ionisation energy

Question 1

what does it mean for an electron to be ionised ?

Answer 1

being removed from an atom or molecule

Question 2

what is energy needed to remove the first electron called?

Answer 2

first ionisation energy

Question 3

what is the equation for first ionisation energy?

Answer 3

1 mol of gaseous element -> 1 mole of gaseous equation 1+ ions + 1 mole of electrons

Question 4

what state symbol is used for ionisation energy ?

Answer 4

(g)

Question 5

the lower the ionisation energy …

Answer 5

the easier it is to form a positive ion

Question 6

what type of process is ionisation ? explain

Answer 6

endothermic , you have to put in energy to remove an electron from an atom or molecule .

Question 7

what does a high ionisation energy mean when trying to remove an electron ?

Answer 7

theirs a high attraction between the electron and the nucleus so more energy is needed to remove an electron

Question 8

what are the three factors affecting ionisation energy ?

Answer 8

nuclear charge
distance from the nucleus
shielding

Question 9

why does nuclear charge affect ionisation energy ?

Answer 9

the more protons in the nucleus ,the more positvley charged the nucleus is and the stronger the attraction for the electrons

Question 10

why does distance from the nucleus affect ionisation energy ?

Answer 10

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

Question 11

Why does shielding affect ionisation energy ?

Answer 11

the number of electron between the nucleus and outer electron increases .
the electrons feel less attraction to the nucleus .

Question 12

what is the second ionisation energy ?

Answer 12

the energy needed to remove an electron from each ion in one mole of gaseous 1+ ions

Question 13

what is the equation for 2nd ionisation energy?

Answer 13

o+(g)->O2++e-

Question 14

which is higher ,first or second ionisation energies ? explain why

Answer 14

second as the electron is being removed from a positive ,ion which will take more energy

Question 15

what factor determines how high the second ionisation energy is ?

Answer 15

electron configuration

Question 16

what is third ionisation energy ?

Answer 16

the energy needed to remove an electron from each ion in 1 mole of 2+ ion

Question 17

is third ionisation energy greater than second ionisation energy ?

Answer 17

yes , more protons means there is more attraction between electrons to nucleus

Question 18

can you leave the nucleus of the atom and nothing else ?

Answer 18

yes ,by removing all the electrons

Question 19

what is successive ionisation energy ?

Answer 19

the ionisation energy after each electron

Question 20

what is the general eqaution for nth ionisation energy?

Answer 20

X^(n-1)(g) -> X^n+(g) + e-

Question 21

what is the trend for first ionisation energy in group two?

Answer 21

decreases as you go down

Question 22

what does the trend in group two for first ionisation energy provide evidence for ?

Answer 22

the existence of electron shells because as each element going down group two has one more electron shell than the last, the extra shell will shield the electron from the nucleus also it will be further from the nucleus which decreases the electrons attraction to the nucleus

Question 23

what happens with ionisation energy as you move across a period ?

Answer 23

ionisation energy increases and it gets harder to remove an electron

Question 24

why does the trend across periods with ionisation energy happen ?

Answer 24

the number of protons increasing ,which means a stronger nuclear attraction

Question 25

what happens with electron energy across a period ?

Answer 25

stays roughly the same level .even if the orbitals are different types.this means there’s generally little extra shielding effect or extra distance to lessen the attraction from nucleus

Question 26

what happens with ionisation energy between group 2 and 3 ?

Answer 26

a small drop in ionisation energy level ,which shows the sub shell structure

Question 27

what happens between group 5 and 6 in ionisation energy ?

Answer 27

a small drop due to electron repulsion between orbitals

Question 28

what does a graph of successive ionisation energies provide evidence for?

Answer 28

the shell structure of atoms

Question 29

what happens within each shell with successive ionisation energy and why ?

Answer 29

increases because electrons are being removed from an increasingly positive ion so there’s less repulsion amongst the remaining electrons and their held more strongly by the nucleus .

Question 30

what does a big jump in ionisation energy mean ?

Answer 30

when a new shell is broken into as a electron is being removed from a shell closer to the nucleus

Question 31

how do you find which group of a periodic table an element belongs to from a ionisation energy graph ?

Answer 31

count how many electrons are being removed before the first big jump to find the group number

Question 32

how can these graphs predict electronic structure ?

Answer 32

count how many point there are between each big jump to find how many electrons are in each shell