Molecular Structure

Question 1

Front: What are the main components of an atom?

Answer 1

Back: An atom consists of a nucleus containing protons and neutrons, surrounded by electrons distributed in orbitals.

Question 2

Front: Where are electrons located in an atom?

Answer 2

Back: Electrons are distributed in orbitals around the nucleus in energy levels or shells.

Question 3

Front: How does electron distribution contribute to bond formation?

Answer 3

Back: Bonds form when atoms share, gain, or lose electrons to achieve a stable electron configuration, often a full outer shell.

Question 4

Front: What are the two main types of bonds based on electron distribution?

Answer 4

Back: Covalent bonds (shared electrons) and ionic bonds (transfer of electrons).

Question 5

Front: Why is electron distribution important for molecular shape?

Answer 5

Back: The repulsion between electron pairs around an atom determines the 3D shape of a molecule.

Question 6

Front: What is the VSEPR theory?

Answer 6

Back: Valence Shell Electron Pair Repulsion (VSEPR) theory predicts molecular shapes based on minimising electron pair repulsion.

Question 7

Front: How do lone pairs of electrons affect molecular shape?

Answer 7

Back: Lone pairs take up more space than bonding pairs, causing bond angles to adjust and altering the molecule’s shape.

Question 8

Front: How is the 3D shape of a molecule described?

Answer 8

Back: The 3D shape is described using geometric terms like linear, trigonal planar, tetrahedral, trigonal bipyramidal, or octahedral.

Question 9

Front: How is the 3D shape of a molecule represented?

Answer 9

Back: It is represented using models like ball-and-stick, space-filling, or wedge-and-dash diagrams to show spatial arrangement.

Question 10

Front: What is hybridisation in chemistry?

Answer 10

Back: Hybridisation is the mixing of atomic orbitals to form new hybrid orbitals that are equivalent in energy and shape, enabling bond formation.

Question 11

Front: Why is hybridisation important in bonding?

Answer 11

Back: Hybridisation allows atoms to form stronger, more stable bonds by creating orbitals that align correctly in 3D space for overlap.

Question 12

Front: What are the common types of hybridisation?

Answer 12

Back: The common types are sp (linear), sp² (trigonal planar), sp³ (tetrahedral), sp³d (trigonal bipyramidal), and sp³d² (octahedral)

Question 13

Front: How does hybridisation affect molecular shape?

Answer 13

Back: The type of hybridisation determines the geometry of the molecule by defining the angles between bonds

Question 14

Front: What is an example of sp hybridisation?

Answer 14

Back: sp hybridisation occurs in molecules like ethyne (C≡C), where carbon forms two sigma bonds in a linear geometry.

Question 15

Front: What is an example of sp² hybridisation?

Answer 15

Back: sp² hybridisation occurs in molecules like ethene (C=C), where carbon forms three sigma bonds in a trigonal planar geometry.

Question 16

Front: What is an example of sp³ hybridisation?

Answer 16

Back: sp³ hybridisation occurs in molecules like methane (CH₄), where carbon forms four sigma bonds in a tetrahedral geometry

Question 17

Front: How does hybridisation relate to lone pairs?

Answer 17

Back: Lone pairs occupy hybrid orbitals just like bonding pairs, influencing bond angles and molecular geometry.

Question 18

Front: How do hybrid orbitals align with electron distribution?

Answer 18

Back: Hybrid orbitals maximise overlap by aligning in 3D space, ensuring the most stable electron distribution for bonding.