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Atoms Flashcards

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
Electrospray ionisation
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
Step two of mass spectrometry
acceleration position ions and accelerated using an electric field so they all have the same kinetic energy
27
Step 3 of mass spectrometry
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
Step 4 of mass spectrometry
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
Electospray ionising equation
X(g) + H+ —> XH+(g) where X is the sample
30
electron impact ionisation equation
X(g) —> X+ (g) + e-
31
Electron configuration
2 8 18
32
Outer electrons have more or less energy
Outer electrons have more energy than those closer to the nucleus
33
What orbital fills up before 3D
4S
34
What do half arrows represent
Electron spin
35
When do electrons pair up
When all orbitals are full
36
What orbital has 2 shapes
S orbital
37
What orbital has 3 shapes
P orbital
38
What orbital has five shapes
D orbital
39
Copper- what shell only half fills
4S half fills then 3D fully fills
40
Copper- what shell only half fills
4S half fills then 3D fully fills
41
ionisation energy units
KJ mol-1
42
Factors that affect ionisation energy
Affective nuclear charge Distance from the nucleus Shielding (how many energy levels)
43
Atom
neutral particle made up from protons and neutrons in a center nucleus and electrons orbiting the nucleus
44
Atomic number
the number of protons in the nucleus of an atom
45
Charge cloud
An area in an atom or molecule where there is a high probability of finding an electron pair
46
Electron
Subatomic particle with a relative mass of 1/1840 located in orbitals around the nucleus
47
electron configuration
the number of electrons in an atom or ion and how they are arranged
48
energy level
region of an atom with a fixed energy that contains electrons
49
first ionisation energy
the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous +1 ions
50
ion
charged particle
51
ion
charged particle
52
mass number
total number of protons and neutrons in the nucleus of an atom
53
mass spectrometry
analytic technique used to identify elements and molecules and determine atom/molecular mass
54
neutron
neutral subatomic particle located in the nucleus of an atom
55
proton
positively charged atom located in the centre of the nucleus
56
ratio for chlorine abundance
9:6:1
57
Massspec. Reason for smaller peaks on graph that are half the mr
2+ ions that are less formed due to more energy needed to form them
58
Are isotopes sizes the same (nucleus radius)
Yes because they have the same affective nuclear charge
59
What speeds up the ions in acceleration
An electric field
60
Why do you not use more than the minimum energy to ionise samples in TOF
so no more than one electron is knocked off
61
Why must the sample be ionised
Acceleration Detection
62
What might be the same on a mass spec of the same sample and why
Same peak same sample
63
How do van der waals arise
Electron movement induces a dipole in another molecule then an adjacent molecule
64
How can a mixture of methanol methanethiol be separated
Fractional distillation
65
How to make a functional group isomer
Make it cyclo
66
What element in period 3 has the highest melted point
Silicon Giant covalent covalent bonds
67
Why is mass spec done under a vacuum
So no other particles can collide affecting the samples speed
68
What are used for stating materials in antifreeze Polymers and paints
Alkenes
69
How does increased carbon length chain affect alkenes solubility in water (polar)
Decreased solubility in polar things but can disolver in other hydrocarbons
70
How are oxides of nitrogen produced during combustion
Oxygen and nitrogen react at high temperatures
71
72
Why do infrared gasses absorb radiation
To make bonds vibrate
73
74
75
Carbon neutral
No net emissions of co2 into the atmosphere
76
Why do samples need to be ionised
For acceleration Detection

Chemistry (15 decks)

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