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Chemistry > Atoms > Flashcards

Atoms Flashcards

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1
Q

John Dalton

A

All matter is made up from atoms

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2
Q

J.J Thompson

A

Plum pudding model, Atoms are divisible and contain tiny little electrons

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3
Q

Ernest Rutherford

A

Atom made up from a nucleus and extra nucleus part

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4
Q

Niels bohr

A

Electrons orbit around the nucleus in orbit

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5
Q

Wolfgang pauli

A

Concept of electron spin

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6
Q

James Chadwick

A

Nucleus contains neutrons

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7
Q

Order of the scientists atom models

A

John Dalton
J.J Thompson
Ernest Rutherford
Niels Bohr
Wolfgang Pauli
James Chadwick

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8
Q

Limitations of the atom model

A

It’s only 2D
Electrons don’t orbit the nucleus
the nucleus is 50,000 times smaller than

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9
Q

Orbitals

A

are mostly empty space (they are electron shells)

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10
Q

Nucleon

A

Term for both protons and neutrons

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11
Q

What force holds protons and neutrons together

A

The strong nuclear force

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12
Q

What holds together protons and electrons

A

Electrostatic forces of attraction

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13
Q

is the electrostatic forces of attraction larger or the strong nuclear force

A

The strong nuclear force is bigger

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14
Q

Proton charge (coulombs)

A

+1.602 times 10 to the power of -19

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15
Q

Neutron charge in coulombs

A

0

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16
Q

Electron charge in coulombs

A

-1.602 times 10 to the power of -19

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17
Q

Proton mass in Kg

A

1.673 times 10 to the power of -27

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18
Q

Neutron mass in Kg

A

1.673 times 10 to the power of -27

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19
Q

Electron mass in Kg

A

0.911 times 10 to the power of -30

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20
Q

RAM definition

A

Relative atomic mass is the average mass of an atom of an element to 1/12 of of the mass of an atom of carbon 12

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21
Q

Molecular mass

A

average mass of a molecule of an atom to 1/12 of of the mass of an atom of carbon 12

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22
Q

What is the empirical formula

A

the simplest ratio of an element in a compound

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23
Q

what is mass spectrometry used for

A

drug development, environmental testing and forensics

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24
Q

electron impact ionisation

A

the sample is vaporised
then high energy electrons from an electron gun
emits an electron which knocks off an electron from the sample forming a 1+ ion

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25
Q

Electrospray ionisation

A

sample is dissolved in a volatile solution and injected through a fine needle which is attached to a high voltage power supply. particles then gain a proton

26
Q

Step two of mass spectrometry

A

acceleration

position ions and accelerated using an electric field so they all have the same kinetic energy

27
Q

Step 3 of mass spectrometry

A

ion drift
the + ions travel though a hole in the negative charged plates into a tube. the time it takes to travel depends on its mass

28
Q

Step 4 of mass spectrometry

A

Detection
the + ions hit a - electrically charged plate where they are discharged by gaining electrons.
this generates a current which can be measured for the number of ions

29
Q

Electospray ionising equation

A

X(g) + H+ —> XH+(g)

where X is the sample

30
Q

electron impact ionisation equation

A

X(g) —> X+ (g) + e-

31
Q

Electron configuration

A

2 8 18

32
Q

Outer electrons have more or less energy

A

Outer electrons have more energy than those closer to the nucleus

33
Q

What orbital fills up before 3D

A

4S

34
Q

What do half arrows represent

A

Electron spin

35
Q

When do electrons pair up

A

When all orbitals are full

36
Q

What orbital has 2 shapes

A

S orbital

37
Q

What orbital has 3 shapes

A

P orbital

38
Q

What orbital has five shapes

A

D orbital

39
Q

Copper- what shell only half fills

A

4S half fills then 3D fully fills

40
Q

Copper- what shell only half fills

A

4S half fills then 3D fully fills

41
Q

ionisation energy units

A

KJ mol-1

42
Q

Factors that affect ionisation energy

A

Affective nuclear charge
Distance from the nucleus
Shielding (how many energy levels)

43
Q

Atom

A

neutral particle made up from protons and neutrons in a center nucleus and electrons orbiting the nucleus

44
Q

Atomic number

A

the number of protons in the nucleus of an atom

45
Q

Charge cloud

A

An area in an atom or molecule where there is a high probability of finding an electron pair

46
Q

Electron

A

Subatomic particle with a relative mass of 1/1840 located in orbitals around the nucleus

47
Q

electron configuration

A

the number of electrons in an atom or ion and how they are arranged

48
Q

energy level

A

region of an atom with a fixed energy that contains electrons

49
Q

first ionisation energy

A

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

50
Q

ion

A

charged particle

51
Q

ion

A

charged particle

52
Q

mass number

A

total number of protons and neutrons in the nucleus of an atom

53
Q

mass spectrometry

A

analytic technique used to identify elements and molecules and determine atom/molecular mass

54
Q

neutron

A

neutral subatomic particle located in the nucleus of an atom

55
Q

proton

A

positively charged atom located in the centre of the nucleus

56
Q

ratio for chlorine abundance

A

9:6:1

57
Q

Massspec. Reason for smaller peaks on graph that are half the mr

A

2+ ions that are less formed due to more energy needed to form them

58
Q

Are isotopes sizes the same (nucleus radius)

A

Yes because they have the same affective nuclear charge

59
Q

What speeds up the ions in acceleration

A

An electric field

60
Q

Why do you not use more than the minimum energy to ionise samples in TOF

A

so no more than one electron is knocked off

61
Q

Why must the sample be ionised

A

Acceleration
Detection

Chemistry (13 decks)

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