Topic 1.1 Atomic structure and the periodic table

Question 1

Molecular ion peak

Answer 1

-The peak furthers to the right
-It is the peak with the highest mass to charge ratio (m/z)
-Whole mass of the compound before its broken down

Question 2

Base peak

Answer 2

-The base peak is always the tallest peak in the spectrum
-It represents the most common and most abundant ion

Question 3

Mass number

Answer 3

Sum of protons and neutrons of a particular isotope
(in the nucleus of an atom).

Question 4

First ionisation energy

Answer 4

-The first ionisation energy is the energy required to remove the first (one) electron from each atom in one mole of atoms in the gaseous state.
log10=x ionisations energy
Inverse: 10^x=IE

Question 5

Electron configuration of copper

Answer 5

1s2 2s2 2p6 3s2 3p6 4s1 3d10
Unstable (without a full 3d orbital)
1e- moves from 4s to 3d so there’s a full orbital in 3d and 4s which is more stable than full 4s, not full 3d.

Question 6

Electron configuration of cr

Answer 6

1s2 2s2 2p6 3s2 3p6 4s1 3d5
Unstable (without a half full 3d orbital)
1e- moves from 4s to 3d so there’s a half full orbital in 3d and 4s which is more stable than full 4s, not full 3d.

Question 7

Second ionisation energy

Answer 7

The energy required to remove an electron from each singly charged positive ion in one mole of positive ions in the gaseous state.

Question 8

Relative atomic mass (Ar)

Answer 8

The weighted mean (average) mass of an atom of an element compared to 1/12 of the mass of an atom of carbon-12.

Question 9

Three factors that determine the magnitude of the first ionisation energy

Answer 9

-The orbital in which the electron exists
-The nuclear change of the atom
-The shielding experienced by the electron from all other electrons present

Question 10

Sub-shell electrons

Answer 10

Sub-shells: Number of electrons:
s sub-shell 2 (1x2)
p sub-shell 6 (3x2)
d sub-shell 10 (5x2)
f sub-shell 14 (7x2)

Question 11

Electron configuration order

Answer 11

1s 2s 2p 3s 3p 4s 3d (4s is filled before 3d)
4s is less compact than 3d so e- fill it first as there is more space: e- repel each other so more space means less repulsion.

Question 12

Relative isotopic mass

Answer 12

The mass of an individual atom of a particular isotope relative to 1/12 of the mass of carbon-12.

Question 13

Quantum shell electrons

Answer 13

1st quantum shell: 2 (no. of electrons)
2nd quantum shell: 8
3rd quantum shell: 18
4th quantum shell: 32

Question 14

First ionisation equation

Answer 14

Na(g) —> Na+(g) + e-

Question 15

Second ionisation equation

Answer 15

Na+(g) —>Na^2+(g) + e-

Question 16

Mass spec

Answer 16

-Analytical technique used to determine the molecular mass of a compound (indirectly proved the existence of isotopes)
-Only a small sample is required
-Pattern of deflection according to charge and mass is depicted on a spectrum
-Ions with a large mass to charge ratio are deflected less than ions with a smaller mass to charge ratio.

Question 17

RAM calculations

Answer 17

Easy:
1. Work out difference in mass between isotopes
2. Work out difference between each isotope mass and RAM
3. Divide answers to 2. by 2
4. Multiply by 100

Question 18

An orbital

Answer 18

An orbital is a region within an atom the can hold up two electrons with opposite spins- in any orbital can fit 2 electrons which fit into sub shells
s orbital- sphere shaped
p orbital- dumbbell shaped