Chemistry CT1

Question 1

What properties are there of a diamond structure?

Answer 1

-High melting point
-High boiling point
-Does not conduct electricity
-Hard/solid

Question 2

What are the properties of a giant covalent structure?

Answer 2

-Very high melting point
-Variable electrical conductivity

Question 3

What are the properties of a giant ionic structure?

Answer 3

-Strong electrostatic force
-High melting point
-Poor conduct electricity when solid
-Good conduct in molten

Question 4

What are the properties of a covalent simple molecular?

Answer 4

-low melting point
-Weak intermolecular attractions between molecules
-Poor conductor

Question 5

What is needed to break the bonds of a diamond structure?

Answer 5

Large amount of (heat) energy

Question 6

What is the mass of a proton?

Answer 6

1

Question 7

What is the mass of a neutron?

Answer 7

1

Question 8

What is the mass of an electron?

Answer 8

0

Question 9

What is an isotope?

Answer 9

an atom with a different amount of neutrons and there mass changes

Question 10

How do you calculate ram?

Answer 10

mass number x abundance and then divide by 100

Question 11

What does ionic bonding involve?

Answer 11

a metal and a non-metal

Question 12

What does covalent bonding involve?

Answer 12

2x non-metal

Question 13

What does ionic bonding do?

Answer 13

It gives it electron to another atom to have a full outer shell/#

Question 14

What does covalent bonding do?

Answer 14

It shares its electrons

Question 15

What does delocalised mean?

Answer 15

Not attached to any specific centre

Question 16

What is a lattice structure?

Answer 16

a solid metal structure that consists of closely packed metal ion, arranged in a regular way.

Question 17

When does a metallic bond occur?

Answer 17

when the positive ions are joined by the delocalised electrons linking each positive ion together

Question 18

What did dalton and thomson think the atomic structure was?

Answer 18

a solid

Question 19

What does inert mean?

Answer 19

stable and unreactive under specified conditions

Question 20

What is an alpha particle?

Answer 20

Positively charged particles

Question 21

What does an alpha particle consist of?

Answer 21

two protons and two neutrons

Question 22

What is an atom?

Answer 22

The smallest particle that exists.

Question 23

Why are ionic compounds so strong?

Answer 23

The positive and negative ions are attracted, so ionic compounds have strong electrostatic forces.

Question 24

Why do ionic compounds conduct electricity when they are molten and aqueous?

Answer 24

Ionic compounds are only conductive if their ions are free to move around?

Question 25

What does aqueous mean?

Answer 25

solution

Question 26

What is the name of the biggest carbon structure?

Answer 26

Buckminsterfullerene

Question 27

How many carbon atoms are there in a buckminsterfullerene?

Answer 27

60

Question 28

What is a monomer?

Answer 28

one molecule

Question 29

What is a polymer?

Answer 29

long chain of monomers

Question 30

How does metals conduct heat and electricity?

Answer 30

They have delocalised electrons that are free to move about and can transfer energy or charge much easier.

Question 31

Where is the energy transferred to and from?

Answer 31

hotter areas to colder areas

Question 32

Why is the structure of a diamond so strong?

Answer 32

Lots of strong covalent bonds

Question 33

Why does graphite conduct electricity and heat?

Answer 33

It has layers of carbon atoms, there are free electrons which are able to conduct.

Question 34

What is graphene?

Answer 34

A single layer of graphite?

Question 35

What are cations?

Answer 35

Positively charged ions

Question 36

What are anions?

Answer 36

Negatively charged ions

Question 37

what are the names of some common molecular elements?

Answer 37

H2-hydrogen O2-oxygen cl2-chlorine N2-Nitrogen

Question 38

What is the bonding that is found in molecules?

Answer 38

Covalent bonding

Question 39

What is the approximate size of atoms and smaller molecules?

Answer 39

Around 0.1nm

Question 40

Why does covalent, simple molecular compounds have low melting and boiling points?

Answer 40

-weak intermolecular forces -These forces are overcome with very little energy

Question 41

Why are covalent, simple molecular compounds poor conductors of electricity?

Answer 41

-Electrons are shared within the bonds meaning there is not free electron or ions available.