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SCIENCE GCSE > Chemistry CT1 > Flashcards

Chemistry CT1 Flashcards

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1
Q

What properties are there of a diamond structure?

A

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

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2
Q

What are the properties of a giant covalent structure?

A

-Very high melting point
-Variable electrical conductivity

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3
Q

What are the properties of a giant ionic structure?

A

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

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4
Q

What are the properties of a covalent simple molecular?

A

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

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5
Q

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

A

Large amount of (heat) energy

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6
Q

What is the mass of a proton?

A

1

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7
Q

What is the mass of a neutron?

A

1

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8
Q

What is the mass of an electron?

A

0

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9
Q

What is an isotope?

A

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

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10
Q

How do you calculate ram?

A

mass number x abundance and then divide by 100

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11
Q

What does ionic bonding involve?

A

a metal and a non-metal

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12
Q

What does covalent bonding involve?

A

2x non-metal

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13
Q

What does ionic bonding do?

A

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

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14
Q

What does covalent bonding do?

A

It shares its electrons

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15
Q

What does delocalised mean?

A

Not attached to any specific centre

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16
Q

What is a lattice structure?

A

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

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17
Q

When does a metallic bond occur?

A

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

18
Q

What did dalton and thomson think the atomic structure was?

A

a solid

19
Q

What does inert mean?

A

stable and unreactive under specified conditions

20
Q

What is an alpha particle?

A

Positively charged particles

21
Q

What does an alpha particle consist of?

A

two protons and two neutrons

22
Q

What is an atom?

A

The smallest particle that exists.

23
Q

Why are ionic compounds so strong?

A

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

24
Q

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

A

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

25
Q

What does aqueous mean?

A

solution

26
Q

What is the name of the biggest carbon structure?

A

Buckminsterfullerene

27
Q

How many carbon atoms are there in a buckminsterfullerene?

A

60

28
Q

What is a monomer?

A

one molecule

29
Q

What is a polymer?

A

long chain of monomers

30
Q

How does metals conduct heat and electricity?

A

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

31
Q

Where is the energy transferred to and from?

A

hotter areas to colder areas

32
Q

Why is the structure of a diamond so strong?

A

Lots of strong covalent bonds

33
Q

Why does graphite conduct electricity and heat?

A

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

34
Q

What is graphene?

A

A single layer of graphite?

35
Q

What are cations?

A

Positively charged ions

36
Q

What are anions?

A

Negatively charged ions

37
Q

what are the names of some common molecular elements?

A

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

38
Q

What is the bonding that is found in molecules?

A

Covalent bonding

39
Q

What is the approximate size of atoms and smaller molecules?

A

Around 0.1nm

40
Q

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

A

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

41
Q

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

A

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

SCIENCE GCSE (5 decks)

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