Module 2 Chapter 5

Question 1

What happens as the shell number increases

Answer 1

The more electrons can be contained in the shell

Question 2

What happens in terms of energy as the shell number increases

Answer 2

As the shell number increases the energy of the shells also increases

Question 3

Why does the energy of the shells increase as the shell number increases

Answer 3

More energy is required to keep them in the atom as they are further away from the nucleus

Question 4

What is another name for the shell number or energy level number

Answer 4

Principal quantum number

Question 5

What can the maximum number of electrons in each shell be calculated by

Answer 5

2N squared (where n is the principal quantum number)

Question 6

What are the maximum number of electrons in each shell

Answer 6

N = 1, maximum number 2
N = 2, maximum number 8
N = 3, maximum number 18
N = 4, maximum number 32

Question 7

What do electrons behave like

Answer 7

Electrons have wave particle duality meaning they behave both as a wave and a particle

Question 8

What are shells made up of

Answer 8

They are made up of atomic orbitals

Question 9

What can orbitals hold

Answer 9

They are a region around the nucleus that can hold up to 2 electrons with 2 opposite spins.

Question 10

What is an orbital

Answer 10

It’s visualised as a region in space where there is a high probability of finding an electron.

Question 11

What is a property of the electrons in the orbitals

Answer 11

They have either up or down spin. When one electron has up spin the other has down spin.

Question 12

Without observation what state are electrons in

Answer 12

They are in superposition when neither is in up spin or down spin, it is in the spin up and down state.

Question 13

What are the 4 different orbitals

Answer 13

S-, p-, d-, and f- orbitals

Question 14

What is an s orbital

Answer 14

Electron orbital in the shape of a sphere.
They can hold two electrons
Each shell from n=1 contains one s orbital

Question 15

What happens to the s orbital as the principle quantum number increases

Answer 15

the radius of the orbital increases

Question 16

Draw an s orbital

Question 17

What is a p orbital

Answer 17

The orbital is in the shape of a dumbell
Each p orbital contains 2 electrons

Question 18

What are the three types of p orbitals

Answer 18

Px,Pz,Py, where the small letter is the axis that they lie on

Question 19

What do each of the p orbitals look like

Answer 19

Draw it

Question 20

What principle quantum number 1 what is the maximum number of electrons and number of each orbitals

Answer 20

2 electrons
1S

Question 21

What principle quantum number 2 what is the maximum number of electrons and number of each orbitals

Answer 21

8 electrons
1S, 2S, 2P (2Px, 2Py, 2Pz)

Question 22

What principle quantum number 3 what is the maximum number of electrons and number of each orbitals

Answer 22

18 electrons
1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D

Question 23

What principle quantum number 4 what is the maximum number of electrons and number of each orbitals

Answer 23

32 electrons

1S, 2S, 2P (2Px, 2Pz, 2Py), 3S, 3P (3Px, 3Py, 3Pz), 3D, 4S, 4P (4Px, 4Py, 4Pz), 4D, 4F

Question 24

How many d and f orbitals exist in principle quantum number 4

Answer 24

5 - d
7 - f

Question 25

What does the average energy in the subshells do as the principle quantum number increases

Answer 25

the average energy in the subshells increases as the principle quantum number increases

Question 26

What is the exception to this rule

Answer 26

The 4S orbital is lower in energy than 3D orbital

Question 27

How do we fill orbitals

Answer 27

We fill orbitals in increasing energy

Question 28

What do you use to represent the spin of an electron

Answer 28

You represent the different spins with up and down arrows

Question 29

What is Hund’s rule

Answer 29

If there are three electrons in a p subshell, one electron will go into each Px, Py, Pz orbital before doubling up

Question 30

What is Pauli’s exclusion principle

Answer 30

An orbital can only hold two electrons and they must have opposite spin

Question 31

What are cations and anions

Answer 31

Cations = positive ions = lost electrons Anions = negative ions = gained electrons

Question 32

When forming ions what occurs

Answer 32

the highest energy subshells lose or gain electrons

Question 33

How does the exception of 3D and 4S apply to this rule

Answer 33

3D is filled last/emptied last 4S is filled first/ emptied first

Question 34

What happens during a chemical reaction between a metal and a non metal

Answer 34

The non metal gains electrons forming anions and the metal loses electrons forming cations

Question 35

What is an ionic bond

Answer 35

The strong electrostatic forces of attraction between oppositely charged ions.

Question 36

What is the arrangement of ionic structures

Answer 36

They are arranged in a giant lattice, and each ion experiences many attractions (as there are ionic bonds in all directions)

Question 37

Why do ionic compounds have a high melting point

Answer 37

They are held together by many strong ionic bonds. These take lots of energy to break so ionic compounds have very high melting points.

Question 38

What is the correlation between ion charge and melting point

Answer 38

The greater the ion charge the higher the melting point

Question 39

What is the solution lily of ionic compounds

Answer 39

Many ionic compounds are soluble in polar solutions. This is because water molecules attract and surround the ions once the lattice is broken.

Question 40

What does the solubility of an ionic compounds depend on

Answer 40

It depends on the relative strengths of attraction within the giant ionic lattice structure and the attractions between ions and water molecules.

Question 41

What is the general rule of solubility for ionic compounds

Answer 41

Solubility decreases as ionic charge increases

Question 42

What is the electrical conductivity of ionic compounds

Answer 42

In the solid state the ions are in fixed positions and are not free to move, they don’t conduct electricity. When liquid or in solution, the charge carrying ions are free to move so conduct electricity.

Question 43

What is a covalent bond

Answer 43

The strong electrostatic forces of attraction between a shared pair of electrons and the positive nuclei of the bonded non-metallic elements.

Question 44

What is covalent bonding in terms of 1 bond (orbitals)

Answer 44

The overlap between 2 atomic orbitals where each orbital contains 1 electrons, making a shared pair in the overlap

Question 45

What is a double covalent bond

Answer 45

The electrostatic forces of attraction between 2 shared pairs of electrons and nuclei of bond atoms

Question 46

What is a triple covalent bond

Answer 46

The electrostatic forces of attraction between 3 shared pairs of electrons and nuclei of bond atoms.

Question 47

What is a dative covalent bond

Answer 47

The pair of bonding electrons are donated by one of the bonding atoms. You denote this with an arrowhead from the element that provides it.