Brainscape's Knowledge GenomeTM

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


See full index

Science > Chemistry Paper One > Flashcards

Chemistry Paper One Flashcards

You may prefer our related Brainscape-certified flashcards:
Biology 101 flashcards
1
Q

What is the dimension of a nanoparticle? How many atoms can a nanoparticle include?

A

Nanoscience refers to structures that are 1 to 100nm in size (1nm = 1x10-9m). This contains structures up to about 100 atoms.

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

What are the dimensions of a fine particle?

A

Fine particles have diameters between 100 and 2500 nm (1x10-7m and 2.5x10-6m)

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

What are the dimensions of a coarse particle? What are they also know as?

A

Coarse particles have diameters between 1x10-5m and 2.5x10-6m). These are often referred to as dust.

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

Why do nanoparticles have different properties to bulk materials?

A

Nanoparticles may have properties different from those for the same materials in bulk because of their high surface area to volume ratio. This means that smaller quantities are needed to be effective than for materials with normal particle size.

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

What is bronze an alloy of?

A

Bronze is an alloy of copper and tin

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

What is brass an alloy of?

A

Brass is an alloy of Copper and Zinc

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

What is gold an alloy of?

A

Gold is usually alloyed with silver, copper and zinc.

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

What is an isotope?

A

Atoms of the same element with a different number of neutrons.

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

What are the properties of noble gases (Group 0)?

A
  • Very stable
  • Monatomic
  • Melting point increases as you get further down
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the properties of the alkali metals?

A
  • Very reactive, stored in oils.
  • Reactivity increases as you go down.
  • They burn vigorously.
  • Low mp/bp.
  • Produces hydrogen.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the properties of the halogens?

A
  • Low melting/boiling points, they increase as you go down.

- Poor conductors of heat and electricity.

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

What are the 3 raw materials used to make soda-lime glass?

A

Sand + Sodium Carbonate + Limestone

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

What is borosilicate glass made from?

A

Sand + Boron Trioxide.

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

Explain the paper chromatography experiment.

A
  1. Draw a line at the bottom of the filter paper (in pencil).
  2. Add a spot of ink and place the sheet in a beaker of solvent.
  3. The solvent used depends on what’s being tested. Some compounds dissolve well in water, sometimes other solvents are needed.
  4. Make sure the ink isn’t touching the solvent.
  5. Place a lid on top to stop evaporating.
  6. The solvent seeps up the paper, carrying the ink with it.
  7. Each different dye will move up the paper at different rates.
  8. If any dyes are insoluble they’ll stay at the baseline.
  9. Take the paper out and leave it to dry.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Explain why the plum pudding model was wrong.

A

Rutherford fired positively charged alpha particles at a thin sheet of gold. Most of the particles went straight through, more were deflected than expected and some deflected backwards.

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

What are the properties of the transition metals.

A
  • Often coloured compounds.

- Make good catalysts.

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

What are polymers?

A

Long chains of repeating units.

18
Q

What are the properties of polymers intermolecular forces?

A

Forces are much larger than covalent intermolecular forces so more energy is needed to break them. This makes them a solid at room temperature. Still weaker than ionic or covalent bonds so their boiling/melting points are lower.

19
Q

What are fullerenes, what are they used for?

A

Fullerenes are molecules of carbon, shaped like closed tubes or hollow balls.
They are used to cage other molecules. So they can deliver drugs.
They have a huge surface area so they make great industrial catalysts.
They make great lubricants.

20
Q

What is the Avogadro constant?

A

6.02 x 10(23)

21
Q

How do you find out the number of moles?

A

mass in g ÷ Mr

22
Q

How do you calculate concentration?

A

mass of solute ÷ volume of solvent

23
Q

How do you calculate atom economy?

A

relative formula mass of desired product ÷ relative formula mass of all reactants X 100

24
Q

How do you calculate percentage yield?

A

mass of product made ÷ maximum theoretical mass X 100

25
Q

What happens when an acid reacts with:
a metal oxide
metal hydroxide
metal carbonate

A

Acid + Metal Oxide → Salt + Water

Acid + Metal Hydroxide → Salt + Eater

Acid + Metal Carbonate → Salt + Water + Carbon Dioxide

26
Q

What is the reactivity series?

A 
Potassium K
Sodium Na
Lithium Li 
Calcium Ca
Magnesium Mg
Carbon C 
Zinc Zn
Iron Fe
Hydrogen H
Copper Cu
27
Q

What is meant by oxidation/reduction in both oxygen and electrons?

A

Oxidation = Gain of Oxygen
Reduction = Loss of Oxygen
Oxidation is Loss
Reduction is Gained

28
Q

What happens in electrolysis?

A

An electric current is passed through an electrolyte, this is a molten or dissolved ionic compound.
The ions move towards the electrodes.
The positive ions in the electrolyte will move towards the cathode and gain electrons.
The negative ions in the electrolyte will move towards the anode and lose electrons.
This creates a flow of charge through the electrolyte as ions travel to the electrodes.

29
Q

What happens in an exothermic reaction?

A

An exothermic reaction is one which transfers energy to the surroundings usually by heating.

30
Q

What happens in an endothermic reaction?

A

An endothermic reaction is one which takes in energy from the surroundings. This is shown by a fall in temperature.

31
Q

Define isotopes?

A

Different forms of the same element, which have the same number of protons but a different number of neutrons.

32
Q

Define relative atomic mass?

A

An average mass taking into account the different masses and abundances of all the isotopes that make up the element.

33
Q

Formula for relative atomic mass?

A

Sum of (isotope abundance x isotope mass number) divided by sum of abundance of all the isotopes.

34
Q

Compounds..?

A

When elements react, atoms combine with other atoms to form compounds.

35
Q

What are compounds?

A

Substances formed from two or more elements, the atoms of each are in fixed proportions throughout the compound and they’re held together by chemical bonds.

36
Q

How do mixtures differ from compounds?

A

Unlike in a compound there’s no chemical bond between the different parts of the mixture.
Mixtures are easily separated.`

37
Q

Name the two methods that can be used to separate soluble solids from solutions?

A

Evaporation and Crystallisation.

38
Q

Explain simple distillation.

A

Distillation is used to separate mixtures (solutions) which contain liquids.
The solution is heated, the part of the solution that has the lowest boiling point evaporates first.
The vapour is then cooled, condenses and is collected.
The rest of the solution is left behind in the flask.

39
Q

Name a disadvantage of fractional distillation?

A

The problem with simple distillation is that you can only use it to separate things with very different boiling points - if the temperature goes higher than the boiling point of the the substance with the higher boiling point then they will mix again.

40
Q

Name an alternative to simple distillation.

A

Fractional distillation.

41
Q

Explain fractional distillation.

A

Place your mixture in a flask and stick a fractionating column on the top. Then heat it.
The different liquids will all have different boiling points so will evaporate at different times.
The liquid with the lowest boiling point evaporates first, when the temp on the thermometer matches the boiling point of this liquid it will reach the top of the column.
Liquids with higher boiling points may also start to evaporate. But the column is cooler towards the top so they will only get part of the way up before condensing and running back down towards the flask.
When the first liquid has been collected, you raise the temp until the next one reaches the top.

42
Q

I GOT TO PAGE 30 WITH IN DEPTH DETAIL

A

««<

Science (7 decks)

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