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A Level Chemistry- KE > Atomic structure and the periodic table > Flashcards

Atomic structure and the periodic table Flashcards

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1
Q

what is an isotope?

A

element with same number of protons but different number of neutrons

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2
Q

why do isotopes of elements have slightly different physical properties?

A

they have different masses

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3
Q

what is relative isotopic mass?

A

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

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4
Q

what is relative atomic mass?

A

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

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5
Q

how to work out relative molecular mass

A

-used only for simple molecules
-add up relative atomic masses of all atoms in molecule

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6
Q

how to work out relative formula mass

A

-

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7
Q

how many orbitals does ‘s’ have and how many electrons can it hold?

A

1 orbital, 2 electrons

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8
Q

how many orbitals does ‘p’ have and how many electrons can it hold?

A

3 orbitals, holds 2 in each

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9
Q

how many orbitals does ‘d’ have and how many electrons can it hold?

A

5 orbitals, holds 5 electrons

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10
Q

how many orbitals does ‘f’ have and how many electrons can it hold?

A

7 orbitals, holds 2 electrons

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11
Q

how many electrons can each orbital hold?

A

2

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12
Q

what is an orbital?

A

region within an atom that can hold up to 2 electrons with opposite spins (spin pairing)

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13
Q

what is the shape of the ‘s’ orbital?

A

spherical

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14
Q

what is the shape of the ‘p’ orbital?

A

dumbell

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15
Q

what is the structure of an electron shell?

A

shell>subshell>orbital

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16
Q

do shells have more energy closer or further from nucleus?

A

further

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17
Q

when do orbitals have the same energy?

A

when in same subshell e.g. Px Py Pz all have same

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18
Q

how many electrons fill the first quantum shell?

A

2

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19
Q

how many electrons fill the second quantum shell?

A

8

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20
Q

how many electrons fill the third quantum shell?

A

18

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21
Q

how many electrons fill the fourth quantum shell?

A

32

22
Q

how are the p orbitals arranged?

A

dumbbells are are at right angles to one an other

23
Q

how do electrons arrange themselves in the subshells?

A

electrons fill up at lowest energy subshells first singly before pairing up

24
Q

what is the exception in electron configurations?

A

4s has lower energy level than 3d subshell- 4s fills up first

25
Q

what are s block elements?

A

groups 1+2,, have outer shell configuration of 1s or 2s

26
Q

what are p block elements?

A

groups 3,4,5,6,7,0,, have outer shell configuration of s2p1 to s2p6

27
Q

what are d block elements?

A

transition metals,,

28
Q

what is the copper and chromium exception?

A

they donate one of the 4s electrons to the 3d subshell

28
Q

why do Cr and Cu donate electrons from 4s to 3d?

A

more stable with full or half full d-subshell

29
Q

what is first ionisation energy?

A

energy needed to remove 1 electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions

30
Q

what factors affect ionisation energy?

A

nuclear charge, shielding, electron shell

31
Q

how does nuclear charge affect ionisation energy?

A

more protons in nucleus= more positive nucleus= stronger attraction between electrons

32
Q

how do electron shells affect ionisation energy?

A

attraction decreases with distance ∴ electron shell close to nucleus is more attracted to one further away

33
Q

how does shielding affect ionisation energy?

A

more electrons between outer electrons and nucleus= outer electrons feel less attraction to nuclear charge

34
Q

what does high ionisation energy mean?

A

strong attraction between electron+nucleus ∴more energy needed to overcome attraction+remove electron

35
Q

why does the first ionisation energy decrease down a group?

A

-elements further down a group the number of electron shells increase ∴ atomic radii increases ∴ there is less attraction to the nucleus from the outer electrons
-extra inner shells shield outer electrons from attraction of nucleus

36
Q

why does first ionisation energy increase across a period?

A

-number of protons is increasing= stronger nuclear attraction

37
Q

what is periodicity?

A

repeating pattern across different periods e.g. across periods atomic radius decreases

38
Q

how does electron configuration decide the chemical properties of an element?

A

-number of outer shell electrons decides chemical properties because it determines if a positive or negative ion can be made

39
Q

group 0 elements have a full outer shell therefore they are?

A

inert

40
Q

why does atomic radius decrease across a period?

A

number of protons increases= electrons pulled closer to nucleus

41
Q

why don’t the electrons the elements gain across a period effect atomic radius?

A

they are added to the outer energy level ∴ don’t provide extra shielding effect

42
Q

why do melting and boiling points increase across a period for metals? e.g. Li, Be + Na, Mg, Al

A

-metallic bonds get stronger because metal ions have an increasing number of delocalised electrons + decreasing radius ∴ higher charge density
-results in stronger attraction between metal ions+delocalised electrons∴stronger metallic bonding

43
Q

what is periodicity?

A

repeating trends across different periods

44
Q

how to predict mass spectra for diatomic molecules?

A

-put isotope percentage abundance in decimals
-make table of all different diatomic molecules e.g. Cl₂,, Cl-35 and Cl-37
-multiply the abundances of isotopes
-any molecules in table that are the same add them together e.g.Cl-35 and Cl-35
-divide all relative abundances by smallest relative abundance to get the smallest whole number ratio

45
Q

what is successive ionisation energy?

A

energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form one mole of 2+ ions

46
Q

how do successive ionisation energies provide evidence for shell structure?

A

successive ionisation energies increase steadily and will then jump suddenly at one point, this is the point at which electrons are in a different shell

47
Q

how does atomic emission spectra provide evidence for the existence of quantum shells?

A

shows that specific amounts of energy are emitted when electrons drop down from higher to lower energy levels,,,in-between amounts of energy are never emitted suggesting electrons only exist at specific energy levels,,they are discrete

48
Q

what can be identified from successive ionisation energy graphs?

A

group number,, electronic structure,, shell structure

49
Q

how to identify group number on successive ionisation energy graphs?

A

see how many electrons are removed before the first big jump,, shows how many electrons in outer shell

A Level Chemistry- KE (15 decks)

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