Periodic Trends II

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

• the number of protons increases, so attraction to electrons increases

• the number of energy levels increases

• the number of electrons increases

• the atomic mass increases

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NGSS.HS-PS1-1

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 one valence electron is very far from the nucleus, so little energy is needed to remove it

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

The element with the smallest ionization energy in Period 6 is - 

• Rn
• Cs
• Os
• Tm

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NGSS.HS-PS1-1

The element with the smallest ionization energy in Period 6 is - 

• Rn
• Cs
• Os
• Tm

Tags

NGSS.HS-PS1-1

Which element has greater ionization energy?

• Magnesium

• Phosphorus

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Arrange the following in order of increasing ionization energy: Strontium, Aluminum, Indium.

• Strontium, Indium, Aluminum

• Strontium, Aluminum, Indium

• Indium, Aluminum, Strontium

• Aluminum, Indium, Strontium

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Arrange these in increasing order of atomic radii: F, N, B

• B < N < F

• B < F < N

• N < F < B

• F < N < B

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NGSS.HS-PS1-1

Which of the elements Ca, Be, Ba, and Sr has the largest atomic radius?

• Be

• Ba

• Ca

• Sr

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NGSS.HS-PS1-1

Which of these has a greater need for electrons?

• chlorine (Cl)

• Francium (Fr)

Tags

NGSS.HS-PS1-1

Shielding effect

• decreases down and constant across

• Increases down and increases across

• constant down and constant across

• Increases down and constant across

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NGSS.HS-PS1-2