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Chemistry GCSE > Topic 1: Bonding, Structure and Properties > Flashcards

Topic 1: Bonding, Structure and Properties Flashcards

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1
Q

What are the properties of metals? (8)

A

Strong, malleable and ductile, high melting and boiling points, good conductors of electricity and heat, high density, shiny when polished, reacts with oxygen to form basic oxides.

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2
Q

What metal is a particularly good conductor of electricity and heat?

A

copper

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3
Q

What is a lattice?

A

A regular arrangement of ions.

All solid metals are structured like this

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4
Q

What is an ion?

A

Electrically charged particles formed when atoms lose or gain electrons.

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5
Q

What is a metallic bond?

A

The force of attraction between the free moving electrons and positive metal ions.

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6
Q

Why is copper a good thermal conductor?

A

It’s a metal. the free electrons move faster as they are heated and transfer heat throughout the structure.

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7
Q

What is an ionic bond?

A

When metals react with non-metals, electrons are transferred from the metal atoms to the non-metal atoms, forming ions.

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8
Q

What is an ionic compound?

A

Ionic compounds are ones in which the particles are joined by ionic bonds.

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9
Q

What happens when sodium and chlorine react together?

A

It becomes sodium chloride.
The sodium atoms will become sodium ions as they have lost an electron and the chlorine atoms will become chloride ions because they’ve gained an electron.

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10
Q

How are ionic bonds formed?

A

The transfer of electrons from one atom to another.

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11
Q

Why are the ionic compounds neutral?

A

The number of positive charges balances the negative charges.

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12
Q

what is calcium chloride written as?

A

CaCl₂

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13
Q

Which metals are less lustrous?

A

The more reactive ones.

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14
Q

what does a giant ionic lattice have?

A

Strong electrostatic forces of attraction acting in all directions between the oppositely charged ions.

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15
Q

When will there be no electrical conduction?

A

When there are no moving charges particles.

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16
Q

What is a covalent bond?

A

A type of bond formed when two non-metal atoms share a air of electrons.

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17
Q

What is it called when two or more atoms join together by a covalent bond?

A

A molecule.

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18
Q

What are the properties of covalent compounds?

A

Low melting and boiling points and do not conduct electricity.

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19
Q

Why is diamond stronger than graphite despite both being made from carbon?

A

Diamond: each carbon atom forms 4 covalent bonds in a tetrahedral structure.

Graphite: the carbon atoms only form 3 covalent bonds, creating hexagonally packed layers of carbon. The layers= bonded by weaker intermolecular forces.

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20
Q

What are 4 physical properties of a diamond?

A

Transparent and crystalline, extremely hard, electrical insulator and very high melting point (over 3500 degrees)

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21
Q

What are 4 physical properties of graphite?

A

grey/black shiny solid, very soft, non-metal that conducts electricity and very high melting point (over 3600 degrees)

22
Q

How is a covalent bond formed?

A

Two or more atoms share electrons.

23
Q

Why are most covalent compounds a gas or liquid at room temperature?

A

They have low melting and boiling points because the bonds between molecules are weak.

24
Q

Why is graphite a good lubricant?

A

The layers in the graphite molecules can slide over one another (because the bonds between the layers are very weak).

25
Q

Why is diamond so hard?

A

There are a large number of bonds holding the carbons atoms together in a lattice.

26
Q

What are the fullerenes?

A

A group of allotropes of carbon.

27
Q

What is an allotrope?

A

Different physical forms of the same substance. (Diamond and graphite are allotropes of carbon).

28
Q

What are fullerenes made of?

A

Balls, ‘cages’ or tubes of carbon atoms.

29
Q

What is a nanotube?

A

Molecular scale tubes of graphite - like carbon with remarkable properties.

30
Q

What are nanotubes a type of?

A

Fullerene.

31
Q

What is an electron?

A

Subatomic particle with a negative charge and a negligible mass relative to protons and neutrons.

32
Q

What are electrostatic forces?

A

Force of attraction between particles with opposite charges.

33
Q

What is an atom?

A

All elements are made of atoms. An atom consists of a nucleus containing protons and neutrons surrounded by electrons.

34
Q

What is a molecule?

A

A collection of two or more atoms help together by chemical bonds.

35
Q

What is an intermolecular force?

A

Forces between molecules.

36
Q

What is an element?

A

A substance made of one type of atom only.

37
Q

What is the nucleus? (atom)

A

The central part of an atom. It contains protons and neutrons, and contains most of the mass of the atom.

38
Q

What is a crystal?

A

A solid containing particles (atoms, molecules or ions) joined together to form a regular arrangement or repeating pattern.

39
Q

Why do ionic compounds have high melting and boiling points?

A

It takes a lot of energy to overcome the strong electrostatic forces of attraction between oppositely charged ions.

40
Q

Why do covalent bonds have low melting and boiling points?

A

The attractions between molecules are easy to overcome.

41
Q

What nano-particle is found in sun cream?

A

Titanium oxide nano-particles.

42
Q

What is a thermochromic pigment?

A

A pigment that forms the basis of special paint that change their colour at a specific temperature.

43
Q

What are 2 examples of materials with thermochromic pigment?

A

Colour changing mugs and battery power indicators

44
Q

What is a photochromic pigment?

A

A pigment that changes colour with light intensity.

45
Q

What is an example of a material with photochromic pigment?

A

Photochromic lenses in glasses.

46
Q

What are shape-memory polymers?

A

‘Plastics’ that can regain their shape when heated.

47
Q

What is shape retention?

A

When a property remembers its original shape and returns to it (after being reheated).

48
Q

What are 2 examples of shape-memory polymers?

A

The sealing around window frames and gum-shields.

49
Q

What are shape-memory alloys?

A

Metal alloys that regain their original shape when heated.

50
Q

What are 2 examples of shape-memory alloys?

A

Surgical plates for joining bone fractures and surgical wires that replace tendons.

51
Q

What are polymer gel?

A

Hydrogels are polymer gels that absorb or expel water and swell/shrink due to changes in pH or temperature.

52
Q

What are 2 examples of polymer gels?

A

Artificial muscles and fillings for nappies.

Chemistry GCSE (7 decks)

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