Periodic Trends Quiz: Explore Patterns in the Periodic Table

Questions and Answers

The similar atomic structure of the elements within their respective group families or periods

An atom's ability to attract and bind with electrons

Because it is a qualitative property

To quantify the electronegativity of an element Signup and view all the answers

It provides chemists with an invaluable tool to quickly predict an element's properties Signup and view all the answers

Because it requires less energy to lose an electron than to gain one Signup and view all the answers

It decreases Signup and view all the answers

Because their metallic properties affect their ability to attract electrons Signup and view all the answers

Because they possess a complete valence shell Signup and view all the answers

Ionization energy Signup and view all the answers

Study Notes

Most atoms follow the octet rule, having 8 electrons in their valence shell.
Elements on the left side of the periodic table tend to lose electrons, while those on the right side tend to gain electrons.
Electronegativity increases from left to right across a period and decreases from top to bottom down a group.

If the valence shell is less than half full, it's easier to lose an electron than to gain one.
If the valence shell is more than half full, it's easier to pull an electron into the valence shell than to donate one.
Atomic number increases down a group, leading to a greater distance between valence electrons and the nucleus, resulting in decreased electronegativity.

Noble gases have a complete valence shell and do not usually attract electrons.
Lanthanides and actinides have complex chemistry that does not follow trends.
Transition metals have electronegativity values, but with little variance across the period and up and down a group.

Ionization energy is the energy required to remove an electron from a neutral atom in its gaseous phase.
The lower the ionization energy, the more readily the atom becomes a cation.
The higher the ionization energy, the less likely it is for the atom to become a cation.

Periodic trends are patterns in the periodic table that illustrate different aspects of an element, including size and electronic properties.
Major periodic trends include electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character.
Periodic trends exist due to the similar atomic structure of elements within their respective group families or periods, and the periodic nature of the elements.