M2 - Chapter 5

Question 1

Define orbital

Answer 1

an orbital is an area of space about the nucleus that can hold a maximum of two electrons with opposite spins

Question 2

Define shell

Answer 2

a number of orbitals with the same principal quantum number(n)

Question 3

Define subshell

Answer 3

all the orbitals of the same type within one shell

Question 4

What is electron configuration

Answer 4

arrangement of electrons in an atom

Question 5

How are electrons arranged around the nucleus

Answer 5

in principal energy levels or principal quantum shells

Question 6

The lower the principal quantum number,

Answer 6

the closer the shell is to the nucleus

Question 7

The first shell is

Answer 7

n=1

Closest to the nucleus

Question 8

The higher the principle quantum number…

Answer 8

the greater the energy of the shell + further away from the nucleus

Question 9

How many electrons can n=1 hold

Answer 9

2

Question 10

How many electrons can n=2 hold

Answer 10

Up to 8

Question 11

How many electrons can n=3 hold

Answer 11

Up to 18

Question 12

How many electrons can n=4 hold

Answer 12

Up to 32

Question 13

The principle quantum shells are split into…

Answer 13

Sub shells

Question 14

Names of the sub shells

Answer 14

S p and d

Question 15

Which elements have an f shell

Answer 15

Those with more then 57 electrons

Question 16

How does the energy increase in sub shells

Answer 16

o The energy of the electrons in the subshells increases in the order s < p < d

Question 17

What does it mean when it says the energy of the shells can overlap

Answer 17

4s has lower energy than 3d

Question 18

What do subshells contain

Answer 18

One or more orbitals

Question 19

Where can electrons be found

Answer 19

In the orbital not between them

Question 20

How many electrons can each orbital contain

Answer 20

Max 2

Question 21

How many orbitals in s subshell

Answer 21

one orbital (1 x 2 = total of 2 electrons)

Question 22

How many orbitals in p subshell

Answer 22

three orbitals ( 3 x 2 = total of 6 electrons)

Question 23

How many orbitals in d subshell

Answer 23

five orbitals (5 x 2 = total of 10 electrons)

Question 24

How many orbitals in f subshell

Answer 24

seven orbitals (7 x 2 = total of 14 electrons)

Question 25

Shape of s orbitals

Answer 25

Spherical

Question 26

Does the size increase in the s orbitals

Answer 26

Yes - • The size/radius of the s orbitals increases with increasing shell number o E.g. the s orbital of the third quantum shell (n = 3) is bigger than the s orbital of the first quantum shell (n = 1)

Question 27

Shape of p orbitals

Answer 27

dumbbell shape

Question 28

Does every shell have a p orbital

Answer 28

Yes - BUT NOT THE FIRST ONE n=1

Question 29

How many p orbitals in each shell

Answer 29

Three

Question 30

P orbitals occupy..

Answer 30

the x, y and z axes and point at right angles to each other, so are oriented perpendicular to one another

Question 31

Does the size of P orbitals increase

Answer 31

Yes…• The lobes of the p orbitals become larger and longer with increasing shell number

Question 32

Do all shells contain d orbitals

Answer 32

all from n=3

Question 33

How many d orbitals do they contain

Answer 33

5

Question 34

What is spin - pair repulsion

Answer 34

• Electrons with the same spin repel each other

Question 35

How to fill orbitals

Answer 35

electrons will occupy separate orbitals in the same subshell first to minimise this repulsion and have their spin in the same direction o They will then pair up, with a second electron being added to the first p orbital, with its spin in the opposite direction

Question 36

What is Hunds rule

Answer 36

electrons will occupy separate orbitals in the same subshell first to minimise this repulsion and have their spin in the same direction o They will then pair up, with a second electron being added to the first p orbital, with its spin in the opposite direction

Question 37

Example of Hunds rule

Answer 37

there are three electrons in a p subshell, one electron will go into each px, py and pz orbital

Question 38

Box notation for titanium

Answer 38

Question 39

What’s special a lot 4s

Answer 39

• The transition metals fill the 4s subshell before the 3d subshell, but they also lose electrons from the 4s first rather than from the 3d subshell

Question 40

Different blocks on the periodic table

Answer 40

Question 41

Exceptions to periodic table

Answer 41

Chromium and copper

Question 42

Electronic configuration of chromium

Answer 42

o Cr is [Ar] 3d5 4s1 not [Ar] 3d4 4s2

Question 43

Electron configuration of Cu

Answer 43

o Cu is [Ar] 3d10 4s1 not [Ar] 3d9 4s2

Question 44

Why are copper and chromium like this

Answer 44

because the [Ar] 3d5 4s1 and [Ar] 3d10 4s1 configurations are energetically favourable • By promoting an electron from 4s to 3d, these atoms achieve a half full or full d-subshell, respectively

Question 45

Answer 45

Question 46

Answer 46

Question 47

Answer 47

Question 48

Answer 48

A