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GAMSAT > CHM-2-Electronic Structure & Periodic Table > Flashcards

CHM-2-Electronic Structure & Periodic Table Flashcards

1
Q

What are the charges of an:
Electron
Proton
Neutron

A

-1
+1
0

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2
Q

Ionisation of an atom will make it become an…

A

Ion - Either a Cation (Positive) or anion (Negative)

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3
Q

What are valence electrons? (3 Points)

A

The electrons furthest from the nucleus of an atom

  • Responisble for chemical properties
  • Instrumental in chemical bonding
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4
Q

What is an isotope? (2 Points)

A

An element with an unequal number of neutrons to the proton number.
Same atomic number but different atomic mass.

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5
Q

What is the ‘dual nature of matter’?

A

The theory that electrons and subatomic particles are waves as well as particles.

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6
Q

What is the Schrödinger equation?

A

Describes atomic orbitals as complicated wave functions.

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7
Q

What are quantum numbers used for?

A

To describe the theoretical position and therefore energy of an electron.

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8
Q

What are the four quantum numbers?

A

n
ℓ
m\/ℓ
m\/s

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9
Q

Quantum number n (3 Points)

A

The principle quantum number which determines the radial distribution.
-Integer values 1, 2, 3, 4, 5 etc. represent the shell number and orbital size.
-Higher the value of n, the higher the energy
E.g n=1, n=2, n=3

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10
Q

Quantum number - ℓ

A

The Angular Momentum (Azimuthal) quantum number
-Defines the atomic orbital shape
-Takes all integer values between 0 and n -1
E.g n=4 Therefore ℓ=0/1/2/3 (Not 4)

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11
Q

Quantum number - m\/ℓ

A

The Magnetic Quantum Number

  • Defines orientation of an orbital
  • Can have a value of -1, 0 or 1
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12
Q

Quantum number - m\/s

A

The Spin Quantum Number

  • Simply represents the rotational direction of an electron.
  • Can have a value of +1/2 or -1/2 (Antiparalell Spins)
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13
Q

What shape are orbitals with ℓ = 0?

A

s-shaped (Sperical) - Angular distribution that is uniform at every angle

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14
Q

What shape are orbitals with ℓ = 1?

A

p-shaped (2 lobes / Dumbell Shaped)

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15
Q

What shape are orbitals with ℓ = 2?

A

d-shaped (4-leafed Clover shaped)

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16
Q

What shape are orbitals with ℓ = 3?

A

f-shaped

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17
Q

What shape are p orbitals?

A

2 lobes / ‘Dumbell’

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18
Q

What comes after f-shaped orbitals?

A

g, h, I, j etc.

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19
Q

What is heisenberg’s uncertainty principle?

A

You cannot know the exact position and speed of an object E.g An electron in orbit.

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20
Q

When do values of ℓ = 4 and above occur?

A

When n ≥ 4.

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21
Q

What is Pauli’s exclusion principle?

A

No two electrons in an atom can have the same four quantum numbers.

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22
Q

What is Hund’s rule?

A

Electrons fill orbitals singly first until all orbitals of the same energy are filled.

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23
Q

What is the ground state of an atom?

A

When the atom is in it’s lowest overall state of energy.

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24
Q

What occurs when the atom is in it’s ground state?

A

Electronic configuration - where electrons fill orbitals in a set order.

25
Q

For a given m\/ℓ, a maximum of … electrons are allowed.

A

2

26
Q

“Always fill the lowest energy (ground state) orbitals first”

A

Aufbau Principle.

27
Q 
How many orbitals do
s-shapes
p-shapes
d-shapes
f-shapes have?
A

1
3
5
7

28
Q

A paramagnetic material is composed of…

A

atoms with unpaired electrons.

29
Q

A paramagnetic material is …….. a magnetic field.

A

Attracted to

30
Q

A diamagnetic material is composed of…

A

atoms with paired electrons

31
Q

A diamagnetic material is …….. a magnetic field.

A

Repelled by

32
Q

What is the strongest form of magnetism?

A

Ferromagnetic magnetism

33
Q

The excited state configuration is when…

A

Electrons are promoted to higher unoccupied/partially occupied orbitals through energy input into the electron.

34
Q

The ‘n’ value is equal to…

A

The row or period number on the periodic table.

35
Q

When an orbital is one electron from being half full or full, what occurs?

A

An electron from the lower subshel jumps to make the next subshell more stable.

36
Q

In metal ions, transition energies from d-electrons can casue…

A

coloured solutions

37
Q

What is the first Ionisation energy/potenital (IE/IP)?

A

The energy required to remove one of the outermost valence electrons from an atom in it’s gaseous state.

38
Q

First IE/IP increases as…

A

You move from left to right accross a period

You move from the bottom to the top of a group

39
Q

What is the second ionisation energy/potential (IE/IP)

A

The energy required to remove a second valence electron from the ion to form a divalent ion.

40
Q

What is electron affinity (EA)?

A

The energy change that acompanied the following process: X(g) + 1e- ->X-(g)
(X is a given element)

41
Q

What can the electron affinity be used to measure?

A

The ability of an atom to accept an electron - The stronger the attraction of a nucleus, the greater the electron affinity.

42
Q

Why do halogen atoms have a very negative EA?

A

Because they have a great tendancy to form negative ions.

43
Q

Element’s EA become more negative as…

A

You move from left to right on the periodic table

Do not change going down columns

44
Q

From left to right, the atomic radius of elements

A

Decrease

45
Q

What is Electronegativity?

A

Parameter that measures the atom’s ability to pull or repel bond electrons.

46
Q

What is determined to achieve the electronegativity value?

A

1st IE and the EA

47
Q

The greater the value of electronegativity…

A

the greater it’s attraction for bonding electrons

48
Q

The larger the atom…

Electronegativity

A

The less ability for it to attract electrons for itself in chemical bonding.

49
Q

The lower the difference between electronegativity in two covalently bonded atoms…

A

The stronger the bond.

-Due to the bond being shared more equally and thus being more stable.

50
Q

Why are metals good conductors?

A

Their valence electrons can move freely

51
Q

Nonmetals have higher….

A

Electronegativity and ionisation energies

52
Q

General characteristics of Metals

A

Hard/Shiny
3 or less valency electrons
Form + ions by losing e-
Good conductors

53
Q

General characteristrics of Metalloids

A

Varied appearejce
3-7 valence electrons
form + and - ions

54
Q

General characteristics of Nonmetals

A

Gases/Brittle, dull solids
5+ valence electrons
Form - ions by gaining e-

55
Q

Group IA

A

Alkali Metals

56
Q

Group IIA

A

Alkaline Earth Metals

57
Q

Group VIIA

A

Halogens

58
Q

Group 0

A

Noble gases

59
Q

Which groups are the transition elements?

A

IB to VIIIB

GAMSAT (11 decks)

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