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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

Name 3 sub atomic particles, their location, mass and charge

A

Protons, nucleus, 1, +1
Neutrons, nucleus, 1, 0
Electrons, electron shells around the nucleus, 1/2000, -1

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2
Q

Define atomic number

A

Number of protons in an atom
Defines element

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3
Q

Define mass number

A

Number of protons and neutrons in an atom
Defines isotope

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4
Q

Does atomic number or mass number go at the top

A

Mass number

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5
Q

Define an isotope

A

Atoms with the same number of protons/atomic number but different number of neutrons/mass number

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6
Q

Define relative isotopic mass

A

The average mass of one atom in a sample of one isotope of an element only on a scale where one atom of C-12 is 12 units exactly

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7
Q

Define relative atomic mass

A

The average mass of one atom in a naturally occurring sample of an element on a scale where one atom of C-12 is 12 units exactly

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8
Q

Which formula mass should be used for giant structure compounds

A

RFM
Units g/mol

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9
Q

Describe the process of mass spectronomy

A

Sample vaporised
Particles pos ionised by electron gun (knocks of electrons)
Positive ions accelerated
Pass through neg charged grid
Curved mag field (curved mag poles)
Deflect smallest/most charged ions easiest
Detector has a m/z ratio
Records no.ions/ratio
Ratio is changed to count different partciles

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10
Q

Describe a mass spectronomy graph

A

Y axis: relative intensity
X axis: m/z (z usually 1 but CHECK)
Can be 2 clusters of peaks (parent ions and fragments)
Eg. Ionised Cl2 molecules and fragmented Cl molecules

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11
Q

Describe how to calculate RAM
Eg. Cl

A

(Relative intensity x mass number) + (“”) / 100

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12
Q

Describe how to calculate relative abundance of isotope
Eg. Chlorine

A

Fragments: read straight of graph, make ratio
Parent ionised molecules: all combinations, combined mass number, x relative abundances of atoms, combine any same, find probability as a percentage

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13
Q

State 2 things that can happen when an atom gains energy

A

Speed up
Excitation

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14
Q

What is a ground state atom formation

A

Most stable, normal arrangement o electron
Only ever 1
Electrons held in place by ESA with nucleus

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15
Q

What is excitation

A

Electron moves away to a shell further from the nucleus
Energy absorbed to overcome ESA
Many different excited states
Larger distance = layer excitation
Unstable

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16
Q

What is relaxation

A

Electrons drop back down from excited state
Release energy, photons of light (EMR)
Shine through, series of lines, match light of a specific wavelength

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17
Q

What binds an electron the nucleus

A

Fixed energy caused by ESA between neg charged electron and pos charged nucleus

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18
Q

Describe the Lyman series on a line emission spectra graph

A

N=1
High energy
Low wavelength
UV spectrum
Not visible

19
Q

Describe the Balmer series on a line emission spectra graph

A

Only visible series
Followed by further relaxations

20
Q

Describe the Paschen and Brackett series on a line emission spectra graph

A

Infrared spectrum
Non visible
Low energy
High wavelength
Followed by further relaxations

21
Q

What do arrows on a line emission spectra graph represent

A

Possible relaxations
Large length = large energy lost

22
Q

What is an electron address

A

Exact position in cloud of electrons
Principal shell: size of region
Sub shell: shape of region
Orbital: orientation of region
Spin: up/down

23
Q

Describe the patterns of sub shells and principal shells

A

N=3 has 3 sub shells
S, p, d, f

24
Q

What is an orbital

A

A region within an atom that can hold up to 2 electrons with opposite spins

25
Q

Describe the shape, number of orbitals and electrons in each subshell

A

S, spherical, 1, 2
P, bow tie, 3, 6
D, clover, 5, 10
F, -, 7, 14

26
Q

Describe electron configuration, shortcuts, exceptions and what they show

A

2s2
PS=2
SS=s
No.es=2
4s precedes 3d
Shorten using noble gases [Ne]
Exceptions: Cu,Cr (4s1)
They determine chemical properties of an element

27
Q

State 2 rules for electrons in boxes

A

Fill sub shells stay before pairing up
2 electrons in same box must spun in opp direction

28
Q

Describe the ‘block’ of elements

A

Block indicates subshell outer electron is in
S block= G1,2 + He,H
D block= transition metals
P block= G3-0
F block= ones at bottom

29
Q

Describe ionisation

A

Orbitals get closer together
Eventually converge
Give electrons energy
Pass convergence
Electron lost
Atom becomes ion
Always an endothermic reaction (+Kj/mol)

30
Q

Define ionisation energy

A

Minimum energy required to remove 1 electron from each atom in a mole of atom sin the gas state
Units=Kj/mol

31
Q

Describe successive ionisations

A

Atoms with more than one electron (not H)
Each ionisation removes 1 atom
IE increases arch time

32
Q

Describe patterns in an IE graph of one atom

A

Large increase between principal shells (decrease shielding, despite increased ESA)
Small increase across principal shell (shielding approx constant, decrease ESR)

33
Q

What 2 forces determines the binding of an electron to an atom

A

ESA between neg e and pos nucleus
ESR between neg electrons

34
Q

Define shielding

A

Reduction in ESA between e ad atom nucleus due to es in inner shells blocking the full force

35
Q

Name 4 patterns in first IE graphs

A

Increases mostly across period
Decreases between periods
Decreases don a group
2 small decreases across a period

36
Q

Why does IE mostly increase across period

A

Increase no.protons/nuclear charge
Increase ESA
Es held tighter
Despite shielding approx constant
Decrease in steepness/period

37
Q

Why does IE decrease between periods

A

Ionise from new outer principal shell
Increase shielding
Es held looser
Despite increased nuclear barge/ESA

38
Q

Why does IE decrease down a group

A

increased shielding
Increased distance from nucleus
decreased ESA
Despite increased nuclear charge/ESA

39
Q

Why does IE decreased between group 2 and 3 element

A

Ionising from a new p subshell
Looser bound than s
Further from nuclei, decreased ESA

40
Q

Why does IE decrease between group 5 and 6

A

Ionise from doubly occupied p orbitals
Increased ESR

41
Q

Define periodicity

A

A property that follows a recurring pattern through the periodic table

42
Q

Name 3 periodicity patterns

A

Atomic radius
Mp/bp
Electronegativity

43
Q

Explain periodicity of atomic radius

A

Decreases across period, increased nuclear charge/ESA, despite approx constant shielding, es held tighter
Increases between periods, new principal shell, increased shielding, despite increased nuclear charge/ESA
Cations < atom < anion

44
Q

Explain periodicity of melting point/boiling point

A

High values: giant structure
Low values: simple molecular, lack of bonding
Bp is the same but slightly higher values

Chemistry (24 decks)

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