Periodic Trends Knowledge Check

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

As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 

• 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

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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

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Electronegativity is...

• the ability of an atom to attract/ accept electrons
• the ability of an atom to lose electrons
• the energy required to remove an electron from a specific atom
• how easy it is to make friends. 

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Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

• decreases, increases 
• increases, increases
• increases, decreases 
• stays the same, increases

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Ionization energy is the...

• energy needed to remove the outermost electron.
• ability of an atom to attract electrons from another atom.

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Which is larger:
P or P^-3

• P
• P^-3
• both are same size

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

• decreases
• increases
• remains the same
• none of the above

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Metals have the largest - 

• atomic radius and electronegativity
• electronegativity and ionization energy
• atomic radius only
• ionization energy and atomic radius

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Which periodic group has the smallest atomic radius?

• Alkali metals
• Halogens
• Noble Gases
• Transition metals

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