1.the atom and redox

Question 1

define isotopes.

Answer 1

Atoms of the same element (same number protons ) but with a different number of neutrons and different masses.

Question 2

Define relative atomic mass

Answer 2

The WEIGHTED MEAN mass of ONE atom of an element compared with 1/12 the mass of an atom of carbon 12

Question 3

Define relative isotopic mass

Answer 3

The mass of ONE atom of a specific ISOTOPE compared with 1/12 the mass of an atom of carbon 12

Question 4

define 1st ionization energy

Answer 4

The energy required to remove ONE electron from each atom in ONE MOLE in the GASEOUS state, to form 1 move of gaseous 1+ ions.

Question 5

Give a formula for the 2nd ionization energy of oxygen

Answer 5

O+(g) —> O2+(g) +e-

Question 6

Define orbital

Answer 6

a region of space containing up to 2 e- (of opposite spin and of the same energy level)

Question 7

WHat do we assume to use oxidation numbers?

Answer 7

Everything is ionically bonded, with top right being negative.

Question 8

Three rules for determining oxidation number

Answer 8

1.A element in its normal state has O.N 0
2.Group 1 elements are +1
Group 2 elements are +2
Group 7 is usually -1
Oxygen is ‘always’ -2
Hydrogen is ‘always’ +1
3.All other are calculated from this with +7 being the highest.

Question 9

Oxidation is ……

Reduction is …..

Answer 9

….Losing electrons

…Gaining electrons

Question 10

Define oxidizing agent

Answer 10

An oxidizing agent causes a different species to be oxidized
Common O.A , O2 , acidified manganate, acidified dicromate, H2O2
In the reaction the O.A gets reduced.

Question 11

what is a redox reaction

Answer 11

one where both oxidation and reduction happen

Question 12

define disproportionation

Answer 12

The oxidation and reduction of the same element in a redox reaction.

Question 13

£ factors effecting ionisation values and their effect

Answer 13

1. Atomic radius - bigger=less IE
2. No. shielding e- - More=less IE
3. Nuclear charge- More=more IE

Question 14

1st IE trend across a period

Answer 14

IE increases generally over a period.
more nuclear change -increases IE
Shielding e- says the same
Atomic radius gets slightly smaller- slightlyhigher IE

Question 15

1st IE trend down a group

Answer 15

IE decreases down the group
more nuclear change -increases IE
more Shielding e- less IE (cancels out N.C)
Atomic radius increases- lower IE

Question 16

Why is LogIE plotted?

Answer 16

because the range of numbers being plotted is fucking huge, and loging it making it easier to compare by making all the numbers smaller while still keeping their order.

Question 17

What do you need to label in a orbital diagram?

Answer 17

the 90% boundary
the +
or axis if its a p orbital

Question 18

Shapes of p and s orbital

Answer 18

S- spherical

P-Dumb-bell

Question 19

Why are their two deviations in 1st IE across a group?

Answer 19

Due to subshells.
Eg period 2. Li,BE,B,C,N,O,F,Ne
Boron - has 4 shielding e- because it includes the 2s orbital which lowers the IE.
Oxygen-The repulsion of the paired e-s in the p orbital causes it to require less energy.

Question 20

The first row of the D-block is…

Answer 20

3d

Question 21

Why are Cr and Cu odd?

Answer 21

Cr has 5 e- in 3d and 1 in 4s due to a pair of e- causing 4s to have a higher energy level then 3d so one e- moves to 3d
Cu- 10 e- in 3d and 1 in 4s for the same reason

Question 22

what happens (e- wise) when d block elements react?

Answer 22

always lose e- to become a cation

4s orbital always loses e- first.