WorksheetsPeriodic Table & Trends
Total questions: 15
Worksheet time: 8mins
Why do the elements in the same group behave similarly?
They have the same number of protons
They have the same number of outer electrons (valence electrons)
They have the same number of neutrons
They have the same number of shells
As you go down group 2, how many electrons will the elements have in the outer shell?
1
2
3
4
What happens to the size of the atom (atomic radius), as we go down the group?
Increases
Decreases
Stays the same
Why does this trend in atomic radius size occur as we go down the group?
There is an extra shell for each element as we go down the group
There is one shell less for each element as we go down the group
The shell number stays the same as we go down the group
What happens to the size of the atomic radius as we go across the period?
Increases
Decreases
Stays the same
Why do we see this trend in atomic radius as we go across the period?
The number of protons increases as we go across the period and so the attraction between the nucleus and the outer electron increases and pulls the electron towards the nucleus, therefore the atomic radius gets smaller
The number of protons decreases as we go across the period and so the attraction between the nucleus and the outer electron lessens and the electron is not pulled towards the nucleus, therefore the atomic radius gets bigger
Nothing happens
If we add an electron to an atom (so making it a negative ion) what happens to the ionic radius and why?
The electrons repel each other so the radius gets bigger
The electrons increase so it gets bigger
Nothing changes
What is ionisation energy?
The energy needed to remove a proton from the atom
The energy needed to remove a neutron from the atom
The energy needed to remove an electron from the atom
Is it easier to remove an electron that is ...
Closer to the nucleus
Further away from the nucleus
On it's own and unpaired
As we go across the period, we see the atomic radius decreases in size due to increasing protons. So, what happens ionisation energy as we go across the period?
Decreases
Increases
Stays the same
Oxygen has a lower ionisation energy to Nitrogen, why?
Oxygen has a pair of electrons in one of the p-orbitals and these will repel each other, so making it easier to remove an electron.
Nitrogen has a pair of electrons in the p-orbitals and these will repel each other, so making it easier to remove an electron.
No idea
What is electron affinity?
How much an atom wants to lose an electron
How much an atom wants to gain an electron
How much an atom wants to lose a proton
Which element in the periodic table has the highest electron affinity?
Fluorine
Chlorine
Bromine
Why would elements in group 1 have low electron affinities?
No idea
They want to lose an electron, not gain one in order to acquire a full outer shell of electrons.
They hate electrons
What is electronegativity?
The ability of the atoms to become negative
The ability of the atoms to hold on to their electrons
The ability for an atom to conduct electricity
