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WorksheetsPeriodic Trends and Ions
Total questions: 15
Worksheet time: 9mins
As you move down a group, atomic radius increases because
you add more and more neutrons.
you add more and more protons.
you add more and more shells (energy levels).
you add more atomic mass.
Which element in Period 6 has the lowest ionization energy?
Rn
Cs
Os
Tm
As you move across the periodic table from left to right, the atomic radius decreases. Why?
The number of protons increases, so attraction to electrons increases.
The number of energy levels increases.
The number of electrons increases.
The atomic mass increases.
Francium (Fr) has the lowest ionization energy in Group 1 because
it has the smallest number of valence electrons.
it has the greatest atomic mass.
it has the greatest number of protons, so it attracts its electrons the strongest.
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it.
Which atom in Period 4 has the largest atomic radius?
K
Kr
Fe
Fe
The element with the largest electronegativity in the halogen group is
At.
F.
Cl.
Br.
Ions are formed when atoms gain or lose ___.
electrons
protons
neutrons
atomic mass
What periodic trend is illustrated here?
Atomic Radius
Ionization Energy
When an atom loses an electron, it becomes a(n) _____________ ion.
positive
negative
neutral
polyatomic
Which particles change the charge in atoms when ions are formed?
Protons
Electrons
Neutrons
What is the charge of an atom that has gained two electrons?
-1
-2
+1
+2
When the atomic radius increases, electron affinity
Decreases
Increases
Neutral
No effect
