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GCSE Chemistry > Bonding, Structure And The Properties Of Matter > Flashcards

Bonding, Structure And The Properties Of Matter Flashcards

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1
Q

What is ionic bonding?

A

Ionic bonding is bonds that have electrostatic attraction. When oppositely charged ions form an ionic bond you get an ionic compound.

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2
Q

How are ionic compounds held together?

A

They are held together in a giant lattice, it’s a regular structure that extends in all directions in a substance and the electrostatic attraction between positive and negative ions holds the structure together.

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3
Q

State the properties of ionic substances

A

● High melting and boiling point (strong electrostatic forces between oppositely charged ions)
● Do not conduct electricity when solid (ions in fixed positions).
● Conduct when molten or dissolved in water - ions are free to move.

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4
Q

Give five examples of positive ions

A

Na+, Mg2+, Al3+, Ca2+, Rb+

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5
Q

Give five examples of negative ions

A

Cl-, Br-, O2-, S2-, I-

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6
Q

What is important when working out a formula of an ionic compound?

A

Ionic compounds are electrically neutral, i.e. positive and negative charges balance each other.

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7
Q

How are ionic compounds formed?

A

Atoms gain or lose electrons, by transferring as both metal and non metal have an incomplete outer shell

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8
Q

What is a covalent bond?

A

A chemical bond formed when two or atoms share electrons.

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9
Q

Describe the structure and properties of simple molecular covalent substances

A
  • Do not conduct electricity (no ions)
  • Small molecules
  • Weak intermolecular forces
  • Low melting and boiling points
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10
Q

How do intermolecular forces change as the mass/size of the molecule increases?

A

They increase. That causes melting/boiling points to increase as well (more energy needed to overcome these forces).

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11
Q

What are polymers?

A

very large molecules with atoms linked by covalent bonds

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12
Q

What are thermosoftening polymers?

A
  • soften when heated and shaped when hot
  • harden when cooled, but can be reshaped when heated again
  • EXAMPLE: polyethene
  • slide past each other making it flexible
  • forces between polymer chains are weak
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13
Q

What are giant covalent structures?

A

Giant covalent structures have huge networks of covalently bonded atoms. Carbon often forms this type of structure because they can each form four strong covalent bonds.

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14
Q

What are the properties of giant covalent substances?

A
  • solids, atoms covalently bonded together in a giant lattice
  • high melting/boiling points - strong covalent bonds
  • mostly don’t conduct electricity
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15
Q

Describe and explain the properties of allotropes of carbon?

A

Diamond
- four, strong covalent bonds for each carbon atom
- very hard (Strong bonds)
- very high melting point (strong bonds)
- does not conduct (no delocalised electrons)

Graphite
- three covalent bonds for each carbon atom
- layers of hexagonal rings
- high melting point
- layers free to slide as weak intermolecular forces
between layers; soft, can be used as a lubricant
- conduct thermal and electricity due to one delocalised
electron per each carbon atom

Fullerenes
- hollow shaped molecules
- based on hexagonal rings but may have
5/7-carbon rings
- C60 has spherical shape, simple
molecular structure (Buckminsterfullerene)

Nanotubes
- cylindrical fullerene with high length to
diameter ratio
- High tensile strength (strong bonds)
- Conductivity (deloc. electrons)

Graphene - a single layer of graphite.

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16
Q

What is metallic bonding?

A

Forces of attraction between delocalised electrons and nuclei of metal ions.

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17
Q

Describe the properties of metals

A
  • High melting/boiling points (strong forces of attraction)
  • Good conductors of heat and electricity (delocalised electrons)
  • Malleable, soft (layers of atoms can slide over each other whilst maintaining
    the attraction forces)
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18
Q

What are alloys? Why are they harder than pure metals?

A

Alloys:
- mixtures of metal with other elements, usually metals
- different sizes of atoms distorts the layers, so they can’t slide over each other,
therefore alloys are harder than pure metals

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19
Q

What does the amount of energy needed to change state from solid to liquid or liquid to gas depend on?

A

The strength of the forces between the particles of the substance. The nature of the particles involved depends on the type of bonding and the structure of the substance. The stronger the forces between the particles the higher the melting point and boiling point of the substance

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20
Q

What is a pure substance?

A

a substance in which there is only one type of particle

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21
Q

What temperature does a pure substance melt/boil at?

A

Fixed temperature

22
Q

What temperature does a mixture melt/boil at?

A

Over a range of temperature

23
Q

What are the three states of matter?

A

solid, liquid, gas

24
Q

What is nanoscience?

A

Science that studies particles that are 1 - 100nm in size

25
Q

State the uses of nanoparticles

A
  • Medicine (drug delivery systems)
  • Electronics
  • Deodorants
  • Sun creams (better skin coverage and more effective protection against cell damage)
26
Q

What are fine and coarse particles?

A
  • Fine particles (soot), 100-2500 nm diameter
  • Coarse particles (dust), 2500-105 nm diameter
27
Q

Why do nanoparticles have different properties to those for the same material in bulk?

A

high surface area to volume ratio

28
Q

What type of elements does ionic bonding work for?

A

Metal and non-metal

29
Q

What type of elements does covalent bonding work for?

A

Non-metal and non-metal

30
Q

What type of elements does metallic bonding work for?

A

Metals

31
Q

What are the two types of structures that a covalent bond has?

A

Simple and giant lattice

32
Q

How does a simple covalent bond form?

A

Atoms that join together by covalent bonding can form different types of covalent structures
- millions of molecules together

33
Q

How does a giant lattice of covalent bond form?

A

The atoms are join together to each other in regular arrangement
- millions of molecules together

34
Q

What are the properties of simple covalent bonds?

A
  • low melting and boiling points
  • usually soft and brittle -> shatter when hit
  • usually insoluble in water but soluble in other solvents such as petrol
  • can’t conduct electricity (no free electrons to carry an electrical charge)
35
Q

What are the properties of a giant lattice of covalent bonds?

A
  • solid at room temperature
  • high melting and boiling points
  • very strong
  • insoluble in water
  • most don’t conduct electricity
36
Q

How does a metallic bond form?

A

Each atom donates an electron in its outside shell forming an positive ion. The electrons are delocalised. The metal ions and delocalised electrons are attached together by electrostatic attraction because opposite changes

37
Q

What is the structure of metallic bonding?

A

The atoms in a metallic element are all the same size and are packed closely together in layers to form a giant lattice

38
Q

What are the properties of metallic bonding?

A
  • conduct heat
  • malleable (bent or hammered into shape)
  • ductile
  • shiny
39
Q

What does delocalised mean?

A

be shared among more than two atoms in a molecule

40
Q

What is formation of metal ions?

A

Atoms lose outer electrons

41
Q

What is the formation of non-metal ions?

A

Atoms gain electrons

42
Q

What is a lattice?

A

Regular arrangement of particles

43
Q

What are electrostatic forces of attraction?

A

Strong forces of attraction between oppositely charged particles

44
Q

Why can metals conduct heat well?

A

Delocalised electrons can transfer heat energy quickly

45
Q

Why can metals conduct electricity well?

A

Delocalised electrons can carry electrical change through the structure

46
Q

What is a triple covalent bond?

A

A bond formed by sharing three pairs of electrons

47
Q

What are intermolecular forces?

A

Forces of attraction between molecules

48
Q

What are the properties for molecular substances?

A
  • low melting and boiling points -> intermolecular forces are weak
  • larger the molecule is the stronger the intermolecular forces are
  • low conductivity of electricity -> molecules are neutral
49
Q

What is the particle theory?

A

Matter is made up of tiny particles which are represented as small solid spheres which are constantly moving -> explaining changes of states

50
Q

What is the number of bonds between atoms in diamond?

A

4 bonds

51
Q

What is allotrope?

A

Different forms of the same element

52
Q

What number of bonds between atoms in graphite?

A

3 bonds

GCSE Chemistry (9 decks)

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