Brainscape's Knowledge GenomeTM

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


See full index

CHEMISTRY A-LEVEL > Atomic Structure > Flashcards

Atomic Structure Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

Relative atomic mass

A

The average mass of an atom of an element compared to 1/12th the mass of an atom of carbon-12

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

Relative molecular mass

A

The average mass of a molecule of an element or compound compared to 1/12th the mass of an atom of carbon-12

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

Isotope

A

Atoms of the same element with the same number fo protons but a different number of neutrons

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

Mass number

A

The total number of protons and neutrons in the nucleus

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

Atomic number

A

The number of protons in the nucleus

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

First ionisation energy

A

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

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

Second ionisation energy

A

The energy required to remove 1 mole of electrons from 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions

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

Orbital

A

The region where an electron is most likely to be found

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

How many electrons does energy level 1 have

A

2 electrons

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

How many electrons does energy level 2 have

A

8 electrons

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

How many electrons does energy level 3 have

A

18 electrons

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

How many electrons does energy level 4 have

A

32 electrons

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

How many electrons does orbital p have

A

2

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

How many electrons does orbital s have

A

2

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

What is the shape and max number of electrons in sub shell s

A

2 - Max núm of electrons
Shape of sub shell- spherical

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

What is the max num of electrons in sub shell p

A

Max num of electrons - 6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Sub shell d max num of electrons

A

Max num of electrons 10

18
Q

Sub shell f max number of electrons

A

Max number- 14

19
Q

Concentration (g dm^-3) equation

A

Mass of solute(g) / volume of solution (dm^3)

20
Q

Concentration (mol dm^-3)

A

Amount of solute(mol) /vol of solution(dm^3)

21
Q

Concentration (mol dm^-3)
(Conversion to gdm^-3)

A

Concentration (g dm^-3)/ molar mass (g mol^-1) aka mr

22
Q

Relationship between empirical and molecular formula

A

Empirical formula is the simplest whole number ratio of atoms of each element in a compound.

Molecular formula is the actual number of atoms of each element in a compound.

23
Q

the lower the ionisation energy…

A

the easier it is to form an ion

24
Q

name the 3 factors affecting ionisation energy

A
  • Nuclear charge
    -atomic radius
    -shielding
25
Q

what affect does nuclear charge have on ionisation energy

A

more protons mean more positively charged nucleus is and the stronger the attraction of electrons

26
Q

what affect does atomic radius have on ionisation energy

A

attraction falls off rapidly with distance. electron closer will be more attracted than those further

27
Q

what affect does shielding have on ionisation energy

A

when number of electrons between outer electrons and nucleus increase the outer electrons feel less attraction to nuclear charge.

lessening of the pull of the nucleus by inner shells of electrons is called shielding.

28
Q

what does high ionisation energy mean

A

high attraction between electron and the nucleus so more energy is needed to remove electrons

29
Q

why do the ionisation energies increase for increasingly positive ions

A

because there is less repulsion amongst remaining electrons so they are held more strongly by the nucleus

30
Q

Describe the ionisation stage of electron impact

A
  • high energy electrons are fired at the sample from an electron gun
  • this knocks off one electron from each atom or molecule to form a 1+ ion :

X(g) → X+(g) + é

31
Q

Describe the ionisation stage electronspray ionisation

A
  • the sample is dissolved in a volatile solvent

-it’s injected through a fine hypodermic needle at a very high voltage
- the particles gain a proton and become ions :
X(g) + H+(g) → XH+(g)

32
Q

describe the acceleration of ions stage

A

the ions are accelerated using an electric field so that all the ions have the same kinetic energy

33
Q

describe the separation of charges ions stage

A
  • ion drift the ions then enter the flight tube
  • ions with different masses have a different time of flight

-the lighter ions travel faster and take less time to reach the detector

34
Q

describe the detetection stage

A
  • the detector is a negatively charged plate- a current is produced when the ions hit the plate- the more ions
35
Q

Explain why the second ionisation energy is greater than the first ionisation energy

A

Electron removed from positive ion

36
Q

Explain why ionisation energy of every element is endothermic

A

Energy is needed to overcome attraction between negative electron and the nucleus

37
Q

State an explain the general trend in first ionisation energies of period 3 elements from sodium to chlorine

A

Bigger nuclear charge
Electrons closer to nucleus
Smaller atomic radius
So increase

38
Q

Started how oxygen deviates from general trend in first ionisation energies

A

Two pairs of electrons in (3)p orbital which repel each other

39
Q

Why does aluminium deviate from the first ionisation energy trend from Na to Ar

A

Electron further away from nucleus so less energy needed

40
Q

Why is second ionisation energy of sodium greater than second ionisation energy of magnesium

A

Na looses electron from a lower orbital less shielding in Na

41
Q

Why does sodium have a smaller melting point than magnesium

A

Na fewer protons smaller attraction between nucleus and delocalised electrons

42
Q

Explain why it is necessary to ionise molecules when measuring their mass in a TOF mass spectrometer.

A

Ions will interact with and be accelerated by an electric field
Only ions will create a current when hitting the detector

CHEMISTRY A-LEVEL (11 decks)

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