2D

Question 1

Metallic bonding

Answer 1

Electrostatic attraction between positive metal ions and negative delocalised electrons

Question 2

What are delocalised electrons

Answer 2

Metals have a relatively low 1st ionisation energy, the valence electrons are held loosely and in a metallic lattice, each atom loses its valence electron/s which then extend through the lattice occupying a new set of energy levels. These are said to be delocalised

Question 3

Ionic bonding

Answer 3

electrostatic attraction between the positive cations and negative anions

Question 4

covalent bonding

Answer 4

Electrostatic attraction between the shared pair of electrons and the nuclei of the bonded atoms

Question 5

Intermolecular bonding

Answer 5

Electrostatic attraction between dipoles on molecules

Question 6

How many bonds can Group 1/ Group 7 make

Answer 6

1

Question 7

How many bonds can Group 6 make

Answer 7

double bond

Question 8

How many bonds can Group 5 make

Answer 8

Triple bonding

Question 9

Octet rule

Answer 9

When an atom of an element has 8 electrons in its outer shell i is said to have an octet

Question 10

When does the octet rule not work?

Answer 10

• Atoms in elements tat are in Group 3 or higher - have access to 3d subshell which holds 10 electrons
• unpaired electrons can pair up - max number of electron pairs in an outer shell is number of electrons in outer shell

Question 11

What is a dative covalent bond?

Answer 11

A covalent bond where both of the electrons come from a single bond
Eg : in an ammonium ion where in ammonia, Nitrogen has 2 free electrons that can form a bond with a hydrogen ion with no electrons

Question 12

What is needed for a dative covalent bond to form

Answer 12

• The acceptor atom must be electron deficient - available orbitals for electrons to occupy

Question 13

In what way is a dative and covalent bond the same

Answer 13

• Dative and Covalent bonds are exactly the same
• Same length
• Same average bond enthalpy

Question 14

What is a lone pair

Answer 14

A pair or electrons not used in bonding on the outer shell

Question 15

What is a Polyatomic ion

Answer 15

A group of atoms with a charge - For example a carbonate ion

Question 16

What is a giant ionic lattice

Answer 16

A regular 3D of oppositely charged ions, held together by electrostatic attractions

Question 17

Features of a giant ionic lattice

Answer 17

• Conducts electricity when molten or aqueous - not solid
• High MP, BP
• Ionic bonding

Question 18

Giant metallic lattice

Answer 18

A regular 3D arrangement of positive ions and delocalised electrons

Question 19

Features of Giant metallic lattice

Answer 19

• High MP and BP
• Conducts electricity when solid or liquid
• Metallic bonding

Question 20

Giant covalent lattice

Answer 20

A 3D structure of atoms that share electrons with each other

Question 21

Features of Giant Covalent lattice

Answer 21

• High MP/BP
• doesn’t conduct electricity when solid or liquid
• Covalent bonding

Question 22

Simple Covalent molecule

Answer 22

• 3D structure of molecules held together by weak intermolecular forces

Question 23

Features of A simple covalent molecule

Answer 23

• Low MP/BP
• Cannot conduct electricity solid or molten

Question 24

Why can’t simple covalent molecules conduct electricity

Answer 24

Negative ions or electrons are no free to move and act as mobile charge carriers as they are fixed in place and can’t carry charge through the structure.

Question 25

What is a Simple covalent molecule

Answer 25

Small units containing a definite number of atoms with a definite molecular formula.

Question 26

What is a Giant covalent molecule

Answer 26

Billions of atoms held together to form a network of strong covalent bonds

Question 27

Structure of Graphite

Answer 27

- Parallel layers of hexagonally arranged carbon atoms. - Layers bonded by weak London forces

Question 28

Features of Graphite

Answer 28

- Can conduct electricity as only 3 of Carbons 4 valence electrons so has free delocalised electrons that can move and carry charge - Soft as weak London Forces between layers easily broken and layers slide over each others

Question 29

What is Graphene

Answer 29

A single sheet of graphite structure, similar conductivity and strength properties

Question 30

Structure and Features of Diamond

Answer 30

- Tetrahedral structure, all 4 valence electrons used so cannot conduct electricity as no delocalised electrons. - Hard as tetrahedral structure of each carbon atom spreads forces through structure and strong covalent bonds need lots of energy to break.

Question 31

Why do metals have a high MP and BP

Answer 31

Due to strong electrostatic attraction between pos metal ions and neg electron

Question 32

Why are Metals better conductors when molten

Answer 32

Both delocalised electrons and positive ions can move and act as mobile charge carriers through the structure

Question 33

Why do MP across period 3 increase

Answer 33

- Metal atoms donate their valence electrons to electron sea - As you go across period valence electrons increase in delocalised electron sea - stronger electrostatic attractions between metal ions and delocalised electrons

Question 34

What does malleable mean?

Answer 34

Easily bent into different shape

Question 35

What does ductile mean

Answer 35

Can be stretched into a wire

Question 36

Why are metals both malleable and ductile?

Answer 36

Layers of ions easily slide over each other

Question 37

What is an alloy, why do alloys have different properties?

Answer 37

Different metal mixtures - metal ions have different sizes so layers cannot slide over each other as easily.

Question 38

What alloy is brass made out of

Answer 38

Copper and Zinc

Question 39

What metals is stainless steel alloy made of?

Answer 39

Iron and Chromium

Question 40

What shape and bond angle does a molecule with 2BP and 0LP have?

Answer 40

Linear shape - bond angle of 180

Question 41

What shape and bond angle does a molecule with 3BP and 0LP have?

Answer 41

Trigonal Planar - bond angle of 120 degrees

Question 42

What shape and bond angle does a molecule with 4BP and 0LP have?

Answer 42

Tetrahedral - bond angle of 109.5 degrees

Question 43

What shape and bond angle does a molecule with 5BP and 0LP have?

Answer 43

Trigonal bipyramidal, bond angles of 90 and 120 degrees

Question 44

Wha shape and bond angle does a molecule with 6BP and 0LP have?

Answer 44

Octahedral - bond angle of 90 degrees

Question 45

What shape and bond angle does a molecule with 2BP and 2LP have?

Answer 45

Non linear shape, bond angle of 104.5

Question 46

What shape and bond angle does a molecule of 3BP and 1LP have?

Answer 46

Pyramidal shape - bond angle of 107 degrees

Question 47

Why is a double bond considered a single bond when regarding shapes?

Answer 47

It is in one region of electron density

Question 48

What is electronegativity

Answer 48

The measure of attraction of a bonded atom for the pair of electrons in a covalent bond