Periodic Trends Review

What is the trend in atomic radius as you move from left to right across a period?

• The atomic radius increases due to decreased nuclear charge.

• The atomic radius remains constant across the period.

• The atomic radius decreases due to increased nuclear charge pulling electrons closer.

• The atomic radius fluctuates without a clear trend.

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What is the trend in ionization energy as you move down a group in the periodic table?

• Ionization energy increases as you move down a group.

• Ionization energy remains constant as you move down a group.

• Ionization energy decreases as you move down a group.

• Ionization energy fluctuates as you move down a group.

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Which element has the highest electronegativity?

• Oxygen (O)

• Chlorine (Cl)

• Fluorine (F)

• Nitrogen (N)

What is the trend in atomic radius as you move down a group in the periodic table?

• The atomic radius decreases due to increased nuclear charge.

• The atomic radius remains constant across the group.

• The atomic radius increases due to the addition of electron shells.

• The atomic radius fluctuates without a clear trend.

What is the trend in electronegativity as you move from left to right across a period?

• Electronegativity decreases as you move from left to right across a period.

• Electronegativity remains constant as you move from left to right across a period.

• Electronegativity increases as you move from left to right across a period.

• Electronegativity first increases and then decreases as you move from left to right across a period.

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What is the trend in electronegativity as you move down a group in the periodic table?

• Electronegativity increases as you move down a group.

• Electronegativity remains constant as you move down a group.

• Electronegativity decreases as you move down a group.

• Electronegativity fluctuates as you move down a group.

How does the position of an element in the periodic table affect its chemical properties?

• It determines the element's atomic mass and size.

• It influences the element's reactivity, ionization energy, electronegativity, and other chemical properties.

• It has no effect on the element's properties.

• It only affects the element's physical state at room temperature.

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Define electronegativity.

• Electronegativity is the ability of an atom to attract electrons in a chemical bond.

• Electronegativity is the measure of an atom's size in a molecule.

• Electronegativity is the energy required to remove an electron from an atom.

• Electronegativity is the tendency of an atom to gain protons.

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What is the effect of increased nuclear charge on atomic size?

• Increased nuclear charge pulls electrons closer, resulting in a smaller atomic size.

• Increased nuclear charge has no effect on atomic size.

• Increased nuclear charge causes atomic size to increase due to electron repulsion.

• Increased nuclear charge leads to the formation of larger atomic orbitals.

Define ionization energy.

• The energy required to remove an electron from an atom in the gas phase.

• The energy released when an electron is added to an atom.

• The energy required to break a bond between two atoms.

• The energy needed to change an atom from solid to liquid.

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