Match with the correct definition.

A.

Each electron state can hold no more than two electrons, which must have opposite spins.

B.

Electron sharing between two adjacent atoms such that each atom assumes a stable electron configuration.

C.

Electrostatic attraction between oppositely charged ions.

D.

The positively charged ion cores are shielded from one another, and also "glued" together by the sea of valence electrons.

Ionic bonding: A, B, C, or D?

Covalent Bonding: A, B, C or, D?

Metallic bonding: A, B, C, or D?

Pauli exclusion principle: A, B C, or D?

Ionic bonding: C

Covalent bonding: B

Metallic bonding: D

Pauli exclusion principle: A

Explanation:

All the electrons in 1 atom are characterized by a series of 4 numbers, known as quantum numbers. These numbers (n, l, ml, ms) describe the state of each electron (in which level, sublevel, orbital it is and its spin). For 2 electrons to coexist in the same atom they must differ in at least of these numbers. If they occupy the same level, sublevel and orbital, then they must have different (and opposite) spins. This is known as Pauli exclusion principle.

Also, to gain stability atoms can gain, lose or share electrons. In doing so they form bonds. There are 3 kinds of bonds:

Ionic bonding: these are formed between metals and nonmetals. Metals tend to lose electrons and form cations (positive ions) and nonmetals tend to gain electrons and form anions (negative ions). Cations and anions attract each other due to electrostatic forces between oppositely charged ions. Covalent bonding: these are formed between nonmetals, which share pairs of electrons so as to reach the electron configuration of the closest noble gas (the most stable electron configuration). Metallic bonding: valence electrons are loose in metals, so they move together as a "sea of electrons", acting as "glue" of the remaining positive cores (electrons that are negative charges serve to attract the positive charges of the cores).