Topic 1

Question 1

sub-shell: s
number of orbitals?
max. number of electrons?

Answer 1

number of orbitals: 1

max. number of electrons: 2

Question 2

sub-shell: p
number of orbitals?
max. number of electrons?

Answer 2

number of orbitals: 3

max. number of electrons: 6

Question 3

sub-shell: d
number of orbitals?
max. number of electrons?

Answer 3

number of orbitals: 5

max. number of electrons: 10

Question 4

sub-shell: f
number of orbitals?
max. number of electrons?

Answer 4

number of orbitals: 7

max. number of electrons: 14

Question 5

electrons spin in orbitals

Answer 5

the electrons in an orbital have opposite spins

Question 6

sub-shell 3d vs 4s

Answer 6

3d is higher in energy than 4s

Question 7

what is an orbital?

Answer 7

a region around the nucleus where there is a high probability of finding an electron

Question 8

how many electrons can an orbital hold?

Answer 8

2

Question 9

Hund’s rule

Answer 9

electrons occupy orbitals singly before pairing occurs

Question 10

Pauli exclusion principle

Answer 10

electrons in the same orbital must have opposite spins

Question 11

what are s-block elements?

Answer 11

elements that have their last added electron in the s-orbital
(group 1 & 2)

Question 12

what are p-block elements?

Answer 12

elements that have their last added electron in a p-orbital

group 3, 4, 5, 6, 7, 8

Question 13

what are d-block elements?

Answer 13

elements that have their last added electron in a d-orbital

transition metals

Question 14

order that electrons fill orbitals

what comes before and after 1s?

Answer 14

before: nothing
after: 2s

Question 15

order that electrons fill orbitals

what comes before and after 2s?

Answer 15

before: 1s
after: 2p

Question 16

order that electrons fill orbitals

what comes before and after 2p?

Answer 16

before: 2s
after: 3s

Question 17

order that electrons fill orbitals

what comes before and after 3s?

Answer 17

before: 2p
after: 3p

Question 18

order that electrons fill orbitals

what comes before and after 3p?

Answer 18

before: 3s
after: 4s

Question 19

order that electrons fill orbitals

what comes before and after 4s?

Answer 19

before: 3p
after: 3d

Question 20

order that electrons fill orbitals

what comes before and after 3d?

Answer 20

before: 4s
after: 4p

Question 21

order that electrons fill orbitals

what comes before and after 4p?

Answer 21

before: 3d
after: 5s

Question 22

order that electrons fill orbitals

what comes before and after 5s?

Answer 22

before: 4p
after: 6s

Question 23

order that electrons fill orbitals

what comes before and after 6s?

Answer 23

before: 5s
after: 4f

Question 24

order that electrons fill orbitals

what comes before and after 4f?

Answer 24

before: 6s
after: 5d

Question 25

order that electrons fill orbitals | what comes before and after 5d?

Answer 25

before: 4f after: 6p

Question 26

what does the value of the first ionisation energy depend upon?

Answer 26

- the effective nuclear charge - the distance between the electron and the nucleus - the shielding produced by lower energy levels

Question 27

what is ionic bonding?

Answer 27

- the transfer of electrons from metal atoms to non-metal atoms to form charged ions - the resulting product is held together by electrostatic attractions

Question 28

what is covalent bonding?

Answer 28

- when atoms share one or more electrons to form a molecule | - a single covalent bond is shared with each atom donating one electron

Question 29

what is co-ordinate / dative covalent bonding?

Answer 29

in a normal covalent bond, each atom donates one electron to the shared pair; in a dative covalent bond, electrons come from the same element

Question 30

what is the shape of a molecule decided by?

Answer 30

the valence shell electron pair repulsion theory

Question 31

what is the valence shell electron pair repulsion theory?

Answer 31

molecules arrange their electron pairs to minimise repulsions between them

Question 32

what do distorted shape molecules arise from?

Answer 32

the presence of lone pairs of electrons that cause greater repulsion than bonding pairs

Question 33

what is relative atomic mass (RAM)?

Answer 33

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

Question 34

what is relative isotopic mass (RIM)?

Answer 34

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

Question 35

what is the molecular ion peak (the M peak)?

Answer 35

the peak with the highest m/z ratio in the mass spectrum

Question 36

what does m/z ratio mean?

Answer 36

mass : charge

Question 37

what does a mass spectrometer do?

Answer 37

measures the masses of atoms and molecules

Question 38

how does a mass spectrometer work?

Answer 38

- produces positive ions that are deflected by by a magnetic field according to their m/z ratio - calculates the relative abundance of each positive ion and displays the percentage

Question 39

how do you determine the relative molecular masses of diatomic molecules?

Answer 39

use a mass spectrometer to observe the peaks with the largest m/z ratios (assuming a value of z=1)

Question 40

what do you need to know to determine the relative molecular mass of a polyatomic molecule?

Answer 40

- need to know the exact relative isotopic masses of all atoms present - need to know the relative composition of all the different molecules

Question 41

quantum shell

Answer 41

defines the energy level of an electron

Question 42

what does electron configuration do?

Answer 42

shows the number of electrons in each sub-level in each energy level of the atom

Question 43

what is first ionisation energy?

Answer 43

the energy required to remove an electron from each atom in one mole of atoms in the gaseous state

Question 44

what is second ionisation energy?

Answer 44

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

Question 45

what are the factors that affect the energy an electron has?

Answer 45

- the orbital in which the electron exists - the nuclear charge of the atom (no. of protons) - the repulsion (shielding) experienced by the electron from the other electrons present

Question 46

what are the 2 major trends in ionisation energies in the Periodic table?

Answer 46

- increases across a period | - increases down a group

Question 47

what is the trend in ionisation across a period?

Answer 47

Looking at Period 2: - nuclear charge increases (on its own this would lead to an increased attraction between the nucleus and the electron, ∴ a decrease in the energy of the outermost electron, and an increase in first ionisation energy) - one more electron is added to the same quantum shell on each occasion, and this increases the electron-electron repulsion within the quantum shell (on its won this would cause an increase in energy of the outermost electron and would lead to a decrease in first ionisation energy) - increase in nuclear charge is more significant than the increase in electron-electron repulsion. So there is a general increase in first ionisation energies across Period 2.