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When going across a period, as you add more protons to the nucleus of an atom, the force of attraction on the electrons

• increases

• decreases

• remains unchanged

As you increase the distance between protons and electrons, the force of attraction between them

• increases

• decreases

• remains unchanged

As you move down a group, atomic radius increases because - 

• you add more and more neutrons
• you add more and more protons
• you add more and more shells (energy levels)
• you add more atomic mass

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

• Ar
• He
• Kr
• Rn

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NGSS.HS-PS1-1

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

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The atom with the largest atomic radius in Period 4 (row 4) is - 

• K
• Kr
• Fe
• Fe

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

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NGSS.HS-PS1-1

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

• Rn
• Cs
• Os
• Tm

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NGSS.HS-PS1-1

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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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NGSS.HS-PS1-1

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The energy required to remove electrons is the definition of: 

• Electronegativity
• Atomic Number
• Atomic Radius
• Ionization