17A.4

Question 1

How do we apply the electron theory of repulsion

Answer 1

by ignoring the electrons in the 3d orbital of the transition metal as well as the overall charge of the complex and just counting the number of the bonding pair electrons and applying that the ligands want minimum repulsion between them

Question 2

when their is six bonding electron pairs what shape does the complex make (and angle bond)

Answer 2

octahedral with 90 angle bond

Question 3

when their is four bonding electron pairs what shape does the complex make (and angle bond)

Answer 3

tetrahedral with 109.5 angle bond

Question 4

when there is 2 bonding electron pairs what shape does the complex make (and angle bond)

Answer 4

linear with 180 bond angel

Question 5

what is six-fold coordination

Answer 5

complexes in which their are six ligands forming coordinate bonds with the transition metal ion

Question 6

why does complexes with Cl usually form only 4 coordinate bonds not more

Answer 6

because Cl is in period 3 so its much bigger than water, hydroxide, ammonia therefore their isn’t enough space for 6 ligands of Cl

Question 7

What are the most important examples of Octahedral complexes and there colour

Answer 7

any octahedral including Ammonia, water, and hydroxide also page (192)

Question 8

what is their to remember about OH, H2O and NH3 (n of lone electrons)

Answer 8

OH was 3 pairs of lone electrons, H2O has 2, NH3 has 1

Question 9

What are the important Tetra complexes to know about

Answer 9

any with Cl and why it doesn’t form Octa

Question 10

what is the only important linear complex that wee need to now about and why it forms like that

Answer 10

Tollens region (ammoniacal silver nitrate) we don’t need to exactly know why but we need to understand that Ag^+ ion is in period 5 so it behaves differently