Chapter 5 - Electrons Bonding

Question 1

what are shells

Answer 1

energy levels
The shells are made up of atomic orbitals, which is a region around the nucleus that can hold up to 2 electrons, with opposite spins.

Question 2

What is a atomic orbital

Answer 2

Modelled to be a region in space where there is a high probability of finding an electron.

Question 3

s orbital

Answer 3

electron cloud is in the shape of a sphere

n= 1, 1 s orbital

Question 4

p orbital

Answer 4

electron cloud is the shape of a dumbell
n=2, 3 p orbital
The greater the shell number, the further the p-orbital if from the nucleus.

Question 5

D orbital

Answer 5

n=3, 5 d-orbital

Question 6

f orbital

Answer 6

n= 4, 7 f-orbital

Question 7

where is the highest energy electrons in the s-subshells

Answer 7

the first 2 groups

Question 8

where is the highest energy electrons in d-subshells

Answer 8

the transition metals

Question 9

where is the highest energy electrons in p-subshells

Answer 9

groups 3-8

Question 10

why is the 4s sub shell before the 3d

Answer 10

because it has slightly less energy than 3d.
However, when it is filled up, the 3d energy levels fall below it.
this means that it fills up before the 3d and also empties before the 3d

Question 11

What is the shorthand electron configuration

Answer 11

You use the last noble gases

useful for emphasising similarities in the outer shell’s electrons

Question 12

What is ionic bonding

Answer 12

the electrostatic attraction between positive and negative ions.

Question 13

Where does ionic bonding occur

Answer 13

It occurs between metal and non-metal ions

Question 14

What is the structure of ionic compounds

Answer 14

A giant ionic lattice.

Question 15

Properties of ionic bonds

Answer 15

High melting and boiling points
Soluble
Electrical conductivity

Question 16

High melting and boiling points of ionic compounds

Answer 16

All ionic compounds are solid at RT, mainly because the electrostatic forces of attraction are too strong, and high temperatures are needed to overcome them.
The melting points are higher for lattices containing ions with higher ionic charges.

Question 17

Solubility in ionic compounds

Answer 17

Many ionic compounds dissolve in polar solvents because the polar molecules break down the lattice and surround each ion in the solution.
However, this depends on the relative strengths of the attractions in the giant ionic lattice and the attractions between the water molecules and the ions.

Question 18

Electrical conductivity in ionic compounds

Answer 18

In solid state, ionic compounds don’t conduct electricity, but they do when melted or dissolved in water. This is because when they are a solid, the ions are in a fixed position in the giant ionic lattice and there are no mobile charge carriers.
As a liquid, the solid ionic lattice breaks down and the ions are now free to move as mobile charge carriers.

Question 19

Covalent Bonding

Answer 19

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms. It occurs between non-metallic elements and
polyatomic ions.

Question 20

The Covalent Bond

Answer 20

It is the overlap of atomic orbitals, each containing an electron to share.

Question 21

1 Difference between ionic and covalent bonding

Answer 21

Ionic attracts in all directions, but covalent attracts in only the shared pair of electron and the nuclei of the bonded atom.

Question 22

What is a triple covalent bond

Answer 22

The electrostatic attraction is between 3 shared pairs of electrons and the nuclei of the bonding atoms.

Question 23

A dative covalent bond

Answer 23

Or called a coordinate bond.

When the shared pair of electrons is supplied by one of the bonding atoms only. Originally, the pair was a lone pair.

Question 24

Average bond enthalpy

Answer 24

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

Question 25

What are the elements called around the dividing line

Answer 25

metalloids

Question 26

Metallic bonding

Answer 26

Each solid atom has donated its negative outer-shell electrons to a pool of electrons.

Question 27

What is metallic bonding

Answer 27

The electrostatic attraction between the cations and the delocalised electrons

Question 28

What are the properties of metals

Answer 28

Strong metallic bonding
High electrical conductivity
High melting and boiling points
Don’t dissolve either

Question 29

Giant covalent structures properties

Answer 29

Held by covalent bonds
High melting and boiling points
Insoluble (bonds too strong)
Non-conductors (except graphite and graphene)

Question 30

Trends across period 2 and 3

Answer 30

Melting points increase from G1 to G4.
Sharp decrease from G14 to G15
Melting points are even lower from G15 to G18.