Atomic size increases as you move down a group in the periodic table.

Atomic size remains constant as you move down a group in the periodic table.

Atomic size decreases as you move down a group in the periodic table.

Atomic size fluctuates randomly as you move down a group in the periodic table.

Lithium (Li)

Neon (Ne)

Beryllium (Be)

Oxygen (O)

Cations are twice the size of their parent atoms.

Cations have the same size as their parent atoms.

Cations are smaller than their parent atoms.

Cations are larger than their parent atoms.

Anions are smaller than their parent atoms.

Anions are only slightly larger than their parent atoms.

Anions are larger than their parent atoms.

Anions have the same size as their parent atoms.

Na+

Mg2+

K+

Ca2+

Electronegativity increases across a period.

Electronegativity fluctuates randomly across a period.

Electronegativity remains constant across a period.

Electronegativity decreases across a period.

Nitrogen

Carbon

Oxygen

Fluorine

Electronegativity remains constant as you move down a group.

Electronegativity fluctuates randomly as you move down a group.

Electronegativity decreases as you move down a group.

Electronegativity increases as you move down a group.

As atomic size decreases, electronegativity generally increases.

As atomic size increases, electronegativity generally decreases.

Atomic size has no effect on electronegativity.

Larger atoms have higher electronegativity.

First ionisation energy remains constant across a period.

First ionisation energy increases across a period.

First ionisation energy decreases across a period.

First ionisation energy fluctuates across a period.

First ionisation energy remains constant as you move down a group.

First ionisation energy fluctuates randomly as you move down a group.

First ionisation energy decreases as you move down a group.

First ionisation energy increases as you move down a group.

Magnesium (Mg)

Argon (Ar)

Chlorine (Cl)

Sodium (Na)

Atomic size, nuclear charge, electron shielding, and subshell type.

Chemical reactivity and phase

Temperature and pressure

Atomic weight and density

Effective nuclear charge has no effect on atomic size.

Effective nuclear charge decreases atomic size.

Effective nuclear charge only affects ionization energy.

Effective nuclear charge increases atomic size.

Electron shielding only affects the mass of the atom.

Electron shielding has no effect on atomic size.

Electron shielding decreases atomic size by increasing the effective nuclear charge.

Electron shielding increases atomic size by reducing the effective nuclear charge on outer electrons.

The presence of d and f orbitals generally leads to smaller cation sizes and larger anion sizes due to increased electron shielding and effective nuclear charge.

d and f orbitals have no effect on ionic size

Cations are larger due to d and f orbitals

Anions become smaller with d and f orbitals present

Larger atomic radius results in higher ionization energy.

Smaller atomic radius has no effect on ionization energy.

Larger atomic radius results in lower ionization energy.

Atomic radius does not influence ionization energy at all.

Larger atoms have lower electronegativity due to increased distance from the nucleus.

Larger atoms have higher electronegativity because they can attract electrons more effectively.

Smaller atoms have higher electronegativity due to decreased distance from the nucleus.

Electronegativity is unaffected by atomic size and remains constant across all elements.

Periodic trends are significant as they allow prediction of chemical behavior and reactivity of elements.

Periodic trends are only relevant for metals.

Periodic trends are solely based on atomic mass.

Periodic trends have no impact on element bonding.