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Thornhill Academy Year 9 Chemistry > Topic 2 - Bonding > Flashcards

Topic 2 - Bonding Flashcards

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1
Q

What does an ionic bond form between?

A

metal and non-metal

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2
Q

What does a covaltent bond form between?

A

non-metal and non-metal

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3
Q

What does a metallic bond form between?

A

metal and metal

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4
Q

How does an ionic bond form?

A

The metal loses electrons to become a positively charged ion, the non-metal gains electrons to become a negatively charged ion

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5
Q

How does a covalent bond form?

A

non-metals share pairs of electrons to gain full outer shells

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6
Q

How does a metallic bond form?

A

Metals lose their outer shell elctrons into a sea of delocalised electrons

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7
Q

Elements in group 0 will form ions with what charge?

A

Group 0 don’t form ions because they already have a full outer shell

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8
Q

When are elements stable?

A

When they have a full outer shell of electrons

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9
Q

In ionic bonding, how are ions held together?

A

Electrostatic forces of attraction

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10
Q

Explain how Calcium Oxide forms. Remember Calcium is in gorup 2 and Oxygen is in group 6

A

Calcium loses electrons becoming a positive ion and Oxygen gains electrons becoming a negative ion

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11
Q

Do ionic compounds have high or low melting points?

A

Ionic compounds have high melting points

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12
Q

Why do ionic compounds have high melting points?

A

Ions are held together by strong electrostatic forces of attraction

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13
Q

How are ions arranged in an ionic compound?

A

Giant ionic lattice

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14
Q

Can ionic compounds conduct electricity?

A

Yes but only when molten or dissolved in water

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15
Q

Why can ionic bonds only conduct electricity when molten or in a solution?

A

When solid, the ions in an ionic compounds can’t move. When molten or in solution th ions are free to move

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16
Q

Define the term: dissociate

A

To separate into separate ions. We talk about dissociation in terms of ions in ionic compounds dissociating when in a solution

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17
Q

True or False: All simple covalent molecular substances are insoluble in water

A

False, Some simple molecular substances are soluble and some are insoluble

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18
Q

Is a covalent bond strong?

A

A single covalent bond is very strong. It is extremely hard to try and bbreak a bond where they are sharing electrons.

19
Q

Why don’t simple molecular substances conduct electricity?

A

There is no charged ions and there is no free electrons that can move to carry electricity

20
Q

Why do simple molecular substances have low melting and boiling points?

A

Simple molecular substances have low melting and boiling points because there was weak intermolecular force of attraction between moleculs that can easily be broken.

21
Q

H2 and CH4 are both covalent compounds. Which would have the highest boiling point?

A

CH4 would have the highest boiling point. The larger the molecule the stonger the intermolecular forces, meaning the more energy needed to break them.

22
Q

Define the term: allotrope

A

Different forms of the same element, for example diamond and graphite are both made from carbon

23
Q

What element is graphite made from?

A

Carbon

24
Q

What element is damond made from?

A

Carbon

25
Q

What is the structure of diamond?

A

Diamong is a tetraheadral structure, where each carbon is covalently bonded to 4 other carbons

26
Q

What is the structure of graphite?

A

Graphite is layers of graphene sheets, with forces acting between the sheets. Each carbon is bonded to 3 other carbon atoms in a hexagonal structure

27
Q

What is the difference between graphite and graphene?

A

Graphene is a single layer of hexagonal lattice structure, where a carbon is bonded to 3 other carbons. Graphite, is layers of graphene sheets

28
Q

Can diamond conduct electricity?

A

No. There are no free electrons in diamond

29
Q

Can graphite conduct electricity?

A

Yes. There are free electrons that can move throughout the structure

30
Q

Why do giant covalent substances have high melting points?

A

They have high melting points because of the strong covalent bonds between the atoms

31
Q

Explain how the structure and bonding of graphite makes it a suitable material for lubricants.

A

Graphite has a layered structure, with only weak forces of attraction between the layers. The layers can break away from each other, makng graphite soft and slippery

32
Q

Describe the structure of fullerenes

A

Fullerenes are molecules of carbon, shaped likeclosed tubes or hollow balls. They have a huge surface area, so many catalyst molecules could be attached to each fullerene

33
Q

Why is graphite used for electrodes?

A

Graphite has the ability to conduct electricity due to the free electrons. Carbon is also unreactive which makes it safer to use in electrodes

34
Q

Where on the periodic table are metals found?

A

Towards the left of the periodic table

35
Q

Describe the bonding in a metal

A

The bonding in a metal consists of strong electrostatic forces of attraction between positive metal ions and the delocalised electrons.

36
Q

Explain why metlas can conduct electricity

A

The have delocalised electrons that can pass through the structure

37
Q

Explain why metlas can conduct heat

A

The have delocalised electrons that can pass through the structure

38
Q

Explain why metals are malleable and ductile

A

Mtels have a layered structure. The layers can slide across each other, meaning when a pressure is applied the layers move.

39
Q

Explain why metals have a high melting and boiling point

A

Metals ions and the delocalised elctrons are held together by strong electrostatic forces of attraction. The electrostatic forces need a large amount of energy to be overcome

40
Q

Define the term: Alloy

A

An allow is a mixture of metals or a mixture containing at least one metal.

41
Q

Why are alloys stonger than pure metals?

A

An alloy has more than one type of atom. The atoms are different sizes, which makes it harder for the layers to pass over each other

42
Q

What type of ions do metals form?

A

Metals always form positive ions

43
Q

What type of ions do non-metals form?

A

Non-metals always form negative ions

Thornhill Academy Year 9 Chemistry (1 decks)

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