8.1 the periodic table Flashcards
What are the different types of blocks
s
p
d
f
why is sodium in S-block
as it has their highest energy electrons (valence) in s-orbitals
what is S-Block
groups 1 and 2
what is P-Block
groups 3 to 0
what is D-Block
transition metals
what is F-block
radioactive elements
what are valence electrons
outer shell electrons
what is periodicity
the study of patterns and trends in the chemical and physical properties of elements
how does the atomic radius differ along a period
atomic radius decreases. This is due to an increased nuclear charge for the same number of electron shells. The outer electrons are pulled in closer to the nucleus as the
increased charge produces a greater attraction. As a result, the atomic radius for that element is reduced
Model answer:
which has a larger radius sodium or chlorine
- Na has less protons then Cl
- Both atoms have the same number of shells and shielding
- greater nuclear charge so a greater attraction between the valence electron and the nucleus
model answer:
which has a larger radius a sodium atom or ion
sodium atom
it has lost 1 electron so it has one less shell
model answer:
why does a chloride ion have a larger radius than a chlorine atom
the ion has more electrons than protons
there is a greater electron on electron repulsion so there is a greater force of attraction
Electron-electron repulsions:
due to their like charges, electron pairs orient themselves as far away as possible from
each other, causing the electron cloud to expand
nuclear charge:
charge of the nucleus
charge of the nucleus and the inner electrons combined
how does the atomic radius differ down the group
atomic radius increases. With each increment down a group, an electron shell is added each time. This increases the distance between the outer electrons and the nucleus, reducing the power of attraction. More shells also increases electron shielding Therefore the nuclear attraction
is reduced further and atomic radius increases.
