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Students ScoreBooster Series Videos
WAEC, SSCE, GCE, JAMB (UTME),
NECO and NABTEB
Chemistry
Presented by
Chemical Combination I
A.A.S Lateef
Chemical combination
• Learning objectives, at the end of this lecture,
Students should be able to explain the concept of bonding.
Students should be able to apply the concept of valency in
forming simple compounds.
Naming of simple compounds is also expected
Properties of the compounds formed should be highlighted and
adequately explained.
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Why do atoms form bond
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Sodium and chlorine are both elements.
When sodium is heated and placed in a jar
of chlorine, it burns with a bright flame
The result is a white solid that has to be scraped
from the sides of the jar. It looks completely
different from the sodium and chlorine.
So a chemical reaction has taken place. The white solid is sodium chloride.
Atoms of sodium and chlorine have bonded (joined together) to form a compound. The
equation for the reaction is:
sodium + chlorine ---------sodium chloride
Why do atoms form bonds
Looking at the elements of the group 0
Atoms bond with each other in order to gain a stable arrangement of outer -
shell electrons, like the atoms of Group 0 (or 8).
In other words, they bond in order to gain 8 electrons in their outer shell (or
2, if they have only one shell).
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How sodium and chlorine form ions
Sodium has only one electron in the outermost shell, so it loses one
electron to obtain a stable configuration of 8 outer electrons.
For Chlorine, it attains its stable 8 electrons by accepting 1 electron
because it has 7 electrons in its outermost shell.
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Ions
An atom becomes an ion when it loses or gains electrons.
An ion is a charged particle. It is charged because it has an unequal
number of protons and electrons.
Valency: This is defined as the combining power of elements. It is, in other
words, the ions of the elements. For radicals, the valency is the power on
the group that makes up the radical.
Sometimes the group to which any element belongs can be used to
determine the valency of such elements.
Examples: Na+, Cl-, K+, Mg2+, NO3- etc
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IA family: Each element has one electron in its outermost shell, so it forms
ions with the loss of its one electron.
IIA family: Each element has two electrons in its outermost shell, so it forms
ions with the loss of the two electrons.
IIIA family: Each element has three electrons in its outermost shell, so it
forms ions with the loss of the three electrons.
VA family: Each element has five valence electrons, so it gains three
electrons to form an anion with a 3- charge.
VIA family: Each element has six valence electrons, so it gains two electrons
to form an anion with a 2- charge.
VIIA family: Each element has seven valence electrons, so it gains one
electron to form an anion with a 1- charge.
Determining the number of electrons that members of the transition metals
(the B families) lose is more difficult. In fact, many of these elements lose a
varying number of electrons so that they form two or more cations with
different charges.
Forming Chemical Bond
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A chemical bond is the physical process that causes atoms and molecules to
be attracted to each other, and held together in more stable chemical
compounds.
There are two ways of forming chemical bond; by balancing the charge and
crisscross rule.
Balancing the charges
The charges on the cations of the participating elements must be balanced
with that on the anion and vice versa.
For example, consider the reaction between calcium and chlorine to form
calcium chloride; (i) Ca = 2+, Cl = -1. Forming the compound, each Ca
atom requires 2 atoms of chlorine to form a neutral compound, hence we
have CaCl2. (ii) Sodium with sulfur to form sodium sulfide reacts as
follows: Na = +1, S = 2-. Two sodium atoms is required to react with one
atom of Sulphur forming Na2S.
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THE CRISSCROSS RULE A quick way to determine the formula of an ionic compound is to use the
crisscross rule: Take the numerical value of the metal ion’s superscript
(forget about the charge symbol) and move it to the bottom right-hand side
of the non-metal’s symbol — as a subscript and vice versa. (Note that if
the numerical value is 1, it’s just understood and not shown.)
Forming Compounds (Crisscross rule)
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Consider aluminium reacting with oxygen as illustrated below;
Compounds involving polyatomic ions work in exactly the same way. For
example, here’s the compound made from the ammonium cation (NH4+) and
the sulfide anion (S2–): (NH4)2S
NB: Because two ammonium ions (two positive charges) are needed to
neutralize the two negative charges of the sulfide ion, the former is enclosed in
the parentheses and a subscript 2 is added.
Also, after the crisscross rule is used, the subscripts are reduced by a common
factor, if possible, to get the right formula. e.g. Mg2O2 = MgO.
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Class Exercise
Using the crisscross rule together with figures on pgs 10 & 11,
write at least 12 ionic compounds.
1. Electrovalent (Ionic) Bonding
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Electrovalent bond is a type of bond that involves transfer of electron
between a highly electropositive metal and electronegative non-metal. e.g
sodium and chlorine. It can also involve a highly electropositive metal and
a moderately electronegative non-metal. e.g magnesium and oxygen,
potassium and hydrogen etc. The electronegativity value is the key here.
The electronegativity value difference must be wide enough to permit
transfer of electrons between the participating elements.
Electrovalent (Ionic) Compounds
The compounds which contain ionic or electrovalent bonds are known as
Electrovalent or Ionic Compounds. Mainly electrovalent compounds are
formed due to reaction between highly electropositive and highly
electronegative atoms. e.g. sodium/ potassium/calcium/magnesium with
chlorine/fluorine.
Creating Ionic Compounds Ionic bonding, the bonding that holds the cations and anions together, is
one of the two major types of bonding in chemistry.
NB: An ionic bond occurs between a metal and a non-metal. The metal
loses electrons (to becomes a positively charged cation), and a non-metal
gains those electrons (to become a negatively charged anion). The ions
have opposite charges so they’re attracted to each other. This attraction
draws them together into a compound.
The transfer of an electron creates ions — cations (positive charge) and
anions (negative charge). Opposite charges attract each other, so the cations
and anions may come together through an ionic bond. An ionic bond is a
chemical bond (a strong attractive force that keeps two chemical elements
together) that comes from the electrostatic attraction (attraction of opposite
charges) between cations and anions. Together, the ions form a compound.
For instance, consider the reaction of sodium with chlorine done earlier!
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Creating Ionic Compounds (cont’d)
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For instance, sodium, a metal, can fill its octet and achieve stability by
losing an electron. Chlorine, a non-metal, can fill its octet by gaining an
electron. If the two are in the same container, then the electron that sodium
loses can be the same electron that chlorine gains. The Na+ cation attracts
the Cl– anion and forms the compound NaCl, sodium chloride.
Compounds that have ionic bonds are commonly called salts. In sodium
chloride — table salt — a crystal is formed in which each sodium cation is
surrounded by six different chloride anions and each chloride anion is
surrounded by six different sodium cations.
Different types of salts have different crystal structures.
Characteristics of electrovalent compounds
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Crystal Structure: In solid state of electrovalent compounds, anions and
cations are arranged in regular manner called crystals.
Electrical Conductivity: In molten and solution forms electrovalent
compounds conduct electricity because ions flows in molten and
solution forms.
Appearance: Ionic or electrovalent compounds are generally hard and
their hardness increases with increasing ionic charge and decreasing
distance between ions.
Solubility: Ionic or electrovalent compounds are soluble in polar
solvents like water and insoluble in non polar solvents like benzene,
ether, alcohol.
Melting point and boiling point: Electrovalent or ionic compounds have
high Melting and boiling points because large amount of energy is
needed to break strong ionic bonds.
Naming ionic compounds
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In naming inorganic compounds, the name of the metal is put first which
is then followed by that of the non-metal with -ide at the end (for
compounds involving monatomic ions).e.g. MgO == Magnesium Oxide.
For polyatomic radical-containing compound, the principle is the same
except that –ide is not necessary. e.g. (NH4)2CO3 ----ammonium
carbonate.
For metals with varying oxidation state, e.g. transition metals, the name of
the metal is written first and the oxidation state is put in parenthesis
followed by the name of the attachment. e.g. Fe(CN)3: iron(III) cyanide
Elements react together to attain a complete and stable octet (8 electrons) or
duplet (2 electrons) configuration.
Formation of a compound results from reaction between elements.
Compound formation either involves transfer or sharing of electrons.
Valency is the combining power of element.
Metals lose electrons while non-metals gain electrons.
The number of electron lose by metal is the valency while the one gained
by non-metal is the valency of that non-metal.
Ionic bonding involves lose of electron(s) by the metal and transfer of such
electron(s) to the non-metal.
Compounds are formed by interchanged of charges and the charges need to
be balanced for such compounds to be neutral.
Ionic compounds are electrolyte in molten and solution forms. They are
soluble in polar solvents etc
The name of the metal is mentioned first and the oxidation number is put in
parenthesis (if required) before the name of the negative ion or radical.
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Points to note:
Examples
•
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JAMB 1988, Q2
JAMB 1998, Q9
The diagram above represents element
that can combine with chlorine to form
a. Covalent bond
b. electrovalent bond
c. Hydrogen bond
d. Coordinate bond
Examples
•
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JAMB 1988, Q2
JAMB 1998, Q9
The diagram above represents element
that can combine with chlorine to form
a. Covalent bond
b. electrovalent bond
c. Hydrogen bond
d. Coordinate bond
Solution
M =3, X= 4, by crisscross
rule, the compound formed
is M4X3. Option C.
Hint: The element has 2
valence electrons, hence a
group metal. Reacting with
Cl will form electrovalent
bond. Option B
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