Which of the following best describes the mechanism of electron transfer in ionic bonding?

A. Sharing of electrons between two atoms

B. Complete transfer of electrons from one atom to another

C. Partial transfer of electrons between atoms

D. No transfer or sharing of electrons

Why do atoms form ions?

A. To gain kinetic energy

B. To achieve a full outer electron shell

C. To become isotopes

D. To increase their atomic size

Which property is NOT associated with ionic compounds?

A. High electrical conductivity in molten state

B. Low melting and boiling points

C. Formation due to electron transfer

D. Strong electrostatic forces between ions

What is the primary reason for the high melting and boiling points of ionic compounds?

A. Covalent bonding

B. Weak van der Waals forces

C. Strong electrostatic forces between ions

D. Hydrogen bonding

Which of the following is NOT a characteristic of the crystal lattice structure of ionic compounds?

A. Organised arrangement of ions

B. High flexibility and malleability

C. Repetitive 3D pattern of ions

D. Maximises attractive forces and minimises repulsive forces

a) Describe the mechanism of electron transfer during the formation of an ionic bond. [2]

b) Explain how the octet rule relates to the stability of ions formed during ionic bonding. [2]

a) Given the properties of ionic compounds, explain why they generally have high melting and boiling points. [2]

b) Describe the arrangement of ions in a crystal lattice and its significance in ionic compounds. [2]

a) Using sodium chloride as an example, explain how the formation of cations and anions leads to the creation of an ionic compound. [2]

b) What is the significance of the sea of delocalised electrons in metallic bonding? [2]

a) Describe the difference between a cation and an anion. [1]

b) Using magnesium oxide as an example, explain the electron transfer that occurs during the formation of this ionic compound. [2]

c) Why do ionic compounds like magnesium oxide exhibit electrical conductivity when dissolved in water? [3]

a) What role does the octet rule play in the formation of ionic bonds? [2]

b) Explain the significance of electrostatic forces in maintaining the structure of ionic compounds. [2]

c) Why do ionic compounds typically have high boiling points compared to covalent compounds? [3]

How do cations differ from anions?

A. Cations are negatively charged; anions are positively charged

B. Cations are positively charged; anions are negatively charged

C. Cations and anions have the same charge but different sizes

D. Cations and anions are both neutral

Which of the following elements is most likely to form a cation?

A. Fluorine

B. Oxygen

C. Sodium

D. Nitrogen

In the context of ionic bonding, what does the octet rule state?

A. Atoms tend to gain, lose, or share electrons to have eight electrons in their outermost shell

B. Atoms always have eight electrons in their nucleus

C. Ionic compounds always contain eight different types of ions

D. Atoms bond with up to eight other atoms

Which of the following ionic compounds is expected to have the highest melting point?

A. NaCl

B. MgO

C. LiF

D. KBr

Why do ionic compounds conduct electricity in the molten state but not in the solid state?

A. Ions are free to move in the molten state

B. Electrons are free to move in the molten state

C. The crystal lattice breaks down in the molten state

D. Covalent bonds are formed in the molten state

a) How does the arrangement of ions in a crystal lattice contribute to the properties of ionic compounds? [3]

b) Define 'electrostatic forces' in the context of ionic bonding. [2]

c) Why might some ionic compounds be soluble in water while others are not? [2]

a) What is the significance of the sea of delocalised electrons in metals? [2]

b) How does metallic bonding differ from ionic bonding? [3]

c) Why are alloys, such as iron and steel, important in society? [2]

a) Describe the process by which sodium and chlorine atoms combine to form sodium chloride. [2]

b) How does the structure of an ionic compound differ from that of a molecular compound? [3]

c) Explain why ionic compounds are generally brittle. [2]

d) Given that ionic compounds have high melting and boiling points, how does this relate to their structure and bonding? [3]

a) What is meant by the term 'crystal lattice' in the context of ionic compounds? [2]

b) Why do ionic compounds conduct electricity when molten or dissolved in water but not in their solid state? [3]

c) How does the size of ions affect the strength of the ionic bond between them? [3]

d) Explain the significance of the octet rule in the context of ionic bonding. [2]

a) How does the charge of an ion relate to its position in the periodic table? [3]

b) Why are the properties of ionic compounds, such as high melting points, not exhibited by covalent compounds? [3]

c) Describe the significance of the sea of electrons in the context of metallic bonding. [2]

d) Given the importance of metals in society, explain why alloys are often preferred over pure metals for various applications. [2]