Topic 1 Atomic Structure and the Periodic Table

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53 Terms

1
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what relative mass does a proton have

whats the relative charge of a proton

where is the proton

1

+1

nucleus

2
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neutron

relative mass

relative charge

where is it located

1

0

nucleus

3
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electron

relative mass

relative charge

where is it located

1/2000

-1

shell

4
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atomic number define

mass number define

how to work out number of neutrons

number of protons

number of particles in nucleus

mass number - atomic number (top number - bottom number )

5
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whats an ion

whats a pos and neg ion

an atom that has lost or gained electrons

positive ion= atom that has lost electrons

negative ion = atom that has gained electrons

6
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how are elements organised

what do elements in a group have in common

what do elements in a period have in common

by the atomic number increasing

how many electrons in the last shell

configuration number gains 1

7
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disolve meaaning

the process where a solute dissolves in a solvent to form a solution

8
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solute define

a substance that is dissolved in a solution

9
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solution define

solute dissolved in a solvent

10
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mixture define

2 or more substances which arent chemically combined

11
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solvent meaning

whats being dissolved in the solute (substance)

12
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what are different ways of separating a solvent from an insoluble solute

  • filteration

  • evaporation (crystalation )

  • distilation

13
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filteration

14
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isotope meaning

different forms of the same element, that have the same number of protons but diff number of neutrons

chemically react the same

15
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calculating an isotopes relative mass equation

sum of (isotope abundance x isotope mass)/ sum of abundance of all isotopes

16
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calculate the relativve atomic mass of copper to 1 dp

copper 63 with an abundance of 69.2%

copper 65 with an abundance of 30.8%

sum of (isotope abundance x isotope mass)/ sum of abundance of all isotopes

=(63 × 69.2) + (65 × 30.8)/69.2 + 30.8

=6361.69/100

=63.6

17
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molecule define

2 or more atoms held together by a chemical bond

can contain different or the same elements

18
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compound define

2 or more DIFFERENT elements held together by chemical bonds

always found in the same proportions

19
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how many atoms of each element are in H2SO4

2 Hydrogen

1 Sulfur

4 Oxygen

20
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how many atoms of each element are in Ca(OH)2

1 Ca

2 OH

21
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filteration

what does it do

method

separates insoluble solids from solids

put filter paper into funnel and pour mixture into it

22
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evaporation

what dones it do

method

advantages

disadvantages

seperates a soluble solid from a solution

put solution into evaporating dish and put over budsen burner with a tripod - solvent evaporates solution more concentyrated , crystals form as solution is so concentrated

quick, easy

some solids decompsose when heated - thermal decomposition

23
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crystalisation

what is it

method

disadvantage

seperating soluble solids from a solution which are solids suseptable to thermal decomposition

place solution into evaporating dish and heat gentkly in a water bath - when some solvent has evaporated and some crystals form stop heating and leave to cool - more crystals form as solids are less soluble at colder temps), filter crystals, and dry them in somewhere warm

slower

24
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simple distillation

what it does

equipment

method

separates out a liquid from a solution

flask (containing solution), sealed with bung so no gas escapes, thermometer inside to measure temp, condenser surrounded by water jacket, beaker at end on condenser, Bunsen burner under flask

heat mixture so liquid we want evaporates, rises up top of flask pressure forces down the condenser and cold water through water jacket cools down the vapour condescending it into liquid collecting into beaker until all we have in flask is salt

25
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fractional distillation

what it does

equipment

method

main techinque of sepearting mixtures of liquids

same as simple distillation but beofe going to condenser vapour goes into fractionating column

which is full of little glass rods (high surface areas), cooler at top than bottom as its so tall

heat mixture to lowest liquids boiling point so it evaporates and rises throughfractionating column and through condenser into liquid

dio the same for the next liquid and so on

its just that pure liquid in the beaker at the end as the clear rods in the reactionating column are so cold the vapour thats evapoarting turns into liquid and falls back into the mixture

26
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When Democritus first conceived of atomic theory, around 500 BC, how did he describe atoms?(3)

Separated from each other by empty space

The smallest possible unit of matter 

Small spheres

27
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john dalton (1800s)

described the atom as (2)

solid neutral ball

different types of sypheres make up diff elements

28
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JJ thomson (1897)

plum pudding atom

neutral solid ball of positive electrons stuffed in it

29
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How Rutherford developed the nuclear model (4)

  • In Rutherford's experiments, alpha particles were fired at a thin sheet of gold foil.

  • Most particles passed through, but some were deflected off course. 

  • This caused him to hypothesise that there was a dense region of positive charge at the centre of the atom that repelled the alpha particles.

  • As a result he developed the nuclear model of the atom, in which there was a central positive nucleus, surrounded by negative electrons. 

30
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what was the issue with rutherfords atom

what was bohrs responce (1913)

the atom should collapse as the negative electrons would be attracted to the positive nucleus, causing them to rush inwards.

electrons orbit the nucleus in shells

31
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who discovered the neutron (20th centry)

Chadwick

32
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who designed the periodic table

why did he leave gaps in his periodic table

dimitri mendeleev

a russian scientist in mid 19th century

for elements that had not yet been discovered (he predicted the mass and properties of missing elements)

33
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whta is on the nuclear symbol (3)

elemental symbol (e.g Na)

bottom left - atomic number (number of protons)

top left - mass number (number of protons and neutrons)

34
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what does each group have in common with each other

same number of electroer ns in their outershell (e.g group 1 has 1 electron in their outershell)

35
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what do metals form when they react

non metals

positive ions

dont form ions/ negative ions

36
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metals + non metals physical properties

metals

  • very strpong bonds (metallic bonding)

  • malluable

  • conductors of heat + electricity

  • high melting/ boiling point

  • shiny

non metals

  • dull

  • brittle

  • low melting/boiling points

  • low density

  • arent good conductors of heat

37
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physicall properties of transitition metals

  • good catalysts

  • can form more than 1 ion

38
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what are group 1 metals called

group 7

group 0

alkali metals

halogens

nobel gases

39
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properties of alkaili metals

  • soft

  • low density

  • low melting/boiling point

40
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as you go down group 1 do the elements get more or less reactive - why

more reactive

as they have more shells so there’s less attractive force from the nucleus to the outer shell - easier to loose the electron in the outer shell

41
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sì melting / boiling point increase/ decrease as you go down group 1

decrease

42
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what forms whrn an alkali metal and water react

e.g sodium

alkali metal + H2O → alkali metalOH(metal hydroxide) + H2

2Na + 2H(2)O → 2NaOH + H2

43
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what happens when alkali metals react with chlorine

what do they form

è.g sodium

Na + Cl → NaCl

shite metal chloride salts

44
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what happens when alkali metals react wiyh oxygen

metal oxides (type of oxide depends on the type of metal)

lithium oxide (Li(2)O

sodium oxide (Na(2)O) / sodium peroxide (Na(2)O(2)

potassium peroxide (K(2)O2) / potassium superoxide (KO2)

45
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halogens - melting/boiling points increase or decrease

increases

46
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halogens - reactivity increase or decrease

why

decrease

outer shell gets further away from nucleus as you go down - attractive force gets weaker so it can’t attract an electron to complete its outer shell then it can’t react

47
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physical properties kf

fluorine

chlorine

bromine

iodine

flourine - poisoness yellow coloured gas

chlorine - green xoloured gas

bromine - red- brown volatile liquid - poisonous

iodine - grey xoloured solid wiyh purple vapor’s

48
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what happens to the names in group 7 whrn they form ionic bonds with metals

adds a ‘D’

e.g floride, chloride, bromide, iodide

49
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arw group 7 atoms diatomic

yes

they share atoms and form a covalent bond

50
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how do noble gases react as

colourless gasses

51
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inert meaning

are noble gases inert

don’t react with anything

yes - arent flammable

52
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does boiling point of noble gases increase/ decrease as you go down the group

increase

same as halogens

53
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what colour is

halide salts

bromide water

chlorine water

iodine water

colourless

orange

colourless

brown