Investigation 1.7.1: GRAPHING PERIODIC TRENDS
QUESTIONS:
Part One:
1. a) H,Li,Na,k
b) He,Ne,Ar,Kr
2. a) the size of atomic radii increases as we go down in single group
b) as we go down the atomic weight increases with a huge value comparing to the
last element in the same group
3. a) the size of atomic radii decreases as we go across a period
b) As we go across the periodic table from left to next element, protons are bigger
than electrons, so adding one proton and one electron to obtain a new atom means that higher
positivity so smaller radius.
4. a) 142 pm
b)205
5. I expect rubidium will have the larger radius as it locates in the next period
QUESTIONS:
Part Two:
1. first ionization energy is the energy needed to remove one mole of the most weakest
held electrons from one mole of gaseous atoms to produce 1 mole of gaseous ions each
with a charge of 1+.
2. a)He,Ne,Ar,kr
b) H,Li,Na,k
3. ionization energy increase as we go through period and decreases as we go down
through the one group as The new subshell is higher in energy (less core-like). Therefore, the
first ionization energy (IE1) for, say, B, is lower than for Be, because the 2p orbitals are
higher in energy than the 2s, and so, B can be more easily ionized than Be.
4. as we mentioned before ionization decreases with moving down in group because going
down increase the atom a new level energy and become more difficult to move electrons
from this atom.
5. the relation between the radii of atom and first ionization energy is reversed from the graph
atoms with high peaks in first curve is the bottom of the second curve as the radii of atoms
increases as easier to be ionized( low energy)
6. 410 kj/mol
7. there is anomaly in ionization energy in the period from the graph (Nitrogen and Oxygen)
this due to in nitrogen, the p-orbital are half filled and this achieve more stability on the
electrons, hence more energy (i.e. high ionization energy) will be needed to remove one of
them. hence, the ionization energy of nitrogen is higher than that of oxygen