Transition metal general properties

Question 1

where are they found

Answer 1

between group 2 and 3 in the d block

Question 2

where are the outer electrons

Answer 2

in the d orbital

Question 3

why do we fill the 4s orbital before the 3d

Answer 3

the 4s orbital is closer to the nucleas so it fills before the 3d orbital

Question 4

what are the exception

Answer 4

chromium and copper

Question 5

what I the structure like in chromium

Answer 5

3d and 4s both contain one elctron each whihcmake the complex more stable

Question 6

what is the structure of copper like

Answer 6

the 3d orbital is and the 4d orbital contains one electron

Question 7

how do we form ion

Answer 7

the 4d orbital are emptied first

Question 8

what are the positions of the 3d and 4s like

Answer 8

they are very close together

Question 9

what happens when energy is supplied

Answer 9

the energy supplied causes the energy level to shift around to expected order as a result of the bombardment of electrons

Question 10

why is scandium/ zinc transition metal

Answer 10

when we remove an electron it has a completely empty d orbital
when we remove an electron it has a completely full d orbital

Question 11

therefore a transition metal has

Answer 11

an incomplete d orbital and they cannot form ions with incomplete d orbitals

Question 12

what are the main characteristics of transition metals

Answer 12

they form colored ions, they can act as catalyst they have variable oxidation states and form complexed

Question 13

what is the most common oxidation state and why

Answer 13

oxidation STATE OF PLUS TWO AS USUALLY THE 4S ORBITAL EMPTIES FIRST WHICH has two electrons in oouter shell

Question 14

why do they form variable oxidation state

Answer 14

as the orbitals are very close together in energy levels so electron can be removed easily

Question 15

what is a complex ion

Answer 15

a central metal ion surrounded by coordinately bonded ligands

Question 16

what is a ligand

Answer 16

a molecule or an ion with a lone pair of electrons which donates to form a coordinate bond

Question 17

what is a monodentate ligand and example

Answer 17

have one atom that can donate a lone pair of electron to form one coordinate bond h20 cl

Question 18

what is bidentate ligand

Answer 18

two atoms each donating a lone pair of electrons to form two coordinate bonds ehandioate ions

Question 19

what are multidentate ligands

Answer 19

several atoms donating a lone pair of electrons to form many coordinate bonds EDTA

Question 20

how to calculate the oxidation state of the metal ions

Answer 20

THE charge of the complex- the charge of the ligands

Question 21

how NOT ict the shape of a complex ions

Answer 21

the electron repulsion cannot be used as there is too many electron in the d orbital to estimate angles

Question 22

so what does the shape depend on

Answer 22

the size of the ligand attached and the number of coordinate bonds

Question 23

what metal ions can form octahedral complexes

Answer 23

cu/fe/co

Question 24

what are the structure of octahedral complexes

Answer 24

form 6 coordinate bonds with water/ammonia as they are small enough to surround central metal atom

Question 25

what angle do they form

Answer 25

90 in the square planar and 180 elsewhere

Question 26

what are the characteristic of the tetrahedral

Answer 26

contain 4 coordinate bonds, with ligands such as cl- as they are too large to form 6 coordinate bonds

Question 27

what is bond angle in tetrahedral

Answer 27

109.5

Question 28

what metal ions form square planar

Answer 28

ni or platinum

Question 29

what are the characteristic of these complexes

Answer 29

form 4 coordinate bonds usually with bondoentate ligands, bond angle 90

Question 30

what are linear complexes

Answer 30

formed using silver and coordination number of 2 and 180 bond angle