Periodic Table Trends Exploration

The video tutorial covers periodic table trends, focusing on atomic radius, electronegativity, and ionization energy. It explains how these properties change across periods and down groups. Atomic radius decreases across a period and increases down a group due to changes in nuclear charge and energy levels. Electronegativity increases across a period and decreases down a group, with fluorine being the most electronegative element. Ionization energy increases across a period and decreases down a group, influenced by the atom's proximity to a full valence shell and electron shielding.

What are the three periodic table trends discussed in this lesson?

• Atomic radius, atomic mass, and ionization energy

• Atomic mass, electronegativity, and ionization energy

• Electronegativity, atomic mass, and reactivity

• Atomic radius, electronegativity, and ionization energy

How is atomic radius defined?

• The distance between the nuclei of two bonded atoms

• Half the distance between the nuclei of two bonded atoms

• The distance from the nucleus to the outermost electron

• The distance between two electrons in an atom

What happens to the atomic radius as you move across a period?

• It remains the same

• It increases

• It decreases

• It fluctuates

Why does the atomic radius increase down a group?

• Because the number of protons increases

• Because the number of energy shells increases

• Because the number of electrons decreases

• Because the number of neutrons increases

What does electronegativity refer to?

• The ability of an atom to repel electrons

• The ability of an atom to lose electrons

• The ability of an atom to attract electrons

• The ability of an atom to share electrons

Which element has the highest electronegativity?

• Fluorine

• Oxygen

• Neon

• Chlorine

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What happens to electronegativity as you move down a group?

• It increases

• It decreases

• It fluctuates

• It remains the same

What does ionization energy refer to?

• The energy required to share an electron with another atom

• The energy required to remove an electron from an atom

• The energy required to add an electron to an atom

• The energy required to repel an electron from an atom

Why does ionization energy increase across a period?

• Because atoms are gaining more neutrons

• Because atoms are losing electrons

• Because atoms are gaining more protons

• Because atoms are getting closer to having a full valence shell

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What is electron shielding?

• When protons shield the electrons from the full attraction to the nucleus

• When valence electrons shield the inner electrons from the full attraction to the nucleus

• When inner electrons shield the valence electrons from the full attraction to the nucleus

• When neutrons shield the electrons from the full attraction to the nucleus