Periodic Table Trends Exploration

Which of the following trends increases as you move up and to the right on the periodic table?

• Atomic radius

• Metallic character

• Ionization energy

• None of the above

What does Z effective represent?

• The number of valence electrons

• The effective nuclear charge experienced by valence electrons

• The total number of electrons in an atom

• The number of protons in an atom

How do you calculate Z effective?

• Subtract the number of protons from the atomic number

• Subtract the number of shielding electrons from the atomic number

• Add the number of protons to the number of valence electrons

• Add the number of shielding electrons to the atomic number

What is the significance of Coulomb's Law in understanding atomic structure?

• It describes the forces between two point charges

• It explains the behavior of gases

• It determines the mass of an atom

• It calculates the speed of light

In Coulomb's Law, what does Q1 represent when applied to atoms?

• The charge of the nucleus

• The charge of a valence electron

• The atomic number

• The number of protons

Why does ionization energy increase as you move up and to the right on the periodic table?

• Because the Z effective decreases

• Because the number of valence electrons decreases

• Because the atomic radius increases

• Because the force between the nucleus and valence electrons increases

What happens to the atomic radius as you move down a group in the periodic table?

• It remains the same

• It increases

• It decreases

• It fluctuates

Which trend increases as you move down and to the left on the periodic table?

• Ionization energy

• Electron affinity

• Electronegativity

• Metallic character

Why does metallic character increase as you move down and to the left on the periodic table?

• Because the atomic radius decreases

• Because the Z effective increases

• Because the force between the nucleus and valence electrons decreases

• Because the number of valence electrons increases

What is the relationship between atomic radius and the force experienced by valence electrons?

• Force is only dependent on Z effective

• Radius does not affect the force

• Smaller radius results in greater force

• Larger radius results in greater force