module 2 section 2 - electrons, bonding and structure

Question 1

Do you think it 1s possible for electrons in the first shell to swap with elections in the second shell-explain your answer (3)

Answer 1

• no
• as each electron shell has a different energy level
• amount of energy needed to transfer an electron from 1 electron shell to another is far too large

Question 2

What are main energy levels called (l)

Answer 2

Principle energy levels

Question 3

What is the number given to each energy level called (1)

Answer 3

Principle quantum number (n)

Question 4

What is the lowest energy level

Answer 4

N=1

Question 5

How many sublevels are in shell n= 1

Answer 5

1

Question 6

What type af sub-shell is present in n=1

Answer 6

1s

Question 7

How many electrons are found in the 1s subshell

Answer 7

2

Question 8

What is the maximum number of electrons in n= 1

Answer 8

2

Question 9

What sub-shells are present in n=2

Answer 9

-2s
- 2p

Question 10

How many electrons can be in the 2s subshell

Answer 10

2

Question 11

How many electrons can be held in the 2p subshell

Answer 11

6

Question 12

What is the maximum number of electrons in shell n=2

Answer 12

8

Question 13

What type af subshells are found in shell n= 3

Answer 13

. 3s
-3p
- 3d

Question 14

How many electrons can be held in 3s

Answer 14

2

Question 15

How many an electrons can be held in 3p

Answer 15

6

Question 16

How many elections can de held in 3d

Answer 16

10

Question 17

How many electrons can the shell n=3 hold

Answer 17

18

Question 18

What sub levels are present in the shell n=4

Answer 18

•4s
• 4p
.4d
-4f

Question 19

How many electrons can 4s hold

Answer 19

2

Question 20

How many electrons can 3p hold

Answer 20

6

Question 21

How many electrons can 4d hold

Answer 21

10

Question 22

How many electrons can 4f hold

Answer 22

14

Question 23

How many electrons can be held in the shell n=4

Answer 23

32

Question 24

How many electrons can an atomic orbital hold?

Answer 24

2

Question 25

Describe the shape of the s-atomic orbital

Answer 25

- Spherical shape

Question 26

Describe who the s-orbital increases un size

Answer 26

. When quantum number increases

Question 27

Describe the shape of the p-atomic orbital

Answer 27

Dumbbell shape

Question 28

Describe the trend of electronic configuration as you move along group 4 in the d-block (2)

Answer 28

- Number of electrons in 3d increases by 1 -Except chromium and copper are anomalous

Question 29

What is the electronic configuration of chromium

Answer 29

1s2. 2s2. 2p6. 3s2. 3p6. 4s1. 3d5.

Question 30

What is the electronic configuration of copper

Answer 30

1s2 2s2. 2p6. 3s2. 3p6. 4s1. 3d10

Question 31

Explain which orbitals d-block elements fill electrons., and remove electrons (2)

Answer 31

The 4s orbital

Question 32

Describe why electrons in an orbital must have opposite spins (2)

Answer 32

- To counteract repulsion - between negatively charged electrons

Question 33

Explain why the 4s orbital is always filed before the 3d orbital (1)

Answer 33

- because it has a lower energy level

Question 34

why do ionic compounds have giant ionic lattices (2)

Answer 34

- oppositely charged ions interact with eachother - in all directions

Question 35

describe the solubility of ionic compounds (2)

Answer 35

- soluble in polar solvents such as water - ions in ionic compounds can interact with polar water mlcl

Question 36

compare the solubility of an ionic compound containing Mg2+ and a different ionic compounds containing Na+ (3)

Answer 36

- ionic compounds containing ions with higher charges (eg Mg2+) = less soluble - ionic compounds w ions w low charge (eg Na+) = more soluble - because electrostatic forces of attraction between ions = too strong for water to break down ionic lattic

Question 37

explain how sodium chloride dissolved in water (4)

Answer 37

- before dissolving sodium and chloride ions held tightly together - due to string electrostatic forces of attraction - Na and all ions broken up by polar h20 mlcls - they interact with water mlcls

Question 38

describe the MP and BP of ionic compounds (3)

Answer 38

- high MP + BP - strong electrostatic forces of attraction between opp charged ions - a lot energy needed to overcome

Question 39

describe and explain the electrical conductivity of ionic compounds (5)

Answer 39

- poor as solid, good when dissolved in water or molten - poor as solid as ions fixed in position - so no mobile charge carriers - good when dissolved or melted and ionic lattice = broken - ions free to move as mobile charge carriers