Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Key Concepts In Chemistry > Flashcards

Key Concepts In Chemistry Flashcards

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

What does (s) mean

A

Solid

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

What does (l) mean

A

Liquid

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

What does (g) mean

A

Gas

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

What does (aq) mean

A

Aqueous - dissolves in water

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

What is the formula for water

A

H20

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

What is the formula for carbon dioxide

A

CO2

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

What is the formula for chlorine

A

Cl2

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

What is the formula for ammonia

A

NH3

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

What is the formula for hydrogen

A

H2

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

What is the formula for oxygen

A

O2

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

What is the ionic formula for ammonium

A

NH4+

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

What is the ionic formula for nitrate

A

NO3-

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

What is the ionic formula for sulfate

A

SO42-

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

What is the ionic formula for hydroxide

A

OH-

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

What is the ionic formula for carbonate

A

CO32-

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

What is a hazard

A

Anything that has the potential to cause harm or damage

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

What is a risk

A

the probability of someone (or something) being harmed if they are exposed to the hazard

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

What are the 3 subatomic particles

A

Protons, neutrons and electrons

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

What are the properties of protons

A

Heavy and positively charged

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

What are the properties of electrons

A

Heavy and neutral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What are the properties of neutrons

A

Hardly any mass and are negatively charged

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Describe the nucleus of an atom

A

In the centre of an atom
Contains protons and neutrons
Has a positive charge because of the protons
It is where almost all of the atoms mass is
It is tiny compared to the overall size of the atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Describe the electrons of an atom

A

Move around the nucleus in electron shells
Negatively charged
Tiny but their shells cover a lot of space
The size of their shells determines the size of the atom
They have a tiny mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Describe the properties of atoms

A

Have the same number of protons as electrons
They are neutral (no charge)
The charge on the electrons is the same size as the charge on the protons but opposite so the charges cancel out

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What does the nuclear symbol of an atom tell you

A

Its mass number and atomic number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What does the atomic number tell you

A

How many protons an atom has

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What does the mass number tell you

A

The total number of protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What are isotopes

A

Different forms of the same element, which have the same number of protons but a different number of neutrons
Same atomic number but different mass numbers
Eg. Carbon-12 and Carbon-13

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Who made the first periodic table

A

Dimitri Mendeleev

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What are the electron shell rules

A

2,8,8 and the lowest energy levels are always filled first

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What are ions

A

Charged particles that can be single atoms or groups of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is an anion

A

A negative ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What is a cation

A

A positive ion

34
Q

How do negative ions form

A

When atoms gain electrons

35
Q

How do positive ions form

A

When atoms lose electrons

36
Q

What groups are most likely to form ions

A

Group 1, 2, 6, 7

37
Q

What are ionic compounds made up of

A

A positively charged part and a negatively charged part

38
Q

What is the overall charge of any ionic compound

A

Zero

39
Q

What is an ionic bond

A

When a metal and a non-metal reacts together.
The metal loses electrons to form a positive ion and the non-metal gains electrons to form a negative ion.
These are strongly attracted to each other with an electrostatic force

40
Q

What do dot and cross diagrams show

A

The arrangement of electrons in an atom or ion

41
Q

What do ionic compounds always have

A

Giant ionic lattice structures

42
Q

What are the properties of ionic compounds

A

High melting and boiling point
Solid ionic compounds cannot conduct electricity
Melted ionic compounds can conduct electricity
Dissolve easily in water

43
Q

Why do ionic compounds have high melting and boiling points

A

Due to their strong attraction between the ions. It takes a large amount of energy to overcome this attraction

44
Q

Why don’t solid ionic compounds conduct electricity but melted ionic compounds do

A

Because in a solid, the ions are fixed in place and cant move but when melted, the ions are free to move and will carry an electric current

45
Q

Why do ionic compounds dissolve easily in water

A

The ions separate and are free to move in the solution so they’ll carry an electric current

46
Q

What are the advantages of showing ionic compounds in 2D representations

A

They are great at showing what atoms something contains and how the atoms are connected

47
Q

What are the disadvantages of 2D representations of ionic compounds

A

They don’t show the shape of the substance and they don’t give you any idea about the sizes of the atoms

48
Q

What are the advantages of a dot and cross diagram

A

They are useful for showing how compounds or molecules are formed and where the electrons in the bonds or ions came from

49
Q

What are the disadvantages of dot and cross diagrams

A

They don’t usually show anything about the size of the atoms or ions or how they are arranged

50
Q

What are the advantages of 3D models showing structures

A

They show the arrangement of atoms

51
Q

What are the disadvantages of 3D models showing structures

A

They only show the outer layer of a substance

52
Q

What are the advantages of a ball and stick model

A

Helps to visualise structures as they show the shape of the lattice or molecule in 3D
They’re more realistic

53
Q

What are the disadvantages of ball and stick models

A

They don’t show the correct scales of the atoms or ions

54
Q

What is a covalent bond

A

A strong bond when a pair of electrons is shared between two atoms

55
Q

What are simple molecular substances made up of

A

Molecules containing a few atoms joined by covalent bonds

56
Q

What do you need to do to melt or boil a simple molecular compound

A

Break the feeble intermolecular forces and not the covalent bonds

57
Q

Do molecular compounds conduct electricity and why

A

No because they haven’t got any free flowing electrons or ions

58
Q

What are the properties of giant covalent structures

A

Strong covalent bonds between each atom
High melting and boiling point - lots of energy needed to break the bonds
Don’t contain charged particles - don’t conduct electricity
Aren’t soluble in water

59
Q

What are 3 examples of carbon-based giant covalent structures

A

Diamond
Graphite
Graphene

60
Q

What is diamond made up of

A

Carbon atoms that each form 4 covalent bonds

61
Q

Does diamond have a high or low melting point

A

High

62
Q

Is diamond hard or soft, why

A

Hard because the strong covalent bonds hold the atoms in a rigid lattice structure

63
Q

Does diamond conduct electricity

A

No because it has no free electrons or ions

64
Q

In graphite, how many covalent bond does a carbon atom form, what does it create

A

3, creating sheets of carbon atoms arranged in hexagons

65
Q

Is graphite hard or soft, why?

A

Soft and slippery because there aren’t any covalent bonds between the layers so they’re held together weakly and free to move over each other

66
Q

Can graphite conduct electricity

A

Yes as only 3 out of 4 electrons are used in bonds so each carbon atom has 1 electron that’s delocalised (free)

67
Q

What is the structure of graphene

A

1 layer of graphite

A sheet of carbon atoms joined together in hexagons

68
Q

Are the electrons in the outer shell of metal atoms localised or delocalised

A

Delocalised

69
Q

What is metallic bonding

A

The forces of attraction between the positive metal ions and the shared negative electrons hold the atoms together in a regular structure.

70
Q

What is the relative formula mass (RFM)

A

The relative atomic masses of all the atoms added together

71
Q

What does the empirical formula of a compound tell you

A

The smallest whole number ratio of atoms in a compound

72
Q

How do you calculate the molecular formula

A

Add the empirical formula and the relative formula mass

73
Q

What is a mole

A

The name given to a certain number of particles

74
Q

What is a mole equal to

A

A number called Avogrado’s constant

75
Q

What is the number of Avogrado’s constant

A

6.02 x10 to the power of 23

76
Q

Why is Avogrado’s constant useful

A

Because when you get the number of atoms or molecules, of any element or compound, then they weigh the same number of grams as the RAM/RFM of the element or compound

77
Q

What is the equation for the number of moles

A

Number of moles = mass in g (of element or compound) / RFM of compound or RAM of element

78
Q

What is the formula triangle involving mass, moles and RFM

A

Mass
—————-
Moles x RFM

79
Q

What is the equation for concentration

A

Concentration = mass of solute / volume of solution

80
Q

When do reactions stop

A

When all of one reactant is used up

81
Q

What is the limiting reactant

A

The reactant that is used up in the reaction

Chemistry (7 decks)

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