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Chemistry AQA > C1- Atomic structure and periodic table > Flashcards

C1- Atomic structure and periodic table Flashcards

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1
Q

What is the composition of the atom

A
  • Atoms are aprox 0.1 nanometers in radius
  • Atoms are made up of three parts
  • Nucleus- Which contains PROTONS and Neutrons- positive charge-
  • Electrons- move around in electronic shells- Negatively charge. Equal to number of protons
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2
Q

What is the charge and mass of each of the parts of the atom

A

Proton- Relative mass 1. Charge 1

Neutron- Relative mass 1. Charge 0

Electron- Relative mass negligible. Charge -1

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3
Q

What do the numbers on periodic tables tell us

A
  • Nuclear symbol tells you its atomic and mass number
  • Atomic number- Bottom- Tells number of protons
  • Mass number- tops - cells total number of protons and neutrons
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4
Q

What is an element

A
  • An element is a substance made up of atoms that have the same number of protons in their nucleus
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5
Q

What is an isotope

A
  • An isotope is a different form of the same element which have the same number of protons, but a different number of neutrons
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6
Q

What is the calculation for relative atomic mass

A
  • Relative atomic mass = (isotope abundance x Isotope mass number)// Sum of abidances of all the isotopes
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7
Q

What is a compound

A
  • A compound is two or more elements that are chemically joined
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8
Q

What is covalent bonding

A
  • The sharing of electrons between non-mental atoms in Compounds
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9
Q

What is ionic bonding

A
  • The compound between a metal and non-metal in which outer shell electrons are lost and gained. This forms a charge
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10
Q

What is a mixture

A
  • A mixture is the mixing f elements or compound that can be physically separated. They have no chemical bond
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11
Q

Describe the steps in chromatography

A
  • Draw a lie near the bottom in panic
  • Place a spot of ink and place in a beaker of solvent
  • Make sure the ink isn’t touching the solvent
  • The solvent sees up taking the ink with it
  • Each different dye in the ink will move up the paper at a different rate so they will separate out
  • If any dyes are insoluble they’ll stay at the bottom
  • When the solvent is close to the top, take the paper out and mark where the ink has moved to
  • This has produced a chromatograph
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12
Q
  • What is filtration
A
  • Filtration is a physical separation technique that separates insoluble solids from liquids
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13
Q

WHAT IS EVAPORATION

A
  • Evaporation is the method of separating soluble solids from solutions
  • The steps are
  • Pour liquid into evaporating dish-
  • Slowly head. eventually crystals will start to form
  • Keep until dry crystals are formed
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14
Q

What is crystallisation

A
  • Crystallisation is used when solids break down when they are heated and evaporation isn’t an option
  • It separates soluble solids from solutions
  • The steps are as follows
  • Pour solution into evaporating dish
  • Gently heat and when some has been evaporated remove wish and cool,
  • Filter the solution and leave in war, place
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15
Q

What are the steps in separating rock salt

A
  • Grind mixture
  • Put mixture into water and stir
  • Filter out the sand-
    _ Evaporate the water and dry crystals are left
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16
Q

What is distillation

A
  • Distillation is used to separate mixtures that only contain liquids
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17
Q

What is simple distillation

A
  • Used for separating liquids in a solution
  • The solution is heated. The part with the lowest boiling point evaporates first
  • The vapour is cooled ,
    condensed and collected
  • The rest of the solution is left behind in the flask
  • An example of the use of this is getting pure water from seawater
  • The issue with it is you can only use it for liquids with drastically different boiling points
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18
Q

What is fractional distillation

A
  • Used for mixtures of liquids with close boiling points
  • Here is how it would be used for crude oil
  • Mixture placed at bottom of flask and a fracturing column would be placed upwards
  • The mixtures would have different boiling points so they evaporate at different temperatures
  • Liquids with lowest boiling point evaporate. When temperature of thermometer at the top matches the boiling point it will rise
  • As it is cooler at the top the liquids that may begin to evaporate which have higher boiling points will not make it all the way to the top. This can be repeated after all the first liquid is collected for multiple liquids.
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19
Q
  • Give brief history on the Atom
A
  • Start of 19th century John Dalton described atoms as solid spheres and said different spheres made up different elements
  • 1897 JJ Thompson concluded that atoms were not solid spheres. he discovered electrons. Plumb pudding model
  • 190 Earnest Rutherford conducted the alpha particle experiment. This concluded that That the Plumb pudding model was wrong and the Nuclear model was proposed
20
Q

What is the plumb pudding model

A
  • Plumb pudding model was proposed by JJ Thompson in 1897 which shows the atom as a ball of positively charged electrons
21
Q

What was the alpha particle scattering experiment

A
  • Disproved plumb pudding model
  • conducted in 1909 by Earnest Rutherford
  • They fired positively charged alpha particles through gold. Plumb pudding model would mean they would pass right through.
  • Some were deflected more than expected and some backwards
  • This meant that the plumb pudding model couldn’t be correct
22
Q

What is the nuclear model

A
  • A model for there atom that states the electrons are in a cloud around a nucleus made up of negative electrons - where most the masses found.
  • Protons were found later in experiments where it was found that the nucleus could be divided further. They have the same charge as Hydrogen nucleuses
  • Neutrons where discovered by James Chadwick who provided evidence for neutral particles
23
Q

What is is Bohr’s nuclear model

A
  • Niel Bohr’s nuclear model of an atom suggested that electrons were contained in shells
  • Bohr proposed that electrons orbit the nucleus in fixed shells.Each shell is a fixed distance from nucleus
  • Supported by many experiments and helped explain other observations at the time
24
Q

Describe the structure of electrons

A
  • Electrons are organised into cells
  • Electrons in an atom occupy the lowest available energy levels- innermost available cells
  • first shell has 2, rest have 8
  • Atom strive for a ful outer shell stable
25
Q

How can the structure of an atom be represented

A
  • Diagram

- Numbers

26
Q
  • What was the first type of periodic table seen
A
  • Tries to organise them according to weights- relative atomic mass
  • 1800
  • Not complete, some elements placed in wrong group
27
Q

What did Dimitri Mendeleev do

A
  • 1869
  • Left gaps
  • took 50 known elements- placed mainly in atomic mass- switched if properties didn’t match
  • Gaps were left to make sure elements with similar qualities could be put in- not yet been discovered
  • Eventually filled
28
Q

-HOW do isotopes make its possible for the elects not to be in exact order

A
  • Isotopes made it clear placing them in order of atomic mss was not correct
  • Different atomic ,asses sa,e chemical properties- cause irregularity
29
Q

How is the periodic table organised

A
  • Elements in periodic table are arranged in order of atomic number so that elements with sillier properties are in the same Columns- Groups
30
Q

What does the group number of an atom tell us

A
  • Same number of electrons in outer shell

- Gives similar chemical properties

31
Q

What are metals- periodic table

A

Elements that react to form positive ions

most elements

Found towards bottom and left

32
Q

What are non-metals-periodic table

A

Elements that do not form positive ions

Found towards right and top

33
Q

How does electronic structure influence how they will react

A
  • Metals don’t need much energy to create ions

- Non-metlas much harder to react

34
Q

What are the physical properties of metals

A
  • Strong, malleable
  • Great conductors of heat and electricity
  • High boiling and melting points
35
Q

What are the physical properties of non metals

A
  • Don’t have ,italic bonding
  • Dull looking
  • Brittle
  • No always solid
  • Bad conductors and lower density
36
Q

What are group one metals

A
  • Alkali metals
  • One electron in outer shells
  • Form ionic compounds with non-metals
37
Q

How do Alkali metals react with water

A
  • Produce hydrogen gas
  • React very rigorously
  • Amount of energy produced increases down the group
  • Form hydroxides that dissolve to give alkaline solutions
  • More around surface and fizz furiously
38
Q

How do alkali metals react with chlorine

A
  • React vigorously
  • Form white salts- metal chloride
  • Reactivity increases down group
39
Q
  • How do alkali metals react with oxygen
A
  • Can react to form a metal oxide
  • different types of oxide form
  • Lithium oxide
  • Sodium oxide and sodium peroxide
  • Potassium peroxide and potassium superoxide
40
Q

What are group 7 elements

A
  • Halogens
  • 7 electrons in outer shell
  • Non-metals that consist of molecules made up of pairs
41
Q

What are the first 4 group 7 metals properties

A
  • Fluorine- Very reactive. Yellow gas
  • Chlorine- Fairly reactive green gas-
  • Bromine- dense red brown volitive liquid
  • Iodine- Dark grey crystalline solid- or purple vapour
42
Q

What are the trends seen in group 7 as you go down

A
  • They become less reactive- outer shell further from nucleus
  • High meting point and boiling point
  • Higher relative atomic mass
43
Q

How do Halogens react to form compounds

A
  • Non metals- covalent bonding - Simple molecular structure
  • Metals- Form ionic bonding.
44
Q

How do halogens displace

A
  • More reactive halogen can displace a less reactive on from an aqueous solution of its salt
45
Q

What is group 0

A
  • Noble gases
  • Include helium, neon , argon
  • Full outer shell
  • Uncreative
46
Q

What is the trend seen in nimble gasses

A
  • BOiling points increase as you move down the group

- This is as due to increase in number of electrons- greater intermolecular forces that are harder to break

Chemistry AQA (10 decks)

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