1. 3ionisation energies

Question 1

first ionisation energy

Answer 1

the fisrt ionisation energy is the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions.

Question 2

first ionisation energy of oxygen

Answer 2

1314kj

Question 3

atoms and ions fact

Answer 3

you must use the gas symbol as ionisation energy are measured for gaseous atoms
you refer as 1 mole of atoms
the lower the ionisation energy the easier it is to form positive ions

Question 4

factors that effect ionisation energy

Answer 4

nuclear charge
distance from nucleus
shielding

Question 5

nuclear charge

Answer 5

the more protons there are in the nucleus the more positively charged the nucleus is and the stronger the nuclear force of attraction for the electrons

Question 6

distance from nucleus

Answer 6

attraction falls off rapidly with distance. an electron close to the nucleus will be much more strongly nuclear attracted than one further away

Question 7

shielding

Answer 7

as the number of electrons between the outer electrons and nucleus increases the outer electrons would fell less attraction to the nucleus. This lessens the pull of the nucleus thanks to the inner shells. This is known as shielding

Question 8

another name for energy

Answer 8

enthalpy

Question 9

nuclear charge

Answer 9

you can only see the effect of nuclear charge on ionisation energy if you compare atoms with outer shell electrons the same distance from the nucleus and with equal shielding effects. that only really happens with elements that are in the same period of the periodic table

Question 10

second ionisation energy

Answer 10

this is the energy required to remove an electron of 1 mole of gaseous 1+ ions

Question 11

second ionisation energy energy

Answer 11

like the first one the value of energy depends on the nuclear charge, distance and shielding.

the energy is greater than the first one as the electron being removed is from a positive ion. the elctron configuration of the atom will also play a role in how much larger the second ionisation energy is than the first.

Question 12

third ionisation energy

Answer 12

this will be greater than the second as there is a greater attraction between and 2+ ions and 1+ ions with its electrons

Question 13

example of ionisation

Answer 13

the first electron removed from lithium comes from the second shell 2s 1 .
the second electron removed would be from the fisrt shell so the second electron would face a stronger nuclear attraction.
the second electron would have no sheilding therefore would be more attracted

Question 14

successive ionisation energy

Answer 14

you can remove all of the electrons in the nucleus however each time you remove an electron the larger the successive energy is.

x (n-1)+ —–> x n+ + e -

Question 15

group 2 ionisation energy

Answer 15

the first ionisation energy decreases down the group.
this provides evidence that electron shells do exist, if each element in group 2 has one more shell than the one above then the extra shell will shield the other shells from the nuclear attraction from the nucleus.

Question 16

distance and group 2 energy

Answer 16

distance decreases energy as well

Question 17

ionisation across periods

Answer 17

if you move across the period the general trend shows that ionisation energy increases.This is because as the number of proton’s increases then the strengh of the nuclear attraction increases also.

Question 18

extra electrons

Answer 18

the extra electrons are at roughly the same energy level even if the outer electrons are in different orbital types. This means that there’s generally little extra shielding effect or extra distance to lesen the attraction from the nucleus.

Question 19

group 2 and 3

Answer 19

aluminium outer electron is in 3 p orbital rather than a 3s . 3p has a slightly higher energy than the 3s orbital, so the electron is on average to be found further from the nucleus.
3p as extra shielding provided from the 3s orbital

these factors together can override the effect of increased nuclear charge , resulting in the ionisation energy dropping slightly. This pattern in ionisation energies provides evidence for the theory of electron sub shell

Question 20

group 2 and 3 factors

Answer 20

these factors together can override the effect of increased nuclear charge , resulting in the ionisation energy dropping slightly. This pattern in ionisation energies provides evidence for the theory of electron sub shell

Question 21

group 5 and 6

Answer 21

the drop between group 5 and 6 is due to electron repulsion.

Question 22

group 5 and 6 example

Answer 22

the shielding is identical in the phosphorus and sulfur and the electron is being removed from an identical orbital.
in phosphorus’s case the electron is being removed from a singly occupied orbital. but in sulfur the electrons is being removed from an orbital containing two electrons

Question 23

group 5 and 6 reasons for drop

Answer 23

the repulsion between two electrons in an orbital means
the repulsion between two electrons in an orbital means
that electrons are easier to remove from shared orbital orbital . it is more evidence for electronic structure model.

Question 24

ionisation energy and shell structure

Answer 24

if you know the successive ionisation energies of an element you can work out the number of electrons in each shell of the atom and which group the element is in. a graph of successive energies provides evidence the shell structure of atoms

Question 25

what happens within each shell

Answer 25

the successive ionisation energies increases

this is because the electron is being removed by an increasingly positive ion

Question 26

why does the successive ionisation energies increases

Answer 26

this is because there’s less of a replusion amongst the remaining electrons so they’re held more strongly by the nucleus.

Question 27

why is there a sometimes a big jump when it comes to successive ionisation

Answer 27

The big jump in ionisation energy happens when a new shell is broken into. an electron that is closer to the nucleus.