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
1 A molecule is a group of atoms that exists together and has characteristic properties. TRUE
2 A single covalent bond involves sharing one electron pair between two atoms. TRUE
3 A single covalent bond involves the sharing of two electron pairs between atoms. FALSE
4 According to Lewis, atoms achieve a stable octet when they are linked by physical bonds. FALSE
5 All atoms in a molecule contribute to forming a stable outer octet of electrons. FALSE
6 All atoms in a molecule have the same formal charge. FALSE
All chemical compounds are formed by the sharing of a pair of electrons between atoms.
7 FALSE
8 All combinations of atoms are possible in chemical bonding. FALSE
9 Atoms achieve a stable octet when linked by covalent bonds. FALSE
10 Atoms achieve a stable octet when linked by ionic bonds. FALSE
Atoms combine due to the electrostatic attraction between their positive and negative
11 FALSE
charges.
12 Atoms combine due to their tendency to achieve stability. TRUE
Atoms combine to achieve (increase) stability by achieving a stable octet of electrons in their
13 TRUE
valence shells.
14 Atoms combine to achieve a stable electronic configuration in their inner shells. FALSE
15 Atoms combine to achieve a stable electronic configuration. TRUE
16 Atoms with an odd number of electrons cannot form molecules. FALSE
17 Bonding helps to lower the energy of a system and achieve stability. TRUE
18 Chemical bond refers to the attractive force that holds different constituents together. TRUE
19 Chemical bonding is a result of repulsion between atoms. FALSE
20 Chemical bonding is a result of the sharing of electrons between atoms. TRUE
21 Chemical bonding is nature's way of raising the energy of a system to achieve stability. FALSE
22 Chemical bonding results from the repulsion between atoms' valence electrons. FALSE
23 Chemical bonds are a result of the attraction between positively charged nuclei. TRUE
24 Chemical bonds are formed due to the electrostatic repulsion between atoms. FALSE
Chemical compounds form by the combination of atoms of different elements in specific
25 TRUE
ways.
26 Compounds with an incomplete octet are commonly found in nature. FALSE
27 Compounds with an odd number of electrons are highly reactive. TRUE
28 Compounds with an odd number of electrons do not follow the octet rule. TRUE
29 Compounds with less than eight valence electrons are common. TRUE
30 Covalent bonding involves the sharing of a pair of protons between two atoms. FALSE
31 Covalent bonds involve the sharing of only one electron pair between atoms. TRUE
32 Covalent bonds involve the sharing of valence electrons. TRUE
33 Covalent bonds satisfy the octet rule for both bonded atoms. TRUE
34 Double bonds involve the sharing of two electron pairs between two atoms. TRUE
Each bonded atom in a covalent bond contributes at least one electron to the shared pair.
35 TRUE
36 Elements beyond the third period can form compounds with an expanded octet. TRUE
37 Elements beyond the third period cannot form compounds with an expanded octet. FALSE
38 Elements beyond the third period cannot have 3d orbitals available for bonding. FALSE
Elements beyond the third period of the periodic table can form compounds with more than
39 TRUE
ten valence electrons.
Elements in and beyond the third period of the periodic table have 3d orbitals available for
40 TRUE
bonding.
41 Elements in the third period can have an expanded octet. TRUE
42 Elements with less than four valence electrons can have an incomplete octet. TRUE
43 Formal charge helps in selecting the highest energy structure for a given species. FALSE
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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
44 Formal charges are a result of electron sharing between atoms. FALSE
45 Formal charges are used to determine the lowest energy structure of a molecule. TRUE
46 Formal charges do not help in selecting the lowest energy structure for a given species. FALSE
47 Formal charges help in determining the real charge separation within a molecule. TRUE
Formal charges help in selecting the lowest energy structure among multiple Lewis structures
48 TRUE
for a given species.
Formation of a negative ion involves gaining electrons, leading to a stable electronic
49 TRUE
configuration.
G.N. Lewis introduced Lewis symbols as a way to represent the number of valence electrons
50 TRUE
in an atom.
51 In a covalent bond, atoms share a pair of electrons. TRUE
In Lewis dot structures, each bonded atom contributes both electrons of the shared pair.
52 TRUE
53 In Lewis structures, formal charges are used to assess the stability of a molecule. TRUE
In Lewis structures, lone pairs are represented as shared pairs of electrons between atoms.
54 FALSE
55 In the CO2 molecule, carbon and oxygen atoms are joined by a single covalent bond. TRUE
56 In the formation of NaCl, an electron is transferred from chlorine to sodium. TRUE
57 In XeF2, xenon forms an incomplete octet with 6 electrons around it. TRUE
58 Ionic crystalline compounds form as a result of the electrovalent bond. TRUE
Kassel and Lewis independently proposed the electronic theory of chemical bonding in 1916.
59 TRUE
Kassel and Lewis provided the first logical explanation of valence based on the reactivity of
60 TRUE
noble gases.
61 Lewis dot structures do not accurately represent the shapes of molecules. FALSE
62 Lewis dot structures do not provide information about the shapes of molecules. TRUE
63 Lewis dot structures help in selecting the lowest energy structure for a given species. TRUE
64 Lewis dot structures provide a partial representation of the actual shapes of molecules. TRUE
65 Lewis dot structures provide a representation of the valence electrons in an atom. TRUE
Lewis succeeded in explaining chemical bonding by incorporating the inertness of noble gases.
66 TRUE
67 Multiple bonds involve the sharing of only one electron pair between atoms. FALSE
Noble gases are exceptions to the octet rule as they form stable compounds with oxygen and
68 TRUE
fluorine.
Noble gases are inert elements that do not combine with other elements to form compounds.
69 FALSE
70 PF3 is an example of a compound with a complete octet around the central atom. FALSE
The attractive force holding constituents together in different chemical species is called a
71 FALSE
molecular bond.
The formation of an ionic bond occurs due to the sharing of electron pairs between atoms.
72 FALSE
73 The Lewis dot structure for NH3 shows three single bonds. TRUE
The Lewis dot structure for NO3- shows a double bond between nitrogen and one oxygen
74 TRUE
atom.
The Lewis dot structure for SO2 involves a double bond between sulfur and one oxygen atom.
75 TRUE
76 The Lewis dot structure of a molecule does not influence its stability or energy. FALSE
77 The Lewis symbols represent the total number of valence electrons in an atom. TRUE
78 The Lewis symbols show only the valence electrons in an atom. TRUE
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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
The octet rule does not apply to compounds involving elements beyond the third period of
79 FALSE
the periodic table.
80 The octet rule is a fundamental principle in explaining chemical bonding. TRUE
81 The octet rule is based on the observation that noble gases have eight valence electrons. TRUE
82 The octet rule is mainly applicable to second-period elements. TRUE
83 The octet rule is not applicable to elements with more than four valence electrons. FALSE
84 The octet theory accounts for the relative stability of molecules. FALSE
3 OF 55 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]
Ammonium ion (NH4+) is an exception in forming ionic compounds, consisting of two non- FALSE
1
metallic elements.
2 An ionic bond is formed between two atoms of the same element. FALSE
3 An ionic bond is formed between two non-metal atoms. FALSE
An ionic compound is composed of neutral atoms that share electrons to achieve stability. FALSE
4
5 Electron gain enthalpy is always endothermic. FALSE
Electron gain enthalpy refers to the enthalpy change (energy release) when a gas phase atom TRUE
6
in its ground state gains an electron.
In an ionic bond, both the cation and anion gain or lose electrons to achieve a stable electron TRUE
7
configuration.
In an ionic bond, both the cation and anion lose or gain electrons to achieve a stable electron FALSE
8
configuration.
In ionic solids, the sum of electron gain enthalpy and ionization enthalpy is always negative. FALSE
9
In ionic solids, the sum of electron gain enthalpy and ionization enthalpy is always positive. FALSE
10
In the formation of NaCl, the energy released in the lattice formation compensates for the TRUE
11
ionization and electron gain enthalpies.
Ionic bonds are primarily formed between elements with low ionization enthalpies and high FALSE
12
negative values of electron gain enthalpy.
13 Ionic bonds involve the sharing of valence electrons between atoms to achieve stability. FALSE
14 Ionic bonds occur between atoms of significantly different electronegativity values. TRUE
15 Ionic bonds occur between atoms of similar electronegativity values. FALSE
16 Ionic compounds are generally insoluble in water due to their strong lattice enthalpies. FALSE
Ionic compounds are generally more stable than covalent compounds due to their strong TRUE
17
lattice enthalpies (enthalpy of lattice formation).
Ionic compounds are generally poor conductors of electricity in both solid and molten states. FALSE
18
19 Ionic compounds are generally poor conductors of electricity in the solid state. FALSE
Ionic compounds are primarily formed due to the arrangement of positive and negative ions TRUE
20
in the solid, specifically the lattice of the crystalline compound.
21 Ionic compounds are typically composed of metal cations and non-metal anions. TRUE
Ionic compounds are typically soluble in nonpolar solvents due to their high lattice enthalpies. FALSE
22
Ionic compounds conduct electricity when molten or dissolved in water due to the mobility of TRUE
23
ions.
Ionic compounds generally have low solubility in polar solvents due to their strong lattice FALSE
24
enthalpies.
Ionic compounds have a high melting and boiling point due to the strong electrostatic forces TRUE
25
between ions in the lattice.
Ionic compounds in the crystalline state have disordered arrangements of cations and anions FALSE
26
held together by coulombic interactions.
Ionic compounds tend to be more soluble in nonpolar solvents due to their nonpolar nature. FALSE
27
Ionic compounds tend to be more soluble in water than covalent compounds due to their TRUE
28
polar nature.
Ionic compounds tend to have higher melting and boiling points compared to covalent TRUE
29
compounds due to stronger intermolecular forces.
30 Ionic compounds with larger lattice enthalpy are more stable. TRUE
4 OF 55 RI_Best Wishes
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