PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph
Course Number:
Course Title:
Instructor:
PH CHEM 101 Lecture
8:30-10:30 Tuesday
Pharmaceutical Inorganic Chemistry (With Qualitative Analysis)
Grace M. Bayeng, RPh.
Modular Learning Activity # 1
Topic: Review of Inorganic Chemistry
A. Learning Outcomes
At the end of this module, you should be able to:
1. Demonstrate competence in the basic concepts and principles of chemistry
2. Demonstrate understanding of chemical, physical and biological processes relevant to pharmaceutical
sciences
3. Demonstrate an appreciation of mathematics and its relevance to science
B. Learning Content
Chemistry is the study of matter and energy and the interactions between them. Chemistry tends to focus
on the properties of substances and the interactions between different types of matter, particularly reactions
that involve electrons.
MATTER - is anything that occupies and has mass. It is the stuff or material of which the earth and all that it
contain.
One of the principal concerns of chemists is to study the composition and structure of matter.
Composition refers to the identity and quantity of the components (ingredients) of matter, and structure
refers to the physical arrangement of the components within matter. Collectively, the composition and
structure determine the properties, or characteristic traits of matter. The space occupied by an object is
called volume. The volume of an object depends upon the size and shape of the object.
Example of matter; water, air, coal, soil oxygen, stone, rocks.
Matter is made up of two or more substances. Substance is a material with a definite composition or
a special kind of matter which can be easily distinguish from the other kind. Ex. Water, sugar, alcohol.
Each type of matter has its own unique set of properties. Thus, different types of matter are
distinguished by their physical appearance and personality traits.
Two General Groups of Properties of Matter
1. Physical property is a characteristic of an individual substance can be determined without
changing the composition of that substance. Examples of physical properties are color, hardness,
electrical conductivity, physical state, melting point, boiling point, and tensile strength.
2. Chemical property describe how the composition of a substance changes does not change when
the substance interacts with other substances or energy forms. Terms used to describe some
chemical properties are reactive, inert, unstable, and combustible. Chemical properties are
observed when a substance changes composition. Examples, paper burns in air, iron rusts, silver
tarnishes, TNT explodes.
Examples: Change in state, density, shape, magnetic properties, conductivity
AY 2020-2021 PH CHEM 1O1 By Michelle T. Onoza, RPh, MS Pharmacy
Page
1. Physical change – physical properties of a substance are altered but the composition remains the
same. No new substance is formed when physical change takes place.
1
Two Kinds of Changes of Matter
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph
2. Chemical change – change in the composition of a substance yielding a new substance. The
composition and properties of the new substance are entirely different from their original
substance.
States of Matter
All matter on earth exist in three physical states: solid, liquid, and gaseous. Various physical
properties distinguished the 3 states of matter are shape, volume, average density, structure, viscosity
and compressibility.
Viscosity is a measure of the resistance to flow Substance with high viscosity does not flow
readily, whereas substance with low viscosity flows more readily.
Compressibility is the measure of the decrease in volume of a substance with an applied pressure.
Three States of Matter
1. Solids have fixed shapes that are independent of their container. The volume of a solid is also fixed, and
does not change when a pressure is exerted. Solids are almost completely incompressible. Solids have high
densities. Particles within solids are usually packed closer than those in liquids or gases. Solid have
practically no ability to flow because the particles that compose a solid are very tightly bonded.
2. Liquids are quite different from solids in many respects, but the two share some characteristics. Liquids are
essentially incompressible. When placed in a container, liquids assume the shape of the container to the
level they fill. Liquids have no fixed shape but have fixed volume. Liquids have lower viscosities than
solids. Liquids are significantly more fluid than solids.
3. Gases have no fixed volume and shape. Gases completely fill the volume of the container, are compressible.
Liquids have lowest densities and lowest viscosities.
Changes of State
1. Melting point – the characteristic temperature at which a particular solid changes to a liquid.
2. Freezing point – the temperature at which a liquid becomes a solid.
3. Boiling point – the temperature at which a liquid change to their vapors. A vapor is the gaseous phase of a
substance.
4. Condensation – the change in the opposite direction from vapor to liquid.
5. Sublimation – the temperature at which solids change directly to their vapors without going through the
state.
Classification of Matter
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Two Major Classes of Matter
1. Pure substance is classified as pure if it meets the following three criteria:
 It has the same composition throughout the sample
 Its components are inseparable using physical methods.
 Changes of state occur at a constant temperature.
 Characteristics
o Percentage composition always the same from sample to sample
o Melt/boil at a characteristic temperature
 note: some compounds decompose before melting or boiling!
2. Mixtures are more complex than pure substances because they are composed of two or more pure
substances that are physically associated.
Three criteria are used to classify a mixture:
2
Matter is found in many different forms throughout the earth.
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph



Its composition is variable.
Its components may be separated by physical methods.
Changes of state occur over a range of temperature.
Subdivisions of Pure substance
1. Elements are basic units of matter. All of the other types of matter contain elements. Today, we
know of approximately 110 elements. About 92 elements occur in nature, and the remaining are
synthetic. At 25 oC, 97 elements are solids, 2 are liquids, and 11 are gases. All the known elements
are listed, using their symbols, in the Periodic table.
Example; H, Cl. O. Na, Br, Ca, He, F, N,
o
elements
 not chemically decomposable into other elements
 properties do not vary
2. Compounds are more complex than elements. Compounds are chemical combinations of elements.
They can only be separated into their component elements by chemical means. Molecule is the
smallest subdivision of a compound and a chemical combination of atoms.



Example; water, sodium chloride, rust, sugar, alcohol.
o compounds
 elements combined chemically in law of definite proportions
 properties do not vary
Elements
elements are made of atoms that all have the same atomic number
obtaining elements from compounds involves chemical change
o electrolysis decomposes some compounds into elements
o some elements displace others from compounds
writing element symbols
o first 1-2 distinguishing letters in name used for symbol
o only the first letter is uppercase!
o memorize symbols derived from ancient names:
Classification of Elements:
1. Metals are base forming elements whose atoms can lose electrons and form positive ions. Metals are usually
solid elements with a silvery gray color. Metals share a set of common properties:
 They have luster or shiny surface.
 They have a high average densities
 They are excellent conductors of heat and electricity
 They are malleable - can be hammered into thin sheets
 They are ductile - can be drawn into a thin wire
Names of metals end in -um or -ium
Example: Sodium, aluminum, calcium, Ferrum, barium
3. Metalloids have properties intermediate between metals and non-metals. They exhibit both the metallic and
non-metallic properties.
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3
2. Non-metals are acid forming elements whose atoms can gain electrons and form negative ions. They posses
properties that, in many cases are opposite to those of a metals.
Names of non metals ends in on, ine & gen
Example: hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, carbon
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph
4. Gases – are substances, which are light and usually naked to the human eye.
Classification of compounds:
1. Acids - compounds containing weekly bonded H+ atoms. It is a proton donor. A substance that yields
hydrogen ions when dissolves in water; a molecular or ionic substance from which under certain conditions,
protons can be detached. The word acid comes from the Latin word which means “sharp”. It is a hydrogen
compound whose hydrogen may be replaced by a metal. The hydrogen is written first in the formula and the rest
of the compound is generally non metal or an acid radical.
Kinds of acid according to the number of hydrogen content
1. Monoprotic acid – acid containing 1 hydrogen atom
Example: HCl, HNO3, HBr, HI, HF
2. Diprotic acid – acid containing 2 hydrogen atoms
Example: H2SO4, H2CO3, H2S
3. Triprotic acid – acid containing 3 hydrogen atoms
Example: H3PO4, H3IO4
Acid are classified according to the number of elements, chemically combined:
1. Binary acid – acid containing 2 elements, chemically combined
Example: HI, HBr
2. Ternary acid – acid containing 3 elements, chemically combined
Example: HNO3, HNO2, H2CO3
Characteristics of acid:
1.
2.
3.
4.
5.
It has a sour taste, example, vinegar owes its taste to acetic acid
Turns blue litmus to red
Reacts with metals producing salts and yielding hydrogen gas
Neutralize hydroxide bases to form salt and water
They are corrosive
2. Bases – any substance, molecular or ionic which accepts protons from an acid. It is called proton acceptors.
These are compounds identified by the presence of OH group.
Example: NaOH, KOH, Ca(OH)2 or Ba(OH)2
Characteristics of a base
1.
2.
3.
4.
Taste bitter
Turn red litmus paper to blue
Neutralize acid to form salt and water
They are slippery (soapy) to the touch
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4. Oxide – is a compound containing oxygen and only other element; is a compound of oxygen with metal and
non metal.
Example: MgO, CO2, BaO, K2O
Kinds of Oxide:
4
3. Salts – defined as an ionic compound cation and anion. Contain metal and non metal.
Example: NaCl, KNO3, CaSO4, CuCO3.Cu(OH)2, NaHPO4.NaHSO4
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph
1. Metallic oxide or ionic oxide – are formed by the union of oxygen with the metals of electronegativity.
2. Non metallic oxide or molecular oxide are also called acid anhydride because when non-metallic oxides
are added to water, it produces an acids.
C
CO2
+
+
O2
H2O
CO2
H2CO3
Mixtures:
Many possibilities exist when a mixture prepared. Two substances can be mixed in virtually any
proportion. For example, a mixture of sugar and water might contain 1 g sugar in 100 ml of water or 15
g of sugar in 80 ml of water, or many other possible combinations. Examples: Milk, gasoline, asphalt,
ocean water, granite and air.
Two Classes of Mixtures:
1. Homogeneous mixtures – is a word derived from the Greek words homo, which means “the same” or
“equal” genus which means kind” or “structure.” Homogeneous mixtures are also called solutions. Only
one phase is found in homogeneous mixtures.
Example: let’s consider a sugar water solution. It is prepared by mixing solid sugar and liquid water. After the
sugar dissolves, a homogeneous mixture results. When looking at sugar water, you can not tell if it is pure or a
solution
Phase is an observable region of matter a composition different from the surrounding medium.
2. Heterogeneous mixtures – derived from “hetero” which is a prefix which means “different”, It is one
that exhibits more than one phase
Example: Granite which is compose of quartz, feldsfars, and mica. When sand is added to water, the sand does
not dissolves; it just falls he bottom of the water. When observing sand and water, you see the solid sand phase,
the liquid water phase. Oil and water, salt and sand.
Processes use to separate components of mixtures:
1. Distillation – a process of changing liquid water into water vapor. Or a chemical separation
procedure in which one component is selectively vaporized and condensed to remove it from other
substance.
2. Filtration – is a method used to separate some heterogeneous mixtures.
Classifying properties as extensive or intensive. Extensive properties change when sample size
changes; intensive properties don't.
100.0 g
10.0 g
Volume of
water
0.100 L
0.010 L
Temperature
of water
25 °C
25 °C
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Mass of water
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph


Density of
1.00 g/Ml
1.00 g/mL
water
A phase is a region with homogeneous (uniform) properties
conversions between states are called "phase transitions" or "changes of state"
States of Matter
Gas



Liquid


low density
easy to
expand/compress
fills container

Solid


high density
hard to
expand/compress
takes shape of
container

high density
hard to
expand/compress
rigid shape
SUMMARY ON THE CLASSIFICATION OF MATTER
Uniform
properties?
Fixed
composition?
YES
NO
chemically
YES
decomposable?
YES
NO
NO
HOMOGENEOUS
MIXTURE
HETEROGENEOUS
MIXTURE
COMPOUND
ELEMENT
Schematic Diagram on the Classification of Matter
MATTER
PURE
SUBSTANCES
COMPOUNDS
HOMOGENEOUS
(Solutions)
HETEROGENOUS
SALTS
(eg. NaCl, FeCl2...)
COLLOIDS
(eg. Foams..)
NON-METALS
(eg. S, Cl, F...)
ACIDS
(eg. HCl, HI ...)
SOLS
(eg. Aerosols)
METALOIDS
(eg. Si, As...)
BASES
(eg. KOH,
NaOH...)
GELS
(eg. Gelatines)
INERT GASES
(eg. Ne, He, Kr...)
OXIDES
(eg. BaO, CO2 ...)
SUSPENSIONS
(eg. Drug susp.)
Element symbols derived from ancient names
English Name
Symbol
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METALS
(eg. Zn, Au, Ag..)
Ancient Name
Page
ELEMENTS
MIXTURES
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph



Sb
Stibium
Copper
Cu
Cuprum
Gold
Au
Aurum
Iron
Fe
Ferrum
Lead
Pb
Plumbum
Mercury
Hg
Hydrargyrum
Potassium
K
Kalium
Silver
Ag
Argentum
Sodium
Na
Natrium
Tin
Sn
Stannum
Tungsten
W
Wolfram
Mixtures
characteristics
o percentage composition varies from sample to sample
o components are chemically different and retain properties in a mixture
o do not melt/boil at a definite temperature
two types
o heterogeneous mixtures
 components not uniformly mixed
 more than one phase
o


Antimony
homogeneous mixtures
 components uniformly mixed
 one phase
 also called solutions
Separating mixtures
mixture's components have different properties
devise a process that selects components with certain properties
o density, melting point, boiling point, solubility, reactivity, magnetism, polarity
some basic techniques
o filtration: select components by particle size
o floatation: select components by density
o crystallization: select components by solubility
o extraction: select components by solubility
o distillation: select components by boiling point
o chromatography: select components by affinity for a 'stationary phase'
ENERGY
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Energy , therefore, is the capacity to move matter or to effect changes in matter.
Two general classes of energy:
1. Potential energy – is stored energy.
7
Energy – is defined as the capacity to do work.
Work is done when matter is moved by applying force. A force is a push or pull.
PINES CITY COLLEGES
COLLEGE OF PHARMACY
Magsaysay Avenue, Baguio City 2600
Tel. No. (074) 445-2210 Loc. 51 Fax : (074) 445-2208
www.pcc.edu.ph
2. Kinetic energy – is the energy associated with matter in motion. Whenever an object is moving , it
posses kinetic energy
Heat is a form of kinetic energy; it can never classified as potential energy.
Measurement of energy:
The joule is the SI unit of energy. It was named after James P. Joule, an English scientist who performed
significant early experiments that related energy forms.
Fundamental Laws of Nature:
1. The law of conservation of mass states that there o detectable change in mass in a chemical reaction.
Stated in another way: The total mass of the reactants equals the total mass of the products
2. The law of conservation of energy states that energy cannot be created or destroyed in chemical
reactions. Energy may be converted from one form to another
C. RESOURCES
The following materials are worthy references for you to understand the course better:
Page
8
Remington (2013). Essential of Pharmaceutics edited by Linda Felton. UK: Pharmaceutical Press
Petrucci, Ralph H., et al. General Chemistry Principles and Modern Applications. (8th ed.) Upper Saddle River,
New Jersey: Macmillan Publishing Company, 2002. 1346p.
AY 2020-2021 PH CHEM 1O1 By Michelle T. Onoza, RPh, MS Pharmacy