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Quizzes > Science

Inorganic Chemistry Quiz: Inorganic Test to Check Your Knowledge

Quick, free inorganic chemistry quiz to test your knowledge. Instant results.

Editorial: Review CompletedCreated By: Chloe UpdikeUpdated Aug 25, 2025
Difficulty: Moderate
Questions: 20
Learning OutcomesStudy Material
Colorful paper art depicting elements for an Inorganic Chemistry Knowledge Test quiz

Use this inorganic chemistry quiz to check your understanding of bonding, periodic trends, and salts. Answer 15 quick questions and get instant results with brief tips. Want more practice? Try a coordination chemistry quiz, build basics with a general chemistry quiz, or take a fast chemistry practice test before your next class.

What is the coordination number of the cobalt ion in the complex [Co(NH3)6]3+?
4
6
12
8
In [Co(NH3)6]3+ the cobalt ion is surrounded by six ammonia ligands, giving it a coordination number of 6. Coordination number refers to the number of ligand donor atoms directly bonded to the metal center.
What is the oxidation state of manganese in the permanganate ion (MnO4âˆ')?
+6
+2
+7
+4
In MnO4âˆ' each oxide has a âˆ'2 charge (total âˆ'8) and the overall charge is âˆ'1, so manganese must be +7 to balance the total charge. Oxidation state calculations sum all contributions to match the ion's net charge.
Which of the following best describes the trend of atomic radius on moving down a group in the periodic table?
Atomic radius remains constant
Atomic radius decreases down a group
Atomic radius first decreases then increases
Atomic radius increases down a group
As you move down a group, additional electron shells are added, increasing the distance of the outer electrons from the nucleus and thereby increasing atomic radius. This is a fundamental periodic trend.
The crystal structure of sodium chloride is an example of which type of lattice arrangement?
Simple cubic
Face-centered cubic
Hexagonal close-packed
Body-centered cubic
NaCl adopts the rock-salt structure, which is a face-centered cubic arrangement of both Na+ and Clâˆ' ions. Each ion is surrounded by six counter-ions in an octahedral geometry.
Which oxide exhibits amphoteric behavior by reacting with both acids and bases?
K2O
Al2O3
SO3
SiO2
Al2O3 reacts with acids to form Al3+ salts and with bases to form aluminate complexes, demonstrating amphoteric behavior. Amphoteric oxides can act as either an acid or a base.
According to the spectrochemical series, which ligand produces the largest crystal field splitting in an octahedral complex?
NH3
Fâˆ'
Clâˆ'
CNâˆ'
CNâˆ' is a strong-field ligand capable of strong σ-donation and Ï€-backbonding, which produces the largest crystal field splitting (Δo) in octahedral complexes. Weaker ligands like Clâˆ' and Fâˆ' produce smaller splittings.
What is the oxidation state of iron in the complex ion [Fe(CN)6]3âˆ'?
+3
+4
+1
+2
Each CNâˆ' ligand has a âˆ'1 charge, giving a total of âˆ'6 from ligands. The complex carries âˆ'3 overall, so iron must be +3 to satisfy +3+(âˆ'6)=âˆ'3.
Which electron configuration corresponds to the Fe2+ ion in its ground state?
[Ar] 3d5
[Ar] 3d6
[Ar] 4s2 3d4
[Ar] 4s1 3d5
The neutral Fe atom is [Ar]4s2 3d6. Upon ionization, 4s electrons are removed before 3d, leaving [Ar]3d6 for Fe2+. Electron removal order is s before d.
Which halogen is the strongest oxidizing agent in its standard diatomic form?
Cl2
Br2
F2
I2
Fluorine has the highest electronegativity and the most positive reduction potential among the halogens, making F2 the strongest oxidizing agent. It undergoes reduction very easily.
Which metal crystal structure is characterized by a coordination number of 8 and atoms at the corners and center of the cube?
Simple cubic
Body-centered cubic
Hexagonal close-packed
Face-centered cubic
In a body-centered cubic lattice, each atom has 8 nearest neighbors: one at each of the eight cube corners and one at the cube center. This gives a coordination number of 8.
Which oxide is classified as acidic due to forming an acid when dissolved in water?
CO2
Al2O3
Na2O
MgO
CO2 dissolves in water to form carbonic acid (H2CO3), which is characteristic of acidic oxides. Basic oxides form hydroxides, and amphoteric oxides can exhibit both behaviors.
Which of the following species acts as a Lewis acid?
OHâˆ'
Clâˆ'
BF3
NH3
BF3 has an empty p-orbital on boron and can accept an electron pair, defining it as a Lewis acid. The others either donate pairs or carry negative charge.
Which element has the highest electronegativity according to the Pauling scale?
F
O
Cl
N
Fluorine has the highest electronegativity value on the Pauling scale due to its small atomic radius and high effective nuclear charge, attracting electrons most strongly.
In coordination chemistry, what type of ligand is ethylenediamine (en)?
Tridentate
Bidentate
Monodentate
Bridging
Ethylenediamine has two donor nitrogen atoms that can simultaneously coordinate to a single metal center, making it a bidentate chelating ligand. It forms stable five-membered rings.
Which alkali metal is expected to be the most reactive based on periodic trends?
Li
Rb
Na
K
Reactivity in alkali metals increases down the group as ionization energy decreases, making rubidium more reactive than potassium, sodium, or lithium.
In crystal field theory for an octahedral complex, which set of d orbitals is antibonding with respect to ligand σ interactions?
Both t2g and eg
Neither set
eg
t2g
The eg orbitals (dz2 and dx2âˆ'y2) point directly toward the ligand donor atoms and experience σ-antibonding interactions, raising their energy above the t2g set.
Doping silicon with phosphorus atoms produces which type of semiconductor?
n-type
Metallic conductor
p-type
Intrinsic
Phosphorus has five valence electrons, one more than silicon, introducing extra electrons into the conduction band and creating an n-type semiconductor.
Which of the following metal complexes exhibits linkage isomerism?
[Cr(H2O)6]3+
[Co(NH3)5NO2]2+
[Fe(CN)6]4âˆ'
[Co(NH3)6]3+
The nitrite ligand (NO2âˆ') can bind through nitrogen (nitro) or oxygen (nitrito), giving distinct linkage isomers in [Co(NH3)5NO2]2+. The others have fixed coordination modes.
Fe3O4 is a mixed-valence oxide. Which oxidation states of iron are present in this compound?
Fe3+ only
Fe2+ and Fe3+
Fe2+, Fe3+, and Fe4+
Fe2+ only
Fe3O4 can be viewed as FeO·Fe2O3, containing both Fe2+ and Fe3+ in its lattice. This mixed-valence nature gives it unique magnetic properties.
Why are ionic solids typically electrical insulators in the solid state?
They have overlapping valence and conduction bands
They have too many mobile ions
They lack free electrons due to a large energy gap between valence and conduction bands
They have delocalized π-bonds
In ionic solids, electrons are localized in bonding orbitals and the valence band is fully occupied. A wide band gap separates it from the conduction band, preventing electron conduction.
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Learning Outcomes

  1. Analyse coordination compound structures and bonding principles
  2. Identify oxidation states in complex inorganic molecules
  3. Apply periodic trends to predict element reactivity
  4. Evaluate crystal lattice arrangements and solid-state properties
  5. Demonstrate acid-base behaviour of inorganic species
  6. Master electron configurations of transition metals

Cheat Sheet

  1. Understanding Structures and Bonding - Dive into the world of coordination compounds where ligands and metal ions team up to create sleek octahedral and tetrahedral shapes. You'll learn how to predict these geometries and why certain ligand "dance moves" matter for stability and color.
  2. Naming Coordination Compounds - Master the art of naming these complex squads by identifying ligands, calculating oxidation states, and following IUPAC rules. With a few simple guidelines, you'll be naming compounds like a pro in no time!
  3. Determining Oxidation States - Become a detective as you assign charges to ligands and central metals to unmask the true oxidation state hidden in a compound's overall charge. This skill is key to predicting reactivity and balancing redox reactions.
  4. Applying Periodic Trends - Use atomic size and electronegativity trends to forecast how elements team up and react in inorganic chemistry. Understanding these patterns will give you a competitive edge in predicting compound stability and reactivity.
  5. Evaluating Crystal Lattice Arrangements - Explore how ions pack into solids and discover why some materials boast high melting points and conductive superpowers. This deep dive into lattice geometry reveals the blueprint behind many everyday materials.
  6. Demonstrating Acid-Base Behavior - Watch metal ions play Lewis acid and ligands step up as Lewis bases to form coordination complexes. You'll see firsthand how these interactions drive catalysis and biochemical processes!
  7. Mastering Electron Configurations - Get the scoop on how filling d-orbitals shapes the colorful personality of transition metals and dictates their favorite oxidation states. This knowledge is your ticket to predicting magnetic properties and reaction pathways.
  8. Exploring the 18-Electron Rule - Uncover the secret rule that helps chemists predict when a transition metal complex hits a "noble gas high score" of stability. It's like giving your metal center a full electronic backpack!
  9. Investigating Crystal Field Theory - Learn how ligand arrangements tweak d-orbital energies, leading to the brilliant colors we see in many metal complexes. Crystal field theory is your backstage pass to understanding spectra and magnetic quirks.
  10. Studying Isomerism in Coordination Compounds - Dive into the intriguing world of geometric and optical isomers to see how swapping ligand positions creates totally different properties. You'll soon spot why one arrangement glows and another might remain colorless!
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