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Chemistry > Bonding,10 > Flashcards

Bonding,10 Flashcards

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1
Q

Observation during chemical reactions

A

Observation during chemical reactions:
1. Change in state
2. Fizzing or bubbling
3. Colour change
4. Temperature
5. Sound produced

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2
Q

Why atoms bond became more stable?

A

Atoms bond to become more stable. To do this they need to achieve “noble gas configuration”

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3
Q

Characteristics about atoms

A
  • atoms can either gain or lose electrons in ionic bonding.
  • which they do depends on how many electrons they have on their outer shell.
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4
Q

Metals

A

Metals lose electrons and form POSITIVE ions.

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5
Q

Non-metals

A

Non-metals gain electrons and form NEGATIVE ions

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6
Q

Charged particles of ions

A

Ions are charged particles formed when atom or groups of atoms gain or lose electrons.

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7
Q

Melting points of ionic compounds

A

Ionic compounds have high melting points and boiling points

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8
Q

Electrostatic forces between ions are:

A

Strong electrostatic forces between ions.

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9
Q

Ionic atoms are…

A

Brittle

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10
Q

When ionic compounds conduct electricity

A

Ionic compounds only conduct electricity when melted ( related to liquid state ) or dissolved in a solution.

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11
Q

Why ions needs to be free

A

Ions need to be free to move and carry charge

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12
Q

Writing formula

A

Group 1 => +1 Group 4 => -3
Group 2 => +2 Group 5 => -2
Group 3 => +3 Group 6 => -1

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13
Q

Covalent molecules, state of matter

A

Simple covalent molecules are liquid or gas at room temperature, eg water, methane and oxygen. They have low melting and boiling points.

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14
Q

Covalent bond

A

Covalent bond = shared pair of electrons

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15
Q

Covalent compounds has weak…. and strong…..

A

Weak intermolecular forces, which require little energy to break.

Strong covalent bond ( requires lots of energy to break)

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16
Q

Polymers

A

Polymers are very large molecules made when hundreds of monomers join together to form long chains.

17
Q

Plastic

A

Plastics are synthetic polymers that can be shaped by heat a pressure.

18
Q

State of matter of plastic

A

Plastics are solid at room temperature. They have high melting and boiling points.

19
Q

Monomers

A

Polymers are made of monomers.
No longer has double bond as this has broken to join monomer together.

20
Q

Size, type of bonding, intermolecular, conductor of electricity, state at room temperature, POLYMER

A

Size:
large molecules.

Type of bonding:
strong covalent bonding within chains

Intermolecular forces:
weak intermolecular forces of attraction between small molecules.

Conductor of electricity:
poor conductor of electricity

State at room temperature:
solid at room temperature

21
Q

Size, type of bonding, intermolecular, conductor of electricity, state at room temperature, SIMPLE MOLECULE

A

Size:
small molecules

Type of bonding:
strong covalent bonding within small molecules

Intermolecular forces:
many weak intermolecular forces of attraction.

Conductor of electricity:
poor conductor of electricity

State at room temperature:
often a gas or liquid at room temperature

22
Q

Diamond and Graphite are….

A

Diamond and Graphite are allotropes of carbon, which are different forms of the same element it is the arrangement of atoms that is responsible but the different properties.

23
Q

Graphite - giant covalent

A
  • each carbon covalently bonded to 3 others.
  • 1 delocalised electron free to carry charge ( electrons).
  • weak intermolecular forces between layers, easily broken, so layers slide (pencils).
  • high melting points ( strong covalent bonds ).
  • uses: pencils, lubricant, electrodes.
23
Q

Diamond - giant covalent

A
  • each electron covalently bonded to 4 others.
  • no free electrons, so does not conduct electricity.
  • hard substance: strong covalent bonds.
  • high melting point: strong covalent bonds require lots of energy to break.
  • uses: jewellery, cutting tools.
24
Q

Fullerenes - simple molecular

A
  • low melting and boiling points, there are weak intermolecular forces between molecules.
  • each carbon covalently bonded to 3 others.
  • conduct across surface.
  • slide over each other.
25
Q

Graphene - giant covalent

A
  • single layer of graphite.
  • 1 atom thick.
  • conducts across surface due to delocalised electrons.
  • each carbon covalently bonded to 3 others.
  • high melting point as covalent bonds require lots of energy to break.
26
Q

Ionic (metals and non-metals)

A

Between metal and non-metal electrons transferred.

27
Q

Covalent (metals and non-metals)

A

Between 2 non-metals shared pair of electrons

28
Q

Metallic (metals and non-metals)

A

Bonding within a metal

29
Q

Lattice (metals and non-metals)

A

Structure regular repeating pattern

30
Q

Delocalised (metals and non-metals)

A

Metals can conduct electricity

31
Q

Metallic bonding, force

A

Strong electrostatic force of attraction between positive metal ions and negative delocalised electrons.

32
Q

Bonding models. Dot and cross diagram.

A

+ show how electrons are shared.
+ explains how we get formula.
- implies electrons differs from different atoms.
- does not show shape of molecule.
- does not show relative size of atom.

33
Q

Bonding models. 3-D image filling model

A

+ shows relative size of atom.
+ show shape of molecule.
- does not explain how bonds are formed.
- does not show the number of bonds.

34
Q

Bonding models, displayed formula

A

+ shows which atoms joined together.
+ can show shape ( 3-D ball + stick)
+ shows formula.
- does not always show shape.
- implies atoms held together with sticks.
- does not show relative size of atom.

35
Q

Bonding models, ionic models

A

+ shows lattice structure.
+ explains why the structure conducts electricity.
- does not show ions viorating.

Chemistry (7 decks)

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