Periodicity

The minimum energy required to remove an electron from the ground state of an atom

• electron configuration
• energy levels
• ionization energy
• ionic bond

The tendency of an atom to attract electrons and acquire a negative charge

• electronegativity
• charge
• bonding ability
• electron configuration

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NGSS.HS-PS1-1

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Vertical columns of elements (families) on the periodic table with similar valence electron configurations and similar properties

• groups
• periods
• quadrants
• rows

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NGSS.HS-PS1-1

An electron that resides in the outermost shell, or principal quantum level, of an atom

• periodic trend
• electron shell
• ionic radius
• valence electron

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NGSS.HS-PS1-1

NGSS.HS-PS1-2

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

• Gallium
• Aluminum
• Magnesium
• Strontium

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NGSS.HS-PS1-1

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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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

Tags

NGSS.HS-PS1-1

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Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

As you move down the periodic table atoms get bigger.  This is because ____________.

• The atoms have more mass.
• The atoms have more protons.
• The atoms have more energy levels
• The atoms have more nuetrons

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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.

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2