3.2 Inorganic Chemistry: .3 Group 7, the halogens Flashcards Preview

Chemistry AS > 3.2 Inorganic Chemistry: .3 Group 7, the halogens > Flashcards

Flashcards in 3.2 Inorganic Chemistry: .3 Group 7, the halogens Deck (49)
Loading flashcards...
1

what is the trend in atomic radius down the group 7 elements?

the atoms gets bigger going down the group because each element has one extra filled main level of electrons compared with the one above it

2

what is electronegativity?

the tendency of a atom to attract the pair of electrons in a covalent bond

3

what is the trend in electronegativity going down the group 2 elements?

-there is a decrease in electronegativity -as the atoms get larger they become less electronegative -this is because the electrons are further away from the nucleus and are more shielded.

4

what is the trend in melting/boiling point down the group 2 elements?

-the melting point increases as you down the group -this is because larger atoms have more electrons (higher electron density) -this means that the Van der Waals forces are greater and stronger

5

the lower the boiling point the more ________ the element.

the lower the boiling point the more volatile the element

6

what is the trend in oxidising ability down the group 2 elements?

-the elements become less oxidising down the group -this is because as you go down the group the elements become less reactive -this is because the atoms get larger as you go down the group meaning that the outer shell is further away from the nucleus -so electrons are less strongly attracted to it

7

when will a halogen displace a halide iron?

if the halide is below it in the periodic table -so if the halogen is more reactive than the halide

8

when an atom gains an element to become a negative ion what do you call it?

-the element is an oxidising agent -this is because it oxidises the other elements (causes other elements to lose an electron) -and it self is reduced because it has gained an electron (RIG- reduction is the gain of electrons)

9

what is the original colour of chlorine?

very pale green

10

what is the original colour of Bromine?

orange/brown solution

11

what is the original colour of Iodine?

brown

12

give the ionic equation for when Bromine reacts with Potassium iodide and state what you would see.

2KI + Br2 ---> 2KBr + I2 -a brown solution is formed (I2)

13

what halide ion does Fluorine displace?

-Chloride -Bromide - -Iodide

14

what halide ion does Chlorine displace?

-bromide -iodide

15

what halide ion does Bromine displace?

-Iodide

16

what halide ion does Iodine displace?

-non

17

give the ionic equation for when Chlorine reacts with Potassium bromide and state what you would see.

-2KBr + Cl2 ---> 2KCl + Br2 an orange solution is formed (Br2)

18

give the ionic equation for when Chlorine reacts with Potassium iodide and state what you would see.

-2KI + Cl2 ---> 2KCl + I2 -a brown solution is formed(I2)

19

When potassium iodide and Potassium bromide are formed they both produce brown solutions. how can you tell the distinguish between the two solutions?

- you add an organic solvent (Hydrogen peroxide H2O2)

-Bromine produces a brown solution

-iodine produces a violet solution

20

what is the trend in the reducing power of halide ions? state why  

-the reducing power of halide ionsm increases down the group

-this is because the reducing power of the halogen depends on how well it can lose an electron on its outer shell

-as you go down the group the atoms increase in size which means that the outer electron that needs to be lost is further away from the nucleus

-the outer electron is shielded from the attraction of the nucleus

-This means that the electron is easier to remove

 

21

what is the relationhsip between reducing power and reactivity?

the greater the reducing power, the greater the reactivity and the faster the reduction takes place

22

out of the halogens, which ones reduces Sulphuric acid?

Bromine and Iodine

23

when reacting halides with concentrated sulphuric acid what state is the halide compound always in?

SOLID

(*so if you see a question like: what is the test for solid NaF then its using hydrochloric acid!!)

24

How would you test for solid NaF? (create a eqaution)

state what the observations in the reaction would be

state whether it is a redox reaction

state what the H2SO4 acts as in this reaction

-you would add sulfuric acid e.g

-NaF(s) + H2SO4(aq) --> HF(g) + NaHSO4(s)

-you would see misty white fumes produced by the Hydrogen Fluoride

-It is not a redox reaction

-The H2SO4 acts as an acid in this reaction.

25

How would you test for solid NaCl? (create a eqaution)

state what the observations in the reaction would be

state whether it is a redox reaction

state what the H2SO4 acts as in this reaction

-you would add sulfuric acid e.g

-NaCl(s) + H2SO4(aq) --> HCl(g) + NaHSO4(s)

-you would see misty white fumes produced by the Hydrogen Chloride

-It is not a redox reaction

-The H2SO4 acts as an acid in this reaction.

26

How would you test for solid NaBr? (create a eqaution)

and what other reactions could take place?

state what the observations in each reaction would be

state whether they are redox reaction

state what the H2SO4 acts as in the reactions

-you would add sulfuric acid e.g

-NaBr(s) + H2SO4(aq) --> HBr(g) + NaHSO4(s)

-you would see misty white fumes produced by the Hydrogen Bromide

-It is not a redox reaction

-The H2SO4 acts as an acid in this reaction.

 

-There could be another reaction:

2HBr(g) + H2SO4(aq) --> SO2 + Br2 + 2H2O

(in this reaction you produce ROW= R: reduction product, O: oxidation product (always the halOgen), W: water)

-for this second reaction you would observe, choking gas (SO2)and orange/brown vapour (Br2)

the second reaction is a redox

27

Hydrogen Bromide reacts with sulphuric acid

-give the full balanced eqaution for the reaction and state what you would observe

2HBr(g) + H2SO4(aq) --> SO2(g) + Br2(g) + 2H2O(l)

(in this reaction you produce ROW= R: reduction product, O: oxidation product (always the halOgen), W: water)

-in this reaction you would observe, choking gas (SO2)and orange/brown vapour (Br2)

this is a redx reaction

28

How would you test for solid NaI? (create a eqaution)

and what other reactions could take place?

state what the observations in each reaction would be

state whether they are redox reaction

state what the H2SO4 acts as in the reactions

-you would add sulfuric acid e.g

-NaI(s) + H2SO4(aq) --> HI(g) + NaHSO4(s)

-you would see misty white fumes produced by the Hydrogen Iodide

-It is not a redox reaction

-The H2SO4 acts as an acid in this reaction.

 

-There could be another reaction:

2HI(g) + H2SO4(aq) --> SO2 + I2 + 2H2O

(in this reaction you produce ROW= R: reduction product, O: oxidation product (always the halOgen), W: water)

-for this second reaction you would observe, choking gas (SO2)and purple gas/black solid (I2)

the second reaction is a redox

 

-there could be another reaction:

6HI + H2SO4 --> S+ 3I2 + 4H2O

you would observe a yellow solid (S), a purple gas/black solid (I2)

this is a redox reactoon

 

-there could be another reaction:

8HI + H2SO4 --> H2S+ 4I2 + 4H2O

you would observe bad egg smell (H2S) and a purple gas/black solid (I2)

 

29

Hydrogen iodide reacts with sulphuric acid to form SO2

-give the full balanced eqaution for the reaction and state what you would observe

2HI(g) + H2SO4(aq) --> SO2 + I2 + 2H2O

(in this reaction you produce ROW= R: reduction product, O: oxidation product (always the halOgen), W: water)

-for this second reaction you would observe, choking gas (SO2)and purple gas/black solid (I2)

this reaction is a redox

30

Hydrogen iodide reacts with sulphuric acid to form Sulphur

-give the full balanced eqaution for the reaction and state what you would observe

6HI + H2SO4 --> S + 3I2 + 4H2O

you would observe a yellow solid (S) and a purple gas/black solid (I2)

this is a redox reactoon