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WorksheetsCHEMICAL BONDING & MOLECULAR STRUCTURE
Total questions: 100
Worksheet time: 50mins
The electronic configuration of four atoms are given in brackets:
P(1s2 2s2 2p1); Q(1s22s22p5)
R( 1s22s22p63s1) S (1s22s22p2)
The element that would most readily form a diatomic molecule is
P
Q
R
S
Two elements P & Q combine to form a compound. If P has 2 & Q has 6 electrons in their outermost shell, what will be formula of the compound formed?
PQ
P2Q
P2Q3
PQ2
How many no. of electrons are involved in the formation of a nitrogen molecule?
3
4
8
6
A pair of electrons present between two identical non-metals
is shifted to one of the atoms
is shared equally between them
undergoes addition reactions
have same spin
In which of the following molecules octet rule is not followed?
NH3
CH4
CO2
NO
In a covalent bond formation,
a transfer of electrons takes place
equal sharing of electrons between two atoms takes place
electrons shared by one atom only
electrons are donated by one atom and shared by both atoms.
During a coordinate bond formation,
one electron from an atom is transferred to other
one electron each is lost from both the atoms
a pair of electrons is contributed by one atom and shared by both the atoms
a pair of electrons is transferred to the other atom
Which of the following molecules contains covalent & co-ordinate bonds?
CCl4
H2SO4
NaCl
Mg(OH)2
How many and what types of bonds are present in NH+4
four covalent bonds
three covalent bonds and one ionic bond
four ionic bonds
three covalent bonds and one co-ordinate bond
Among the following the exceptions of the octet rule is
the incomplete octet of central atom
an odd no. of electrons on central atom
expanded octet of the central atom
all of these
Which of the following shows the lewis dot formula for CO2?
What is the formal charge on carbon atom in the following two structures:
0,-2
0,0
+2,-2
+1,-1
Two elements X & Y combine to form a compound XY. Under what conditions the bond formed between them will be ionic?
if the difference in electronegativities of X & Y is 1.9
if the difference in electronegativities of X & Y is less than 1.9
if both X & Y are highly electronegative.
if the difference in electronegativities of X & Y is more than 1.9
In which of the following species the bond is non- directional?
NCl3
BCl3
RbCl
BeCl2
Sodium chloride has a crystalline structure made up of Na+ & Cl- ions. Why does NaCl not conduct electricity in solid state?
the crystalline structure does not have ions
when a bond is formed between ions they lose their charges
the ions of a NaCl become mobile only in molten state and are not free to move in solid state.
none of these
Which of the following elements forms predominantly covalent compounds as compared to other elements which form ionic compounds?
Mg
Sr
Be
Ca
The correct order of decreasing bond lengths of CO, CO2 and CO32- is
CO2>CO> CO32-
CO>CO2> CO32-
CO2> CO32->CO
CO32- > CO2> CO
The correct sequence of bond length in single bond, double bond and triple bond of C is
(C-C) = (C = C) = (C ≡ C)
C ≡ C<C = C<C-C
C-C<C=C<C ≡ C
C=C<C ≡ C<C-C
Which of the following will be the strongest bond?
O-H
F-O
N-H
O-Cl
Which of the following molecules does not show any reasoning structure ?
CO2-3
SO3
NH3
O3
The canonical or resonating structures of a molecule required to describe the structure of a molecule follow which of the following rules?
the energy of each structure is different
the same no. of unpaired and paired electrons in all structures
like charges are present on adjacent atoms
the relative position of all atoms can differ
Arrange the following in order of increasing dipole moment: H2O,H2S,BF3
H2S< BF3<H2O
BF3< H2O<H2S
BF3<H2S<H2O
H2O<H2S<BF3
Which of the following is non-polar?
SO2
NH3
CO2
H2O
In a diatomic molecule the bond distance is 110-8 cm. Its dipole moment is 1.2D. What is the fractional electronic charge on each atom?
0.50
0.25
1.2
1.2-10
Which of the following are arranged in the decreasing order of dipole moment?
CH3Br, CH3F, CH3Cl
CH3Br, CH3Cl, CH3F
CH3Cl, CH3Br, CH3F
CH3Cl, CH3F, CH3Br
What is the correct dipole moment of NH3 & NF3 respectively?
In water molecule, the two O-H bonds are oriented at an angle of 104.5. In BF3, the three B-F bonds are oriented at an angle of 120. In BeF2, the two Be-F bonds are oriented at an angle of 180. Which of the following will have highest dipole moment?
BF3
all have zero dipole moment
BeF2
H2O
Arrange the following in increasing order of covalent character- NaCl, MgCl2, AlCl3
MgCl2< NaCl< AlCl3
NaCl< AlCl3< MgCl2
NaCl< MgCl2< AlCl3
AlCl3< MgCl2< NaCl
Match the bond enthalpies given in column II with the molecules given in column I and mark the appropriate choice.
(A)(iii),(B)(i),(C)(ii)
(A)(iii),(B)(ii),(C)(i)
(A)(i),(B)(ii),(C)(iii)
(A)(i),(B)(iii),(C)(ii)
The given structures I,II & III of carbonate ion represent:
isomeric structures
canonical structures
hybrid structures
dipole structures
Although F is more electronegative than H, the resultant dipole moment of NH3 is much more than that of NF3, it can be explained as
all the dipoles of NF3 are in same direction
NH3 has a regular geometry while NF3 has irregular geometry which makes dipole moment of NH3 more than NF3.
the lone pair of nitrogen opposes the dipole moment of NF3 while it is added to the dipole moment of NH3
all the dipoles of NH3 are in opposite direction
According to VSPER theory,
the shape of the molecule depends upon the bonded electron pairs
pair of electrons attract each other in valence shells
the pair of electrons tend to occupy such positions that minimize distances from each other.
the pairs of electrons tend to occupy such positions that minimize repulsions
In a bonded molecule, the order of repulsion between the bonded and non-bonded electron is
lone pair-lone pair> lone pair-bond pair> bond pair-bond pair
bond pair-bond pair> lone pair-lone pair> lone pair-bond pair
bond pair-bond pair> lone pair-bond pair> lone pair-lone pair
lone pair-lone pair>bond pair-bond pair>loan pair-bond pair
The shape of water molecule which should be tetrahedral has a bent or distorted tetrahedral shape with a bond angle 104.5. what could be the reason for this?
lp-lp repulsion is equal to lp-bp repulsion
lp-lp repulsion is more than lp-bp repulsion
presence of lone pair does not affect the bond angle
lp-bp repulsion is more than lp-lp repulsion
In which of the following molecules the central atom does not retain any lone pair of electrons?
NO2
BF3
NH3
H2O
Few compounds formed by chemical bonding are given below. Mark the incorrect example.
A molecule with linear shape-CO2
A molecule which is V-shaped with a bond angle 104.5-NH3
A molecule with central atom devoid of octet- BF3
A non-polar covalent compound between two different atoms-CH4
Which of the following statements is correct regarding the structure of PCl5?
The bond angle in all P-Cl bonds is 90
Five P-Cl bonds lie in the same plane
The bond length of all P-Cl bond is same
Three P-Cl bonds lie in one plane and two P-Cl bonds lie above and below the equatorial plane.
What is common between the following molecules SO3, CO2-3,NO-3?
all have trigonal planar shape
all have tetrahedral shape
all have trigonal pyramidal shape
all have linear shape
Which of the following does not show octahedral geometry?
SF6
SF4
IF5
SiF2-6
The BCl3 is a planar molecule whereas NCl3 is pyramidal because,
B-Cl bond is more polar than N-Cl bond
BCl3 has no lone pair but NCl3 has a lone pair of electrons
nitrogen atom is smaller than boron atoms
N-Cl bond is more covalent than B-Cl bond
Structure of XeF4 is
tetrahedral
triangular
octahedral
square planar
Which of the following shapes of SF4 is more stable and why?
(i), due to 3lp-bp repulsions at 90 °
(ii), due to 2 lp-bp repulsions
both are unstable since SF4 has tetrahedral shape
both are equally stable due to 2 lp-bp repulsions
The most stable shape of CIF3 is shown by
only (i)
only (ii)
only (iii)
(i) & (ii)
Match the molecules given in column I with their shapes given in column II and mark the appropriate choice.
(A)(iv),(B)(i),(C)(ii),(D)(iii)
(A)(ii),(B)(iii),(C)(i),(D)(iv)
(A)(iv),(B)(ii),(C)(iii),(D)(i)
(A)(iii),(B)(i),(C)(ii),(D)(iv)
Which molecule is depicted by the given ball and stick models?
(i) BF4, (ii) CH4
(i) BF3, (ii) PCl5
(i) BeCl2 (ii) PCl5
(i) BeCl2, (ii) CH4
Given below is the table showing shapes of some molecules having lone pairs of electrons. Fill up the blanks left in it.
2 - square pyramidal- 2-T-shaped -square planar - H2O2
4 - T-shaped - 5 - square planar - square pyramidal - SO3
2 - T-shaped - 1 - square pyramidal - square planar - XeF4
3 -Square planar - 2 - T-shaped - square pyramidal - BrCl
Which of the following statement is not true?
ionic bonds are non-directional while covalent bond are directional
formation of bond shortens the distance between the two concerned atoms
linear overlapping of atomic p-orbitals leads to a sigma bond
ionic bond is possible between similar & dissimilar atoms
Which of the following will not form sigma bond after overlapping?
s-orbital and pz-orbital
pz-orbital and px-orbital
s-orbital and s-orbital
pz-orbital and pz-orbital
Which type of overlapping is shown by p(px,py,pz orbitals)?
three sidewise overlaps
three end to end overlaps
two end to end and one sidewise overlap
two sidewise and one end to end overlap
Oxygen molecule is formed by
two p-p sidewise overlaps
two p-p axial overlaps
one p-p axial and one p-p sidewise overlap
one axial s-s overlap and one p-p axial overlap
Which types of bonds are present between two carbon atoms in acetylene molecule?
one sigma bond and two pi bond
two sigma bonds and one pi bond
three pi bonds
three sigma bonds
Propyne molecule contains
2 sigma and 3 pi bonds
5 sigma bonds
6sigma and 2pi bonds
5 pi bonds and 1 sigma bond
How many sigma and pi bonds are present in toluene?
12 σ & 3 π bonds
15 σ & 3 π bonds
6 σ & 3 π bonds
10 σ & 3 π bonds
Which of the following is the most stable state when two atoms come closer to each other to form a molecule?
(i), when the bond is formed, the energy is minimum
(ii), when the atoms touch each other, the energy is zero
(iii), when the atoms are isolated, the energy is minimum
(ii), when the attractive forces are more than repulsive forces
Which of the following statements is true about hybridization?
hybrid orbitals form multiple bonds
the orbitals with different energies undergo hybridization
the hybridized orbitals have different energies for each orbital
the no. of hybrid orbitals is equal to the no. of atomic orbitals that are hybridized
Which of the following molecules is formed by sp2 hybrid orbitals?
CO2
BeF2
CH4
BF3
Atomic orbitals of carbon in carbon dioxide are
sp hybridized
sp3 hybridized
sp3 hybridized
sp3d hybridized
Which type of hybridization is shown by carbon atoms from left to right in the given compound CH2=CH-CN?
sp2, sp, sp
sp, sp2,sp3
sp2, sp2,sp
sp3,sp2, sp
On hybridization of one s and 3 p-orbitals, we get
4 orbitals with tetrahedral orientation
2 orbitals with perpendicular orientation
3 orbitals with trigonal orientation
2 orbitals with linear orientation
The molecules like BrF5 & XeOF4 are square pyramidal in shape. What is the type of hybridization shown in these molecules?
dsp2
sp3d2
dsp3
sp3d
Which of the following shows dsp2 hybridization and a square planar geometry?
PCl5
SF6
[Ni(CN)4]2-
BrF5
Which of the following pairs are isostructural?
CO2-3 & CO2
CH4 & BF3
SO2-4 & BF-4
NH3& NH+4
CF4,SF4 and XeF4 contain the following electronic structures on their central atoms. Which one is correct option?
1,2 & 3 lone pairs of electrons respectively
1,1 & 1 lone pairs of electrons respectively
no lone pairs of electrons on any molecule
0,1 & 2 lone pairs of electrons respectively
The hybrid state of carbon in ethyne, graphite and diamond are respectively
sp2, sp3, sp
sp3, sp2,sp
sp2,sp,sp3
sp, sp2, sp3
Given below is the bond angle in various types of hybridization. Mark the bond angle which is not correctly matched.
dsp2-90 °
sp3d-90 °
sp3-109.5 °
sp3d2-90 °
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
HI
H2O
SO2
CO2
The types of hybrid orbitals of nitrogen in NO+2, NO-3 & NH+4 respectively are expected to be
sp2,sp&sp3
sp,sp3&sp2
sp,sp2&sp3
sp2,sp3&sp
In PO3-4 ion, the formal charge on the oxygen atom of P-O bond is
+1
+0.75
-1
-0.75
In NO-3 ion, the no. of bond pairs and lone pairs of electrons on nitrogen atom are
3,1
1,3
2,2
4,0
No. of and bonds in the following structure is
5,20
5,19
4,20
6,19
Which of the following statements is not true regarding molecular orbital theory?
molecular orbitals like atomic orbitals obey Aufbau principle for filling of electrons
an atomic orbital is monocentric while a molecular orbital is polycentric
the atomic orbitals of comparable energies combine to form molecular orbitals
bonding molecular orbital has higher energy than antibonding molecular orbital
2s and 2p-atomic orbitals combine to give how many molecular orbitals?
8
6
4
2
The conditions for the combination of atomic orbitals to form molecular orbitals are stated below. Mark the incorrect condition mentioned here.
the combining atomic orbitals must have nearly same energy
combining atomic orbitals must have same symmetry about the molecular axis
Pi() molecular orbitals are symmetrical around the bond axis
the combining atomic orbitals must overlap to maximum extent
Which of the following species has unpaired electrons?
O-2
N2
O2-2
F2
What will be the bond order of the species with electronic configuration 1s22s22p5?
1
2
3
4
Which molecule/ion out of the following does not contain unpaired electrons?
N+2
O2-2
B2
O2
In which of the following molecule/ion all the bonds are not equal?
BF-4
SiF4
XeF4
C2H4
In which of the following substances will hydrogen bond be strongest?
HI
H2O
HCl
H2S
Match the column I with column II and mark the appropriate choice.
(A)(ii),(B)(iii),(C)(i),(D)(iv)
(A)(iii),(B)(i),(C)(iv),(D)(ii)
(A)(iv),(B)(i),(C)(iii),(D)(ii)
(A)(i),(B)(iii),(C)(ii),(D)(iv)
Which of the following bond order is indication of existence of a molecule?
zero bond order
negative bond order
positive bond order
all of these
According to molecular orbital theory which of the following will not exist?
Be2
B2
C2
H+2
Which of the following facts regarding bond order is not valid?
isoelectronic molecules and ions have identical bond orders
bond order is given by the no. of bonds between the two atoms in a molecule
with increase in bond order, bond length decreases
with increase in bond order, bond enthalpy of the molecule decreases
Which of the following formulae does not show the correct relationship?
B.O. =1/2 (Nb-Na)
B.O. ∝ 1/bond length
B.O. ∝ 1/ bond dissociation energy
Nb-Na , B.O. =+ve
Fill in the blanks with appropriate choice.
Bond order of N+2 is _p_ while that of N2 is __O__ . Bond order of O+2 is __R_ while that of O2 is__S__.N-N bond distance __T__. When N2 changes to N+2 and when O2 changes to O+2, the O-O bond distance is __U__ .
2.5- 3 -2.5- 2- increases- decreases
2.5- 3- 2- 1.5- decreases- increases
2- 2.5- 2.5- 1- increases- decreases
3- 2 -1.5- 1 -increases- decreases
Which of the following relationship is true?
bond dissociation energy of O+2 is higher than O2
bond dissociation energy of O-2 and O2 -2 are same
bond dissociation energy of O2 -2 is higher than O-2
bond dissociation energy of O2 and O-2 are same
Paramagnetism is shown by the molecules which have
bond order more than one
unpaired electrons
paired electrons
lone pair of electrons
Which of the following representations of wave functions of molecular orbitals and atomic orbitals is not correct?
Which of the following molecules is paramagnetic in nature?
Li2
H2
B2
N2
How many orbitals are singly occupied in O2 molecule?
4
3
2
1
Oxygen molecule is paramagnetic because
presence of unpaired electrons in molecular orbitals
no. of bonding electrons < no. of antibonding electrons
no. of bonding electrons > no. of antibonding electrons
no. of bonding electrons = no. of antibonding electrons
Oxygen molecule is paramagnetic in nature. What is the paramagnetic content. In terms of magnetic moment (B.M) in O-2?
2.5
3
1.732
1.5
Which of the following compounds have maximum hydrogen bond strength?
CH3OH
HF
NH3
H2O
Hydrogen bond between two atoms is formed due to
formation of a bond between hydrogen atoms of one molecule and the other
displacement of electrons towards hydrogen atom resulting in a polar molecule
existence of an attractive force which binds hydrogen atom together
displacement of electrons towards more electronegative atom resulting in fractional positive charge on hydrogen
Which of the following statements is true about hydrogen bonding?
ice has maximum density at 0 due to H-bonding
intermolecular H-bonding results in decrease in m.pt and b.pt
KHCl2(HCl-2) exists but KHF2(HF-2) does not exist due to lack of H-bonding in HCl
Cl & N have comparable electronegativitites yet there is no H-bonding in HCl because size of Cl is large
Which of the following has strongest bond?
HI
HF
HCl
HBr
Which of the following observations can be explained on the basis of hydrogen bonding?
i) H-F has higher b.p than other halogen acids
ii) H2O has highest b.p among hydrides of group 16 elements
iii) NH3 has lower b.p than PH3.
(i) & (ii)
(i) & (iii)
(ii) & (iii)
(i),(ii) & (iii)
The correct order of bond lengths P,Q & R is
Q>P>R
P>Q>R
Q>R>P
R>Q>P
PBr2Cl3 can exhibit geometrical isomerism. Geometrical isomers are as follows.
Which of the above mentioned geometrical isomers has/have no dipole(s) ?
only III
only I & II
only II & III
only I
The bond is lengths and bond angles in the molecules of methane, ammonia and water may be represented as follows;
Choose the correct statement regarding the trend.
decreasing bond angle is caused due to decreasing bond pair-bond pair repulsion
bond angle increases due to increase in non-bonding electron pair
increasing s-characteristics in bonding hybridised orbital cause decrease in bond length
increasing repulsion between hydrogen atoms cause bond length to decrease
Mark out the incorrect match of shape
[SbF5]2- -square pyramidal
XeOF2- trigonal planar
NH2- V shaped
ICl-4 – square planar
