Periodic Trends and Electrons Review

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

• Nitrogen (N)
• Lithium (Li)
• Antimony (Sb)
• Germanium (Ge)

Tags

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)

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-2

Which atom has the largest atomic radius?

• potassium
• rubidium 
• francium
• cesium

Tags

NGSS.HS-PS1-1

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.

The vertical columns of the periodic table are called -

• groups.
• rows.
• periods.
• transition.

Tags

NGSS.HS-PS1-1

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

• increasing number of valence electrons.

• increasing shielding.

• increasing effective nuclear charge.

• increasing number of protons in the nucleus.

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 neutrons.

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.

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

• F has more valence electrons 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.

An anion is a negatively charged ion.

• True
• False