Increasing Periodic Trends

Atomic Radius describes:

• atom size

• attraction for valence electrons

• effective nuclear charge

• number of protons

Electronegativity describes:

• atom size

• attraction for valence electrons

• effective nuclear charge

• number of protons

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Ionization Energy describes:

• energy required to remove a neutron

• energy required to remove a shell

• energy required to remove a proton

• energy required to remove a valence electron

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Choose 2 answers:

As you move down a group, which of the following INCREASES:

• atomic radius

• number of shells

• Effective Nuclear Charge

• Ionization Energy

• Electronegativity

CHOOSE 2 answers:

As you move across a period, which of the following INCREASES

• proton number

• effective nuclear charge

• number of shells

• atomic radius

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Which of the following increases DOWN a group?

• Effective Nuclear Charge

• Shielding Effect

• Electronegativity

• Ionization Energy

Which trend does not apply to the Noble Gases?

• Electronegativity

• Ionization Energy

• Atomic Radius

• Effective Nuclear Charge

Which element on the periodic table has the most Electronegativity?

(is the most electron greedy)?

• Fluorine, F

• Helium, He

• Neon, Ne

• Hydrogen, H

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Consider the following elements in Period 3.

Which lists them in order of increasing atomic radius?

• S - Ar - Mg - P

• Ar - S - P - Mg

• Mg - P - S - Ar

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Consider the elements of Group 18.

Which of the following lists them in order of increasing Ionization Energy?

• He - Ar - Xe - Rn

• Rn - Xe - Ar - He

• Rn - Ar - He - Xe

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