Electronegativity, Ionization Energy, Atomic Radius Quiz Study

What is electronegativity?

• How badly an atom wants to take an electron from another atom.

• How large an atom is.

• How easy it is to remove an electron.

• How easy it is to move protons around.

Answer explanation

Electronegativity is how badly an atom wants an electron from another atom.

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What is ionization energy?

• How badly an atom wants to take an electron from another atom.

• How large an atom is.

• How easy it is to remove an electron.

• How easy it is to move protons around.

Answer explanation

Ionization energy is how easy it is to pull an electron off of an atom. It is very easy to pull electrons off of metals, and difficult to pull electrons off of nonmetals.

What is atomic radius?

• How badly an atom wants to take an electron from another atom.

• How large an atom is.

• How easy it is to remove an electron.

• How easy it is to move protons around.

Answer explanation

The atomic radius is how big an atom is.

The higher the period, the larger the atom is because you add rings to the atom. Period 3 elements have 3 rings--Period 4 elements have 4 rings.

Metals are bigger than nonmetals because nonmetal's nucleus holds electrons tighter by pulling the rings in towards the center.

Ionization energy __________ as you go across a period

• stays the same

• decreases

• increases

Answer explanation

Ionization energy is how easy it is to take an electron off of an atom. It increases as you move left to right across a period. This is because the periodic table goes from metals to nonmetals as you go from left to right. Metals have low ionization energy because they want to give away electrons. Nonmetals do not want to give away electrons so their ionization is very high.

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Ionization energy __________ as you go down a group.

• stays the same

• decreases

• increases

Answer explanation

As you move down a group, tre are more rings in the atom. These rings hold electrons further from the nucleus so it is easier to remove because they are not held as tightly.

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Select ALL (2) that explain the ionization energy trend within groups going top to bottom.

• electrons are closer to the nucleus

• their is a weak pull between electrons from the nucleus, making them easily moveable

• feel more of a pull from nucleus, making them harder to move

• electrons are further from the nucleus

Select ALL (2) that explain the ionization energy trend within periods going left to right

• electrons are closer to the nucleus

• their is a weak pull between electrons from the nucleus, making them easily moveable

• feel more of a pull from nucleus, making them harder to move

• electrons are further from the nucleus

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Which element has the greater ionization energy?

• Magnesium (Mg)

• Phosphorus (P)

Answer explanation

Phosphorous is on the right side of the periodic table and is a nonmetal. It does not want to give away any electrons because nonmetals want to TAKE away electrons. Ionization energy goes from low to high as you move from left to right across a period.

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Which element has the greater ionization energy?

• Iodine (I)

• Chlorine (Cl)

Answer explanation

Chlorine is higher up than Iodine on the periodic table. Chlorine has less electrons than Iodine. Because of this, it is more difficult to remove the electron.

As you go down a group, ionization energy goes from high low.

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Which of the following sequences corresponds to a correct trend in ionization energy?

• Cl > S > P > Al

• Sr > Ca > Mg > Be

• Rb > K > Na > Li

• Rb > Sr > I > Xe

Answer explanation

Cl, S, P, Al are all in the same period. Chlorine is on the right most side, making it the most non-metal--therefore its ionization energy is the highest. As you move left from Chlorine, the ionization energy gets progressively lower.

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