Chapter 5: Electrons and Bonding

Question 1

What are shells regarded as?

Answer 1

energy levels

Question 2

What is the energy level called and made up of ?

Answer 2

The principal quantum number (n)
atomic orbitals

Question 3

How many electrons can fill the first energy level?

Answer 3

2

Question 4

How many electrons can fill the second energy level?

Answer 4

8

Question 5

How many electrons can fill the third energy level?

Answer 5

18

Question 6

How many electrons can fill the fourth energy level?

Answer 6

32

Question 7

What is an atomic orbital?

Answer 7

a region in space where there’s a higher probability of finding an electron and it contains a maximum of two electrons with opposite spins

Question 8

Name the types of orbitals in order

Answer 8

s orbitals
p orbitals
d orbitals
f orbitals

Question 9

What is the shape of an s orbital?

Answer 9

Spherical

Question 10

What is the shape of a p orbital?

Answer 10

dumbbell

Question 11

How many sub shells make up s orbital?

Answer 11

one

Question 12

How many electrons can fill the sub shells in s orbital?

Answer 12

2

Question 13

How many sub shells make up p orbital?

Answer 13

3

Question 14

How many sub shells make up d orbital?

Answer 14

5

Question 15

How many electrons can fill the sub shells in p orbital?

Answer 15

6

Question 16

How many electrons can fill the sub shells in d orbital?

Answer 16

10

Question 17

What are the subshells for orbitals in energy level 1?

Answer 17

1s

Question 18

What are the subshells for orbitals in energy level 2?

Answer 18

2s + 2p

Question 19

What are the subshells for orbitals in energy level 3?

Answer 19

3s + 3p + 3d

Question 20

What are the subshells for orbitals in energy level 4?

Answer 20

4s + 4p + 4d + 4f

Question 21

What is the order of filling shells in n=2?

Answer 21

2s then 2p

Question 22

What is the order of filling shells in n=3?

Answer 22

3s then 3p then 3d

Question 23

What is the order of filling shells in n=4?

Answer 23

3p then 4s then 3d

Question 24

How do you fill orbitals with the same subshell?

Answer 24

fill each orbital of a p sub shell with one electron before pairing

Question 25

How is an electron spin shown on 'Electron in box' model?

Answer 25

an arrow up or down

Question 26

Why must electrons have opposite spins?

Answer 26

to counteract the repulsion between the negative charges of the electrons

Question 27

Show the electronic configuration of Z=36 (Krypton)

Answer 27

1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

Question 28

What is ionic bonding?

Answer 28

The electrostatic attraction between positive and negative ions

Question 29

What is the structure of ionic compounds?

Answer 29

Giant ionic lattice due to oppositely charged ions strongly attracted in all directions

Question 30

Why do ionic compounds have high melting and boiling points?

Answer 30

high temperatures are needed to provide the large quantity of energy to overcome the strong electrostatic attraction between the ions.

Question 31

Why do ionic substances dissolve in water?

Answer 31

because water is polar and stabilises the separated ions by surrounding the ions

Question 32

Why do ionic substances conduct electricity when aqueous?

Answer 32

ions are free to move and conduct

Question 33

Why don't ionic substances conduct electricity when solid?

Answer 33

ions are held strongly in a lattice

Question 34

What does 1st Ionisation energy mean?

Answer 34

The energy required to remove one mole of electrons from one mole of gaseous atoms X(g) ---> X^+(g) + e

Question 35

What does electron affinity mean?

Answer 35

The energy when one mole of gaseous atoms acquires one mole of electrons to form one mole of gaseous negative ions

Question 36

What is a covalent bond?

Answer 36

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Question 37

What is a dative/coordinate covalent bond?

Answer 37

When the shared pair of electrons has been supplied by one of the bonding atoms only

Question 38

What does average bond enthalpy mean?

Answer 38

a measurement of covalent bond strength

Question 39

What are the three most electronegative elements?

Answer 39

F, N, O

Question 40

What is an oxidising agent?

Answer 40

an element that takes the electrons from the element being oxidised

Question 41

Where is the s, p and d block on the periodic table?

Answer 41

s block = left two groups p block = right six groups d block = centre groups

Question 42

Why would Na2S have a higher melting temperature than NaCl

Answer 42

Na2S = sulphur has 2- NaCl = chlorine has 1- Na2S has stronger ionic bonds due to the higher charge therefore more energy is needed to overcome bonds