Reading the Table Trivia Quiz

Answer: Burgium has two more electrons in its valence shell than Loonium

The group (or column) in which an element is found is a good indicator of the number of electrons in its valence (outermost) electron shell. Elements in group 1 have one valence electron, elements in group 2 have two valence electrons, and noble gases (in group 8 (or 18)) have a full outer shell of electrons.

Answer: Mimoium has one more electron shell than Dazzium

Whilst the group number indicates the number of valence electrons, the period number tells us how many electron shells an element contains. For example, hydrogen, in period 1, has only one electron shell. Lithium, in period 2, has two electron shells, and so on.

Answer: Glendium is larger than Jabberium

The period number is an indication of how many electron shells an element possesses. Since the definition of an electron shell (and an electron orbital) is a 3D space where there is a high probability of finding an electron, more electron shells mean a larger atomic radius.

Answer: It will lose an electron to form a valence shell more like Aerolancium's

Elements lose, gain, or share electrons, forming ions or compounds in order to obtain a full outer shell of electrons, like the noble gases. The noble gases are stable and unreactive, and usually exist in their monatomic form.

Answer: Emmium

In this instance, the reactivity of a group 1 element can be defined by the ease with which the element is able to lose (or donate) its single valence electron, thus forming an ion which has a full outermost shell. Emmium is in period 5, so its valence electron is found in the 5th electron shell.

This is far from the positively charged nucleus and so there is a smaller attractive force holding the valence electron in orbit. This is in comparison to Salamium, which has its valence electron in the second electron shell, much closer to the positive nucleus.

Answer: A grey/black solid

When constructing the periodic table, Mendeleev was able to leave blank spaces for where he thought an as of yet undiscovered element should be placed. This was largely based on trends of chemical and physical properties. The halogens provide a good example of a change in physical properties. Going down the group, we begin with fluorine and chlorine, both yellowy-green gases, then bromine is a brown liquid and iodine a bluish-grey solid.

There is a clear trend, becoming darker and less fluid as we move down the group.

The last element of the halogens, astatine, is very unstable and sufficient amounts have not been collected to characterise it, though it is believed to follow the trend and be a black solid.

Answer: Elainium

This is slightly trickier than comparing the size of elements in different periods (where the higher the period number, the larger the atomic radius). Instead, Elainium and Kylium are in the same period and have the same number of electron shells. The difference is that Kylium has 3 more protons in its nucleus than Elainium (since Kylium is in group 5 and Elainium is in group 2).

This more positive nucleus is able to attract the valence electrons more strongly, therefore pulling the outermost electrons in and decreasing the atomic radius.

Answer: Babium can form a number of possible positive ions, whereas Bassium will only usually form one

Although, as a transition element, Babium is likely to be a metal, there is no way of telling whether or not Bassium is a metal. Instead, the defining characteristic of a transition element is the ability to form a number of positively charged ions. For example, iron can form stable 2+ ions and 3+ ions. Elements found in groups 1, 2, 3 etc. tend to lose (or gain) a set number of electrons and so form ions of consistent charge.

Answer: Aprilium

In contrast to group 1 elements, the reactivity of group 7 elements is defined by their ability to gain an electron. Elements whose valence shells are closer to the positive nucleus will therefore be more reactive. Since Aprilium is in period 3, its valence electrons are closer to the nucleus than in Jamillium, which is in period 5.

Answer: Exitium

Excluding the transition block, there are eight groups (or columns) along which there is a clear progression in the way that electron sub-shells are filled. In a new electron shell, the first electron fills an s orbital, and so does the second one. The s sub-shell holds a maximum of two electrons.

The next six electrons fill orbitals in the p sub-shell, which holds a maximum of six electrons. Therfore, groups 1 and 2 are defined as s-block elements and groups 3-8 are p-block elements. The valence electrons in transition elements fill d orbitals and so this is called the d block. Elements known as lanthanoids and actinoids have their valence electrons in a fourth type of electron sub-shell (the f sub-shell) and these are called the f-block elements.