Concepts of Inorganic Chemistry Practice Exam
Which of the following is the most appropriate description of the modern atomic theory?
Atoms are indivisible particles
B. Electrons orbit the nucleus in fixed orbits
C. Electrons exist in orbitals based on probability
D. Atoms are made up of only protons and neutrons
The Aufbau principle states that electrons will fill:
The orbitals with the highest energy first
B. The orbitals with the lowest energy first
C. The orbitals randomly
D. The 3d orbitals before the 4s orbitals
The ionization energy generally:
Decreases across a period from left to right
B. Increases down a group
C. Decreases down a group
D. Remains constant across periods
Which of the following compounds is named correctly according to IUPAC nomenclature?
NaCl – Sodium chloride
B. SO3 – Sulfur trioxide
C. NH4Cl – Nitrogen tetrahydride chloride
D. H2O – Dihydrogen oxide
Which of the following statements about ionic bonding is correct?
Ionic bonds result from the sharing of electrons between atoms
B. Ionic bonds are formed between two nonmetals
C. Ionic bonds are formed between a metal and a nonmetal
D. Ionic bonds are weak and non-conductive in solid form
Which of the following is a characteristic of a covalent bond?
Electrons are transferred from one atom to another
B. Both atoms gain a full outer shell of electrons
C. Atoms form a lattice structure
D. One atom completely loses electrons
What type of bonding is found in the molecule O2?
Ionic bonding
B. Covalent bonding
C. Metallic bonding
D. Hydrogen bonding
In which of the following does the element exhibit its highest oxidation state?
Potassium (K)
B. Sulfur (S)
C. Nitrogen (N)
D. Iron (Fe)
The periodic trend for atomic radius generally:
Increases from top to bottom within a group
B. Increases across a period from left to right
C. Decreases as you move down a group
D. Is not related to any periodicity
Which of the following elements has the largest ionization energy?
Sodium (Na)
B. Chlorine (Cl)
C. Oxygen (O)
D. Argon (Ar)
Which of the following is an example of a paramagnetic substance?
Oxygen (O2)
B. Neon (Ne)
C. Argon (Ar)
D. Helium (He)
What is the electron configuration of a neutral oxygen atom (atomic number 8)?
1s² 2s² 2p⁴
B. 1s² 2s² 2p⁶
C. 1s² 2p⁶
D. 1s² 2p³
Which of the following compounds is an example of an ionic compound?
Cl2
B. H2O
C. NaCl
D. CH4
The term “ligand” refers to:
An atom in the center of a coordination complex
B. A molecule or ion that donates electrons to a metal ion
C. The bond formed between two ions
D. A type of covalent bond
Which of the following is a characteristic of transition metals?
They only form anions
B. They typically have a low melting point
C. They exhibit a variety of oxidation states
D. They form very stable compounds
Which of the following is true about the crystal field theory?
It explains the color of coordination compounds
B. It describes the bonding in covalent molecules
C. It only applies to organic molecules
D. It explains the formation of covalent bonds
The magnetic property of a molecule is primarily determined by:
The number of protons in the nucleus
B. The number of neutrons in the nucleus
C. The presence of unpaired electrons
D. The size of the molecule
Which of the following elements is least likely to form a stable ion?
Potassium (K)
B. Calcium (Ca)
C. Iron (Fe)
D. Argon (Ar)
In an organometallic compound, the metal atom is usually bonded to:
A non-metal
B. A carbon atom
C. A noble gas
D. An oxygen atom
Which of the following is a property of transition metal complexes?
They are typically colorless
B. They exhibit various colors due to d-d transitions
C. They are always diamagnetic
D. They only form octahedral complexes
Which of the following elements is an example of a lanthanide?
Cerium (Ce)
B. Lead (Pb)
C. Titanium (Ti)
D. Uranium (U)
The main group elements typically follow which type of bonding?
Ionic bonding only
B. Covalent bonding only
C. Both ionic and covalent bonding
D. Metallic bonding
Which of the following statements is true about the bonding in NaCl?
Sodium donates two electrons to chlorine
B. The sodium ion gains an electron from chlorine
C. Sodium and chlorine share electrons equally
D. Sodium loses an electron to chlorine, forming an ionic bond
What is the primary characteristic of bioinorganic chemistry?
The study of organic molecules containing metals
B. The role of metals in biological systems
C. The study of inorganic compounds without metals
D. The use of metals in industrial processes
Which of the following transition metals exhibits the highest oxidation state in its compounds?
Chromium (Cr)
B. Manganese (Mn)
C. Iron (Fe)
D. Copper (Cu)
What does the crystal field splitting energy (Δ) depend on?
The temperature of the environment
B. The nature of the ligand and the metal ion
C. The ionic radius of the metal ion
D. The shape of the coordination complex
The chemical reactivity of an element is primarily determined by:
The atomic number
B. The number of protons
C. The arrangement of electrons in the outer shell
D. The mass of the atom
Which of the following is a characteristic of organometallic compounds?
They are typically unstable and highly reactive
B. They contain metal-carbon bonds
C. They have no applications in catalysis
D. They are always insoluble in organic solvents
Which of the following statements about the transition metals is false?
They have high melting points
B. They tend to form colored compounds
C. They typically have large atomic and ionic radii
D. They have a partially filled d-subshell
Which of the following best explains the periodic trend of electron affinity?
Electron affinity increases across a period from left to right
B. Electron affinity decreases as you move down a group
C. Electron affinity is not periodic
D. Electron affinity increases down a group
31. Which of the following compounds exhibits covalent bonding?
NaCl
B. MgO
C. CO2
D. K2O
32. The ionic radius of an element decreases when it:
Gains electrons
B. Loses electrons
C. Gains protons
D. Loses protons
33. Which of the following is true for the electron configuration of transition metals?
They fill the s-orbital before the d-orbital
B. They always have completely filled d-orbitals
C. They lose electrons from the s-orbital before the d-orbital
D. They never lose electrons from their d-orbitals
34. Which element has the highest electronegativity?
Oxygen (O)
B. Fluorine (F)
C. Chlorine (Cl)
D. Nitrogen (N)
35. Which of the following statements about transition metals is correct?
Transition metals have completely filled d-orbitals in their neutral state
B. Transition metals generally form only one stable oxidation state
C. Transition metals have variable oxidation states
D. Transition metals never form complex ions
36. In a coordination complex, what is the role of the ligand?
It donates electrons to the metal center
B. It stabilizes the metal’s oxidation state
C. It forms ionic bonds with the metal
D. It oxidizes the metal ion
37. What is the crystal field splitting energy (Δ) in an octahedral complex related to?
The atomic size of the central metal
B. The ligand field strength
C. The oxidation state of the metal ion
D. The number of electrons in the d-orbitals
38. Which of the following is NOT a characteristic of transition metal chemistry?
Formation of colored complexes
B. High ionization energies
C. Formation of complexes with ligands
D. Predominance of high oxidation states
39. Which of the following would be considered a hard acid according to Pearson’s Hard and Soft Acids and Bases (HSAB) theory?
Hg²⁺
B. Na⁺
C. Cu²⁺
D. I⁻
40. Which of the following is a property of ionic solids?
They are good conductors of electricity in the solid state
B. They have high melting and boiling points
C. They are not soluble in water
D. They tend to form molecular structures
41. In which type of bond are electrons shared equally between two atoms?
Polar covalent bond
B. Nonpolar covalent bond
C. Ionic bond
D. Metallic bond
42. What is the expected geometry of a molecule with a steric number of 4 and no lone pairs?
Linear
B. Trigonal planar
C. Tetrahedral
D. Octahedral
43. Which of the following transition metals commonly forms a square planar complex?
Copper (Cu)
B. Iron (Fe)
C. Nickel (Ni)
D. Platinum (Pt)
44. Which of the following is an example of an organometallic compound?
NaCl
B. Fe(CO)₅
C. H₂O
D. CCl₄
45. The magnetic behavior of a molecule is explained by:
The number of protons in the nucleus
B. The number of neutrons in the nucleus
C. The number of paired and unpaired electrons
D. The number of bonds between atoms
46. Which of the following is a characteristic of the d-block elements?
They have a single oxidation state
B. They form complexes with ligands
C. They tend to form highly stable compounds
D. They exhibit no magnetic properties
47. Which of the following compounds has an expanded octet?
H2O
B. NH3
C. SF6
D. CH4
48. Which of the following transition metals has the most stable +2 oxidation state?
Copper (Cu)
B. Iron (Fe)
C. Zinc (Zn)
D. Chromium (Cr)
49. What is the hybridization of the central atom in the molecule CH4?
sp
B. sp²
C. sp³
D. sp³d²
50. Which of the following is the correct electron configuration for the Fe²⁺ ion?
[Ar] 3d⁶
B. [Ar] 3d⁷
C. [Ne] 3s² 3p⁶
D. [Ar] 3d⁸
51. Which of the following is true about the concept of effective nuclear charge (Zeff)?
It increases from left to right across a period
B. It decreases down a group
C. It is the net attraction between electrons and the nucleus
D. All of the above
52. Which of the following would you expect to be a good ligand in a coordination complex?
I⁻
B. Na⁺
C. F⁻
D. Cl₂
53. The coordination number of a metal ion refers to:
The number of bonds formed between metal and ligand
B. The total number of electrons donated by the ligands
C. The number of valence electrons on the metal
D. The charge of the metal ion
54. Which of the following elements is most likely to form an ion with a +2 charge?
Fluorine (F)
B. Oxygen (O)
C. Calcium (Ca)
D. Nitrogen (N)
55. What is the primary reason for the stability of transition metal complexes?
The ability to form covalent bonds
B. The stability provided by ligand field splitting
C. The high atomic radius of transition metals
D. The formation of stable oxidation states
56. Which of the following is a defining feature of a polar covalent bond?
Electrons are shared equally between atoms
B. Electrons are transferred from one atom to another
C. Electrons are shared unequally between atoms
D. Both atoms have the same electronegativity
57. Which of the following is an example of a chelate?
Water (H₂O)
B. EDTA
C. Sodium chloride (NaCl)
D. Methane (CH₄)
58. Which of the following metals typically forms a +3 ion?
Sodium (Na)
B. Iron (Fe)
C. Aluminum (Al)
D. Zinc (Zn)
59. Which of the following best describes the bonding in a metal?
Electrons are shared equally between two atoms
B. Electrons are delocalized and move freely throughout the structure
C. Electrons are transferred from one atom to another
D. Electrons are held tightly in individual atoms
60. What is the oxidation state of sulfur in the compound H₂SO₄?
-2
B. +2
C. +4
D. +6
61. Which of the following is true about the bonding in an ionic compound?
Electrons are shared equally between atoms
B. Electrons are transferred from one atom to another
C. Electrons are delocalized and move freely throughout the structure
D. Electrons are shared unequally between atoms
62. Which of the following compounds is an example of a coordination compound?
NaCl
B. H₂O
C. [Cu(NH₃)₄]²⁺
D. CO₂
63. The oxidation state of manganese in MnO₄⁻ is:
+2
B. +4
C. +7
D. +3
64. Which of the following best describes the magnetic behavior of a paramagnetic substance?
It has all electrons paired
B. It is weakly attracted to a magnetic field
C. It is strongly repelled by a magnetic field
D. It is not affected by a magnetic field
65. The molecular geometry of a molecule with the formula AB₄ (where A is the central atom and B are identical atoms) and no lone pairs on the central atom is:
Linear
B. Trigonal bipyramidal
C. Tetrahedral
D. Octahedral
66. Which of the following elements will exhibit the highest first ionization energy?
Na
B. Cl
C. Ne
D. Ar
67. Which of the following statements best explains the periodic trend in electronegativity?
Electronegativity increases as the atomic radius increases
B. Electronegativity decreases as the atomic radius increases
C. Electronegativity increases as you move down a group
D. Electronegativity is independent of atomic radius
68. Which of the following coordination compounds has a square planar geometry?
[Cu(H₂O)₆]²⁺
B. [Ni(CO)₄]
C. [PtCl₄]²⁻
D. [Fe(H₂O)₆]²⁺
69. Which of the following is the strongest oxidizing agent?
Fe²⁺
B. Mn²⁺
C. Cr₂O₇²⁻
D. Cu²⁺
70. The transition from one oxidation state to another in transition metals is often accompanied by:
A change in atomic size
B. A change in electron configuration
C. A change in bond polarity
D. All of the above
71. Which of the following species has the largest ionic radius?
Na⁺
B. Mg²⁺
C. Al³⁺
D. K⁺
72. Which of the following types of bonds does not occur in molecular compounds?
Covalent bonds
B. Ionic bonds
C. Polar covalent bonds
D. Metallic bonds
73. Which of the following describes the process of ligand exchange in a coordination complex?
A ligand binds to the metal ion, replacing another ligand
B. A ligand loses its electrons and dissociates from the metal ion
C. A ligand donates electrons to a different molecule
D. A ligand changes its charge
74. Which of the following elements is most likely to form a +1 ion?
Oxygen (O)
B. Sodium (Na)
C. Aluminum (Al)
D. Fluorine (F)
75. Which of the following is the correct order of increasing atomic radius?
Na < K < Mg
B. K < Na < Mg
C. Mg < Na < K
D. Na < Mg < K
76. Which of the following is the correct electron configuration for an O²⁻ ion?
[He] 2s² 2p⁴
B. [Ne]
C. [He] 2s² 2p⁶
D. [Ne] 3s²
77. Which of the following elements is most likely to form a stable complex with a ligand?
Ne
B. Mg
C. Cu
D. Cl
78. Which of the following best describes the bonding in a metallic solid?
Electrons are delocalized and form a “sea” around metal cations
B. Electrons are shared equally between two atoms
C. Electrons are transferred from one atom to another
D. Electrons are tightly held in individual atoms
79. Which of the following ions is an example of a hard acid according to the HSAB theory?
Pb²⁺
B. Hg²⁺
C. Ca²⁺
D. Cu²⁺
80. Which of the following is true for a compound with a high lattice energy?
It is likely to have a high boiling point
B. It is likely to be a gas at room temperature
C. It has weak ionic bonds
D. It is highly soluble in nonpolar solvents
81. Which of the following elements exhibits the highest first ionization energy?
Potassium (K)
B. Magnesium (Mg)
C. Oxygen (O)
D. Fluorine (F)
82. Which of the following metals typically exhibits multiple oxidation states?
Zinc (Zn)
B. Sodium (Na)
C. Iron (Fe)
D. Chlorine (Cl)
83. In the context of molecular orbital theory, which of the following describes the bonding in O₂?
O₂ has two bonding and two antibonding electrons, resulting in a bond order of 0
B. O₂ has two bonding and four antibonding electrons, resulting in a bond order of 1
C. O₂ has eight bonding and two antibonding electrons, resulting in a bond order of 3
D. O₂ has four bonding and four antibonding electrons, resulting in a bond order of 2
84. Which of the following metal ions would be expected to form a tetrahedral coordination complex?
Fe²⁺
B. Cu²⁺
C. Ti⁴⁺
D. Mn²⁺
85. Which of the following would be classified as a ligand with a chelating ability?
H₂O
B. Cl⁻
C. EDTA
D. NH₃
86. Which of the following statements is true about the effective nuclear charge (Zeff)?
It decreases across a period
B. It increases across a period
C. It remains constant across a period
D. It decreases down a group
87. Which of the following statements is true for the chemistry of transition metals?
They only exhibit one oxidation state
B. They form only ionic compounds
C. They exhibit a wide range of oxidation states
D. They are all highly electropositive
88. Which of the following compounds is an example of a d-block metal complex?
NaCl
B. [Ni(CO)₄]
C. Al₂O₃
D. H₂O
89. Which of the following is a property of a covalent bond?
Electrons are transferred from one atom to another
B. Electrons are shared equally or unequally between atoms
C. The resulting compound is always a solid
D. It only occurs between metals
90. Which of the following is true for a compound with a trigonal planar geometry?
It has three bonding pairs and no lone pairs on the central atom
B. It has four bonding pairs and one lone pair on the central atom
C. It has two bonding pairs and two lone pairs on the central atom
D. It has five bonding pairs and no lone pairs on the central atom
91. Which of the following elements is most likely to form an ionic bond with chlorine?
Sodium (Na)
B. Sulfur (S)
C. Nitrogen (N)
D. Phosphorus (P)
92. Which of the following species has the highest ionization energy?
Na
B. Mg
C. Al
D. Si
93. Which of the following best describes the electronic configuration of an iron(III) ion, Fe³⁺?
[Ar] 3d⁶
B. [Ne] 3s² 3p⁶
C. [Ar] 3d⁵
D. [Ar] 3d⁸
94. The geometry of a molecule with the formula AB₂ (where A is the central atom and B are identical atoms) and no lone pairs on the central atom is:
Linear
B. Bent
C. Trigonal planar
D. Tetrahedral
95. Which of the following compounds will exhibit the highest melting point?
NaCl
B. H₂O
C. CO₂
D. CH₄
96. Which of the following metals is most likely to form a +2 ion?
Na
B. Ca
C. Fe
D. Cu
97. What type of hybridization occurs in a molecule with the formula AB₃, where A is the central atom and B are identical atoms?
sp
B. sp²
C. sp³
D. sp³d
98. Which of the following compounds contains a metal-metal bond?
NaCl
B. Fe₃O₄
C. [Fe(CO)₅]
D. H₂O
99. Which of the following is true about the bond length in a molecule?
Longer bonds are typically stronger than shorter bonds
B. Bond length decreases with increasing bond order
C. The bond length is unaffected by the size of atoms involved
D. Bond length increases with increasing bond order
100. Which of the following transition metals forms a stable complex with a ligand such as ammonia (NH₃)?
Sodium (Na)
B. Iron (Fe)
C. Calcium (Ca)
D. Lithium (Li)
101. Which of the following transition metals has the highest magnetic susceptibility?
Copper (Cu)
B. Iron (Fe)
C. Manganese (Mn)
D. Nickel (Ni)
102. Which of the following is true regarding the electronegativity of elements across a period?
Electronegativity decreases as you move from left to right
B. Electronegativity increases as you move from left to right
C. Electronegativity is highest in the middle of the period
D. Electronegativity is the same across the period
103. Which of the following coordination complexes is an example of a 6-coordinate complex?
[Cu(NH₃)₄]²⁺
B. [Cr(H₂O)₆]³⁺
C. [NiCl₄]²⁻
D. [PtCl₃(NH₃)]²⁺
104. Which of the following is an example of a ligand that can only act as a monodentate ligand?
EDTA
B. Ammonia (NH₃)
C. Carbon monoxide (CO)
D. Ethylenediamine (en)
105. The effective nuclear charge (Zeff) experienced by an electron in an atom is:
The number of protons in the nucleus
B. The shielding effect of other electrons
C. The total number of electrons
D. The number of neutrons in the nucleus
106. Which of the following is the strongest acid?
HCl
B. H₂SO₄
C. HF
D. H₂CO₃
107. Which of the following ligands is known for its ability to form a strong coordination bond with transition metals?
Water (H₂O)
B. Chlorine (Cl⁻)
C. Cyanide (CN⁻)
D. Oxygen (O₂)
108. What is the hybridization of the central atom in a molecule with the formula AB₅?
sp
B. sp²
C. sp³
D. sp³d
109. Which of the following elements will most likely form a compound with a trigonal planar geometry?
Oxygen (O)
B. Carbon (C)
C. Boron (B)
D. Nitrogen (N)
110. Which of the following best describes the behavior of a ferromagnetic material?
It is not attracted to a magnetic field
B. It becomes magnetized in the presence of an external magnetic field
C. It has a permanent magnetic moment but does not align with an external magnetic field
D. It is weakly repelled by a magnetic field
111. Which of the following factors can affect the lattice energy of an ionic compound?
The charge of the ions
B. The size of the ions
C. The type of bonding involved
D. Both A and B
112. Which of the following elements has the highest first ionization energy?
Lithium (Li)
B. Oxygen (O)
C. Hydrogen (H)
D. Neon (Ne)
113. Which of the following transition metals forms a +3 ion as its most stable oxidation state?
Chromium (Cr)
B. Manganese (Mn)
C. Iron (Fe)
D. Copper (Cu)
114. Which of the following is a property of ionic solids?
High melting points
B. Low electrical conductivity
C. Soluble in nonpolar solvents
D. Malleable and ductile
115. Which of the following types of bonding occurs between atoms in a metal?
Ionic bonding
B. Covalent bonding
C. Metallic bonding
D. Hydrogen bonding
116. Which of the following is the most likely oxidation state of copper in a copper(I) chloride complex?
+1
B. +2
C. +3
D. 0
117. The structure of a molecule with the formula AB₄, where A is the central atom and B are identical atoms, and two lone pairs on the central atom, is:
Trigonal bipyramidal
B. Tetrahedral
C. Trigonal planar
D. Bent
118. Which of the following is an example of a covalent network solid?
Sodium chloride (NaCl)
B. Diamond (C)
C. Iron (Fe)
D. Magnesium oxide (MgO)
119. Which of the following transition metals does not typically form a +2 ion?
Zinc (Zn)
B. Copper (Cu)
C. Iron (Fe)
D. Magnesium (Mg)
120. Which of the following is the most likely oxidation state for a transition metal in a complex with chloride (Cl⁻) and water (H₂O) ligands?
+1
B. +2
C. +3
D. +4
121. Which of the following is an example of an amphoteric oxide?
Na₂O
B. Al₂O₃
C. FeO
D. MgO
122. Which of the following transition metals exhibits a +3 oxidation state as its most stable state?
Scandium (Sc)
B. Chromium (Cr)
C. Manganese (Mn)
D. Iron (Fe)
123. Which of the following ligands is a bidentate ligand?
Ammonia (NH₃)
B. Cyanide (CN⁻)
C. Ethylenediamine (en)
D. Chloride (Cl⁻)
124. Which of the following ions has the largest ionic radius?
Na⁺
B. Mg²⁺
C. Al³⁺
D. K⁺
125. Which of the following compounds has the lowest lattice energy?
NaCl
B. LiCl
C. KCl
D. CsCl
126. The geometry of the molecule BF₃ (boron trifluoride) is:
Linear
B. Trigonal planar
C. Tetrahedral
D. Bent
127. Which of the following elements has the highest electronegativity?
Oxygen (O)
B. Nitrogen (N)
C. Fluorine (F)
D. Chlorine (Cl)
128. The bond between sodium and chlorine in sodium chloride (NaCl) is best described as:
Covalent
B. Polar covalent
C. Ionic
D. Metallic
129. Which of the following is the correct order of increasing atomic radius?
Na < Mg < Al
B. Al < Mg < Na
C. Na < Al < Mg
D. Mg < Na < Al
130. Which of the following is true about transition metals?
They only form +2 oxidation states.
B. They are typically nonmetals.
C. They form colored complexes.
D. They do not form coordination compounds.
131. Which of the following compounds contains an example of a ligand that can form coordinate covalent bonds with metal centers?
NaCl
B. H₂O
C. NaOH
D. CO₂
132. Which of the following ions has the highest charge density?
Na⁺
B. Mg²⁺
C. Al³⁺
D. Fe³⁺
133. Which of the following ions is paramagnetic?
O₂⁻
B. N₂
C. O₂
D. Ne
134. Which of the following best describes the electronic structure of a copper(II) ion (Cu²⁺)?
[Ar] 3d⁸
B. [Ar] 3d⁷
C. [Ar] 3d⁶
D. [Ar] 3d⁵
135. Which of the following molecules exhibits sp³ hybridization?
CH₄
B. CO₂
C. BF₃
D. C₂H₂
136. The element that is most likely to form a +1 ion is:
Calcium (Ca)
B. Potassium (K)
C. Aluminum (Al)
D. Nitrogen (N)
137. The structure of the [Ni(CO)₄] complex is:
Square planar
B. Tetrahedral
C. Octahedral
D. Linear
138. Which of the following compounds will most likely have the highest melting point?
NaCl
B. Cl₂
C. CH₄
D. H₂O
139. Which of the following molecules has a trigonal bipyramidal geometry?
PCl₅
B. NH₃
C. CO₂
D. CH₄
140. The compound TiCl₄ has what type of molecular geometry?
Linear
B. Tetrahedral
C. Octahedral
D. Trigonal planar
141. Which of the following is true about the periodic trends in atomic radii?
Atomic radii increase from left to right across a period.
B. Atomic radii increase as you move down a group.
C. Atomic radii do not change in the periodic table.
D. Atomic radii decrease from left to right across a period and increase down a group.
142. Which of the following transition metal complexes is likely to be diamagnetic?
[Fe(CO)₆]
B. [Mn(CO)₆]
C. [Cu(NH₃)₄]²⁺
D. [NiCl₄]²⁻
143. Which of the following elements has the highest first ionization energy?
Sodium (Na)
B. Magnesium (Mg)
C. Oxygen (O)
D. Nitrogen (N)
144. Which of the following is a characteristic of ionic compounds?
They have low melting points.
B. They are poor conductors in the solid state.
C. They are usually gases at room temperature.
D. They have high volatility.
145. The color of a transition metal complex is primarily due to:
The energy gap between the metal’s d-orbitals
B. The absorption of ultraviolet light
C. The overlap of metal and ligand orbitals
D. The ionic radius of the metal ion
146. The compound CH₃OH (methanol) contains which type of bond?
Ionic
B. Covalent
C. Metallic
D. Hydrogen
147. Which of the following elements is least likely to form an octahedral complex?
Fe²⁺
B. Co³⁺
C. Cu²⁺
D. Zn²⁺
148. The type of hybridization of the central atom in a molecule with a formula AB₂, where A is the central atom and B are identical atoms, and the molecule has a linear geometry is:
sp
B. sp²
C. sp³
D. sp³d
149. Which of the following elements has the largest ionization energy?
Hydrogen (H)
B. Lithium (Li)
C. Oxygen (O)
D. Fluorine (F)
150. Which of the following compounds contains a covalent bond?
NaCl
B. MgO
C. H₂O
D. K₂S
151. Which of the following molecules has a tetrahedral geometry?
CH₄
B. CO₂
C. H₂O
D. NH₃
152. Which of the following is the electron configuration of a neutral calcium atom (Ca)?
[Ar] 3d¹⁰ 4s²
B. [Ar] 4s²
C. [Ne] 3s² 3p⁶
D. [Ar] 4s² 3d⁶
153. Which of the following is a property of transition metal compounds?
They are always colorless.
B. They have low melting points.
C. They can exhibit multiple oxidation states.
D. They do not form coordination complexes.
154. Which of the following transition metal complexes is expected to exhibit a low-spin configuration?
[Fe(CO)₆]²⁺
B. [Ni(CO)₄]
C. [Mn(H₂O)₆]²⁺
D. [Cr(H₂O)₆]³⁺
155. Which of the following elements has the highest second ionization energy?
Sodium (Na)
B. Magnesium (Mg)
C. Chlorine (Cl)
D. Oxygen (O)
156. Which of the following ions will most likely form a colorless solution?
Cu²⁺
B. Fe²⁺
C. Ni²⁺
D. Zn²⁺
157. The oxidation state of chlorine in the compound NaClO₃ is:
-1
B. +1
C. +3
D. +5
158. The coordination number of the metal ion in a square planar complex is:
2
B. 4
C. 6
D. 8
159. The ion [Cu(NH₃)₄]²⁺ is:
Paramagnetic
B. Diamagnetic
C. Colorless
D. Inert
160. Which of the following has a closed shell configuration and is inert in reactions?
Na⁺
B. Mg²⁺
C. Ar
D. Xe
161. Which of the following is the strongest oxidizing agent?
Cl₂
B. F₂
C. Br₂
D. I₂
162. Which of the following is a characteristic of covalent compounds?
High melting points
B. Low melting points
C. They conduct electricity in molten state
D. They form crystalline structures
163. Which of the following is a correct statement about the periodic table?
Atomic size decreases across a period from left to right.
B. Electronegativity decreases as you go down a group.
C. Ionization energy decreases as you move from left to right across a period.
D. Nonmetals are found on the left side of the periodic table.
164. The compound CuCl₂ has which type of bonding?
Ionic
B. Covalent
C. Metallic
D. Coordinate covalent
165. Which of the following transition metal ions has the highest magnetic moment?
Fe²⁺
B. Fe³⁺
C. Cu²⁺
D. Mn²⁺
166. Which of the following elements is most likely to form an octahedral complex?
Co³⁺
B. Fe³⁺
C. Zn²⁺
D. Ni²⁺
167. Which of the following is true about the transition metals?
They have completely filled d-orbitals in their ground state.
B. They have low melting points compared to s-block metals.
C. They can form alloys.
D. They do not form any covalent bonds.
168. Which of the following ions has the smallest radius?
Mg²⁺
B. Na⁺
C. K⁺
D. Ca²⁺
169. The Lewis dot structure of which of the following molecules exhibits resonance?
CH₄
B. CO₂
C. O₃
D. NH₃
170. Which of the following is a common feature of the lanthanide series?
They all have the same number of valence electrons.
B. They are all radioactive.
C. They are all metals with high melting points.
D. They form covalent bonds only.
171. The molecular geometry of the NH₃ molecule is:
Linear
B. Trigonal planar
C. Tetrahedral
D. Trigonal pyramidal
172. The bond angle in a molecule with an sp hybridization is:
90°
B. 120°
C. 180°
D. 109.5°
173. Which of the following compounds is formed by the combination of an alkali metal with a halogen?
NaCl
B. MgO
C. Al₂O₃
D. CO₂
174. The magnetic behavior of a substance is due to:
The presence of unpaired electrons
B. The ionic bonds in the substance
C. The presence of a closed electron shell
D. The type of hybridization
175. The coordination number of the metal ion in a [Co(NH₃)₆]³⁺ complex is:
2
B. 3
C. 4
D. 6
176. Which of the following is true for the ionization energies of elements?
Ionization energy increases from left to right across a period.
B. Ionization energy decreases as you go up a group.
C. Ionization energy increases down a group.
D. Ionization energy does not change across a period.
177. Which of the following has the highest boiling point?
CH₄
B. H₂O
C. CO₂
D. NaCl
178. Which of the following types of bonding is found in metals?
Covalent bonding
B. Ionic bonding
C. Metallic bonding
D. Hydrogen bonding
179. Which of the following transition metal ions is most likely to have a high-spin configuration?
Fe³⁺
B. Cu²⁺
C. Co²⁺
D. Ni²⁺
180. Which of the following is a characteristic of the d-block elements?
They only form ionic compounds.
B. They have a completely filled d-subshell in their ground state.
C. They form colored ions and complexes.
D. They do not form coordination complexes.
The bond angle in a perfect octahedral molecule is:
109.5°
B. 120°
C. 180°
D. 90°
Which of the following compounds is paramagnetic due to unpaired electrons?
O₂
B. N₂
C. CO₂
D. H₂
Which element in Group 15 has the smallest atomic radius?
Nitrogen (N)
B. Phosphorus (P)
C. Arsenic (As)
D. Antimony (Sb)
The ability of a ligand to donate electron density to a metal center is best described by:
Electronegativity
B. Oxidation state
C. Basicity
D. Ligand field strength
Which of the following molecules exhibits hydrogen bonding?
CH₄
B. NH₃
C. HCl
D. CCl₄
Which is true for the lanthanide contraction?
Atomic radii increase across the lanthanides.
B. Atomic radii decrease due to poor shielding by f-orbitals.
C. Lanthanides exhibit an increase in metallic character.
D. Electronegativity decreases across the lanthanide series.
Which of the following is an example of a chelating ligand?
H₂O
B. NH₃
C. EDTA
D. Cl⁻
What is the oxidation state of chromium in K₂Cr₂O₇?
+3
B. +6
C. +7
D. +2
Which of the following is a soft acid according to Pearson’s Hard and Soft Acids and Bases (HSAB) theory?
H⁺
B. Ag⁺
C. Al³⁺
D. Na⁺
Which of the following halides is most ionic?
AlF₃
B. AlCl₃
C. AlBr₃
D. AlI₃
The splitting of d-orbitals in an octahedral crystal field leads to:
Equal energy levels
B. Two orbitals at lower energy and three at higher energy
C. Three orbitals at lower energy and two at higher energy
D. Uniform energy across all orbitals
Which element shows the highest electronegativity?
Oxygen (O)
B. Fluorine (F)
C. Nitrogen (N)
D. Chlorine (Cl)
Which compound is an example of a sigma-donor and pi-acceptor ligand?
NH₃
B. H₂O
C. CO
D. Cl⁻
Which transition metal ion forms a deep blue-colored complex with ammonia?
Cu²⁺
B. Fe³⁺
C. Ni²⁺
D. Co²⁺
Which of the following describes ferromagnetic materials?
All electrons are paired.
B. Magnetic domains align in the same direction.
C. Magnetic susceptibility is negative.
D. They are not influenced by external magnetic fields.
Which of the following statements about organometallic compounds is true?
They contain only ionic bonds.
B. They involve metals bonded to organic groups.
C. They are insoluble in all organic solvents.
D. They do not exhibit catalytic activity.
The oxidation state of iron in Fe(CO)₅ is:
+1
B. +2
C. 0
D. +3
Which of the following describes a dative bond?
Bond formed by equal sharing of electrons
B. Bond formed when one atom donates both electrons
C. Bond formed by the overlap of orbitals
D. Bond formed due to electrostatic attraction
The most abundant element in the Earth’s crust is:
Aluminum
B. Silicon
C. Oxygen
D. Iron
Which of the following is an interhalogen compound?
ClF
B. Br₂
C. I₂
D. NaCl
The hybridization of the central atom in XeF₄ is:
sp³
B. sp²
C. sp³d²
D. sp³d
Which of the following has the highest lattice energy?
NaCl
B. MgO
C. CsCl
D. KBr
What is the major product formed when Fe reacts with Cl₂?
FeCl
B. Fe₂Cl₃
C. FeCl₂
D. FeCl₃
In a coordination complex, the number of bonds between the central metal and the ligands is called:
Oxidation state
B. Coordination number
C. Bond order
D. Multiplicity
Which of the following compounds contains an alkali metal?
K₂O
B. Al₂O₃
C. CaO
D. Fe₂O₃
The Jahn-Teller effect is observed in:
Linear complexes
B. Square planar complexes
C. Octahedral complexes
D. Tetrahedral complexes
Which of the following species is a strong field ligand?
H₂O
B. NH₃
C. CO
D. Cl⁻
Which metal is commonly used in the catalytic converter of automobiles?
Platinum
B. Gold
C. Iron
D. Zinc
The most stable oxidation state of manganese is:
+2
B. +3
C. +4
D. +7
What is the primary role of transition metals in biological systems?
To act as structural components
B. To serve as electron carriers
C. To form ionic compounds
D. To increase pH
The electronic configuration of Cu⁺ is:
[Ar] 4s¹ 3d⁹
B. [Ar] 3d¹⁰
C. [Ar] 4s² 3d⁸
D. [Ar] 3d⁹
The molecule with the smallest bond angle is:
H₂O
B. NH₃
C. CH₄
D. CO₂
Which of the following ligands is bidentate?
CN⁻
B. NH₃
C. C₂O₄²⁻
D. Cl⁻
The Haber process is used for:
Synthesizing nitric acid
B. Producing ammonia
C. Manufacturing sulfuric acid
D. Electrolysis of water
Which element forms the most acidic oxide?
Sodium
B. Sulfur
C. Magnesium
D. Potassium
The compound with the highest boiling point is:
NaCl
B. H₂O
C. CH₄
D. NH₃
Which transition metal ion has a d⁵ configuration in its ground state?
Fe³⁺
B. Mn²⁺
C. Cr³⁺
D. Co²⁺
In VSEPR theory, the geometry of a molecule with AX₃E₂ notation is:
Linear
B. Trigonal planar
C. T-shaped
D. Bent
Which property decreases across a period in the periodic table?
Atomic size
B. Ionization energy
C. Electronegativity
D. Effective nuclear charge
Which of the following is an example of a homoleptic complex?
[Fe(H₂O)₆]³⁺
B. [CrCl₂(NH₃)₄]⁺
C. [Ni(CN)₄]²⁻
D. [Co(NH₃)₅Cl]²⁺
Which of the following is a typical property of transition metals?
High electronegativity
B. High melting points
C. Low density
D. Poor conductivity
The color of transition metal complexes is due to:
Electron transfer between ligands
B. d-d transitions in the metal ion
C. Vibrational energy levels
D. The ionic character of the metal-ligand bond
Which of the following molecules has sp hybridization?
CH₄
B. CO₂
C. BF₃
D. NH₃
The most common oxidation state of lanthanides is:
+1
B. +2
C. +3
D. +4
The ligand strength in the spectrochemical series increases in the order:
CO < H₂O < NH₃
B. Cl⁻ < H₂O < CN⁻
C. H₂O < CN⁻ < Cl⁻
D. NH₃ < H₂O < F⁻
Which of the following is a diamagnetic substance?
O₂
B. N₂
C. Fe
D. MnO
Which of the following is the weakest acid?
HCl
B. HF
C. HI
D. HBr
Which of the following is a strong oxidizing agent?
KMnO₄
B. H₂O
C. CH₄
D. NaOH
Which of the following shows a tetrahedral structure?
[Ni(CN)₄]²⁻
B. [NiCl₄]²⁻
C. [Co(CN)₆]³⁻
D. [Cr(H₂O)₆]³⁺
In the periodic table, the elements with the largest atomic radii are found in:
Group 1
B. Group 7
C. Group 17
D. Group 18
Which of the following has the highest electronegativity?
Lithium
B. Beryllium
C. Boron
D. Fluorine
Which of the following statements is true for ionic bonds?
They are directional in nature.
B. They result from the sharing of electrons.
C. They are stronger in polar solvents.
D. They form between elements with a large electronegativity difference.
Which of the following is NOT a transition metal?
Scandium
B. Zinc
C. Chromium
D. Nickel
The effective nuclear charge experienced by outer electrons increases:
Across a group
B. Across a period
C. From nonmetals to metals
D. From cations to anions
Which molecule is polar?
CCl₄
B. BF₃
C. CH₃Cl
D. BeCl₂
Which element has the lowest ionization energy?
Potassium
B. Calcium
C. Magnesium
D. Aluminum
Which of the following best describes d-block elements?
Nonmetals
B. Metalloids
C. Transition metals
D. Noble gases
The most common geometry for a coordination complex with a coordination number of 6 is:
Square planar
B. Tetrahedral
C. Octahedral
D. Linear
Which halogen has the highest boiling point?
Fluorine
B. Chlorine
C. Bromine
D. Iodine
The oxidation state of sulfur in H₂SO₄ is:
+2
B. +4
C. +6
D. +8
Which of the following is the correct order of increasing bond strength?
C=C < C≡C < C-C
B. C-C < C=C < C≡C
C. C≡C < C=C < C-C
D. C-C < C≡C < C=C
Which of the following elements exhibits diagonal relationships in the periodic table?
Magnesium
B. Aluminum
C. Lithium
D. Sodium
What is the oxidation state of chromium in potassium dichromate (K₂Cr₂O₇)?
+2
B. +3
C. +6
D. +7
Which of the following is NOT an interhalogen compound?
ClF
B. BrCl
C. F₂
D. IF₅
Which metal has the highest thermal and electrical conductivity?
Copper
B. Silver
C. Gold
D. Platinum
The magnetic moment of a d⁵ system in the high-spin state is:
0 μB
B. 5.92 μB
C. 3.87 μB
D. 1.73 μB
Which is the hardest naturally occurring substance?
Corundum
B. Diamond
C. Quartz
D. Topaz
Which of the following is an organometallic compound?
Na₂SO₄
B. Fe(CO)₅
C. CH₃OH
D. NH₃
The splitting of d-orbitals in an octahedral field leads to:
Degenerate orbitals
B. Two sets of orbitals: t₂g and eg
C. Equal energy for all d-orbitals
D. None of the above
Which of the following is a lanthanide element?
Thorium
B. Uranium
C. Dysprosium
D. Actinium
The color of K₂CrO₄ is:
Yellow
B. Green
C. Orange
D. Red
Which element has the highest ionization energy in the periodic table?
Oxygen
B. Neon
C. Fluorine
D. Helium
Which of the following has sp² hybridization?
CH₄
B. C₂H₂
C. BF₃
D. NH₃
In the context of coordination chemistry, the term “chelate” refers to:
A ligand forming multiple bonds to a central atom
B. A ligand that donates only one pair of electrons
C. A ligand that forms ionic bonds
D. A monodentate ligand
Which of the following compounds has a square planar geometry?
[Ni(CN)₄]²⁻
B. [Cu(NH₃)₄]²⁺
C. [CoCl₆]³⁻
D. [Fe(CN)₆]³⁻
Which gas is used in the preparation of silicon wafers?
SiH₄
B. SiF₄
C. SiCl₄
D. SiO₂
The main component of the mineral bauxite is:
Al₂O₃
B. Fe₂O₃
C. SiO₂
D. CaO
Which of the following has the highest lattice energy?
NaCl
B. MgO
C. CaO
D. KBr
The unit cell of a face-centered cubic lattice contains how many atoms?
1
B. 2
C. 4
D. 8
Which element forms the most stable oxides?
Sodium
B. Carbon
C. Sulfur
D. Fluorine
Which of the following elements shows +7 oxidation state?
Chlorine
B. Manganese
C. Sulfur
D. Nitrogen
The most abundant element in Earth’s crust is:
Oxygen
B. Silicon
C. Aluminum
D. Iron
Which of the following is a pseudo halogen?
CN⁻
B. F⁻
C. Cl⁻
D. Br⁻
In the solid state, sodium chloride adopts a:
Body-centered cubic lattice
B. Simple cubic lattice
C. Face-centered cubic lattice
D. Hexagonal lattice
The flame test color for potassium is:
Red
B. Green
C. Violet
D. Blue
Which of the following is true for ionic compounds?
They are good conductors of electricity in solid form.
B. They are soluble in nonpolar solvents.
C. They have high melting and boiling points.
D. They form directional bonds.
Which of the following species is paramagnetic?
N₂
B. NO
C. CO
D. O₂²⁻
Which reagent is commonly used to test for the presence of sulfate ions?
AgNO₃
B. BaCl₂
C. NaOH
D. HCl
The oxidation state of nitrogen in NH₄Cl is:
-3
B. +1
C. +3
D. 0
Which of the following molecules is nonpolar?
NH₃
B. H₂O
C. CO₂
D. SO₂
Which of the following represents the Aufbau principle?
Electrons are added to orbitals in order of increasing energy.
B. No two electrons in an atom can have the same set of quantum numbers.
C. Electrons occupy degenerate orbitals singly before pairing.
D. None of the above.
Which of the following has the smallest atomic radius?
Na
B. Mg
C. Al
D. Si
Which of the following is the most reactive halogen?
Fluorine
B. Chlorine
C. Bromine
D. Iodine
What is the geometry of the PCl₅ molecule in the gas phase?
Octahedral
B. Square planar
C. Trigonal bipyramidal
D. Tetrahedral
The oxidation number of phosphorus in H₃PO₄ is:
+3
B. +5
C. -3
D. +4
Which of the following species has sp hybridization?
CO₂
B. CH₄
C. BF₃
D. H₂O
The color of the complex [Cu(H₂O)₆]²⁺ is:
Yellow
B. Blue
C. Green
D. Red
Which of the following is NOT a noble gas?
Argon
B. Neon
C. Radon
D. Hydrogen
Which property decreases across a period from left to right?
Ionization energy
B. Electronegativity
C. Atomic radius
D. Nuclear charge
The bond angle in ammonia (NH₃) is approximately:
109.5°
B. 104.5°
C. 107°
D. 120°
What is the primary role of ligands in a coordination complex?
They provide the central metal ion.
B. They donate electron pairs to the central metal ion.
C. They determine the oxidation state of the central atom.
D. They stabilize the metal ion through ionic bonds.
The catalyst in the Haber process for ammonia synthesis is:
Iron
B. Nickel
C. Platinum
D. Copper
The oxidation state of sulfur in SO₄²⁻ is:
-2
B. +2
C. +6
D. +4
Which of the following is an application of bioinorganic chemistry?
Photosynthesis
B. Catalytic converters
C. Nanotechnology
D. Polymerization
Which of the following is a weak acid?
HCl
B. H₂SO₄
C. HF
D. HNO₃
Which compound is used as a desiccant to absorb water?
NaCl
B. CaCl₂
C. KCl
D. MgCl₂
The oxidation state of oxygen in H₂O₂ is:
0
B. +1
C. -2
D. -1
What is the hybridization of the central atom in SF₆?
sp³
B. sp²
C. sp³d²
D. sp³d
Which element is essential for the formation of hemoglobin?
Copper
B. Zinc
C. Iron
D. Magnesium
The geometry of [Ni(CO)₄] is:
Square planar
B. Tetrahedral
C. Linear
D. Trigonal planar
Which of the following is the hardest transition metal?
Tungsten
B. Iron
C. Chromium
D. Titanium
Which of the following oxides is amphoteric?
Na₂O
B. Al₂O₃
C. SO₂
D. MgO
Which type of magnetism is exhibited by [Mn(H₂O)₆]²⁺?
Diamagnetism
B. Paramagnetism
C. Ferromagnetism
D. Antiferromagnetism
Which of the following is the most electronegative element?
Oxygen
B. Fluorine
C. Nitrogen
D. Chlorine
The stability of alkali metal halides decreases as:
The size of the halide ion increases.
B. The size of the halide ion decreases.
C. The charge density of the halide ion decreases.
D. None of the above.
Which gas is released during the thermal decomposition of KClO₃?
Oxygen
B. Nitrogen
C. Chlorine
D. Hydrogen
Which of the following is NOT a characteristic of ionic compounds?
High melting points
B. Good electrical conductivity in molten state
C. Solubility in polar solvents
D. Malleability
Which of the following is a non-stoichiometric compound?
NaCl
B. FeO
C. KCl
D. CaO
What is the charge of the cobalt ion in [Co(NH₃)₆]³⁺?
+1
B. +2
C. +3
D. +4
Which of the following species is isoelectronic with O₂?
N₂
B. CO
C. NO⁺
D. F₂
Which of the following has the highest first ionization energy?
Boron
B. Carbon
C. Nitrogen
D. Oxygen
What is the molecular shape of XeF₄?
Square planar
B. Trigonal bipyramidal
C. Octahedral
D. Tetrahedral
Which of the following is the correct order of increasing bond strength?
Single bond < Double bond < Triple bond
B. Triple bond < Single bond < Double bond
C. Double bond < Triple bond < Single bond
D. Single bond < Triple bond < Double bond
Which of the following ions has a d⁵ electronic configuration?
Mn²⁺
B. Fe²⁺
C. Cr²⁺
D. Ni²⁺
The crystal field splitting in an octahedral field is denoted by:
Δt
B. Δo
C. Δsp
D. Δcf
Which of the following is NOT a property of transition metals?
High melting points
B. Variable oxidation states
C. Poor conductivity
D. Formation of colored compounds
The compound K₂Cr₂O₇ is commonly used as:
A reducing agent
B. An oxidizing agent
C. A desiccant
D. A catalyst
The effective nuclear charge experienced by outer electrons increases across a period because:
Shielding decreases.
B. The number of protons increases.
C. The size of the atom increases.
D. Both A and B.
Which of the following is a diamagnetic ion?
Fe²⁺
B. Cu²⁺
C. Zn²⁺
D. Mn²⁺
The Haber process is used to produce:
Ammonia
B. Methane
C. Hydrogen
D. Oxygen
What is the coordination number of the central metal in [Co(NH₃)₄Cl₂]⁺?
4
B. 5
C. 6
D. 7
Which of the following molecules is polar?
BF₃
B. CO₂
C. H₂O
D. BeCl₂
What type of hybridization occurs in the central atom of SF₄?
sp³
B. sp³d
C. sp²
D. sp³d²
The splitting of d-orbitals in a tetrahedral crystal field is:
Greater than in octahedral fields.
B. Equal to that in octahedral fields.
C. Less than in octahedral fields.
D. None of the above.
Which of the following has the highest lattice energy?
NaCl
B. MgO
C. CsCl
D. KBr
The oxidation state of cobalt in [Co(CN)₆]³⁻ is:
+1
B. +2
C. +3
D. +4
Which of the following is a neutral ligand?
Cl⁻
B. OH⁻
C. NH₃
D. CN⁻
What is the hybridization of the central atom in CO₂?
sp
B. sp²
C. sp³
D. sp³d
The term “chelate” refers to:
A compound containing multiple central metal ions.
B. A ligand that forms multiple bonds to a single metal ion.
C. A metal ion surrounded by ionic bonds.
D. A reaction involving a metal and a gas.
Which of the following exhibits metallic bonding?
NaCl
B. H₂O
C. Cu
D. CO₂
The oxidation number of Mn in KMnO₄ is:
+5
B. +7
C. +6
D. +4
Which of the following molecules has a bond angle of 180°?
H₂O
B. CO₂
C. NH₃
D. CH₄
The periodic law states that:
Properties of elements are a periodic function of their atomic mass.
B. Properties of elements are a periodic function of their atomic number.
C. Elements with similar properties are grouped together.
D. All elements have isotopes.
Which of the following is a d-block element?
Magnesium
B. Iron
C. Sulfur
D. Boron
What is the primary function of a ligand in a complex ion?
To donate protons.
B. To donate electron pairs.
C. To increase the size of the complex.
D. To reduce the oxidation state of the metal ion.
The property of being ferromagnetic is exhibited by:
Zinc
B. Copper
C. Nickel
D. Sodium
Which of the following halogens is the most electronegative?
Chlorine
B. Fluorine
C. Bromine
D. Iodine
The energy gap between t₂g and eg orbitals in an octahedral crystal field is called:
Crystal field stabilization energy (CFSE).
B. Ligand field splitting energy (LFSE).
C. Δo.
D. All of the above.
Which of the following compounds is ionic?
CO₂
B. HCl
C. NaCl
D. CH₄
The correct order of increasing metallic character is:
F < O < N
B. O < F < N
C. N < F < O
D. F < N < O
What is the oxidation state of sulfur in H₂SO₄?
+4
B. +6
C. -2
D. +2
Which type of hybridization is present in the NH₃ molecule?
sp
B. sp²
C. sp³
D. sp³d
The magnetic moment of a transition metal complex can be used to determine:
Its charge.
B. The number of unpaired electrons.
C. Its oxidation state.
D. The ligand field strength.
Which of the following is a weak field ligand?
CN⁻
B. CO
C. H₂O
D. NH₃
The geometry of [Ni(CN)₄]²⁻ is:
Tetrahedral
B. Square planar
C. Trigonal planar
D. Octahedral
The bond order of O₂ is:
1
B. 2
C. 3
D. 1.5
The lanthanide contraction is caused by:
Poor shielding by f-electrons.
B. Increase in effective nuclear charge.
C. Decrease in atomic size.
D. Both A and B.
What is the color of Fe²⁺ ion in aqueous solution?
Pale green
B. Blue
C. Yellow
D. Colorless
Which of the following is NOT a characteristic of ionic compounds?
High melting points
B. Conductivity in molten state
C. High solubility in nonpolar solvents
D. Hard and brittle nature
Which molecule does NOT follow the octet rule?
BF₃
B. CO₂
C. NH₃
D. CH₄
In the solid state, NaCl forms a:
Simple cubic structure
B. Face-centered cubic structure
C. Body-centered cubic structure
D. Hexagonal structure
Which of the following metals is extracted by the Hall-Héroult process?
Iron
B. Aluminium
C. Copper
D. Zinc
Which compound contains a coordinate covalent bond?
NaCl
B. NH₄⁺
C. CH₄
D. H₂O
Which of the following has the smallest atomic radius?
Li
B. Be
C. B
D. C
Which statement is true for paramagnetic substances?
They have no unpaired electrons.
B. They are repelled by a magnetic field.
C. They have unpaired electrons.
D. They are diamagnetic in nature.
The stability of an oxidation state increases:
With the decrease in ionization energy.
B. With the increase in effective nuclear charge.
C. With the decrease in shielding effect.
D. Both B and C.
Which of the following molecules has sp² hybridization?
CH₄
B. C₂H₄
C. C₂H₂
D. NH₃
The reaction of a metal with dilute acid produces:
Oxygen
B. Hydrogen
C. Chlorine
D. Carbon dioxide
Which of the following is a monodentate ligand?
EDTA
B. H₂O
C. C₂O₄²⁻
D. en
What is the coordination number of the central metal in [Fe(C₂O₄)₃]³⁻?
3
B. 6
C. 4
D. 2
Which of the following is an alloy?
Brass
B. Diamond
C. Graphite
D. Quartz
Which element is a metalloid?
Sodium
B. Silicon
C. Aluminum
D. Bromine
The radius of a cation is always:
Smaller than its parent atom.
B. Larger than its parent atom.
C. Equal to its parent atom.
D. Dependent on its charge only.
Which of the following is NOT a property of alkali metals?
High ionization energy
B. High reactivity
C. Low melting points
D. Formation of basic oxides
Which element is the most reactive halogen?
Fluorine
B. Chlorine
C. Bromine
D. Iodine
The shape of [BF₄]⁻ is:
Trigonal planar
B. Tetrahedral
C. Linear
D. Square planar
Which of the following species is amphoteric?
Al₂O₃
B. Na₂O
C. SO₂
D. CaO
What type of isomerism is shown by [Co(NH₃)₅Br]SO₄ and [Co(NH₃)₅SO₄]Br?
Structural isomerism
B. Ionization isomerism
C. Linkage isomerism
D. Coordination isomerism
Which of the following molecules has a dipole moment?
CO₂
B. CCl₄
C. H₂O
D. BeCl₂
Which of the following exhibits hydrogen bonding?
CH₄
B. NH₃
C. C₂H₂
D. CO
The most abundant element in the Earth’s crust is:
Silicon
B. Oxygen
C. Aluminum
D. Iron
Which of the following has a d²sp³ hybridization?
[Fe(CN)₆]³⁻
B. [Co(NH₃)₆]³⁺
C. [Ni(CN)₄]²⁻
D. [Cu(NH₃)₄]²⁺
The molecule XeF₂ has a shape that can be described as:
Linear
B. Trigonal planar
C. Tetrahedral
D. Bent
The compound NaCl is best described as:
Covalent
B. Metallic
C. Ionic
D. Hydrogen-bonded
Which of the following species is isoelectronic with Ne?
O²⁻
B. F⁻
C. Na⁺
D. All of the above
The bond angle in a perfect tetrahedral molecule is:
90°
B. 109.5°
C. 120°
D. 180°
Which of the following has the highest electronegativity?
F
B. Cl
C. Br
D. I
The principal quantum number (n) primarily determines:
The shape of an orbital.
B. The size and energy of an orbital.
C. The orientation of an orbital.
D. The spin of an electron.
Which of the following is a Lewis base?
NH₃
B. BF₃
C. H⁺
D. Fe³⁺
The color of a transition metal complex arises due to:
Charge transfer.
B. d-d electronic transitions.
C. Lattice vibrations.
D. Both A and B.
Which of the following is a radioactive element?
Uranium
B. Calcium
C. Carbon
D. Silicon
The number of unpaired electrons in a high-spin Fe³⁺ ion is:
1
B. 3
C. 5
D. 0
Which gas is released when limestone (CaCO₃) is heated?
CO
B. CO₂
C. O₂
D. N₂
The process used to extract metals from their ores by chemical reduction is called:
Roasting
B. Calcination
C. Smelting
D. Electrolysis
The shape of the PF₅ molecule is:
Tetrahedral
B. Trigonal bipyramidal
C. Octahedral
D. Square planar
Which of the following is an example of a basic oxide?
SO₂
B. CO₂
C. Na₂O
D. SiO₂
Which of the following has a zero dipole moment?
NH₃
B. H₂O
C. BF₃
D. CHCl₃
What type of bond is present in the N₂ molecule?
Single bond
B. Double bond
C. Triple bond
D. Ionic bond
Which of the following is a d-block element?
Sodium
B. Magnesium
C. Copper
D. Aluminum
The basicity of a ligand is determined by its:
Electron withdrawing ability.
B. Electron donating ability.
C. Steric hindrance.
D. Coordination number.
The most common oxidation state of lanthanides is:
+1
B. +2
C. +3
D. +4
Which of the following acids is strongest?
HF
B. HCl
C. HBr
D. HI
The molecule SF₆ has which type of geometry?
Square planar
B. Octahedral
C. Tetrahedral
D. Trigonal planar
Which compound is used as an antifreeze in car engines?
Ethylene glycol
B. Glycerol
C. Methanol
D. Propanol
Which of the following complexes is chiral?
[Co(en)₃]³⁺
B. [Ni(H₂O)₆]²⁺
C. [Zn(NH₃)₄]²⁺
D. [Fe(CN)₆]³⁻
The major ore of aluminum is:
Hematite
B. Bauxite
C. Galena
D. Cinnabar
Which of the following species is diamagnetic?
O₂
B. NO
C. N₂
D. C₂
The stability of a complex depends on:
Nature of the metal ion.
B. Nature of the ligand.
C. Chelation effect.
D. All of the above.
Which of the following is a pseudohalogen?
Cl₂
B. CN⁻
C. F₂
D. Br₂
The flame test color for potassium is:
Yellow
B. Violet
C. Red
D. Green
The most stable oxidation state of manganese is:
+2
B. +3
C. +4
D. +7
Which of the following compounds is an interhalogen compound?
ClF₃
B. HCl
C. HF
D. Br₂
The common oxidation state of alkali metals is:
+1
B. +2
C. +3
D. +4
The bond order of O₂ molecule is:
1
B. 2
C. 2.5
D. 3
The IUPAC name of [Co(NH₃)₅Cl]Cl₂ is:
Pentamminechlorocobalt(III) chloride
B. Pentachlorocobalt(III) ammine
C. Chloropentaamminecobalt(III) chloride
D. Chloropentamminecobalt(II) chloride
The lattice energy of an ionic compound increases with:
Increase in ionic radius
B. Decrease in ionic radius
C. Increase in covalent character
D. None of the above
The geometry of [Ni(CN)₄]²⁻ is:
Tetrahedral
B. Square planar
C. Octahedral
D. Trigonal bipyramidal
The most abundant noble gas in the Earth’s atmosphere is:
Helium
B. Neon
C. Argon
D. Krypton
Which of the following ligands is a bidentate ligand?
NH₃
B. Cl⁻
C. C₂O₄²⁻
D. CN⁻
Which of the following is an example of a polar molecule?
CO₂
B. CH₄
C. NH₃
D. BF₃
The effective nuclear charge experienced by the outermost electrons increases:
Down a group
B. Across a period
C. With increasing atomic radius
D. With increasing number of shells
The element with the highest ionization energy in the periodic table is:
Fluorine
B. Helium
C. Neon
D. Oxygen
The color of Cu²⁺ ions in aqueous solution is:
Green
B. Blue
C. Yellow
D. Pink
Which of the following is an organometallic compound?
FeCl₃
B. [Co(NH₃)₆]³⁺
C. (CH₃)₄Sn
D. Na₂[Fe(CN)₆]
The hybridization of the central atom in SF₄ is:
sp³
B. sp²
C. sp³d
D. sp³d²
Which of the following is a paramagnetic species?
H₂
B. O₂
C. N₂
D. F₂
The oxidation state of chromium in K₂Cr₂O₇ is:
+3
B. +4
C. +5
D. +6
The name of the compound PCl₅ is:
Phosphorus pentachloride
B. Pentachlorophosphide
C. Phosphorus chloride
D. Pentachlorophosphorus
Which of the following elements is a d-block element?
Sodium
B. Titanium
C. Aluminum
D. Sulfur
Which of the following species has a tetrahedral geometry?
SF₆
B. NH₃
C. CH₄
D. XeF₄
Which element is present in hemoglobin?
Zinc
B. Copper
C. Iron
D. Manganese
Which of the following has the smallest atomic radius?
Na
B. K
C. Rb
D. Cs
The type of hybridization in PCl₃ is:
sp³
B. sp²
C. sp³d
D. sp
Which compound is used in the manufacture of fertilizers?
NH₃
B. H₂SO₄
C. HNO₃
D. All of the above
Which of the following is a property of metals?
High electrical conductivity
B. Brittle nature
C. Low density
D. Non-malleable
Which of the following pairs are isotopes?
¹H and ²H
B. ¹²C and ¹³C
C. ³⁵Cl and ³⁷Cl
D. All of the above
The type of magnetism shown by [Fe(CN)₆]³⁻ is:
Paramagnetism
B. Diamagnetism
C. Ferromagnetism
D. Antiferromagnetism
Which of the following is a good oxidizing agent?
KMnO₄
B. HCl
C. NaOH
D. CCl₄
The number of valence electrons in sulfur is:
2
B. 4
C. 6
D. 8
The gas responsible for the greenhouse effect is:
CO₂
B. O₂
C. H₂
D. HeInorganic Chemistry for Students