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GCSE CHEMISTRY PAPER 1 > C1 > Flashcards

C1 Flashcards

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1
Q

What is the relative charge of:
a) a proton
b) an electron
c) a neutron

A

a) proton= +1

b) electron= -1

c) neutron= 0

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2
Q

What are the relative masses of the three sub-atomic particles?

A
  • proton= 1
  • neutron= 1
  • electron= virtually nothing
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3
Q

What is the radius of an atom and the nucleus of an atom?

A
  • atom= 1 x 10-10
  • nucleus= 1 x 10-14
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4
Q

What is an element?

A

An element is substance made up of only one type of atom

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5
Q

What is an ion?

A

an ion is an atom or element that has lost or gained electrons, therefore giving it a charge

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6
Q

True or False? Elements only contain atoms with the same number of protons.

A

True

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7
Q

What does the relative mass number of an element tell us?

A

the total number of protons and neutrons

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8
Q

What does the relative atomic number of an element tell us?

A

the number of protons

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9
Q

Define an isotope

A

An isotope is a form of an element with the same number of protons but a different number of neutrons

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10
Q

Define a molecule

A

A molecule is two or more atoms, held together by chemical bonds

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11
Q

What is the difference between mixtures and compounds?

A

A compound is two or more different elements that are chemically combined in fixed proportions bonds whilst a mixture is two or more elements that are not chemically joined

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12
Q

Before the discovery of the electron, what were atoms thought to be?

A

Tiny spheres that could not be divided

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13
Q

What did the discovery of the electron lead to and what did this model suggest?

A

The plum pudding model:
the atom is a ball of positive charge with
negative electrons embedded in it

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14
Q

Which scientist did the alpha particle scattering experiment and what conclusions could be made from the experiment?

A

Ernest Rutherford

  1. the mass of an atom in concentrated in the centre
  2. the atom is mostly empty space
  3. the nucleus was charged
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15
Q

What replaced the plum pudding model and how did Neil Bohr adapt the model?

A

The nuclear model

he suggested that electrons orbit the nucleus at specific distances; his theoretical calculations agreed with experimental observations

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16
Q

Who provided evidence of the neutron within the nucleus?

A

James Chadwick

17
Q

What are the 5 methods that can be used to separate mixtures?

A
  1. Filtration
  2. Crystallisation
  3. Simple Distillation
  4. Chromatography
  5. Fractional Distillation
18
Q

Describe when simple distillation is used and explain

A

Used to separate a liquid from a solution (with different boiling points) e.g. separating pure water from sea water

• Equipment-conical flask, thermometer, condenser, beaker, Bunsen burner

• The mixture is heated up so the liquid we want evaporates as it rises up the pressure will force it down the condenser and the vapor will cool and condense into a liquid that would flow into the beaker

19
Q

Describe when fractional distillation is used and explain

A

used for separating mixtures of liquids with different boiling points

• equipment-fractionating column, conical flask condenser

  • The mixture would be heated to the boiling point of the substance which has a lower boiling point, causing it to evaporate and rise up the fractionating column and pass into the condenser and cool into liquid that will flow into the beaker
  • Same thing done again to heat the remaining mixture the next boiling point
20
Q

Why can evaporation always be used to separate soluble solids from solutions?

A

some solids decompose when heated (thermal decomposition)

21
Q

Describe and explain crystallisation

A

separates solutions into their different parts: dissolved solids(solutes) and liquids(solvents) & separates a soluble solid from a solution

• equipment: crucible(evaporation dish), tripod, Bunsen burner or water bath, heat proof mat, filter paper, funnel

  1. Place the solution into a crucible and heat it gently(a water bath would be appropriate)
  2. Once some of the solvent has evaporated and you can see crystals forming stop heating the solution
  3. Leave the solution to cool. As the solution cools more crystals will start to form (because solids are less soluble at colder temperatures)
  4. filter out the solution using filter paper and a funnel
  5. dry the crystals e.g. by leaving them somewhere warm.
22
Q

Describe and explain filtration

A

used to separate insoluble solids and
liquids

• equipment- funnel, filter paper, beaker
- the mixture is poured through the filter paper

  • the insoluble solid is trapped by the filter paper whilst the liquid runs through and is collected below
23
Q

Describe and explain chromatography

A

used to separate solutions with a number of different solutes in the solvent

• equipment: filter paper, beaker, solvent(e.g.) water, pencil

  1. draw a line on the filter paper in pencil and place dots of ink along the line
  2. fill the beaker with the solvent but make sure it is below the pencil line
  3. as the solvent moves up the paper it carries the solutes with it (different solutes move at different speeds so they separate.)
24
Q

How are the elements of the periodic table arranged?

A

The elements are arranged by atomic number

25
Q

What are the rows called?

A

Periods

26
Q

What are the columns called?

A

Groups

27
Q

What does the period and group of an element tell you?

A

group number= number of electrons on the outer(most) shell

period=number of shells

28
Q

How was the periodic table arranged before?

A

by atomic weight

29
Q

How did Dimitri Mendeleev fix the periodic table

A
  • left gaps for elements he believed were yet to be discovered
  • changed the order based atomic weights to atomic number
30
Q

Where are metals located on the periodic table?

A

To the left (of the ‘stairs’)

31
Q

Where are the non-metals located?

A

to the right of the ‘stairs’

32
Q

What is the difference between metals and non-metals ?

A

non-metals - form negative ions (anions), dull, poor conductors, brittle

metals- form positive ions (cations), shiny, malleable, good conductors of electricity + heat , ductile

33
Q

What is group 0 known as and what are properties/trends of group 0?

A

Noble gases

  • they are inert as they have a full outer shell (typically 8, but 2 for helium)
  • the boiling/melting points increase as you go down the group
34
Q

What are group 1 metals known as and what are properties/ trends of group 1 metals?

A

Alkali metals

  • soft
  • low density
  • low boiling point
  • highly reactive- easy to lose the single outer electron
  • boiling/ melting points decrease as you go down the group
  • reactivity increases as you go down the group because the distance from the nucleus increases and this means there are weaker forces of attraction between the outer electron and nucleus
35
Q

How do group 1 metals (alkali metals) react with:
a)water
b)oxygen
c)chlorine

A

Water ~ react vigorously and form
metal hydroxide + hydrogen

Oxygen ~ vigorous, react to produce metal oxides: sodium oxide, sodium peroxide, potassium peroxide, potassium superoxide etc…

Chlorine ~ react vigorously, ionic compounds with chlorine

36
Q

What are group 7 metals known as and what are the properties/trends of group 7 metals?

A

Halogens

  • the reactivity decreases as you go down the group- weaker attraction means it’s harder to gain and electron
  • as you go down the group the melting and boiling point increases
  • more reactive halogen can displace a less reactive halogen from an aqueous solution of its salt
37
Q

True of False: group 7 elements are not found in pairs

A

False: group 7 elements are diatomic

38
Q

compare: Transition metals vs Group 1 metals

A
  • transition metals are harder, greater strength
  • transition metals have higher boiling points and densities
  • transition metals have ions with different charges whilst group 1 metals only have one
  • transition metals can form coloured compounds
  • transition metals can be used as catalysts(e.g. Iron in the haber process)
  • reaction with oxygen: very slow or not at all(at room temp) vs. group 1 elements which react quickly with oxygen
  • reaction with water: very slow with cold water or not at all
  • some transition metals react to with halogens such as iron

GCSE CHEMISTRY PAPER 1 (5 decks)

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