topic 1

Question 1

what is the structure of an atom

Answer 1

nucleus- protons and neutrons
electrons - orbit nucleus

Question 2

what are the relative charges and masses of the sub atomic particles

Answer 2

relative charge
proton - 1
neurton - 0
electron - -1

relative mass
proton - 1
neutrons - 1
electrons - 1/2000

Question 3

wwhat is the mass number and where is it on the periodic table

Answer 3

top number
protons and neutrons

Question 4

what is the atomic number and where is it on the periodic table

Answer 4

bottom number
protons

Question 5

what are ions

Answer 5

have a different number of electrons and protons
negative ions have gained electrons
positive ions have lost electrons

Question 6

what is an isotope

Answer 6

elements with same number of protons but different number of neutrons

Question 7

what is relative atomic mass

Answer 7

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

Question 8

what is relative isotopic mass

Answer 8

the mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon-12

Question 9

what is relative molecular mass

Answer 9

the mean mass of a molecule compared to 1/12th of the mass of an atom of carbon-12

Question 10

how to work out relative atomic mass

Answer 10

total abundance

Question 11

how to calculate isotopic mass

Answer 11

place x in isotopic mass you dont know
(abundance A X m/zA)+(abundance B X m/z B)
———————————
total abundance

Question 12

how to predict mass spectra from % abundance

Answer 12

1. write % as decimals
2. create a table with isotope combinations
   multiply decimal form abundances to get relative abundance from each molecule
3. any molecules which are the same add the aundances
4. divide the relative abundances worked out by the smallest value to give whole number ratio to put on spectra

Question 13

what is M+1 peak

Answer 13

molecular peak ion
same as Mr

Question 14

what are the subshells with number of orbitals and number of electrons

Answer 14

s- 1 orbital 2 electrons
p- 3 orbitals 6 electrons
d- 5 orbitals 10 electrons
f- 7 orbitals 14 electrons

Question 15

what subshells do shells 1 2 and 3 have and how many electrons can they hold

Answer 15

shell 1 - 1s- 2 electrons
shell 2 - 2s 2p- 8 electrons
shell 3 - 3s 3p 3d - 18 electrons

Question 16

what is the shape of a s orbital

Answer 16

spherical

Question 17

what is the shape of a p orbital

Answer 17

dumbells

Question 18

what is spin pairing

Answer 18

when 2 electrons occupy 1 orbital they spin in opposite directions

Question 19

how do electrons fill orbitalsand why

Answer 19

singly first the pair up due to electron repulsion

Question 20

when are subshells most stable

Answer 20

when full or half full

Question 21

where are the s d p and f blocks on the periodic table

Answer 21

s - group 1 and 2
d- transition metals
p - group 5 6 7 and 0
f - under d block

Question 22

what is the electromagnetic spectrum

Answer 22

radiowaves
microwaves
infrared
vissible light
ultra violet
x rays
gamma rays

Question 23

which side of the electromagnectic has the largest energy and frequcency of radiation

Answer 23

gamma rays side

Question 24

what is line spectra evidence for and how

Answer 24

quantum shells
energy levels have discrete values and electrons can move from one shell to another
a line spectra shows the frequency of light given when a electron moves down

Question 25

on line spectra where has the electron dropped to if lines are at ultraviolet

Answer 25

ground state

Question 26

on line spectra where has the electron dropped to if lines are at visible light

Answer 26

n = 2

Question 27

one line spectra where has the electron dropped to if lines are at infrared

Answer 27

n = 3

Question 28

why is emission spectra evidence for quantum shells

Answer 28

they are diffined lines prove electrons exist in shells only and never between them

Question 29

what is ionisation energy

Answer 29

min amount of energy required to remove 1 mole of electrons from 1 mole of atoms in gaseous state

Question 30

what is the equation for the 1st ionisation energy Na

Answer 30

Na (g) --> Na^+ (g) + e^-

Question 31

what affects the 1st ionisation energy

Answer 31

shielding - more shells between positive nucleus and negative electrons means weaker attraction = less energy nuclear charge - more protons in nucleus the greater the attraction between outer electrons = more energy atomic size - bigger the atom the further the outer electrons, attractive force reduces = less energy

Question 32

what happens to ionisation energy down group and why

Answer 32

decreases atomic radius increases sheilding increases

Question 33

what is successive ionisation energy

Answer 33

the removal of more than 1 electrons from the same atom

Question 34

draw a graph a the successive ionisation of Mg and explain

Answer 34

gerneral increase - more positive ion large increase after 1st 2 electrons as removing from a shell closer to nucleus large increase after next 8 as new shell

Question 35

what happens to atomic radii across a period amd why

Answer 35

decreases across increased nuclear charge- more protons pulls outer shell towards nucleus extra electrons go into same shell

Question 36

what is the trend in 1st ionisation energy across a period and why

Answer 36

increases increased nuclear charge similar sheilding

Question 37

draw a graph to show 1st ionisation energy from Na to Ar

Answer 37

see flash card

Question 38

what does the fact the 1st ionisation energy of Al lower than Mg provide evidence for

Answer 38

subshells 3p1 higher enrgy subshell further from nucleus

Question 39

what does the fact that the 1st ionisation energy of S being similar to P provide evidence for

Answer 39

for electron repulsion 3p4

Question 40

draw a graph for the melting points of Na ro Ar

Answer 40

see flash card

Question 41

explain the bp of Na Mg and Al

Answer 41

metalic bonding general increase as metal ions have increasing positive charge and delocalised electrons and have smaller ionic radius

Question 42

explain the mp of Si

Answer 42

giant covalent many covalent bonds

Question 43

explain the mp of P

Answer 43

weaker simple molecular structure weak london forces

Question 44

expkain the mp of S

Answer 44

larger simple molecular structure larger london forces

Question 45

explain the mp of Cl

Answer 45

simple mocleular structure smaller london forces

Question 46

explain the mp of Ar

Answer 46

exists as individual atoms smaller london forces