Understanding Periodic Trends

What determines the structure of the periodic table?

• The number of neutrons in an atom

• The density of elements

• The electron configurations of elements

• The atomic mass of elements

How is the atomic radius conventionally measured?

• By the distance from the nucleus to the outermost electron

• By the diameter of the atom

• By half the distance between the nuclei of two bonded identical atoms

• By the volume of the atom

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

• It decreases

• It remains constant

• It increases

• It fluctuates randomly

Why does the atomic radius decrease across a period?

• Because the atomic mass decreases

• Because the effective nuclear charge increases

• Because protons are lost

• Because electrons are lost

What is ionization energy?

• The energy required to add an electron to an atom

• The energy required to remove an electron from an atom

• The energy released when an atom forms a bond

• The energy absorbed when an atom is heated

How does ionization energy change as you move across a period?

• It increases

• It remains constant

• It decreases

• It fluctuates randomly

What is electron affinity?

• The energy released when an atom is ionized

• The energy required to break a chemical bond

• The energy change when an electron is removed from a neutral atom

• The energy change when an electron is added to a neutral atom

Which element is likely to have a high electron affinity?

• Sodium

• Helium

• Fluorine

• Argon

Why do noble gases generally not follow the electron affinity trend?

• They are highly reactive

• They have a low atomic number

• They have a high atomic mass

• They have a full outer shell of electrons

What is the significance of electronegativity in chemistry?

• It determines the atomic mass of an element

• It influences the formation of chemical bonds

• It affects the color of an element

• It determines the density of an element