Topic 1 Flashcards

1
Q

What is an element

A

Elements consist of atoms with the same atomic number

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2
Q

How to calaculate relative atomic mass

A

Sum of (isotope abundance x isotope mass number
_______________________
Sum of abundances of all the isotopes

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3
Q

What is a compound

A

A substance formed by two or more atoms that are chemically bonded together

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4
Q

What is a mixture and how can they be separated and give examples

A

A mixture has no chemical bonds and can be separated by physical methods eg filtration,crystaliseation,fractional distilleration,chromatography

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5
Q

What is filtration and give an example

A

Filtration separates insoluble solids from liquids
It can be used for purification

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6
Q

What is the first way you can separate soluble solids from solutions

A

Evaporation
Pour solution into evaporating dish
Heat solution,solvent will evaporate then getting more concentrated,the crystals will form
Keep heating till your left with dry crystals

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7
Q

What is the second way you can separate soluable solids from solutions

A

Crystallisation
Pour solution into evap dish ,gentally heat ,some solvent will evap making solution more concentrated
When you see crystals start to form remove dish from heat and leave to cool
Salt should start to form crystals as it becomes insoluble to cold and place in warm place to dry

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8
Q

What is fractional distilleration

A

Used to separate a mixture of liquids

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9
Q

Decribe the practical of distilleration

A

put mixture in flask and put fracturing column on top then heat it
Diff liquids will have diff boiling points and evap at diff temps
Liquid with lowest boiling point evap a first ,when the temp on thermometer matches boiling point of liquid it will reach top of column
When first liquid has been collected raise temp UNTILL next one reaches top

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10
Q

Who described atoms as solid spheres

A

John dalton

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11
Q

What did jj Thomson conclude from his exeripemts

A

That atoms wernt solid spheres
His measurements of charge and mass shows that an atom must contain even smaller and negatively charged particles

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12
Q

What did the solid sphere idea get changed to

A

Plum pudding model

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13
Q

What does the plum pudding model show

A

Ball of positive charge with electrons stuck in

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14
Q

What did Rutherford show

A

That the plum pudding model is wrong

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15
Q

In 1909 what happened

A

Rutherford and marsden conducted alpha particle scattering experiments

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16
Q

What is the alpha particle scattering experiments

A

Fired positvely charged alpha particles at and extremely thing peice of gold

17
Q

How did the alpha particle scatting experiment prove that the plum pudding wasn’t right

A

The expectation was that only the particles would pass through the sheet or be slightly deflected due to the positive charge of each atom being spread out
However while most going through some were deflected more than expected and a small number were deflected backwords so plum pudding couldn’t be right

18
Q

What idea did Rutherford come up with to explain this new evidence

A

The nuclear model
Where there’s a tiny positively charged Nucleas at the centre where most mass is concentrated

19
Q

How did rutherfords nuclear model differ from bohrs model

A

Rutherford thought that electrons clouded the nucleus so most of atom is empty space
Bohr suggest that electrons were in shells that orbit the nucleus

20
Q

In the 1800 how were elements arranged

A

By atomic weight

21
Q

How were the early periodic tables wrong

A

They were not complete and some events were places in wrong group due to elements being placed in order of atomic weight and did not take into account of their properties

22
Q

Why were gaps left in dmitri Mendeleev table of elements

A

Because there was undiscovered elements and allowed Mendeleev to predict what properties they had

23
Q

What are group 1 called

A

Alkali metals

24
Q

What are the properties of the group 1 element

A

Soft ,low density and the first 3 elements are less dense than water

25
Q

Why are the alkali metals very reactive

A

Due to them only having 1 electron in outer shell

26
Q

What are the trends for the alkali metals as you go down the group

A

Increasing reactivity
Due to electron being further away from nucleus
Lower melting point and boiling point
Higher relative atomic mass

27
Q

What are the propers ionic compounds of alkali metals

A

Usually white solids that dissolve in water to produce a colourless solution

28
Q

What happens when alkali metals react with water

A

React vigously to prouduce hydrogen gas and metal oxides
The more reactive the more violent it is
The energy given out also increases

29
Q

What happens when you react a alkali metal with chlorine

A

React vingoursly when heated in chlorine gas to form white metal chloride salts
As you go down the group reactivity increases making reaction more vigouros

30
Q

What happens when you react a alkali metal with oxygen

A

Lithium reacts to form lithium oxide
Sodium reacts to form a mixture of sodium oxide and sodium peroxide
Potassium reacts to form a mixture of potassium peroxide and potassuim superoxide

31
Q

What are the halogens colours vapours

A

Fluorine poisionous yellow gas
Chlorine fairly reactive dense green gas
Bromine dense poisonous red brown volitile liquid
Iodine dark dark grey crystalline solid or purple vapour
All in pairs

32
Q

What trends happen in group 7

A

Become less reactive harder to gain an extra electron
Higher melting and boiling points
Higher relative atomic masses

33
Q

What are halogens that form ionic bonds with metals called

A

1- ions called halides

34
Q

What happens with more reactive halogens

A

They will displace less reactive ones

35
Q

Properties of noble gasses

A

Monatomic gases
Coulorless gasses at room temps
Non flammable due to them being inert

36
Q

What happens to the boiling points of the halogens as you go down the group

A

Boiling points increase