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Chemistry > marmar atomic structure > Flashcards

marmar atomic structure Flashcards

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1
Q

what are charges and weights

of the fundamental particles and how are they arranged in an atom

A

proton - +1 weight 1
neutron- 0 weight 1
electron- -1 weight 1/2000

protons and electrons are placed in the nucleus and electrons prbit around the nucleus in 3d fields called
orbitals

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2
Q

how may kinds

of orbitals are there and what order do they fill up in

A

s , p , d , f

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3
Q

how many s orbitals can fit

in one energy level

A

1

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4
Q

how many p orbitals can fit in one energy

level ?

A

3

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5
Q

how many d orbitals can fit in one energy level

A

5

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6
Q

how many f orbitals can fit

in one energy level

A

7

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7
Q

how many electrons can be placed in one orbital ?

describe the electrons

A

2 electrons with opposite spins

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8
Q

how do the electrons

fill up each set of orbitals

A

they fill up one in each orbital and them two - bus analogy

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9
Q

define
an
orbital

A

a region of
space
you are likely to find an electron

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10
Q

how does the periodic table show which orbital the element should end
in

A
  • transitional metals d
  • non metals p
  • reactive metals ( far right ) s
  • bottom bar f
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11
Q

what is the rule about 4s and 3d

A

the shells fill up

3s 3p 4s 3d 4p 4d 4f

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12
Q

what are the two exceptions to the 4s 3d rule

A

copper and chromium fill 3d then 4s

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13
Q

what should the electron configuration

for an ion be the same as

A

the noble gas on the period above it

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14
Q

whats the electron notation for a magnesium atom - atomic number 12

A

1s(2)2s(2)2p(6)3s(2)

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15
Q 
whats the electron comfiguration for
a magnesium ion ?
if the atomic
number
of
magnesium is 12
A

1s(2)2s(2)2p(6)

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16
Q

define first ionisation energy ?

A

the energy needed to remove on
mole of electrons from one
mole of gaseous ayoms to form one mile
of positive ions

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17
Q

define second ionisation energy

A

the energy required to
remove one mole of electrons
from one
mole of gaseous charged positive ions

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18
Q

what is successive ionisation energy

A

often a group of several ionisation energies . each one is the removal of an electron from the shells of an
atom or ion

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19
Q

how do you tell what group an atom is in from
its successive ionisation energy table
of graph

A 
you see when the first big
jump is and after how many values . the number of values before the first big
jump represents the number
of electrons
on the outermost shell
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20
Q

which shell requires the most energy to remove an electron from

A

shell 1 - closest to nucleus strongest attraction least shielding

21
Q

describe in details the graph of first ionisation energy in the third period

A
  • na goes up
  • mg goes up
  • al goes down
  • si goes up
  • p goes up
  • s goes down
  • cl goes up
  • ar goes up
22
Q

why does the ionisation energy in al and s change , and what is the change

A

the ionisation energy required decreases
this is because aluminiums first electron is a lone electron in 3p orbital
sheilding from the 3s orbital means the electron is lost easier
the electron is easier to remove from sulphur because the final electron is placed in the first full pair of electrons in the 3px orbital .this means there is an increase in repulsive forces making it easier to to be removed

23
Q

how do first ionisation energy change down a group ?

A

it decreases -mainly because the atomic radius increases

24
Q

describe a graph of atomic radius across the third period

A

na ——->Ar

high atomic radius——>low atomic radius

25
Q

describe a graph for melting point for the third period

A
  • na -mg increase
  • mg -al smaller gradient increase
  • al-si dramatic increase
  • si-p DRAMATIC DROP
  • p-s low gradient increase
  • s-cl decrease
  • cl-ar decrease
26
Q

describe a graph for electronegativity across the third period ?

A

increase from na -cl

then drop to ar

27
Q

describe the graph of boiling point across the third period

A
  • general increase from na to al
  • decrease down si and p
  • up a little bit for s
  • down to cl and ar
28
Q

how does atomic radius change over a period

A

-decrease
-further across you go , greater attractive forces between nucleus and shells
-that force pulls them
closer together

29
Q

whats an IMPORTANT THING to remember when doing ionisation equations

A

EVERYTHING IS GASEOUS

30
Q

describe the graph for conductivity and why it is like this for the third period

A

flat na -mg
up from mg -a
-down to 0 for silicon
-and zero for the rest

na , mg and al )all metals with sea of delocalised electrons

31
Q

what is electronegativity

A

THE ABILITY OF AN ATOM TO ATTRACT THE PAIR OF ELECTRONS IN A COVALENT BOND TO ITSELF

32
Q

whats the general trend for electronegativity across a period

A
  • increase

- nuclear charge increases therefore so does the attraction for the shared pair of electrons

33
Q

who proposed the idea that tiny particles called atoms exist and when

A

JOHN DALTON

1803

34
Q

who realised atoms are divisible and contain tiny negatively charged particles called electrons

A

J.J.THOMSON

1897

35
Q

who discovered an atom is made of a nucleus and extra nuclear part .and that the nucleus is positive and electrons orbit it

A

ERNEST RUTHERFORD

1911

36
Q

who proposed electrons orbit

in orbitals with set sizes and energies

A

NIELS BOHR

1915

37
Q

who proposed the idea that electrons spin around due to repellant
forces

A

WOLFGANG PAULI

1924

38
Q

who discovered that atoms contain neutrons

A

JAMES CHADWICK

1932

39
Q

describe what happens to the particles that go throgh a mass spectrometer

A

-its vapourised as atoms must be gaseous
to be ionised
-it goes through an ion source becoming +1 as an electrons is fired at it
knocking off an electron
-a vacuum pump ensures no air molecules are present
-it is accelerated through an electrical field
-then deflected by the electrical field
-then it hits a detector, the heavier the atom the smaller the arc of deflection

40
Q

what does m/z mean in mass

spectrometry and why does mass only matter really

A

m/z means mass / charge
the charge of
particles is pretty much always +1 but sometimes +2

41
Q

what are the uses of a mass

spectrometer

A
  • characterises compounds-tells you what in it
  • detects counterfeit medications
  • security -detects bombs and drugs
42
Q

whats the acronym for the process in a mass spectrometer

A 
V-vaporisation
I-ion source
A-acceleration
D-deflection by magnetic or electric field 
D-detection
43
Q

how do you find the atomic

mass of a compound on a spectrum graph

A

you look for the heaviest peak -peak furthest to the right

44
Q

in general if you get a m/z of
-15
-29
what molecules are they

A
  • CH3

- c2h5

45
Q

describe the melting point graph of the third period element

A 
-na-al ---> general increase
   (metallic bonding but increase in charge density so more energy needed)
-si-----> goes up dramatically
(giant covalent,more energy needed
to break bonds)
-p--->sudden drop , p4
(simple covalent molecule)
-s---->very slight increase, s8
(still simple covalent)
-cl---->goes downcl2
(simple covalent but angas at room temp)
-ar---->down 
(monatomic )
46
Q

explain why the melting point of thenthird period

follows this trend

A

-first 3 are metals so a pretty regular increase shows that the more charged a molecule is the more powerful the attraction is between each atom
-silicone is a giant covalent structure with hundreds
of covalent bonds so the melting point goes up dramatically
-phosphor decreases as its simple covalent but has weak intermolecular forces
-sulphur goes up because its s8 meaning its a bigger structure and
has slightly bigger molecules so strong intermolecular forces
-cl goes down becausneits diatomic and a gas
-ar is monatomic and easy

47
Q

how do you predict the element with highest ionisation energy on any ionisation energy

A

its the same as the first ionisation energy but the trend has MOVED ONE TO THE LEFT

48
Q

whats the formula for finding out the relative atomic mass in reverse
using the isotopes 10 and 11 and the ram 10.8

A

(10x x)+(11(100-x))
——————–=10.8
100

Chemistry (10 decks)

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