Atomic structure and bonding Generix Content - Atomic structure and bonding
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JAMB questions for "Chemistry :: Atomic structure and bonding"
Q1

Moving from left to right across a period, the general rise in the first ionization energy can be attributed to the 

A

decrease in screening effect

B

increase in screening effect

C

decrease in nuclear charge

D

increase in nuclear charge

E
Q2

How many unpaired electron(s) are there in the nitrogen sub-levels ?

A

1

B

0

C

3

D

2

E
Q3

The maximum number of electrons in the L shell of an atom is 

A

18

B

32

C

2

D

8

E
Q4

Elements in the same period in the periodic table have the same

A

chemical properties

B

physical properties

C

number of shells

D

atomic number

E
Q5

The reaction above illustrates 

A

nuclear fussion

B

nuclear fission

C

alpha decay

D

artificial transmutation

E
Q6

If an atom is represented as 2311X which of the following deductions is correct?

A

it contains 12 protons

B

it forms a covalent chloride

C

its atomic number is 23

D

it is an alkali metal

E
Q7

If the relative molecular mass of an element is not a whole number, it can be deduced that the element is

A

naturally radioactive

B

abundant in nature

C

a transition metal

D

an isotopic mixture

E
Q8

Cathode rays cause an object placed behind a perforated anode to cast a shadow on the screen. This observation shows that the rays 

A

are positively charged

B

are negatively charged

C

have mass

D

travel in straight lines

E
Q9

Which quantum number divides shells into orbitals?

A

principal

B

azumuthal

C

magnetic

D

spin

E
Q10

The type of bonding in [Cu(NH3)2]2+ is

A

coordinate

B

electrovalent

C

metallic

D

covalent

E
Q11

16.8g of sodium hydrogen trioxocarbonate (IV) is completely decomposed by heat. Calculate the volume of carbon (IV) oxide given off at s.t.p?

 

[Na = 23, C = 12, O = 16, H = 1

Molar volume of a gas at s.t.p = 22.4 dm3]

A

22.40 dm3

B

11.20 dm3

C

2.24dm3

D

1.12dm3

E
Q12

The experiment that showed that atoms have tiny positively charged nucleus was first carried out by

A

Moseley

B

Rutherford

C

Milikan

D

Dalton

E
Q13

The atom of an element X is represented as YZX. The basic chemical properties of X depend on the value of

A

Y

B

Z

C

Y - Z

D

Z - Y

E
Q14

In the periodic table, electrical and thermal conductivities are properties of elements that

A

decrease across the period and increase down the group

B

increase across the period and decrease down the group

C

decrease across the period and down the group

D

increase across the period and down the group

E
Q15

The reaction above is an example of 

A

nuclear fission

B

nuclear fusion 

C

artificial transmutation

D

beta decay

E
Q16

The type of isomerism shown by cis-and transisomers is 

A

optical isomerism

B

positional isomerism

C

functional isomerism

D

geometrical isomerism

E
Q17

A metal X forms two bromides with the formula XBr2 and XBr3. What type of bonding exists between X and bromine in the bromides?

A

Metallic bonding

B

Ionic bonding

C

Covalent bonding

D

Dative bonding

E
Q18

How many electrons are in the L shell of 3115P?

A

2

B

5

C

8

D

18

E
Q19

Which experiment led to the measurement of the charge on an electron?

A

Scattering α - particles

B

Discharging-tube experiment

C

Oil-drop experiment

D

Mass spectrometric experiment

E
Q20

If the electronic configuration of an element is 1s2 2s2 2p5, how many unpaired electrons are there

A

1

B

2

C

3

D

5

E
Q21

The element that belongs to the third period of the periodic table are 

A

B, C, N and O

B

Na, Mg, S and Ar

C

Li, Be, Al and P

D

Na, P, O and Cl

E
Q22

The efficiency of a solid catalyst to increase reaction rates depends on its

A

surface area

B

solubility

C

concentration

D

quantity

E
Q23

Which of the following pairs of substances will react further with oxygen to form a higher oxide

A

CO2 and H2O

B

NO and H2O

C

CO and CO2

D

SO2 and NO

E
Q24
A decrease in atomic size and an increase in nuclear charge across a period lead to 
A
an increase in the tendency to lose electrons
B
an increase in chemical reactivity
C
a decrease in electropositivity
D
a decrease in covalency in bond formation
E
Q25
What is the valence shell electron configuration of the element with atomic number 17?
A
1s2 2s2 2p6 3s2 3p5
B
1s2 2s2 2p6 3s2 3p4
C
3s2 3p5
D
2s2 2p6 
E
Q26
The component of an atom that contributes least to its mass is the
A
nucleus
B
neutron
C
electron
D
proton
E
Q27
How many hydrogen atoms does a single ring cycloalkane have less than the corresponding open-chain alkane?
A
Three
B
One
C
Four
D
Two
E
Q28
Chlorine consisting of two isotopes of mass number 35 and 37 in the ratio 3:1 has an atomic mass of 35.5. Calculate the relative abundance of the isotope of mass number 37
A
60
B
20
C
75
D
25
E
Q29
an electron can be added to a halogen atom to form a halide uon with
A
8 valence electrons
B
7 valence electrons
C
2 valence electrons
D
3 valence electrons
E
Q30
What is the value of x in the nuclear reaction above?
A
226
B
220
C
227
D
222
E
Q31
The shape of the s-orbital is 
A
elliptical 
B
spiral
C
circular
D
spherical
E
Q32
The property of chlorine which causes hydrogen chloride to be more ionic than the chlorine molecule is its
A
electronegativity
B
electropositivity
C
electron affinity
D
electrovalency
E
Q33
Which of these reagents can confirm the presence of triple bond 
A
Bromine gas
B
Bromine water
C
Acidified KMnO4
D
Copper (I) chloride
E
Q34
Vulcanization involves the removal of
A
the single bond
B
the double bond
C
a polymer
D
a monomer
E
Q35
Which of the following hydrogen halides has the highest entropy value?
A
HBr
B
HF
C
HI
D
HCl
E
Q36
The process by which atoms are rearranged into different molecular structures in the petroleum refining process is referred to as
A
polymerization
B
reforming
C
hydrocracking
D
catalytic cracking
E
Q37
Neutral atoms of neon with atomic number 10 have the same number of electrons as
A
K+
B
Mg2+
C
Ca2+
D
O2+
E
Q38
The noble gases owe their inactivity to 
A
hexagonal shape
B
octet configuration 
C
obtuse configuration
D
cyclic shape
E
Q39
The postulate of Dalton's atomic theory which still holds is that
A
atoms can neither be created nor destroyed
B
the particles of the same element are exactly alike
C
particles of different elements combine in a simple whole number ratio
D
all elements are made of small indivisible particles.
E
Q40
The property which makes alcohol soluble in water is the
A
boiling point
B
hydrogen bonding
C
ionic bonding
D
covalent nature
E
Q41
Which of the following gases contains the least number of atoms at s.t.p.?
A
1 mole of butane
B
3 moles of ozone
C
4 moles of chlorine
D
7 moles of argon
E
Q42
Milikan's contribution to the development of atomic theory is the determination of 
A
positive rays
B
cathode rays
C
charge to mass ratio
D
charge on electron
E
Q43
An oxide XO2 has a vapour density of 32. What is the atomic mass of X?   [O = 16]
A
20
B
32
C
14
D
12
E
Q44
What mass of water is produced when 8.0 g of hydrogen reacts with excess oxygen?   [H = 1, O = 16]
A
72.0 g
B
36.0 g
C
16.0 g
D
8.0 g
E
Q45
Four elements W, X, Y and Z have atomic numbers 2, 6, 16, and 20 respectively. Which of these elements as a metal?
A
X
B
Z
C
W
D
Y
E
Q46
The diagram above represents the formation of 
A
a metallic bond
B
a covalent bond
C
an electrovalent bond
D
a co-ordinate covalent bond
E
Q47
The shapes of CO2, H2O, and CH4 respectively are
A
bent, linear and tetrahendral
B
bent, tetrahendral and linear
C
linear, bent and tetrahendral
D
tetrahendral, linear and bent
E
Q48
The distance between the nuclei of chlorine atoms in a chlorine molecule is 0.194 nm. The atomic radius of chlorine atom is
A
0.097 nm
B
0.194 nm
C
0.388 nm
D
2.388 nm
E
Q49
How many moles of HCl will be required to react with potassium heptaoxodichromate (VI) to produce 3 moles of chlorine?
A
14
B
12
C
11
D
10
E
Q50
Which of the following statements is correct about the periodic table?
A
Elements in the same period have the same number of valence electrons.
B
The valence electrons of the elements in the same period increase progressively across the period.
C
Elements in the same group have the same number of electron shells.
D
The non-metallic properties of the elements tend to decrease across each period.
E
Q51
Which of the following types of bonding does not involve the formation of new substances?
A
Metallic
B
Covelent
C
Co-ordinate
D
Elcetrovalent
E
Q52
The element that is likely to participate in covalent rather than ionic bonding is
A
Z
B
Y
C
X
D
W
E
Q53
The diagram beside represents an atom that can combine with chloride to form
A
a covalent bond
B
an electrovalent bond
C
a hydrogen bond
D
a co-ordinate bond
E
Q54
Which of the following electron configurations indicates an atom with the highest ionization energy?
A
2,8,7
B
2,8,8,1
C
2,8,8,2
D
2,8,8,7
E
Q55
If 30cm3 of oxygen diffuses through a porous plug in 7s, how  long will it take 60cm3 of chlorine to diffuse through the same plug?   [O = 16, Cl = 35.5]
A
12s
B
14s
C
21s
D
30s
E
Q56
In the periodic table, what is the property that decreases along the period and increases down the group?
A
Atomic number
B
Electron affinity
C
Ionization potential
D
Atomic radius
E
Q57
Two elements, P and Q with atomic numbers 11 and 8 respectively, combine chemically to form the compound PxQy. The respectively values of x and y are
A
1 and 1
B
1 and 2
C
2 and 1
D
3 and 1
E
Q58
Which of the letters indicate an alkali metal and a noble gas respectively?
A
M and E
B
G and E
C
R and L
D
G and L
E
Q59
In the oil drop experiment, Milikan determined the
A
chare of mass ration of the electron
B
mass of the electron
C
charge of the electron
D
mass of the proton
E
Q60
The stability of ionic solids is generally due to the
A
negative affinity of most atoms
B
crystal lattice forces
C
electron pair sharing
D
positive ionization potentials
E