Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > 2.1+2.2 Structure and Bonding > Flashcards

2.1+2.2 Structure and Bonding Flashcards

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

Top number on an element on periodic table and what is it?

A

Atomic mass- mass of neutrons and protons.

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

Bottom number on an element on periodic table and what is it?

A

Atomic number- number of protons ( so therefore electrons- atoms are usually neutral)

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

Metals tend to…

A

Lose electrons and therefore become positive ions.

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

Non-metals tend to…

A

Gain electrons and are therefore negative ions.

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

What is an ion?

A

A charged atom

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

What is ionic bonding?

A

The electrostatic force of attraction, in all directions, between metal and non-metal ions.

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

Why are some transition metals written with their charges in brackets?

A

Because they can form ions with different sizes of positive charges.

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

What do the ionic bonds between charged particles result in?

A

An arrangement of ions that we call a giant structure or a giant lattice.

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

Why do ionic compounds have high melting and boiling points?

A

Because the bonds are held together by strong electrostatic forces of attraction which take a lot of energy to overcome to break up a lattice.

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

Can ionic compounds conduct electricity?

A

Solid ionic compounds- cannot as can only vibrate in a fixed position and the ions are not free to move.

Molten or dissolved ionic compounds- they can, because the ions have been separated (either through dissolving or through melting and becoming a liquid allowing them to move) and are free to move around so can carry electrical charges through molten liquid/ solution.

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

The period on the periodic table is the same as…

A

The number of shells in an atom.

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

The group number tells you…

A

How many electrons are on the outside shell.

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

An ion

A

Is an atom which has lost or gained one or more electrons. Because the electrons and protons no longer balance, a particle with charge has formed.

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

Valency of an atom

A

The number of bonds that it can form e.g carbon had valency 4.

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

Structural formula

A

Shows the arrangement of atoms in a compound. (Diagram)

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

Molecular formula

A

Shows the number of each type of atom present e.g C2H6

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

Empirical formula

A

Shows the simplest whole no. Ratio of the different atoms present e.g CH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How can you figure out alkanes?

A

Monkeys. Methane
Eat. Ethane
Peanut. Propane
Butter. Butane

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Hydroxide

A

OH

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Nitrate

A

NO3

21
Q

Sulfate

A

SO4

22
Q

Carbonate

A

CO3

23
Q

What are the diatomics?

A

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

24
Q

Covalent bonding

A

The atoms in covalent compounds share electrons in their outer shells. Therefore, each atom gains the electron arrangement of a noble gas. Compound contains only non-metals.

25
Q

Can covalent compounds conduct electricity?

A

No because there is no charge on the atoms, so the molecules cannot carry an electrical charge.
Although graphite conducts electricity but for another reason.

26
Q

What are giant covalent structures known as?

A

Macromolecules

27
Q

What are some giant covalent structures?

A

Diamond
Silicon dioxide (sand)
Graphite

28
Q

Covalent bonding

A

The atoms in covalent compounds share electrons in their outer shells. Therefore, each atom gains the electron arrangement of a noble gas. Compound contains only non-metals.

29
Q

Can covalent compounds conduct electricity?

A

No because there is no charge on the atoms, so the molecules cannot carry an electrical charge.
Although graphite conducts electricity but for another reason.

30
Q

What are giant covalent structures known as?

A

Macromolecules

31
Q

What are some giant covalent structures?

A

Diamond
Silicon dioxide (sand)
Graphite

32
Q

Diamond and graphite are different forms of the same element carbon, what do we call these?

A

Allotropes of carbon.

33
Q

What is metallic bond?

A

The bonding of pure metals kept together by strong electrostatic attraction between positive metal ions and negative electrons.

34
Q

Alloy and is it harder?

A

Is a mixture of 2 elements/metals, the atoms are all different sizes, which distorts the regular arrangement of atoms. This makes it more difficult for layers to slide over each other so harder then pure metals.

35
Q

Crystals

A

Have a highly ordered structure, with atoms arranged in repeating patterns and very tightly held together.

36
Q

Are metals easy to shape?

A

Metals are often easy to shape (malleable) as the delocalised electrons enable the lattice to distort, layers can slide over each other easily.

37
Q

Metals

A

A lattice of positively charged ions arranged in regular layers one on top of another, held together by electrostatic forces of attraction between the positive metal ions and the negative electrons.

38
Q

Displacement reaction

A

More reactive substance displaces less reactive substance.

E.g copper + silver nitrate👉 copper nitrate + silver

39
Q

Polymerisation

A

When alkene molecules join together, the double bond between the carbon atoms in each molecule ‘opens up’. It is replaced by single bonds as thousands of molecules join together.

40
Q

Properties of a polymer depend on…

A

The monomers used to make it and the conditions we choose to carry out the reaction.

41
Q

What are the two main types of polymers e.g ethene?

A

Low density poly(ethene) (LDPE)

Or

High density poly(ethene) (HDPE)

42
Q

Reaction conditions for LD POLY(ethene)?

A

Very high pressures

Trace of oxygen

43
Q

Reaction conditions for HD poly(ethene)?

A

Uses of a catalyst
50 degrees celsius
Slightly raised pressure

44
Q

What is a thermosoftening polymer ?

A

It is made up of individual polymer chains that are tangoed together and when they are heated, they soften quite easily and will reset (to same tangled together structure) when they cool.

45
Q

What is a thermosetting polymer?

A

It does not melt when heated, will eventually char at high enough temperatures. They have STRONG covalent bonds forming ‘crosslinks) between their polymer chains.👉 heat resistant and rigid.

46
Q

Shape memory alloys (smart materials)

A

Is an alloy which has a special property in the fact that they can be bent or deformed into different shapes like other metals, but when you heat them up, they then return to their ORIGINAL shape all by themselves.

47
Q

A nanometre is…

A

1 billionth of a metre

48
Q

Why do materials behave differently on a nanoscale?

A

Because nanoparticles are so tiny that they have a huge surface area for a small volume of material.

49
Q

Some uses of Nano-science:

A 
Glass coated with titanium oxide nanoparticles-cleans window.
Sunscreens
Creams
Nano cages (carbon(tennis rackets),gold)
Bucky balls

Chemistry (12 decks)

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