The transition metals are defined in the region of the periodic table in which atoms are being added to the d subshell. As a result, the transition metals have unfilled or incomplete orbitals within the d shell. Since each orbital is filled with one electron before orbitals start to become completely filled, there are increasing numbers of unpaired d shell orbitals. This allows transition metals to give up variable numbers of electrons, while maintaining stability, as electrons move between d orbitals.

A common example is iron, which is stable in both the and electron configurations.

The non-metals in group 8 are called noble gases because they tend to resist reactions with other atoms. Noble gases are the only elements to have valence octets in their ground states ().

Halides are the gases in group 7, which are most stable as negative ions to reflect the octet configurations of the noble gases. Lanthanides are the elements in period 6 that have an incomplete f shell. The metalloids are arranged along the diagonal between boron and polonium and divide the periodic table between the metals (to the left) and nonmetals (to the right).

Elements are generally more reactive the closer they are to the stable noble gas configuration (eight valence electrons). Halogens have seven valence electrons, so only need one more to achieve a full valence shell, thus they are said to have high "electron affinity" since they react easily to gain the final valence electron. All the other options are correct statements about halogens.

Metals are found on groups on the left side of the period table (groups 1, 2, and 3, and transition metals). The groups on the left side have fewer valence electrons than the groups on the right side. Groups 1, 2, and 3 have one, two, and three valence electrons, respectively. Metals thus have fewer valence electrons than non-metals.

Electronegativity is a chemical property that is defined as the ability of an element to attract electrons towards itself. Since they have fewer valence electrons, metals find it easier to lose electrons to generate a complete octet (have eight valence electrons). Rather than attract electrons to fill octet, metals give them away. On the other hand, it is easier for non-metals to gain electrons to complete octet because they have larger amounts of valence electrons in their ground state. This means that non-metals have higher attraction for electrons and, consequently, have higher electronegativities.

Alkaline earth metals are found in the second group of the periodic table and include beryllium, magnesium, calcium, strontium, barium, and radium. These compounds are not as reactive as the alkali metals (found in group 1), but still participate in many reactions due to their electron configuration. Alkaline earth metals carry two valence electrons, located in the s orbital. Loss of these two electron leaves the alkaline earth metals with a full octet, giving them a stable oxidation state of +2. In contrast, the alkali metals have a stable oxidation state of +1. Both compounds have very low first ionization energies, but the second ionization energies of the alkaline earth metals are much lower than those of corresponding alkali metals. Removing a second electron from an alkali metal removes it from a stable octet, while removing an additional electron from an alkaline earth metal results in a stable octet.

While all alkali metal salts are soluble, the alkaline earth metals result in several exceptions to the solubility rules. For example, is not soluble in aqueous solutions.

Beryllium (Be), magnesium (Mg), calcium (Ca), and strontium (Sr) are all alkaline earth metals with two valence electrons.

Rubidium (Rb) is an alkali metal and has only one valence electron.

Good insulators are usually non-metals, in which the electrons are not able to freely move. Insulators, unlike conductors, do not carry current. This is because charges cannot move freely in an insulating material, making this choice the correct answer.

Sound would travel slowest through an insulating material, as there is less ability to compress and propagate the sound wave. Copper is an example of a good conductor, and is a poor insulator.

The halogens are the second to last column in the periodic table, meaning that they have an affinity for a single additional electron. Halogens would be most likely to react with alkali metals, which contain only one loosely bound electron in the valence shell. Alkali metals have very low ionization energy, readily losing an electron, while halogens have very high electronegativity, readily gaining an electron. This interaction allows the alkali metals to form ionic bonds with the halogens.

The properties described fit well with the noble gases. Alkali and alkaline earth elements are solid at room temperature, meaning that they have a high boiling point. Halogens can be gaseous at room temperature, but are very reactive. Noble gases have low boiling points and rarely act in spontaneous reactions. Their properties are due to their full valence shell, which is the source of their stability. Changes to their electron configuration (such as removing an electron) require large amounts of energy.

Halogens are in the group next to the noble gasses. They have seven valence electrons, and therefore have a high electronegativity. The addition of only a single electron (production of an anion) generates a full valence octet.

Their diameters vary within the group. The diameter can be very small, like fluorine, or large, like iodine. They do not conduct electricity well, as they are non-metals.