Group 17

Question 1

halogens

Answer 1

fluorine, chlorine, bromine, iodine

Question 2

fluorine state under room conditions

Answer 2

gas

Question 3

chlorine state under room conditions

Answer 3

gas

Question 4

bromine state under room conditions

Answer 4

liquid

Question 5

iodine state under room condition

Answer 5

solid

Question 6

fluorine color

Answer 6

pale yellow

Question 7

chlorine color

Answer 7

yellowish - green

Question 8

bromine color

Answer 8

orange / brown

Question 9

iodine color

Answer 9

grey/ black/ purple vapour

Question 10

increase in Vander force

Answer 10

decreases volatality

Question 11

order of vander vaals force

Answer 11

Question 12

graph of MP of group 17 elements

Answer 12

Question 13

bond energy

Answer 13

energy required to break a particular covalent bond in one mole of molecule in a gaseous state

Question 14

bond enthalpy decreases

Answer 14

down the group because the distance between the nucleus and the bonding electron pair increases, the bonding electrons will be less attracted an need less energy to break the bond

Question 15

the bond enthalpy of flourine is exceptionally low because

Answer 15

F2 is a small molecule with six lone pairs of electrons. the repulsion created between the electrons reduces the energy required to break the covalent bond

Question 16

what decreases down the group

Answer 16

atomic radius, reducing power , MP and BP

Question 17

what increases down the group

Answer 17

reactivity, electronegativity and oxidising power

Question 18

oxidising power - OA

Answer 18

the ability to accept electrons - substances that undergoes reduction

Question 19

oxidising power decreases down the group

Answer 19

as size of the atom increases and shielding effect increases

Question 20

Answer 20

increase in oxidising power