3.1.1 Periodicity

Question 1

the periodic table as the arrangement of

elements:

Answer 1

• by increasing atomic (proton) number
• in periods showing repeating trends
  in physical and chemical properties
  (periodicity)
• in groups having similar chemical properties

Question 2

elements are classified into ______ within the Periodic Table and elements in the same block have their _____ _________ in the same type of _______

Answer 2

blocks, outer electrons, orbital

Question 3

s-block=

Answer 3

groups 1 and 2

Question 4

p-block=

Answer 4

groups 3 to 0

Question 5

d-block=

Answer 5

transition metals

Question 6

f-block=

Answer 6

lanthanides and actinides

Question 7

______ ______ _____________ are often _______ __ _____ ______ within the Periodic Table. __________ is the study of these ______.

Answer 7

direct electron configurations, linked to other trends, periodicity, trends

Question 8

for period _ and _, first the _ ________ are ______, followed by the _ ________.

Answer 8

2, 3, s orbitals, filled, p orbitals

Question 9

first IE _______ AS U GO ALONG A PERIOD

• atomic radius ________ and nuclear attraction _______.
• this is due to an _________ ______ ______ for the same ______ of _______ ______.
• same____: similar _______
• more _____ is required to remove ____ electron

Answer 9

• INCREASES,
• decreases, increases
• increased nuclear charge, number, electron shells,
• shell, shielding
• energy, outer

Question 10

first IE _________ AS U GO DOWN A GROUP

• atomic radius _______.
• more inner shells so shielding _______ so the _____ attraction on outer electrons _______
• therefore ______ required to remove electron __________

~ this data provides strong evidence for ______ in atoms and proves Bohr’s model of the atom is correct BUT didnt explain data shown across a period

Answer 10

DECREASES,

• increases,
• increases, nuclear, decreases
• energy, decreases

Question 11

first ionisation energy is defined as: (+ measured in)

EXAMPLE: FIRST IONISATION ENERGY FOR IT:

Answer 11

the minimum energy required to move one mole of electrons from one mole of atoms in a gaseous state (kJmol-1)

EXAMPLE: Na(g) –> + e-
FIRST IONISATION ENERGY: +496kJmol-1

Question 12

successive ionisation energy: removal of …. read description on pg 96 for the rest

Answer 12

… more than one electron from the same atom

Question 13

Ionisation requires energy so they always have an _________ and have a ________ value

Answer 13

endothermic, positive

Question 14

shielding

Answer 14

the more electron shells between the positive nucleus and negative electrons that is being removed the less energy is required.
there is a weaker attraction and is therefore easier to lose outer (valence?) electrons

Question 15

second ionisation energy

Answer 15

energy required to remove the electron from each ion in 1 mol of gaseous 1+ ions of an element to form 1 mol of gaseous 2+ ions of an element

Question 16

why are successive energy always bigger

Answer 16

because the ion formed, is smaller than the atom and the proton to electron ratio in
the 2+ ion is greater than in the 1+ ion. The attraction between nucleus and electron is
therefore stronger

Question 17

general trends in first ionisation energies

• general ______ in first IE across each _____
• ____ decrease in first IE between end of one ____ to ____ of the next period

Answer 17

• increase, period

- sharp, period, start