periodic trends review pt.1

The ability to attract an electron in a chemical bond

• electronegativity

• electron affinity

• metallic character

• ionization energy

The energy it takes to remove an electron from an atom in the gas phase

• electron affinity

• electronegativity

• metallic character

• ionization energy

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NGSS.HS-PS1-1

Ionization energy increases

• from L to R and from bottom to top

• from L to R and from top to bottom

• from R to L and from bottom to top

• from R to L and from top to bottom

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Atomic radius decreases from left to right across a period because from left to right there is

• increasing number of valence electrons

• increasing shielding

• increasing effective nuclear charge

• increasing number of protons in the nucleus

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NGSS.HS-PS1-1

Which of the following will have a lower ionization energy than Scandium (Sc)?

• Helium (He)
• Titanium (Ti)
• Calcium (Ca)
• Magnesium (Mg)

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NGSS.HS-PS1-2

As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....

• decreases
• increases
• remains the same
• none of the above

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

• Ar
• He
• Kr
• Rn

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NGSS.HS-PS1-1

The element with the highest electronegativity is -

• At

• F

• Cl

• Br

The ionization energy of Na is larger than Cs because...

• Na has a greater effective nuclear charge

• Na has fewer energy levels and less shielding

• Cs has a greater effective nuclear charge than Na

• Cs has more valence electrons than Na

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Fluorine has a smaller atomic radius than B because...

• F has more valence e- than B

• F has more shielding than B

• F has a larger atomic number than B

• F has a greater effective nuclear charge than B

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NGSS.HS-PS1-1