Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

GCSE Chemistry > Bonding Structure And Properties Of Matter > Flashcards

Bonding Structure And Properties Of Matter Flashcards

1
Q

Name three types of chemical bonds

A

Ionic, covalent and metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are the particles like in an ionic bond?

A

Oppositely charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What do atoms do in a covalent bond to get a full outer shell?

A

Share pairs of electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What particles are involved in metallic bonding

A

Positive ions and delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What type of bond is formed between a metal and a nonmetal

A

Ionic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What type of bonding is forms between just nonmetals?

A

Covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What type of bonding occurs in metals and alloys?

A

Metallic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What type of bonding involves gain or loss of electrons

A

Ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What happens when a metal and a nonmetal form an ionic bond?

A

Electrons in the outer shell of the metal atom are transferred to the nonmetal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the group number if an element forms of -2 ion

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

If an atom loses two electrons to form an ion, what charge will the ions have?

A

2+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What happens to a metal when forming an ionic bond?

A

Loses electrons and becomes positively charged - size of a charge is the same as the number of electrons lost. AKA lose one electron= +1 loses two electrons = +2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What happens to a nonmetal when forming an ionic bond

A

Gains electrons and becomes negatively charged -size of the charged is the same as the number of electrons gained. AKA gain one election = -1 charge and gain two electrons = -2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why do metals and nonmetals form ionic bonds?

A

To get a full outer shell and therefore have the electronic structure of a noble gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How can the transfer of electrons when forming an ion be represented?

A

Dot And cross diagram is

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the limitations of using dot and cross diagram to represent ionic compounds?

A

It does not show how the ions are arranged in the space and does not show structure in 3-D.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What type of bonding is likely to occur between group one and two metals with group 6 and seven nonmetals

A

Ionic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Describe how magnesium and oxygen form an ionic bond

A

Magnesium loses two electrons and forms of 2+ ion magnesium gains two electrons and forms of 2- ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is a type of force that exist between oppositely charged ions?

A

Electrostatic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What type of structure is found in ionic compounds

A

Giant lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Describe the bonding and structure in an ionic compound

A

Giant lattice
Strong electrostatic attraction between oppositely charged ions with the forces acting in all directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

How can the structure of sodium chloride be represented, what are the limitations?

A

Space fill model: shows relative sizes of ions and regular pattern but can only see outer layer.

Ball and stick model: shows all the ions, bonds aren’t represented by lines, don’t show outer electrons.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What must the charges do when working out the formula of an ionic compound?

A

Cancel out

Eg

Na(+) and Cl(-)is NaCl

Mg(2+) and Cl(-) need 2 of cl- to cancel out the 2+ from mg

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What are the properties of ionic compounds?

A

have a high melting points/high boiling point

Can conduct when molten (melted so liquid) or when in solution (dissolved in water)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Why do ionic compounds have high melting points?
Due to the strong electrostatic attraction between oppositely charged ions, which requires a lot of energy to break
26
Why do ionic compounds conduct when melted or dissolved in water?
Ions are free to move,they can’t move when they’re solid, and can carry a charge.
27
How do you workout the empirical formula of ionic compounds from a diagram?
Work out the chargers on the ions and balance them out
28
A compound is made up of calcium ions and chloride what is it empirical formula?
Calcium is in group 2, so forms of, 2+ ion Chloride in group 7 so forms of 1- ion Need two chlorides to balance out the charge on the calcium
29
How are covalent bonds formed?
By sharing electrons
30
How many electrons does each atom donate in a single covalent bonds?
One
31
What is the strength of a covalent bond?
Strong
32
What are the two types of covalent structure?
Small molecules and giant covalent
33
How are covalent bonds represented in small molecules?
Dot And cross - shows electrons shared Displayed formula - shows covalent bonds as lines Space fill - shows arrangement of atoms in 3-D
34
What type of structure is shown? H-C-H
Displayed - it shows covalent bonds as single lines between atoms
35
What are the limitations of using a displayed formula?
Does not show 3-D structure Does not show where the electrons in a covalent bonds have come from
36
What type of bonding do you get in polymers?
Covalent, where N is a large number this is polyethylene
37
How are the atoms links in a polymer?
By strong covalent bonds between the atoms weak intermolecular forces between the polymer chains
38
What are the properties of small covalent molecules?
Low melting points/boiling points, therefore gases mostly at room temperature do not conduct electricity
39
Why do small covalent molecules have low boiling points, are gases and evaporate easily?
They have a weak intermolecular forces, which don’t require much energy to break
40
What happens to the boiling point of simple covalent molecules with increasing size?
Increases because there are more of the weak intermolecular forces present
41
Which has the highest boiling point of hydrogen or methane
Methane as it is a large molecule, so there are more intermolecular forces present so more energy need to break this
42
Why don’t simple, covalent molecules, conduct electricity
they have no ions (charged particles), or free delocalised electrons
43
Name three giant covalent structures
Diamond graphite silicon dioxide
44
What are the melting point of the giant covalent structures?
Hi
45
What are the properties of diamonds?
High, melting point Hard Does not conduct electricity
46
Explain the properties of diamonds
High melting points/hard because it has lots of strong covalent bonds (each C atom bonded to 4 other atoms) which require a lot of energy to break Does not conduct electricity because it has no free delocalised electrons
47
Describe the structure and bonding in diamond
Giant covalent held together by lots of strong covalent bonds
48
What are the properties of graphite?
High melting point Soft/slippery Does conduct electricity because only three out of four carbon electrons in valent shell are being used so has a delocalised electron
49
Explain the properties of graphite
High melting point because it has a lot of strong covalent bonds (each C is bonded to 3 other atoms) which require a lot of energy to break Soft/slippery because the layers are held together, by weak intermolecular forces, which can slide over each other Does conducts electricity because it has delocalised electrons that are able to move through structure and carry charge
50
Why is graphite soft and slippery?
Weak intermolecular forces between layers, which means the layers can slide past each other
51
Why does graphite conduct?
As each C atom is bonded to 3 other C atoms leaves a delocalised electron which is able to move through the structure and carry a charge
52
What is graphene
A single layer of graphite
53
What are the properties of graphene?
Strong - strong, covalent bonds Can conduct electricity for the same reason as graphite
54
What are the uses of graphene?
Electronics Composites - as strong and light can be added as composite to improve strength without adding much weight
55
What are carbon nanotubes
Sheet of graphene roles as a tube, call them a cylinder shape
56
What are the properties of carbon nano tube?
Strong -strong, covalent bonds Conducts electricity -delocalised electrons free to move through structure
57
What are the uses of carbon nanoubes?
Electronics Nanotechnology Materials
58
What are fullerenes?
Molecules of carbon atoms with hollow shapes based on hexagons of carbon atoms
59
What was the first fullerene discovered?
Buckminsterfullerene C60 which is a spherical shape
60
What are the properties of fullerenes?
Strong Conduct electricity and thermal energy due to delocalised electrons
61
What are the use of fullerenes?
Drug delivery Catalysts
62
What is the structure of metallic substances
Giant lattice
63
What are the properties and bonding in a metal?
High melting points, (most) Can conduct electricity Malleable
64
Describe the structure and bonding in metal
Giant lattice Strong electrostatic attraction between positive metal ions and delocalised electrons
65
Why do metals mostly have high, melting and boiling points
Strong electrostatic attraction between positive metal ions and delocalised electrons which require lots of energy to break
66
Why do metals conduct?
They have Delocalised elections which are free to move through the structure and carry the current
67
Why are metals malleable?
Layers of atoms can slide past each other
68
Why are pure metals not suitable for many uses?
Too soft
69
What is an alloy?
A mixture of metals
70
Why are alloys harder than pure metals
Different size atoms disrupt the layers so layers of atoms can’t slide past each other as easily
71
What are the three states of matter?
Solid liquid gas
72
What takes place at the melting point
Melting and freezing
73
What takes place at the boiling point
Boiling and condensing
74
How can you represent the three states of matter?
Using a simple model represented small, solid spheres
75
What does the energy needed to change the state depend upon?
The strength of force between the particles, the stronger the force, which depends upon the bonding and structure the higher, melting point and boiling point
76
What are the limitations of the particle model
The model assumes no forces involved. All the particles represent as a spheres on the spheres are solid.
77
What are the four state symbols?
Solid (s) Liquid (l) Gas (g) Aqueous solution (aq) when something is dissolved in water
78
How are the particles arranged in a solid?
Tightly packed Regular arrangement and fix position Have a definite shape and volume Can’t be compressed
79
How are the particles arranged in a liquid?
Close together Disordered arrangement for free to move past each other Able to flow Have a fixed volume Take the shape of its container Can’t be compressed
80
How are the particles arranged in a gas
Far apart Random arrangement No fixed volume or shape Can be compressed
81
What happens to bonds/forces when melting
They are weakened
82
What happens to the bonds/forces when boiling
They are broken
83
What is gains during melting and boiling?
Energy
84
What is the name of the process turning a liquid to a gas?
Evaporation/boiling
85
What is the name of the process turning a gas to a liquid?
Condensation
86
What is the name of the process turning a liquid to a solid
Freezing
87
What is the name of the process trying a solid to a liquid
Melting
88
What is nano science?
Structures that are 1-100nm in size of the order of a few hundred atoms (1x10(-9)m
89
What size are fine particles PM2.5
Have diameters between 100-2500nm
90
What size are coarse particles PM10
Have diameters between 1x10(-5) m - 2.5x10(-6) m Referred to as dust
91
Which particles are the smallest - Nano particles, fine particles or coarse particles
Nano particles -have the smallest size
92
Give some uses of nano particles
Many applications in medicine Electronics Cosmetics Suncream Deodorant Catalysts
93
Suggest a use for a nano particle which has antibacterial properties
Bandages Wound dressings Face masks Deodorant Socks
94
Give a property of a nanoparticle if it is to be used in a computer chip?
Conduct electricity
95
What are the suggest a possible risks of using nano particles in cosmetics?
Potential cell damage to the body(small enough to pass through the skin and remain in the body) harmful effects on the environment after being washed off the skin
96
Why are catalysts in the form of nano particles more efficient?
A much higher surface area for reactions take place
97
Why did the properties of nano particles differ to bulk materials
Due to the high surface area to volume ratio, smaller quantities are needed to be as effective as normal sized particles
98
Suggest reasons why it costs less to use nano particles rather than fine particles in suncream
Greater surface area to volume ratio less can be used for the same affect
99
Give me advantage of using nano particles in sun creams than other sun creams
Better coverage More protection from the sun ultra Violet waves
100
What happens to the surface area to volume ratio when the side of a cube decreases by a factor of 10
The area to volume ratio increases by a factor of 10
101
How to workout the surface area to volume ratio
1. Calculate the area of the cube. 2. calculate the volume of the cube 3. Divide areas by the volume. 4. Write values in format surface area: volume
102
Example of a calculation to determine the service area to volume ratio of a cube with side lengths of 50nm
1. SurfaceArea = 50x50x6 —> 15000nm 2. Volume is 50x50x50 —> 125000nm 3. 15000/125000 —> 0.12nm Ratio = 0.12 : 1

GCSE Chemistry (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions