Atomic Structure: Nucleus, Protons, and Electrons

The number of protons in an atom, known as its atomic number, dictates its chemical identity.

An atom with more electrons than protons has a net negative charge and is called an anion.

Electrons fill orbitals in an orderly manner, starting with the highest energy orbitals and moving to the lowest.

Valence electrons, residing in the filled orbitals of lowest energy, primarily participate in chemical reactions.

Inert elements, like neon and argon, are chemically unreactive because their series of valence orbitals are completely filled.

A stable interaction between atoms leading to molecule formation always involves ionic bonds.

In a covalent bond, the nitrogen atom always contributes two electrons to form a pair.

A nitrogen atom, with its half-filled 2px, 2py, and 2pz orbitals, tends to form exactly two covalent bonds.

A 'lone pair' refers to two electrons in a filled nonbonding valence orbital that are directly involved in covalent bonds.

Oxygen atoms tend to form two covalent bonds due to possessing two half-filled valence orbitals.

In oxygen gas (O2), the two oxygen atoms share electrons resulting in the formation of a triple bond.

The 4s orbitals possess significantly lower energy levels than the 3d orbitals.

Ionization is the process by which a neutral atom or molecule gains or loses electrons, resulting in a net charge.

When creating an atom, the first electron added would occupy the orbital of highest energy.

The number of neutrons in an atomic nucleus dictates its chemical nature.

Atoms tends to gain or lose electrons to the extent that a particular series of valence orbitals is half full.

Carbon atoms have 6 electrons that fill the 1s and 2s orbitals and completely fill the 2px and 2py orbitals.

In the hydrogen molecule (H2), the repulsion of electrons results in formation of a bonding orbital.

In ammonia (NH3), the nitrogen atom forms a triple bond with each of the three hydrogen atoms.

The nitrogen atom, with an atomic number of 7, contains filled 1s and 3s orbitals and half-filled 2px, 2Py, and 2pz orbitals.

In water (H2O), the oxygen atom forms a double bond with each of the two hydrogen atoms.

The appearance of an electron as it moves about in its orbital is generally a straight line.

The electron cloud resides within the nucleus of the atom.

Neutrons carry a positive charge, balancing the negative charge of electrons in an atom.

Conversion of a charged atom (or molecule) to one with a neutral charge is called ionization.

The number of protons in an atom, known as its atomic number, determines its chemical nature.

Atoms with a positive or negative charge due to the gain or loss of electrons are called ions .

An atom's valence electrons, which reside in the filled orbitals of lowest energy, primarily participate in chemical reactions.

A covalent bond is formed through the transfer of electrons from one atom to another.

In ammonia (NH3), the nitrogen atom forms a single bond with each of the three hydrogen atoms, and also possesses a lone pair of electrons that contribute to the molecule's chemical characteristics.

Neutrons within the atomic nucleus possess a net negative charge.

The 3px, 3py, and 3pz orbitals possess differing energy levels within an atom.

A triple bond involves the sharing of six electrons between two atoms.

Ionization is the process of converting a neutral atom into one with either a positive or negative electric charge.

The number of neutrons always determines the chemical nature of an atom.

Electrons reside in specific regions around the nucleus called isotopes.

In a water molecule (H2O), the oxygen atom forms a double bond with each of the two hydrogen atoms.

The inert elements, like helium and neon, are chemically unreactive due to their incompletely filled valence orbitals.

The removal of an electron from a neutral atom results in a net negative charge on the atom, forming a positively charged ion, also known as a cation.

Electrons fill atomic orbitals starting with the highest energy orbitals.

A bonding orbital formed by sharing electrons between two atoms is equivalent to a single covalent bond.

Sodium (Na) readily gains one electron to achieve a stable electronic structure similar to argon.

Electrons in lower energy levels are more easily dislodged from the atom than higher-energy electrons.

An atomic orbital can hold a maximum of two electrons, each with opposite spin.

The atomic number of carbon is 8.

Hydrogen atoms form double bonds with each other in molecular hydrogen (H2).

Ionic bonds involve the sharing of electrons between two atoms.

The number of electrons in an atom is always equal to the number of neutrons.

Lone pairs of electrons are directly involved in covalent bonds.