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chemistry > atomic structure and periodic table > Flashcards

atomic structure and periodic table Flashcards

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1
Q

the model of an atom consists of what?

A

a small nucleus and electrons in orbital

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2
Q

who found this current model ?

A

rutherford

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3
Q

how did rutherford find it

A

scattering experiment 1911

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4
Q

what does the nucleus consist of?

A

protons and neutrons

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5
Q

whats the charge of a nucleus

A

positive

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6
Q

what is the atomic mass

A

the number of protons and neutrons

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7
Q

how is the atomic mass represented

A

A

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8
Q

what is the atomic number

A

the number of protons

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9
Q

how is the atomic mass represented

A

z

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10
Q

what is an isotope

A

different atom of the same element, same atomic number but different Atomic mass

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11
Q

what is relative atomic mass

A

mass of an atom of an element relative to 1/12 t of the mean mass of C-12

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12
Q

what is relative isotopic mass

A

the isotopic mass of an isotope relative to 1/12 the mean mass of the C-12 isotope

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13
Q

what is relative molecular mass

A

mean mass of a molecule of a compound relative to 1/12 the mean mass of the C-12 isotope

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14
Q

what is relative formula mass

A

Mr but used for compounds with giant structures

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15
Q

how are ions formed

A

when an atom gains or looses an electron

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16
Q

what are they used for

A

the analytical technique of mass spectrometry

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17
Q

what is time of flight

A

time of flight records the time it takes for ions of each isotope to reach a detector

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18
Q

what is step 1 of mass spectrometry

A

ionisation

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19
Q

how is step 1 of mass spectrometry done

A

atom in gaseous state is bombarded with electrons

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20
Q

what is step 2 of mass spectrometry

A

acceleration

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21
Q

how is step 2 of mass spectrometry done

A

positively charged ions are accelerated to a negative detector

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22
Q

what is step 3 of mass spectrometry

A

ion drift

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23
Q

how is step 3 done

A

ions are deflected by a magnetic field into a curved path

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24
Q

what is step 4 of mass spectrometry

A

detection

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25
Q

how is step 4 of mass spectrometry done

A

+ ions git the - detection plate. they gain an electron, producing a current. the greater the abundance, the greater the current produced

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26
Q

what is step 5 of mass spectrometry

A

analysis

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27
Q

how is step 5 of mass spectrometry done

A

current values are used in a combination with the flight times

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28
Q

how can u calculate the Ar using printed spectra

A

Ar-(m/z x abundance)/ total abundance

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29
Q

what is ionisation energy

A

the minimum energy required to remove the highest energy electron from an atom in its gaseous state

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30
Q

what is successive ionisation energies

A

when further electrons are removed- usually requires more energy because as electrons are removed, the electrostatic forces increase between the nucleus and electrons

31
Q

trend in 1st ionisation across a period

A

increases as the radius decreases due to more electrons and more electrostatic forces

32
Q

trend in 1st ionisation down a group

A

decreases as there are more shells that act as shielding and therefore there are less electrostatic forces

33
Q

what does a sudden large increase in successive ionisation energies on a graph indicate

A

a change in energy levels

34
Q

why is the first ionisation energy of aluminium lower than expected?

A

it has a single pair of electrons with opposite spin. this means there is a repulsion

35
Q

what is the current model of electronic configuration based on

A
  • emmission spectra provides evidence for quantum shells
  • successive ionisation energies prove quantum shells within atoms and sugest the atoms group
  • first ionisation energy
36
Q

what are electron orbitals

A

a cloud of negative charge where electrons are held

37
Q

what are the different types of electron orbitals

A

S P D & F

38
Q

what is the shape os the S orbital

A

spherical

39
Q

what is the shape of the P orbital

A

dumbbell

40
Q

what do the electron orbitals corrispond with

A

blocks in the periodic table

41
Q

what periods fall in the S block

A

periods 1&2

42
Q

what periods fall in the D block

A

Transition metals

43
Q

what periods fall in the P block

A

3,4,5,6,7&8

44
Q

what periods fall in the F block

A

the two at the bottom

45
Q

how many electrons can the S subshell hold

A

2 electrons

46
Q

how many electrons can the P subshell hold

A

6 electrons

47
Q

how many electrons can the D subshell hold

A

10 electrons

48
Q

what is the energy trend of the orbitals from S-D

A

the energy of the orbitals increase which means that the orbitals are filled from S-D

49
Q

whats the order of the orbitals being filled

A

S P D F

50
Q

sodium has 11 electrons . how will the configuration be written

A

Na=1s2, 2s2, 2p6,3s1

51
Q

how many energy levels does sodium have

A

3

52
Q

how many orbitals does sodium have?

A

4

53
Q

what is spin in an electron

A

within an orbital, electrons pair up with opposite spin

54
Q

why do electrons pair up with opposite spin?

A

so the atom has maximum stability

55
Q

how is spin represented

A

opposite arrows

56
Q

rule one for writing out electron configurations

A

the lowest energy orbital is filled first

57
Q

rule two for writing out electron configuration

A

electrons with the same spin fill up an orbital first before pairing begins

58
Q

what is rule 3 for electron configuration

A

no single orbital holds more than 2 electrons

59
Q

what is an exception to the rule?

A

if electron spins are unpaired and therefore unbalanced, it produces a natural repulsion between the electrons

60
Q

what does a natural repulsion within the electrons result in

A

a very unstable atom

61
Q

what happens when the atom is unstable

A

the electrons may take a different arrangement to improve stability

62
Q

the 3p4 orbital has a single pair of electrons with opposite spins making it unstable, what then happens

A

an electron moves to the 4s shell to make it more stable and the configuration is now 3p3 4s1

63
Q

what does periodicity refer to

A

the study of patterns of physical atomic and chemical properties

64
Q

what does the periodic table arrange the elements by

A

the atomic (proton) number

65
Q

what do the elements along a period have in common

A

they have the same number of shells

66
Q

what do elements down a group have in common?

A

they have the same umber of electrons in its outer shell

67
Q

what happens to the atomic radius across a period and why

A

decreases because there are more electrons which means there is a higher nuclear charge and more inter molecular forces

68
Q

what happens to atomic radius down a group and why

A

increases because there are more shells

69
Q

ionisation energy along a period

A

increases because of the decreased atomic radius which results in higher attractions

70
Q

ionisation energy down a group

A

decreases because of more shells which act as sheilds and higher atomic radius

71
Q

where do the melting points of period 2 element peak

A

around the middle

72
Q

boron and carbon form what?

A

giant covalent lattices with strong covalent bonds

73
Q

what bonding does lithium and beryllium have?

A

metallic bonding

74
Q

what is the general trend in ionisation energies along period 2

A

it increases because the atomic radius is decreasing

chemistry (11 decks)

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