Topic 5- Bonding 📄/📄📄

Question 1

What is an ion?

Answer 1

A charged particle

Question 2

What is a bond?

Answer 2

Forces of attraction which hold atoms together

Question 3

Why do atoms bond?

Answer 3

To become more stable, by achieving noble gas configuration

Question 4

What do metals form when they bond ionically?

Answer 4

Cations

Question 5

What do non metals form when they bond ionically?

Answer 5

Anions

Question 6

When is an ionic bond formed?

Answer 6

When valence electrons are transferred from one atom to another to complete the outer shell electron

Question 7

What determines whether atoms gain or lose electrons?

Answer 7

The number of electrons on the outer shell, also known as the group number

Question 8

What is meant by noble gas configuration?

Answer 8

Ions have a full outer shell of electrons which is the same as the electronic configuration of atoms in group 0

Question 9

What is an ionic lattice?

Answer 9

Millions of ions are packed together in a regular cubic arrangement and are joined by covalent bonds. This forms a giant 3D structure known as an ionic lattice.

Lattice= regular repeating pattern

Question 10

What holds ions together?

Answer 10

Strong electrostatic forces of attraction which are difficult to break

Question 11

What is the charge of ionic compounds?

Answer 11

There is no charge. The ions are charged and overall the charges cancel each other out

Question 12

What do you have to do in order to cancel out the ionic charges?

Answer 12

Finding the lowest common multiple

(Or crossing charges over)

Question 13

When non metals form ions the suffix changes to..

Answer 13

IDE

Question 14

Example: How is calcium chloride formed?

Answer 14

Each calcium loses 2 electrons to become Ca2+ and each chlorine gains 1 electron to become Cl-. 2 chlorine atoms are needed for every calcium atom. This forms MgCl2, overall charge is 0 as the ions cancel each other out

Question 15

What are 3 properties of ionic compounds?

Answer 15

High melting and boiling points
Brittle
Only conduct when molten or in solution

Question 16

Explain the property of ionic compounds
High melting and boiling points

Answer 16

There are strong electrostatic forces of attraction between oppositely charged ions. These require a lot of energy to break

Question 17

Explain the property of ionic compounds
Brittle

Answer 17

Like charges repel when the layers are shifted, this causes the ionic lattice to shatter

Question 18

Explain the property of ionic compounds
Only conduct electricity when in solution or molten

Answer 18

Because the ions are free to move and carry charge

Question 19

What are polyatomic ions?

Answer 19

Sometimes there are more than 2 atoms involved in the bonding, sometimes they can contain more than one atom

Question 20

What is the ionic charge of carbonate?

Answer 20

CO3 2-

Question 21

What is the ionic charge of hydroxide?

Answer 21

OH-

Question 22

What is the ionic charge of ammonium?

Answer 22

NH4 +

Question 23

What is the ionic charge of sulfate?

Answer 23

SO4 2-

Question 24

What is the ionic charge of nitrate?

Answer 24

NO3 -

Question 25

What happens in covalent bonding?

Answer 25

Electrons are shared

Question 26

What forms covalent bonds?

Answer 26

Non metals

Question 27

What holds covalent bonds together?

Answer 27

Strong electrostatic forces of attraction, strong covalent bonds

Question 28

What state are covalent bonded molecules at room temperature?

Answer 28

Liquid or gas

Question 29

What are some examples of covalent bonded simple molecules?

Answer 29

Water Oxygen Carbon dioxide Bromine Hydrogen

Question 30

What is a covalent bond?

Answer 30

A shred pair of electrons

Question 31

What is a covalent bond?

Answer 31

A shred pair of electrons

Question 32

What are 3 properties of covalents?

Answer 32

Liquid or gas at room temp Don’t conduct Weak intermolecular forces

Question 33

Explain the covalent property of liquid or gas at room temp

Answer 33

Forces between moelcules are relatively weak so don’t take a lot of energy to break.

Question 34

Explain the covalent property of not conducting electricity

Answer 34

Made up of non metals

Question 35

Explain the covalent property of low melting and boiling points

Answer 35

Weak intermolecular forces don’t require a lot of energy to break

Question 36

What are polymers?

Answer 36

Long chains of monomers joined together

Question 37

How are polymers made?

Answer 37

A double bond that opens to join more monomers together

Question 38

How do you name polymers?

Answer 38

Poly in front of monomer name

Question 39

What are 3 properties of polymers?

Answer 39

Solid at room temp Polymers chains intertwined Many intermolecular forces along chains require a lot of energy to break

Question 40

What are allotropes?

Answer 40

Different forms of the same element

Question 41

What is the arrangement of the giant covalent diamond?

Answer 41

Tetrahedral

Question 42

What is diamond made of?

Answer 42

Carbon

Question 43

Does diamond conduct electricity?

Answer 43

No Each carbon atom is covertly bonded to 4 other atoms so there are no delocalised ejections to carry charge

Question 44

What are some uses of diamond?

Answer 44

Drill bits Jewellery

Question 45

What are some uses of diamond?

Answer 45

Drill bits Jewellery

Question 46

What are the bonds like in diamond?

Answer 46

Strong covalent bonds require a lot of energy to break

Question 47

What is graphite made of?

Answer 47

Carbon

Question 48

What are uses of graphite?

Answer 48

Pencils, good equipment, lubricant, electrodes

Question 49

What are the forces like in graphite?

Answer 49

Weak so layers can easily slide over each other

Question 50

What’s the arrangement in graphite?

Answer 50

Hexagonal

Question 51

Can graphite conduct electricity?

Answer 51

Yes Each atom is bonded to 3 others leaving one delocalised electron which can move and carry charge

Question 52

What are the bonds like in graphite?

Answer 52

Solid at room temp as there are lots of strong covalent bonds

Question 53

What are fullerenes?

Answer 53

Simple molecules

Question 54

Example of fullerenes

Answer 54

Buckminster Nanotube

Question 55

What are fullerenes made of?

Answer 55

Carbon making them an allotrope of carbon

Question 56

What are some properties of fullerenes?

Answer 56

Low melting and boiling points meaning there are weak intermolecular forces Strong covalent bonds between molecules

Question 57

Can fullerenes conduct electricity?

Answer 57

Yes, each carbon atom is covalent bonded to 4 others meaning it can conduct across the surface as die to 1 free electron which

Question 58

What is graphene?

Answer 58

An allotrope of carbon which is an individual layer of graphite, one layer thick

Question 59

Is graphene simple or giant covalent?

Answer 59

Giant

Question 60

Can graphene conduct electricity?

Answer 60

Each carbon atom is covalent bonded to 3 others the one free electrons conducting across the surface

Question 61

What are the 5 bonding models?

Answer 61

1. Dot and cross 2. Ball and stick 3. Displayed formula 4. 3D space filling model 5. Ionic models

Question 62

Advantages of dot and cross diagrams:

Answer 62

Shows where electrons come from Can easily draw to identify formula Shows how electrons are shared Easy to identify which atoms/ions

Question 63

Disadvantages of dot and cross diagrams

Answer 63

Doesn’t show fact that electrons move Only show outer electrons Could imply electrons are different atoms due to crosses and dots Doesn’t show relative side of atoms Doesn’t show it in 3D arrangement

Question 64

Advantages of ball and stick model and displayed formula

Answer 64

Can easily identify formula Shows Clearer for large repeating units Can show if molecule is 3D Easier to identify single, double bonds

Question 65

Disadvantages of ball and stick and displayed formula

Answer 65

Doesn’t show where electrons come from Doesn’t show relative size of atoms Doesn’t show 3D arrangement unless3D model Implies atoms are held with sticks Can’t see attending of electrons

Question 66

Advantages of 3D space filing model

Answer 66

Shows relative size of atoms Doesn’t Can show which atoms are bonded Shows 3D arrangement

Question 67

Disadvantages of 3D space filling model

Answer 67

Die yes always show what atoms they are Doesn’t show electrons involved in binding Doesn’t show the bonds formed and number

Question 68

Advantages of ionic models

Answer 68

Shows lattice arrangement Explains why they conduct electricity Shows charges

Question 69

Disadvantages of ionic models

Answer 69

Doesn’t show relative size of ions Doesn’t always show which ion is which Doesn’t show vibration of ions (Not quick to draw)