Atomic Structure and Bonding Quiz - ICSE Class 9 Chemistry

Free practice quiz: Atomic Structure and Bonding (ICSE Class 9 Chemistry). 50 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This ICSE Class 9 Chemistry practice quiz has 50 multiple-choice questions on Atomic Structure and Bonding, and 50 of them come with an explanation. Try the 5 sample questions below (tap an option to check yourself), then play the full quiz online. No sign-up needed.

Sample questions

1. Which of the following quantum numbers describes the orientation of an atomic orbital in space?

   1. Principal quantum number (n)
   2. Azimuthal quantum number (l)
   3. Magnetic quantum number (ml)
   4. Spin quantum number (ms)
   Show answer

   Answer: C. Magnetic quantum number (ml)

   The principal quantum number (n) determines the energy level and size of an atomic orbital. The azimuthal quantum number (l) determines the shape of an atomic orbital. The magnetic quantum number (ml) determines the orientation of an atomic orbital in space. The spin quantum number (ms) describes the intrinsic angular momentum of an electron.

2. Which element has the electronic configuration 1s²2s²2p⁶3s¹?

   1. Sodium (Na)
   2. Magnesium (Mg)
   3. Aluminum (Al)
   4. Silicon (Si)
   Show answer

   Answer: A. Sodium (Na)

   The atomic number of Sodium (Na) is 11. Its electronic configuration is 1s²2s²2p⁶3s¹. Magnesium (Mg) has atomic number 12 (1s²2s²2p⁶3s²). Aluminum (Al) has atomic number 13 (1s²2s²2p⁶3s²3p¹). Silicon (Si) has atomic number 14 (1s²2s²2p⁶3s²3p²).

3. Which of the following elements is diamagnetic?

   1. Oxygen (O₂)
   2. Nitrogen (N₂)
   3. Neon (Ne)
   4. Sulfur (S)
   Show answer

   Answer: C. Neon (Ne)

   Diamagnetic substances are weakly repelled by an external magnetic field. This occurs when all electrons in the atom or molecule are paired. Oxygen (O₂) has unpaired electrons and is paramagnetic. Nitrogen (N₂) has all paired electrons in its molecular orbital diagram. Neon (Ne) has a full electron shell with all paired electrons. Sulfur (S) in its elemental form has unpaired electrons. Therefore, Neon is diamagnetic.

4. Which type of bond is responsible for holding the atoms together in a diatomic molecule of oxygen (O₂)?

   1. Ionic bond
   2. Single covalent bond
   3. Double covalent bond
   4. Triple covalent bond
   Show answer

   Answer: C. Double covalent bond

   Oxygen atoms achieve a stable octet by sharing two pairs of electrons, forming a double covalent bond (O=O) in the O₂ molecule.

5. Which of the following has the largest atomic radius?

   1. Fluorine (F)
   2. Chlorine (Cl)
   3. Bromine (Br)
   4. Iodine (I)
   Show answer

   Answer: D. Iodine (I)

   Atomic radius generally increases as you move down a group. Fluorine, Chlorine, Bromine, and Iodine are all in Group 17 (halogens). As you move down the group, the number of electron shells increases, and the valence electrons are further from the nucleus, leading to a larger atomic radius. Thus, Iodine has the largest atomic radius.

More questions in this quiz

Answers and explanations are in the full quiz.

1. According to Hund's rule, which configuration is the most stable for a p-orbital with three electrons?
2. The Aufbau principle states that electrons fill atomic orbitals in order of:
3. What is the maximum number of electrons that can occupy an 'f' subshell?
4. Which type of covalent bond involves the sharing of three pairs of electrons between two atoms?
5. Ionic bonds are typically formed between:
6. What is the characteristic property of a metallic bond that allows metals to conduct electricity?
7. The Pauli Exclusion Principle states that no two electrons in an atom can have the same set of:
8. Which of the following is NOT a characteristic of hydrogen bonding?
9. What is the atomic number of an element with the electronic configuration 1s²2s²2p⁶3s²3p⁴?
10. The chemical formula of magnesium oxide is MgO. This indicates that magnesium forms:
11. What is the approximate atomic mass of an atom if it has 12 protons and 13 neutrons in its nucleus?
12. An isotope of carbon has 6 protons and 8 neutrons. What is its mass number?
13. Which of the following statements about the Bohr model of the atom is INCORRECT?
14. The element with atomic number 17 is Chlorine. Its electronic configuration is 2, 8, 7. How many valence electrons does Chlorine have?
15. Which of the following is a polar covalent bond?
16. What is the shape of a molecule with two electron domains around the central atom, both of which are bonding pairs?
17. If an atom has 10 protons and 10 electrons, it is:
18. What is the fundamental difference between an atom and an ion?
19. The bond length generally decreases as:
20. Which of the following is an example of a polar molecule?
21. The 'electron sea' model is used to explain the bonding in:
22. What is the ground state electronic configuration of a neutral sodium atom (Na, atomic number 11)?
23. In the formation of a sodium chloride (NaCl) compound, what type of chemical bond is formed?
24. Which of the following sets of quantum numbers is NOT allowed for an electron in an atom?
25. Which of the following elements is expected to have the highest electronegativity?
26. The number of electrons in the outermost shell of an atom of element X is 6. What is the likely group number of element X in the periodic table?
27. What is the molecular geometry of methane (CH₄)?
28. The Aufbau principle, Pauli Exclusion Principle, and Hund's rule are collectively known as:
29. An atom has 12 protons, 12 neutrons, and 10 electrons. What is its net charge?
30. Which of the following describes an atom's atomic number?
31. What type of bonding leads to the formation of a crystal lattice with high melting and boiling points, typically observed in compounds like sodium chloride?
32. Which subshell can hold a maximum of 10 electrons?
33. The magnetic quantum number (ml) for a p-orbital can have values of:
34. Which statement best describes the metallic bond?
35. If an atom loses one electron, it becomes:
36. The element with electron configuration 1s²2s²2p⁶3s²3p² belongs to which block of the periodic table?
37. What is the correct order of filling the orbitals according to the Aufbau principle?
38. Which of the following is a characteristic of a nonpolar covalent bond?
39. What is the number of unpaired electrons in a nitrogen atom (atomic number 7) in its ground state?
40. The attraction between oppositely charged ions in an ionic compound is called:
41. What is the electronic configuration of a sodium ion (Na⁺)?
42. Which factor, when it increases, generally leads to a decrease in atomic radius?
43. Which of the following is a property of substances with strong metallic bonds?
44. According to the Bohr model, an electron in an atom:
45. What is the total number of electrons in an atom with 15 protons and a mass number of 31?

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