1- Atomic Structure and the Periodic Table

Question 1

Who discovered the electron

Answer 1

J.J Thomson 1897

Question 2

Who discovered the proton

Answer 2

Ernest Rutherford 1917

Question 3

Who discovered the neutron

Answer 3

James Chadwick 1932

Question 4

Proton charge, mass and position

Answer 4

mass: 1
charge: +1
position: nucleus

Question 5

Neutron charge, mass and position

Answer 5

mass: 1
charge: 0
position: nucleus

Question 6

Electron charge, mass and position

Answer 6

mass: 1/1840
charge: -1
position: energy levels surrounding nucleus

Question 7

Mass number

Answer 7

number of protons + number of neutrons

Question 8

Atomic number

Answer 8

number of protons (=number of electrons)

Question 9

Isotopes

Answer 9

atoms of the same element with different number of neutrons resulting in different mass numbers

Question 10

Relative atomic mass

Answer 10

the weighted mean mass of an atom of an element compared to 1/12 of the mass of carbon-12

Question 11

Relative isotopic mass

Answer 11

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

Question 12

Mass spectrometer

Answer 12

measures the masses of atoms and molecules

Question 13

Process of mass spectrometry

Answer 13

1) vaporisation
2) ionisation
3) acceleration
4) deflection
5) detection

Question 14

Describe step 1 of mass spectrometry

Answer 14

vaporisation turns the element into a gas so they can be ionised

Question 15

Describe step 2 of mass spectrometry

Answer 15

ionisation bombards the atoms with electrons knocking some of their electrons off turning them into positive ions

Question 16

Describe step 3 of mass spectrometry

Answer 16

acceleration positive ions are attracted to negative charged plates

Question 17

Describe step 4 of mass spectrometry

Answer 17

deflection happens by a magnetic field which depends on ratio of ion’s mass:charge

Question 18

Describe step 5 of mass spectrometry

Answer 18

Detection current is generated proportional to the abundance of each ion

Question 19

Mr of diatomic molecules on mass spectrometry graph

Answer 19

peaks are caused by single ions and larger peaks are caused by diatomic ions where two of the isotopes are bonded together
multiple peaks are caused from different ions joining together

Question 20

Molecular ion peak

Answer 20

the M peak
last peak indicates the Mr
M+1 peak small peak after last peak showing presence of isotopes

Question 21

Quantum shells

Answer 21

the energy levels of an atom

Question 22

Orbtials

Answer 22

each sub-shell contains orbitals
a region within an atom that can hold up to two electrons with opposite spins

Question 23

S orbital

Answer 23

a spherical shape

Question 24

P orbitals

Answer 24

a dumbbell/hourglass shape
three orientations
holds up to 6 electrons

Question 25

First quantum level

Answer 25

one sub-shell 1s holds up to two electrons

Question 26

Second quantum level

Answer 26

two sub-shells 2s and 2p holds up to eight electrons

Question 27

Third quantum level

Answer 27

three sub-shells 3s, 3p and 3d holds up to 18 electrons

Question 28

Fourth quantum level

Answer 28

four sub-shells 4s, 4p, 4d and 4f holds up to 32 electrons

Question 29

Why 4s fills before 3d

Answer 29

4s is a lower energy level than 3d

Question 30

Hund's rule

Answer 30

electrons will occupy orbitals singly before pairing takes place

Question 31

Pauli exclusion principle

Answer 31

two electrons cannot occupy the same orbital unless they have opposite spins spins shown by upwards or downwards arrows

Question 32

Exclusions to electronic configuration filling order

Answer 32

copper and chromium do not fill their 4s orbital completely before filling 3d as they are more stable this way

Question 33

Isoelectronic

Answer 33

same number of electrons (ions or atoms)

Question 34

First ionisation energy

Answer 34

the energy requires to remove an electron from each atom in one mole of atoms in a gaseous state F(g) -------> F+(g) + e-

Question 35

Second ionisation energy

Answer 35

amount of energy require to remove an electron from 1+ ions in one mole of positive ions in the gaseous state

Question 36

Successive ionisation energy

Answer 36

it is harder to remove more electrons due to increasing magnitude of nuclear charge that is greater than negative electron charge so pull is greater and shielding decreases

Question 37

Why are there ionisation energy jumps

Answer 37

entering a new period requires more energy as it is closer to the nucleus

Question 38

Factors affecting ionisation energy

Answer 38

atomic radius nuclear charge electron shielding

Question 39

Trend in ionisation energy across a period

Answer 39

energy needed increases increased positive charge from more protons

Question 40

Trend in ionisation energy down a group

Answer 40

energy needed decreases more shielding and distance from nucleus

Question 41

What determines chemical properties of an element

Answer 41

electronic configuration

Question 42

Groups

Answer 42

vertical columns

Question 43

Periods

Answer 43

horizontal rows

Question 44

Periodicity

Answer 44

the regular repeating pattern of atomic, physical and chemical properties with increasing atomic number

Question 45

Atomic radi

Answer 45

the distance between the outermost electron of an atom and centre of the nucleus It is hard measured where an electron is so it is measured from the distance between two nuclei and dividing by two

Question 46

Why does first ionisation energy drop between N-->O

Answer 46

nitrogen has no paired electrons but O starts to pair uo so there is electron repulsion