Exploring the Structure of Atoms

Who proposed the first atomic theory in the early 1800s?

What is the main idea of Dalton's atomic theory?

• All matter is composed of a single type of atom that varies in size.

• Matter is composed of indivisible atoms that combine in fixed ratios.

• Atoms are the smallest units of matter and cannot combine with each other.

• Matter is made up of molecules that can be divided indefinitely.

Which scientist is known for the discovery of the electron?

• J.J. Thomson

• Niels Bohr

• Isaac Newton

• Albert Einstein

What model of the atom did J.J. Thomson propose?

• Plum pudding model

• Quantum mechanical model

• Nuclear model

• Solid sphere model

What is the significance of the quantum mechanical model of the atom?

• It provides a more accurate understanding of atomic structure and electron behavior, incorporating wave-particle duality and uncertainty principles.

• It describes the fixed orbits of electrons around the nucleus.

• It suggests that atoms are indivisible and cannot be split.

• It eliminates the need for quantum mechanics in atomic theory.

How many electrons can the first shell of an atom hold?

• 10

• 1

• 2

• 8

What is the electron configuration for carbon?

• 1s² 2s² 2p²

• 1s² 2s² 2p³

• 1s² 2s² 2p¹

• 1s² 2s² 2p⁴

What is the principle that states electrons occupy the lowest energy orbitals first?

• Aufbau principle

• Hund's rule

• Quantum mechanical model

• Pauli exclusion principle

How does the Pauli exclusion principle apply to electron configuration?

• The Pauli exclusion principle allows for multiple electrons in the same quantum state.

• Electrons are arranged randomly in orbitals without any restrictions.

• The Pauli exclusion principle requires that no two electrons in an atom can have the same set of quantum numbers, influencing how electrons are arranged in orbitals.

• Electrons can occupy the same orbital if they have different energies.

What is the electron configuration for a sodium ion (Na+)?

• 1s² 2s² 2p⁶ 3p⁶

• 1s² 2s² 2p⁶ 3s¹

• 1s² 2s² 2p⁶

• 1s² 2s² 2p⁵