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Chemistry > c2- the periodic table > Flashcards

c2- the periodic table Flashcards

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1
Q

periodic table are arranged in columns called
and what ae periods ,

A

groups
rows

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2
Q

where are the trasition metals ?

A

se to zn .

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3
Q

where are the non metals ?

A

A staircase from aluminium .

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4
Q

Why is it called the periodic table ?

A

As it is arrnaged with elements with similar propeorties at regular intervals .

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5
Q

All elements in a group have …

A

simialr chemical propeorites .
-they all reacti in a similar way - as all the lements ina group have the same number of electrons in their outer energy level .

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6
Q

What did Johann Dobereiner notice ?

A

-He noticed that elemnts with similar properties often occured in threes , these are called “triads”.

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7
Q

What happend 40 years after Johann ?

A

John Newlands arranged the elements in order of increasing atomic weiht .
-He saw that every eight elemnt react in the ame way - called this his law of octaves .

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8
Q

Problem with John Newlands idea .

A

-y always sticking to the exact order of the atmoic weight
some elements grouped and togther and they had totally differnet propeorties ,
-meant that law of octaves wasnt taken seriously y other scienitsts .

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9
Q

What Dmitri Mendeleev do ?

A

-e devloped the first modern Peroidic table .
-Mendeleev started by arranging the elemnts in order of increasign atmoic weight .

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10
Q

What Dmitri Mendeelv do that ONLY he did ?

A

-If he needed to swwitch the order of speicific elements , he did so it fitted patterns of elements in the same group .
-also realised , some elemnts have not been yet discovered , so he left gaps for them

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11
Q

what happened next with mendeelev’s gaps ?

A

-as he was so confident in his periodi ctabe , he actulaly predicted propeorties of some undiscovered elements , when they later were found , mendeleev’s predcitions were correct .

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12
Q

What was one way the modern periodc table differs from Mendeeleev;s .

A

The modern periodic table , elements arranged in order of atmoic number . (protons werent discoevrred tthen so mendeelev ordered in ATMOIC WEIGHT ).

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13
Q

What is the problem with ordering in atomic weight ?

A

-Elements can appear in wrong order due to presence of isotopes .

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14
Q

What is another way the modern periodic table differs from Mendeelev’s ?

A

The modern periodic table has group 0 ; noble gases (had not been discoevred when Mendeleev published his table ).

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15
Q

What are group 1 metals called ?

A

The alkali metals .
-All group 1 metals havw 1 electron in their outer enegry level .
-group 1 metals are soft .
-low melting points and densities
-form 1+ions

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16
Q

Hhow do group one metals react with oxygen .

A

all group 1 metals react rapidly with oxygen .
group 1 metals react more rapidly as we move down group 1 .

17
Q

Write symbol equation for group 1 metals reacting with oxygen .

A

4Li+O2—->2Li20
change the metal for all others group 1 metals .

18
Q

How do group 1 metals react with chlorine .

A

React rapidly with chlorine .
2Li+Cl2—>2iICl

DIATOMIC CHLORINEEEE

change the metal for all other group 1 meals .

19
Q

How do group 1 metals react with water ?

A

-Universal indicator in water .
Lithium reatcs rapidly with water (more rapid down g1)
-fizzinng (hydrogen produced ).
universal indicator goes purple showing ALKALINE prsent hence alkali metals .

20
Q

State symbol and word equation for alkalines reacting with water .

A

Lithium + water — > Lithium hydroxide +hydrgoen
Lithium hydroxide is a alkaline hence pirple colour , hydrogen is the fizzing effervescence .
2li +2H20—>2LIOH+H2
change for different metals in different metls .

21
Q

As we move down group 1…

A

metals get more reactive .
g1 looses ouer electron when they react .
-As we move down the group the outer electron is less attarcted to the nucleus and easier to loose .
-As there is a greater distance beween positive nucleus and negative outer electron .
-The outer electron is shielded from the nucleus’s intenral energy levels .

22
Q

What are elemnts in group 7 known as ?

A

The halogens .

23
Q

How manye elctrons do Group 7 elemnts have ?

A

They have 7 electrons on their outer shell .

24
Q

How do group 7 elemnts form molecules ?

A

Form molecules with two atoms joined bby a covalnet bond .

25
Q

What temperature is roomt temperature .

A

20 degrees .

26
Q

As you go down group 7 , the melting and boiling point …

A

Increase .

27
Q

What are Fluorine and Chlorine at Room temperature ?

A

Gases at room tempeatrue as their melting and boling points less than 20 l.

28
Q

What is Bromine at room temperature ?

A

Liquid , meltin point lower than 20 , but boiling point higher than 20 .

29
Q

Iodine at room temperature ?

A

Idoine is a solid , but metling and boiling point higher than 20 .

30
Q

The relative molecule mass of group 7 …

A

Increases as you go down gthe group
Group 7 elemnts form covalent compounds when they react wwith other non-meals . .

31
Q

Grooup 7 non -metals react with metals to form …

A

ionc compounds .
-the gain one electon also .
so have an overall 1minus charge when they react with METALS . end in ide instead of INE as well .

32
Q

What is the reactivity series in group 7 ?

A

The elems get less reactive as you gown the group.
Chlrine gains electron less easily than fluroine WHY ?
-Greater neergy level from nucleus
-shieldign bby internal electors .
-harder for chlrine to attarct an electron than for fluroine .

33
Q

displacement reactions in Halogens abt reaction ?

A

-A more reactive halgoen will displace a less reactive halogen froma n aqueous solution of its salt .

34
Q

Example of key rule in Halgoen displacement reactions .

A

Fluorine+Sodium Chloride —>Sodim fluoride+chlorine
Chlorine gets displaced as Fluorine is MORE reactive .

35
Q

What are transition metals ?

A

-Hard and strong metals .
-HIgh melting point (mercury excepition )
-HIgh denisty .

36
Q

What are transition metals (2)

A

-Much less reactive than group 1 metals (with oxygen chlorine and water .)
-can form ions with differen charged
-form coloured copounds
-used as catlaysts .

37
Q

Example of coloured compounds in Transiiton metals ?

A

Iron oxide (III) Reddish
Manganese Chlirde (II) Pink
Chromium Chloride (III) Purple

Chemistry (20 decks)

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