Transition Metals
Content Review:
ChemEd
BBC Bitesize
Chemical Elements
Mission 1: Transitioning...
Mission Objectives. You should be able to:
1. Explain why transition metals can have multiple oxidation states.
2. Describe the properties of transition metals.
3. Write and name ionic formulas that contain transition metals.
4. Explain why some ionic compounds are colored.
Watch the below video. Stop at 3:10.
ChemEd
BBC Bitesize
Chemical Elements
Mission 1: Transitioning...
Mission Objectives. You should be able to:
1. Explain why transition metals can have multiple oxidation states.
2. Describe the properties of transition metals.
3. Write and name ionic formulas that contain transition metals.
4. Explain why some ionic compounds are colored.
Watch the below video. Stop at 3:10.
Image courtesy of derekcarrsavvychemist.
When you look at orbital diagrams of transition metals (we are focusing on period 4 d-block), you will notice that mostly all of them will form a cation with a 2+ charge. This is due to the loss of valence electrons in the 4s orbital. Once those electrons are stripped, other electrons in the 3d orbital can also be lost. This is why certain metals can have multiple oxidation states.
It's important to know the oxidation states of transition metals because when you are identifying ionic compounds, you must specify which state is represented in the compound. For example, copper has two oxidation states: +2 and +3. If you combine copper with the chloride ion, it becomes copper chloride...but which one? The compounds do not behave the same way due to the extra lost electron. The correct way to identify the compound would be:
copper (II) chloride (+2 ox state)
copper (III) chloride (+3 ox state)
Tyler DeWitt goes into detail. Watch.
When you look at orbital diagrams of transition metals (we are focusing on period 4 d-block), you will notice that mostly all of them will form a cation with a 2+ charge. This is due to the loss of valence electrons in the 4s orbital. Once those electrons are stripped, other electrons in the 3d orbital can also be lost. This is why certain metals can have multiple oxidation states.
It's important to know the oxidation states of transition metals because when you are identifying ionic compounds, you must specify which state is represented in the compound. For example, copper has two oxidation states: +2 and +3. If you combine copper with the chloride ion, it becomes copper chloride...but which one? The compounds do not behave the same way due to the extra lost electron. The correct way to identify the compound would be:
copper (II) chloride (+2 ox state)
copper (III) chloride (+3 ox state)
Tyler DeWitt goes into detail. Watch.
Some transition metal compounds will have certain colors. A few weeks ago, you guys investigated the flame test, where you viewed the flames of different halides. Those colors are due to the number of electrons in the d valence shells. The colors come from the transition of electrons from the lower energy d-orbitals to the higher energy d-orbitals.