Periodic Trends

Which element in Period 2 has the greatest atomic radius?

• Be

• C

• Na

• Li

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Of the halogens, which has the smallest radius?

• F

• Br

• He

• At

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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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Atoms that have a high electronegativity, _______________.

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

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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

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Which statement correctly and completely identifies a trend?

• Atomic radius decreases across a period and increases down a group.
• Electronegativity decreases across a period and decreases down a group.
• Ionization energy increases across a period and increases down a group.
• Ionic radius increases across a period and increases down a group.

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The element with the largest electronegativity in the halogens is - 

• At
• F
• Cl
• Br

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The atom with the largest atomic radius in Group 18 is - 

• Ar
• He
• Kr
• Rn

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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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As you move down a group on the periodic table atoms get bigger. This is because ____________.

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more energy levels

• The atoms have more neutrons

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