Complete the table for atom X and ions Y³⁻ and Z²⁺.

• Atom X:
  • Mass number = 23
  • Protons (A) = Electrons = 11 (for a neutral atom)
  • Neutrons (B) = Mass number - Protons = 23 - 11 = 12
• Ion Y³⁻:
  • Mass number = 14
  • Neutrons = 7
  • Protons (C) = Mass number - Neutrons = 14 - 7 = 7
  • Electrons (D) = Protons + charge magnitude = 7 + 3 = 10
• Ion Z²⁺:
  • Protons = 12
  • Neutrons = 12
  • Mass number (E) = Protons + Neutrons = 12 + 12 = 24
  • Electrons (F) = Protons - charge magnitude = 12 - 2 = 10

The completed values are:

• A = $\boxed{11}$
• B = $\boxed{12}$
• C = $\boxed{7}$
• D = $\boxed{10}$
• E = $\boxed{24}$
• F = $\boxed{10}$

• A cation is a positively charged ion. From the table, $Z^{2+}$ is a cation.

• An anion is a negatively charged ion. From the table, $Y^{3-}$ is an anion.

• Cation: $\boxed{Z^{2+}}$

• Anion: $\boxed{Y^{3-}}$

• To form a neutral compound, the charges must balance.

  • $Z^{2+}$ has a charge of +2.
  • $Y^{3-}$ has a charge of -3.

• The least common multiple of 2 and 3 is 6.

  • We need three $Z^{2+}$ ions ($3 \times +2 = +6$).
  • We need two $Y^{3-}$ ions ($2 \times -3 = -6$).

• The formula of the compound is $Z_3Y_2$.

• Since the compound is formed between a metal ion ($Z^{2+}$) and a non-metal ion ($Y^{3-}$), the bond type is ionic.

• Formula of the compound: $\boxed{Z_3Y_2}$

• Bond type: $\boxed{\text{Ionic bond}}$