Exploring Periodic Table Trends: Electronegativity, Ionization Energy, and Atomic Radius

What is the primary focus of periodic trends in chemistry?

• To help make decisions with bonding and chemical reactions

• To classify elements by their state of matter

• To understand the color of elements

• To determine the weight of elements

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Which periodic trend is defined as the energy released when adding an electron to an atom?

• Electron affinity

• Atomic radii

• Electronegativity

• Ionization energy

How is atomic radii measured?

• By the distance between the nucleus and the outermost electron

• By the distance between the protons in the nucleus

• By the distance between the nuclei of two atoms of the same element, divided by two

• By the distance between the outermost electrons

What happens to atomic radii as you move from left to right across a period?

• It fluctuates

• It remains the same

• It increases

• It decreases

What is ionization energy?

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

• The energy required to add an electron to an atom

• The energy released when an atom forms a bond

• The energy required to remove an electron from an atom

Which elements tend to have low ionization energies?

• Halogens

• Metals

• Noble gases

• Nonmetals

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What does electronegativity measure?

• An atom's ability to release energy

• An atom's ability to form bonds

• An atom's ability to attract electrons

• An atom's ability to lose electrons

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Which element has the highest electronegativity?

• Neon

• Oxygen

• Chlorine

• Fluorine

On the Linus Pauling scale, what is the electronegativity of noble gases?

• Four

• Zero

• One

• Two

Which element has the lowest electronegativity, excluding noble gases?

• Sodium

• Francium

• Magnesium

• Calcium