The periodic table and ionisation energy

Question 1

How is the periodic table arranged

Answer 1

By increasing proton number

Question 2

periodicity?

Answer 2

Repeating trend in properties of elements across each period

Question 3

Name for group one elements (Li onwards)

Answer 3

alkali metals

Question 4

Name group 2

Answer 4

Alkaline earth metals

Question 5

Name group 7

Answer 5

Halogens

Question 6

name group 0

Answer 6

noble gases

Question 7

What does period number describe

Answer 7

The principle quantum number of the highest energy electron shell in an elements atom

Question 8

What do elements in the same group have in common regarding electrons

Answer 8

Same number of electrons in their outer shell and in each sub shell

Question 9

what gives elements in a group their similar chemical properties

Answer 9

their similar electron structures

Question 10

what did Mendeleev do to the periodic table of elements ordered by atomic mass

Answer 10

Leave gaps for undiscovered elements
Predict the properties of those elements based on the surrounding
Swap the order of some elements so they fit into groups based on properties

Question 11

First ionization energy?

Answer 11

Energy required to remove one electron from each atom in one mole of gaseous atoms of an element

Question 12

unit for first ionization energy?

Answer 12

kJ mol-1

Question 13

factors affecting ionization energy

Answer 13

Atomic radius, nuclear charge inner shell shielding

Question 14

How does atomic radius affect ionization energy

Answer 14

The greater the distance between the nucleus and outer shell the weaker the attraction on outer shell electrons therefore less energy req to remove electron

Question 15

how does nuclear charge affect ionization energy

Answer 15

More protons in the atom, greater attraction to outer shell electrons so req more energy to move electrons

Question 16

how does inner shell shielding affect ionization energy

Answer 16

The shielding effect reduces the attraction between the nucleus and outer shell electrons. More inner shells means less energy required to remove an electron

Question 17

shielding affect?

Answer 17

Idea that inner shell electrons repel outer shell electrons

Question 18

group trends in first IE

Answer 18

FIE decrease going down a group
FIE increase across a period

Question 19

why does FIE decrease down a group

Answer 19

Atomic radius increases
More inner shells so shielding increases
Overall nuclear attraction decreases

Question 20

why does FIE generally increase across a period

Answer 20

Nuclear charge increases
Atomic radius decreases ( not bc of number of shells but bc a more positive nucleus will attract the electrons more)
Overall nuclear attraction increases

Question 21

Between which elements are there anomalies in the increasing of FIE across a period

Answer 21

Berillium to Boron
Nitrogen to Oxygen
There is a decrease in FIE rather than an increase

Question 22

what is the reason for the decrease of FIE from beryllium to boron

Answer 22

Boron marks the start of filling th p6 sub shell, it has 1 electron in this sub shell. Bc the 2p has more energy than 2s it is easier to remove the outer 2p electron in boron than the 2s electron in Be

Question 23

what causes the decrease in FIE from N to O

Answer 23

O Mark’s the start of spin pairing electrons in the 2p orbital, it is easier to remove a spin paired electron because of the repulsion that it experiences

Question 24

successive ionization energy?

Answer 24

like first ionization energy but is the energy required to remove the following electrons (an element can have as many successive IE as it has electrons)

Question 25

How many outer shell electrons are removed at a time in relation to successive IE

Answer 25

one at a time

Question 26

how does the successive IE change as the number increases ( 2nd to 3rd to 4th etc)

Answer 26

It increases bc after an electron is lost, the remaining electrons are pulled closer to the nucleus so the nuclear attraction on the remaining electrons has increased so they require more energy to remove

Question 27

what can first and successive IE provide evidence for

Answer 27

The different electron energy levels (shells) in an atom

Question 28

On an IE graph what characterises a change in shells

Answer 28

A large difference in ionization energy bc the next shell is much closer to the nucleus so attraction is higher so electrons require more energy to remove

Question 29

on an IE graph what characterises the number of electrons in a shell

Answer 29

the IEs increasing by small increments