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IGCSE Chemistry > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

What is a bond between two non-metals called

A

A covalent bond

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2
Q

Define compound

A

A chemically bonded substance made of 2 or more elements with fixed proportions

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3
Q

What is a diatomic molecule

A

A molecule made of two atoms

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4
Q

What is covalent bonding in terms of electrons

A

A chemical bond through shared electrons

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5
Q

What is covalent bonding in terms of components

A

Two or more non-metals

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6
Q

What forces are in lattice covalent bonds

A

Strong covalent bonds

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7
Q

Molecules can only have one type of bonding and structure, which is:

A

discrete covalent

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8
Q

What forces are there INSIDE discrete covalent molecules

A

Strong Covalent Bonds

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9
Q

What forces are there BETWEEN discrete covalent molecules

A

Weak Inter Molecular Forces

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10
Q

How big is a lattice structure

A

infinite

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11
Q

How big is a discrete covalent structure

A

Very small, sometimes only 2 atoms.

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12
Q

Example question 1: How many electrons are shared in H2

A

2 electrons (1 pair)

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13
Q

Example question 1: How many electrons are shared in N2

A

6 electrons (3 pairs)

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14
Q

What is the number of shared electron pairs based on

A

The combining power of the atoms

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15
Q

Example question 1: describe the shared electron pairs in NH3

A

3 H have a pair of shared electrons with one N
H N H
H

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16
Q

Example question 1: describe the shared electron pairs in CO2

A

2 O have 2 pairs of shared electrons with one C
O=C=O

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17
Q

How are covalent bonds drawn

A

Like a venn diagram, with the number of pairs of shared electrons drawn in the center. ONLY the OUTER energy level is drawn.

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18
Q

What are the melting points of discrete covalent structures

A

Very low

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19
Q

Why are the melting points of discrete covalent structures low

A

Because they have weak IMFs, which do not require lots of force to break apart.

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20
Q

Discrete covalent structures are soluble in ___________

A

Nothing

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21
Q

Discrete covalent structures are conductive in what forms?

A

None.

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22
Q

Why don’t discrete covalent structures conduct?

A

Because they have no charged particles

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23
Q

What is a bond between a metal and a non-metal called

A

Ionic Bond

24
Q

What are the forces in ionic bonds

A

electrostatic forces

25
Q

What is an ionic lattice structure

A

A structure of alternating atoms of positive and negative charges.

26
Q

What happens physically for an atom to become an ion?

A

It either gains or loses electron(s)

27
Q

What happens physically for an ionic bond to occur

A

One atom takes electron(s) from another atom

28
Q

How are ionic compounds drawn

A

The ion version of the atom (having lost or gained e-(s) with all its energy levels that contain e-(s), in [] with its charge at the top right corner, and ……. (electrostatic force) between the ions.

29
Q

How is charge written

A

Magnitude of charge followed by type of charge (2+, 3-, +, 4-)

30
Q

What is charge based on?

A

How many e-(s) an atom has to lose to have a full outer energy level

31
Q

Ionic substances are soluble in _______

A

water

32
Q

The melting points of ionic substances are _______

A

very high

33
Q

Why are the melting points of ionic substances high?

A

Because strong electrostatic forces require lots of energy to break apart.

34
Q

Ionic substances conduct as _______

A

liquid (l) or aqueous (aq)

35
Q

How do ionic substances conduct (What carries charge?)

A

Electrons carry charge

36
Q

Why do ionic substances conduct as fluids except gases

A

They don’t conduct as gases, because gases can’t carry charge, and not as solids, because the electrons can’t move to carry charge

37
Q

Are ionic substances malleable

A

No

38
Q

Why aren’t ionic substances malleable?

A

Because if the atoms are moved from their pattern of opposing charges, and atoms have the same charges, they will repel each other and therefore break apart.

39
Q

What are cations

A

Positive ions (Having lost electrons)

40
Q

What are anions

A

Negative ions (Having gained electrons)

41
Q

Why does graphite conduct electricity, but diamond doesn’t?

A

Because graphite has seas of delocalised electrons which can move and carry charge

42
Q

What are the forces in lattice covalent structures

A

Strong covalent bonds

43
Q

Is graphite malleable

A

Yes

44
Q

Why is graphite malleable

A

Because it is in layers which can easily maintain their shape when bent or hit

45
Q

Are lattice covalent structures GENERALLY malleable

A

No

46
Q

Why are lattice covalent structures brittle

A

Because if one bond breaks, many more tend to break with it

47
Q

What are lattice covalent structures soluble in

A

Nothing

48
Q

Melting points of lattice covalent structures are _____

A

Very high

49
Q

Why are melting points in lattice covalent structures high

A

Because it requires a lot of energy to break so many strong covalent bonds

50
Q

What is it called when metals bond with metals

A

Metallic bonding

51
Q

What is it called when two DIFFERENT metals are chemically bonded

A

An alloy

52
Q

Are metals malleable

A

Yes

53
Q

Why are metals malleable

A

Because they are in layers which can easily maintain their shape when bent or hit

54
Q

How do metals carry charge

A

Through delocalized e-(s)

55
Q

Metals conduct as ______

A

solids

56
Q

What does metallic structure look like

A

There are layers of the metal, arranged in a pattern, altetnating with layers of delocalised e-s in a random pattern (same as graphite)

IGCSE Chemistry (22 decks)

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