The Periodic Table and Periodicity Flashcards
what groups in the periodic table are in the s-block
group 1 and 2
what groups in the periodic table are in the p-block
group 3 to 8
what groups in the periodic table are in the d-block
the transition metals (3 to 13 in a group 1 to 18 periodic table)
what is the general trend in the blocks as you go across them and why does the number of groups each block occupies make sense
- there is one more electron in the outer shell for every group you go across (left to right)
- this makes sense as the s orbital can only hold 2 electrons
- so the s-block stops at group 1 and 2 which consist of an s orbital in their outer shells
- the p-block consists of 6 groups
- which matches with the 6 electrons a p subshell can hold with 3 p orbitals
- the d subshell that has 5 d orbitals can hold 10 electrons
- which matches with the ten ‘groups’ the d-block encompasses (the transition metals)
if the periodic table has the s-block on the left, d-block in the middle and p-block on the right, what does that imply about the actual order or arrangement of the periodic table
- that the table is divided into blocks
- rather than simply groups and periods
what is the definition of peridicity
- the regularly repeating pattern
- of atomic, physical and chemical properties
- with increasing atomic mass
what is the atomic radius of an element
- the measure of the size of its atoms
- measured by the distance from the centre of the nucleus to the boundary of the electron cloud
since the atom doesnt have a well defined boundary, how is the atomic radius of an atom practically calculated
- by determining the distance between two nuclei
- and dividing it by 2
what is the covelant radius of an atom
the radius of the atom when it is covelantly bonded with another atom
why are the covelant radii and atomic radii different, even for the same atom of the same element
- when measuring the atomic radii practically, the boundaries of the two atoms would only be touching and not overlapping
- this means that the distance between the two nuclei can be measured (diameter)
- which would give you the radius of the atom
- but for a covelantly bonded atom the boundaries of the electron clouds are overlapping
- which means that the distance between the two nuclei (the diameter) would be decreased
why are the boundaries of the electron clouds overlapping for the covelantly bonded atoms whereas they are only touching for the other example
- because covelant bonding consists of the sharing of electrons
- so their outer shells would have to overlap to do this
- whereas for the atomic example, there is no bond
- so the outer shells dont interact with each other, they would more likely repel
which one between the covelant radius and atomic radius is usually shorter and why
- the covelant radius
- because the boundaries of their electrons clouds are overlapping
- which means that the measured distance between the nuclei is smaller
- leading to a smaller radius
what is the real name of the radius that can only be determined for group 8 elements (other than calling it the atomic radius)
the van der Waals radius
why can only one type of radius be determined for the group 8 elements
- because they dont bond with other elements voluntarily
- so they can only have a ven der waals radius and not a covelant radius
what is the third radius called and what is it used for
- the metallic radius
- which is used for metals