Periodicity

Question 1

Classical structure of electrons

Answer 1

It is a particle

Question 2

quantum mechanics

Answer 2

is used to describe small particles such as electrons which have a wave-particle duality.

Question 3

atoms and electrons are described as both

Answer 3

particle and waves

Question 4

E

Answer 4

= hv

Question 5

v

Answer 5

c / wavelength

Question 6

quanta

Answer 6

a packet of energy or matter

Question 7

electrons have

Answer 7

certain allowed energies

Question 8

quantum number

Answer 8

label for allowed energy

Question 9

where do the quantum numbers come from

Answer 9

Schrodinger equation

Question 10

principal quantum number

Answer 10

describes the distance away from the nucleus and size of orbital

Question 11

Azimuthal quantum number

Answer 11

the shape of the orbital and the angular momentum

Question 12

magnetic quantum number

Answer 12

the orientation of the orbital

Question 13

spin quantum number

Answer 13

the intrinsic angular momentum of an electron

Question 14

Each orbital defined by an allowed value of
.

Answer 14

n, l and ml

Question 15

what defines an allowed energy of an electron in an atom .

Answer 15

the first three quantum numbers

Question 16

Hunds rule

Answer 16

this describes that in degenerate orbitals, electrons enter in seperate orbital before they start to fill in orbital with a second electron

Question 17

pauli exclusion rule

Answer 17

electrons can have no more than 3 quantum numbers the same. it cannot have 4 quantum numbers the same

Question 18

aufbau principle

Answer 18

electrons fill in by the lowest energy energy orbital first available. this is an exception with hydrogen

Question 19

sp

Answer 19

two sp orbital. two p orbitals

Question 20

sp2

Answer 20

three sp orbitals. one p orbital

Question 21

sp3

Answer 21

4 sp4 orbitals

Question 22

valence electrons feel less of the

Answer 22

positive nucleur charge

Question 23

why do valence electrons feel less charge?

Answer 23

the core electrons cancel out some of the positive nuclear charge and shields the valence electrons

Question 24

what is the effective nuclear charge?

Answer 24

it is the charge that the valenve electrons feel, this is calculated by subtracting the nuclear charge against the shielding constant

Question 25

the effective nuclear charge

Answer 25

increases along period

Question 26

the effective nuclear charge increases

Answer 26

down a group

Question 27

ionisation energy

Answer 27

the is the energy it takes for isolated atoms the ground electrontric atate in the gaseous state to form 1+ gaseous ions

Question 28

the ionisation energy increases

Answer 28

along the row. This is because the eefective nuclear charge increases and the atomic radii decreases

Question 29

the ionisation energy in a group

Answer 29

decreases. although the atomic effective nuclear chrage increases the distance from the nucleus increases and the valence electrons are in a higher quantum shell

Question 30

in a new row the ionisation energy

Answer 30

decreases. the valence electrons are in a higher quantum shell

Question 31

what will cause a decrease

Answer 31

sharing orbital. Hunds rule. there will be a force of replusion

Question 32

orbital types

Answer 32

going from s to p will cause a fall in ionisation energy

Question 33

electronegativity

Answer 33

the ability for an atom to draw electron density towards itself within it being in a molecule

Question 34

what are the general values for electronegativity?

Answer 34

betweenj 1-4

Question 35

electronegativity

Answer 35

increases along the row but decreases down a group

Question 36

electronegativity shows

Answer 36

if the bond will be ionic or covalent. the greater the difference in electrongetivity, the more likely it will be ionic bonding vice versa ,

Question 37

what do atoms try and achieve by bonding

Answer 37

noble gas configuration

Question 38

ionic bonding

Answer 38

electrons are formally transferred from one atom and the ions are held together by electrostatic interactions

Question 39

covalent bonding

Answer 39

atoms share electrons

Question 40

metallic bonding

Answer 40

sharing of free electrons among a structure of positively
charged ions (cations).

Question 41

ionic bonding charcteristics

Answer 41

no directional restrictions
infinite 3D arrays
favors polaar subctances
high energy to break up interactions. so it has a high boiling and melting point

Question 42

Ga

Answer 42

consists of covalently-bound pairs of atoms in both liquid
and solid state - these atomic pairs form with metallic
bonding between them.

Question 43

covalent characteristics

Answer 43

directional. orbitals point at specific directions
forms both infinite and discrete arrays
prefers non polar substances

Question 44

polarisability,

Answer 44

how easily an electron cloud is distorted by an
electric field

Question 45

what impacts polarisability

Answer 45

charge and size of ion s

Question 46

Size of the ion:

Answer 46

Smaller cation, and larger anion, give greater
covalent character.

Question 47

The charge of cation:

Answer 47

Greater the charge of cation, greater is
the covalent character of the bond.

Question 48

• Dative Bonding -

Answer 48

both electrons in a bond come from
one atom

Question 49

Multicentre Bonding

Answer 49

• a pair of electrons is involved in
  bonding between 3 or more atoms

Question 50

Hydrogen Bonding

Answer 50

• polar molecules experience
  attractive permanent dipole-dipole forces

Question 51

Pi-stacking

Answer 51

• Attractive, non-covalent interactions
  between aromatic rings

Question 52

• Dispersive forces -

Answer 52

forces arising
from the interactions of instantaneous multipoles