Chapter 7- Periodicity Flashcards
how did Mendeleev order the periodic table
by atomic mass - he left gaps where required so that elements could be in groups of similar chemical properties
what happens to atomic number moving left to right
it increases
what are groups
elements with the same chemical properties because they have the same number of outer electrons
what are periods
horizontal rows, period number relates to the highest energy level held by electrons in that atom
what does periodicity include
- electron configuration
- ionisation energy
- structure
- melting/boiling points
what are the blocks of the periodic table
+ s-block = groups 1 and 2 –> outermost electrons in the s-subshell
+ d-block = transition metals - outer electrons in d subshell
+ p-block = right side = outermost electrons in the P subshell
what is the definition of ionisation energy
“the energy required to remove one electron from each atom in one mole of gaseous atoms”
what are the 3 factors affecting ionisation energy
nuclear charge, atomic radius, shielding
MENTION ALL 3 IN ANSWERS
explanation of how nuclear charge affects ionisation energy
the greater the atomic number/nuclear charge, the more protons there are; this exerts a greater pull on the outer electrons / more electrostatic forces, so more energy is required to remove the outer electron
explanation of how atomic radius affects ionisation energy
a greater atomic radius leaves the outer electrons further from the nucleus, across a period atomic radius decreases due to increased nuclear charge, a greater distance gives less electrostatic force so less ionisation energy
explanation of how shielding affects ionisation energy
greater shielding reduces the attraction from the nucleus to the outer electrons, this decreases ionisation energy. so more electron shells gives a lower ionisation energy
what happens to ionisation energy across a period
- nuclear charge increases across a period so electrostatic attraction increases
- atomic radius decreases across a period due to greater nuclear charge. this means the outer electrons are closer to the nucleus so attraction increases
- shielding remains constant
- overall ionisation energy increases
what are the two exceptions to the general ionisation energy rule across a period
- where a higher energy subshell is being filled/electron being removed from; this is further away so ionisation energy decreases
- paired electrons in P subshell are easier to remove due to the repulsion between electrons (only for first paired p electron)
explanation of ionisation energy down a group
- shielding increases as you move down a group; this decreases attraction to outer electrons
- atomic radius increases down a group; this decreases electrostatic attraction to outer electrons
- nuclear charge increases down a group but this is not sufficient to overcome the changes due to the other factors
- overall ionisation energy decreases
how does energy change with successive ionisations
- with each successive ionisation, more energy is required as you are then removing an electron from a positive ion
- this increases the effective nuclear charge