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Chemistry > Atomic structure > Flashcards

Atomic structure Flashcards

0
Q

Strong nuclear force

A

Holds protons and neutrons together

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1
Q

Relative mass of electron

A

1/1840

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2
Q

Electrostatic force

A

Hold electrons and protons together

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3
Q

Number of electrons in each shell

A

2n^2

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4
Q

Atomic number (Z)

A

Number of protons

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5
Q

Mass number (A)

A

Number of protons + neutrons

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6
Q

Isotope

A

Same number of protons but different number of neutrons

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7
Q

Order of sub-levels

A

s, p, d, f

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8
Q

s-sub shell

A

Hold up to 2 electrons

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9
Q

p-sub shell

A

Hold up to 6 electrons

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10
Q

d-sub shell

A

Hold up to 10 electrons

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11
Q

f-sub shell

A

Hold up to 14 electrons

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12
Q

Order of sub shells

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 5s, 4d, 5p

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13
Q

Ionisation energy

A

The energy requires to remove one mole of electron from one mole of a gaseous atom

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14
Q

Jump in successive ionisation energies

A

Tells the number of electrons in each main level

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15
Q

Mass spectrometer

A

Identify different isotopes
Determine relative atomic masses & relative molecular masses
Under vacuum condition + gaseous sample

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16
Q

Mass spectrometer

Ionisation

A

A beam of electron from ELECTRON GUN removes electrons from atoms of the sample > positive ions

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17
Q

Mass spectrometer

Acceleration

A

Positive ions attracted towards negatively charged plates.
Speed depends on their mass.
Forms the ions into a beam

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18
Q

Mass spectrometer

Deflection

A

magnetic field deflects the beam of ions (depends on ratio m/z and magnetic field strength)

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19
Q

Mass spectrometer

Detection

A

Detector accept electrons > lose energy > create current (proportional to the ABUNDANCE off each ion)

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20
Q

Relative atomic mass

A

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

21
Q

Avogrado constant

A

6.022 x 10^23

Number of atoms in 12g of carbon-12

22
Q

Idea gas equation

A

P(Pa) V(m^3) = n R T(K)

23
Q

Mole equation

A

Mass = mole x atomic no,Z

24
Q

Concentration

A

Mole = M(mol dm-3) V(dm3)

25
Q

Atom economy

A

Mass of desired product /

total mass of reactant x 100

26
Q

Percentage yield

A

Actual / theory x 100

27
Q

Ionic bond

A

A transfer of electron from metals to non-metals

28
Q

Properties of ionically bonded compound

A

Brittle - the force may move the ions and produce repulsive force as they form a lattice of alternating + and - ions
Conduct electricity when molten or in solution

29
Q

Covalent bond

A

Is sharing a pair of electrons btw non-metals

30
Q

Co-ordinate bond

A

Covalent bond btw 2 atoms where one of the atoms provide both electrons that form the bond

31
Q

Co-ordinate bond

Electron deficient

A

Atom that accepts electron pair

Doesn’t have full outtershell

32
Q

Co-ordinate bond

Donating atom

A

The atom donating the electrons

Has a pair of unused electrons or lone pairs

33
Q

Electronegativity

A

The power of an atom to attract the electron density in covalent bond

34
Q

Electronegativity depends on

A
  1. effective nuclear charge (no of protons)
  2. atomic radius
  3. shielding
35
Q

Polarity

A

Unequal sharing of electrons btw atoms in covalent bond

36
Q

Properties of simple covalently bonded compound

A

Low mp/bp - weak intermolecular force btw molecules
Dissolve in water
Doesn’t conduct electricity

37
Q

Metallic bond

A

Merging of outer main level electrons forming a lattice of positive ions existing in the sea of delocalised electrons

38
Q

Metallic bind strength depends on

A
  1. effective nuclear charge(no of protons)

2. size of ion (smaller=electrons closer)

39
Q

Properties of metals

A

Malleable and ductile - still in the same environment
Conduct electricity - free electrons in sea of delocalised electron to carry charge
High mp/bp - strong attraction btw giant structure

40
Q

van der Waals

A

Instantaneous dipole-induced

Distribution of charge is changing at every instant

41
Q

Dipole-dipole forces

A

Btw molecules with permanent dipole (polarity)

42
Q

Hydrogen bond

A

Bond btw hydrogen and O N or F (very electronegative atoms)

43
Q

2 centre of charges

A

Linear shape

180

44
Q

3 centre of charges

A

Trigonal plannar

120

45
Q

4 centre of charges

A

Tetrahedral

109.5

46
Q

5 centre of charges

A

Trigonal bipyramid

120 and 90

47
Q

6 centre of charges

A

Octahedral

90

48
Q

5 centre of charges

4electron + lone pair

A

Triangular pyramid

107.5

49
Q

4 centre of charges

2electrons + 2lone pairs

A

V-shape

104.5

Chemistry (2 decks)

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