Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

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

The types of atoms which form ionic bonds

A

Metals with Non-Metals

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

The location of metals in the Periodic Table

A

Left

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

The location of non-metals in the Periodic Table

A

Right

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

The types of atoms which form positive ions

A

Metals

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

The number of electrons in a full outer shell

A

8

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

Description of the structure in covalent compounds

A

Simple molecules containing a small number of bonded atoms

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

The seven diatomic elements

A

H2, N2, O2, F2, Cl2, Br2, I2

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

Definition of diatomic

A

An element which exists as molecules containing two atoms

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

Conductivity of simple covalent molecules

A

Poor, because there are no charged particles to carry the charge

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

Melting point of simple covalent molecules

A

Low, because weak intermolecular forces require little energy to break

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

How to identify the number of shared electrons

A

The number of electrons an atom needs to gain a full outer shell, it shares.

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

The attractive force between covalent molecules

A

Weak intermolecular forces

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

The attractive force in a covalent bond

A

Electrostatic attraction between the shared electrons and the nuclei

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

The type of atoms which form covalent bonds

A

Non-metals

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

The electrical conductivity of graphite

A

Good, because delocalised electrons are able to move and carry the charge

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

The electrical conductivity of diamond and silicon dioxide

A

Poor, as there are no charged particles

17
Q

The melting point of diamond, graphite and silicon dioxide

A

Very high, as strong covalent bonds require a lot of energy to break

18
Q

The structure of graphite

A

Hexagonal layers of carbon atoms with three bonds each, and one delocalised electron

19
Q

The structure of diamond

A

A lattice of carbon atoms with four bonds each

20
Q

The structure in giant covalent structures

A

A lattice of many non-metal atoms held together by strong covalent bonds

21
Q

The types of atoms which form negative ions

A

Non-metals

22
Q

The formula and charge of the sulfate ion

A

SO4 2-

23
Q

The formula and charge of the ammonium ion +

A

NH4

24
Q

The formula and charge of the carbonate ion

A

CO3 2-

25
Q

The formula and charge of the nitrate ion

A

NO3 -

26
Q

The formula and charge of the hydroxide ion

A

OH -

27
Q

The formula and charge of the phosphate ion

A

PO4 3-

28
Q

Description of the bonding in ionic compounds

A

Strong electrostatic forces between positive and negative ions

29
Q

Description of the structure of ionic compounds

A

A lattice of alternating positive and negative ions

30
Q

The melting points of ionic compounds

A

High, because the strong electrostatic forces require a lot of energy to break

31
Q

The conductivity of ionic compounds

A

Only in the liquid state, when ions are free to move to carry the charge

32
Q

The types of ions formed by metal atoms

A

Positive ions

33
Q

The structure of a metal

A

A lattice of positive ions with a sea of delocalised electrons

34
Q

Melting point of metals

A

High because strong electrostatic forces require a lot of energy to break

35
Q

Electrical conductivity of metals

A

Good because the delocalised electrons are able to move to carry the charge

36
Q

Bonding in metals

A

Strong electrostatic forces between positive ions and delocalized electrons

37
Q

Three examples of giant covalent structures

A

Diamond, silicon dioxide, graphite

38
Q

The bonding in giant covalent structures

A

Sharing of electrons between atoms

Chemistry (4 decks)

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