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Chemistry > Structure And Bonding > Flashcards

Structure And Bonding Flashcards

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1
Q

What are bonds?

A

Forces of attraction that hold atoms together

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2
Q

What do electrostatic forces hold together?

A

Oppositely charged ions forming an ionic bind between them

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3
Q

What is a lattice structure?

A

Billions of ions packed together in a regular repeating arrangement called a lattice structure

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4
Q

Why do ionic compounds have no overall charge?

A

They are electrically neutral

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5
Q

What is the ion formula of sodium?

A

Na+

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6
Q

What is the ion formula of lithium?

A

Li+

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7
Q

What is the ion formula for potassium?

A

K+

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8
Q

What is the ion formula for magnesium?

A

Mg2+

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9
Q

What is the ion formula for calcium?

A

Ca2+

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10
Q

What is the ion formula for aluminium?

A

Al3+

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11
Q

What is the ion formula for fluoride?

A

F-

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12
Q

What is the ion formula for chloride?

A

Cl-

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13
Q

What is the ion formula for bromide?

A

Br-

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14
Q

What is the ion formula for oxide?

A

O2-

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15
Q

What is the ion formula for sulfide?

A

S2-

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16
Q

What is the ion formula for phosphide?

A

P3-

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17
Q

What 2 conditions does a substance need to conduct electricity?

A
  • just contain charged particles

- these particles must be free to move

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18
Q

What are negative ions known as?

A

Anions

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19
Q

What are positive ions known as?

A

Cations

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20
Q

What are covalent bonds formed between?

A

Between non-metal atoms

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21
Q

How are covalent bonds produced?

A

By sharing pairs of electrons

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22
Q

What are electrostatic forces of attraction between?

A

Between the positive nuclei and negative electrons in bonded atoms

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23
Q

What is a compound?

A

A substance with atoms of more than one element

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24
Q

What do intermolecular forces hold together?

A

Water molecules

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25
Q

What must be overcome when turning water into gas?

A

Intermolecular forces

26
Q

What are monomers?

A

Small simple molecules that cane be joined in a chain to form a polymer

27
Q

What do linger polymers have more of?

A

Intermolecular forces

28
Q

Why do longer polymers have higher melting and boiling points than shorter ones?

A

The longer chains tend to get tangled up with one another

29
Q

What are allotropes?

A

A different structural form of an element, e.g graphite and diamond are allotropes of carbon

30
Q

What are molecules joined together by?

A

Covalent bonds

31
Q

What is a fullerene?

A

A molecule in which each carbon atom is covalently bonded to three other carbon atoms, forming spheres or tube shapes

32
Q

Do fullerenes have high or low melting points?

A

Low

33
Q

Do fullerenes have strong or weak intermolecular forces?

A

Weak

34
Q

Is graphene a good electrical conductor?

A

Yes

35
Q

How thick is graphene

A

1 atom thick, making it the lightest known material

36
Q

Why is graphene extremely strong?

A

Covalent bonds

37
Q

Give 2 examples of covalent, giant molecular structures

A

Diamond and graphite

38
Q

Why do graphite and diamond have high melting points?

A

They have many strong covalent bonds that need to be broken down to melt the solids

39
Q

Why are not all of graphite’s electrons held in covalent bonds?

A

Has a layered structure, so not all electrons are held together by covalent bonds, these delocalised electrons are free to move and carry an electrical current

40
Q

Why is graphite used in electrolysis?

A

It conducts electricity well and is cheap and not very reactive

41
Q

Why is graphite a good lubricant?

A

The sheets in carbon atoms are held together by weak forces of attraction, these weak forces allow the layers to slide past each other, which makes graphite a good lubricant

42
Q

What do atoms in a metallic element form?

A

Lattice

43
Q

How many electrons do metals have in there outer shell?

A

1, 2 or 3

44
Q

What is metallic bonding?

A

Electrostatic attraction between the positive metal ions and negative delocalised electrons

45
Q

Do metals have high melting and boiling points?

A

Yes

46
Q

Properties of metals?

A
  • malleable
  • conduct electricity
  • conduct heat
  • high melting and boiling points
47
Q

What is electrical conductivity?

A

Allowing electricity to pass through

48
Q

What does a substance having a higher electrical conductivity mean?

A

They conduct electricity better than other substances

49
Q

Why does the electrical conductivity of a metal increase?

A

When the number of delocalised electrons increase

50
Q

Where are ionic bonds found?

A

In most compounds containing metal and non-metal atoms

51
Q

How are ionic bonds formed?

A

The loss or gain of electrons to produce oppositely charged ions that attract one another

52
Q

What is the structure of ionic bonds?

A

Billions of ions held together in a lattice structure

53
Q

Properties of of ionic bonding?

A
  • high melting/boiling points
  • many are soluble in water
  • conduct electricity when liquid but not when solid
54
Q

Where are giant covalent bonds found?

A

In a few non-metal elements and some compounds of non-metals

55
Q

When are covalent bonds formed?

A

When atoms share pairs of electrons

56
Q

Properties of giant covalent bonds?

A
  • high melting /boiling points
  • insoluble in water
  • most do not conduct electricity (except carbon as graphite)
57
Q

Where are simple molecular bonds found?

A

In most non-metal elements and compounds

58
Q

Properties of simple molecular bonds?

A
  • low melting/boiling rates
  • insoluble in water
  • conduct electricity when solid or liquid
59
Q

Where are metallic bonds found?

A

In all metals

60
Q

What are metallic bonds?

A

Electrostatic attraction between positive metal ions and negative delocalised electrons

Chemistry (8 decks)

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