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GCSE - Chemistry (Old) > Bonding and structures > Flashcards

Bonding and structures Flashcards

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1
Q

What is a covalent bond?

A

When two or more atoms share pairs of electrons

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2
Q

With which atoms do covalent bonds form?

A

Two non-metals

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3
Q

What type of bonding forms between two oxygen atoms?

A

Double covalent bonds

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4
Q

What type of bonding forms between two nitrogen atoms?

A

Triple covalent bonds

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5
Q

Why do non-metals form covalent bonds?

A

To complete their outer energy shell

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6
Q

Are covalent bonds strong or weak ?

A

Very strong

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7
Q

What are the two types of substances that can be made from covalent bonds?

A

Simple molecular substances and giant covalent structures

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8
Q

What are the characteristics of a simple covalent molecule?

A
  • Only NON-METAL atoms
  • Strong bonds IN molecules
  • Weak forces BETWEEN molecules
  • When broken heated, molecules are not split apart so low boiling point
  • Varied Solubility
  • Poor Conductor
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9
Q

In simple covalent molecules, what allows them to have a low boiling point?

A

Weak intermolecular forces of attraction require little energy to be broken

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10
Q

What are most simple molecular molecules at room temperature?

A

Gases or liquids

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11
Q

Learn these examples of simple covalent molecules

A

Chlorine
Oxygen
Water

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12
Q

What are the properties of giant covalent structures?

A
  • Only NON-METALS
  • High Melting Point
  • Insoluble in Water
  • Poor Conductor
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13
Q

What is the only exception to the property that giant covalent structures are poor conductors?

A

Graphite, free electron can carry a charge

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14
Q

Properties of graphite

A
  • 3 Bonds per Carbon
  • Free Electrons
  • Layers which make it soft and slippery
  • Conductor
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15
Q

Diamond

A
  • 4 Bonds per Carbon
  • No Free Electrons
  • Hard
  • Not a Conductor
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16
Q

Main use of graphite

A

Lubricant, as layers slide over eachother

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17
Q

What do ionic bonds form between?

A

Metals and non-metals

18
Q

In ionic bonding electrons are transported where?

A

From the metal atoms to the non-metal atoms

19
Q

What do metals become in ionic bonding?

A

Positively charged ions

20
Q

What is the electronic configuration of a ion in a ionic bond?

A

Full outer energy level (like a noble gas)

21
Q

Where on a ionic bond diagram does the charge and amount of atoms appear?

A

Top right

Bottom right

22
Q

What is ionic bonding?

A

Strong electrostatic attraction between oppositely charge ions

23
Q

Are ionic compounds soluble?

A

Yes

24
Q

What colour are most ionic compounds?

A

White

25
Q

What colour are group 1/2 ionic compounds?

A

Always White

26
Q

What does the formula of a giant structure show?

A

Fixed ratio of different elements

27
Q

Do ionic compounds conduct electricity when molten or in an aqueous solution?

A

Yes

28
Q

What are the melting and boiling points of ionic compounds?

A

Relatively high

29
Q

Ionic bonding always forms what type of compound?

A

Giant ionic structure

30
Q

Giant ionic structure

A
  • High Melting Point
  • Soluble in Water
  • Conductor
  • Lattice structure
31
Q

How do giant ionic structures form into lattice?

A

Held together by the attraction between oppositely charged ions

32
Q

Why do ionic structures have high melting and boiling points?

A

The electrostatic attraction between oppositely charged ions is very strong, therefore a lot of energy is needed to break them apart

33
Q

What affects the strength of ionic bonding?

A

The stronger the charge, stronger forces of attraction occur
E.g 2+ and 2- ions are stronger than 1+ and 1-ions

34
Q

What are ionic structures made from?

A

Crystals

35
Q

Metals

A
  • have high melting points
  • are good conductors of heat and electricity
  • are hard and dense
  • malleable
  • ductile
36
Q

Describe metallic bonding

A

Positive ions in a lattice, surrounded by a sea of delocalised electrons

37
Q

What does metallic bonding allow metals to be?

A

Malleable, ductile, and very conductive

38
Q

How does metallic bonding enable metals to be conductive?

A

Delocalised electrons carry charge around the molecule

39
Q

Why does the metallic structure allow metals to be malleable?

A

Layers can slide over each other, still stuck together because of “electron sea”

40
Q

Properties of buckminsterfullerene

A

“Bucky ball”

  • 60 carbon atoms
  • arranged in a hollow sphere
41
Q

What is a fullerene?

A

Group of allotropes of carbon which are in the form of cages

GCSE - Chemistry (Old) (14 decks)

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