Ionic Bonding and Ionic CompoundsAQA GCSE Chemistry: Flashcards

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Define ionic bonding.

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Define ionic bonding.: Ionic bonding is the electrostatic attraction between oppositely charged ions. It forms when electrons are transferred from a metal atom to a non-metal atom, creating positive ions (cations) and negative ions (anions) that attract each other.
What happens to electrons when ionic bonding occurs?: Electrons are transferred from the metal atom to the non-metal atom. The metal loses electrons to form a positive ion (cation), and the non-metal gains electrons to form a negative ion (anion).
Explain how a metal atom forms a positive ion (cation).: A metal atom loses electrons from its outer shell. This loss of negatively charged electrons means the atom has more protons than electrons, resulting in a positive charge.
Explain how a non-metal atom forms a negative ion (anion).: A non-metal atom gains electrons into its outer shell. This gain of negatively charged electrons means the atom has more electrons than protons, resulting in a negative charge.
State the charges of the following common ions: Na⁺, K⁺, Ca²⁺, Mg²⁺, Al³⁺.: Na⁺ is +1 (sodium), K⁺ is +1 (potassium), Ca²⁺ is +2 (calcium), Mg²⁺ is +2 (magnesium), Al³⁺ is +3 (aluminium).
State the charges of the following common ions: Cl⁻ and O²⁻.: Cl⁻ is −1 (chloride), O²⁻ is −2 (oxide).
What is a dot-and-cross diagram used for in ionic bonding?: A dot-and-cross diagram represents the formation of an ionic compound by showing the outer electrons only. Dots represent electrons from one atom and crosses represent electrons from the other atom, showing the transfer of electrons between the metal and non-metal.
Describe the structure of a giant ionic lattice.: A giant ionic lattice is a regular, repeating three-dimensional arrangement of oppositely charged ions. The ions are held together by strong electrostatic forces of attraction acting in all directions between the positive and negative ions.
Why do ionic compounds have high melting and boiling points?: Ionic compounds have high melting and boiling points because there are very strong electrostatic forces of attraction between the oppositely charged ions in the lattice. A lot of energy is required to break these strong forces and overcome the structure.
Why does an ionic compound not conduct electricity when solid?: When solid, the ions are held in fixed positions in the lattice structure and cannot move. Since electrical conduction requires the movement of charged particles (ions), a solid ionic compound cannot conduct electricity.
Why does an ionic compound conduct electricity when molten?: When molten (melted), the lattice structure breaks down and the ions are free to move. These mobile ions can carry electrical charge through the molten compound, allowing it to conduct electricity.
Why does an ionic compound conduct electricity when dissolved in water?: When dissolved in water, the ionic lattice structure breaks apart and the ions are released and free to move through the solution. These mobile ions can carry electrical charge, allowing the solution to conduct electricity.
Name the type of force that holds ions together in an ionic compound.: Electrostatic force (or electrostatic attraction). This is the force of attraction between opposite electrical charges.
What is the difference between a cation and an anion?: A cation is a positively charged ion formed when a metal atom loses electrons. An anion is a negatively charged ion formed when a non-metal atom gains electrons.
Explain why transition metals can form ions with different charges.: Transition metals can lose electrons from both their outer shell and their penultimate d-shell, allowing them to form ions with variable charges (e.g. Fe²⁺ and Fe³⁺). This is unlike main group metals which typically form ions with a single fixed charge.