Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

RSFC chemistry > 1.1 Atomic structure > Flashcards

1.1 Atomic structure Flashcards

1
Q

Bohr model

A

Consists of protons and neutrons in a nucleus and electrons in shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

JJ Thompson

A

Plum pudding model

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Ernest Rutherford

A

Nuclear model

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Properties of subatomic particles

A

Relative mass p-1 n-1 e-1/1840
Relative charge p-+1 n-0 e–1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Atomic number

A

Number of protons
Z

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Mass number

A

Protons and neutrons
A

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Cations

A

Lost electrons
Always paws-ative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Anions

A

Gained electrons
Negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Isotopes

A

Atoms with the same number of protons but different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why do isotopes of the same elements have the same chemical properties

A

They have the same electron configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Gold sheet experiment

A

Rutherford fired He2+ ions at a gold sheet
Most particles passed through as mostly empty space, some were deflected
Concluding, atoms are mostly empty space but have a small positive nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the Bohr model have

A

Electron shells
Small positive nucleus
Neutrons in nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Ionisation energy

A

The amount of energy it takes to remove one mole of electrons from one mole of atoms in a gaseous state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

First ionisation of rubidium equation

A

Rb (g) –> Rb+ (g) + e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Effect of nucleus charge on IE

A

More protons, stronger electrostatic attraction, more energy needed to remove outer electron
IE across period will increase as more protons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Effect of distance from nucleus on IE

A

Shorter distance, stronger electrostatic attraction, more energy required to remove outer electron
IE down group will decrease as more shells

17
Q

Effect of shielding on IE

A

more shells, larger distance between outer electron and nucleus, weaker electrostatic attraction, less energy needed to remove outer electron
IE down a group decreases as distance increases as more shells

18
Q

S orbital shape

A

Spherical

19
Q

P orbital shape

A

Dumbell

20
Q

Cr - electron config

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5
one electron moves from the 4s orbital to 3d to make it more stable

21
Q

Cu - electron config

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10one electron moves from the 4s orbital to 3d to make it more stable

22
Q

Boron deviation ionisation energy explanation

A

The first e- removed from Be is 2s subshell
The first e- removed from B is 2p subshell
2s is lower than 2p
Less energy is required to remove the B electron

23
Q

Oxygen deviation ionisation energy explanation

A

The first e- removed from N is 2p subshell unpaired
The first e- removed from O is 2p subshell paired
Due to electron pair repulsion, less energy is required to remove the electron from O

24
Q

Deviations in period 3

A

Aluminium and Sulfur

25
Q

Ionisation energy down a group

A

IE decreases
Protons and shielding increases
Distance from nucleus increases
Electrostatic attraction gets weaker
Less energy needed

26
Q

Ionisation energy across a period

A

IE increases
Same shielding
More electrons
Electrostatic attraction stronger
Atomic radius smaller

27
Q

What does mass spectrometry measure

A

Relative abundance
Mass / charge ratio

28
Q

Steps to mass spectrometry

A

Ionisation
Acceleration
Ion drift
Detection

29
Q

Why are sample particles ionised

A

So they can be accelerated towards the negative plate and generate a current by the detector

30
Q

How are ions accelerated

A

Positive ions attracted to negative plate
All ions have the same kinetic energy

31
Q

How are ions separated in the flight tube

A

Small m/z ions travel at higher speeds than ions will large m/z

32
Q

How are ions detected

A

Ions hit the detector
Ion gains an electron
Generates a current
Size of current is proportional to abundance

33
Q

Electron impact

A

Sample vaporised
High energy electrons are fired at sample from an electron gun
One electron is knocked off
X (g) –> X+ (g) + e-

34
Q

Electospray

A

Sample dissolved in volatile solvent
Injected through fine, hypodermic needle into a fine mist
Positive particles gain a proton

X (g) + H+ –> XH+ (g)

35
Q

Ar formula

A

(Mass x abundance) / total abundance

36
Q

Kinetic energy formula

A

KE = 1/2 mv2

37
Q

Velocity formula

A

V=d/t

38
Q

Avogadro constant

A

6.022 x 10^23 mol

RSFC chemistry (19 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions