1. atomic structure (as)

Question 1

give all the charges of the subatomic structures in an atom

Answer 1

positive proton
negative electron
neutral neutron

Question 2

reactive charges + relative masses of subatomic particles

Answer 2

proton- charge- +1- mass 1
neutron- charge- 0- mass 1
electron- charge-(-1)- mass 1/1836

Question 3

atomic number and mass number + symbols

Answer 3

atomic- number of protons symbol Z

mass- nucleon number- proton and neutron number- symbol A

Question 4

how are ions formed

Answer 4

when an atom gains or loses an electron causing them to be charged

Question 5

physical and chemical properties of isotopes + why

Answer 5

chemical:
. same chemical characteristics- same no of e in outer shell- e take place in chemical reactions ,, determine chem of atom

physical:
.diff neutrons ,, only add mass
. diff densities
. diff mp / bp

Question 6

calculate mass no + proton no

Answer 6

mass no= no of protons + no of neutrons

no of protons= mass no - no of neutrons

Question 7

isotopes definition

Answer 7

atoms of the same element that contain the same number of protons and electrons but different number of neutrons

Question 8

relative isotopic mass def

Answer 8

the mass of an isotope relative to 1/12 of a c-12 atom

Question 9

relative atomic mass def

Answer 9

the average mass of an atom relative to 1/12 of the mass of a carbon-12 atom

Question 10

what are protons + neutrons called

Answer 10

nucleons

Question 11

relative formula mass MR how is it calculated

Answer 11

(total mass of a substance)

add up the relative atomic masses of all atoms present in formula

ex.H2 2x1=2

Question 12

Relative atomic mass formula

Answer 12

AR= (relative abundance1 x mass isotope1) + ( relative abundance2 x mass isotope2) /100

Question 13

what happens when a compound is analysed in a mass spectrometer

Answer 13

vaporised molecules are bombarded with a beam of high speed electrons
they knock off an electron from some molecules causing molecular ions

Question 14

ionisation energy def

Answer 14

the amount of emery required to remove one mole of electrons from each mole of gaseous atoms of an element to form a mole of gaseous ions

Question 15

ionisation energies measured under standard conditions + units of IE

Answer 15

. 298k
. 101kPa

units kilojoules per mol (kJ/mol)

Question 16

second ionisation energy def

Answer 16

energy required to remove one mole of electrons from one mole of gaseous +1 ion to form one mole of gaseous 2+ ions

Question 17

draw first IE and second IE of x

Answer 17

x —> x+ (g) + e-

x+ —-> x2+ (g) + e-

Question 18

why does successive IE of an element increase

Answer 18

because once you remove outer electron from an atoms you form a positive ion

removing an electron from a positive ion is more difficult than a neutral atom

more electrons removed attractive forces increase due to decreased shielding and more protons than electrons

Question 19

side of first IE is affected by

Answer 19

• size of nuclear charge
• distance of outer electrons from nucleus
• shielding effect of inner electrons
• spin pair repulsion

Question 20

IE across a period

Answer 20

generally increases due to :

. nuclear charge increases across period
. causing atomic radius to decrease as outer shell pulled close to nucleus ,, decreases distance between nucleus and outer e
. shielding by inner electrons remains constant as e enter same shell
. becomes harder to remove across period
. more energy required some IE increases

Question 21

dips in trend for IE across period

Answer 21

beryllium and boron because boron 2p sub shell further away from nucleus

nitrogen and oxygen because oxygen has more spin pair repulsion in 2p orbital

Question 22

what happens to IE between last element in period and first element in next period

Answer 22

decrease in IE because

. increased distance between nucleus and outer e bcs in new shell
. increased shielding in inner e because of new shell
. these factors outweigh nuclear charge increases across

Question 23

IE down a group

Answer 23

decreases because:

. no of protons increases ,, nuclear charge increases
. atomic radius increases
. distance between nucleus and outer electron increases
. shielding by inner shell electrons increases
. factors outweigh nuclear charge ,, easier to remove the outer electron
IE decreases

Question 24

what do electrons do around the nucleus in energy shells

Answer 24

move rapidly
if energy increases they can jump to a higher energy level
process is reversible ,, can return to their original energy level when they emit energy

frequency or energy is exactly the same when being emitted or absorbed

Question 25

what happens when the energy electrons emit is mixture of different frequencies

Answer 25

thought that many electrons jump between energy levels and the emitted energy is visible and can be analysed by passing rethought a diffraction grating and results to line emission spectrum

Question 26

explain line emission spectra

Answer 26

each line is a specific energy value packets of energy called quanta in the blue end lines get closer together -convergence lines converging towards the higher end electrons reaching for max amount of energy

Question 27

successive IE first e to fourth removed

Answer 27

first- removed has low IE due to spin pair repulsion of e second- more difficult because there is no spin pair repulsion third-much more difficult bcs closer to nucleus fourth- most difficult bcs no longer full orbital + less spin pair repulsion

Question 28

what does the jumps on the successive IE graphs show

Answer 28

change of shell small jumps are change in sub shell

Question 29

electron configuration def

Answer 29

the arrangement of electrons in an atom

Question 30

principle quantum shells

Answer 30

used to number the energy levels the lower the principle quantum number the closer the shell is to the nucleus where electrons are arranged around nucleus

Question 31

the higher the principle quantum number what does it do to energy of shell and distance from nucleus

Answer 31

the greater the energy of shell the further away from the nucleus

Question 32

formula to calculate how much each principle quantum number can hold electron

Answer 32

2n^2

Question 33

orbitals can exist at

Answer 33

specific energy levels and electrons can be only found at these specific levels

Question 34

how many orbitals in each sub shell

Answer 34

s: one orbital p: three orbitals d: five orbitals f: seven orbitals

Question 35

types of sub shells

Answer 35

s p d f

Question 36

s orbital shape + size

Answer 36

spherical shape size of s orbital increases with increasing shell number

Question 37

p orbital shape

Answer 37

dumbbell

Question 38

hunds rule

Answer 38

electrons will occupy separate orbitals in same sub shell to minimise repulsion and have spin in same direction then start to pair up in opposite direction

Question 39

pauli exclusion principle

Answer 39

orbital can only hold two electrons and they must have opposite spins

Question 40

sub shell energy order + exception

Answer 40

s

Question 41

when something is said to be degenerate it means

Answer 41

all the orbitals in the same sub shell have the same energy

Question 42

chromium configuration + copper configuration

Answer 42

Cr= 1s2 2s2 2p6 3s2 3p6 3d5 4s1 cu= 1s2 2s2 2p6 3s2 3p6 3d10 4s1

Question 43

where in periodic table would s p d f block

Answer 43

s- g1/2 d- metal p- g7/8 f- below periodic table

Question 44

melting point trend of period 3 (2 is the same)

Answer 44

increases up until silicon silicon is highest mp after silicon mp decreases significantly

Question 45

bonding in period 3 elements

Answer 45

Na-Al: metallic Si- cl: covalent

Question 46

structure of elements in period 3

Answer 46

Na to Al: giant metallic Si: giant molecular P to Ar: simple molecular

Question 47

metallic elements formed

Answer 47

positive ions arranged in a giant lattice in which ions are held together by a sea of delocalised electrons

Question 48

meltallic bonding explained in Na- Mg- Al

Answer 48

Na donates one electron Mg donates two electrons Al donates three electrons ,, Al electrostatic forces between 3+ion and negatively charged electron

Question 49

Si why does it have highest mp

Answer 49

giant molecular structure which Si atom is held together to neighbouring atoms by strong covalent bonds

Question 50

mp between P, S , Cl , Ar

Answer 50

simple molecules covalent bonds within molecules are sting but between molecules only weak instantaneous dipole-dipole forces ,, doesn’t take much energy to break intermolecular forces

Question 51

atomic radius

Answer 51

distance between nucleus and outermost electron or an atom

Question 52

atomic radius name in metals and nonnmetals

Answer 52

metals- metallic radius non metals- covalent radius

Question 53

across period what happens to atomic radii + why

Answer 53

radii decreases bcs no of protons and electrons increases (nuclear charge) shielding remains the same nucleus attracts electrons more strongly ,, pulls them closer to nucleus ,, atomic radius decreases

Question 54

ionisation energy across period 2/3

Answer 54

IE increases due to . nuclear charge increases . atomic radius decreases . shielding by inner shells electrons remains same . harder to remove an electron . more energy needed

Question 55

dips in the trend for period 3 IE energy trends across period

Answer 55

Mg and Al slight decrease bcs sulfur has spin pair repulsion in 3p orbital which makes its easier to remove electrons

Question 56

relative molecular mass def

Answer 56

average mass of a molecule or formula unit compared to 1/12th of the mass of an atoms of c-12

Question 57

what’s used for relative molecular mass, relative formula mass, relative atomic mass

Answer 57

. simple molecules . compounds . ions and atoms