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Chemistry GCSE AQA > Bonding, Stucture And The Properties Of Matter > Flashcards

Bonding, Stucture And The Properties Of Matter Flashcards

(54 cards)

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1
Q

What are the three types of strong chemical bonds

A

Ionic bonding
covalent bonding
metallic bonding

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2
Q

When does ionic bonding occur

A

Ionic bonding occurs in compounds formed from metals combined with non-metals

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3
Q

When does covalent bonding occur

A

Covalent bonding occurs in most non-metallic elements and in compounds of non-metals

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4
Q

When does metallic bonding occur

A

Metallic bonding occurs in metallic elements and alloys 

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5
Q

For ionic bonding the particles are… 

A

Oppositely charged ions

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6
Q

For covalent bonding the particles are atoms which…

A

Share pairs of electrons

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7
Q

For metallic bonding the particles are atoms which…

A

Share delocalized electrons

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8
Q

What is an ionic compound

A

An ionic compound is a giant covalent structure of ions

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9
Q

How are ionic compounds held together

A

Ionic compounds are held together by strong electrostatic forces of attraction between oppositely charged ions.

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10
Q

How do the forces act in ionic bonding

A

The forces act in all directions in the lattice (This is called ionic bonding)

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11
Q

What is electrostatic forces

A

Non-contact forces they pull or push on objects without touching them

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12
Q

What is ionic bonding

A

When a metal atom reacts with a nonmetal atoms and electrons in the outer shell of the metal atom are transferred.
Metals lose electrons to become positively charged ions and nonmetal atoms gain electrons to become negatively charged ions

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13
Q

What happens when atoms share pairs of electrons

A

they form a covalent bond these bonds between atoms are strong

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14
Q

Define oxidation

A

The Gaining of oxygen is called oxidation

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15
Q

Define reduction

A

The losing of oxygen is called reduction 

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16
Q

When metals react what happens to the electrons

A

When metals react they lose electrons and form a positive ion

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17
Q

What happens to a more reactive element when it reacts with a less reactive element

A

A more reactive element will push out (displace) a less reactive elements from its compound

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18
Q

What does AQ stand for

A

Aqueous Solution (Dissolved in water)

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19
Q

What are bases

A

Bases are chemicals which can neutralize acids producing a salt and water

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20
Q

What is the equation for naturalization

A

Hydrogen ion + hydroxide ion > water
H+. +. OH- > H2O

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21
Q

Bases that are soluble in water are called…

A

Alkalis

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22
Q

In aqueous solution what happens to the acid molecules

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A

acid molecules ionise (split) and release H+

23
Q

What happens to strong acids in aqueous solutions

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A

Strong acids fully ionise (split and form H+) in aqueous solutions

24
Q

Name three weak acids

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A

Carbonic acid
Ethanonic acid
citric acid

25
Ionic compounds have a structure called 
Giant ionic lattices 
26
What are the functions of a giant ionic lattice
They have a strong elastic force of attraction in all directions between oppositely charged ions
27
What melting and boiling points do Ionic compounds have
They have a high melting points and a high boiling point because they are large amount of energy needed to break down many strong bonds
28
When metal are dissolved in water what happened to Ionic compounds
They conduct electricity because the ions are free to move so charge can flow
29
Name one ionic compound (Giant ionic lattice)
Sodium chloride
30
What are all particles represented as
Solid spheres 
31
What type of molecules does covalent bonding have
Covalently bonded substances consist of small molecules
32
What type of molecules does polymers have
A covalently bonded substance that has very large molecules
33
Name some giant covalent structures
Diamond Silicon dioxide Graphite
34
What do metals consist of
Metals consist of giant structures of atoms are arranged in a regular pattern
35
The electrons on the outer shell of metal atoms are what
Delocalized so are free to move through the whole structure
36
Substances that consist of small molecules are usually what
Gases or liquids that have a relatively low melting point and boiling point
37
Substances of small molecules consists of
Weak force between molecules (Intermolecular force)
38
The intermolecular forces increase with the size of the molecules what does this mean
Larger molecules have a high melting and boiling point
39
Substances that consist of small molecules do not conduct electricity why
The molecules do not have an overall electric charge
40
What are polymers
They are very large molecules the atom in the polymer molecules are linked to other atoms by strong covalent bonds the intermolecular forces between polymer molecules are relatively strong and theses substances are solid at room temperature
41
What do giant Covalent structures consist of
They are solids with very high melting points all the items in the structures are linked to other atoms by strong covalent bonds these bonds must overcome to melt or boil substances
42
Atoms are arranged in layers in pure metals what does this allow
It allows metals to be in Bend and shaped. pure metals are too soft for and are mixed with other metals to make alloys which are harder
43
Why are alloys harder than pure metals
Metal alloys are made up of different atoms, unlike pure metal, where the atoms are all the same. This makes it harder for the atoms to move around in metal alloys because they consist of different sizes of atoms, which is why they are typically much stronger and harder than pure metals. One example of an exceptionally strong alloy is stainless steel.
44
Why are metals good conductors of electricity
The delocalized electrons in the metal carry electric charge through the metals and metals are good conductors of thermal energy because the energy is transferred by the delocalized electrons
45
What is the structure of diamond
Diamond has carbon atoms that form 4 covalent bonds with carbon atoms in a Giant covalent structure so diamonds are very hard and has a very high melting points that does not conduct electricity
46
What happens to one electron in graphite
One electron from each carbon atom is delocalized
47
What’s the structure of graphite
In graphite, each carbon atom forms three covalent bonds with three other carbon atoms forming layers of hexagonal rings which have no covalent bonds between the layers
48
How is graphite similar to metals
They both have delocalized electrons
49
What is the structure of graphene
Graphene is a single layer of graphite
50
Explain the properties of graphene in terms of structure and bonding
Graphene has a very high melting point and is very strong because of its large regular arrangement of carbon atoms joined by covalent bonds . Like graphite, graphene conducts electricity well because it has delocalised electrons that are free to move through its structure.
51
What are fullerenes 
Fullerenes are molecules of carbon atoms with hollow shapes. the structure of fullerenes are hexagonal rings of carbon atoms but they may also contain rings with 5 or 7 carbon atoms
52
What was the first fullerene to be discovered
Buckminsterfullerene (c60) which has a spherical shape
53
What are carbon nanotubes
Carbon nanotubes are cylindrical fullerene with very high length to diameter ratio. they are useful for nanotechnology electronics and materials.
54
What does pure mean
A substance made from one element or just one compound

Chemistry GCSE AQA (12 decks)

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