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Chemistry > C1 - Atomic Structure And The Periodic Table > Flashcards

C1 - Atomic Structure And The Periodic Table Flashcards

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1
Q

Information on filtration.

A

Filtration separates insoluble solids from liquids
Used if your project is an insoluble solid that needs to be separated
Solid impurities in the reaction mixture can be separate with filtration ‘purification’

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2
Q

Information on evaporation

A

Separates soluble solids from solutions
Solution into evaporation dish
Slowly heat solution > solvent evaporates and solution will get more concentrated > crystals will start to form
Only use if salt doesn’t decompose when heated otherwise have to use crystallisation

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3
Q

Information on crystallisation

A

Pour solution into evaporation dish and gently heat
Some solvent will evaporate and solution becomes more concentrated, once crystals start to form, leave it to cool and the salts will form crystals as it becomes insoluble in cold, concentrated solutions

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4
Q

Filtration and crystallisation to separate rock salt

A

Mixture of salt and sand, salt dissolves, sand doesn’t.
Grind mixture and make sure salt crystals are small
Pour into water and stir until salt dissolved
Filter mixture to remove sand
Evaporate water so salt forms dry crystals

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5
Q

Number of protons =

A

Number of electrons

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6
Q

Why do atoms have no charge

A

Protons and electrons charge cancel each other out

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7
Q

Relative mass and charge of proton, neutron and electron

A

Electron mass of almost 0, charge of -1
Proton mass of 1, charge is +1
Neutron mass of 1, charge is 0

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8
Q

What’s the atomic number

A

How many protons

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9
Q

What’s the mass number

A

Total number of protons and neutrons

Neutrons = atomic number - mass number

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10
Q

What’s an isotope

A

Different forms of the same elements
Same protons but different number of neutrons
E.g carbon 12 and carbon 13

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11
Q

What are elements

A

Elements consists of atoms with the same atomic number.

Each atom has a different number of protons, neutrons and electrons. The proton amount determines what atom it is

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12
Q

Why is there a relative atomic mass

A

As many elements exists as isotopes

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13
Q

Formula of relative atomic mass (Ar)

A

Relative atomic mass = sum of (isotope Abundance x isotope mass number)/ sum of abundance’s of all isotopes

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14
Q

Example of relative atomic mass calculation

A

Copper
Cu 63 abundance of 69.2%
Du 65 abundance of 30.8%

(69.2 x 63) + (30.8 x 65) / 69.2 + 30.8 = 63.6

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15
Q

What are compounds

A

Two or more atoms joined together to make a compound
Substances formed from 2 or more elements.
Atoms in fixed proportions and chemically bonded

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16
Q

Why is it hard to separate compounds

A

Because you need a chemical reaction
Properties of a compound are different to elements
Compound with metals and non-metals consist of ions
Compounds with non-metals consist of molecules
Compounds can be shown with a formula

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17
Q

Common compound formulas of ammonia, sodium chloride, carbon monoxide, hydrochloric acid, calcium chloride, sodium carbonate and sulphuric acid

A 
Ammonia - NH3 
Sodium chloride - NaCl 
Carbon monoxide - CO 
hydrochloric acid - HCl 
Calcium carbonate - CaCl2
Sodium carbonate - NaCO2
Sulphuric acid - H2SO4
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18
Q

What are chemical equations

A

Equations that show a chemical reaction

Symbol equations are shorthand

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19
Q

What is meant by balancing an equation

A

Same number of atoms on each side

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20
Q

John Dalton to atom

A

Described atoms as solid spheres

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21
Q

JJ Thomson on atoms

A

Atoms contained smaller electrons - plum puddin

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22
Q

Rutherford on atoms

A

Alpha particle scattering experiment
Fired positively charged alpha particles at gold foil - most of through
Some deflected, some changed direction kind of due to alpha particles hitting tiny nucleus
Therefore atom mostly empty space

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23
Q

Bohrs nuclear Model

A

Suggested atoms in shells - electrons orbit at fixed shells(energy levels)

24
Q

James Chadwick on atoms

A

Provided evidence for neutrons

25
Q

Where’s the lowest energy level

A

Closest to the nucleus - always filled first

26
Q

Electronic structure of electrons

A

Always 2, 8, 8, 8 etc

27
Q

Why is it better to have a full outer shell

A

So the atom doesn’t want to react to fill it - unstable

28
Q

Early 1800s periodic table

A

Elements arranged by atomic mass - no idea on protons, neutrons or electrons
Only measure relative atomic mass

29
Q

Dimitri Mendeleev’s periodic table

A

1869 Mendeleev took 50 known elements and arranged them and left gaps
He put in order of atomic mass but switched order if properties didn’t match
E.g iodine has a smaller mass, but placed after tellurium as it had similar properties to elements in that group
Some gaps indicated undiscovered elements

30
Q

How did isotopes support mendeleev’s table

A

Proved not to order on relative atomic mass but to take into account properties
Isotopes have different masses but same chemical properties

31
Q

Information on modern periodic table

A

Ordered in increasing atomic number - repeating properties
Metals on left, non-metals on right
Elements with similar properties form columns
Vertical columns form groups

32
Q

What do group numbers on the period table tell you

A

Group number tells you how many electrons on the outer shell
Group 1 = 1 electron
Group 0 = full outer shell
This is useful as atoms react depending on number of electrons in outer shell

33
Q

Rows are called…

A

Periods. Each new period represents another full outer shell of electrons

34
Q

Information on metal elements

A

Metal Elements form positive ions when reacted

They’re on the bottom and left of table

35
Q

Information on non-metal elements

A

Non-metals are far right and top

Don’t generally form positive ions when they react

36
Q

Why do atoms react

A

To try form a full outer shell of electrons - by gaining, loosing or sharing electrons

37
Q

How to metals to the left and bottom react

A

Left - Don’t have many electrons to remove - easier to remove electrons as there’s not as many
Bottom - more electrons but they’re further away from nucleus so feel a weaker attraction - not much energy needed to remove so it’s feasible for these elements to form positive ions

38
Q

How do non-metals to the top and right react

A

Right - lots of electrons to remove
Top- outer electrons close to the nucleus - strong attraction
Therefore more likely to gain or share electrons so not as much energy is used to get rid of them

39
Q

Properties of metals

A

Metallic bonding
Strong, can be bent or hammered(malleable)
Good heat + electric conductors
High boiling and melting points

40
Q

Properties of non-metals

A 
No metallic bonding 
Dull looking
Brittle 
Aren’t always solid at room temperature 
Lower density 
Don’t really conduct electricity
41
Q

What are group 1 metals

A

Alkali metals, they’re reactive soft metals

42
Q

List the Alkali metals(group 1)

A

Lithium Li, sodium Na, potassium K, rubidium Rb, caesium Cs, francium Fr

43
Q

Properties of group 1 alkali metals

A

1 electron in outer shell, very reactive soft and low density
Increasing reactivity as you go down - electrons further from nucleus
Lower melting and boiling points as you go down
Higher relative atomic mass as you go down

44
Q

What do alkali metals form with non metals

A

Form ionic compounds
Group 1 don’t need much energy to lose their outer electron - readily forms 1+ ion
So easy they only ever react to form ionic compounds
Compounds generally white solids that dissolve in water to form colourless solutions

45
Q

What happens when group 1 reacts with water

A

Vigorous reaction
Li, Na and K float, move and fizz on surface. They produce hydrogen when reacting
K and below ignite hydrogen with their energy

46
Q

Group 1 reaction with oxygen

A

Lithium oxide
Sodium oxide or potassium peroxide
Potassium peroxide or potassium superoxide

47
Q

Group 1 reaction with chlorine - what does it produce

A

Produces salt.
Group 1 reacts vigorously when heated in chlorine gas to form white salts and metal chlorides
Go down group = more vigorous

48
Q

What are the group 7 elements

A

Called halogens - all non metals and coloured vapours

49
Q

Group 7 coloured vapours and their reactive ness

A

Fluorine - very reactive, poisonous yellow gas
Chlorine - fairly reactive, poisonous dense green gas
Bromine - dense, poisonous red brown volatile liquid
Iodine - dark grey crystalline solid or purple vapour
There’s also astatine

50
Q

Properties of group 7 elements

A

All exist as molecules which are pairs of atoms
As you go down - become less reactive as it’s harder to gain an electron - further away
Higher melting/boiling points
Higher relative atomic mass

51
Q

Halogens can form…

A

Molecular compounds
Halogens share electrons via covalent bonding with other non-metals to achieve full outer shell
Compounds that form when halogens react with non metals all have simple molecular structures

52
Q

What do halogens form with metals

A

Form ionic bonds
Halogens with 1- Ions are halides when they bond with metals
Compounds formed have ionic structures

53
Q

More reactive halogens will displace…

A

Less reactive ones
Displacement reaction can happen between more reactive halogens and the salt of a less reactive one.
E.g chlorine displace bromine and iodine form an aqueous solution of its salt
Chlorine + potassium iodide -> iodine + potassium chloride

54
Q

What are group elements

A

All inert colourless gases

55
Q

Properties of group 0 elements

A

All eight electrons in outer (helium has 2)
Outer shell energetically stable - don’t have to give up or gain electron
Inert as they don’t react much - also non flammable
Exist as monatomic gases - single atoms NOT bonded to each other
All colourless at room temperature
As you go down, increase boiling point, increase relative atomic mass
Increase in boiling due to the number of electrons in each atom - greater inter molecule forces between them - harder to overcome

Chemistry (10 decks)

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