Atomic Structure and Bonding

Vocabulary flashcards covering atomic structure, subatomic particles, quantum numbers, periodic values, primary bonds, and secondary bonds based on Lecture 02.

Atom

The basic unit of an element.

Nucleus Diameter

The diameter of an atom's nucleus, equal to $10^{-14}\,\text{m}$.

Electron

A subatomic particle with a negative charge and a mass of $9.109 \times 10^{-28}\,\text{g}$, located in the electron cloud surrounding the nucleus.

Proton

A subatomic particle located in the nucleus with a positive charge and a mass of $1.673 \times 10^{-24}\,\text{g}$.

Neutron

A subatomic particle located in the nucleus with a neutral charge and a mass of $1.675 \times 10^{-24}\,\text{g}$.

Bohr Atomic Model

An atomic model depicting orbital electrons circulating around a central nucleus in designated shells or orbits.

Principal Quantum Number ($n$)

A quantum number representing main energy levels ranging from $1$ to $7$, where a larger $n$ indicates higher energy, and the maximum number of electrons per shell is calculated as $2n^2$.

Valence Shell

The outermost electron shell or orbit of an atom.

Atomic Number

The number of protons present in the nucleus of an atom.

Atomic Mass

The total number of protons and neutrons in an atom.

Primary Bonding

Strong atomic bonding mechanisms that hold atoms together, consisting of ionic, covalent, and metallic bonds.

Ionic Bond

A strong atomic bond formed by the transfer of electrons between positive and negative ions, requiring a large difference in electronegativity.

Covalent Bond

A strong primary bond involving a large interactive force produced by the sharing of electrons between atoms.

Metallic Bond

A non-directional primary bond formed in metals where closely packed atoms share loosely bound valence electrons, creating an electron cloud.

Secondary Bonding

Weak physical bonds (such as van der Waals forces) formed when an uneven charge distribution creates dipoles within or between atoms or molecules.

Dipole

A pair of equal and opposite electric charges created by an uneven charge distribution or random fluctuation of electrons around an atom or molecule.

Hydrogen Bonding

The strongest form of secondary bonding, occurring when hydrogen attached directly to an electronegative element acquires a significant positive charge and attracts the negative end of another molecule.