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XI_Chemistry_New_Chapter_4_Chemical_Bonding_&_Molecular_Structure

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  • June 23, 2024
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  • 2023/2024
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XI Chemistry_New Chapter-4_Chemical Bonding Molecular Structure [True or False Statement Questions]
Sl # Statement [INTRO & 4.1 KOSSEL-LEWIS APPROACH TO CHEMICAL BONDING] True/False

A compound with an odd number of electrons always violates the octet rule for all atoms
1 FALSE
involved.
2 A molecule is a group of atoms with characteristic properties. TRUE
All compounds with more than eight valence electrons around the central atom exhibit
3 FALSE
expanded octets.
4 All elements in and beyond the third period of the periodic table follow the octet rule. FALSE
5 All noble gases can form compounds that obey the octet rule. FALSE
Atoms achieve stable octets through chemical bonds, either by transferring or sharing
6 TRUE
electrons.
7 BeH2 violates the octet rule due to the presence of boron. FALSE
8 Chemical bonding is a result of the sharing of electrons between atoms. FALSE
Chemical bonds refer to attractive forces holding constituents together through electron
9 TRUE
sharing or transfer.
Compounds like PF5, SF6, and H2SO4 exhibit expanded octets with more than eight electrons
10 TRUE
around the central atom.
11 Compounds with odd numbers of electrons cannot exist according to the octet rule. FALSE
Covalent bonds are formed by the electrostatic attraction between positive and negative
12 FALSE
ions.
Covalent bonds form through the sharing of electron pairs between atoms, and multiple
13 TRUE
bonds involve sharing more than one electron pair.
Covalent bonds involve the sharing of electron pairs between atoms to achieve a stable octet
14 FALSE
in their valence shells.
15 Electrostatic attraction stabilizes negative and positive ions in chemical bonds. TRUE
Elements beyond the third period can exhibit an expanded octet phenomenon due to
16 TRUE
available 3d orbitals.
Elements beyond the third period cannot exceed an octet in their valence shells due to the
17 FALSE
lack of available d orbitals.
Expanded octet occurs in compounds of elements from the first two periods of the periodic
18 FALSE
table.
19 Formal charge helps in selecting the most stable Lewis structure for a molecule. TRUE
20 Formal charge helps select the lowest energy Lewis structure in a molecule. FALSE
Formation of negative ions from halogen atoms and positive ions from alkali metal atoms
21 TRUE
involves electron gain and loss.
Group valence can be calculated based on the number of dots in Lewis symbols or by
22 TRUE
subtracting the number of dots from eight.
Highly electronegative halogens and electropositive alkali metals are separated by noble
23 FALSE
gases in the periodic table.
Hybridization involving s, p, and d orbitals leads to the formation of different covalent
24 TRUE
molecules with varying shapes.
Hybridization involving s, p, and f orbitals leads to the formation of different types of covalent
25 FALSE
molecules with varying shapes.
Hydrogen bonding is a strong covalent bond formed between hydrogen atoms and non-metal
26 FALSE
atoms.
Hydrogen bonding is a weak electrostatic attraction between hydrogen and highly
27 TRUE
electronegative atoms.
In 1916, Kössel and Lewis independently explained chemical bonding based on electrons and
28 TRUE
noble gas inertness.
29 In H2O, each hydrogen atom forms a single covalent bond with the oxygen atom. FALSE
In Kössel and Lewis's model, the maximum number of electrons that can surround a nucleus is
30 FALSE
six.

1 OF 31 RI_Best Wishes

, XI Chemistry_New Chapter-4_Chemical Bonding Molecular Structure [True or False Statement Questions]
Sl # Statement [INTRO & 4.1 KOSSEL-LEWIS APPROACH TO CHEMICAL BONDING] True/False

In Lewis structures, each shared electron pair is equally owned by both the combining atoms.
31 FALSE
In molecules with an odd number of electrons, the octet rule is always satisfied for all atoms.
32 FALSE
Incomplete octets are common in compounds of elements with less than four valence
33 FALSE
electrons, such as LiCl, BeH2, and BCl3.
Incomplete octets are observed in compounds where the central atom has fewer than eight
34 TRUE
valence electrons.
35 Ionic bonds are stabilized by electrostatic attraction between positive and negative ions. TRUE
36 Lewis dot structures accurately represent the actual shapes of molecules. FALSE
Lewis dot structures help in understanding the formation and properties of molecules by
37 FALSE
representing shared pairs of electrons and the octet rule.
Lewis dot structures represent shared electron pairs and adherence to the octet rule in
38 TRUE
molecules.
Lewis postulated that atoms achieve a stable octet only by the sharing of a pair of electrons.
39 FALSE
40 Lewis structures help in predicting the shapes of molecules. FALSE
Lewis structures provide a useful picture of bonding in molecules and ions based on shared
41 TRUE
electron pairs and octet rule.
Lewis symbols represent all electrons in an atom, including inner shell electrons involved in
42 FALSE
chemical combinations.
Lewis symbols represent the total number of electrons in an atom, including both inner and
43 FALSE
outer shell electrons.
Maisel highlighted that the formation of ions results in stable noble gas electronic
44 TRUE
configurations.
45 Multiple bonds can only be formed between identical atoms. FALSE
46 Multiple bonds form when atoms share more than one electron pair. FALSE
Nitric oxide (NO) and nitrogen dioxide (NO2) both have complete octets around their nitrogen
47 FALSE
atoms.
48 Noble gases do not follow the octet rule due to their special electronic configurations. FALSE
Noble gases have a stable outer shell configuration of eight electrons, except for helium,
49 TRUE
which has a duplet.
50 Noble gases never form compounds since they are chemically inert. FALSE
Noble gases separate highly electronegative halogens and highly electropositive alkali metals
51 TRUE
in the periodic table.
52 Octet rule accounts for the shape and relative stability of molecules. FALSE
Sodium chloride (NaCl) is formed by the sharing of a pair of electrons between the sodium
53 FALSE
and chlorine atoms.
Some compounds have exceptions to the octet rule, such as incomplete octets and odd-
54 TRUE
electron molecules.
Stable octet formation is essential for atoms to achieve a noble gas electronic configuration
55 TRUE
through chemical bonds.
The atom has a positively charged 'Kernel' surrounded by an outer shell with a maximum of
56 TRUE
eight electrons.
The bond formed by electrostatic attraction between positive and negative ions is called the
57 TRUE
electrovalent (ionic) bond.
The expanded octet occurs when elements have less than eight valence electrons around the
58 FALSE
central atom.
The expanded octet occurs when elements have more than eight valence electrons around
59
the central atom. TRUE

2 OF 31 RI_Best Wishes

, XI Chemistry_New Chapter-4_Chemical Bonding Molecular Structure [True or False Statement Questions]
Sl # Statement [INTRO & 4.1 KOSSEL-LEWIS APPROACH TO CHEMICAL BONDING] True/False

The formal charge of an atom in a Lewis structure is defined as the difference between its
60 TRUE
valence electrons and the assigned electrons.
61 The formation of an ionic bond involves the sharing of electrons between atoms. FALSE
The Kassel-Lewis approach explains chemical bonding based on the reactivity of noble gases.
62 FALSE
63 The Lewis dot structure for NH3 shows three single bonds. FALSE
The Lewis structure of a molecule accurately represents the actual bond lengths and angles.
64 FALSE
65 The Lewis structure of CO2 involves a single bond between carbon and oxygen. FALSE
The Lewis structure of NH3 involves a triple bond between nitrogen and three hydrogen
66 FALSE
atoms.
The Lewis structure of O3 shows that all oxygen atoms have a complete octet of electrons.
67 FALSE
68 The Lewis structure represents the actual shape of a molecule. FALSE
The Lewis structure with the smallest formal charges on the atoms is always the lowest
69 FALSE
energy structure for a given species.
The molecular orbital theory explains the formation of homonuclear diatomic molecules
70 FALSE
through the transfer of electrons.
71 The octet rule applies mainly to second-period elements. FALSE
72 The octet rule is a fundamental principle in explaining chemical bonding. TRUE
The octet rule limitations include exceptions with incomplete octets, odd-electron molecules,
73 FALSE
and expanded octets.
74 Triple bonds occur in N2 and C2H2, with three shared electron pairs between atoms. TRUE
Valence Shell Electron Pair Repulsion (VSEPR) theory predicts the geometry of simple
75 TRUE
molecules based on the arrangement of valence electrons around the central atom.
VSEPR theory predicts the geometry of simple molecules based on the arrangement of core
76 FALSE
electrons around the central atom.
Xenon and krypton are examples of noble gases that form compounds with oxygen and
77 TRUE
fluorine.




3 OF 31 RI_Best Wishes

, XI Chemistry_New Chapter-4_Chemical Bonding Molecular Structure [True or False Statement Questions]
True/False
Sl # Statement [4.2 IONIC OR ELECTROVALENT BOND]
Crystal geometry affects the direct calculation of lattice enthalpy from ion attraction and TRUE
1
repulsion.
2 Crystal geometry factors play a negligible role in determining lattice enthalpy. FALSE
Electron affinity is the enthalpy change when a gas phase atom gains an electron. (Electron FALSE
3
affinity is the negative of the energy change accompanying electron gain.)
Electron gain enthalpy refers to the enthalpy change (energy release) when a gas phase atom TRUE
4
in its ground state gains an electron.
5 Elements like sulfur obey the octet rule in most of their compounds. FALSE
Factors associated with crystal geometry are not relevant in determining the lattice enthalpy FALSE
6
of an ionic solid.
Factors associated with crystal geometry must be considered when calculating lattice TRUE
7
enthalpy, as it involves both attractive and repulsive forces between ions.
Formation of ionic compounds depends on ease of ion formation and lattice arrangement. TRUE
8
In an ionic bond, both the cation and anion gain or lose electrons to achieve a stable electron TRUE
9
configuration.
In ionic solids, despite positive sums of electron gain and ionization enthalpy, lattice TRUE
10
formation stabilizes the crystal structure.
In ionic solids, the sum of the electron gain enthalpy and the ionization enthalpy is always FALSE
11
negative.
Ionic bonds are always formed between elements with low ionization enthalpies and FALSE
12
elements with high electron gain enthalpies.
Ionic bonds are formed more easily between elements with low ionization enthalpies and TRUE
13
high negative electron gain enthalpies.
Ionic compounds are generally more stable than covalent compounds due to their strong TRUE
14
lattice enthalpies (enthalpy of lattice formation).
Ionic compounds conduct electricity when molten or dissolved in water due to the mobility of TRUE
15
ions.
Ionic compounds formed by the ammonium ion (NH4+) as the cation are exceptions to the TRUE
16
rule that cations come from metallic elements.
Ionic compounds have a high melting and boiling point due to the strong electrostatic forces TRUE
17
between ions in the lattice.
Ionic compounds have disordered three-dimensional arrangements of cations and anions held FALSE
18
together by weak interactions.
Ionic compounds in the crystalline state form orderly three-dimensional arrangements of TRUE
19
cations and anions held together by coulombic interaction energies.
Ionic compounds tend to be more soluble in water than covalent compounds due to their TRUE
20
polar nature.
Ionic compounds tend to have higher melting and boiling points compared to covalent TRUE
21
compounds due to stronger intermolecular forces.
Ionization enthalpy for Na+ formation from Na(g) is 495.8 kJ/mol, and electron gain enthalpy TRUE
22
for Cl(g) + e– → Cl–(g) is –348.7 kJ/mol.
Ionization involves adding electrons to form a positive ion, while negative ions result from the FALSE
23
removal of electrons.
Lattice enthalpy can be directly calculated from the interaction of forces of attraction and FALSE
24
repulsion between ions in the solid crystal.
Lattice enthalpy can't be directly calculated from forces of attraction and repulsion between TRUE
25
ions; crystal geometry factors are essential.
Lattice enthalpy doesn't determine ionic compound stability; stability depends on achieving FALSE
26
an octet of electrons around the ionic species in the gaseous state.

4 OF 31 RI_Best Wishes

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