDS
MOLECULAR COMPOUND
Dr. LAILA AL-HARBI
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Name the following compounds
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Cu(NO3)2
Cupper(II)nitrate
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KH2PO4
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Potassium dihydrogen phosphate
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NH4ClO3
NH4 is not metal but NH4ClO3 ionic compound
Ammonium chlorate
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Dr. LAILA AL-HARBI