Ionic Bonding Flashcards Preview

Chemistry Module 4 > Ionic Bonding > Flashcards

Flashcards in Ionic Bonding Deck (10)
Loading flashcards...
1
Q

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

A

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

2
Q

Compare the melting points of sodium chloride and magnesium oxide

A

Sodium chloride - high melting point

Magnesium oxide - even higher melting point

3
Q

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

A

They have a stable electronic structure

4
Q

Explain how and why metal form from positive ions

A

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

5
Q

Explain and why non-metal atoms form negative ions

A

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

6
Q

What happens in ionic bonding?

A

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

7
Q

Describe the structure of sodium chloride or magnesium oxide

A

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

8
Q

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

A
  • high melting points

- electrical conductivity of solid, molten liquid and solution

9
Q

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

A

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

10
Q

What is an ion?

A

A charged atom or group of atoms