Periodic Trends Assessment (M/C)

First Name

Last Name

Period

• Chemistry 1A
• Chemistry 3A
• Chemistry 4A

Which trend correctly describes atomic radius across a period from left to right?

• Increases due to greater nuclear charge
• Decreases due to greater effective nuclear charge
• Increases due to electron shielding
• Remains constant due to equal energy levels

The first ionization energy of elements generally increases across a period because:

• Atomic size increases
• Nuclear charge decreases
• Electron affinity decreases
• Effective nuclear charge increases

Which element would have the highest electronegativity?

• Sodium
• Chlorine
• Fluorine
• Oxygen

What happens to electron affinity as you move down a group?

• Generally becomes more negative
• Generally becomes less negative
• Stays exactly the same
• Shows no predictable trend

Which statement about atomic radius is correct?

• It increases going down a group
• It decreases going across a period
• It increases going across a period
• It decreases going down a group

The element with the lowest first ionization energy would be:

• Lithium
• Potassium
• Francium
• Sodium

Electronegativity values are highest near which element?

• Cesium
• Neon
• Fluorine
• Nitrogen