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IGCSE Chemistry > Structure and Bonding 1.37-1.60C > Flashcards

Structure and Bonding 1.37-1.60C Flashcards

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1
Q

What is an ion and how are they formed?

A

Charged particle

Formed by gain or loss of electrons which dictates the charge of an ion

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2
Q

What is a cation and how is it formed?

A

Positive ions - lose electrons

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3
Q

What is an anion and how is formed?

A

Negative ion - gain electrons

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4
Q

How do groups 1,2 and 3 (metals) form ions?

A

Lose electrons to form positive ions
Group 1 = 1+
Group 2 = 2+
Group 3 = 3+

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5
Q

How do groups 5,6, and 7 (non-metals) form ions?

A

Gain electrons to form negative ions
Group 5 = 3-
Group 6 = 2-
Group 7 = 1-

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6
Q

What is the charge of Ag?

A

+

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7
Q

What is the charge of Cu?

A

2+

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8
Q

What is the charge of Fe (II)?

A

2+

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9
Q

What is the charge of Fe (III)

A

3+

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10
Q

What is the charge of Pb?

A

2+

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11
Q

What is the charge of Zn?

A

2+

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12
Q

What is the charge and formula of hydrogen?

A

H+

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13
Q

What is the charge and formula of hydroxide?

A

OH-

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14
Q

What is the charge and formula of ammonium?

A

NH4+

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15
Q

What is the charge and formula of carbonate?

A

CO3^2-

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16
Q

What is the charge and formula of nitrate?

A

NO3^-

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17
Q

What is the charge and formula of sulfate?

A

SO4^2-

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18
Q

What happens when a metal reacts with a non-metal?

A

Ionic compound
Metal loses electrons = Positive ion
Non-metal gains electrons = Negative ion
These ions are strongly attracted to one another by electrostatic attractions - ionic bond

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19
Q

Define ionic bond

A

The strong electrostatic force of attraction between positive and negative ions

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20
Q

How are ionic compounds represented?

A

Dot and cross diagrams

21
Q

What structure do ionic compounds have?

A

Giant ionic lattice

22
Q

Why do ionic compounds have high melting and boiling points?

A

Structure - they have a giant ionic lattice structure
Bonding - Held together by the strong electrostatic force of attraction between positive and negative ions
Energy - a large amount of energy is required to break the attraction to melt the substance

23
Q

Can ionic compounds conduct electricity and why?

A

Can in solution and molten NOT solid
Solid - ions are fixed in the lattice (no charged particles can move)
Molten and solution - ions no longer fixed and free to move

24
Q

What are the conditions for electricity?

A

Charged particles that can move

25
Q

What types of element is covalent bonding between?

A

Non-metal and non-metal

26
Q

Define covalent bonding

A

The strong electrostatic force of attraction between the negatively charged shared pair of electrons and the positive nuclei of both atoms in the bond

27
Q

ON PAPER draw the dot and cross diagrams of:
hydrogen, chlorine, hydrogen chloride, ammonia, nitrogen, oxygen, water, methane, carbon dioxide, chloromethane, ethane, ethene

A
28
Q

What is a simple molecules substance?

A

Substance made up of molecules (which are joined together by covalent bonds) - weak intermolecular forces of attraction between molecules

29
Q

Why do simple molecular structures have low melting/boiling points?

A

Structure - simple molecular structure
Bonding - weak intermolecular forces of attraction
Energy - not much energy is required to break the weak intermolecular forces of attractions between molecules

30
Q

Why do melting and boiling increase as molecular mass increase? (simple molecular substances)

A

Intermolecular forces of attraction become stronger as relative molecular mass increases so more energy is needed to break the attraction = higher boiling point

31
Q

Can simple molecular substances conduct electricity?

A

No because the molecules don’t have any overall electrical charge (no ions) and all electrons are held tight in atoms or in covalent bonds so cannot move from molecule to molecule

32
Q

Why do giant covalent structures have high melting and boiling points?

A

Structure - giant covalent lattice structure
Bonding - held together by strong covalent bonds
Energy - therefore a large amount of energy is required to break the bonds

33
Q

Why is diamond very hard?

A

Made up of carbon atoms in a rigid tetrahedral lattice that each form 4 covalent bonds

34
Q

Why can diamond and giant covalent structures not conduct electricity?

A

Electrons are localised in covalent bonds
Atoms are localised
Therefore no charge particles can move

35
Q

How does the structure of graphite differ from other giant covalent structures?

A
  • Each carbon atom only forms three covalent bond so they are arranged in layers of hexagons
  • Weak forces of attraction between layers
36
Q

Does graphite have a high or low melting point and why?

A

High

  • Giant covalent lattice structure with strong covalent bonds
  • Need lots of energy to overcome the forces of attraction
37
Q

What is a characteristic of graphite as a material and explain why this is

A

Soft material

Weak forces of attraction between the layers so slide over each other easily

38
Q

Does graphite conduct electricity and why?

A

Yes
Only 3 out of each carbon’s four outer shell electrons are used in bonds so each carbon has one delocalised electron which is free to move

39
Q

Does C60 fullerene have a low or high melting/boiling point and why?

A

Structure - simple molecular structure
Bonding - weak intermolecular forces of attraction between molecules
Energy - not a lot of energy required to overcome the forces of attraction

40
Q

Why is C60 soft and slippery?

A

Weak intermolecular forces of attraction so molecules slide over each other easily

41
Q

Can C60 fullerene conduct electricity? Explain why

A

Electrons are localised on each molecules
Molecule is neutral overall
Therefore no charged particles can move

42
Q

Define metallic bonding

A

The strong electrostatic force of attraction between the positive ions and delocalised electrons

43
Q

Do metallic bonded substances have high or low melting/boiling points?

A

High
Structure - Giant metallic lattice
Bonding - strong electrostatic forces of attraction between positive ions and delocalised electron
Energy - large amount of energy needed to break bonds

44
Q

Do metals conduct electricity and heat?

A

Yes
Sea of delocalised electrons which can move
Movement of electrons means energy can be transferred quickly through the material, so metals are good conductors of heat

45
Q

Describe the structure of metallic bonding

A

Sea of delocalised electrons

Giant lattice of positive ions

46
Q

What does malleable mean?

A

Can be hammered or rolled into flat sheets

47
Q

Why are metals malleable?

A

The atoms are arranged in layers

Easy for the layers of atoms to slide over each other

48
Q

What is an alloy?

A

A mixture of two or more metals

IGCSE Chemistry (10 decks)

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