Atomic Structure and Chemical Bonds Quiz

Electron orbitals have a maximum capacity of 2 electrons each, and there are 3 2p orbitals, hence 2*3 = 6, but Pauli exclusion principle restricts it to 2 electrons per orbital, so 2p orbital can have 6/3 = 2 electrons

Protons possess a positive charge and are found in the nucleus of an atom.

Niels Bohr proposed the Bohr model, suggesting electrons orbit the nucleus in fixed paths or energy levels.

Oxygen has 6 valence electrons, occupying the 2s and 2p orbitals.

Neutrons have a mass approximately equal to 1 atomic mass unit and are found in the nucleus of an atom.

An orbital is a region around the nucleus where electrons are most likely to be found.

Carbon has 6 electrons, distributed as 1s² 2s² 2p², following the Aufbau principle.

Covalent bonds are formed by the sharing of electrons between atoms, creating a stable electron configuration for both.

Water has a bent molecular shape due to its two lone pairs of electrons on the oxygen atom.

Hydrogen bonds are formed between the partial positive hydrogen atom of one molecule and the partial negative oxygen atom of another.

Fluorine has the highest electronegativity among all elements.

The bond angle in methane (CH₄) is approximately 109.5° due to the tetrahedral geometry of its molecular structure.

Ionization energy is the energy required to remove an electron from an atom, typically from the outermost shell.

Electrovalency refers to the process of an atom gaining or losing electrons to become an ion.

Ionic bonds are formed between ions with opposite charges through electrostatic attraction.

Covalent bonds are formed by the sharing of electron pairs between atoms.

A dipole moment occurs when there is an uneven distribution of electron density in a molecule, leading to a partial positive and partial negative charge.