5. Electrons and bonding

Question 1

What are shells?

Answer 1

A group of atomic orbitals with the same principal quantum number N.

Question 2

What are atomic orbitals?

Answer 2

A region around the nucleus that can hold up to two electrons, with opposite spins.

Question 3

What are the 4 types of orbitals?

Answer 3

1. s
2. p
3. d
4. f

Question 4

What is the shape of s-orbital?

Answer 4

Spherical

Question 5

What is the shape of p-orbital?

Answer 5

Dumb-bell shape

Question 6

How many orbitals make up a s-subshell?

Answer 6

1

Question 7

How many orbitals make up a p-subshell?

Answer 7

3

Question 8

How many orbitals make up a d-subshell?

Answer 8

5

Question 9

How many orbitals make up a f-subshell?

Answer 9

7

Question 10

How many orbitals are there in the 1st shell?

Answer 10

1

Question 11

How many orbitals are there in the 2nd shell?

Answer 11

4

Question 12

How many orbitals are there in the 3rd shell?

Answer 12

9

Question 13

How many orbitals are there in the 4th shell?

Answer 13

16

Question 14

How many electrons can fill a s-orbital?

Answer 14

2

Question 15

How many electrons can fill a p-orbital?

Answer 15

6

Question 16

How many electrons can fill a d-orbital?

Answer 16

10

Question 17

How many electrons can fill a f-orbital?

Answer 17

14

Question 18

How many electrons can fill the 1st shell?

Answer 18

2

Question 19

How many electrons can fill the 2nd shell?

Answer 19

8

Question 20

How many electrons can fill the 3rd shell?

Answer 20

18

Question 21

How many electrons can fill the 4th shell?

Answer 21

32

Question 22

What orbital is in the 1st shell?

Answer 22

s-orbital

Question 23

What orbitals are in the 2nd shell?

Answer 23

s- and p-orbital

Question 24

What orbitals are in the 3rd shell?

Answer 24

s-, p- and d- orbital

Question 25

What orbitals are in the 4th shell?

Answer 25

s-, p-, d- and f-orbital

Question 26

Rearrange the orbitals in terms of energy level.

Answer 26

1s > 2s > 2p > 3s > 3p> 4s > 3d > 4p > 4d > 4f

Question 27

What is ionic bonding?

Answer 27

Electrostatic attraction between positive and negative ions.

Question 28

What are giant ionic lattices?

Answer 28

A three-dimensional structure of oppositely charged ions that are strongly attracted in all directions, bonded together by strong ionic bonds.

Question 29

How are ionic compounds' melting point and boiling point? Why?

Answer 29

Ionic compounds have high melting point and boiling point, because they have strong electrostatic attractions between ions, which requires a lot of energy to overcome.

Question 30

How are ionic compounds' solubility?

Answer 30

Ionic compounds dissolve in polar solvents, eg. water. Polar molecules break down the lattice and surround each ion in solution.

Question 31

How are ionic compounds' electrical conductivity in solid state? Why?

Answer 31

Ionic compounds can't conduct electricity in solid state, because ions are fixed and can't move to carry electric charge.

Question 32

How are ionic compounds' electrical conductivity in liquid state? Why?

Answer 32

Ionic compounds can conduct electricity in liquid state, because ions can move freely and carry electric charge.

Question 33

How are ionic compounds' electrical conductivity in aqueous state? Why?

Answer 33

Ionic compounds can conduct electricity in aqueous state, because ions can move freely and carry electric charge.

Question 34

What is covalent bonding?

Answer 34

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

Question 35

What is dative covalent bonding?

Answer 35

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atom only.

Question 36

What is average bond enthalpy?

Answer 36

A measurement of covalent bond strength

Question 37

What does a larger value of average bond enthalpy suggest?

Answer 37

The larger the value of the average bond enthalpy, the stronger the covalent bond.

Question 38

How are covalent compounds' electrical conductivity? Why?

Answer 38

Covalent compounds can't conduct electricity in any state, because they don't have mobile electrons.

Question 39

How are simple covalent compounds' melting point and boiling point? Why?

Answer 39

Simple covalent compounds have low melting point and boiling point, because they have weak London forces between molecules, which are easy to overcome.

Question 40

How are giant covalent compounds' melting point and boiling point? Why?

Answer 40

Giant covalent compounds have high melting point and boiling point, because they have a lot of strong covalent bonds between molecules, which requires a lot of energy to overcome.