Electron Shielding and Effective Nuclear Charge

The Shielding Effect is the result of interference between the

• protons and neutrons
• protons and electrons
• nucleus and valence orbital
• atoms and molecules

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The valence electrons are located on 

• the orbital closest to the nucleus
• the orbital furthest from the nucleus
• the orbital with the most electrons
• the orbital with the least electrons

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What creates a SHIELDING EFFECT by interfering with the attractive forces between the protons and the electrons.

• nucleus
• valence electrons
• core electrons
• protons

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As you move down a group, shielding 

• increases because there are more  orbitals
• increases because there are more protons
• decreases because the atomic radius increases
• stays constant because the number of valence electrons stays the same

As you move across a period (row), the shielding effect

• increases by a factor of 2
• decreases by a factor of 2
• stays constant
• alternates for metals an nonmetals

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Which element has the least amount of shielding?

• Potassium (K)
• Iron (Fe)
• Oxygen (O)
• Barium (Ba)

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Which of the following elements has the largest shielding effect?/

• Li
• Na
• K
• Rb

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Put the following elements in order of increased shielding effect.

• Sodium (Na), Silicon (Si), Chlorine (Cl)
• Silicon (Si), Chlorine (Cl), Sodium (Na), 
• Chlorine (Cl), Sodium (Na), Silicon (Si)
• Each of these has the same amount of shielding.

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When shielding increases, it causes 

• the atomic radius to increase
• the ionization energy to increase
• the metallic properties to decrease
• the ionic radius to decrease

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If shielding remains constant, which of the following is NOT true when moving from left to right across a period (row)?

• the atomic radius decreases
• the metallic properties decrease
• the electronegativity increases
• the atomic number decreases

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