Atomic Structure Flashcards

1
Q

Atomic structure of an atom (3)

A

Mostly empty space
Very dense Nucleus made of protons and neutrneutrons
Electrons in energy shells

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2
Q

Mass of electron

A

1/1840

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3
Q

Proton number

A

Number of protons in the nucleus of an atom

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4
Q

Behaviour of subatomic particles in an electric field

A

Protons deflected to negative
Electrons deflected (more because they’re lighter) to positive

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5
Q

Atomic radius

A

Half the distance between the nuclei of 2 covalently bonded atoms (just measuring 1 will give you a different reading)
-only for neutral atoms
-cannot determine atomic radius of noble gases
-measured in nanometres x10^-9

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6
Q

Trends in atomic radius down a group

A

Atomic radius increases due to an increase in the number of energy shells and the shielding effect

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7
Q

Trends in atomic radius across the period (2)

A

-Atomic radius decreases across a period due to an increase in the number of protons resulting in a greater nuclear attraction between the electrons and the nucleus
-All atoms in the same period experience similar shielding

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8
Q

Ionic radius rule

A

The more positive the ion the smaller the atomic radius
The more negative the ion the larger the ionic radius

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9
Q

Graph to show the trend in ionic radius of successive elements in a period

A
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10
Q

Isotopes

A

Atoms having the same number of protons but a different number of neutrons
-have the same reactivity as they have the same no. Of valence electrons
-physical properties like mass + density change due to neutron no. Change

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11
Q

Relative isotopic mass

A

Relative mass of a single isotope compared with an isotope of carbon-12 which is assigned a relative mass of 12

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12
Q

Important rounding rules for Relative Atomic Mass and isotopic mass

A

RAM : 1dp
Isotopic mass : always a whole number

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13
Q

Rules for orbital diagrams (2)

A

Pauli’s exclusion principle - each orbital may contain a maximum of 2 electrons spinning oppositely
Hound’s rule - orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron

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14
Q

Free radical

A

Species with 1 or more unpaired electron

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15
Q

Ionisation energy

A

Energy required to remove the outermost electron from each atom in one mole of gaseous atoms to form one mole of gaseous ions with a charge of +1

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16
Q

Trends/factors that affect ionisation energy (3)

A

Distance from nucleus + shielding
Nuclear charge
Spin-pair repulsion

17
Q

How distance from nucleus + shielding affects IE

A

As you move down a group, valence electrons are further from the nucleus and experience more shielding, reducing the force of nuclear attraction resulting in a lower ionisation energy

18
Q

group with the highest ionisation energy

19
Q

How nuclear charge affects IE

A

Proton number increases as you move across a period, resulting in an increase in nuclear charge and a stronger nuclear attraction. ?The elements experience similar shielding, resulting in an increase in ionisation energy?

20
Q

How spin-pair repulsion affects IE

A

Spin pair repulsion results in a lower ionisation energy as the paired electrons repel each other

21
Q

Describe electron configuration

A

Electrons occupy orbitals that are found within energy shells

22
Q

How are energy shells named

A

By quantum number (starting closest to the nucleus (1))

23
Q

Orbitals

A

Areas within energy shells where electrons are found
S, p, d and f

24
Q

Sub-shell

A

one or more orbitals in the same shell which have the same energy levels

25
Orbital rule
Each orbital can only hold 2 electrons
26
S-orbital
Only 1 Spherical in shape Holds 2 total electrons
27
P-orbitals
3 - x y and z (each hold 2) 6 total electrons in P-subshell Dumbbell shaped
28
D-orbitals
5 d-orbitals in d-subshell Holds 10 electrons in total
29
Full electron configuration Rules (2)
Big numbers never change Fill 4s before 3d (3d has higher energy) and 5s before 4d
30
Why are there electron configuration exceptions
A half filled or full d-orbital is more stable than a partially filled one. (Stability is the goal)
31
Electron configuration exceptions (2)
32
Describe formation of ions (removing electrons)
The electrons are always removed from the shell furthest from the nucleus
33
How are energy levels numbered
According to their distance from the nucleus (lowest energy, n=1, closest to the nucleus
34
General ionisation energy equation
35
Representing electron configuration diagram (Aufbau) + rule
Always put one electron in each p orbital before pairing them
36
What type of reaction is ionisation energy
Endothermic
37
Relative atomic mass
Average mass of one atom of an element relative to the mass of one carbon-12 atom to which a value of 12 units is assigned