Unit 3 Practice/Review

Which of the following elements has the smallest radius?

• Mg
• Al
• Si
• K

Which element in Period 2 has the greatest atomic radius?

• Be

• C

• Na

• Li

Of the halogens (group 7A), which has the smallest radius?

• F

• Br

• He

• At

Ionization energy is...

• the energy required to add an electron to a specific atom
• how much energy it takes to remove an electron from an atom
• the energy required to shield the outer electrons from the nucleus
• a measure of the ability of an atom to attract electrons

The atom with the largest atomic radius in Group 8A is -

• Ar

• He

• Kr

• Rn

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

Atoms that have a high electronegativity, _______________.

• give up their electrons more easily.
• hold on to their electrons more tightly.
• have more electron shells.

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)

• Neon (Ne)

• Antimony (Sb)

• Germanium (Ge)

As you move left to right across a period, ionization energy

• increases

• decreases

• says the same

This is the only non-metal to have 1 valence electron. 

• Hydrogen
• Carbdon
• Nitrogen
• Phosphorus