Periodicity

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

• The atoms have more mass.

• The atoms have more protons.

• The atoms have more shells

• The atoms have more nuetrons

Atomic radius generally increases as we move __________.  

• down a group and from right to left across a period 

• up a group and from left to right across a period 

• down a group and from left to right across a period 

• up a group and from right to left across a period 

The electronegativity of Cl is the highest in Period 3. Why?

• Cl is the largest and has the greatest effective nuclear charge

• Cl is the smallest and has the lowest effective nuclear charge

• Cl is the largest and has the lowest effective nuclear charge

• Cl is the smallest and has the greatest effective nuclear charge

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As you move across the periodic table atoms tend to get smaller because, ______________.

• the atoms have more mass.

• the atoms have less mass

• the atoms have more protons.

• the atoms have less electrons.

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• A

• B

• C

• D

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Row of elements on the periodic table that represent the number of energy levels.

• Atomic Number

• Atomic Mass

• Period

• Group

What period does the element I - Iodine belong to?

• 17

• 6

• 3

• 5

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What category is silicon (Si) a part of?

• Metal

• Nonmetal

• Metalloid

• Halogens

The trends on the periodic table are dependent on..

• how attracted a valence electron is to the nucleus

• how attracted valence electrons are to each other

• how attracted a valence electrons is to a non valence electron

• how attracted a non valence electron is to the nucleus

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The higher the ionization energy...

• the more attracted the valence electron is to the nucleus so it is harder to remove

• the less attracted the valence electron is to the nucleus so it is easier to remove

• the more attracted the valence electron is to another electron, so it is harder to remove

• the more repelled a valence electron is to another electron, so it is easier to remove

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