Transition Metals Presentation

Transition metals

Fatimah and Zahraa

Intro to transition metals

• found in the middle lower block
• unreactive
• used widely in electronics, technology, building materials and some can be used to catalyse reactions
• found naturally in many biological systems like iron in haemoglobin and zinc in enzymes

StRUCTURE OF TRANSITION METALS

• Contains metallic bonding
• Positive metal ions surrounded by their outer electrons
• These electrons are delocalised and free to move throughout the metal structure
• Creates very strong electrostatic forces of attraction - electrons holding together the metallic lattice
• Very important to the physical and chemical properties that transition metals have

PHYSICAL PROPERTIES

• high melting points - electrostatic forces of attraction
• high densities - lattice structure
• malleable and ductile - 'sea' of delocalised electrons
• good conductors of heat and electricity - free electrons

variable charges (Mn can exist as a 2+,3+4+6+ and 7+ ion!)

CHEMICAL PROPERTIES

form coloured compounds e.g Fe2+ green Fe3+ is brown

Mostly unreactive/slower reactions compared to other metals e.g alkalis

common reactions of transitions metals include: NaOH, NH3, OH

adding hydroxide ions [Cr(H206)]3+ + 3OH- ⇌ [Cr(OH)3 (H2O)3] + 3H2O

VS

transition metals

Group 1 metals

• Highly reactive

• Mostly unreactive

• Low densites

• High densities

• Soft

• Hard, but malleable

• Form white compounds

• Form coloured compounds

• Fixed +1 charge

• Variable charges

QUIZ TIME

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