Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Ionic bonding > Flashcards

Ionic bonding Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Describe the reaction of Sodium
(alkali metals)

A

Reacts with O₂ - turns dull quickly
Reacts with H₂O - fizzes, and moves around quickly

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Describe the reaction of Magnesium

A

Reacts with O₂ - bright white light, white powder formed
Reacts with H₂O - slow reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Describe the reaction of Aluminium
(transition metals)

A

Reacts with pure O₂ - new solid slowly formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Describe the reaction of Silicon

A

Reacts with pure O₂ when heated with a Mg fuse

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Describe the reaction of Phosphorous

A

Reacts with air (not pure O₂) when heated - yellow flame

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Describe the reaction of Chlorine
(halogens)

A

Reacts with sodium when warm - bright yellow flame, white solid formed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Describe the reaction of Argon
(noble gases)

A

Unreactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Describe the reactivity of Sodium

A

more reactive than magnesium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Describe the reactivity of Magnesium

A

Faster reaction when heated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Describe the reactivity of Aluminium

A

Less reactive than magnesium
(pure oxygen used to encourage reaction to speed up)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Describe the reactivity of Silicon

A

Less reactive than magnesium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Describe the reactivity of Phosphorous

A

More reactive than silicon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Describe the reactivity of Chlorine

A

More reactive than sulphur and phosphorous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Describe the reactivity of Argon

A

All noble gases are unreactive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is an ion?

A

A charged particle (gained or lost electrons) containing a different number of protons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is an atom?

A

a neutral particle containing an equal number of protons and electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the name for a metal ion?

A

____ ion
eg magnesium ion

18
Q

What is the name for a non metal ion?

A

change to ____ide ion
eg oxide ion

19
Q

What is the carbon ion?

A

Doesn’t form an ion
semi stable

20
Q

What is oxidation?

A

gain of oxygen, loss of electrons

21
Q

What is reduction?

A

loss of oxygen, gain of electrons

22
Q

Is an oxygen atom (O) turning into an oxygen ion (O⁻²) oxidation or reduction?

A

Reduction as it has gained 2 electrons

23
Q

Is a lithium atom (Li) turning into a lithium ion (Li⁺¹) oxidation or reduction?

A

oxidation as it has lost 1 electron

24
Q

What is an ionic bond?

A

A strong electrostatic attraction between positive and negative ions

25
Q

What is an ionic compound?

A

more than one type of ion chemically bonded

26
Q

What structure will ionic compounds form?

A

giant ionic lattice

27
Q

What group will not form ions?

A

group 8 as its outer shell is already full

28
Q

Why will a magnesium and oxide ion react?

A

Oxygen needs to gain 2 electrons to become stable and magnesium needs to loose 2 electrons to become stable. This overall charge 2⁺ 2⁻ is equal. Mg gives 2 electrons to O.

29
Q

What type of melting point do ionic compounds have and why?

A

high due to strong electrostatic attraction between positive and negative ions that takes lots of energy to overcome

30
Q

Why are ionic compounds brittle?

A

Force moves ions causing them to repel from each other and break apart

31
Q

What is the conductivity of ionic compounds have and why?

A

non-conductive when solid as ions are not free to move
conductive when molten or in a solution as ions are free to move

32
Q

What is the strength of ionic compounds and why?

A

Very hard - Strong electrostatic attraction between positive and negative ions

33
Q

What is the solubility of ionic compounds and why?

A

Usually soluble in water - sodium is attracted to oxygen and chlorine attracted to hydrogen, ions attract to water molecules
Usually insoluble in organic solvents - ions are not attracted to the organic molecules

34
Q

What forms an ionic compound?

A

metal + non metal

35
Q

What is the formula for Hydroxide?

A

OH⁻¹

36
Q

What is the formula for Ammonium?

A

NH₄⁺¹

37
Q

What is the formula for Nitrate?

A

NO₃⁻¹

38
Q

What is the formula for Carbonate?

A

CO₃⁻²

39
Q

What is the formula for Sulphate?

A

SO₄⁻²

40
Q

What is the formula for Phosphate?

A

PO₄⁻³

41
Q

What does polyatomic ion mean?

A

many atoms

Chemistry (18 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions