Periodic Trends

Which element, oxygen or sulfur, has a greater electronegativity and why?

• Sulfur, because it has more energy levels

• Oxygen, because it has a greater effective nuclear charge

• Oxygen, because the outermost electrons are closer to the nucleus therefore experience a greater attraction to the nucleus

• Sulfur, because it has a greater effective nuclear charge

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which has the greater electronegativity:

N or C?

• C

• N

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NGSS.HS-PS1-1

Which of the following will have a larger radius than Zinc?

• Gallium
• Aluminum
• Magnesium
• Strontium

Which of the following will have a higher electronegativity than arsenic (As)?

• Carbon (C)
• Neon (Ne)
• Antimony (Sb)
• Germanium (Ge)

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NGSS.HS-PS1-1

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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-PS1-1

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

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NGSS.HS-PS1-2

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.

Atoms that have a high electronegativity, _______________.

• give up their electrons more easily.
• hold on to their electrons more tightly.
• have more electron shells.

Electronegativity is...

• how good an atom is at attracting electrons
• the ability of an atom to lose electrons
• the energy required to remove an electron from a specific atom
• how easy it is to make friends. 

Ionization energy is...

• the energy required to add an electron to a specific atom
• how much energy it takes to remove an electron from an atom
• the energy required to shield the outer electrons from the nucleus
• a measure of the ability of an atom to attract electrons

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NGSS.HS-PS1-1