Ionic Compounds Ionic Compounds Ionic Compounds Ionic Compounds Ch.6 & 7.
Chemistry 2 Lesson 2.1 Ionic Compounds AQA Additional Science.
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Transcript of Chemistry 2 Lesson 2.1 Ionic Compounds AQA Additional Science.
Aims
Class work Structures and Properties
Ionic CompoundsLO’s• What are the properties of ionic
compounds?
Write it down!! Page 48© C Meyer
Chemistry Unit 2 Sections
Structures Structures and bonding and properties How
much? 2 of 7
© C Meyer
All• Know the main properties of ionic
compounds
Most/Some• Relate their properties to their
structure
Aims
• Metals (left side) lose electrons to get a full shell• Non metals (right side) gain electrons to get a full shell• + and - ions that form strongly attract each other
• What are ionic bonds? Use sodium chloride as an example
What have I learnt?
• What are ionic bonds? Use sodium chloride as an example (Na =11, Cl = 17)
What have I learnt?
m2
• What structure do ionic compounds have/what do they look like?
What have I learnt?
m1
+-+
-
- -
-+
+
+ -+-
+
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-+ +
+-+
-
- -
-+
++ -
+-
+
-
-+ +
+ -+-
+
-
-+ +
+-+
-
- -
-+
+
Lots ofionic bonds
+ and –attract
strongly
Background - water, water everywhere• What is the formula for water?• What does a molecule look like?
What are the properties of ionic compounds?
O
HH
O H
H
Covalent bondsm3
• You will do a series of experiments
• For each experiment write a conclusion/say why the ionic compound has that property using your knowledge of ionic bonding
What are the properties of ionic compounds?
1. Observation – look at the crystals under a hand lens. What is structure, is it solid, liquid or gas? Why?
2. Scratch test – Take a needle. Try to scratch the surface CARE. Is the surface hard or soft? Why?
3. Melting point – Place a spatula full of the crystals in a boiling tube. Heat in the blue flame CARE. Do they have high or low melting points? Why?
4. Solubility – Take a small beaker, half filled with water. Add 2 spatulas full of crystals. What happens? Why?
SAFETY 18 mins
5. Conductivity – Take a small beaker. Put a layer of crystals on the bottom. Dip in the electrodes, does the lamp light? Why? Now add water CARE - Chlorine. Does the lamp light? Why?
Tidy UP!!!
• Stack items tidily• Clean up bench/floor• Sit down when finished
• List the main properties of ionic compounds and explain why they have those properties
Homework
1. ObservationWhat are the properties of ionic compounds?
• Solid, crystals – due to strong ionic bond. Particles close and hard to break apart
2. Scratch test• Hard, scratch resistant – strong ionic
attractive bonds3. Melting point• High melting point. Did not melt (easily)
– strong ionic attractive bonds m3
What are the properties of ionic compounds?4. Solubility• Easily dissolves – Water is not neutral,
has a charge so can attract ions in lattice and pull them apart
m1
m1
What are the properties of ionic compounds?5. Conductivity• Solid does not conduct. When solution
conducts – in solution ions are free to move. They carry a charge so go to the opposite electrode.
• Ions would also conduct when at very high temperature and molten
What are the properties of ionic compounds?
The End