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Y10 CH > Block 1 > Flashcards

Block 1 Flashcards

1
Q

How is a compound formed?

A

When the atoms of two or more elements react chemically.

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2
Q

What is covalent bonding?

A

When two non-metals share electrons.

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3
Q

What is ionic bonding?

A

When a non-metal and metal exchange electrons.

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4
Q

What happens to form an ionic bond?

A

The atoms lose or gain electrons to form charged particles known as ions.

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5
Q

Describe what would happen to sodium (2,8,1) if it lost an electron.

A

The sodium atom would now be stable (2,8). However, it would have one more proton than electrons, so the formula of a sodium ion would be written as Na+.

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6
Q

When ionic bonding occurs, will the metal or non-metal lose electrons?

A

The metal typically loses electrons.

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7
Q

Describe what would happen to chlorine (2,8,7) if it gained an electron.

A

The chlorine atom would now be stable (2,8,8). However, it would have one more electron than protons, so the formula of a chloride ion is written as Cl-.

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8
Q

What are the forces called which hold together ions.

A

Electrostatic forces of attraction. (Ionic bonding)

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9
Q

What do the ionic bonds between the charged particles result in?

A

An arrangement of ions known as a giant lattice/giant structure.

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10
Q

Describe what would happen to magnesium (2,8,2) and oxygen (2,6) if they bonded together to form an ionic compound.

A

The magnesium atom would lose 2 electrons and become Mg2+. The oxygen atom would gain 2 electrons and become O2-. Both atoms would become stable.

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11
Q

IONIC CHARGES INFO

A

https://imgur.com/a/2dyZz7c

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12
Q

What is metallic bonding?

A

The force of attraction between delocalised electrons and positive metal ions.

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13
Q

What is meant by a ‘sea of electrons’.

A

When the electrons on the outer shells of the metal ions are delocalised which keeps the positively charged ions packed together.

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14
Q

What is a giant metallic structure?

A

When atoms in a pure metal are tightly packed together in layers.

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15
Q

Why can’t the layers of atoms in alloys slide over each other easily?

A

The atoms of other elements distort the layers.

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16
Q

Why are metals good conductors of thermal energy and electricity?

A

The delocalised electrons can carry the charge and transfer thermal energy.

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17
Q

What are copper alloys useful for and why?

A

Making statues and decorative items because it is resistant to corrosion.

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18
Q

What are aluminium alloys useful for and why?

A

Building aircraft and other vehicles because it is lightweight and strong.

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19
Q

What are gold alloys useful for and why?

A

Making jewellery because it wears away less easily than pure gold.

20
Q

What are carbon steels useful for and why?

A

Building ships, cars and machinery because it is cheap .

21
Q

What are alloy steels useful for and why?

A

Building bridges, military armour and making bicycle chains because they do not rust and are quite strong.

22
Q

Why do giant ionic lattices have high melting/boiling points?

A

Strong electrostatic forces of attraction.

23
Q

What is an ionic compound?

A

Giant structures of ions arranged in a lattice.

24
Q

In what states of matter can ionic lattices conduct electricity and why?

A

Solid - No, the ions are held in fixed positions in the lattice and therefore can’t carry a charge.

Liquid - Yes, the ions are free to move anywhere in the liquid and therefore can carry a charge.

25
Q

Explain how strong the bonds are in covalent bonds compared to bonds with neighbouring molecules.

A

Covalent bonds are held very tightly together. However, the bonds between molecules are known as weak intermolecular forces and are easily broken.

26
Q

Why do polymer chains get higher melting/boiling points as they become longer?

A

The intermolecular forces become stronger.

27
Q

What are giant covalent structures?

A

Giant structures where huge numbers of atoms are held together by strong covalent bonds.

28
Q

Give three examples of giant covalent structures.

A

Diamond, silicon dioxide and graphite.

29
Q

Give three properties of giant covalent structures.

A

High melting and boiling points because of the strong covalent bonds.

Insoluble in water. (can’t be dissolved)

Hard and do not conduct electricity (except graphite).

30
Q

Describe the covalent bonds in diamond.

A

Each carbon atom is covalently bonded to four other carbon atoms which forms a perfectly arranged symmetrical lattice.

31
Q

Describe the covalent bonds in graphite.

A

Each carbon atom is covalently bonded to three other carbon atoms in hexagonally shaped giant layers.

32
Q

Describe the bonds between the layers of graphite.

A

The bonds are intermolecular, meaning that the layers can slide over each other easily.

33
Q

Describe the electron arrangement of carbon atoms in graphite.

A

Each carbon atom has four electrons in its outer shell which are available for bonding. This leaves one spare outer electron on each carbon atom in graphite.

34
Q

Why can graphite conduct electricity?

A

Each carbon atom has one delocalised electron which does not belong to any particular carbon atom (similar to metallic structures). These delocalised electrons can carry charge and allowed graphite to conduct electricity.

35
Q

What are fullerenes?

A

Large hollow cages made out of carbon atoms.

36
Q

What are some properties of fullerenes?

A

High tensile strength and high electrical and thermal conductivity because of delocalised electrons.

37
Q

What are some uses for fullerenes?

A

Drug delivery to the body or lubricants.

38
Q

What is graphene?

A

A single sheet of carbon atoms from graphite which is one atom thick.

39
Q

What are some properties of graphene?

A

It is an excellent conductor of thermal and electrical energy, has a low density, is the most reactive form of carbon and is the hardest material ever made.

40
Q

How is glass made?

A

Sand, limestone and sodium carbonate - soda are heated to 1500 degrees Celsius and form molten glass. It cools to become a solid.

41
Q

How are ceramics made?

A

A combination of compounds of metals and non-metals are combined and heated.

42
Q

What are some properties of ceramics?

A

Hard, brittle, electrical conductors and resistant to chemical attack.

43
Q

How are composites made?

A

By combining two materials to make a product with improved properties for a particular use.

44
Q

What is nanoscience?

A

The science of really tiny things.

45
Q

Why do nanoparticles have a high surface area to volume ratio?

A

A large percentage of the atoms are exposed at the surface.

46
Q

Name some uses of nanoparticles.

A

Breaking down dirt on glass, making improved sun creams, making improved cosmetics, delivering drugs to the body through nanocages, inhibit the growth of microorganisms and making wires for electric circuits.

47
Q

What is the main downside of nanoparticles?

A

More research needs to be done on them.

Y10 CH (1 decks)

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