COURSE: BASIC TECHNICIAN IN PHARMACEUTICAL SCIENCES
NTA LEVEL 4: SEMESTER II
MODULE TITLE: INORGANIC CHEMISTRY
MODULE CODE: PST04210
CONTINUOUS ASSESSMENT TEST 1 MARKING GUIDE
TIME: 2:00 HRS
November, 2019
INSTRUCTIONS:
Read all instructions carefully.
2. Write your examination number on each page of the answer sheet you use.
3. Attempt all questions.
4. Cellular phones are NOT allowed in the examination room.
5. Each essay question to be answered on not more than3 handwritten papers.
6. This paper consists of five (5) sections.
7. The table below is for OFFICIAL USE ONLY
MARKS DISTRIBUTION
SCORED
MARKS
Section A: Multiple Choice
10 Marks
Section B: True and False
10Marks
Section C: Matching Item
10 Marks
Section D: Short answer Questions
40 Marks
Section E: Essay questions
30 Marks
TOTAL
100 marks
INTERNAL
EXAMINER
VERIFIER
SECTION A: MULTIPLE CHOICE QUESTIONS
(10 MARKS)
INSTRUCTIONS:
 This section consists of ten (10) Questions
 One (1) mark will be awarded for each correct answer
1. Answer item one (i) to ten (x) by choosing the letter of the most correct answer and write it
in the provided box using CAPITAL letter
i) ......................................is the number of protons in the nucleus of each atom of an element
A. Atomic weight
B. Atomic Number
C. Atomic mass
D. Atomic ratio
E. Mass number
ii) The branch of pharmaceutical chemistry which deals with study of all elements is
A. Organic chemistry
B. Physical chemistry
C. Soil chemistry
D. Inorganic chemistry
E. Analytical chemistry
iii) All elements have neutrons and protons present in the nucleus of an atom except
A.
B.
C.
D.
E.
Carbon
Argon
Carbon cation
A or C
Hydrogen
iv) With regard to group 2A elements; the first and the second ionization energies
A.
B.
C.
D.
E.
Increases from beryllium to barium
Decrease from beryllium to barium
Increases from barium to beryllium
Decrease from barium to beryllium
Ionization energy is constant
v) It is impossible to measure precisely both the position and the momentum of a particle
A.
B.
C.
D.
Uncertainty principle (Werner Heisenberg)
The wave-particle nature of matter (De Broglie’s)
Bohr's solar system model of the atom (Niels Bohr)
Planetary model of the atom(nuclear) (Rutherford)
E. None of the above
vi) The total numbers of protons and neutrons is
A.
B.
C.
D.
E.
Atomic number
Mass number
Number of electrons
Atomic mass
B or D
vii) Which of the following is a good example of acidic oxide
A.
B.
C.
D.
E.
B203
CO
SiO2
B and C
A and C
viii) Group eight elements of periodic table are called
A.
B.
C.
D.
E.
Transition metal
Alkaline earth metals
Noble gas
Alkali metal
Halogen
ix) When the angular momentum quantum number (Azimuthal quantum number (ℓ)) is 1 (one).
Determine the value of the orbitals can be formed
A.
B.
C.
D.
E.
1
5
3
4
2
x) Which of the following is the true configuration of copper?
A. 29Cu: 1s22s22p63s23p64s23d4
B. 29Cu: 1s22s22p63s23p64s13d5
C. 29Cu: 1s22s22p63s23p64s23d9
D. 29Cu: 1s22s22p63s23p64s13d10
E. None of the above
SECTION B: MULTIPLE TRUE AND FALSE QUESTIONS (20 MARKS)
INSTRUCTIONS:
 This section consists of eight (4) questions with five options
 Write the word TRUE for correct statement and word FALSE for wrong
statement in the space provided
 0.5 mark will be awarded for each correct answer
2. with respect to group 5A elements
i. Nitrogen exists as N4 molecules
ii. It consist 4 electrons in the outermost shell
iii. Phosphorous exist as diatomic molecules
iv.
Antimony also has a covalent network structure
v.
Their oxides change from acidic to amphoteric to basic
FALSE
FALSE
FALSE
TRUE
TRUE
3. Regarding to transition elements
i. Reactivity decreases from right to left across the periodic table
ii. Transition metals are found in group 12 of period table
iii. Transition metal atoms are either Lewis acid or Lewis base
iv.
All transition element are having high melting and boiling points
v. Have partial or full filled d orbital
FALSE
FALSE
TRUE
FALSE
TRUE
4. Regarding properties of element in periodic table;
i. Core charge increases from left to right
ii. Ionic radius increases from left to right
iii. Density increases from right to left
iv.
Electron affinity increases as you go down the group
v. Metallic properties increases from right to left
FALSE
FALSE
TRUE
FALSE
FALSE
5. Regarding to electronic configuration;
i.
ii.
iii.
iv.
v.
The electron configuration of copper is 29Cu: 1s22s22p63s23p64s23d4
FALSE
One or more orbitals with the same n and ℓ values are referred to as a shell.
FALSE
Both Copper and chromium violet the Hund’s rule
FALSE
Spin quantum numbers are used to describe atomic orbital and to label electrons that
reside in them
FALSE
A collection of orbitals with the same value of n is frequently called a shell TRUE
6. According to Dalton’s Atomic theory;
i.
A chemical reaction is the rearrangement of atoms
TRUE
ii.
iii.
iv.
v.
All matter is composed of tiny, indivisible particles called atoms
TRUE
Atoms cannot be made or destroyed
TRUE
All atoms of one element are identical in weight and atoms of different elements have
different weight
TRUE
Compounds are formed by joining the atoms of two or more elements TRUE
SECTION C MATCHING ITEMS QUESTIONS (10 MARKS)
INSTRUCTIONS:
 This section consists of ten (10) matching item questions with two parts each containing
five questions
 Match the items in COLUMN A with corresponding statements in COLUMN B by
writing a letter of correct response in the space provided
 Each correct response is awarded one mark
 Each item from column B is used only once
10A) Match the uses from COLUMN B with their corresponding compounds of group five
elements in COLUMN A
COLUMN A
(Compounds of group five elements)
(i) Nitrogen (I) Oxide (nitrous oxide) USP
(ii) Sodium Nitrite USP
(iii) The organic nitrites and sodium nitroprusside
(iv) Dibasic sodium phosphate
(v) Tribasic calcium, magnesium, and aluminum phosphates
COLUMN B
(Uses)
A. Used as an inhalatory general anesthetic
B. Used as gastric antacids
C. Antidote for cyanide poisoning
D. Used as urinary acidifiers
E. Used to form soluble salts of insoluble medicinal bases
F. Active ingredient in various saline cathartics and enemas
G. Used to lower blood pressure
COLUMN A
COLUMN B
I
A
ii
C
iii
G
iv
F
v
B
10B) Match the compounds of different elements from COLUMN B with their corresponding
Pharmaceutical uses in COLUMN A by writing the letter of the correct responses in the table
provided
COLUMN A
(Uses)
(i)
Gastric antacid
(ii)
Anticonvulsant preparation
(iii)
Used as intestinal adsorbent
(iv)
Radiopaque and imaging
(v)
Systemic alkalizer and acidifiers
COLUMN B
(Compounds of different elements)
A. Magnesium sulphate
B. Kaolin
C. Sodium bicarbonate
D. Aluminum chloride
E. Zinc stearate
F. Barium sulphate
G. Milk of magnesia
H. Sodium chloride
COLUMN A
COLUMN B
I
G
ii
A
iii
B
iv
F
v
C
SECTION D: SHORT ANSWERS QUESTIONS (40MARKS)
INSTRUCTIONS:
 This section consists of five (5) questions.
 Write a readable handwrite; DIRTY WORK IS NOT ALLOWED.
 Each question carry eight (8) marks
8 (a) Define the term diagonal relationship (1 mark)
 Refers to similarities between pairs of elements in different groups and periods of
the periodic table
(b) Differentiate between the periods and groups of element in the periodic table (1 mark @)
The vertical columns of the table are called groups or families
The horizontal rows of the table are called periods
9. Outline five (5) physical characteristics of group one elements
1 mark @
 They are shiny, have the consistency of clay,
 are easily cut with a knife
 Have low densities and low melting points.
 Have low ionization energies
 Alkali metals are never found as free elements in nature
10. Mention four branches of Pharmaceutical chemistry (4 marks)
Answer (any 4 points @ 1 mark)
i.
ii.
iii.
iv.
v.
Pharmaceutical organic chemistry
Pharmaceutical inorganic chemistry
Analytical chemistry
Physical chemistry
Biochemistry
11. Outline four (4) importance of chemistry in pharmacy (4 marks)
Answers (any 4 points @ 1 marks)
i.
Exploration of suitable sources of drugs
(5 Marks)
ii.
iii.
iv.
v.
vi.
vii.
Exploration of the chemical and physical properties of the drugs
Determination of storage conditions
Determination of the packaging material
Choice of the appropriate route of administration
Study of the biopharmaceutical parameters
Diagnosis and treatment of disease
12. List four categories of oxides in the periodic table with one example for each (4 marks)
(@ 1 mark)
i.
ii.
iii.
iv.
Basic Oxides Example Mgo,
Amphoteric Oxides Example Al2O3,
Neutral Oxides Example CO And
Acidic Oxides example SiO2
13. Describe how chemistry can be useful in the following area (2 marks@)
i. Determination of storage condition
Through the knowledge of different function groups and their properties, such as stability,
one can propose the appropriate storage conditions. Example; drug with ester function like
aspirin can be affected by moisture and so should be kept in dry and cool place
ii.
Packaging material
Knowing effect of light to the drugs and contained molecules through knowledge of
chemistry, proper choice of material for packaging can be suggested. Example; light
sensitive drugs be stored in amber colored bottle
14 (a) Define Catenation (1 mark)
Is a process whereby carbon bonds to itself to form stable chains, branches, and
rings
(b) Mention two (2) allotropies of carbon (1 mark)
Diamond
Graphite
(c) Use noble gas to write electronic configuration of Carbon (6C) and Silicon (14Si) (@1
mark)
Carbon (6C) = [He] 2s2 2p2
Silicon (14Si) = [Ne] 3s2 3p2
(d) With example, list four (4) uses of carbon in pharmacy (4 marks)
 Carbon is used in preparation of activated charcoal
 Sodium bicarbonate and the slightly soluble carbonates or basic carbonates
of calcium, magnesium, and aluminium are used as gastric antacids
 Potassium bicarbonate is used as source of potassium ion in electrolyte
replenishers.
 Bismuth sub carbonate is an astringent and protective
 Ammonium carbonate is an effective reflex stimulant and expectorant
15 (a) Define the term ionization energy (2 marks)
 Refers to the minimum amount of energy required to remove the highest
energy electron from an atom (energy to steal an electron)
or
 The minimum energy (in kJ/mol) required to remove an electron from a
gaseous atom in its ground state.
(b) Describe the ionization energy trend down the group (2 marks)
Ionization energy decrease down the group
(c) Describe the ionization energy trend across the period (2 marks)
Ionization energy increases across the period
(d) Arrange the following cations in order of increase in ionization energy Al+ Al3+ Al2+(2
marks)
Al+ <Al2+ <Al3+
SECTION E: ESSAY TYPE QUESTIONS (30MARKS)
INSTRUCTIONS:
 This section consits of three (3) questions
 Write your answer on sheet of paper provided; each question should start on a new
page
 Each question carry 10 marks
16. Electronic configuration describes how the electrons are distributed among the various
atomic orbitals.
a) Define quantum number (1 mark)
b) Explain four types of quantum numbers used in electronic configuration. (9marks)
Quantum numbers are numbers used to describe atomic orbitals and to label electrons that
reside in them. (1 mark)
 The Principal Quantum Number (n) (2 marks)
 Have integral values 1, 2, 3, and so forth
 The value of n determines the energy of an orbital.
 The principal quantum number also relates to the average distance of the
electron from the nucleus in a particular orbital
 The larger n is, the greater the average distance of an electron in the orbital
from the nucleus and therefore the larger the orbital
 The Angular Momentum Quantum Number (Azimuthal quantum number (ℓ)) (2
marks)
 This quantum number defines the shape of the orbital
 The values of ℓ depend on the value of the principal quantum number, n
 Has integral values of ℓ = 0 to ℓ = n - 1 for each value of n.
 Magnetic quantum number (ml) (2 marks)
 Describes the orientation(number) of the orbitals in space
 Has integral values of m = - ℓ to + ℓ including 0
 For example, if n = 3 and ℓ = 2 then the possible values of m are -2, -1, 0, +1,
+2
 The number of values indicates the number of orbitals in a sub shell with a
particular value
 The spin quantum number, ms (2 marks)
 sometimes called the spin angular momentum of an electron
 spin makes the electron behave like a tiny magnet
 spin can be clockwise or counterclockwise
 spin quantum number can have only two possible states +1/2 (spin up) or -1/2
(spin down)
Conclusion (1 mark)
17. Explain eight (8) uses of Transition elements in Pharmacy
(10 marks)
Introduction (1 mark)
Use of Group Transition elements (Eight points @1 mark)
 Copper is an essential trace element and small quantities enhance the physiological
utilization of iron
 Manganese is an essential trace element, being necessary for the activation of a
variety of enzymes such as pyruvate carboxylase
 Various copper compounds are used as fungicides and insecticides, and they are
particularly effective algaecides
 Silver sulfadiazine is used topically as a germicide
 Gold compounds are employed in the treatment of lupus erythematosus and
rheumatoid arthritis
 Zinc is used in the treatment of various external surfaces of the body and in wound
healing, taste acuity, and various ophthalmic problems
 Soluble cadmium compounds are astringent
 CdSO4 has been used both as a topical astringent and for eye infections
 Potassium Permanganate USP is used as a local anti-infective and is also an
astringent, powerful deodorant and cleanser
 Titanium dioxide is also a popular ingredient in various lotions and creams for the
prevention of sunburn
 Iron (III) compounds are astringent
 Sodium nitroprusside USP,
is used as a vasodilator
 Ferrous Fumarate (Tablets), Ferrous Gluconate (Tablets, Capsules, and Elixir),
Ferrous Sulphate (Oral Solution, Syrup, and Tablets) and Dried Ferrous Sulphate
are used as Hematinics
 Iron Dextran Injection (a colloidal iron (III) hydroxide with partially hydrolyzed
dextran) and Iron Sorbitex Injection (a complex of iron with sorbitol and citric acid)
are cited in the USP as injectable forms for patients with poor gastrointestinal
tolerance or poor absorption of iron
 Titanium dioxide TiO2 is used as a solar-ray protective
 Tantalum is unaffected by the body fluids and is used in sheet form for the surgical
repair of bones
 Radioactive technetium, 99Tc is used for diagnosis in various forms
 The radioactive isotopes have been employed in mineral metabolism studies
 Copper(II) sulphate is the basis for Fehling's and Benedict's Solutions, the classic test
solutions for reducing sugars
Conclusion (1mark)
18. The properties of the elements in a periodic table are periodic functions of their atomic
weights as developed by Dmitri Ivanovitch Mendeléev.
a) Define periodic table (1 mark)
Refers to a table in which elements are arranged by the order of increasing atomic
number
b) Describe the arrangement of elements in the periodic table (9marks)
Core Charge (2 marks)
 Refers to the attraction that an outer shell electron feels towards the nucleus
 Down the group it is constant
There is always equal number of electron in the outer shell example in the alkaline metals
there is always one electron in the outer shell.
 Across a period it increases
There are more electrons in the outer shell which are greatly attracted to the nucleus
Atomic radius or size (2 marks)
One-half the distance between the two nuclei in two adjacent metal atoms /two atoms in
diatomic molecule
 Down the group it increases
There is an increase in the number of shells
 Across the period it decreases
There is an increase in core charge, the outer shell electrons are attracted closer to the
nucleus
Ionisation Energy (2 marks)
 Refers to the minimum amount of energy required to remove the highest energy
electron from an atom (energy to steal an electron)
 Down the group it decreases
The size of the atom is increasing, the attraction is weaker between the outer shell
electrons and the nucleus therefore electrons are easier to remove
 Across a period it increases
There is an increase in core charge, the attraction is greater between the outer shell
electrons and the nucleus. Therefore electrons are harder to remove
Electro negativity and Electron affinity (2 marks)
 Refers to measure of the ability of an atom to attract an electron towards itself.
(love of electrons)
 Down the group it decreases
The electrons are further from the nucleus, there is a weaker attraction
 Across a period it increases
There is an increase in core charge, there is a greater attraction of the outer shell
electrons to the nucleus
Conclusion (1 mark)