Electron Configuration and Structure

Question 1

Define electron configuration?

Answer 1

The arrangement of electrons in an atom

Question 2

How are electron arranged in an atom?

Answer 2

In energy levels/ shells numbered linearly, with number 1 being closest to the nucleus.

Question 3

What are the first 10 energy levels in electron configuration?

Answer 3

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

Question 4

What are subshells made up of?

Answer 4

Subshells are made up of orbitals - a region the nucleus that can hold up to 2 electrons with opposite spin.

Question 5

What do orbitals represent?

Answer 5

They represent the mathematical probabilities of finding an electron at any point within certain spatial distributions around the nucleus.

Question 6

What is the Aufbau principle?

Answer 6

Electrons fill up the lowest energy subshells first

Question 7

What is the Pauli exclusion principle?

Answer 7

Electrons fill up orbitals singly before pairing up

Question 8

What is the Hund’s rule?

Answer 8

Each orbital holds 2 electrons with opposite or ‘paired spins’

Question 9

What is the exception in the pattern that orbitals fill up in?

Answer 9

The 4s- subshell is filled before the 3d- subshell.

Question 10

When is a cation formed?

Answer 10

Formed when electrons are lost

Question 11

When is an anion formed?

Answer 11

Formed when electrons are gained

Question 12

What rule do Hydrogen and Helium follow?

Answer 12

The duet rule

Question 13

What are the four types of chemical bonds?

Answer 13

1. Ionic
2. Covalent
3. Metallic
4. Dative covalent

Question 14

What is an ionic bond?

Answer 14

An electrostatic attraction between oppositely charged ions. Ionic bonds act in all different directions so each ions will be surrounded on all sides by ions of the opposite charge.

Question 15

When is an ionic bond formed?

Answer 15

Results from electron transfer from a metal atom to a non-metal atom.

Question 16

What is a covalent bond?

Answer 16

An electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms. Sigma bonds are formed by the overlap of an s and p orbital or 2 p-orbitals meeting end to end.

Covalent bonds are directional unlike ionic bonds

Question 17

When is a covalent bond formed?

Answer 17

Occurs between non-metal atoms and each atom provides an electron for the bonded pair

Question 18

What is a dative covalent bond and when is it formed?

Answer 18

In dative covalent bonds, one atom provides both electrons for the bonded pair

Question 19

What is metallic bonding and how is it formed?

Answer 19

Electrostatic attraction between a lattice of metal cations and delocalised electrons.

Question 20

What do dot and cross diagrams show?

Answer 20

The bonding of the outer shell electrons

Question 21

What is a lone pair?

Answer 21

A pair of non-bonded electrons

Question 22

How many covalent bonds can Hydrogen make?

Answer 22

1

Question 23

How many covalent bonds can Oxygen make?

Answer 23

2

Question 24

How many covalent bonds can Nitrogen make?

Answer 24

3

Question 25

How many covalent bonds can Carbon make?

Answer 25

4

Question 26

What is the substance if there is no bonding?

Answer 26

A monoatomic gas

Question 27

What are the two main structures of bonding?

Answer 27

1. Giant lattice structures | 2. Simple covalent structures

Question 28

What is a giant lattice structure?

Answer 28

Have a regular 3-D arrangement of atoms which extends throughout the compound

Question 29

What is a simple covalent structure?

Answer 29

Consists of many small molecules held together by weak intermolecular forces.

Question 30

When do giant lattice structures occur?

Answer 30

In ionic compounds

Question 31

What is the melting point of giant lattice structure like? why?

Answer 31

High melting point because lots of energy is required to break the strong ionic bonds in the lattice.

Question 32

Are giant lattice structures soluble in water?

Answer 32

Often

Question 33

Do giant lattice structure conduct electricity? Why?

Answer 33

Yes when molten or in solution because ions become free to move as mobile charge carriers.

Question 34

When do simple covalent molecular structures occur?

Answer 34

Occurs in small covalent molecules

Question 35

What is the melting point of simple covalent molecular structures like? why?

Answer 35

Low melting point as little energy is required to break weak intermolecular forces

Question 36

Are simple covalent molecular structures soluble in water?

Answer 36

Often insoluble in water

Question 37

Do simple covalent molecular structures conduct electricity? Why?

Answer 37

Do not conduct electricity as lack mobile ions or electrons to act as charge carriers.

Question 38

When do Giant covalent lattice structures occur?

Answer 38

Found in diamond, graphite, silica etc | They have a lattice of strong covalent bonds throughout the compound

Question 39

What is the melting point of Giant covalent lattice structures like? why?

Answer 39

Very high melting point because a large amount of energy is required to overcome the covalent bonds

Question 40

Are Giant covalent lattice structures soluble in water?

Answer 40

Usually insoluble

Question 41

Do Giant covalent lattice structures conduct electricity? Why?

Answer 41

Do not conduct electricity except graphite

Question 42

When do Giant metallic lattice structures occur?

Answer 42

Strong electrostatic attraction between metal cations and delocalised electrons

Question 43

What is the melting point of Giant metallic lattice structures like? why?

Answer 43

High melting point because of strong intermolecular forces

Question 44

Are Giant metallic lattice structures soluble in water?

Answer 44

Usually insoluble in water

Question 45

Do Giant metallic lattice structures conduct electricity? Why?

Answer 45

Conduct electricity when molten or solid because delocalised electrons are free to move as mobile charge carriers.