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C2 Knowledge Organiser > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

1
Q

Compound

A

A substance with two or more elements chemically bonded

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2
Q

Chemical bond

A

Involves either transferring (losing or gaining) OR sharing electrons in the highest occupied energy levels (shells) of atoms in order to achieve the electronic structure of a noble gas.

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3
Q

Element

A

A substance that is made from one type of particle – named on the periodic table.

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4
Q

Mixture

A

A substance with two or more elements that is not chemically bonded and therefore can be separated.

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5
Q

Giant Covalent Structure

A

Made of only non-metal elements

Each atom is joined to adjacent atoms by covalent bonds.

The atoms are usually arranged into giant regular lattice.

Examples: Graphite, Diamond, Silicon dioxide

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6
Q

Describe Graphite

A

Each carbon atom forms three covalent bonds.

Sheet of carbon atoms are arranged into layer.

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7
Q

Properties of Graphite

A

Used for pencils and as a lubricant.

High melting point:

Conducts:

insolubility/does not dissolve

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8
Q

Explain why Graphite can be used for pencils and lubricants.

A

Layers can slide over each other therefore can be used for pencils and as a lubricant

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9
Q

Explain the melting point of Graphite

A

High melting point: -

3 strong covalent bonds need to be broken

therefore requires lots of energy to break these covalent bonds.

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10
Q

Explain why Graphite can conduct electricity

A

Conducts because each carbon has an electron that is free (or delocalised)

so can move through the whole structure.

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11
Q

Explain the solubility of graphite

A

Not soluble as water cannot separate the layers or atoms

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12
Q

Describe the bonding of diamond

A

Each carbon atom forms 4 covalent bonds to 4 carbon atoms

in an extended lattice structure

resulting in a rigid structure.

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13
Q

Properties of Diamond

A

High melting point:

Does not conduct

insoluble/not soluble

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14
Q

Explain the melting point of diamond

A

4 strong covalent bonds need to be broken

therefore requires lots of energy to break to these covalent bonds

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15
Q

Explain the conductivity of diamond

A

Does not conducts

because no electrons

to transfer charge through whole of the structure.

as the electrons are in covalent bonds

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16
Q

Explain the solubility of diamond

A

Insoluble/Not soluble

as water cannot separate the carbon atoms

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17
Q

Describe the bonding of silicon dioxide

A

Each silicon forms covalent bonds to 4 oxygen atoms and each oxygen forms 2 covalent bonds to silicon atoms,

which results in a rigid lattice structure.

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18
Q

Properties of silicon dioxide

A

High melting point

Does not conducts

insoluble/not soluble

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19
Q

Explain the melting point of Silicon dioxide

A

High melting point:

Each silicon has 4 strong covalent bonds need to be broken

therefore requires lots of energy to break.

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20
Q

Explain the conductivity of silicon dioxide

A

Does not conducts

because no electrons

to transfer charge through whole of the structure.

as the electrons are in covalent bonds

21
Q

Explain the solubility of silicon dioxide

A

insoluble /not soluble

as water cannot separate the carbon atoms

22
Q

Covalent bond

A

Chemical bond that involves the sharing of electron pairs between atoms.

23
Q

Electron configuration

A

Description of how the electrons are arranged. E.g. 2, 8, 8 or Dot-cross diagrams.

Element have the same number of electrons in outer shell as it group number (Group 0 having a full shell)

Ions have a full outer shell of electrons

24
Q

Covalent compounds

A

Compounds formed between non-metal atoms.

Each bond consists of a shared pair of electrons, and is very strong.

Covalently bonded substances fall into two main types:

  1. Simple covalent and
  2. Giant covalent structures.
25
Q

Describe Simple covalent

A

Made of only non-metal elements only

These contain only a few atoms held together by strong covalent bonds.

usually small molecules like chlorine, bromine, iodine, water, ammonia, hydrogen, oxygen, nitrogen, etc

26
Q

Properties of simple covalent compounds

A

Low melting points:

Does not conduct electricity

27
Q

Explain why simple covalent compounds have a low melting point.

A

Due to weak intermolecular bonds

between molecules

that do not require much energy to break.

28
Q

Explain why simple covalent compounds do not conduct electricity.

A

They do not have any free electrons or ions

Hence no overall electric charge.

29
Q

Ions

A

Atoms that have lost electrons and are positively charged

OR

atoms that have gained electrons and are negatively charged.

30
Q

Ionic bond

A

Chemical bond

that involves the electrostatic attraction

of oppositely charged ion.

31
Q

Positive ion

A

Atoms that have lost electrons

so have more protons than electrons.

32
Q

Negative ion

A

Atoms that have gained electrons

so have more electrons than protons.

33
Q

Describe the Ionic lattice Structure

A

Made from Metal and non-metal ions

Closely packed rows

of alternating positive and negative ions:

34
Q

Properties of ionic compounds

A

High melting point:

Conducts when dissolved and molten

Does not conduct when solid

35
Q

Explain the melting point of ionic compounds.

A

High melting point

Due to strong electrostatic attraction between oppositely charged ions

that require a lot of energy to break.

36
Q

Explain the conductivity of ionic compounds when dissolved or molten.

A

Conducts electricity

when dissolved and molten as the ions are free to move

and transfer the charge.

37
Q

Explain the conductivity of ionic compounds when Solid

A

Does not conduct electricity

ions are fixed in a lattice structure

cannot transfer the charge.

38
Q

Metallic bond

A

Chemical bond that involves the electrostatic attraction

between positive ion and delocalised electrons.

39
Q

Describe the Metallic lattice structure

A

Closely packed rows of positive ions

and a sea of free/delocalised electrons

40
Q

Properties of Metals

A

High melting point

Conducts

Can be easily shaped or bend

41
Q

Explain the melting point of metals

A

High melting point:

strong electrostatic attraction between positive metal ion and delocalised electrons

which required lots of energy to break

42
Q

Explain why metals can conduct electricity

A

Due to the free delocalised electron

that can move through the whole structure.

43
Q

Explain why metals can conduct heat

A

Due to the free delocalised electron

that can move and transfer heat through the whole structure

44
Q

Explain why metals can be easily shaped or bend

A

because the positive ions arranged in layers

which can easily slide over each other.

45
Q

Alloy

A

Made from two or more different metals.

46
Q

Explain why alloys are stronger than pure metals

A

Alloys have different sized ions in the metal

distorts the layers (of positive ions) in the structure.

making it more difficult for them to slide over each other.

47
Q

Memory Shape Alloys

A

Returns to their original shape after being deformed (reshaped) –

usually by warming up the metal.

48
Q

Nitinol

A

Example of a memory shape metal

used in braces for teeth

C2 Knowledge Organiser (8 decks)

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