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GCSE Revision Flashcards > C2 Structure And Bonding > Flashcards

C2 Structure And Bonding Flashcards

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1
Q

Ionic substances can not conduct electricity unless…

A

They are molten or in solution (aq)

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2
Q

Metals can conduct electricity: True or False?

A

True. They can also conduct thermal energy.

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3
Q

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

A

When aqueous, ions move place to place and are free to carry a charge.

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4
Q

Ionic substances have high melting and boiling points because…

A

They contain strong ionic bonds, which require more energy to overcome.

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5
Q

Do metals have high or low melting and boiling points?

A

High

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6
Q

Why do metals have high melting and boiling points?

A

Metallic bonds are strong and require lots of energy to overcome.

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7
Q

Alloys are stronger than metals: True or False?

A

True. Alloys are much stronger.

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8
Q

What type of bonding was NON-METAL + NON-METAL?

A

Covalent

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9
Q

What type of bonding was METAL + METAL?

A

Metallic

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10
Q

What type of bonding was METAL + NON-METAL?

A

Ionic

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11
Q

Do ionic bonds have high or low melting points?

A

High melting/boiling points - strong electrostatic attraction between oppositely charged ions

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12
Q

Can ionic bonds conduct electricity?

A

Only when molten or in solution

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13
Q

What happens during ionic bonding?

A

Electrons are transferred to gain full outer shells

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14
Q

Which ions are attracted to each others?

A

Oppositely charged ions - electrostatic attraction

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15
Q

What substances are ionic bonds found in?

A

Ionic compounds

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16
Q

What are ionic bonds held together by?

A

Electrostatic attraction between oppositely charged ions

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17
Q

What are ionic compounds?

A

Consist of a regular arrangement of positive and negative ions

18
Q

When are giant ionic structures/lattices formed?

A

Formed by oppositely charged ions being attracted together

19
Q

What type of compounds contain covalent bonding?

A

Covalent compounds

20
Q

What is a covalent bond?

A

When electrons are shared to gain full outer shells

21
Q

What do covalent bonds result in?

A

Simple molecular or giant covalent structures

22
Q

What is the name of group 1 elements?

A

Alkali metals

23
Q

What is the charge of group 1 on the periodic table?

A

+1

24
Q

What is the name of the group 2 elements?

A

Alkaline Earths

25
Q

What is the charge of group 2 on the periodic table?

A

+2

26
Q

What is the charge of group 7 on the periodic table?

A

-1

27
Q

What is the name of group 7 on the periodic table?

A

Halogens

28
Q

What is the name of group 0 on the periodic table?

A

Noble Gases

29
Q

What is the charge of group 0 on the periodic table?

A

0

30
Q

What is the charge of group 6 on the periodic table?

A

-2

31
Q

What is the charge of atoms which gain electrons?

A

Atoms which gain electrons have a negative charge - reduced

32
Q

What is the charge of atoms which lose electrons?

A

Atoms which lose electrons have a positive charge - oxidised

33
Q

What is metallic bonding?

A

Involves electrons being delocalised

34
Q

What elements feature metallic bonding?

A

Metals

35
Q

What does metallic bonding result in?

A

Giant metallic structures

36
Q

What do metals consist of?

A

A regular arrangement of positive ions in a sea of delocalised electrons

37
Q

Why are metals malleable (what holds them together)?

A

Held together by delocalised electrons makes it malleable

38
Q

What are metallic structures held together by?

A

Strong electrostatic forces caused by this arrangement

39
Q

Do metals have high/low boiling points?

A

High melting/boiling points

40
Q

Why do metals have high melting and boiling points?

A

Lots of energy required to overcome these electrostatic forces

41
Q

Why do metals conduct electricity?

A

They contain free delocalised electrons which move around and carry a charge

42
Q

What do ionic bonds consist of?

A

Strong electrostatic attraction between oppositely charged ions

GCSE Revision Flashcards (21 decks)

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