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A Level Chemistry- KE > Atomic structure and the periodic table (TOPIC 1) > Flashcards

Atomic structure and the periodic table (TOPIC 1) Flashcards

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?

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
what are s block elements?
groups 1+2,, have outer shell configuration of 1s or 2s
26
what are p block elements?
groups 3,4,5,6,7,0,, have outer shell configuration of s2p1 to s2p6
27
what are d block elements?
transition metals,,
28
what is the copper and chromium exception?
they donate one of the 4s electrons to the 3d subshell
28
why do Cr and Cu donate electrons from 4s to 3d?
more stable with full or half full d-subshell
29
what is first ionisation energy?
energy needed to remove 1 electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions
30
what factors affect ionisation energy?
nuclear charge, shielding, electron shell
31
how does nuclear charge affect ionisation energy?
more protons in nucleus= more positive nucleus= stronger attraction between electrons
32
how do electron shells affect ionisation energy?
attraction decreases with distance ∴ electron shell close to nucleus is more attracted to one further away
33
how does shielding affect ionisation energy?
more electrons between outer electrons and nucleus= outer electrons feel less attraction to nuclear charge
34
what does high ionisation energy mean?
strong attraction between electron+nucleus ∴more energy needed to overcome attraction+remove electron
35
why does the first ionisation energy decrease down a group?
-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
why does first ionisation energy increase across a period?
-number of protons is increasing= stronger nuclear attraction
37
what is periodicity?
repeating pattern across different periods e.g. across periods atomic radius decreases
38
how does electron configuration decide the chemical properties of an element?
-number of outer shell electrons decides chemical properties because it determines if a positive or negative ion can be made
39
group 0 elements have a full outer shell therefore they are?
inert
40
why does atomic radius decrease across a period?
number of protons increases= electrons pulled closer to nucleus
41
why don't the electrons the elements gain across a period effect atomic radius?
they are added to the outer energy level ∴ don't provide extra shielding effect
42
why do melting and boiling points increase across a period for metals? e.g. Li, Be + Na, Mg, Al
-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
what is periodicity?
repeating trends across different periods
44
how to predict mass spectra for diatomic molecules?
-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
what is successive ionisation energy?
energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form one mole of 2+ ions
46
how do successive ionisation energies provide evidence for shell structure?
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
how does atomic emission spectra provide evidence for the existence of quantum shells?
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
what can be identified from successive ionisation energy graphs?
group number,, electronic structure,, shell structure
49
how to identify group number on successive ionisation energy graphs?
see how many electrons are removed before the first big jump,, shows how many electrons in outer shell

A Level Chemistry- KE (18 decks)

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