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A-Level Chemistry > Chapter 1 - Atomic Structure > Flashcards

Chapter 1 - Atomic Structure Flashcards

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1
Q

what is the relative mass and charge on a neutron

A

mass: 1
charge: 0

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2
Q

what is the relative mass and charge of a proton

A

mass: 1
charge: +1

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3
Q

what is the relative mass and charge of an electron

A

mass: 1/1840
charge: -1

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4
Q

define relative atomic mass

A

the average mass of an atom of an element relative to one twelfth of the mass of an atom of carbon-12.

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5
Q

what must initially happen to an atom or molecule before it is put into a mass spectrometer

A

it must be ionised

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6
Q

how can atoms or molecules be ionised

A

using an electron gun
or using electrospray ionisation

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7
Q

describe how the electron gun ionises atoms

A

en electron is shot at an atom in a high vacuum chamber
the electron knocks off an electron off the atom to form a positive ion

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8
Q

how is electrospray ionisation carried out

A

a high voltage is applied to a solution with dissolved biomolecules
the high voltage causes the solvent to become ionised and break into many small droplets which are small enough to be considered a gas

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9
Q

what conditions must be present for electron impact ionisation to be successful

A

there must be a high vacuum in the chamber
the atom must be in a gaseous state

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10
Q

pros of electron impact ionisation

A

it can be done on individual atoms
it is very powerful and effective

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11
Q

cons of electron impact ionisation

A

it’s powerful so it may cause fragmentation in biomolecules which may cause inaccuracy in the mass spectrometer reading

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12
Q

describe the method of mass spectroscopy

A

sample introduced at low pressure
electron gun or electrospray used to ionise sample
the sample becomes a positive ion
the ions are accelerated with a negatively charged plate, then focused into a beam using a magnetic field
the ions are deflected, the deflection depends on the mass to charge ratio of each ion
lightest ions are deflected the most
ions reach the detector where they gain an electron and produce a current which is detected
the size of the current is proportional to the abundance of each isotope
a mass spectrum can be produced which cab be used to calculate the Ar of the sample

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13
Q

what does m/z mean

A

mass to charge ratio

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14
Q

if two molecules of different mass are in one spectroscope, what about them is the same

A

the energy they are accelerated to is the same
the distance they travel is the same
the time taken to travel the distance is different
the mass is different (it is usually what you are finding)

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15
Q

what equation can be used to find the velocity of a particle in a mass spectrometer given its distance and time taken to travel said distance

A

velocity = distance/time
v=d/t

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16
Q

what equation can be used to find the mass of a sample when the velocity and energy are known

A

1/2mv² = KE

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17
Q

how many atomic orbitals are there
name them in order of energy

A

four
s, p, d, f

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18
Q

how many electrons can one orbital hold

A

2

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19
Q

how many electrons can the s orbital hold in total

A

2

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20
Q

how many electrons can the p orbital hold in total

A

6

21
Q

how many electrons can the d orbital hold in total

A

10

22
Q

how many electrons can the f orbital hold in total

A

14

23
Q

What orbitals does the first shell contain

A

only 1s

24
Q

What orbitals does the second shell contain

A

1s, 2s, 2p

25
Q

as you get further from the nucleus, how do the intervals in energy between the shells change, and what does this affect

A

the interval decreases, meaning that the order of shells will change, this first happens when the 4s orbital has less energy than the 3d orbital
the order becomes more complicated as the number of shells increases

26
Q

What do blocks in the periodic table indicate

A

the last energy level of the atom

27
Q

why must the ‘electrons’ in boxes have different pointing arrows

A

to show th at they have different directions in their spin

28
Q

what are the three rules for filling orbitals

A

orbitals with lower energy are filled first
orbitals of the same energy fill singly before they pair up
only 2 elections to an orbital

29
Q

define ionisation energy (word for word)

A

the energy required go remove one electron from each atom in one more of gaseous atoms to form one mole of gaseous 1+ ions

30
Q

what is the unit of IE

A

kJ/mol

31
Q

how does the IE change as electrons are removed and why

A

the energy needed becomes greater because as each electron is removed, the remaining ion becomes more positively charged
as the ion becomes more positive, the electrons experience more attraction to the nucleus
which required more energy to overcome

32
Q

what is the equation for the first ionisation energy of sodium

A

Na(g) —> Na(g)^+ + -e^-

33
Q

what s the second ionisation energy for sodium

A

Na^+(g) —-> Na^2+(g) + e^-

34
Q

what factors affect ionisation energy

A

atomic radius
nuclear charge
electron shielding

35
Q

how does the atomic radius affect IE

A

as the radius increaces, the IE decreaces

36
Q

how does the nuclear charge affect the IE

A

the greater nuclear charge the more energy required

37
Q

how does the electron shielding affect the IE

A

the more shells, the less energy required

38
Q

define shielding in an atom

A

the number of shells in the atom

39
Q

how does IE change as you go across periods

A

there is a general increace across a single period
but the IE drops dramatically at the start of a new period

40
Q

how does the IE change from group 2 to 3 and why

A

group 3 requires less energy than group 3
in group 2 the outermost electron is in an s orbital, meanwile group 3 is in a p orbital
p orbitals have more energy than s orbitals so the electron needs less energy supplied to it to leave its arrangement

41
Q

how does the IE change from group 5 to 6 and why

A

group 6 requires less energy than group 5
in group 5 the p orbital is filled singly, meanwhile in group 6 an one of the of the p orbitals is fully filled
the 2 electrons repel eachother in addition to the energy supplied
so less energy is needed to ionise a group 6 atom than a group 5 atom

42
Q

what is hunds rule

A

within a sublevel, place one electron per orbital before pairing them

43
Q

what is the pauli exclusion principle

A

each orobital can only hold up to two electrons with opposite spins

44
Q

what is the equation to find a particles mass from its mass number

A

mass number = (mass of particle in kg / avogadros constant) × 1000

45
Q

what equation can be used to find a particles energy from its mass, time, and distance travelled

A

2KE = m(d^2/t^2)

46
Q

what equation can be used to find the mass or time of one isotope from the mass and time of another

A

m1/t1^2=m2/t2^2

47
Q

what values do two particles share when they are measured using the same mass spectrometer

A

the energy and distance travelled

48
Q
A

A-Level Chemistry (5 decks)

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