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Chemistry Module 4 > Ionic Bonding > Flashcards

Flashcards in Ionic Bonding Deck (10):

Compare the electrical conductivity of sodium chloride in solid, molten liquid and solution

Solid - not conduct electricity
Molten liquid - conduct electricity
Solution - conduct electricity


Compare the melting points of sodium chloride and magnesium oxide

Sodium chloride - high melting point
Magnesium oxide - even higher melting point


What does it mean if an atom has an outer shell of 8 electrons

They have a stable electronic structure


Explain how and why metal form from positive ions

Metal atoms lose the electron, or electrons, in their highest energy level and become positively charged ions


Explain and why non-metal atoms form negative ions

Non-metal atoms gain an electron, or electrons, from another atom to become negatively charged ions


What happens in ionic bonding?

A metal and non-metal combine by transferring electrons to form positive ins and negative ions which then attract one another


Describe the structure of sodium chloride or magnesium oxide

A giant ionic lattice in which positive ions are strongly attracted to negative ions


Explain, in terms of structure and bonding, some of the physical properties of sodium chloride

- high melting points
- electrical conductivity of solid, molten liquid and solution


Explain, in terms of structure and bonding, why the melting point of sodium chloride is lower than that of magnesium oxide

Because it has weaker ionic bonds, which need less heat energy to overcome


What is an ion?

A charged atom or group of atoms