Atomic structure oxidation number and and redox

Question 1

Recall the number of electrons inhabiting the first 4 shells.

Answer 1

1 - 2
2- 8
3- 18
4- 32

Question 2

Define orbital.

Answer 2

A region around the nucleus that can hold up to 2 electrons with opposite spins.

Question 3

What is the shape of an S orbital?

Answer 3

Sphere

Question 4

What is the shape of a P orbital?

Answer 4

Dumb-bell

Question 5

How many orbitals make up an S-subshell?

Answer 5

One orbital

Question 6

How many orbitals make up a P-subshell?

Answer 6

Three orbitals at right angles to one another.

Question 7

How many orbitals make up a D-subshell?

Answer 7

Five orbitals

Question 8

How many electrons can fill up an S subshell?

Answer 8

2

Question 9

How many electrons can fill up a P subshell?

Answer 9

6

Question 10

How many electrons can fill up a D subshell?

Answer 10

10

Question 11

Why is subshell 4s filled first?

Answer 11

The 3D subshell si at a higher energy level than the 4s sub-shell.

Question 12

Write the order of subshells in the electron configuration.

Answer 12

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

Question 13

Complete the sentence…
Electrons fill orbitals…

And why does this happen?

Answer 13

Fill orbitals with the same energy singly before pairing.

This happens to prevent any repulsion between paired electrons.

Question 14

What do roman numerals show in a compound name?

Answer 14

Shows the oxidation state of the element without a sign.

Question 15

Define oxidation in terms of electron transfer.

Answer 15

Oxidation is loss of electrons

Question 16

Define reduction in terms of electron transfer.

Answer 16

Reduction is the gain of electrons

Question 17

Define oxidation in terms of oxidation number.

Answer 17

Increase in oxidation number

Question 18

Define reduction in terms of oxidation number.

Answer 18

Decrease in oxidation number.

Question 19

What do the oxidation numbers of an ionic compound sum up to?

Answer 19

The relative charge of the ionic charge

Question 20

What do the oxidation numbers of a compound sum up to?

Answer 20

0

Question 21

What is ionic bonding defined as?

Answer 21

The electrostatic attraction between positive and negative ions.

Question 22

How is a giant ionic lattice formed?

Answer 22

Each ion attracts oppositely charged ions in all directions.

Question 23

Give some properties of ionic compounds.

Answer 23

High melting and boiling points. 
Solid at room temperature . 
Dissolve in polar solvents.
Does not conduct electricity when solid.
Can conduct electricity when molten or dissolved.

Question 24

Why do ionic compounds have high melting and boiling points?

Answer 24

High temperatures are needed to overcome the strong electrostatic attraction between the ions.

Question 25

Why are ionic compounds solid at room temperature?

Answer 25

At room temperature there is insufficient amount fo energy to overcome the string electrostatic forces of attraction between the oppositely charged ions.

Question 26

Why do ionic compounds dissolve in polar solvents?

Answer 26

Polar water molecules break down the lattice and surround each ion in solution. The water molecules attract and surround the ions because water is a polar molecules and has charged ends.

Question 27

Why do ionic compounds only conduct electricity when molten or dissolved?

Answer 27

When solid the ions are in a fixed position and are not mobile which prevents charge ti be carried in the structure however when the compound is molten or dissolved the solid ionic lattice breaks down and the ions are now free to move as mobile charge carriers.

Question 28

What is a covalent bond?

Answer 28

It is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

Question 29

``` How many bonds can the following form? Carbon Nitrogen Oxygen Hydrogen ```

Answer 29

Carbon- 4 Nitrogen- 3 Oxygen-2 Hydrogen-1

Question 30

What is a dative covalent bond?

Answer 30

A covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only.

Question 31

What is the measurement of covalent bond strength ?

Answer 31

Average bond enthalpy.