Inorganic chemistry and the periodic table; IONISATION

Question 1

what is ionisation energy?

Answer 1

minimum amount of energy needed to remove 1 MOLE OF ELECTRONS from 1 MOLE OF ATOMS in the GASESOUS state

Question 2

what is the definition of the FIRST ionisation enthalpy and what do they form?

Answer 2

energy needed to remove 1 ELECTRON from EACH ATOM in 1 MOLE of gaseous atoms–> to form 1 mole of gaseous 1+ ions

Question 3

what is an example equation of a first ionisation enthalpy?

Answer 3

O(g)–> O+(g) + e-

Question 4

what are the key points for ionisation enthalpies?

Answer 4

-must have state symbol gas (g)
-Always refer to 1 mole in the defintion
-the lower the ionisation enthalpy –>easier to remove the OUTER electron and from an ion
-always endothermic–>always postitive values

Question 5

what 3 things effect the ionisation enthalpies?

Answer 5

-electron sheilding
-nuclear charge
-atomic size/radius

Question 6

how does the factor electron sheilding influence ionisation enthalpy?

Answer 6

-more electron shells between positive nucleus and negative electron being removed –>weaker attraction–>lower energy required to remove electron–> lower ionisation enthalpy

Question 7

how does the factor nuclear charge influence ionisation enthalpy?

Answer 7

more protons+positive charge in nucleus–> stronger attraction betweeen nucleus and outer electron–>more energy required to remove elctron–>higher ionisation enthalpy

Question 8

how does the factor atomic size influence ionisation enthalpy?

Answer 8

bigger the atom–>outer elctrons are further away from nucleus–>due to more sheilding–>weaker attractive force–>less energy required to remove electron–> lower ionisation enthalpy.

Question 9

explain the ionisation trend for atomic size going down group 1/2.

Answer 9

atomic radius increases–> number of electrons increase+ OUTER electrons are further from the nucleus–>weaker force of attraction–>energy required to remove electron DECREASES down groups.

Question 10

explain the ionisation trend for sheiding going down group 1/2.

Answer 10

sheilding increases down the group–>more shells filled with electrons–>less nucelar attraction–>weaker force of attraction–>energy required to remove electron DECREASES down the group

Question 11

for groups, why is there no increase in ionisation enthalpy?

Answer 11

Although there is an increase in proton number–>does not lead to increase in ionisation enthalpy–>sheilding +atomic size are MORE IMORTANT factors

Question 12

what is the trend for ionisation enthalpy across periods for nuclear charge?

Answer 12

ionisation increases across periods–>elements are in order of proton number which increases along–>increases nuclear charge–>increased attraction between positive nucleus +outer electron

Question 13

what is the trend for ionisation enthalpy across periods for sheilding+atomc radius?

Answer 13

ionisation STLL increases –> becauses outer shell electrons are roughly at the same level–>just a little extra sheileding and distance–>attraction lessened a littlebit BUT nuclear charge prioritises.

Question 14

explain ionisation enthalpy for s block elements

Answer 14

low first ionisation comapred to different elements in different blocks–>low nuclear charge as genral lower number of protons on left side of peridoic table –>s block =more reactive

Question 15

explain ionisation for elements in the p block

Answer 15

higher first ionisation–>increase in number of protons in right side/across the period–>more difficult to loose outer electron.