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AS-Level Chemistry Unit 1 > 1.2 Basic Ideas of Atoms > Flashcards

1.2 Basic Ideas of Atoms Flashcards

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1
Q

What effects ionisation energy?

A

Distance of outer shell from nucleus – the attraction decreases the further away the outer electron is from the nucleus
Nuclear charge – the greater the nuclear charge, the greater the attraction for the outer electron.
Electron shielding – filled inner shells or subshells of electrons act as shields. The outer electron is shielded from the nuclear charge by these shells or sub-shells

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2
Q

What is molar ionisation energy?

A

the energy required to completely remove one mole of electrons from one mole of its gaseous atoms to form 1 mole of gaseous 1+ ions

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3
Q

What is standard molar ionisation energy?

A

At 1 atm pressure and 25 degrees, the energy required to completely remove one mole of electrons from one mole of its gaseous atoms to form 1 mole of gaseous 1+ ions

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4
Q

how many electrons in the s orbital?

A

2

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5
Q

how many electrons in the p orbital?

A

6

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6
Q

how many electrons in the d orbital?

A

10

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7
Q

What is the shape of a s orbital?

A

spherical

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8
Q

What is the shape of a p orbital?

A

dumbell

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9
Q

Why has lithium got a higher first ionisation energy compared to sodium?

A

Li has a higher first ionisation energy because the outermost electron is closer to the nucleus experiencing less shielding, outweighing the increased nuclear charge of sodium

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10
Q

Why does Kr have a lower first ionisation energy than Ne?

A

Kr has a lower first ionisation energy than Ne because its outer electron is further away from the nucleus, experiencing greater shielding that outweighs the increased nuclear charge

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11
Q

What is the general trend of ionisation energy in groups?

A

as you go down the group, the first ionisation energy decreases
because the outer electron becomes further away from the nucleus, experiencing greater shielding, outweighing the increased nuclear charge

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12
Q

What is the general trend of ionisation energy in periods?

A

as you go from left to right across a period, the ionisation energy increases
because the outermost electron remains the same distance from the nucleus and experiences the same shielding, while the nuclear charge increases

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13
Q

Why is the second ionisation energy of sodium greater than that of magnesium?

A

Na- 1s2, 2s2, 2p6, 3s1
Mg- 1s2, 2s2, 2p6, 3s2
the second electron being removed in sodium is closer to the nucleus than that of magnesium, therefore experiences less shielding

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14
Q

What is the relative mass of a proton?

A

1

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15
Q

What is the relative mass of a electron?

A

almost 0
1/1840

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16
Q

What is the relative mass of a neutron?

A

1

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17
Q

What is the relative charge of a proton?

A

+1

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18
Q

What is the relative charge of a electron?

A

-1

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19
Q

What is the relative charge of a neutron?

A

0

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20
Q

What is an isotope?

A

the same element, with the same number of protons but different number of neutrons

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21
Q

What are ions?

A

charged particles where the number of electrons is not equal to the number of protons.

22
Q

What are the types of radioactive emission?

A

alpha
beta
gamma

23
Q

What is alpha?

A

2 protons and 2 neutrons
helium nucleus

24
Q

What is beta?

A

high energy electron

25
Q

What is gamma?

A

High energy electromagnetic wave

26
Q

What is the mass of alpha?

A

4 atomic mass unit

27
Q

What is the mass of beta?

A

almost 0
negligible

28
Q

What is the mass of gamma?

A

almost 0

29
Q

What is the effect of the electromagnetic field on alpha?

A

attracted to the negative plate

30
Q

What is the effect of the electromagnetic field on beta?

A

attracted to the positive plate

31
Q

What is the effect of the electromagnetic field on gamma?

A

no effect

32
Q

What is the penetrating power of alpha?

A

stopped by a sheet of paper

33
Q

What is the penetrating power of beta?

A

stopped by 0.5cm of aluminium

34
Q

What is the penetrating power of gamma?

A

stopped by more than 2cm of lead

35
Q

Does gamma change the mass/atomic number of an atom?

A

no
because it is a form of energy and is not an atomic particle

36
Q

Does alpha emission change the mass/atomic number of an atom?

A

yes
when emitted it cause the mass number to decrease by 4 and the atomic number to decrease by 2
2 places to the left in the periodic table

37
Q

Does beta change the mass/atomic number of an atom?

A

yes
mass number is unchanged and the atomic number increases by 1
1 place to the right in the periodic table

38
Q

What is electron capture?

A

when one of the electrons is captured by a proton, turning it into a neutron
Atomic number goes down by one

39
Q

What is positron emission?

A

a proton is converted to a neutron resulting in the emission of a positron
Atomic number goes down by one
1 to the left in the periodic table

40
Q

What is half-life?

A

the time taken for half of the radioactive nuclei in a sample to decay

41
Q

What can ionising radiation do to the body?

A

DNA can become damaged, which can cause mutations and cancerous cells

42
Q

Which wave has the highest frequency?

A

gamma rays

43
Q

What equation links energy and frequency?

A

E=hf

44
Q

What is h?

A

planck’s constant and is unchanged

45
Q

What equation links speed of light and frequency?

A

c=f x lamda(wavelength)

46
Q

What is c?

A

speed of light which is unchanged

47
Q

What is the absorption spectra?

A

this displays an entire spectrum with black lines for the ‘missing’ frequencies of photons that have been absorbed when an electron moves up an energy level

48
Q

What is the emission spectra?

A

this displays lines at the specific frequencies of emitted photons from when an electron moves down an energy level

49
Q

What is the hydrogen spectrum?

A

it is an emission spectrum
the lines represent energy released as the promoted electron falls back down to lower energy levels or shells. Each line is equal to the difference in energy, between two particular energy levels, which means it is a quantum

50
Q

What is Lyman’s series?

A

The lines in the Lyman series are in the area with highest frequency/energy (ultraviolet)
This is because they are due to electrons falling down to the n=1 shell (closest to the nucleus)

51
Q

What is Balmer’s series?

A

is in the visible part of the spectrum, which has lower energy. Lines here are due to electrons falling down to the n=2 shell

52
Q

Ionisation of the hydrogen atom

A

can be measured using the convergent frequency of the Lyman series
the spectral lines get closer and closer together as the frequency of the radiation increases until eventually they converge together
This is known as the convergence limit. When the electron reaches this, its energy is no longer quantised and the nucleus has lost all influence over the electron, so the atom has become ionised

AS-Level Chemistry Unit 1 (8 decks)

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