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GCSE CHEMISTRY > P1- Bonding, structure, and the properties of matter > Flashcards

P1- Bonding, structure, and the properties of matter Flashcards

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1
Q

What happens to an atom if it loses an electron

A

Becomes a positive ion

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2
Q

What happens if an atom gains an electron

A

Becomes a negative ion

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2
Q

What is the drop and swap method

A

Write down the ions of the elements involved, drop the number and ignore the charge, swap the numbers over

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3
Q

What is a covalent bond

A

A bond between non-metals. It is the sharing of a pair of electrons

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4
Q

What is ionic bonding

A

Transfer of electrons between a metal and a nonmetal. Metal loses an electron making it positively charged and nonmetal gains an electron, making it negatively charged. The ions are held together by a strong electrostatic attraction between oppositely charged atoms

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5
Q

Do covalent bonds have a high or low boiling point

A

Low

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6
Q

Why do covalent bonds have a low boiling point

A

They have weak intermolecular forces between molecules which need little amount of energy to break

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7
Q

Do polymers have strong or weak forces

A

Strong intermolecular forces meaning they’re solid at room temperature

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7
Q

What is a polymer

A

A plastic made up of lots of single units called monomers that join together to from a long chain polymer

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8
Q

What are the particle diagrams

A

Dot and cross, displayed formula, ball and stick

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9
Q

Advantage of dot and cross diagram

A

Shows the bonding and which atoms the elements come from

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10
Q

Disadvantage of dot and cross diagram

A

Size of each atoms and how they are arranged in space

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11
Q

Advantages of displayed formula diagram

A

Shows bonds are single lines between atoms, good for showing how they’re bonded in large molecules

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12
Q

Disadvantage of displayed formula diagram

A

Doesn’t show which atoms the electrons have come from or the 3D structure

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13
Q

Advantages of ball and stick diagram

A

Tells us the atoms, the covalent bonds, the arrangement in space

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13
Q

Disadvantages of ball and stick diagram

A

Confusing for large molecules and doesnt tell us where electrons come fork

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14
Q

What is metallic bonding

A

Bonding in a metal, True, static attraction between positive metal ions and delocalised negative electrons

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15
Q

What are ions like in metallic bonding

A

in a regular pattern and they form crystals. They are giant lattices

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15
Q

Properties of metals in metallic bonding

A

Soft so they can slide over eachother, high melting point meaning string bonds so lot of energy needed to break, conduct electricity so have free electrons to move and carry charge throughout structure

16
Q

What is an alloy

A

A mixture of at least two elements where at least one of these is a metal

17
Q

What are the atoms like in a pure metal

A

All same size and arranged in a regular arrangement of layers meaning layers can slide over each other making it soft

18
Q

What are particles like in a liquid

A

Close together, not regularly arranged, able to move a little

18
Q

What are particles like in a solid

A

All close together and touch, regularly arranged, can’t move a lot, strong bonds

19
Q

What are particles like in a gas

A

Lot of energy, randomly move around at any soled and direction

20
Q

Process of turning solid to liquid

A

Melting

20
Q

Process of turning Gas to liquid

A

Condensation

21
Q

Process of turning liquid to gas

A

Evaporation

22
Q

Process of turning liquid to solid

A

Freezing

23
Q

Process of turning solid to gas (skipping liquid)

A

Sublimation

24
Q

What does aqueous mean

A

To be dissolved in water

25
Q

What is nanoscience

A

Referring to structures that are 1-100 nm in size (small)

26
Q

Is the surface area to volume ratio of nanoscience structure large or small

A

Large meaning only a small quantity of them are needed to be effective compared to normal particles

27
Q

Uses of nanoscience

A

Medicine , electronics, cosmetics, sun cream, deodorants, catalysts

28
Q

What do nanoparticles do (examples)

A

Get absorbed dipper in the skin in cosmetics, nano cages of gold to deliver drugs to body for cancer treatment, nano tubes for improved performance of electronic devices, nano particles in sun cream are more effective in blocking

29
Q

Examples of giant covalent structures

A

Graphite, diamond, silicon and fullerene

30
Q

How are the layers held together in graphite

A

By weak forces which are easily broken

31
Q

Properties of graphite

A

Weak forces allowing them to slide over easily, delocalised electrons carry charge throughout structure allowing graphite to conduct electricity, high melting point, soft, good electrical conductor

32
Q

How is graphite an allotrope of carbon

A

Each carbon atom is bonded to only 3 other carbon aroma meaning graphite is structured in hexagonal rings and has delocalised electrons

33
Q

What is graphite used for

A

Pencils and as a lubricant to reduce friction on moving surfaces

34
Q

How does diamond form a giant covalent structure

A

carbon atom is bonded to 4 other carbon atoms by very strong covalent bonds. there are no three electrons, so there is nothing to carry charge to the structure

35
Q

Properties of diamond

A

Very hard, extremely high melting point, high boiling point insoluble in water, doesn’t conduct electricity

36
Q

What is diamond used for

A

Jewellery and in drills for cutting through rock

37
Q

Properties of silicon

A

High melting point (1600 degrees celsius), hard, insoluble in water, poor electrical conductor, silicon dioxide is obtained by mining and purifying quartz. Silica is the main constituent of sand

38
Q

Explain fullerene

A

carbon atoms are joined together to make large cages, which can have all sorts of shapes looking like balls, onions, tubes, doughnuts, corkscrews and cones. they are built of hexagonal rings of carbon atoms

39
Q

What can fullerene be used for

A

Delivering drugs to specific parts of the body, or as a catalyst and lubricants

GCSE CHEMISTRY (9 decks)

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