Brainscape's Knowledge GenomeTM

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


See full index

Chemistry LV3 > Ionic, covalent and metallic crystals COPY COPY > Flashcards

Ionic, covalent and metallic crystals COPY COPY Flashcards

1
Q

Substances with simple molecular structures are…

A

Gases or liquids, or solids with low melting points

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

Why do substances with simple molecular structures have low melting points?

A

It doesn’t take much heat energy to break the relatively weak intermolecular attractions

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

Substances with giant covalent structures have…

A

High melting and boiling points

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

Why do substances with giant covalent structures have high melting and boiling points?

A

Because You need a lot of heat energy to break the many strong covalent bonds

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

Describe the positions of the atoms in a diamond

A

In diamond, each carbon bonds strongly to four other carbon atoms in a tetrahedral arrangement. It is a giant covalent structure - it carries on and on in three dimensions. It is not a molecule as the number of atoms joined up in a real diamond is completely variable- depending on the size of the crystal

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

What is diamonds purpose

A

Saw blades can be tipped with diamonds in high speed cutting tools used in stone and concrete

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

Why are diamonds used to tip high speed cutting tools

A

Diamond is very hard because of the very strong carbon - carbon covalent bonds, which extend throughout the structure in three dimensions.

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

Describe the positions of the atoms in graphite

A

Graphite has a giant layered structure, rather like a pack of cards. In a pack of cards. Each card is strong but the individual cards are easily separated. The same is true in graphs. The gaps between the layers are much bigger than the distances between the atoms in the layers.

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

What is covalent bonding

A

A strong attraction between the bonding pair of electrons and the nuclei of the atoms involved with the bond

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

Why does graphite structure make it useful

A

Graphite is a soft material with a slimy feel Although the forces holding the atoms together in each layer are very strong, the attractions between the layers are much seeker. Layers can easily be flaked off. Pure graphite is so slippery that it is used as a lubricant - eg powdered graphite is used to lubricate locks.

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

What can a metal be described as

A

A giant structure of positive ions surrounded by a sea of delocalised electrons

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

Why can metals conduct electricity

A

Because the delocalised electrons are free to move thought the structure

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

Why are metals malleable

A

Metals are usually easy to shape because their regular packing makes it simple for the atoms to slide over each other

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

Ionic bonding

A

A strong electrostatic attraction between oppositely charged ions

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

Why do ionic compounds have high melting and boiling points

A

Because of strong electrostatic forces between oppositely charged ions

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

Why do ionic compounds have high melting and boiling points

A

Because of the strong forces holding the lattices together

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

What is an ionic crystal

A

An ionic crystal is a giant three dimensional lattice structure held together by the attraction between oppositely charged ions

18
Q

Describe what happens during ionic bonding

A

When metals react with non metals, electrons are transferred from the metal atoms to the non metal atoms, forming ions. He resulting compound is called an ionic compound

19
Q

What is ionic bonding

A

A strong electrostatic attraction between oppositely charged ions

20
Q

Do ionic compounds have low or high melting points

A

They have high melting and boiling points

21
Q

Why do ionic compounds have high melting and boiling points

A

Because of the strong electrostatic forces between oppositely charged ions

22
Q

What is ionic crystal

A

Ionic crystal is a giant three dimensional lattice structure held together by the attraction between oppositely charged ions

23
Q

Describe ionic bonding

A

When metals react with nonmetals, electrons are transferred from the metal atoms to the non metal atoms, forming ions The resulting compound is called an ionic compound

24
Q

What can a metal be described as

A

A metal can be described as a giant structure of positive ions surrounded by a sea of delocalised electrons

25
Q

Why do metals conduct electricity

A

Because the delocalised electrons are free to move throughout the structure

26
Q

Why are metals malleable

A

Metals are usually easy to shake because their regular packing makes it simple for the atoms to slide over each other

27
Q

What is ionic bonding

A

A strong electrostatic attraction between oppositely charged ions

28
Q

Do ionic compounds have low or high melting points

A

They have high melting and boiling points

29
Q

Why do ionic compounds have high melting and boiling points

A

Because of the strong electrostatic forces between oppositely charged ions

30
Q

What is ionic crystal

A

Ionic crystal is a giant three dimensional lattice structure held together by the attraction between oppositely charged ions

31
Q

Describe ionic bonding

A

When metals react with nonmetals, electrons are transferred from the metal atoms to the non metal atoms, forming ions The resulting compound is called an ionic compound

32
Q

What can a metal be described as

A

A metal can be described as a giant structure of positive ions surrounded by a sea of delocalised electrons

33
Q

Why do metals conduct electricity

A

Because the delocalised electrons are free to move throughout the structure

34
Q

Why are metals malleable

A

Metals are usually easy to shake because their regular packing makes it simple for the atoms to slide over each other

35
Q

What is ionic bonding

A

A strong electrostatic attraction between oppositely charged ions

36
Q

Do ionic compounds have low or high melting points

A

They have high melting and boiling points

37
Q

Why do ionic compounds have high melting and boiling points

A

Because of the strong electrostatic forces between oppositely charged ions

38
Q

What is ionic crystal

A

Ionic crystal is a giant three dimensional lattice structure held together by the attraction between oppositely charged ions

39
Q

Describe ionic bonding

A

When metals react with nonmetals, electrons are transferred from the metal atoms to the non metal atoms, forming ions The resulting compound is called an ionic compound

40
Q

What can a metal be described as

A

A metal can be described as a giant structure of positive ions surrounded by a sea of delocalised electrons

41
Q

Why do metals conduct electricity

A

Because the delocalised electrons are free to move throughout the structure

42
Q

Why are metals malleable

A

Metals are usually easy to shake because their regular packing makes it simple for the atoms to slide over each other

Chemistry LV3 (13 decks)

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